diff --git "a/.lancedb/cbse.lance/data/b00781f6-2e9f-4311-8c98-f4a05bfc535f.lance" "b/.lancedb/cbse.lance/data/b00781f6-2e9f-4311-8c98-f4a05bfc535f.lance" new file mode 100644--- /dev/null +++ "b/.lancedb/cbse.lance/data/b00781f6-2e9f-4311-8c98-f4a05bfc535f.lance" @@ -0,0 +1,4204 @@ +CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-VERY SHORT QUESTIONS.txt +Very Short Answer Type Question [1 mark] +One Sentence Answer +1. What is a redox reaction? +2. What is corrosion? Explain its advantage and disadvantage. +3. What is rancidity? How can we reduce the problem of rancidity? +4. How is corrosion different from rusting? +5. What is meant by endothermic and exothermic reactions? Give suitable example +for each. +6. Define different types of chemical reaction and give examples for each. +7. Why is photosynthesis considered as an endothermic reaction? +8. In electrolysis of water, why is the volu me of gas collected over one electrode +double that of the other electrode? +9. What happens when water is added to solid calcium oxide taken in a container? +Write a chemical formula for the same. +10. Give three types of decomposition reaction. +11. Name the compound us ed for testing CO2-gas.CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-VERY SHORT QUESTIONS.txt +Direction (Q 12 to 16): In the following Questions, the Assertion and Reason have +been put forward. Read the statements carefully and choose the correct +alternative from the following:CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-VERY SHORT QUESTIONS.txt +(a) Both the Assertion and Reason are correct and the reason is the correct +explanation of the Assertion. +(b) The Assertion and the reason are correct but the Reason is not the correct +explanation of the Assertion. +(c) Assertion is true but the Reason is false. +(d) The statement of the Assertion is false but the reason is true. +12. Assertion : AgBr is used on photographic and X -ray film +Reason : AgBr is photosensitive and changes to Ag and bromine in presence + of sunlight and undergoes decomposition reaction. +13. Assertion: Magnesium ribbon keeps on burning in atmosphere of nitrogen. +Reason : Magnesium reacts with nitrogen to form magnesium nitride and + this reaction is combination reaction . +14. Assertion :Zinc reacts with sulphuric acid to form to form zinc sulphate and + Hydrogen gas and it is displacement reaction. +Reason : Zinc reacts with oxygen to form Zinc oxideCHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-VERY SHORT QUESTIONS.txt +Hydrogen gas and it is displacement reaction. +Reason : Zinc reacts with oxygen to form Zinc oxide +15. Assertion : MnO 2 + 4 HCl --- MnCl 2 + Cl 2 + 2 H 2O is r edox reaction. +Reason : MnO 2 oxides HCl to Cl 2 and gets reduced to MnCl 2 +16. Assertion : lead nitrate on thermal decomposition gives lead oxide , brown + coloured nitrogen dioxide and oxygen gas . +Reason : Lead nitrate reacts wi th potassium iodide to form yellow ppt of lead +iodide + And the reaction is double displacement as well as precipitation +reaction.CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-MCQ.txt +Chemical Reactions and Equations +MCQ Type Questions +1. Some crystal s of copper sulphate were dissolved in water. The colour of the +solution obtained would be +(a) Green +(b) Red +(c) Blue +(d) Brown +2. When dilute HCl is added to zinc pieces taken in a test tube +(a) No change take place +(b) The colour of the solution becomes yellow +(c) A pungent smelling gas gets liberated +(d) A small bubbles of H2 gas appear on the surface of zinc pieces. +3. PbS reacts with ozone (O3) and forms PbSO4. As per the balanced equation, +molecues of ozone required for e very one molecule of PbS is/are +(a) 4 +(b) 3 +(c) 2 +(d) 1 +4. Chemically rust is +(a) Hydrated ferrous oxide +(b) Hydrated ferric oxide +(c) Only ferric oxide +(d) None of these +5. Which of the following reactions is not correct +(a) Zn + CuSO 4 ----- ZnSO 4 +Cu +(b) 2 Ag + Cu(NO 3)2 -- 2 AgNO 3 + Cu +(c) Fe + CuSO 4 - FeSO 4 + Cu +(d) Mg + 2 HCl --- MgCl 2 + H 2CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-MCQ.txt +5. Which of the following reactions is not correct +(a) Zn + CuSO 4 ----- ZnSO 4 +Cu +(b) 2 Ag + Cu(NO 3)2 -- 2 AgNO 3 + Cu +(c) Fe + CuSO 4 - FeSO 4 + Cu +(d) Mg + 2 HCl --- MgCl 2 + H 2 +6. Copper displaces which of the following metals from its salt solution: +(a) ZnSO 4 +(b) FeSO 4 +(c) AgNO 3 +(d) NiSO 4 +7. In an electric cell where electrolysis is carried out , anode has: +(a) Positive charge +(b) Negative charge +(c) Connected to negative terminal of the battery +(d) None of these is correct +8. The reaction H 2 + Cl 2 -- 2 HCl represents: +(a) oxidation +(b) reduction +(c) decomposition +(d) combination +9. In the reaction PbO + C -- Pb + CO +(a) PbO is oxidized +(b) C act as an oxidizing agent +(c) C act as a reducing agent (d) Reaction does not represent redox reaction +10. A substance which oxidizes itself and reduces other is known as +(a) Oxidizing agent +(b) Reducing agent +(c) Both (a) and (b) +(d) None of these.CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-MCQ.txt +10. A substance which oxidizes itself and reduces other is known as +(a) Oxidizing agent +(b) Reducing agent +(c) Both (a) and (b) +(d) None of these. +11. Take about 5 ml of dil.HCl in a test tube and add a few pieces of fine granules +of zinc in it. Which gas is evolved? +(a) Chlorine +(b) Hydrogen +(c) HCl +(d) Nitrogen +12. Dissolving sugar is an example of: +(a) Physical change +(b) Chemical change +(c) Redox reaction +(d) None of these +13. Heat is evolved during: +(a) Endother mic reaction +(b) Displacement reaction +(c) Combustion reaction +(d) Combination reaction +14. Which of the following is not a balanced equation? +(a) Fe + Cl 2 ---- FeCl 3 +(b) Mg + CuSO 4 ----- MgSO 4 +Cu +(c) NaOH + HCl -- NaCl + H 2O +(d) Zn + S - ZnS +15. The reaction between lead nitrate and potassium iodide present in aqueous +solution is an example of +(a) Decomposition reaction +(b) Displacement reation +(c) Double displacement reaction +(d) Neutralization reactionCHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-MCQ.txt +solution is an example of +(a) Decomposition reaction +(b) Displacement reation +(c) Double displacement reaction +(d) Neutralization reaction +16. What happens when dilute hydrochloric acid is added to iro n filings? +(a) hydrogen gas and iron chloride are produced +(b) chlorine gas and iron hydroxides are produced +(c) no reaction takes place +(d) iron salt and water are produced. +17. Which of the following gases can be used for the storage of fresh sample of +an oil for a longer time? +(a) Carbon dioxide or oxygen +(b) Nitrogen or helium +(c) Helium or oxygen +(d) Nitrogen or oxygen. +18. In the decomposition of lead (II) nitrate to give lead (II) oxide, nitrogen dioxide +and oxygen gas, the coefficient of nitrogen dioxide ( in the balanced equation) +is +(a) 1 +(b) 2 +(c) 3 (d) 4 +19. We store silver chloride in dark coloured bottles because it is +(a) A white solid +(b) Undergoes redox reaction +(c) To avoid action by sunlight +(d) None of the above.CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-MCQ.txt +(b) 2 +(c) 3 (d) 4 +19. We store silver chloride in dark coloured bottles because it is +(a) A white solid +(b) Undergoes redox reaction +(c) To avoid action by sunlight +(d) None of the above. +20. Silver articles turn blak when kept in the open for a few days due to formation +of +(a) H2S +(b) AgS +(c) AgSO 4 +(d) Ag2SCHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +Chapter 1 +CHEMICAL REACTIONS AND EQUATIONS +Chem ical Reaction: The tra nsformation of chemical substance into another +chemical substance is known as Chemical Reaction. +For example: Rusting of iron, the setting of milk into curd, digestion of food, +respiration, etc. +In a chemical reaction, a new substance is formed which is completely different in +properties from the original substance, so in a chemical reaction, a chemical change +takes place. +Only a rearrangement of atoms takes place in a chemical r eaction. +• The substances which take part in a chemical reaction are called reactants. +• The new substances produced as a result of a chemical reaction are called +products. +Example: The burning of magnesium in the air to form magnesium oxide is an +example of a chemical reaction. + 2Mg(s) + O 2(g) 2MgO(s) +Before burning in air, the magnesium ribbon is cleaned by rubbing with sandpaper.CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +example of a chemical reaction. + 2Mg(s) + O 2(g) 2MgO(s) +Before burning in air, the magnesium ribbon is cleaned by rubbing with sandpaper. +This is done to remove the protective layer of basic magnesium carbonate from the +surface of the magnesi um ribbon. +Reactant: Substances which take part in a chemical reaction are called reactants. +Example: Mg and O 2. +Product: New substance formed after a chemical reaction is called a product. +Example: MgO. +Characteristics of Chemical Reactions: +(i) Evolution of gas: The chemical reaction between zinc and dilute sulphuric acid is +characterised by the evolution of hydrogen gas. + Zn(s) + H 2SO 4(aq) → ZnSO 4(aq) + H 2(g) ↑ +(ii) Change in Colour: The chemical reacti on between citric acid and purple +coloured potassium permanganate solution is characterised by a change in colour +from purple to colourless. +The chemical reaction between sulphur dioxide gas and acidified potassiumCHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +coloured potassium permanganate solution is characterised by a change in colour +from purple to colourless. +The chemical reaction between sulphur dioxide gas and acidified potassium +dichromate solution is characterized by a change in colour from orange to green. +(iii) Change in state of substance: The combustion reaction of candle wax is +characterised by a change in state from solid to liquid and gas (because the wax is a +solid, water formed by the combustion of wax is a liq uid at room temperature +whereas, carbon dioxide produced by the combustion of wax is a gas). There are +some chemical reactions which can show more than one characteristics. +(iv) Change in temperature: The chemical reaction between quick lime water to +form slaked lime is characterized by a change in temperature (which is a rise in +temperature). +The chemical reaction between zinc granules and dilute sulphuric acid is also +characterised by a change in temperature (which is a rise in temperature).CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +temperature). +The chemical reaction between zinc granules and dilute sulphuric acid is also +characterised by a change in temperature (which is a rise in temperature). +(v) Formation of precipitate: The chemical reaction between sulphuric acid and +barium chloride solution is characterised by the formation of a white precipitate of +barium sulphate. + BaCl 2(aq) + H 2SO 4(aq) → BaSO 4(s) (ppt) + 2HCl(aq) +What is a chemical Equation +Chemical Equation: Representation of chemical reaction using symbols and +formulae of the substances is called Chemical Equation. +Example: A + B → C + D +In this equation, A and B are called reactants and C and D are called the p roducts. +The arrow shows the direction of the chemical reaction. Condition, if any, is written +generally above the arrow. +When hydrogen reacts with oxygen, it gives water. This reaction can be represented +by the following chemical equation: + Hydroge n + Oxygen → WaterCHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +generally above the arrow. +When hydrogen reacts with oxygen, it gives water. This reaction can be represented +by the following chemical equation: + Hydroge n + Oxygen → Water + H2 + O 2 → H 2O +In the first equation, words are used and in second, symbols of substances are used +to write the chemical equation. For convenience, the symbol of substance is used to +represent chemical equatio ns. +A chemical equation is a way to represent the chemical reaction in a concise and +informative way. +A chemical equation can be divided into two types: Balanced Chemical Equation and +Unbalanced Chemical Equation. +(a) Balanced Chemical Equation: A balanced chemical equation has the number of +atoms of each element equal on both sides. +Example: Zn + H 2SO 4 → ZnSO 4 + H 2 +In this equation, numbers of zinc, hydrogen and sulphate are equal on both sides, so +it is a Balanced Chemical Equation.CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +Example: Zn + H 2SO 4 → ZnSO 4 + H 2 +In this equation, numbers of zinc, hydrogen and sulphate are equal on both sides, so +it is a Balanced Chemical Equation. +According to the Law of Conservation of Mass, mass can neither be created nor +destroyed in a chemical reaction. To obey this law, the total mass of elements +present in reactants must be equal to the total mass of elements present in products. +(b) Unbalanced Chemical Equation: If the number of atoms of each element in +reactants is not equal to the number of atoms of each element present in the product, then the chemical equation is called Unbalanced Chemical Equation. +Example: Fe + H 2O → Fe 3O4 + H 2 +In this exa mple, a number of atoms of elements are not equal on two sides of the +reaction. For example; on the left -hand side only one iron atom is present, while +three iron atoms are present on the right -hand side. Therefore, it is an unbalanced +chemical equation.CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +reaction. For example; on the left -hand side only one iron atom is present, while +three iron atoms are present on the right -hand side. Therefore, it is an unbalanced +chemical equation. +Balancing a Chemical Equation: To balance the given or any chemical equation, +follow these steps: +Fe + H 2O → Fe 3O4 + H 2 +Write the number of atoms of elements present in reactants and in products in a +table as shown here. +Name of atom No. of atoms in the rea ctant No. of atoms in the product +Iron 1 3 +Hydrogen 2 2 +Oxygen 1 4 +Balance the atom which is maximum in number on either side of a chemical +equation. +In this equation, the number of oxygen atom is the maximum on the RHS. +To balance the oxygen, one needs to multiply the oxygen on the LHS by 4, so that, +the number of oxygen atoms becomes equal on both sides. +Fe + 4 × H 2O → Fe 3O4 + H 2 +Now, the number of hydrogen atoms becomes 8 on the LHS, which is more than thatCHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +the number of oxygen atoms becomes equal on both sides. +Fe + 4 × H 2O → Fe 3O4 + H 2 +Now, the number of hydrogen atoms becomes 8 on the LHS, which is more than that +on the RHS. To balance it, one needs to multiply the hydrogen on the RHS by 4. +Fe + 4 × H 2O → Fe 3O4 + 4 × H 2 +After that, the number of oxygen and hydrogen atoms becomes equal on both sides. +The number of iron is one on the LHS, while it is three on the RHS. To balance it, +multiply the iron on t he LHS by 3. +3 × Fe + 4 × H 2O → Fe 3O4 + 4 × H 2 +Now the number of atoms of each element becomes equal on both sides. Thus, this +equation becomes a balanced equation. Name of atom +No. of atoms in the reactant + No. of atoms in the product +Iron 3 3 +Hydrogen 8 8 +Oxygen 4 4 +After balancing, the above equation can be written as follows: +3Fe + 4H 2O → Fe 3O4 + 4H 2. +To Make Equations More Informative: +Writing the symbols of physical states of substances in a chemical equation:CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +3Fe + 4H 2O → Fe 3O4 + 4H 2. +To Make Equations More Informative: +Writing the symbols of physical states of substances in a chemical equation: +By writing the physical states of substances, a chemical equation becomes more +informative. +• Gaseous state is represented by symbol (g). +• Liquid state is represented by symbol (l). +• Solid state is written by symbol (s). +• Aqueous solution is written by symbol (aq). +• Writing the condition in which reaction takes place: The condition is generally +written above and/or below the arrow of a chemical equation. +Thus, by writing the symbols of the physical state of substances and condition under +which reaction takes place, a chemical equation can be made more informative.CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +What are the types of a chemical reaction Types of Chemical Reactions: Combination Reaction, Decomposition Reaction, +Displacement Reaction, Double Displacement Reaction, Neutralization Reactions, +Exothermic – Endothermic Reactions and Oxidation -Reduction Reactions. +Types of Chemical Reactions: +Chemical reactions can be classified in following types: +(i) Combination Reaction: Reactions in which two or more reactants combine to +form one product are c alled Combination Reactions. +A general combination reaction can be represented by the chemical equation given +here: + A + B → AB +Examples: +When magnesium is burnt in the air (oxygen), magnesium oxide is formed. In this +reaction, magnesium is combine d with oxygen. + 2Mg(s) + O 2(g) → 2MgO(s) + Magnesium + Oxygen → Magnesium Oxide +When carbon is burnt in oxygen (air), carbon dioxide is formed. In this reaction, +carbon is combined with oxygen. +C (s) + O 2(g) → CO 2(g)CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +Magnesium + Oxygen → Magnesium Oxide +When carbon is burnt in oxygen (air), carbon dioxide is formed. In this reaction, +carbon is combined with oxygen. +C (s) + O 2(g) → CO 2(g) +Carbon + Oxyge n → Carbon dioxide +(ii) Decomposition Reaction: Reactions in which one compound decomposes in +two or more compounds or elements are known as Decomposition Reaction. A +decomposition