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• Latest Syllabus and Blueprint 5 - 12 • II PUC Solved Examination Paper - July 2016 13 - 23• II PUC Solved Examination Paper - April 2016 24 - 32• II PUC Solved Examination Paper - March 2016 33 - 42 • Topper Answers - March 2015 43 - 56

CONTENT

Chapter 1. Solid State 57 - 79 l�Topic 1 Classification of Soilds based on different

binding forces, Crystal lattices, Unit cell, packing in solids, Packing efficiency, voids, calculation of density of unit cell.

l�Topic 2 Defects in electrical and magnetic prope-rties, Band theory of metals.

Chapter 2 . Solutions 80 - 104 l�Topic 1 Types of Solutions, Expression of concent-

ration of solutions of solids in liquids, solu- bility of gases in liquids, solid solutions.

l�Topic 2 Vapour pressure, Raoult's law, Ideal and Non-ideal solutions.

l�Topic 3 Colligative properties, Determination of molar mass, Abnormal molar mass, Van't Hoff factor.

Chapter 3. Electro-Chemistry 105 - 124 l�Topic 1 Conductance in Electrolytic solutions,

Specific and Molar Conductivity, Variations of Conductivity with concentration, Gibb's energy, Kohlrausch's Law.

l�Topic 2 Redox reaction, Electrochemical cell, Galvanic cell, EMF of cell, Standard electrode potential, Nernst equation.

l�Topic 3 Electrolysis, Laws of electrolysis, Batteries, Fuel, cells and Corrosion.

Chapter 4. Chemical Kinetics 125 - 143 l�Topic 1 Rate of chemical reaction and factors

affecting rate of reaction. l�Topic 2 Order of a reaction, integrated rate

equations and Half life of a reaction. l�Topic 3 Concept of Collision theory, Activation

energy and Arrhenius equation. Chapter 5. Surface Chemistry 144 - 158 l�Topic 1 Adsorption and its types, Factors affecting

Adsorption and Applications. l�Topic 2 Catalysis and its types, Enzyme catalysis.

l�Topic 3 Colloids, Types of Colloids, Characteristics and preparation of Colloids.

Chapter 6. General Principles and Processes of Isolation of Elements 159 - 178

l�Topic 1 Principles and Methods of Extraction.l�Topic 2 Principles of Extraction of Aluminium

Copper, Zinc and Iron. Chapter 7. p-Block Elements 179 - 209 l�Topic 1 Group-15 Elements their properties and

Some important compounds.

l Topic 2 Group-16 Elements, their properties and Some Important compounds.

l�Topic 3 Group-17 Elements, their properties and Some Important compounds.

l�Topic 4 Group-18 Elements, their properties and some important compounds.

Chapter 8. d-Block and f-Block Elements 210 - 230 l�Topic 1 d-Block Elements , their propert ies

compounds. l�Topic 2 f-Block Elements, Lanthanoids and

Actinoids. Chapter 9 . Co-Ordination Compounds 231 - 246 l�Topic 1 Co-ordination compounds and their

properties, IUPAC nomenclature of Mono nuclear Co-ordination compounds.

l�Topic 2 Werner's Theory Bonding in Co-ordination Compounds, VBT, CFT and importance of Co-ordination Compounds.

Chapter 10. Haloalkanes & Haloarenes 247 - 260 l�Topic 1 Some important terms and definitions. l�Topic 2 Properties of Haloarenes and Haloalkanes . Chapter 11. Alcohols, Phenols and Ethers 261 - 280 l�Topic 1 Alcohols, Phenols and Ethers. l�Topic 2 Methods of preparation of Alkanols. l�Topic 3 Phenols l�Topic 4 Classification and nomenclature of Ethers. Chapter 12. Aldehydes, Ketones and Carboxylic Acid 281 - 298 l�Topic 1 Aldehydes, Ketones and Carboxylic acids. l�Topic 2 Methods of Preparation of Aldehydes and

Ketones. l�Topic 3 Methods of preparation of Carboxylic acid,

properties and Uses. Chapter 13.Organic compounds containing Nitrogen 299 - 312 l�Topic 1 Amines : Methods of preparation, Physical

and Chemical properties, uses. l�Topic 2 Cyanides, Isocyanides and and Diazonium

salts preparation, Physical and Chemical properties, uses.

