CONTENTS

•Syllabus v - viii

• Solved Paper (KVS), 2016 Agra region 9 - 16

• Solved Paper (KVS), 2016 Guwahati region 17 - 24

• Solved Paper (KVS), 2016 Mumbai region 25 - 32

•On Tips Notes 33 - 72

Sample Question Papers (Solved)

Sample Question Paper - 1 73 - 76

Sample Question Paper - 2 77 - 79

Sample Question Paper - 3 80 - 82

Sample Question Paper - 4 83 - 85

Sample Question Paper - 5 86 - 88

Sample Question Papers for self assessment

Sample Question Paper - 6 89 - 91

Sample Question Paper - 7 92 - 94

Sample Question Paper - 8 95 - 97

Sample Question Paper - 9 98 - 100

Sample Question Paper - 10 101 - 104

Solutions

Sample Question Paper - 1 105 - 111

Sample Question Paper - 2 112 - 117

Sample Question Paper - 3 118 - 123

Sample Question Paper - 4 124 - 130

Sample Question Paper - 5 131 - 136

* SOLUTIONS for Sample Question Paper 6 to 10 can be downloaded from

www.OswaalBooks.com

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Latest Syllabus for Academic Year 2016-17

CHEMISTRY (Code No. 043)Total Periods (Theory 160 + Practical 60)

Time : 3 hours Total Marks 70

Unit No. Title No. of Periods Marks

Unit I Some Basic Concepts of Chemistry 12

Unit II Structure of Atom 1411

Unit III Classification of Elements and Periodicity in Properties 08 04

Unit IV Chemical Bonding and Molecular Structure 14

Unit V States of Matter: Gases and Liquids 12

Unit VI Chemical Thermodynamics 1621

Unit VII Equilibrium 14

Unit VIII Redox Reactions 06

Unit IX Hydrogen 08

Unit X s -Block Elements 1016

Unit XI Some p -Block Elements 14

Unit XII Organic Chemistry: Some basic Principles and Techniques 14

Unit XIII Hydrocarbons 12 18

Unit XIV Environmental Chemistry 06

Total 160 70

Unit I : Some Basic Concepts of Chemistry 12 Periods

General Introduction : Importance and scope of chemistry.

Nature of matter, laws of chemical combination. Dalton's atomic theory : concept of elements, atoms and

molecules.

Atomic and molecular masses. Mole concept and molar mass : percentage composition, empirical and molecular

formula; chemical reactions, stoichiometry and calculations based on stoichiometry.

Unit II : Structure of Atom 14 Periods

Discovery of electron, proton and neutron; atomic number, isotopes and isobars. Thomson's model and its

limitations, Rutherford's model and its limitations. Bohr's model and its limitations, concept of shells and

subshells, dual nature of matter and light, De Broglie's relationship, Heisenberg uncertainty principle, concept

of orbitals, quantum numbers, shapes of s, p and d orbitals, rules for filling electrons in orbitals - Aufbau

principle, Pauli’s exclusion principle and Hund's rule, electronic configuration of atoms, stability of half filled

and completely filled orbitals.

Unit III : Classification of Elements and Periodicity in Properties 08 Periods

Significance of classification, brief history of the development of periodic table, modern periodic law and the

present form of periodic table, periodic trends in properties of elements-atomic radii, ionic radii, inert gas radii.

Ionization enthalpy, electron gain enthalpy, electronegativity, valency. Nomenclature of elements with atomicnumber greater then 100.

Unit IV : Chemical Bonding and Molecular Structure 14 Periods

Valence electrons, ionic bond, covalent bond : bond parameters. Lewis structure, polar character of covalent

bond, covalent character of ionic bond, valence bond theory, resonance, geometry of covalent molecules,

( v )

ijh{kk lEcU/kh vko';d tkudkjh

VSEPR theory, concept of hybridization, involving s, p and d orbitals and shapes of some simple molecules,

molecular orbital; theory of homonuclear diatomic molecules (qualitative idea only), hydrogen bond.

Unit V : States of Matter : Gases and Liquids 12 Periods

Three states of matter. Intermolecular interactions, types of bonding, melting and boiling points. Role of gas

laws in elucidating the concept of the molecule, Boyle's law. Charles law, Gay Lussac's law, Avogadro's law.