reaction is just the opposite of combination reaction. +A general decomposit ion reaction can be represented as follows: + AB → A + B +Examples: +When calcium carbonate is heated, it decomposes into calcium oxide and carbon +dioxide. +CaCO 3(s) CaO(s) + CO 2(g) +Calcium carbonate → Calcium oxide + Carbon dioxide +When ferric hydroxide is heated, it decomposes into ferric oxide and water + 2Fe(OH) 3(s) Fe 2O3(s) + 3H 2O(l) +Thermal Decomposition: The decomposition of a substance on heating is known +as Thermal Decomposition.CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +2Fe(OH) 3(s) Fe 2O3(s) + 3H 2O(l) +Thermal Decomposition: The decomposition of a substance on heating is known +as Thermal Decomposition. +Example: 2Pb(NO 3)2(s) 2PbO(s) + 4NO 2(g) + O 2(g) +Electrolytic Decomposition: Reactions in which compounds decompose into +simpler compounds because of passing of electricity, are known as Electrolytic +Decomposition. This is also known as Electrolysis. +Example: When electricity is passed in water, it decomposes into hydrogen and +oxygen. + 2H 2O(l) 2H 2(g) + O 2(g) +Photolysis or Photo Decomposition Reaction: Reactions in which a compound +decomposes because of sunlight are known as Photolysis or Photo Decomposition +Reaction. +Example: When silver chloride is put in sunlight, it decomposes into silver metal and +chlorine gas. + 2AgCl(s) (white) 2Ag(s) (grey) + Cl 2(g) +Photographic paper has a coat of silver chloride, which turns into grey when exposedCHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +chlorine gas. + 2AgCl(s) (white) 2Ag(s) (grey) + Cl 2(g) +Photographic paper has a coat of silver chloride, which turns into grey when exposed +to sunlig ht. It happens because silver chloride is colourless while silver is a grey +metal. +(iii) Displacement Reaction: The chemical reactions in which a more reactive +element displaces a less reactive element from a compound is known as +Displacement Reactions. Displacement reactions are also known as Substitution +Reaction or Single Displacement/ replacement reactions. +A general displacement reaction can be represented by using a chemical equation +as follows : + A + BC → AC + B +Displa cement reaction takes place only when ‘A’ is more reactive than B. If ‘B’ is +more reactive than ‘A’, then ‘A’ will not displace ‘C’ from ‘BC’ and reaction will not be +taking place. +Examples: +When zinc reacts with hydrochloric acid, it gives hydrogen gas an d zinc chloride.CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +taking place. +Examples: +When zinc reacts with hydrochloric acid, it gives hydrogen gas an d zinc chloride. + + Zn(s) + 2HCl(aq) → ZnCl 2(aq) + H 2(g) +When zinc reacts with copper sulphate, it forms zinc sulphate and copper metal. + + Zn(s) + CuSO 4(aq) → ZnSO 4(aq) + Cu(s) +(iv) Double Displacement Reaction: Reactions in which ions are exchanged +between two reactants forming new compounds are called Double Displacement +Reactions. + AB + CD → AC + BD +Examples: +When the solution of barium chloride reacts with the solutio n of sodium sulphate, +white precipitate of barium sulphate is formed along with sodium chloride. + + BaCl 2(aq) + Na 2SO 4(aq) → BaSO 4(s) (Precipitate) + 2NaCl(aq) +When sodium hydroxide (a base) reacts with hydrochloric acid, sodium chloride and +water are formed.CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +NaOH(aq) + HCl(aq) → NaCl(aq) + H 2O(l) +Note: Double Displacement Reaction, in which precipitate is formed, is also known +as precipitation reaction. Neutralisation reactions are also examples of double +displacement reaction. +Precipitation Reaction: The reaction in which precipitate is formed by the mixing of +the aqueous solution of two salts is called Precipitation Reaction. +Example: + +Neutralization Reaction: The reaction in which an acid reacts with a base to form +salt and water by an exchange of ions is called Neutralization Reaction. +Example:CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +(v) Oxidation and Reduction Reactions: +Oxidation: Addition of oxygen or non -metallic element or removal of hydrogen or +metallic element from a compound is known as Oxidation. +Elements or compounds in which oxygen or non -metallic element is added or +hydrogen or metallic element is removed are called to be oxidized . +Reduction: Addition of hydrogen or metallic element or removal of oxygen or non - +metallic elemen t from a compound is called Reduction. +The compound or element which goes under reduction in called to be reduced . +Oxidation and Reduction take place together. +Oxidizing agent: +• The substance which gives oxygen for oxidation is called an Oxidizing agent. +• The substance which removes hydrogen is also called an Oxidizing agent. +Reducing agent: +• The substance which gives hydrogen for reduction is called a Reducing agent. +• The substance which removes oxygen is also called a Reducing agent.CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +Reducing agent: +• The substance which gives hydrogen for reduction is called a Reducing agent. +• The substance which removes oxygen is also called a Reducing agent. +The reaction in which oxi dation and reduction both take place simultaneously is +called Redox reaction. +When copper oxide is heated with hydrogen, then copper metal and hydrogen are +formed. +CuO + H 2 → Cu + H 2O +(i) In this reaction, CuO is changing into Cu. Oxygen is being removed f rom copper +oxide. Removal of oxygen from a substance is called Reduction, so copper oxide is +being reduced to copper. +(ii) In this reaction, H 2 is changing to H 2O. Oxygen is being added to hydrogen. +Addition of oxygen to a substance is called Oxidation, so hydrogen is being oxidised +to water. +• The substance which gets oxidised is the reducing agent. +• The substance which gets reduced is the oxidizing agent. +(vi) Exothermic and Endothermic Reactions:CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +to water. +• The substance which gets oxidised is the reducing agent. +• The substance which gets reduced is the oxidizing agent. +(vi) Exothermic and Endothermic Reactions: +Exothermic Reaction: Reaction which produces energy is called Exothermic +Reaction. Most of the decomposition reactions are exothermic. +Example: +Respiration is a decomposition reaction in which energy is released.CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +When quick lime (CaO) is added to water, it releases energy. + +Endothermic Reaction: A chemi cal reaction in which heat energy is absorbed is +called Endothermic Reaction. +Example: Decomposition of calcium carbonate. + +Effects of Oxidation Reactions in Everyday life: Corrosion and Rancidity. +Corrosion: The process of slow conversion of metals i nto their undesirable +compounds due to their reaction with oxygen, water, acids, gases etc. present in the +atmosphere is called Corrosion. +Example: Rusting of iron. + + +Rusting: Iron when reacts with oxygen and moisture forms red substance which is +called Rust .CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +Rusting: Iron when reacts with oxygen and moisture forms red substance which is +called Rust . + +The rusting of iron is a redox reaction. +Corrosion (rusting) weakens the iron and steel objects and structures such as +railings, car bodies, bridges and ships etc. and cuts short their life. +Methods to Prevent Rusting +• By painting. +• By greasing and oilin g. +• By galvanisation. +Corrosion of Copper: Copper objects lose their lustre and shine after some time +because the surface of these objects acquires a green coating of basic copper +carbonate, CuCO 3.Cu(OH) 2 when exposed to air.CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +Corrosion of Silver Metal: The surface of silver metal gets tarnished (becomes dull) +on exposure to air, due to the formation of a coating of black silver sulphide(Ag 2S) on +its surface by the action of H 2S gas present in the air. + + 2 Ag(s) + H 2S -------- ----→ Ag2S + H 2 +Rancidity: The taste and odour of food materials containing fat and oil changes +when they are left exposed to air for a long time. This is called Rancidity. It is caused +due to the oxidation of fat and oil present in food materials. +Methods to prevent rancidity: +• By adding anti -oxidant. +• Vacuum packing. +• Replacing air by nitrogen. +• Refrigeration of foodstuff. +Quick Notes +1. Chemical Reaction: During chemical reactions, the chemical composition of +substances changes or new substances are formed. +2. Chemical Equation: Chemical reactions can be written in chemical equation form +which should always be balanced. +3. Types of Chemical Reactions:CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +2. Chemical Equation: Chemical reactions can be written in chemical equation form +which should always be balanced. +3. Types of Chemical Reactions: +Combination reaction: A single product is formed from two or more reactants. +2Mg + O 2 → 2MgO +Decomposition reaction: A single reactant breaks down to yield two or more +products. +• Thermal decomposition: 2Pb(NO 2)2 → 2PbO + 4NO 2 + O 2 +• Electrolysis: 2H20 → 2H 2 + O 2 +• Photochemical reaction: 2AgBr → 2Ag + Br 2 +Displacement reaction: One element is displaced by another element. +Zn + CuSO 4 → ZnSO 4 + Cu +Double displacement reaction: Exchange of ions between reactants. +AgNO 3 + NaCl → AgCl + NaNO 3 +Redox reaction: Both oxidation and reduction take place simultaneously. +CuO + H 2 → Cu + H 2O +Exothermic reaction: A chemical reaction in which heat energy is evolved. +C + O 2 → CO 2 (g) + heat +Endothermic reaction: A chemical reaction in which heat energy is absorbed. +ZnCO 3 + Heat → ZnO + CO 2CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +C + O 2 → CO 2 (g) + heat +Endothermic reaction: A chemical reaction in which heat energy is absorbed. +ZnCO 3 + Heat → ZnO + CO 2 +Redox reaction: Chemical reaction in which both oxidation and reduction take place +simultaneously. +4. Oxidation: Reaction that involves the gain of oxygen or loss of hydrogen. +5. Reduction: Reaction that shows the loss of oxygen or gain of hydrogen. +ZnO + C → Zn + CO +ZnO is reduced to Zn —reduction. C is oxidized to CO —Oxidation. +6. Effects of Oxidation Reactions in Our Daily Life: +• Corrosion: It is an undesirable change that occurs in metals when they are +attacked by moisture, air, acids and bases. +Example, Corrosion (rusting) of Iron: Fe 2O3. nH 2O (Hydrated iron oxide) • Rancidity: Undesirable change that takes place in oil containing food items +due to the oxidation of fatty acids. +Preventive methods of rancidity: Adding antioxidants to the food materials,CHAPTER 1 -CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +due to the oxidation of fatty acids. +Preventive methods of rancidity: Adding antioxidants to the food materials, +storing food in the airtight container, flush ing out air with nitrogen gas and +refrigeration.CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-COMPETENCY BASED QUESTIONS.txt +Chemical Reactions and Equations +Competency Based QuestionsCHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-COMPETENCY BASED QUESTIONS.txt +1. A compound 'X' used for drinking, has pH =7. Its acidified solution +undergoes decomposition in presence of electricity to produce gases ' +Y' and 'Z' The volume of Y is double than Z. Y is highly combustible +whereas Z is supporter of combustion. identify X. Y & Z and write th e +chemical reactions involved. +2. An aqueous solution of metal nitrate P reacts with sodium bromide +solution to form yellow not of compound O which is used in +photography. O on exposure to sunlight undergoes decomposition +reaction to form metal present in P a long with reddish brown gas. +Identify P & O. Write the chemical reaction & type of chemical reaction. +3. Bhawana took a pale green substance A in a test tube, and heated it +over the flame of a burner. A brown coloured residue B was formed +along with evolution of two gases with burning smell of sulphur. Identify +A & B. Write the chemical reaction involved. +4. A student took 2 -3 g of a substance X in a glass beaker & poured waterCHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-COMPETENCY BASED QUESTIONS.txt +along with evolution of two gases with burning smell of sulphur. Identify +A & B. Write the chemical reaction involved. +4. A student took 2 -3 g of a substance X in a glass beaker & poured water +over it slowly. He observed bubbles along with hissing noise. The +beaker becomes quite hot. Identify X. What type of reaction is it? +5. A substance X used for coating iron articles is added to a blue solution +of a reddish brown metal Y. The colour of the solution gets discharged . +Identify X and Y & also the type of reaction. +6. A reddish brown ve ssel developed a green coloured solid X when left +open in air for a long time. When reacted with dil H 2S04. it forms a blue +coloured solution along with brisk effervescence due to colourless & +odourless gas Z. X decomposes to form black coloured oxide Y of a +reddish brown metal along with gas Z. Identify X. Y. & Z. +7. A student has mixed the solutions of lead (II) nitrate and potassium +iodide,CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-COMPETENCY BASED QUESTIONS.txt +reddish brown metal along with gas Z. Identify X. Y. & Z. +7. A student has mixed the solutions of lead (II) nitrate and potassium +iodide, +(i) What was the colour of the precipitate fo rmed? Can you name the +compound precipitated? +(ii) Write the balanced chemical equation for this reaction, +(iii) What type of reaction is it? 8. Observe the following activity & answer the QuestionsCHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-COMPETENCY BASED QUESTIONS.txt +a. Do you observe anything happening around the zinc granules +b. Is there any change in its temperature? +c. Why is glass tube not dipp ed in dil H 2SO 4? +d. How is H 2 gas collected by downward displacement or upward +displacement of water? +e. Is H 2 gas soluble or insoluble in water? +f. Is H 2 gas heavier or lighter than air? +9. A reddish brown metal X when heated in presence of oxygen forms a +black compound Y which is ba sic in nature when heated with hydrogen +gas gives back X. Identify X & Y. Write the chemical reaction between Y +& H 2 .Identify the substance being oxidized & reduced +10. Name the type of reaction seen in the diagram below. Write the equation +for the reaction.CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-COMPETENCY BASED QUESTIONS.txt +11. A student burnt a metal A found in the form of ribbon. The ribbon burnt +with a dazzling flame & a white powder B is formed which is basic in +nature. Identify A & B. Write the balanced chemical equation. +12. A student drop ped few p ieces of marble in dilute H Cl contained in a test +tube. The gas evolved was passed through lime water. What change +would be observed in lime water? Write chemical reactions for both the +changes observed. +13. Astha has been collecting silver coins and Co pper coins. One day she +observed a black coating on silver coins and a green coating on Co pper +coins. Which chemical phenomenon is responsible for these coatings? +Write the chemical name of black and green coatings +14. Identify the type of chemical reaction +(i) +(ii) +15. A student took 2 -3 g o f a substance X in a glass beaker & poured water +over it slowly. He observed bubbles along with hissing noise. The +beaker becomes quite hot. Identify X. What type of reaction is it?CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-COMPETENCY BASED QUESTIONS.txt +over it slowly. He observed bubbles along with hissing noise. The +beaker becomes quite hot. Identify X. What type of reaction is it? +16. A substance X used for coating iron articles is added to a blue sol ution +of a reddish brown metal. T he colour of the solution gets discharged +Identify X and Y & also the type of reaction. +17. A solution of a substance ‘X’ is used for white washing + i. Name the substance ‘X’ and writes its formula. + ii. Write the reaction of the substance ‘X’ named in (i) above with water +18. A shiny brown coloured element ‘X’ on heating in air becomes black in +colour. Name the element ‘X’ and the black coloured compound formed. +19. An aqueous solution of metal nitrate P reacts with sodium bromide +solution to form yellow ppt of compound Q which is used in +photography. Q on exposure to sunlight undergoes decomposition +reaction to form metal present in P along with reddish brown gas.CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-COMPETENCY BASED QUESTIONS.txt +solution to form yellow ppt of compound Q which is used in +photography. Q on exposure to sunlight undergoes decomposition +reaction to form metal present in P along with reddish brown gas. +Identify P &Q. Write the chemical reaction & type of chemic al reaction. +20. A reddish brown vessel developed a green coloured solid X When left +open in air for a long time. When reacted with dil , it forms a blue +coloured solution along with brisk effervescence due to colourless & +odourless gas Z. X decomposes to for m black coloured oxide Y of a +reddish brown metal along with gas Z, Identify X, Y, & Z. +21. A metal is heated with dil H 2SO 4. The gas evolved is collected by the +method shown in the figure: Answer the followingCHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-COMPETENCY BASED QUESTIONS.txt +(a) Name the gas. +(b) Name the method of collection of gas. +(c) Is the gas soluble or insoluble in water? +(d) Is the gas lighter or heavier than air?CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN TEACHER.txt +1 + SALWAN PUBLIC SCHOOL , RAJENDRA NAGAR +CLASS – X +LESSON PLAN +CHAPTER -1: CHEMICAL REACTIONS AND EQUATIONS +CHAPTER -1: Science :( CHEMICAL REACTIONS AND EQUATIONS ) +Class Transaction + + + +(9-10 days) PART -I + +Total: 4 periods (approx. 