Chapter 14. Biomolecules 313 - 323 l�Topic 1 Carbohydrates, their classification and

Importance. l�Topic 2 Proteins, Hormones, Vitamins and Nucleic

Acids. Chapter 15. Polymers 324 - 336

PREFACE

Malcolm Forbes said “Education's purpose is to replace an empty mind with an open one” and this is something which is always followed by Directorate of Pre-University Education whether through their education system framework or regular enhancement in curriculum. The aim of the curriculum is not just to let learners obtain basic knowledge but to make them life-long learners.

The purpose of this book is to nurture individuality and thus enhance one's innate potentials which help in increasing the self-study mode for students. This book strengthens knowledge and attitude related to subject. This book is designed in such a way that students can set their own goals and can improve their problem solving and thinking skills.

This book is strictly as per the latest blueprint & syllabus for II PUC examination. It contains variety of questions from textbooks. It contains all types of questions necessary for exam oriented preparation. A synopsis is given for every chapter which contains important points from that chapter. Each chapter has high quality figures wherever required for better, fast and clear understanding.

OSWAAL II PUC Question Bank is different and better in terms of High Quality Questions which are developed by 'OSWAAL Expert Panel' which ensures success in examination. The Question Bank is arranged ‘Topic-Wise’ where each topic from every chapter is explained in detail. ‘SCHEME OF VALUATION’ answer are highlighted to develop student understanding of Marking scheme. It also adheres to the blueprint which enables exam oriented preparation.

Through OSWAAL Books students are taught how to think, not what to think. We at OSWAAL Books try to use quality content, standard language, creativity and high quality figures, which makes readers to enjoy it because we believe if our readers don't enjoy reading our book then there is no use in reading it at all. This is one of the reasons that the scope of this book extends from students to teachers. Teachers can use this book as a perfect teaching guide and students can use this book for good learning and practice.

At last we would like to thank our authors, editors, reviewers and specially students whom we request to send suggestions regularly which will help in continuous improvement of this book and will make this book “One of the Best”. Wish you all Happy Learning.

–Publisher

Why Topic Wise Question Banks are A Better Choice than Previous Year’s Papers ?

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1. Chapter-wise and Topic –wise resentation in Question Banks facilitates systematic study.

2. Question Banks can be referred to by the

students throughout the year as well as at

the completion of each chapter in school.

3. Question Banks, take into account any

changes in syllabus or layout and hence are

fully updated and aligned as per the latest

specifications by the Board.

Question Bank Previous Years' Paper

1. Year Wise presentation restricts methodical flow of learning.

2. These can be referred to only after the completion of the full syllabus in school.

3. Previous Years' questions cannot be changed and hence fail to be adept with the latest Board specifications

(5)

II PUC CHEMISTRY SYLLABUS BLOW-UP

UNIT-I Solid State 8 hrs

General characteristics of solids: amorphous and crystalline solids – examples, differences. Classification of crystalline solids – based on binding forces: molecular solids – (non-polar, polar, H-bonded), ionic solids, metallic solids, covalent or network solids – examples for all. Definitions – lattice point, crystal lattice, unit cell, coordination number. Parameters of a unit cell, names of seven crystal systems , calculation of number of atoms in a cubic unit cell – simple cubic, bcc, fcc. Close packing in two dimensional and three dimensional lattices - brief information, voids - types of voids, tetrahedral and octahedral and their relative numbers, calculation of the formula of the compounds based on the number of voids filled. Packing in solids - calculation of packing efficiency- fcc/ccp, bcc, simple cubic. Formula to calculate the density of the unit cell to be assumed- use the formula to calculate a, d , z , M , N . Numerical problems.A

Point defects-types, a brief account of Frenkel and Schottky defects, metal excess defect and metal deficiency defect with examples. Electrical properties: classification into conductors, insulators and semiconductors - their comparison based on band theory of metals, n- type and p-type semiconductors – differences and examples. Magnetic properties of substances – paramagnetism, diamagnetism and ferromagnetism, examples.

