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ON TIPS NOTES Note making is a skill that we use in many walks of life : at school, university and in the world of work. However, accurate note making requires a thorough understanding of concepts. We, at Oswaal, have tried to encapsulate all the chapters from the given syllabus into the following ON TIPS NOTES. These notes will not only facilitate better understanding of concepts, but will also ensure that each and every concept is taken up and every chapter is covered in totality. So go ahead and use these to your advantage… go get the OSWAAL ADVANTAGE!! CHAPTER 1 : Chemical Reactions and Equations Key Points and Concepts A complete chemical equation represents the reactants, products, conditions of reactions and their physical states symbolically. Oxidation : loss of electrons. Reduction : gain of electrons. Important Equations Types of Reactions : S. No. 1. 2. 3. 4. 5. 6. Name and Definition Example In a combination reaction, two or more reactants combine to give a single product. In a decomposition reaction, a single reactant breaks down into two or more simpler products. When decomposition reaction is carried out by heating, it is called thermal decomposition reaction. CaO(s) (Quick lime) (Lead nitrate) In a displacement reaction, a more reactive element displaces a less reactive element from a compound. H2O(l) → Ca(OH)2(aq) (water) 2Pb(NO3)2 Heat → → (Calcium carbonate) 2H2O(l) Fe(s) (Oxygen) CaO(s) + CO2(g) (Quicklime) Sunlight → 2Ag(s) + Br2(g) (Silver) Electric current → 2H2(g) (Water) (Iron) + O2(g) (Nitrogen dioxide) Heat CaCO3(s) (Slaked lime) 2PbO(s) + 4NO2(g) (2PbO) When decomposition reaction is 2AgBr(s) carried out in the presence of sunlight, (Silver bromide) the process is called photochemical decomposition. Electrolysis : When decomposition reaction is carried out with the help of electric current, the process is called electrolysis. + (Bromine) + (Hydrogen gas) + CuSO4(aq) (Copper sulphate) → FeSO4(aq) (Iron sulphate) O2(g) (Oxygen gas) + Cu(s) (Copper) On Tips Notes 7. 9 Na2SO4(aq) + BaCl2(aq) → BaSO4(s) + 2NaCl(aq) The reactions in which two different atoms or groups of atoms are displaced by other atoms or groups of atoms, i.e., two compounds exchange their ions and one of the products formed is insoluble, are said to be double displacement reactions. 8. (Sodium sulphate) The reactions in which acid or acidic oxide reacts with the base or basic oxides to form salt and water are called neutralization reactions. (Barium chloride) 2NaOH + (Sodium hydroxide) (Barium sulphate) (Sodium) chloride) H2SO4 → Na2SO4 + 2H2O (Sulphuric acid) (Sodium sulphate) (Water) Some usually asked equations in exams for balancing : 2CO(g) l + (Carbon monoxide) → O2(g) (Oxygen) 2CO2(g) (Carbon dioxide) Heat l l l → ZnCO3 ZnO + CO2 2FeSO4(s) → Fe2O3(s) + SO2(g) + SO3(g) Pb(NO3)2 + 2KI → 2KNO3 + (Lead nitrate) l CaO(s) (Quick lime) l l NaCl (Sodium chloride) (Potassium iodide) + H2O → (Potassium nitrate) Ca(OH)2 PbI2 (Lead Iodide) + Heat (Slaked lime) + AgNO3 → (Silver nitrate) AgCl + NaNO3 (Silver chloride) (Sodium nitrate) Ca + 2HNO3 → Ca(NO3)2 + H2 ↑ l Mg + 2HNO3 → Mg(NO3)2 + H2 ↑ l 2Al + 3H2SO4 → Al2(SO4)3 + 3H2 ↑ l Na2CO3 + 2HCl → 2NaCl + H2O + CO2 l Ca(OH)2 + CO2 → CaCO3 + H2O l Zn + H2SO4 → ZnSO4 + H2 ↑ l Zn + 2HCl → ZnCl2 + H2 ↑ l 4Zn + 10HNO3 → 4Zn(NO3)2 + 5H2O + N2O l Zn + 2NaOH Heat → Na2ZnO2 + H2 ↑ Redox (Oxidation and Reduction) Reaction : Oxidation (HCl is oxidized) MnO2 (s) +4HCl (conc.) MnCl 2(aq) +Cl 2(g) + 2H 2O Reduction (MnO2 is reduced) CHAPTER 2 : Acids, Bases and Salts Key Points and Concepts Those substances which turn blue litmus solution into red are called acids. Acids are sour in taste. They give H+ ions in aqueous solution. e.g. : HCl, H2SO4, HNO3, CH3COOH