35 min each) + +Sub-Topic: Introduction regarding situations of daily life -Physical and + chemical changes +Sub-Topic: Chemical equations(writing equations) + +Sub-Topic: Chemical equations(writing balancing equations) + +Sub-Topic : Type of chemical reactions (combina tion and decomposition) + +Pre-requisite for the +course (KNOWLEDGE) This lesson requires: + Basic knowledge of the situations of daily life and think what happens +when physical and chemical changes take place + The nature and the identity of the initial substance have somewhat +changed. + What is actually meant by a chemical reaction? How do we come to +know that a chemical reaction has taken place? + +Learning ObjectivesCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN TEACHER.txt +Learning Objectives + + Students will be able to: + recognize the Physical and chemical processes associated with +biological and industrial processes affecting life and the +environment. + understand chemical reaction they encounter every day. + represent equations to represent the reactions . + apply the principles of conservation of mass to balance chemical +reactions + identify the different types of chemical reaction and explain.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN TEACHER.txt +Teachers ' activity + Introduction: Teacher will introduce the topic by asking various questions +from previous knowledge : + Analytical skills (scrutinizing an observation): To identify physical +and chemical changes. Example -Paper is torn or Paper is burnt, ice +is melting or iron nail is kept exposed to moist air. + Evidence -based active -learning instructional strategies : + Problem solving (investigating and applying established principles +to justify an observation) + 2 + +Example - Activity: -Burning of a magnesium ribbon in air and collection of +magnesium oxide in a watch -glass. +Concept insight: Always remember that magnesium being a reactive metal will +react with oxygen if kept in open. So, it has to be cleaned before it is burned in +air. +Activity: -Formation of hydrogen gas by the action of dilute hydrochloric acid on +zinc. +Concept insight: The key to this answer is to remember that metals react withCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN TEACHER.txt +air. +Activity: -Formation of hydrogen gas by the action of dilute hydrochloric acid on +zinc. +Concept insight: The key to this answer is to remember that metals react with +hydrochloric acid to form respective metal chlorides an d liberate hydrogen gas. + Critical thinking and collaboration (Competitive evaluation of given +information) +Example - To make a chemical equation more informative, the physical states of +the reactants and products are mentioned along with their chemical form ulae +from given information of different activities. +Concept insight: First convert the word equation into skeletal equation with +state and then balance the different atoms on both sides of the equation. + The ability to understand complex concepts (Inspect ing and analyzing +reasons for variation in established principles);Types of chemical +reactions: +Example - Combination and decomposition reactions : Chemical reactionsCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN TEACHER.txt +reasons for variation in established principles);Types of chemical +reactions: +Example - Combination and decomposition reactions : Chemical reactions +involve the breaking and making of bonds between atoms to produce new +substances and balan cing equations with the help of law of conservation of +mass +Concept insight: Remember that a chemical equation should be balanced to +follow the Law of conservation of mass. +Recapitulation (working effectively with others): +Example -Discuss brain storming questions in class in group.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN TEACHER.txt +Learning Outcomes Students will be able to know: + A complete chemical equation which represents the reactants, +products and their physical states symbolically. + How to write the balanced chemical equation . + A combination and d ecomposition reactions. + Reactions in which heat is given out along with the products are +called exothermic reactions. + Reactions in which energy is absorbed are known as endothermic +reactions.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN TEACHER.txt +Assessment  Continuously monitor student progress by asking oral questions. + Providing active involvement of students in their own learning by +giving daily Practice Problems in the class. + Peer assessment in Lab Activities + Written test +Self-Study,  Self-Study (Independent Practice) -The teacher would ensure that 3 + Assignments , +Homework each student should bring NCERT Book and tries to be independent +at the work as well as be under the teacher’s guidance. + Guided practice followed by Independent Practice ( Question +Bank): +On completion of the chapter, students will be answer the following +revision questions: +Q.1.Why should a magnesium ribbon be cleaned before burning in air? +Q.2. Write a balanced chemical equation with state symbols for the +reactions: Sodium hydroxide solution (in water) reacts with hydrochloric +acid so lution (in water) to produce sodium chloride solution and water.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN TEACHER.txt +reactions: Sodium hydroxide solution (in water) reacts with hydrochloric +acid so lution (in water) to produce sodium chloride solution and water. +Q.3.Take a few zinc granules in a conical flask or a test tube and a dd dilute +hydrochloric acid or sulphuric acid to this. +(a)Do you observe anything happening aroun d the zinc granules? +(b)Touch the conical flask or test tube. Is there any change in its +temperature? +Q.4.Take a small amount of calcium oxide or quick lime in a beaker , slowly +add water to this and touch the beaker. +(a)Do you feel any change in temperature? +(b) Write the balanced chemical equation with physical state. +Q.5.Take about 2 g silver chloride in a china dish and Place this china dish in +sunlight for some time. +(a)Observe the colour of the silver chloride after some time +(b).Name type of the reaction. +Q.6.Take about 2 g barium hydroxide in a test tube. Add 1 g of ammoniumCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN TEACHER.txt +sunlight for some time. +(a)Observe the colour of the silver chloride after some time +(b).Name type of the reaction. +Q.6.Take about 2 g barium hydroxide in a test tube. Add 1 g of ammonium +chloride and mix with the help of a glass rod. Touch the bottom of the test +tube with your palm. +(a)What do you feel? +(b)Is this an exothermic or endothermic reaction? +Homework: The students, with the help of the teacher, will solve the +questions from NCERT back e xercise in their notebook.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN FOR TEACHERS.txt +1 + SALWAN PUBLIC SCHOOL , RAJENDRA NAGAR +CLASS – X +LESSON PLAN +CHAPTER -1: CHEMICAL REACTIONS AND EQUATIONS +CHAPTER -1: Science :( CHEMICAL REACTIONS AND EQUATIONS ) +Class Transaction + + + + +(10-12 days) PART -IICHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN FOR TEACHERS.txt +(10-12 days) PART -II + +Total: 5 periods (approx. 35 min each) +Sub-Topic: Types of chemical reactions -Combination Reaction and different +activities. +Sub-Topic: Types of chemical reactions -Decomposition Reaction and different +activities. +Sub-Topic: Types of chemical reactions -Displacement Reaction and different +activities. +Sub-Topic : Type of chemical reactions –Double displacement reaction and +different activities. +Sub-Topic :- Oxidation and reduction reaction (Corrosion and rancidity) +Pre-requisite for the +course (KNOWLEDGE) This lesson requires: + Knowledge of the basic properties and mechanisms of chemical +reactions. + The nature and the identity of the initial substance have somewhat +changed. + What is actually meant by a chemical reaction? How do we come to +know that a chemical reaction has taken place? + +Learning ObjectivesCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN FOR TEACHERS.txt +Learning Objectives + + Students will be able to: + Classify a chemical reaction as a combination, decomposition, +single replacement, double replacement, exothermic or +endothermic reaction. + Differentiate between the types of chemical reactions. + Predict the products of a chemical reaction. + Understand the different sets of conditions required such as +temperature, light etc in reactions. + Know the effects of oxidation reactions in everyday life like +corrosion and rancidity.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN FOR TEACHERS.txt +Teachers ' activity + Introduction: Teacher will introduce the topic by performing various +activities: +Evidence -based active -learning instructional strategies : + Problem solving (investigating and applying established principles +to justify an observation) Activity: - +Example -1-: Formation of calcium hydroxide +Example -2: Heating of calcium carbonate +Example -3: Electrolysis of water 2 + Example -4: Reaction of iron nails with copper sulphate solution +Example -5: Reaction between Sodium Sulphate and Barium Chloride +Example -6: Reaction between Cu and O 2; CuO and H 2. + Critical thinking and collaboration (Competitive evaluation of given +information) +Recall Activity : +You are given test tube, the solutions of lead (II) nitrate and potassium iodide +and are instructed to mix together in a test tube. Give answers by activity : +(i)What was the colour of the precipitate formed? Can you name the + compound precipitated?CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN FOR TEACHERS.txt +and are instructed to mix together in a test tube. Give answers by activity : +(i)What was the colour of the precipitate formed? Can you name the + compound precipitated? +(ii)Write the balanced chemical equation for this reaction. +(iii)Is this also a double displacement reaction?CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN FOR TEACHERS.txt + The ability to understand the effects of oxidation reactions in +everyday life? +Example - Browning of cut surfaces of fruits. Formation of metal oxide on +metal like iron rust -Corrosion, Burning of crackers , Rancidity: + Recapitulation (working effectively with others): + Example -Discuss brain storming questions in class in group. + +Learning Outcomes Students will be able to know + displacement and double displacement reaction. + precipitation reactions which produce insoluble salts. + importance of Redox reaction in ever day life. Oxidation is the gain of +oxygen or loss of hydrogen. Reduction is the loss of oxygen or gain of +hydrogen. + molecular interactions and chemical reactions in the body .CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN FOR TEACHERS.txt +Assessment  Continuously monitor student progress by asking oral questions. + Providing active involvement of students in their own learning by +giving daily Practice Problems in the class. + Peer assessment in Lab Activities + Written test +Self-Study, +Assignments , +Homework  Self-Study (Independent Practice) -The teacher would ensure that +each student should bring NCERT Book and tries to be independent +at the work as well as be under the teacher’s guidance. + Guided practice followed by Independent Practice ( Question +Bank): +On completion of the chapter, students will be answer the following +revision questions: +Q.1.Give some examples of combination and decomposition reactions. +Q.2. What happens when Ferrous sulphate crystal is heated? Write the +equations also. +Q.3.Dissolve 0.5 gram silver nitrate 10 ml of water in a test tube and place a 3 + Copper wire in a test tube. +Explain your observation.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN FOR TEACHERS.txt +equations also. +Q.3.Dissolve 0.5 gram silver nitrate 10 ml of water in a test tube and place a 3 + Copper wire in a test tube. +Explain your observation. +Q.4. What is the difference between displacement and double displacement +reactions? Write equations for these reactions. +Q.5.Take about 2 g silver bromide in a china dish and Place this china dish in +sunlight for some time. +(a)Observe the colour of the silver bromide after some time +(b).Name type of the reaction. +Q.6.An iron knife kept dipped in a blue copper sulphate solution turns the +blue solution light green. Why? +Homework: The students, with the help of the teacher, will solve the +questions from NCERT back e xercise in their notebook.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-5 MARKS.txt +Long Answer Type Questions [ 5 Marks ] +1. (a) Define a balanced chemical equation. Why should an equation be +balanced? +(b) Write the balanced chemical equation for the following reaction: +(i) Phosphorus burns in presence of chlorine to form phosphorus penta +chloride. +(ii) Burning of natural gas. +(iii) The process of respiration. +2. (a) Explain two ways by which food industries prevent rancidity. +(b) Discuss the importance of decomposition reacti on in metal industry with +three points. +3. (a) Write one example for each of decomposion reaction carried out with help +of +(i) Electricity (ii) Heat (iii) Light +(b) Which of the following statements is correct and why copper can displace +silver from silver ni trate and silver can displace copper from copper sulphate +solution. +4. What happens when a piece of +(a) Zinc metal is added to copper suphste solution? +(b) Aluminium metal is added to dilute hydrochloric acid?CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-5 MARKS.txt +solution. +4. What happens when a piece of +(a) Zinc metal is added to copper suphste solution? +(b) Aluminium metal is added to dilute hydrochloric acid? +(c) Silver metal is added to copper sulphate solution? +Also write the balanced chemical equation if the reaction occurs. +5. On heating blue coloured powder of copper (II) nitrate in a boiling tube , +copper oxide (black), oxygen gas and a brown gas X is formed. +(a) Write a balanced chemical equation of the reaction +(b) Identif y the brown gas x evolved. +(c) Identify the type of reaction +(d) What could be the pH range of aqueous solution of the gas x? +6. On adding a drop of barium chloride solution to an aqueous solution of +sodium sulphate, white precipitate is obtained. +(a) Write the balanced chemical equation of the reaction involved. +(b) What other name can be given to this precipitation reaction? +(c) On adding diu te hydrochloric acid to the reaction mixture, white precipitate +disappears. Why?CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-5 MARKS.txt +(b) What other name can be given to this precipitation reaction? +(c) On adding diu te hydrochloric acid to the reaction mixture, white precipitate +disappears. Why? +7. You are provided with two containers made up of copper and aluminium. You +are aso provided with solutions of dilute HCl, dilute HNO 3, ZnCl 2 and H 2O. In +which of the above cont ainers of these solutions can be kept?CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN FOR TEACHERS.txt +LESSON PLAN +Class: 10 Chapter: 1 ( Chemical Reactions and Equations )CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN FOR TEACHERS.txt +Topics to be covered Chemical reactions, writing chemical equations, Balancing +chemical equations, types of chemical reactions - +combination reactions, decomposition reactions, +displacement reactions, double displacement reactions, +neutralization reactions , precipitation reactions, redox +reactions +Previous Knowledge • Students know differences between physical +change and chemical change +• Studied the symbols of elements and chemical +formulae of molecules. +• Also studied law of conservation of mass. +Learning Objectives • To understand the chemical reactions in daily life +• Able to write the chemical equations from the +statements +• Understand how to balance chemical reactions +• Study different types of chemical reactions +• Define the terms reactants, products, precipitate, +neutralization etc. +Learning Experiences • In combination reactions two or more substances +combine to form a single compound . +• In decomposition reactions a single compoundCHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN FOR TEACHERS.txt +neutralization etc. +Learning Experiences • In combination reactions two or more substances +combine to form a single compound . +• In decomposition reactions a single compound +breaks down into two or more substances. +• Displacement reactions are the reactions in which a +more active element displace a less active element +from its solution. +• In double displacement reactions ions are +exchanged between two compounds. +• REDuction + Oxidation = REDOX reaction +Resources NCERT book +Reference book –Prdeeps Publications +You tube ,education channelsCHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-LESSON PLAN FOR TEACHERS.txt +Teaching Aids Usage of ICT( power point) multimedia., Lab activities( +virtual lab also) + +Procedure Class starts with the introduction +The topics are presenting with power point , audiovisual +aids, virtual lab and lab activities +At the end homework and assignments are given + +Assessment Methods Oral questioning , class tests and monthly testsCHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-IMPORTANT NOTES.txt +Focus Points +1.Chemical Reaction: During chemical reactions, the chemical composition of +substances changes or new substances are formed. +2. Chemical Equation: Chemical reactions can be written in chemical equation form +which should always be balanced. +3. Types of Chemical Reactions: +Combination reaction: A single product is formed from two or more reactants. +2Mg + O 2 → 2MgO +Decomposition reaction: A single reactant breaks down to yield two or more +products. + Thermal decomposition: 2Pb(NO 2)2 → 2PbO + 4NO 2 + O 2 + Electrolysis: 2H20 → 2H 2 + O 2 + Photochemical reaction: 2AgBr → 2Ag + Br 2 +Displacement reaction: One element is displaced by another element. +Zn + CuSO 4 → ZnSO 4 + Cu +Double displacement reaction: Exchange of ions between reactants. +AgNO 3 + NaCl → AgCl + NaNO 3 +Redox reaction: Both oxidation and reduction take place simultaneously. +CuO + H 2 → Cu + H 2OCHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-IMPORTANT NOTES.txt +Double displacement reaction: Exchange of ions between reactants. +AgNO 3 + NaCl → AgCl + NaNO 3 +Redox reaction: Both oxidation and reduction take place simultaneously. +CuO + H 2 → Cu + H 2O +Exothermic reaction: A chemical reaction in which heat energy is evolved. +C + O 2 → CO 2 (g) + heat +Endothermic reaction: A chemical reaction in which heat en ergy is absorbed. +ZnCO 3 + Heat → ZnO + CO 2 +Redox reaction: Chemical reaction in which both oxidation and reduction take place +simultaneously. +4. Oxidation: Reaction that involves the gain of oxygen or loss of hydrogen. 