UNIT-II Solutions 9 hrs

Types of Solutions – binary – gaseous, liquid and solids, expressing the concentration of a solution of asolid in a liquid mole fraction, molarity and molality. Solubility, solubility of a gas in a liquid – Henry'slaw, graph of partial pressure of a gas vs its mole fraction in solution, effect of pressure, temperature, applications of Henry's law. Solution of liquid in liquid – Raoult's law- statement, mathematical expression, numerical problems, ideal solution – characteristics, graph, non - ideal solution –types - their characteristics and differences, examples, azeotropes – types, examples. Solution of a solid in a liquid – Raoult's law – colligative properties – relative lowering of vapour pressure, elevation in boiling point, depression in freezing point, graphs for elevation in boiling point and depression in freezing point, SI units for K , K , osmosis – osmotic pressure, isotonic, hypertonic, hypotonic solutions, b f

reverse osmosis – application in desalination of water. Numerical problems on determination of molar mass using colligative properties. Abnormal molar mass, van't Hoff factor i, value of i for non-electrolytes and solutes that associate or dissociate in dilute solution.

UNIT-III Electrochemistry 9 hrs Redox reaction – As fundamental reaction in electrochemical cells, electronic and electrolytic conductors – differences, strong and weak electrolytes, examples-Ionic conductance- factors affecting ionic conductance,conductivity and molar conductivity of electrolytic solutions definitions, mathematical expressions,relationship between them, SI units, numerical problems. Variation of conductivity and molar conductivity

0with concentration, graph for variation of,L vs for strong and weak electrolytes using equation L =L – A m m m

(measurement of conductivity from Wheatstone network not included), limiting molar conductivities,0Kohlrausch law and applications, numerical problems on calculation of L for weak electrolytes. Electrolysis m

n+–Faraday’s laws of electrolysis (elementary idea) , concept of nF required to discharge one mole of M ions, numerical problems on I law.Galvanic cells : Electrode potential , half cell concept, standard electrode potential, galvanic cell, Daniell cell,

0 0 0cell potential, EMF (emf), E = E –E . Measurement of electrode potential – SHE - diagram, half cellR L0 0representation, half cell reaction, E taken as ± 0.0 V (at all temperatures). Measurement of E of Zn and Cu

0 0 0using SHE (experimental details not expected) numerical problems on E = E E , importance of standard R L

electrode potentials- to decide and compare the strengths of oxidizing and reducing agents . Nernst equation (derivation not required) : Nernst equation at 298 K for single electrode potential and cell potential, numerical problems to calculate half cell and cell potentials (only for metal electrodes). Relationship between

0equilibrium constant and E (derivation not required), numerical problems. Relationship between standard cell

LATEST SYLLABUS(Issued by Department of PUE, Karnataka)

cc

...Contd.0Gibbs energy and E , numerical problems.cell

Factors affecting the products of electrolysis, examples – molten and aqueous solution of NaCl only.Batteries: types-difference, examples, Leclanche cell (dry cell) and Lead acid battery–anode, cathode, electrolyte, reactions at anode and cathode (diagram not required), Fuel cell – definition – examples, H -O fuel cell – schematic diagram, anode, cathode, electrolyte, reactions at anode and cathode.2 2

Corrosion – rusting of iron- anodic, cathodic reactions, composition of rust, methods of prevention.

UNIT-IV Chemical Kinetics 9 hrs

Rate of a reaction – average and instantaneous ,with graphs, SI unit, rate of a reaction expressed as rate ofchange in molar concentration of reactants and products using balanced equation, factors affecting rate of a reaction, dependence of rate on concentration – rate expression (rate law),specific rate constant, order, units for rate constant of zero, first and, second order reactions. Molecularity – uni, bi and termolecular reactions – examples. Derivation of integrated rate equation for the rate constant of zero and first order reactions, graphs for zero and first order reactions-analysis, half life – derivation of relationship between t and k for zero and first order 1/2

reactions. Numerical problems on first order and half life, Pseudo first order reaction- examples. Temperature dependence: Arrhenius equation – activation energy, energy distribution curve showing

temperature dependence of the rate of the reaction, problems based on log , graph of ln

k vs with intercept and slope. Effect of catalyst, explanation with graph. An elementary idea of collision

theory, criteria for effective collision – threshold energy and orientation factor.

UNIT-V Surface chemistry 6 hrs Adsorption: adsorbate, adsorbent, examples, distinction between adsorption and absorption. DH, DS and

DG for adsorption of gas on a solid. Physisorption and chemisorption-characteristics and differences. Factors

affecting adsorption of a gas on a solid. Applications (to be mentioned). Catalysis: homogeneous and heterogeneous catalysis, examples, activity and selectivity of a catalyst ,examples, shape selective catalysis, examples. Enzyme catalysis: examples, characteristics (to be mentioned), mechanism. Colloids: colloidal state-distinction of true solution, colloids, and suspension based on particle size. Classification of colloids-types of colloidal systems- examples, lyophilic and lyophobic— differences and examples, macromolecular, multimolecular and associated colloids, examples, formation of micelle, cleansing action of soaps. Preparation of colloids-chemical methods-sulphur and ferric hydroxide sols, Bredig's arc method for metal sols, peptisation. Purification– dialysis, electro-dialysis, ultrafiltration (in brief). Properties of colloids: Tyndall effect, Brownian movement, charge on colloidal particles, examples, electrophoresis, coagulation – methods of coagulation of lyophobic sols, Hardy- Schulze rule-examples, coagulating value. Protective colloid - example. Applications: In industries, medicines, purification of drinking water. Emulsions : types , examples.

UNIT-VI General Principles and Processes of Isolation of Elements 5 hrs

Principles and methods of extraction: concentration of ores – hydraulic washing, magnetic separation, froth floatation, leaching -of alumina from bauxite, roasting and calcination – examples. Occurrence (ores) of Al, Cu, Zn and Fe. Principles of extraction of aluminium, copper, zinc, iron: highlight the principle of extraction of iron from its oxide using Ellingham diagram. Extraction of iron from its oxides - blast furnace – diagram, reactions, equations as:

C + O ¾® CO CO + C ¾® 2CO, 2 2 2

Fe O + CO ¾® 2FeO + CO , FeO + CO ¾® Fe + Co 2 3 2 2

CaCO ¾® CaO + CO , CaO + SiO ¾® CaSiO . 3 2 2 3

Extraction of copper from sulphide ore containing iron impurity, extraction of zinc from zinc oxide, extraction of aluminium from purified alumina, oxidation-reduction - extraction of gold. Refining: principles and examples each for distillation, liquation, electrolytic method, zone refining, vapour phase refining- details for Mond's and Van Arkel processes.

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–

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° ù= ê ú

ë û1

T

UNIT-VII p-Block Elements 11 hrs

Group 15 elements - General introduction, occurrence, electronic configuration, oxidation states, anomalous behavior of nitrogen with reasons, trends in physical and chemical properties - reactivity towards hydrogen and oxygen.Dinitrogen: preparation- from (NH ) Cr O , laboratory method from NH Cl, properties and uses.4 2 2 7 4

Compounds of nitrogen: ammonia – manufacture by Haber's process, properties – basic character, reaction 2+with ZnSO and Cu ion. Nitric acid – manufacture by Ostwald's process , laboratory method – from NaNO , 4 3

properties – oxidizing properties – dilute HNO with Zn and Cu, concentrated HNO with Cu, Zn, I2 and 3 3

carbon , passivity with Al and Cr with reason, Brown ring test. Oxides of nitrogen – structures for NO, NO2

and N O only.2 5

Phosphorus: allotropic forms – white and red (brief account), phosphine – laboratory preparation, properties – basic nature, PCl and PCl – preparation from dry chlorine, properties- action on water (hydrolysis). 3 5