5. Reduction: Reaction that shows the loss of oxygen or gain of hydrogen. + ZnO + C → Zn + CO + ZnO is reduced to Zn —reduction. + C is oxidized to CO —Oxidation. +6. Effects of Oxidation Reactions in Our Daily Life: + Corrosion: It is an undesirable change that occurs in metals when they are +attacked by moisture, air, acids and bases.CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS-IMPORTANT NOTES.txt +6. Effects of Oxidation Reactions in Our Daily Life: + Corrosion: It is an undesirable change that occurs in metals when they are +attacked by moisture, air, acids and bases. +Example, Corrosion (rusting) of Iron: Fe 2O3. nH 2O (Hydrated iron oxide) + Rancidity: Undesirable change that takes place in oil containing food items +due to the oxidation of fat ty acids. +Preventive methods of rancidity: Adding antioxidants to the food materials, +storing food in the airtight container, flushing out air with nitrogen gas and +refrigeration.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +Chemical Reactions +and Equations1 CHAPTER +Consider the following situations of daily life and think what happens +when – +„milk is left at room temperature during summers. +„an iron tawa/pan/nail is left exposed to humid atmosphere. +„grapes get fermented. +„food is cooked. +„food gets digested in our body. +„we respire. +In all the above situations, the nature and the identity of the initialsubstance have somewhat changed. We have already learnt about physicaland chemical changes of matter in our previous classes. Whenever a chemicalchange occurs, we can say that a chemical reaction has taken place. +You may perhaps be wondering as to what is actually meant by a +chemical reaction. How do we come to know that a chemical reactionhas taken place? Let us perform some activities to find the answer to +these questions. +Figure 1.1 +Burning of a magnesium ribbon in air and collection of magnesiumoxide in a watch-glassActivity 1.1Activity 1.1Activity 1.1Activity 1.1Activity 1.1CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +these questions. +Figure 1.1 +Burning of a magnesium ribbon in air and collection of magnesiumoxide in a watch-glassActivity 1.1Activity 1.1Activity 1.1Activity 1.1Activity 1.1 +CAUTION: This Activity needs +the teacher’s assistance. It +would be better if studentswear eye protection. +„Clean a magnesium ribbonabout 2 cm long by rubbingit with sandpaper. +„Hold it with a pair of tongs.Burn it using a spirit lamp orburner and collect the ash so +formed in a watch-glass as +shown in Fig. 1.1. Burn themagnesium ribbon keeping it +as far as possible from your +eyes. +„What do you observe? +“Facts are not science — as the dictionary is not literature.” +Martin H. FischerScience 2Activity 1.2Activity 1.2Activity 1.2Activity 1.2Activity 1.2 +Figure 1.2 +Formation of hydrogengas by the action ofdilute sulphuric acid onzincFrom the above three activities, we can say that any ofthe following observations helps us to determine whethera chemical reaction has taken place – +„change in state +„change in colourCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +„change in state +„change in colour +„evolution of a gas +„change in temperature. +As we observe the changes around us, we can see +that there is a large variety of chemical reactions taking +place around us. We will study about the various types +of chemical reactions and their symbolic representationin this Chapter.Activity 1.3Activity 1.3Activity 1.3Activity 1.3Activity 1.3 +„Take a few zinc granules in a conical flask or a test tube. +„Add dilute hydrochloric acid or sulphuric acid to this +(Fig. 1.2).CAUTION: Handle the acid with care. +„Do you observe anything happening around the zinc +granules? +„Touch the conical flask or test tube. Is there any change inits temperature?„Take lead nitratesolution in a testtube. +„Add potassiumiodide solutionto this. +„What do youobserve? +1.1 CHEMIC1.1 CHEMIC1.1 CHEMIC1.1 CHEMIC1.1 CHEMIC AL EQUAAL EQUAAL EQUAAL EQUAAL EQUA TIONSTIONSTIONSTIONSTIONS +Activity 1.1 can be described as – when a magnesium ribbon is burnt inCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +1.1 CHEMIC1.1 CHEMIC1.1 CHEMIC1.1 CHEMIC1.1 CHEMIC AL EQUAAL EQUAAL EQUAAL EQUAAL EQUA TIONSTIONSTIONSTIONSTIONS +Activity 1.1 can be described as – when a magnesium ribbon is burnt in +oxygen, it gets converted to magnesium oxide. This description of achemical reaction in a sentence form is quite long. It can be written in ashorter form. The simplest way to do this is to write it in the form of aword-equation.The word-equation for the above reaction would be – +Magnesium + Oxygen →Magnesium oxide (1.1) + (Reactants) (Product) +The substances that undergo chemical change in the reaction (1.1), +magnesium and oxygen, are the reactants. The new substance,magnesium oxide, formed during the reaction, is the product. +A word-equation shows change of reactants to products through anCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +magnesium and oxygen, are the reactants. The new substance,magnesium oxide, formed during the reaction, is the product. +A word-equation shows change of reactants to products through an +arrow placed between them. The reactants are written on the left-handside (LHS) with a plus sign (+) between them. Similarly, products arewritten on the right-hand side (RHS) with a plus sign (+) between them.The arrowhead points towards the products, and shows the direction ofthe reaction.You must have observed that magnesium ribbon burns with a +dazzling white flame and changes into a white powder. This powder is +magnesium oxide. It is formed due to the reaction between magnesiumand oxygen present in the air.Chemical Reactions and Equations 31.1.1 Writing a Chemical Equation +Is there any other shorter way for representing chemical equations? +Chemical equations can be made more concise and useful if we use +chemical formulae instead of words. A chemical equation represents aCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +Chemical equations can be made more concise and useful if we use +chemical formulae instead of words. A chemical equation represents a +chemical reaction. If you recall formulae of magnesium, oxygen andmagnesium oxide, the above word-equation can be written as – +Mg + O +2 → MgO (1.2) +Count and compare the number of atoms of each element on the +LHS and RHS of the arrow. Is the number of atoms of each element the +same on both the sides? If not, then the equation is unbalanced because +the mass is not the same on both sides of the equation. Such a chemicalequation is a skeletal chemical equation for a reaction. Equation (1.2) is +a skeletal chemical equation for the burning of magnesium in air. +1.1.2 Balanced Chemical Equations +Recall the law of conservation of mass that you studied in Class IX; mass +can neither be created nor destroyed in a chemical reaction. That is, thetotal mass of the elements present in the products of a chemical reactionCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +can neither be created nor destroyed in a chemical reaction. That is, thetotal mass of the elements present in the products of a chemical reaction +has to be equal to the total mass of the elements present in the reactants. +In other words, the number of atoms of each element remains the +same, before and after a chemical reaction. Hence, we need to balance a +skeletal chemical equation. Is the chemical Eq. (1.2) balanced? Let us +learn about balancing a chemical equation step by step. +The word-equation for Activity 1.3 may be represented as – +Zinc + Sulphuric acid → Zinc sulphate + Hydrogen +The above word-equation may be represented by the following +chemical equation – +Zn + H +2SO4 → ZnSO4 + H2(1.3) +Let us examine the number of atoms of different elements on both +sides of the arrow. +Element Number of atoms in Number of atoms +reactants (LHS) in products (RHS) +Zn 1 1 +H2 2 +S1 1 +O4 4 +As the number of atoms of each element is the same on both sides ofCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +sides of the arrow. +Element Number of atoms in Number of atoms +reactants (LHS) in products (RHS) +Zn 1 1 +H2 2 +S1 1 +O4 4 +As the number of atoms of each element is the same on both sides of +the arrow, Eq. (1.3) is a balanced chemical equation. +Let us try to balance the following chemical equation – +Fe + H2O → Fe3O4 + H2(1.4)Science 4Step I: To balance a chemical equation, first draw boxes around each +formula. Do not change anything inside the boxes while balancing theequation. +Fe + H +2O → Fe3O4 + H2(1.5) +Step II: List the number of atoms of different elements present in the +unbalanced equation (1.5). +Element Number of atoms Number of atoms +in reactants (LHS) in products (RHS) +Fe 1 3 +H2 2 +O1 4 +To equalise the number of atoms, it must be remembered that we +cannot alter the formulae of the compounds or elements involved in thereactions. For example, to balance oxygen atoms we can put coefficient‘4’ as 4 H +2O and not H2O4 or (H2O)4. Now the partly balanced equation +becomes –CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +2O and not H2O4 or (H2O)4. Now the partly balanced equation +becomes – +Fe + 4 H2O → Fe3O4 + H2 +Step IV: Fe and H atoms are still not balanced. Pick any of these elements +to proceed further. Let us balance hydrogen atoms in the partly balancedequation. +To equalise the number of H atoms, make the number of molecules +of hydrogen as four on the RHS.Step III: It is often convenient to start balancing with the compound +that contains the maximum number of atoms. It may be a reactant or aproduct. In that compound, select the element which has the maximumnumber of atoms. Using these criteria, we select Fe +3O4 and the element +oxygen in it. There are four oxygen atoms on the RHS and only one onthe LHS. +To balance the oxygen atoms – +The equation would be – + Fe + 4 H2O → Fe3O4 + 4 H2Atoms of In reactants In products +oxygen +(i) Initial 1 (in H2O) 4 (in Fe3O4) +(ii) To balance 1×4 4 +Atoms of In reactants In products +hydrogen +(i) Initial 8 (in 4 H2O) 2 (in H2)CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +oxygen +(i) Initial 1 (in H2O) 4 (in Fe3O4) +(ii) To balance 1×4 4 +Atoms of In reactants In products +hydrogen +(i) Initial 8 (in 4 H2O) 2 (in H2) +(ii) To balance 8 2 × 4(1.6) +(partly balanced equation) +(1.7) +(partly balanced equation)Chemical Reactions and Equations 5To equalise Fe, we take three atoms of Fe on the LHS. +3 Fe + 4 H2O → Fe3O4 + 4 H2(1.8) +Step VI: Finally, to check the correctness of the balanced equation, we +count atoms of each element on both sides of the equation. +3Fe + 4H2O → Fe3O4 + 4H2 +The numbers of atoms of elements on both sides of Eq. (1.9) are +equal. This equation is now balanced. This method of balancing chemicalequations is called hit-and-trial method as we make trials to balancethe equation by using the smallest whole number coefficient. +Step VII: Writing Symbols of Physical States Carefully examineCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +Step VII: Writing Symbols of Physical States Carefully examine +the above balanced Eq. (1.9). Does this equation tell us anything aboutthe physical state of each reactant and product? No information hasbeen given in this equation about their physical states. +To make a chemical equation more informative, the physical states +of the reactants and products are mentioned along with their chemicalformulae. The gaseous, liquid, aqueous and solid states of reactantsand products are represented by the notations (g), (l), (aq) and (s),respectively. The word aqueous (aq) is written if the reactant or productis present as a solution in water. +The balanced Eq. (1.9) becomes +3Fe(s) + 4H +2O(g) → Fe3O4(s) + 4H2(g) (1.10) +Note that the symbol (g) is used with H2O to indicate that in this +reaction water is used in the form of steam. +Usually physical states are not included in a chemical equation unless +it is necessary to specify them. +Sometimes the reaction conditions, such as temperature, pressure,CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +Usually physical states are not included in a chemical equation unless +it is necessary to specify them. +Sometimes the reaction conditions, such as temperature, pressure, +catalyst, etc., for the reaction are indicated above and/or below the arrowin the equation. For example – +CO(g) + 2H (g)2340atmCH OH(l)3 → (1.11) +6CO (aq) 6H O(l) C H O (aq) 6O22 6 1 2 62 ++Sunlight +Chlorophyll→  ((aq) (1.12) + (Glucose) +Using these steps, can you balance Eq. (1.2) given in the text earlier?Step V: Examine the above equation and pick up the third element which +is not balanced. You find that only one element is left to be balanced,that is, iron. +Atoms of In reactants In products +iron +(i) Initial 1 (in Fe) 3 (in Fe3O4) +(ii) To balance 1×3 3 +(1.9) +(balanced equation)Science 61.2 TYPES OF CHEMIC1.2 TYPES OF CHEMIC1.2 TYPES OF CHEMIC1.2 TYPES OF CHEMIC1.2 TYPES OF CHEMIC AL REAAL REAAL REAAL REAAL REA CTIONSCTIONSCTIONSCTIONSCTIONSCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +(1.9) +(balanced equation)Science 61.2 TYPES OF CHEMIC1.2 TYPES OF CHEMIC1.2 TYPES OF CHEMIC1.2 TYPES OF CHEMIC1.2 TYPES OF CHEMIC AL REAAL REAAL REAAL REAAL REA CTIONSCTIONSCTIONSCTIONSCTIONS +We have learnt in Class IX that during a chemical reaction atoms of one +element do not change into those of another element. Nor do atoms +disappear from the mixture or appear from elsewhere. Actually, chemicalreactions involve the breaking and making of bonds between atoms to +produce new substances. You will study about types of bonds formed +between atoms in Chapters 3 and 4. +1.2.1 Combination Reaction +Activity 1.4Activity 1.4Activity 1.4Activity 1.4Activity 1.4 +„Take a small amount of calcium oxide +or quick lime in a beaker. +„Slowly add water to this. +„Touch the beaker as shown in Fig. 1.3. +„Do you feel any change in temperature? +Figure 1.3 +Formation of slakedlime by the reaction ofcalcium oxide withwater +Calcium oxide reacts vigorously with water to produce slaked limeCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +„Do you feel any change in temperature? +Figure 1.3 +Formation of slakedlime by the reaction ofcalcium oxide withwater +Calcium oxide reacts vigorously with water to produce slaked lime +(calcium hydroxide) releasing a large amount of heat. +CaO(s) + H2O(l) → Ca(OH)2(aq) (1.13) +(Quick lime) (Slaked lime) +In this reaction, calcium oxide and water combine to form a single +product, calcium hydroxide. Such a reaction in which a single productis formed from two or more reactants is known as a combination reaction.QUESTIONSQUESTIONSQUESTIONSQUESTIONSQUESTIONS +1. Why should a magnesium ribbon be cleaned before burning in air? +2. Write the balanced equation for the following chemical reactions. +(i) Hydrogen + Chlorine → Hydrogen chloride +(ii)Barium chloride + Aluminium sulphate → Barium sulphate + + Aluminium chloride +(iii)Sodium + Water → Sodium hydroxide + Hydrogen +3. Write a balanced chemical equation with state symbols for the +following reactions.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +Aluminium chloride +(iii)Sodium + Water → Sodium hydroxide + Hydrogen +3. Write a balanced chemical equation with state symbols for the +following reactions. +(i) Solutions of barium chloride and sodium sulphate in water react +to give insoluble barium sulphate and the solution of sodiumchloride. +(ii) Sodium hydroxide solution (in water) reacts with hydrochloric +acid solution (in water) to produce sodium chloride solution andwater.?Chemical Reactions and Equations 7Let us discuss some more examples of combination reactions. +(i) Burning of coal +C(s) + O2(g) → CO2(g) (1.15) +(ii) Formation of water from H2(g) and O2(g) +2H2(g) + O2(g) → 2H2O(l) (1.16) +In simple language we can say that when two or more substances +(elements or compounds) combine to form a single product, the reactionsare called combination reactions. +In Activity 1.4, we also observed that a large amount of heat is evolved.