Oxoacids: hypophosphorous acid, orthophosphorous acid, orthophosphoric acid –formula, structure, reducing property, basicity. Group 16 elements - General introduction, occurrence, electronic configuration, oxidation states, anomalous behaviour of oxygen with reasons, trends in physical and chemical properties, reactivity with hydrogen and halogen.Dioxygen - preparation from KClO , properties- reaction with Al, CH , C, uses. Oxides – simple oxides – 3 4

classification – acidic, basic and amphoteric, examples.Ozone: preparation, properties, oxidising properties - with PbS and NO.Sulphur: allotropic forms - brief account of rhombic and monoclinic.

2–Compounds of sulphur : SO - laboratory preparation from SO , properties – reaction with NaOH, Cl , 2 3 23+ –reducing property – with Fe and MnO , uses, sulphuric acid: manufacture by contact process – flow chart 4

and equations, properties- acidic, dehydrating and oxidizing, reaction with metal halides (halide = F,Cl), uses.Oxoacids of sulphur: sulphurous acid, sulphuric acid, peroxodisulphuric acid and pyrosulphuric acid – formula, structure. Group 17 elements : General introduction, occurrence, electronic configuration, oxidation states, trends in physical and chemical properties, anomalous behaviour of fluorine with reasons, reactivity towards hydrogen and oxygen.Chlorine: preparation– from HCl with KMnO , properties – reaction with Al, S , H S, NH , NaOH, Ca(OH) , 4 8 2 3 2

oxidising property – with FeSO , Na SO , bleaching property, uses. Hydrogen chloride: laboratory 4 2 3

preparation, properties – acidic nature, reaction with NH , aqua regia, uses. Oxoacids of halogen: names, 3

formulae and structures of oxoacids of chlorine only.Interhalogen compounds: Preparation of ClF , ICl, BrF , properties- reactivity compared with halogens, 3 5

hydrolysis – general equation.Group 18 elements: General introduction, occurrence, electronic configuration, trends in physical and chemical properties – reason for their inertness, formation and formula of Bartlett compound, preparation of XeF and XeO , XeO F (by hydrolysis of XeF ), uses of noble gases.6 3 2 2 6

UNIT - VIII d and f Block Elements 9 hrs General introduction, electronic configuration, characteristics of transition metals (d-block) - variation in atomic and ionic size.Electronic configuration of 3d series elements, general trends in properties of the first row transition metals (3d series) – metallic character, ionization enthalpies, oxidation states, magnetic properties, colour, catalytic properties, formation of interstitial compounds, alloy formation.

–Potassium dichromate: preparation from chromite ore (FeCr O ). Properties – oxidizing property – with I , 2 42+ 2+H S, Sn , Fe , interconversion of chromates and dichromates in aqueous solution depending on pH.2

Potassium permanganate: Preparation from MnO by fusion with KOH and acidification. Properties-action of 2– 2+ 2– 2–heat, oxidising property – oxidation of I , Fe ,C O , H S in acidic medium, S O , I , in neutral / alkaline 2 4 2 2 3

medium.

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...Contd.

f-block elements: Lanthanoids-electronic configuration, atomic size – lanthanoid contraction and its consequences, oxidation states, chemical reactivity – general characteristics.Actinoids: electronic configuration, ionic size – actinoid contraction – compared to lanthanoid contraction, oxidation states– general characteristics compared with lanthanoids.

UNIT - IX Coordination Compounds 7 hrs

General introduction to salts, difference between double salt and coordination (complex salt) compound with respect to their ionization in water, with an example.Coordination entity, central metal ion, coordination number, coordination sphere, oxidation state of central metal ion, homoleptic and heteroleptic complexes , examples. Ligands -types-unidentate, didentate, polydentate, ambidentate, examples.Nomenclature of coordination compounds – mononuclear compounds. Werner's theory – postulates,

3– 3+ 2–limitations. VBT : salient features, application of VBT for the formation of - [CoF ] , [Co(NH ) ] , [NiCl ] , 6 3 6 4

[Ni(CN)4]2 , magnetic properties – low spin and high spin complexes with examples, limitations of VBT. CFT (crystal field theory): crystal field splitting-meaning, crystal field splitting in octahedral and tetrahedral coordination entities using energy level diagram and their comparison. Spectrochemical series, compare

weak field ligand – strong field ligand with respect to d4 ions in octahedral field ( D < P, D > P). Explanation 0 0

for colour of complexes using CFT, examples.Isomerism: Structural – linkage, ionization, solvate, coordination – definition and examples. Stereoisomerism – geometrical and optical, examples, facial and meridional as geometrical isomers- example. Importance of coordination compounds: In biological systems, qualitative analysis, extraction of metals, examples.

UNIT - X Haloalkanes and Haloarenes 7 hrs

Classification based on hybridization of carbon to which halogen is bonded-alkyl halides (haloalkane), allylic, benzylic, vinylic, aryl halides. Primary, secondary and tertiary alkyl halides, nomenclature, nature of C X bond. Preparation - From alcohols- using HCl / ZnCl , PX (Cl, Br), PCl , SOCl - general reactions and examples with 2 3 5 2

R = CH , C H , Halogen exchange method- Finkelstein reaction – general equation and examples with 3 2 5

R = CH , C H , X = Cl, Br, Swarts reaction – statement, example. Physical properties – density, melting point, 3 2 5

boiling point, solubility.Reactions of haloalkanes: Nucleophilic substitution reactions: with aqueous KOH / NaOH, alcoholic KCN, alcoholic AgCN, R'COOAg , general reactions, examples (R as CH and C H ).3 2 5

– –Mechanisms - S 1 and S 2 - HO and CH Cl for S 2, OH and tertiary butyl bromide for S 1 as examples. Trend N N 3 N N

in reactivity towards S 1 and S 2 - 1°, 2°, 3° haloalkanes and R – I, R – Br , R – Cl, with reasons. Optical N N

isomerism - optical activity, d form (+) and l form (–) isomers, chirality, enantiomers, racemic mixture, racemisation, examples. Reaction at a chiral carbon – inversion, retention, racemisation . Stereochemistry of 2-bromobutane and 2-bromooctane in S 1 and S 2 reaction, respectively.N N

Elimination reaction (b elimination)- dehydrohalogenation- general reaction, Zaitsev rule – statement,

example taking 2-bromopentane. Reaction with metals – organo - metallic compounds - Grignard reagent,(RMgX) ,general reaction, its preparation fromCH Br and C H Br, importance of dry ether.3 2 5

Haloarenes: Nucleophilic substitution reactions: reasons for haloarenes to be less reactive , replacement of Cl by hydroxyl group in chlorobenzene and nitro substituted chlorobenzenes to compare the reactivity when –NO group/s are in o- and p- positions .2

Electrophilic substitution reactions for chlorobenzene - chlorination, nitration, sulphonation, Friedel-Crafts reaction (alkylation, acetylation).Reaction with metals - Wurtz-Fittig reaction – statement – general reaction, example (R= CH and C H ). Fittig 3 2 5

reaction – statement, example – formation of biphenyl.Uses and environmental effects of dichloromethane, trichloromethane, tetrachloromethane, iodoform, freons and DDT.

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...Contd.