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +(elements or compounds) combine to form a single product, the reactionsare called combination reactions. +In Activity 1.4, we also observed that a large amount of heat is evolved. +This makes the reaction mixture warm. Reactions in which heat isreleased along with the formation of products are called exothermicchemical reactions. +Other examples of exothermic reactions are –(i) Burning of natural gas +CH +4(g) + 2O2 (g) → CO2 (g) + 2H2O (g) (1.17) +(ii) Do you know that respiration is an exothermic process? +We all know that we need energy to stay alive. We get this energy +from the food we eat. During digestion, food is broken down into simplersubstances. For example, rice, potatoes and bread containcarbohydrates. These carbohydrates are broken down to form glucose.This glucose combines with oxygen in the cells of our body and providesenergy. The special name of this reaction is respiration, the process ofwhich you will study in Chapter 6. +CCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +C +6H12O6(aq) + 6O2(aq) → 6CO2(aq) + 6H2O(l) + energy (1.18) +(Glucose) +(iii) The decomposition of vegetable matter into compost is also an +example of an exothermic reaction. +Identify the type of the reaction taking place in Activity 1.1, where +heat is given out along with the formation of a single product. +Do You Know?A solution of slaked lime produced by the reaction 1.13 is used for white washing +walls. Calcium hydroxide reacts slowly with the carbon dioxide in air to form a thin +layer of calcium carbonate on the walls. Calcium carbonate is formed after two to +three days of white washing and gives a shiny finish to the walls. It is interesting tonote that the chemical formula for marble is also CaCO +3. +Ca(OH)2(aq) + CO2(g) →CaCO3(s) + H2O(l) (1.14) +(Calcium (Calcium +hydroxide) carbonate)Science 8Figure 1.5 +Heating of lead nitrate andemission of nitrogen dioxide +Figure 1.4Correct way of heatingthe boiling tubecontaining crystalsof ferrous sulphateand of smelling theodourCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +Heating of lead nitrate andemission of nitrogen dioxide +Figure 1.4Correct way of heatingthe boiling tubecontaining crystalsof ferrous sulphateand of smelling theodour +Activity 1.6Activity 1.6Activity 1.6Activity 1.6Activity 1.6 +„Take about 2 g lead nitrate powder in a boiling +tube. +„Hold the boiling tube with a pair of tongs andheat it over a flame, as shown in Fig. 1.5. +„What do you observe? Note down the change,if any. +You will observe the emission of brown fumes. +These fumes are of nitrogen dioxide (NO2). The +reaction that takes place is –Activity 1.5Activity 1.5Activity 1.5Activity 1.5Activity 1.5 +„Take about 2 g ferrous sulphate crystals +in a dry boiling tube. +„Note the colour of the ferrous sulphatecrystals. +„Heat the boiling tube over the flame ofa burner or spirit lamp as shown inFig. 1.4. +„Observe the colour of the crystals afterheating. +Have you noticed that the green colour of the ferrous sulphate crystalsCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +„Observe the colour of the crystals afterheating. +Have you noticed that the green colour of the ferrous sulphate crystals +has changed? You can also smell the characteristic odour of burningsulphur. +2FeSO +4(s) Heat→ Fe2O3(s) + SO2(g) + SO3(g) (1.19) +(Ferrous sulphate) (Ferric oxide) +In this reaction you can observe that a single reactant breaks down +to give simpler products. This is a decomposition reaction. Ferroussulphate crystals (FeSO +4, 7H2O) lose water when heated and the colour +of the crystals changes. It then decomposes to ferric oxide (Fe2O3), +sulphur dioxide (SO2) and sulphur trioxide (SO3). Ferric oxide is a solid, +while SO2 and SO3 are gases. +Decomposition of calcium carbonate to calcium oxide and carbonCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +sulphur dioxide (SO2) and sulphur trioxide (SO3). Ferric oxide is a solid, +while SO2 and SO3 are gases. +Decomposition of calcium carbonate to calcium oxide and carbon +dioxide on heating is an important decomposition reaction used invarious industries. Calcium oxide is called lime or quick lime. It hasmany uses – one is in the manufacture of cement. When a decompositionreaction is carried out by heating, it is called thermal decomposition. +CaCO +3(s) Heat→ CaO(s) + CO2(g) (1.20) +(Limestone) (Quick lime) +Another example of a thermal decomposition reaction is given +in Activity 1.6.1.2.2 Decomposition ReactionChemical Reactions and Equations 9Activity 1.7Activity 1.7Activity 1.7Activity 1.7Activity 1.7 +Activity 1.8Activity 1.8Activity 1.8Activity 1.8Activity 1.8 +„Take about 2 g silver chloride in a china dish. +„What is its colour? +„Place this china dish in sunlight for some time +(Fig. 1.7). +„Observe the colour of the silver chloride after sometime. +Figure 1.7CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +„What is its colour? +„Place this china dish in sunlight for some time +(Fig. 1.7). +„Observe the colour of the silver chloride after sometime. +Figure 1.7 +Silver chloride turns greyin sunlight to form silvermetalYou will see that white silver chloride turns grey in sunlight. This is +due to the decomposition of silver chloride into silver and chlorine bylight. +2AgCl(s) +Sunlight→ 2Ag(s) + Cl2(g) (1.22)„Take a plastic mug. Drill two holes at its +base and fit rubber stoppers in these holes.Insert carbon electrodes in these rubberstoppers as shown in Fig. 1.6. +„Connect these electrodes to a 6 voltbattery. +„Fill the mug with water such that theelectrodes are immersed. Add a few dropsof dilute sulphuric acid to the water. +„Take two test tubes filled with water andinvert them over the two carbon electrodes. +„Switch on the current and leave theapparatus undisturbed for some time. +„You will observe the formation of bubblesat both the electrodes. These bubbles displace water in thetest tubes.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +„Switch on the current and leave theapparatus undisturbed for some time. +„You will observe the formation of bubblesat both the electrodes. These bubbles displace water in thetest tubes. +„Is the volume of the gas collected the same in both the test tubes? +„Once the test tubes are filled with the respective gases, remove +them carefully. +„Test these gases one by one by bringing a burning candle close +to the mouth of the test tubes. +CAUTION: This step must be performed carefully by the teacher. +„What happens in each case? +„Which gas is present in each test tube?Figure 1.6 +Electrolysis of water2Pb(NO3)2(s) Heat→ 2PbO(s) + 4NO2(g) + O2(g) (1.21) +(Lead nitrate) (Lead oxide) (Nitrogen (Oxygen) +dioxide) +Let us perform some more decomposition reactions as given in +Activities 1.7 and 1.8.Science 10 +Figure 1.8 +(a) Iron nails dipped in copper sulphate solution?QUESTIONSQUESTIONSQUESTIONSQUESTIONSQUESTIONS +1. A solution of a substance ‘X’ is used for white washing.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +Figure 1.8 +(a) Iron nails dipped in copper sulphate solution?QUESTIONSQUESTIONSQUESTIONSQUESTIONSQUESTIONS +1. A solution of a substance ‘X’ is used for white washing. +(i) Name the substance ‘X’ and write its formula. +(ii) W rite the r eaction of the substance ‘X’ named in (i) above with +water. +2. Why is the amount of gas collected in one of the test tubes in Activity +1.7 double of the amount collected in the other? Name this gas. +1.2.3 Displacement Reaction +Activity 1.9Activity 1.9Activity 1.9Activity 1.9Activity 1.9 +„Take three iron nails and clean them by +rubbing with sand paper. +„Take two test tubes marked as (A) and(B). In each test tube, take about 10 mLcopper sulphate solution. +„Tie two iron nails with a thread andimmerse them carefully in the coppersulphate solution in test tube B forabout 20 minutes [Fig. 1.8 (a)]. Keep oneiron nail aside for comparison. +„After 20 minutes, take out the iron nailsfrom the copper sulphate solution.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +„After 20 minutes, take out the iron nailsfrom the copper sulphate solution. +„Compare the intensity of the blue colourof copper sulphate solutions in test tubes(A) and (B), [Fig. 1.8 (b)]. +„Also, compare the colour of the iron nailsdipped in the copper sulphate solutionwith the one kept aside [Fig. 1.8 (b)].Take about 2 g barium hydroxide in a test tube. Add 1 g of ammonium chloride and mixwith the help of a glass rod. Touch the bottom of the test tube with your palm. What do youfeel? Is this an exothermic or endothermic reaction?Carry out the following ActivitySilver bromide also behaves in the same way. +2AgBr(s)Sunlight→ 2Ag(s) + Br2(g) (1.23) +The above reactions are used in black and white photography. +What form of energy is causing these decomposition reactions? +We have seen that the decomposition reactions require energy either +in the form of heat, light or electricity for breaking down the reactants.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +We have seen that the decomposition reactions require energy either +in the form of heat, light or electricity for breaking down the reactants. +Reactions in which energy is absorbed are known as endothermicreactions.Chemical Reactions and Equations 11Why does the iron nail become brownish in colour and the blue colour +of copper sulphate solution fade? +The following chemical reaction takes place in this Activity– +Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s) (1.24) + (Copper sulphate) (Iron sulphate) +In this reaction, iron has displaced or removed another element, +copper, from copper sulphate solution. This reaction is known asdisplacement reaction. +Other examples of displacement reactions are +Zn(s) + CuSO +4(aq) → ZnSO4(aq) + Cu(s) (1.25) + (Copper sulphate) (Zinc sulphate) +Pb(s) + CuCl2(aq) → PbCl2(aq) + Cu(s) (1.26) + (Copper chloride) (Lead chloride) +Zinc and lead are more reactive elements than copper. They displace +copper from its compounds.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +Pb(s) + CuCl2(aq) → PbCl2(aq) + Cu(s) (1.26) + (Copper chloride) (Lead chloride) +Zinc and lead are more reactive elements than copper. They displace +copper from its compounds. +1.2.4 Double Displacement Reaction +Activity 1.10Activity 1.10Activity 1.10Activity 1.10Activity 1.10 +„Take about 3 mL of sodium sulphate +solution in a test tube. +„In another test tube, take about 3 mL ofbarium chloride solution. +„Mix the two solutions (Fig. 1.9). +„What do you observe? +Figure 1.9Formation of bariumsulphate and sodiumchlorideYou will observe that a white substance, which is +insoluble in water, is formed. This insoluble substanceformed is known as a precipitate. Any reaction thatproduces a precipitate can be called a precipitation reaction. +Na +2SO4(aq) + BaCl2(aq) → BaSO4(s) + 2NaCl(aq) (1.27) +(Sodium (Barium (Barium (SodiumCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +Na +2SO4(aq) + BaCl2(aq) → BaSO4(s) + 2NaCl(aq) (1.27) +(Sodium (Barium (Barium (Sodium +sulphate) chloride) sulphate) chloride)Figure 1.8 (b) Iron nails and copper sulphate solutions compared before and after the experimentScience 121.2.5 Oxidation and Reduction +Activity 1.11Activity 1.11Activity 1.11Activity 1.11Activity 1.11 +„Heat a china dish containing about 1 g +copper powder (Fig. 1.10). +„What do you observe? +Figure 1.10 +Oxidation of copper tocopper oxideThe surface of copper powder becomes coated with +black copper(II) oxide. Why has this blacksubstance formed?This is because oxygen is added to copper andcopper oxide is formed. +2Cu + O +2 Heat→ 2CuO (1.28) +If hydrogen gas is passed over this heated material (CuO), the black +coating on the surface turns brown as the reverse reaction takes placeand copper is obtained. +CuO +H Cu+H O22Heat→  (1.29) +If a substance gains oxygen during a reaction, it is said to be oxidised.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +CuO +H Cu+H O22Heat→  (1.29) +If a substance gains oxygen during a reaction, it is said to be oxidised. +If a substance loses oxygen during a reaction, it is said to be reduced. +During this reaction (1.29), the copper(II) oxide is losing oxygen and +is being reduced. The hydrogen is gaining oxygen and is being oxidised.In other words, one reactant gets oxidised while the other gets reducedduring a reaction. Such reactions are called oxidation-reduction reactionsor redox reactions. +(1.30) +Some other examples of redox reactions are: +ZnO + C →+Zn CO (1.31) +MnO HCl MnCl H O Cl22 2 242+→ + + (1.32)Recall Activity 1.2 , where you have mixed the solutions of lead(II) nitrate +and potassium iodide.(i) What was the colour of the precipitate formed? Can you name the compound +precipitated? +(ii) Write the balanced chemical equation for this reaction.(iii) Is this also a double displacement reaction?What causes this? The white precipitate of BaSO +4 is formed by the +reaction of 2–CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +(ii) Write the balanced chemical equation for this reaction.(iii) Is this also a double displacement reaction?What causes this? The white precipitate of BaSO +4 is formed by the +reaction of 2– +4SO and Ba2+. The other product formed is sodium chloride +which remains in the solution. Such reactions in which there is an +exchange of ions between the reactants are called double displacementreactions.Chemical Reactions and Equations 13In reaction (1.31) carbon is oxidised to CO and ZnO is reduced to Zn. +In reaction (1.32) HCl is oxidised to Cl2 whereas MnO2 is reduced to MnCl2. +From the above examples we can say that if a substance gains oxygen +or loses hydrogen during a reaction, it is oxidised. If a substance losesoxygen or gains hydrogen during a reaction, it is reduced. +QUESTIONSQUESTIONSQUESTIONSQUESTIONSQUESTIONS +?1. Why does the colour of copper sulphate solution change when +an iron nail is dipped in it? +2. Give an example of a double displacement reaction other thanCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +?1. Why does the colour of copper sulphate solution change when +an iron nail is dipped in it? +2. Give an example of a double displacement reaction other than +the one given in Activity 1.10. +3. Identify the substances that are oxidised and the substances +that are reduced in the following reactions. +(i) 4Na(s) + O2(g) → 2Na2O(s) +(ii) CuO(s) + H2(g) → Cu(s) + H2O(l)1.31.31.31.31.3HAHAHAHAHAVE YOU OBSERVED THE EFFECTS OF OVE YOU OBSERVED THE EFFECTS OF OVE YOU OBSERVED THE EFFECTS OF OVE YOU OBSERVED THE EFFECTS OF OVE YOU OBSERVED THE EFFECTS OF O XIDXIDXIDXIDXIDAAAAATIONTIONTIONTIONTION +REAREAREAREAREACTIONS IN EVERYDCTIONS IN EVERYDCTIONS IN EVERYDCTIONS IN EVERYDCTIONS IN EVERYD AAAAAY LIFE?Y LIFE?Y LIFE?Y LIFE?Y LIFE? +1.3.1 Corrosion +You must have observed that iron articles are shiny when new, but get +coated with a reddish brown powder when left for some time. This processis commonly known as rusting of iron. Some other metals also getCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +coated with a reddish brown powder when left for some time. This processis commonly known as rusting of iron. Some other metals also get +tarnished in this manner. Have you noticed the colour of the coating +formed on copper and silver? When a metal is attacked by substancesaround it such as moisture, acids, etc., it is said to corrode and this +process is called corrosion. The black coating on silver and the green +coating on copper are other examples of corrosion. +Corrosion causes damage to car bodies, bridges, iron railings, ships +and to all objects made of metals, specially those of iron. Corrosion of +iron is a serious problem. Every year an enormous amount of money isspent to r eplace damaged iron. You will learn more about corrosion in +Chapter 3. +1.3.2 Rancidity +Have you ever tasted or smelt the fat/oil containing food materials leftfor a long time? +When fats and oils are oxidised, they become rancid and their smell +and taste change. Usually substances which prevent oxidationCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +When fats and oils are oxidised, they become rancid and their smell +and taste change. Usually substances which prevent oxidation +(antioxidants) are added to foods containing fats and oil. Keeping food +in air tight containers helps to slow down oxidation. Do you know thatchips manufacturers usually flush bags of chips with gas such as +nitrogen to prevent the chips from getting oxidised ?Recall Activity 1.1 , where a magnesium ribbon burns with a dazzling flame in air (oxygen) +and changes into a white substance, magnesium oxide. Is magnesium being oxidised orreduced in this reaction?Science 14What you have learnt +„A complete chemical equation represents the reactants, products and their physical +states symbolically. +„A chemical equation is balanced so that the numbers of atoms of each type involvedin a chemical reaction are the same on the reactant and product sides of theequation. Equations must always be balanced.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +„In a combination reaction two or more substances combine to form a new singlesubstance. +„Decomposition reactions are opposite to combination reactions. In a decompositionreaction, a single substance decomposes to give two or more substances. +„Reactions in which heat is given out along with the products are called exothermicreactions. +„Reactions in which energy is absorbed are known as endothermic reactions. +„When an element displaces another element from its compound, a displacementreaction occurs. +„Two different atoms or groups of atoms (ions) are exchanged in double displacementreactions. +„Precipitation reactions produce insoluble salts. +„Reactions also involve the gain or loss of oxygen or hydrogen by substances.Oxidation is the gain of oxygen or loss of hydrogen. Reduction is the loss of oxygenor gain of hydrogen. +EXERCISES +1. Which of the statements about the reaction below are incorrect? +2PbO(s) + C(s) → 2Pb(s) + CO2(g) +(a) Lead is getting reduced.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +EXERCISES +1. Which of the statements about the reaction below are incorrect? +2PbO(s) + C(s) → 2Pb(s) + CO2(g) +(a) Lead is getting reduced. +(b) Carbon dioxide is getting oxidised. +(c) Carbon is getting oxidised. +(d) Lead oxide is getting reduced. +(i) (a) and (b) +(ii) (a) and (c) +(iii) (a), (b) and (c) +(iv) all +2. Fe2O3 + 2Al → Al2O3 + 2Fe +The above reaction is an example of a +(a) combination reaction. +(b) double displacement reaction.Chemical Reactions and Equations 15(c) decomposition reaction. +(d) displacement reaction. +3. What happens when dilute hydrochloric acid is added to iron fillings? Tick the +correct answer. +(a) Hydrogen gas and iron chloride are produced. +(b) Chlorine gas and iron hydroxide are produced. +(c) No reaction takes place. +(d) Iron salt and water are produced. +4. What is a balanced chemical equation? Why should chemical equations be +balanced? +5. Translate the following statements into chemical equations and then balance them.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +4. What is a balanced chemical equation? Why should chemical equations be +balanced? +5. Translate the following statements into chemical equations and then balance them. +(a) Hydrogen gas combines with nitrogen to form ammonia. +(b) Hydrogen sulphide gas burns in air to give water and sulpur dioxide. +(c) Barium chloride reacts with aluminium sulphate to give aluminium chloride +and a precipitate of barium sulphate. +(d) Potassium metal reacts with water to give potassium hydroxide and hydrogen +gas. +6. Balance the following chemical equations. +(a) HNO3 + Ca(OH)2 → Ca(NO3)2 + H2O +(b) NaOH + H2SO4 → Na2SO4 + H2O +(c) NaCl + AgNO3 → AgCl + NaNO3 +(d) BaCl2 + H2SO4 → BaSO4 + HCl +7. Write the balanced chemical equations for the following reactions. +(a) Calcium hydroxide + Carbon dioxide → Calcium carbonate + Water +(b) Zinc + Silver nitrate → Zinc nitrate + Silver +(c) Aluminium + Copper chloride → Aluminium chloride + CopperCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +(a) Calcium hydroxide + Carbon dioxide → Calcium carbonate + Water +(b) Zinc + Silver nitrate → Zinc nitrate + Silver +(c) Aluminium + Copper chloride → Aluminium chloride + Copper +(d) Barium chloride + Potassium sulphate → Barium sulphate + Potassium chloride +8. Write the balanced chemical equation for the following and identify the type of +reaction in each case. +(a) Potassium bromide(aq) + Barium iodide(aq) → Potassium iodide(aq) + +Barium bromide(s) +(b) Zinc carbonate(s) → Zinc oxide(s) + Carbon dioxide(g) +(c) Hydrogen(g) + Chlorine(g) → Hydrogen chloride(g) +(d) Magnesium(s) + Hydrochloric acid(aq) → Magnesium chloride(aq) + Hydrogen(g) +9. What does one mean by exothermic and endothermic reactions? Give examples. +10. Why is respiration considered an exothermic reaction? Explain. +11. Why are decomposition reactions called the opposite of combination reactions? +Write equations for these reactions.Science 16Group Activity +Perform the following activity.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +11. Why are decomposition reactions called the opposite of combination reactions? +Write equations for these reactions.Science 16Group Activity +Perform the following activity. +„Take four beakers and label them as A, B, C and D. +„Put 25 mL of water in A, B and C beakers and copper sulphate solution in beaker D. +„Measure and record the temperature of each liquid contained in the beakers above. +„Add two spatulas of potassium sulphate, ammonium nitrate, anhydrous copper +sulphate and fine iron fillings to beakers A, B, C and D respectively and stir. +„Finally measure and record the temperature of each of the mixture above. +Find out which reactions are exothermic and which ones are endothermic in nature.12. Write one equation each for decomposition reactions where energy is supplied in +the form of heat, light or electricity. +13. What is the difference between displacement and double displacement reactions? +Write equations for these reactions.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS -TEXTBOOK NOTES.txt +the form of heat, light or electricity. +13. What is the difference between displacement and double displacement reactions? +Write equations for these reactions. +14. In the refining of silver, the recovery of silver from silver nitrate solution involved +displacement by copper metal. Write down the reaction involved. +15. What do you mean by a precipitation reaction? Explain by giving examples.16. Explain the following in terms of gain or loss of oxygen with two examples each. +(a) Oxidation +(b) Reduction +17. A shiny brown coloured element ‘X’ on heating in air becomes black in colour. +Name the element ‘X’ and the black coloured compound formed. +18. Why do we apply paint on iron articles?19. Oil and fat containing food items are flushed with nitrogen. Why?20. Explain the following terms with one example each. +(a) Corrosion +(b) RancidityCHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS.txt +Chemical Reactions & +equations +Power Point Presentation ENDCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +Very Short Answer Type Questions [2 Marks]CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +1. “We need to balance a skeletal chemical equation.” Give reason to justify the +statement. +2. Giving an example list two information which make a chemical equation +more useful (informative). +3. Name the reducing agent in the following reaction: + 3MnO 2 + 4Al ———— > 3Mn + 2Al 2O3 +State which is more reactive, Mn or Al and why? +4. (i) Write a balanced chemical equation for process of photosynthesis. + (ii)When do desert plants take up carbon dioxide and perform +photosynthe sis? +5. What is observed when a solution of potassium iodide solution is added to +a solution of lead nitrate? Name the type of reaction. Write a balanced +chemical equation to represent the above chemical reaction. +6. Write balanced chemical equations for the fol lowing reactions. +(i) Silver bromide on exposure to sunlight decomposes into silver and +bromine, +(ii) Sodium metal reacts with water to form sodium hydroxide and hydrogen +gas.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +(i) Silver bromide on exposure to sunlight decomposes into silver and +bromine, +(ii) Sodium metal reacts with water to form sodium hydroxide and hydrogen +gas. +7. Identify the type of reaction(s) in the following equations. +(i)CH 4 + 2O 2 ---- CO 2 + 2 H2O +(ii) Pb(NO 3)2 + 2KI ——–>Pbl 2 + 2KNO 3 +(iii) CaO + H2O ——–> Ca(OH) 2 +(iv) CuSO 4 + Zn ——–> ZnSO 4 + Cu +8. Write balanced equation for the reaction between magnesium and +hydrochloric acid. Name the products obtained, identify the type of reaction. +9. Describe an activity to observe what happens when quick lime is added to +water taken in a beaker. State two important observations and name the type +of reaction taking place. +10. What is the colour of ferrous sulphate crystals? How does this colour change +after heating? +11. Why does the colour of copper sulphate solution change when an iron nail is +dipped in it? Write two observations.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +after heating? +11. Why does the colour of copper sulphate solution change when an iron nail is +dipped in it? Write two observations. +12. Translate the following statement into chemical equation and then balance it : +Barium chloride reacts with aluminium sulphate to gi ve aluminium chloride +and a precipitate of barium sulphate. State the two types in which this reaction +can be classified. +13. Why decomposition reactions are called the opposite of combination +reactions? Write equations for these reactions. +14. AgN0 3 (aq) + NaCl( aq)—————— – > AgCl (s)↓ + NaN0 3(aq) +FeS + H 2S0 4———— - > FeS0 4 + H 2S↑ +Consider the above mentioned two chemical equations with two different +kinds of arrows (↑and ↓) along with product. What do these two different +arrows indicate? +15. Hydrogen being a highly infla mmable gas and oxygen being a supporter of +combustion, yet water which is a compound made up of hydrogen and oxygenCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +arrows indicate? +15. Hydrogen being a highly infla mmable gas and oxygen being a supporter of +combustion, yet water which is a compound made up of hydrogen and oxygen +is used to extinguish fire. Why? 16. Using a suitable chemical equation, justify that some chemical reactions are +determined by: +(i) change in c olour, (ii) change in temperature. +17. (a) A solution of substance ‘X’ is used for white washing. What is the +substance ‘X’? State the chemical reaction of ‘X’ with water. +(b) Why does the colour of copper sulphate solution change when an iron nail +is dipped i n it? +18. Write the balanced equation for the following reaction and identify the type of +reaction in each case. +(i) Potassium bromide + Barium iodide —-> Potassium iodide + Barium +bromide. +(ii) Hydrogen(g) + Chlorine(g) —-> Hydrogen chloride(g) +19. A zinc plate was put into a solution of copper sulphate kept in a glass +container. It was found that blue colour of the solution gets fader and faderCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +19. A zinc plate was put into a solution of copper sulphate kept in a glass +container. It was found that blue colour of the solution gets fader and fader +with the passage of time. After few days, when zinc plate was taken out of the +solution, a number of holes were observed o n it. +(i) State the reason for changes observed on the zinc plate. +(ii) Write the chemical equation for the reaction involved. +20. A white salt on heating decomposes to give brown fumes and a residue is +left behind. +(i) Name the salt. +(ii) Write the equation f or the decom -position reaction. +21. When a solution of potassium iodide is added to a solution of lead nitrate in a +test tube, a reaction takes place. +(a) What type of reaction is this? +(b) Write a balanced chemical equation to represent the above reaction. +22. Define combination reaction. Give one example of a combination reaction +which is also exothermic +23. (a) Classify the following reactions into different types.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +22. Define combination reaction. Give one example of a combination reaction +which is also exothermic +23. (a) Classify the following reactions into different types. + (i) Na 2SO 4 + BaCl 2 ----- BaSO 4 + NaCl + (ii) CaO + H 2O -------- Ca(OH) 2 + (iii) CaCO 3 ---------- CaO + CO 2 +(b) Which of the above reaction(s) is/are precipitation reaction(s)? Why a +reaction is called precipitation reaction?CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +24. Write a balanced chemical equation for the reaction between sodium chloride +and silver nitrate indicating the physical state of the reactants and the +products. +25. What is a redox reaction? When a magnesium ribbon burns in air with a +dazzling flame and forms a white ash, is magnesium oxidized or reduced? +Why? +26. Write any two observations in an activity w hich may suggest that a +chemical reaction has taken place. Give an example in support of your +answer. +27. When the powder of a common metal is heated in an open china dish, its +colour turns black. However, when hydrogen is passed over the hot black +substance s o formed, it regains its original colour. Based on the above +information, answer the following questions. +(i) What type of chemical reaction takes place in each of the two given steps? (ii) Name the metal initially taken in the powder form. Write balanced chemical +equations for both reactions.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +(i) What type of chemical reaction takes place in each of the two given steps? (ii) Name the metal initially taken in the powder form. Write balanced chemical +equations for both reactions. +28. In electrolysis of water, why is the volume of gas collected over one electrode +double that of gas collected over the other electrode? +29. Name the products formed on strongly heating ferrous sulphate crystals. What +type of chemical reaction occurs in this change? +30. What is an oxidation reaction? Give an example of oxidation reaction. Is +oxidation an exothermic or an endothermic reaction? +31. Describe an activity to demonstrate the change that takes place when white +silver chlor ide is kept in sunlight. State the type of chemical reaction which +takes place. +32. When magnesium ribbon burns in air or oxygen, a product is formed. State +the type of chemical reaction and name the product formed in the reaction. +Write balanced chemical equa tion of this reaction.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +the type of chemical reaction and name the product formed in the reaction. +Write balanced chemical equa tion of this reaction. +33. Distinguish between a displacement reaction and a double displacement +reaction. Identify the displacement and the double displacement reaction from +the following reactions. +(i) CuSO 4 + Zn ---- ZnSO 4 +Cu +(ii) Pb(NO 3)2 + KI ----- PbI 2 + 2 KNO 3CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +Short Answer Type Questions (II) [3 Marks] + +34. Write the chemical equation of the reaction in which the following changes +have taken place with an example of each: +(i) Change in colour +(ii) Change in temperature +(iii) Formation of precipitate +35. State the type of chemical reactions and chemical equations that take place in +the following: +(i) Magnesium wire is burnt in air. +(ii) Electric current is passed through water. +(iii) Ammonia and hydrogen chloride gases ‘are mixed. +36. (a) Write the essential c ondition for the following reaction to take place: + 2AgBr —-> 2Ag + Br 2 +Write one application of this reaction. +(b) Complete the following chemical equation of a chemical reaction + Heat + 2FeS0 4 — Fe2O3 +……. + …… +(c) What happens when water is added to quick lime? Write chemical +equation.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +37. 2g of ferrous sulphate crystals are heated in a dry boiling tube. +(i) List any two observations. +(ii) Name the type of chemical reaction taking place. +(iii) ‘Write the chemical equation for the reaction. +38. Write chemical equation reactions taking place when carried out with the help +of +(a) Iron reacts with steam (b) Magnesium reacts with dil HCl +(c) Copper is heated in air. +39. Which products will be obtained when lead nit rate is heated simply? Write +balanced chemical equation for the reaction? State the type of chemical +reaction that occur in the change. +40. What is meant by skeletal type chemical equation? What does it represent? +Using the equation for electrolytic decomposit ion of water, differentiate +between a skeletal chemical equation and a balanced chemical equation. +41. What is rancidity? Mention any two ways by which rancidity can be prevented. +42. Write balanced chemical equation for the reactions that take place duringCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +41. What is rancidity? Mention any two ways by which rancidity can be prevented. +42. Write balanced chemical equation for the reactions that take place during +respir ation. Identify the type of combination reaction that takes place during +this process and justify the name. Give one more example of this type of +reaction. +43. What is redox reaction? Identify the substance oxidised and the substance +reduced in the following reactions. +(i)2PbO + C —–> 2Pb + CO 2 +(ii)MnO 2 + 4HCl —–> MnCl 2 + 2H 20 + Cl 2 +44. Write the balanced chemical equations for the following reaction and identify +the type of reaction. +Thermite reaction, iron (III) oxide reacts with aluminium and gives molten iron +and aluminium oxide. +45. A solution of potassium chloride when mixed with silver nitrate solution, an +insoluble white substance is formed. Write the chemical reaction involved and +also mention the type of the chemica l reaction?CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +insoluble white substance is formed. Write the chemical reaction involved and +also mention the type of the chemica l reaction? +46. Write balanced equations for the following mentioning the type of reaction +involved. +(i) Aluminium + Bromine —–> Aluminium bromide +(ii) Calcium carbonate —–> Calcium oxide + Carbon dioxide +(iii) Silver chloride —–>Silver + Chlorine +47. (a) Why is res piration considered as an exothermic reaction? +(b) Define the terms oxidation and reduction. +(c) Identify the substance that is oxidised and reduced in the following +reaction + Zn + CuO ---- ZnO + CuCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +48. What is meant by +(i) precipitation reac tion, +(ii) exothermic reaction, +(iii) oxidation reaction? +Write balanced chemical equations for an example of each . +49. You might have noted that when copper powder is heated in a china dish, the +surface of copper powder becomes coated with a black colour substance. +(i) How has this black coloured substance formed? +(ii) What is that black substance? +(iii) Write the chemical equation of the reaction that takes place. +50. (a) What happens chemically when quicklime is added to water filled in a +bucket? +(b) On what basis is a chemical equation balanced? +(c ) What change in colour is observed when white silver chloride is left +exposed to sunlight? State the type of chemical reaction in this change. 