UNIT - XI Alcohols, Phenols and Ethers 8 hrs

Classification: mono, di, tri ,allylic, and benzylic alcohols, mono, di and trihydric phenols and cresols. Ethers – simple and mixed, nomenclature of alcohols, phenols, ethers.Preparation of alcohols: by acid catalysed hydration of alkene, general reaction and examples, by hydroboration-oxidation of propene, from carbonyl compounds: hydrogenation of aldehydes, ketones, reduction of carboxylic acids and using Grignard reagent- general reactions and examples (R as H, CH and 3

C H wherever applicable.2 5

Preparation of phenol: From i) benzene via sulphonation ii) diazonium salt iii) cumene. Physical properties of primary alcohols and phenol: Boiling point and solubility.Chemical properties of primary alcohols and phenol: discuss and compare acidic nature of alcohol and phenol ,with reasons. Effect of electron withdrawing groups(EWG) E.g.:NO and electron donating groups 2

(EDG) E.g.; –CH , on acid strength of phenol, with reasons. Esterification and acylation of alcohols/phenols- 3

general reactions, examples with R=CH , C H , conversion of salicylic ac d into aspirin. Dehydration of 3 2 5 i

alcohols, oxidation using PCC -general reactions, examples with R = CH , C H . Mechanism of dehydration of 3 2 5

ethanol into ethene.Identification of 1°, 2°, 3° alcohols: Lucas test–observation and ference, reaction in presence of heated copper, in

equations .Uses: methanol and ethanol Reactions of phenol: 1) Electrophilic substitution: a) with dil. HNO and conc. HNO b) Br in CS (0°C) and Br 3 3 2 2 2

/water c) Kolbe’s reaction d) Riemer-Tieman reaction 2) Reaction of phenol with zinc dust 3) Oxidation of phenol by air and by chromic acid. Uses of phenols. Ethers: Preparation - by dehydration of ethanol, Williamson’s ether synthesis – general reaction - for aliphatic and phenolic ethers, examples- giving reason for proper choice of reactants wherever applicable. Physical Properties: boiling points and solubility. Chemical reactions: discuss the reaction of ethers with HX (reactivity of HX to be compared).Electrophilic substitution reaction for anisole: bromination, nitration, acetylation, alkylation (methylation). Uses of ethers.

UNIT - XII Aldehydes, Ketones and Carboxylic acids 9 hrs

Aldehydes and ketones: nomenclature, nature of carbonyl group. M thods of preparation: Aldehydes- e

Stephen reduction – general reaction and examples (R=CH and C H ). Preparation of benzaldehyde -3 2 5

Rosenmund reduction, Etard reaction and Gatterman Koch reaction. Ketones-from RCOCl with dialkyl cadmium, Friedel-Crafts reaction – general reactions and examples (R=CH and C H ).3 2 5

Physical properties: boiling points and solubility.Chemical properties: Nucleophilic addition reactions- HCN and NaHSO - general reaction, and examples, -3

mechanism of addition (HCN) .Condensation reactions with derivatives of ammonia- NH OH, NH NH , NH NHC H , 2,4- DNPH, 2 2 2 2 6 5

Clemmensen and Wolff-Kishner reductions -general equations and examples by taking HCHO, CH CHO, 3

CH COCH , C H CHO. Tests to distinguish aldehydes from ketones - Tollens’ reagent and Fehling’s solution 3 3 6 5

(equation not required). Addition of alcohol to aldehyde (to form an acetal) and ethylene glycol to ketone –general equations and examples.For ketones: Haloform reaction for methyl ketones – general reaction, examples with CH COC H , 3 6 5

CH COCH .3 3

Reactions due to -hydrogen:

1. Reason for acidic nature of a -hydrogen

2. Aldol reaction: addition and condensation for CH CHO, CH COCH3 3 3

3. Crossed aldol condensation: between benzaldehyde and acetophenoneCannizzaro’s reaction (disproportionation reaction) for HCHO and C H CHO.6 5

Electrophilic substitution reaction: nitration of C H CHO. Uses of aldehydes and ketones.6 5

...Contd.

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Oswaal Karnataka II PUC QuestionBank With Complete Solutions ForChemistry For March 2017 Exams

Publisher : Oswaal Books ISBN : 9789386177032 Author : Panel Of Experts

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