51. What happens when an aqueous solution of sodium sulphate reac ts with an +aqueous solution of barium chloride? State the physical conditions ofCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +aqueous solution of barium chloride? State the physical conditions of +reactants in which the reaction between them will not take place. Write the +balanced chemical equation for the reaction and name the type of reaction. +52. When you have mixed the solutions of lead(II) nitrate and potassium iodide, +(i) what was the colour of the precipitate formed and can you name the +precipitate? +(ii) Write the balanced chemical equation for this reaction. +(iii) Is this also a double displac ement reaction? +53. Name the type of reaction represented by the following equation: +(i) CaO + H 2O --- Ca(OH) 2 +(ii) 3BaCl 2 + Al 2(SO 4)3 --- 3 BaSO 4 + 2 AlCl 3 + heat +(iii) 2 FeSO 4 -----------------  Fe2O3 + SO 2 + SO 3 +54. Write the chemical equation of the reaction in which the following changes +have taken place with an example of each: +(i) Change in colour +(ii) Change in temperature +(iii) Formation of precipitateCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +have taken place with an example of each: +(i) Change in colour +(ii) Change in temperature +(iii) Formation of precipitate +55. Balance the following chemical equations. +(i) BaCl 2 + H 2SO 4 ------ BaSO 4 + HCl +(ii) Ca(OH) 2 + HNO 3 ---- Ca(NO 3)2 + H 2O +(iii)Pb(NO 3)2 ------ PbO +NO 2 +O 2 +(iv) MnO 2 + HCl ---- MnCl 2 + H 2O + Cl 2 +56. Balance the following chemical reactions and identify the type of reaction. +(a) Mg (s) + Cl 2 (g) --- MgCl 2(s) +(b) HgO (s) -- Hg(l) + O 2(g) +(c) Na(s) + S (s) ---------- Na2S(s) +(d) TiCl4 (l) + Mg (s) ---- Ti(s) + MgCl 2(s) +(e) CaO (s) + SiO 2(s) --- CaSiO 3(s) +(f) H2O2(l) -------- H2O(l) + O 2(g) +57. During the reaction of some metas with dilute hydrochloric acid, following +oberservations were made. +(a) Silver meta does not show any change +(b) The temperature of the reaction mixture rises when aluminium (Al) is +added. +(c) The reaction os sodium metal is found to be highly explosiveCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-SHORT ANSWER TYPE QUESTIONS.txt +(a) Silver meta does not show any change +(b) The temperature of the reaction mixture rises when aluminium (Al) is +added. +(c) The reaction os sodium metal is found to be highly explosive +(d) Some bubbles of a gas are seen when lead (Pb) is reacted with acid. +Explain these observations givi ng suitable reasons.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +Test items + + + +LOB: Compare the characteristics of initial & final substances in order to check whether the +change is physical or chemical + +1) A student poured 100 mL of water in a bottle and added 40 mL vinegar to it. A balloon was filled +with 20 g baking soda and was fixed at the mouth of the bottle. Slowly the shape of the balloon +changed, as shown. + + + +The student claims that a chemical change happened when the two substances were mixed. Is +the claim made by the student correct? + +(a) Yes, as a new substance was formed in the form of a gas. +(b) Yes, as the mass remains the same throughout the experiment. +(c) No, as the formation of bubbles in the mixture shows a physical change. +(d) No, as the change in the shape and size of the balloon shows a physical change. +Correct Answer: Option (a) + +2) A student makes a list of some activities he observes one day.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +2) A student makes a list of some activities he observes one day. + + + + +Which activity can the student classify as a chemical change? + +(a) Activity 1, as the properties of the substances in the mixture change. +(b) Activity 2, as the physical state of the apple pie changes when cut. +(c) Activity 3, as the shape of the can changes. +(d) Activity 4, as the shape and size of the wooden log changes. +Correct Answer: Option (a) +LOB : Relate the substances taking part in the chemical reaction & substances formed in the +chemical reaction in order to classify them as reactants & products +1) Sodium and chlorine are reacted and as a result, sodium chloride is formed which is also called +table salt. What option gives the reactants and products of the reaction?CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +(a) reactants -sodium; products - chlorine +(b) reactants -sodium and table salt; products - chlorine +(c) reactants -tables salt; products - sodium and chlorine +(d) reactants -sodium and chlorine; products - sodium chloride +Correct Answer: Option (d) + + +2) The image shows some chemical reactions. + + + +Which option identifies the reactants and products of the reactions? + +(a) +(b) +(c) +(d) +Correct Answer: Option (c) +LOB : Use chemical symbols & chemical formulae correctly in order to acquire the skill of writing +chemical equations +1) A student performs an experiment to form aluminium chloride from aluminium and chlorine. +Which options gives the chemical equation of the reaction? +(a) Al + Cl2 AlCl 2 +(b) 2Al + Cl2 2AlCl +(c) 2Al + 3Cl 2 2AlCl 3 +(d) 3Al + 3Cl 2 3AlCl 3 + +Correct Answer: Option (c)CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +Correct Answer: Option (c) + + +2) A researcher adds barium hydroxide to hydrochloric acid to form a white -colored barium +chloride. Which option gives the balanced chemical equation of the reaction? + +(a) HCl + Ba(OH) 2 BaCl 2 + 2HOH + +(b) 2HCl + Ba(OH) 2 BaCl 2 + 2HOH + +(c) 2HCl + Ba(OH) 2 BaH 2 + 2HCl + O2 + +(d) HCl + 2Ba(OH) 2BaCl 2 + 2HOH + O2 + +Correct Answer: Option (b) + + + + + + + +LOB : Apply Law of Conservation of Mass in order to balance chemical equations +1) A student writes a balanced chemical equation. +Pb(s) + CuCl 2(aq) PbCl 2(aq) + Cu(s) +Which option gives the number of elements on the LHS and RHS of the chemical equation? +(a) + + +(b) + + + +(c) + + +(d) + + + +Correct Answer: Option (d) + + +2) The image shows a balanced chemical equation of the reaction between sodium and chlorine to +form sodium chloride. + + + +Which option shows the number of atoms on both sides of the reaction? +(a)CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +Which option shows the number of atoms on both sides of the reaction? +(a) + + +(b) + + +(c) + + +(d) + + +Correct Answer: Option (b)CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +LOB: Categorize the given reactions as (combination/ decomposition) based on the reactants & +products of a chemical reaction +1) A student writes a chemical equation of the reaction between carbon monoxide and hydrogen. +CO 2 + 2H 2 -> CH 3OH +How can the reaction be classified? +(a) The reaction is an example of a combination reaction as a compound separates into two +compounds. +(b) The reaction is an example of a decomposition reaction as a compound dissociates into +two compounds. +(c) The reaction is an example of a combination reaction as two compounds react to form a +single compound. +(d) The reaction is an example of a decomposition reaction as two compounds react to form +a single compound. +Correct Answer: Option (c) +2) A student learns that some products are formed as a result of combining two compounds while +some compounds are formed as a result of dissociation of two compounds. The image showsCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +some compounds are formed as a result of dissociation of two compounds. The image shows +two reactions.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +Which reaction is an example of a combination reaction and a decomposition reaction? +(a) both the reactions are examples of combination reaction +(b) both the reactions are examples of a decomposition reaction +(c) reaction P is an example of a combination reaction while reaction Q is an example of a +decomposition reaction +(d) P is an example of a decomposition reaction while reaction Q is an example of a +combination reaction +Correct Answer: Option (c)CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +LOB: Classify the given reaction as displacement or double displacement based on the type of +reactants used & products formed +1) A student adds lead and silver to two different test tubes containing an equal amount of copper +sulphate solution. The student observes that the color of the solution in the test tube with lead +changes. What explains the change in the colour of the solution? +(a) A displacement reaction takes place as lead replaces copper from the solution. +(b) A combination reaction takes place as lead combines with sulpha te in the solution. +(c) decomposition reaction takes place as copper dissociates from sulphate in the solution. +(d) A double displacement reaction takes place as copper dissociates from sulphate and +lead combines with sulphate in the solution. +Correct Answer: Option (a) +2) The chemical reaction between potassium chloride and silver nitrate is given by the chemicalCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +lead combines with sulphate in the solution. +Correct Answer: Option (a) +2) The chemical reaction between potassium chloride and silver nitrate is given by the chemical +equation.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +What can be inferred from the chemical equation? +(a) silver nitrate and potassium undergo a decomposition reaction to form silver chloride +and potassium nitrate +(b) silver nitrate and potassium undergo a displacement reaction to form silver chloride +and potassium nitrate +(c) silver nitrate and potassium undergo a combination reaction to form silver chloride and +potassium nitrate +(d) silver nitrate and potassium undergo double displacement reaction to form silver +chloride and potassium nitrate +Correct Answer: Option (d) + + +LOB: Predict the reaction as Oxidation or Reduction based on the addition/ removal of oxygen/ +hydrogen/ electrons to the reactants to form products. +1) The image shows a reaction between zinc and hydrogen. + Which option shows oxidation? +(a) Zn Zn!" +(b) 2H! H2 +(c) Zn!" Zn +(d) H 2 2H! +Correct Answer: Option (a) + + +2) The image shows a reaction between iron oxide and hydrogen.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +2) The image shows a reaction between iron oxide and hydrogen. + + +Which option shows the compounds undergoing oxidation and reduction? +(a) + + + +(b) + + +(c) + + +(d) + + +Correct Answer: Option (a) + + + + + +LOB: Observe colour change in iron, copper and silver articles over time in order to outline the +effects of corrosion in our surroundings (real life situations, stating any two)CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +LOB: Observe colour change in iron, copper and silver articles over time in order to outline the +effects of corrosion in our surroundings (real life situations, stating any two) + +1) A student notices that a new hammer made of iron is shiny while an old one kept in the toolbox +for long has a reddish -brown powder deposit over it. What does the change in colour of the +hammer indicate? +(a) effect of moisture on metals +(b) iron hammer turns brown after some time +(c) effects of kept in a box for a longer duration +(d) iron changes colour when kept with other tools +Correct Answer: Option (a) +2) A student notices that her silver jewellery turned dull and had a gray -black film over it after +wearing for a few months. What results in the change in colour of the silver metal? +(a) dust deposits over the jewellery which changes its colourCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +(b) the jewellery comes in contact with air, moisture, and acids and corrodes +(c) the polish over the jewellery was removed after wearing for a few months +(d) silver breaks due to wear and tear and turns its colour changes due to rusting +Correct Answer: Option (b) + + +LOB: Detect changes in smell, colour, taste of food items overtime, in order to explain effects of +oxidation on food items + +1) A student learns that food companies fill bags of chips with nitrogen gas. What is the purpose +packing it with nitrogen? +(a) it prevents rancidity of chips +(b) it keeps the mosquitoes away from chips +(c) it keeps the chips dry if the pack falls in water +(d) prevents chips from spilling out when the pack is opened + +Correct Answer: Option (a)CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +Correct Answer: Option (a) + + + + +2) A student notices that the bread kept out has a green coloured coating over it after a few days. +What explains the reason for the student’s observation? +(a) the oils in the bread oxidises and causes rancidity +(b) bread comes in contact with atmospheric moisture and corrodes +(c) the oils in the bread reduces and cause the change in the colour of the bread +(d) comes in contact with the atmospheric nitrogen and a layer deposit over itCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +Correct Answer: Option (a) +Suggested Teacher Resources +1 Activity +Objective Categorize the given reactions as (combination/ decomposition) based on the +reactants & products of a chemical reaction. +Prerequisite Identify the changes that a reaction mixture undergoes during a chemical +reaction, what are reactants, what are products +Material +Required Test tubes, boiling tube, distilled water, burner, sugar, iron fillings, sulphur +powder +Vocabulary Combination Reaction: A reaction in which a single product is formed from +two or more reactants is known as a combination reaction. + +Decomposition Reaction: A reaction in which a single substance decomposes +to give two or more substances. + +Procedure Procedure 1: +1. Take a small amount of iron fillings and sulphur powder in a boiling +tube. +2. Heat the boiling tube strongly over the flame of a burner or spirit lamp +and observe changes.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +Procedure 2: +1. Take about 2 g sugar crystals in a dry boiling tube. (Note the colour of +the crystals.) +2. Heat the boiling tube over the flame of a burner or spirit lamp and +observe changes. +Reflection +Questions +Text to real +world +connection Propane is a fuel used to provide heat for some homes. It is stored in large +tanks as shown here. Can you predict the chemical equation for burning of +propane? + + +Beyond the +classroom What type of reaction takes place inside the human and plant cells? + + + + +Material +required Fresh potato chips, 2 glass jars with lid, Aluminium foil. +Procedure 1. Wrap the glass jar with aluminium foil. Tape the foil in place so that no +light can enter the container. +2. Place fresh potato chips in the foil -wrapped jar and in a similar clear jar +without foil around it.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +Activity + Reaction No. Materials +used Chemicals +used Describe the +reactants +(number of +reactants) Procedure Describe +the +products +(number of +products) Type of +reaction +Calcium +Oxide + +water +Heating +Sugar + + 3. Taste the potato chips and rate their flavour on a 5-point scale, 1 being +extremely dislike the flavour and 5 being extremely like the flavour. +(Enter your data in a table.) +4. Place the two jars on a window sill where they will be exposed to +sunlight. +5. Taste potato chips from each jar at intervals of 1-2 days for 1-2 weeks +and record the taste of potatoes in both the jars. +6. Make a graph of your data, noting the flavor of the potato chips stored +these two ways versus storage time. The y-axis should be the flavor +score and the x-axis the time in days. +Reflection +questions 1. What effect does the aluminium foil have on the taste of potatoes after 2 +weeks?CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-TEST QUESTIONS.txt +score and the x-axis the time in days. +Reflection +questions 1. What effect does the aluminium foil have on the taste of potatoes after 2 +weeks? +2. Is there anything else that will affect the taste of potatoes over 2 weeks +apart from the sunlight?CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +Chemical Reactions and Equations +Introduction to Chemical Reactions and Equations +Physical and chemical changes +Chemical change - one or more new substances with new physical and chemical properties +are formed. +Example: Fe(s)  +  CuSO 4(aq) →FeSO 4(aq) +Cu(s)  +       (Blue)                      (Green)        +Here, when copper sulphate reacts with iron, two new substances, i.e., ferrous sulphate and +copper are formed. +Physical change - change in colour or state occurs but no new substance is formed. +Example: Water changes to steam on boiling but no new substance is formed(Even though +steam and water look different when they are made to react with a piece of Na, they react +the same way and give the exact same products). This involves only change in state (liquid +to vapour).  +Observations that help determine a chemical reaction +A chemical reaction can be determined with the help of any of the following observations: +a) Evolution of a gas +b) Change in temperatureCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +Observations that help determine a chemical reaction +A chemical reaction can be determined with the help of any of the following observations: +a) Evolution of a gas +b) Change in temperature +c) Formation of a precipitate +d) Change in colour +e) Change of state +Chemical reaction +Chemical reactions are chemical changes in which reactants transform into products by +making or breaking of bonds(or both) between different atoms. +Types of chemical reactionsTaking into consideration different factors, chemical reactions are grouped into multiple +categories. +Few examples are: +●Combination +●Decomposition +●Single Displacement +●Double displacement +●Redox +●Endothermic +●Exothermic +●Precipitation +●Neutralisation +Chemical Reactions and Equations I +Word equation +A  word equation is a chemical reaction expressed in words rather than chemical +formulas. It helps identify the reactants and products in a chemical reaction. +For example,  +Sodium + Chlorine → Sodium chlorideCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +formulas. It helps identify the reactants and products in a chemical reaction. +For example,  +Sodium + Chlorine → Sodium chloride +The above equation means: "Sodium reacts with chlorine to form sodium chloride."  +Symbols of elements and their valencies +A symbol is the chemical code for an element. Each element has one or two letter atomic +symbol, which is the abbreviated form of its name. +Valency is the combining capacity of an element. It can be considered as the number of +electrons lost, gain or shared by an atom when it combines with another atom to form a +molecule. +Writing chemical equations +Representation of a chemical reaction in terms of symbols and chemical formulae of the +reactants and products is known as a chemical equation. +Zn(s) +dil.H2SO 4(aq) →ZnSO 4(aq) +H2(↑) + (Reactants)   (Products) +• For solids, the symbol is "(s)". +• For liquids, it is "(l)". +• For gases, it is "(g)".• For aqueous solutions, it is "(aq)".CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +Zn(s) +dil.H2SO 4(aq) →ZnSO 4(aq) +H2(↑) + (Reactants)   (Products) +• For solids, the symbol is "(s)". +• For liquids, it is "(l)". +• For gases, it is "(g)".• For aqueous solutions, it is "(aq)". +• For gas produced in the reaction, it is represented by "(↑)". +• For precipitate formed in the reaction, it is represented by "(↓)". +Balancing of a Chemical Reaction +Conservation of mass +According to the law of conservation of mass, no atoms can be created or destroyed in a +chemical reaction, so the number of atoms for each element in the reactants side has to +balance the number of atoms that are present in the products side. +In other words, the total mass of the products formed in a chemical reaction is equal to the +total mass of the reactants participated in a chemical reaction. +Balanced chemical equation +The chemical equation in which the number of atoms of each element in the reactants side +is equal to that of the products side is called a balanced chemical equation.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +Balanced chemical equation +The chemical equation in which the number of atoms of each element in the reactants side +is equal to that of the products side is called a balanced chemical equation. +Steps for balancing chemical equations +Hit and trial method: While balancing the equation, change the coefficients (the numbers in +front of the compound or molecule) so that the number of atoms of each element is same +on each side of the chemical equation.  +Short-cut technique for balancing a chemical equation +Example: +aCaCO 3+bH3PO 4→cCa 3(PO 4)2+dH2CO 3 +Set up a series of simultaneous equations, one for each element. +Ca: a=3c +C:   a=d +O:   3a+4b=8c+3d +H:   3b=2d +P:    b=2c +Let's set c=1 +Then a=3 and +d=a=3 +b=2c=2So a=3; b=2; c=1; d=3 +The balanced equation is +3CaCO 3+ 2H 3PO 4→Ca3(PO 4)2+ 3H 2CO 3 +Chemical Reactions and Equations II +Types of chemical reactions +Taking into consideration different factors, chemical reactions are grouped into multiple +categories. +Few examples are: +●CombinationCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +Chemical Reactions and Equations II +Types of chemical reactions +Taking into consideration different factors, chemical reactions are grouped into multiple +categories. +Few examples are: +●Combination +●Decomposition +●Single Displacement +●Double displacement +●Redox +●Endothermic +●Exothermic +●Precipitation +●Neutralisation +Combination reaction +In a combination reaction, two elements or one element and one compound or two +compounds combine to give one single product. +H2+Cl2→ 2HCl +element + element → compound +2CO +O2→ 2CO 2 +compound + element → compound +NH 3+HCl →NH 4Cl +compound + compound → compound +Decomposition reaction +A single reactant decomposes on the application of heat or light or electricity to give two or +more products. +Types of decomposition reactions: +a. Decomposition reactions which require heat - thermolytic decomposition or thermolysis. +Thermal decomposition of HgO +b. Decomposition reactions which require light - photolytic decomposition or photolysis.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +Thermal decomposition of HgO +b. Decomposition reactions which require light - photolytic decomposition or photolysis. +Photolytic decomposition of H2O2 +c. Decomposition reactions which require electricity - electrolytic decomposition or +electrolysis. +Electrolytic decomposition of H 2O +Displacement reaction +More reactive element displaces a less reactive element from its compound or solution.i)Zn(s) +CuSO 4(aq) →ZnSO 4(aq) +Cu(s) +ii)Cu(s) + 2AgNO 3(aq) →Cu(NO 3)2(aq) + 2Ag (s) +Double displacement reaction +An exchange of ions between the reactants takes place to give new products. +For example, Al 2(SO4)3(aq) + 3Ca( OH)2(aq) → 2Al (OH)3(aq) + 3CaSO 4(s) +Precipitation reaction +An insoluble compound called precipitate forms when two solutions containing soluble salts +are combined.  +For example, Pb( NO 3)2(aq) + 2KI (aq) → 2KNO 3(aq) +PbI 2(↓)(s)(yellow ) +Redox reaction +Oxidation and reduction take place simultaneously. +Oxidation: Substance loses electrons or gains oxygen or loses hydrogen.CHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +Redox reaction +Oxidation and reduction take place simultaneously. +Oxidation: Substance loses electrons or gains oxygen or loses hydrogen. +Reduction: Substance gains electrons or loses oxygen or gains hydrogen. +Oxidising agent - a substance that oxidises another substance and self-gets reduced. +Reducing agent - a substance that reduces another substance and self-gets oxidised. +Examples: +1.Fe(s) +CuSO 4(aq) →FeSO 4(aq) +Cu(s)       (Blue)                (Green) +Fe→Fe+2+ 2e −  (oxidation ) ; Fe - reducing agent. +Cu+2+ 2e − →Cu(s) (reduction ) ; Cu - oxidising agent. +2.ZnO +C→Zn+CO +ZnO reduces to Zn → reduction +C oxidises to CO → oxidation +ZnO - Oxidising agent +C - Reducing agent +Endothermic and exothermic reaction +Exothermic reaction - heat is evolved during a reaction. Most of the combination reactions +are exothermic. +Al+Fe2O3→Al2O3+Fe+heat +CH 4+ 2O 2→CO 2+ 2H 2O+heat +Endothermic - Heat is required to carry out the reaction. +6CO 2+ 6H 2O+Sunlight →C6H12O6+ 6O 2 +       GlucoseCHAPTER 1- CHEMICAL REACTIONS AND EQUATIONS-REVISION NOTES.txt +are exothermic. +Al+Fe2O3→Al2O3+Fe+heat +CH 4+ 2O 2→CO 2+ 2H 2O+heat +Endothermic - Heat is required to carry out the reaction. +6CO 2+ 6H 2O+Sunlight →C6H12O6+ 6O 2 +       Glucose +Most of the decomposition reactions are endothermic. +Corrosion +Gradual deterioration of a material, usually a metal, by the action of moisture, air or +chemicals in the surrounding environment. +Rusting: +4Fe(s) + 3O 2(from  air) +xH 2O(moisture ) → 2Fe 2O3.xH 2O(rust) +Corrosion of copper: +Cu(s) +H2O(moisture ) +CO 2(from  air) →CuCO 3.Cu(OH)2(green ) +Corrosion of silver: +Ag(s) +H2S(from  air) →Ag2S(black) +H2(g) +Rancidity +It refers to oxidation of fats and oils in food that is kept for a long time. It gives foul smell +and bad taste to food. Rancid food causes stomach infection on consumption. +Prevention: +(i) Use of air-tight containers(ii) Packaging with nitrogen +(iii) Refrigeration +(iv) Addition of antioxidants or preservativesCHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS 2.txt +Chemical Reactions & +equations +Power Point Presentation ENDCHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS5.txt +Chemical Reactions and Equations +Chemical Reactions and Equations +Any process that involves the rearrangement of structure of the substance or conversion of +reactants into products is defined as Chemical Reaction . +For a Chemical Reaction to occur, the change can be observed in the form of - + Change in State : Melting of ice into water. + Change in Colour : Iron rusting which has colour change from silver to reddish brown.CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS5.txt + Change in Temperature : There are two types of reaction i.e Exothermic and Endothermic +Reaction. +Exothermic Reactions: Those reactions in which energy is released in the form of heat are +called Exothermic Reactions . +Examples - +(1) All combustion reactions e.g. +CH 4+ 2O 2 —> CO 2 + 2H 2O + Heat +(2) Thermite reactions e.g. +2A 1 + Fe 2O3 —> 2Fe + Al 2O3 + Heat +Combinations are generally exothermic in nature. The decomposition of organic matters into +compost is an example of exothermic reaction. +Endothermic Reactions: Those reactions in which energy is absorbed are called Endothermic +Reactions . +Examples - + +also, the reaction of photosynthesis -CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS5.txt +also, the reaction of photosynthesis - + + Evolution of any gas: When Zinc reacts with sulphuric acid it gives hydrogen gas. +Zn + H2 SO 4 → ZnSO 4 + H2 +Formation of Precipitate : When a soluble carbonate reacts with Barium, Barium Carbonate +precipitate can be observed. +Change in State +Some chemical reactions are characterized by a change in state. + When wax is burned (in the form of wax candle,) then water and carbon dioxide are formed. + Now, wax is a liquid whereas carbon dioxide is a gas. This means that during the combustion +reaction of wax, the physical state changes from solid to liquid and gas. +Physical Change + In this change identity of the substance remains same. + For Example, Melting, Boiling etc. +Chemical Change + The identity of the substances change + Reactants are converted into substance due to formation or broken down of older bondsCHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS5.txt +Chemical Equation +The symbolic representation of chemical reaction using symbols and formulae is known +as Chemical Equation . For this, reactants are written in left hand side whereas products are +written on the right. +Balanced Chemical Equation +A balanced chemical equation is the one where the number of atoms involved in reactants side is +equal to number of atoms on product side. + +Eq.1. Example of Balanced Chemical Equation +Steps to form Balanced Equation +To show how to balance the equation, the following equation is used - +Fe + H2O → Fe 3O4 + H2 +Step 1: First of all, draw the boxes around each formula as shown below -CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS5.txt +Step 2: Find out the number of atoms of each element. For Example , on reactant side, 1 for Fe, +2 H, and 1 O and on product side we have, 3 for Fe, 4 for O and 2 for H. +Step 3: Start to balance the equation with the compound having maximum number of atoms. While +balancing does not alter the formula of the compound. +Step 4: One by one balance each element on reactant and product side. + +Step 5: After balancing number of atoms on both the side of the equation, finally check the +correctness of the balanced equation. + +Step 6: then write the symbols of the physical state of reactants and products as shown below - +3Fe(s) + 4H 2O (g) → Fe 3O4 (s) + 4H 2 (g) +This above equation represents the balanced equation. +Balancing a Redox Reaction +The basic ionic form of the equation is - +Fe2+ + Cr 2O72- → Fe3+ + Cr3+ +Oxidation half reaction is - + +Reduction half reaction is -CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS5.txt +Reduction half reaction is - + +Use the reduction half method to balance the equation. Balance the atoms in each half of the +reaction except H and O atoms. +Cr 2O72- (aq) → 2 Cr3+(aq) +Add water molecules as the reaction is taking place in acidic solution. This is to balance the O +atoms and hydrogen ions. +Cr 2O72- (aq) + 14 H+(aq) → 2 Cr3+(aq) + 7H 2O (I) +Then balance the charges in both half reactions. +Fe2+(aq) → Fe3+(aq) + e- +Cr 2O72- (aq) + 14 H+ + 6e- → 2 Cr3+ + 7H 2O +6 Fe2+(aq) → 6 Fe3+(aq) + 6e- +Two half of the equations are added to get the overall reaction +6Fe2+(aq) + Cr 2O72-(aq) + 14H+(aq) → 6Fe3+(aq) + 2Cr3+(aq) + 7H 2O (I) +Types of Chemical Reaction + Combination Reaction is reaction when single product is formed from the combination of two +or more reactants. For Example -CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS5.txt +Eq.2. Example of Combination Reaction +Reactions can be exothermic as well as endothermic. Exothermic reaction release heats and +raises the temperature of the surroundings. For Example , Respiration is an example of exothermic +reaction. + +Eq.3. Example of Exothermic Reaction +Endothermic reaction involved the absorption of the heat and thus it cools the surrounding. The +decomposition of dead organic material is an endothermic reaction. +�� Decomposition Reaction is type of reaction which involves breakdown of single reactant into +simpler products. Decomposition of silver chloride into silver and chlorine in presence of +sunlight is an example of decomposition reaction. + +Eq.4. Example of Deco mposition Reaction + Displacement Reaction is a reaction in which more reactive element will +displaces the less reactive element.CHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS5.txt +Eq.4. Example of Deco mposition Reaction + Displacement Reaction is a reaction in which more reactive element will +displaces the less reactive element. + +Eq. 5. Example of Displacement Reaction + Double Displacement Reaction is a type of reaction in which cations and anions in the +reactants switch the places to form new products. + +Eq. 6. Example of Double Displacement Reaction + Redox Reaction is also known as Oxidation -reduction Reaction . In this type of reaction +transfer of electrons occurs between the two species. Oxidation is def ined as addition of oxygen +or removal of hydrogen. Reduction is defined as removal of oxygen or addition of hydrogen. +Oxidizing agent is the one which gains the electrons and is reduced in a chemical reaction. +Reducing agent is oxidized in a chemical react ion and it loses the electrons. Fluorine is the +strongest oxidizing agent. Formic acid is a reducing agentCHAPTER 1 CHEMICAL REACTIONS AND EQUATIONS5.txt +Eq.7. Example of Redox Reaction +Corrosion +Metals are prone to corrosion. It is a slow conversion of metals into some undesirable compounds. +This occur may be due to reaction with oxygen, gases, acids etc. When irons reacts with +atmospheric oxygen and moisture, a red layer is formed on the surface of the iron, this process is +known as Rusting . + +Eq. 8. Equation for Iron Rusting +Rancidity +When food containing fats and oils are exposed to the atmosphere, the oxidation of fat and oil +occurs, this is known as Rancidity . +Methods to Prevent Rancidity + Store cooking oils from direct sunlight. + Food should be placed at low temperature. + By adding antioxidants food can be protected from rancidity. + Packing material should replace the air with nitrogen. + Minimize the use of salts in fried foods.���M GTs��� %@)J-9105$9==h@�D�HwL�PpT�V�Z�^�`Gc�ej6n(r:s�s�w�{�}݀��G�,�T�w�q�`���ȟʣ����خ �6����� ������k���3�������[�p����� ����F�j0 +=NW1"&G)l-�1�5�9�=�AjEoI�M�Q�U�Y�]�a�e�i�m�q^u�u@vMzD~Y�����Ȍ�����������d�P�p���0�&���]���Y�q��G�_�^���e�6������������(�C�@�g����A %��j,�� $�'~+�.�g +�5��ꋼ�(Ƽ1�b���(�t�2�O7e/��<��=G<4~"<�<ꪉ���o{;=���/��<�r<|��ˑȼ(o9�R+=��J��<<(gợߴ<� =�c�<�TS=���-"-= 9��ԯļ�n����;-_"�:,p= �&���[ҹ<�-=\����Dt<��?��݆�n�D<���<���;(/a�-it<�]3=m�=Rc�;�&�<~5�<ޗ�s=�wE<�<;@����B���&����;����ȾQ����M�������; =�����L=8M3���&�F�6=� �=e<9m�;8�b=O*=�~mB<������Լ�����Y';�;��f����;/U���� �As+��� ���j:��ּcy�<��< �;���<�\���O�:�ض<qY�|-���dk��KD=�a=E-�<�t���k���t=����G���u�< �w<0#=a"��k�׺�"�<� =˴(=�z�=2/F�s�=� �K�<=�\=��3<��4�{�<�����M=U��<Ⱥ�<��+�;�=��0���`���N=zĘ�s��;�U&����}����V>*'���ʼ��།���' �.-;�q���_����6��nhZ;����~�j<���;37,=<�+���X=uֻ����<�d3=������=��\s �.-<\�=���;w�L�bUA=H�2����;�e = �:��o��\��<���<�������e��>����=݅?=S3���%9�� u�< Je�Rx�=�\=�=��;�<�֊=� =��~=��8�h8=M*�-ق�����#=g�(�ħ����P��:c3%=d��<�9!=��>�v�<���=)z����;�a��f��Y��ut�c=��;Q����&=.���MH�;w}H=�hF9�;����K+J�.��7�Z�;��96=mmk=!2��Or���銽���Y،<5��� +¶�<�,��ג�2�#��To=M�<� �;RA<&3�dhU;�[=:�*��B.���3���=���<�[=�"C�R�I<����Ú��觻1�:�P�;)G!:td�<кB����;�B��< �٦1��M����B��m��f�< N=�ݼy��;�b�� ��d�n=hk�+�U�<{.:" %�7��������<��5=85�S��<������<>̛�����K����<�r=�7���v��m�;�(q�0w�Q���V�Cئ;W�=�>K��m�1�ռ +����T�<�F��]c�!�;ɂZ����;C�;��ϼ8��<����W�һ �:��+E�/�:g;=�H�W�ӻ����y�2�!Ml=�=�ѕ;�@<�)м��T��jw<1C�<�c��=oA:��u�j~3<Pʼ}=�� ����������<��i-�R� 9��l;��F�@�=q�"��C �h����������;��0�ɛ�<\d=a�2�Tar<�X <�q=Uf[=��<9ܚ�q�ͻ����Q�<��<΃=�B���1����������=2лWB�ƥ5<��<�p=b|2�&�=%�<6a���+9��T�=W`�sС��^鴼&�>= ݘ�3'w<�%I�t��<��(=^׻$��:ir0< ?�x �����hȯ<��< V_ƥ���ͻ����a(���#��(��8�<�� +����=!�=ic-��K��Z�;��=z1��g��<�a�<�[*=Y���-�<����<=W��=v=IX�;u�=�����:���=�_4���P�(��b�;�1��)���fAn���06�W��:�"�J<[H�=��<��˅��� +=5銼[���i���`^�W؟<�'<���<*�;��<����8&=��Z���z�\g~��;�:M�=6�#��N���N=�Γ�~-����;�*��'=��6e���=�`$<�]!���S=�M����J<�3����~��@=��E:8w3=�����8<���<��<#�Q=�p�=Hu�m=?α�وO=:\>=�I�<�E��!�<��;�g��Yp9=�o <�L�<����<6�<P��������;i�(�V�#������ۼ \��ݺ�5 �X�e�z.�<��<�u+=�(�=�LE�'�����'=I͐<�';�o�<���<M�;YV�;��d9Ȗ�<��9��M��I�<��O=� Q;���;$d�qa=�m=�;$=����db<)�=�읽�7N=:]��F�ؼ��=��<(4$<����X=H<�)Ώ��g�����3�<2�A��y; 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