Ideal behaviour, empirical derivation of gas equation, Avogadro's number. Ideal gas equation. Derivation from

ideal behaviour, liquefaction of gases, critical temperature. Kinetic energy and molecular speeds (elementary

idea). Liquid State - Vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical

derivations).

Unit VI : Chemical Thermodynamics 16 Periods

Concepts of System, types of systems, surroundings. Work, heat, energy, extensive and intensive properties,

state functions.

First law of thermodynamics - internal energy and enthalpy, heat capacity and specific heat, measurement of

∆U and ∆H, Hess's law of constant heat summation, enthalpy of bond dissociation, combustion, formation,

atomization, sublimation. Phase transition, ionization, Solution and dilution. Second law of thermodynamics

(brief introduction)

Introduction of entropy as a state function, Gibbs energy change for spontaneous and non-spontaneous

processes, criteria for equilibrium. Third law of thermodynamics (brief introduction).

Unit VII : Equilibrium 14 Periods

Equilibrium in physical and chemical processes, dynamic nature of equilibrium, law of mass action, equilibrium

constant, factors affecting equilibrium - Le Chatelier's principle; ionic equilibrium - ionization of acids and

bases, strong and weak electrolytes, degree of ionization, ionozation of poly basic acids, acid strength, concept

of pH. Henderson equation hydrolysis of salts (elementary idea). buffer, solutions, solubility product, common

ion effect (with illustrative examples).

Unit VIII : Redox Reactions 06 Periods

Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions, in terms of

loss and gain of electrons and change in oxidation number, applications of redox reactions.

Unit IX : Hydrogen 08 Periods

Position of hydrogen in periodic table, occurrence, isotopes, preparation, properties and uses of hydrogen;

hydrides - ionic, covalent and interstitial; physical and chemical properties of water, heavy water; hydrogen

peroxide-preparation, reactions and structure and use; hydrogen as a fuel.

Unit X : s-Block Elements (Alkali and Alkaline Earth Metals) 10 Periods

Group 1 and Group 2 elements :

General introduction, electronic configuration, occurrence, anomalous properties of the first element of each

group, diagonal relationship, trends in the variation of properties (such as ionization enthalpy, atomic and ionic

radii), trends in chemical reactivity with oxygen, water, hydrogen and halogens; uses.

Preparation and properties of some important compounds :

Sodium Carbonate, Sodium Chloride, Sodium Hydroxide and Sodium Hydrogencarbonate, Biological importanceof Sodium and Potassium.

Calcium Oxide and Calcium Carbonate and their industrial uses, biological importance of Magnesium andCalcium.

Unit XI : Some p-Block Elements 14 Periods

General Introduction to p-Block Elements

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Group 13 elements : General introduction, electronic configuration, occurrence. Variation of properties,oxidation states, trends in chemical reactivity, anomalous properties of first element of the group, Boron-physical and chemical properties, some important compounds : Borax, Boric acids, Boron Hydrides. Aluminium:Reactions with acids and alkalies, uses.

Group 14 elements : General introduction, electronic configuration, occurrence, variation of properties,oxidation states, trends in chemical reactivity, anomalous behaviour of first element, Carbon- catenation,allotropic forms, physical and chemical properties; uses of some important compounds : oxides. Importantcompounds of Silicon and a few uses: Silicon Tetrachloride, Silicones, Silicates and Zeolites their uses.

Unit XII : Organic Chemistry - Some Basic Principles and Technique 14 Periods

General introduction, methods of purification, qualitative and quantitative analysis, classification and IUPACnomenclature of organic compounds. Electronic displacements in a covalent bond : inductive effect, electromericeffect, resonance and hyper conjugation. Homolytic and heterolytic fission of a covalent bond : free radicals,carbocations, carbanions; electrophiles and nucleophiles, types of organic reactions.

Unit XIII : Hydrocarbons 12 Periods

Classification of hydrocarbons

Aliphatic Hydrocarbons : Alkanes - Nomenclature, isomerism, conformations (ethane only), physicalproperties, chemical reactions including free radical mechanism or halogenation, combustion and pyrolysis.

Alkenes - Nomenclature, structure of double bond (ethene) geometrical isomerism, physical properties, methodsof preparation; chemical reactions : addition of hydrogen, halogen, water, hydrogen halides (Markownikov'saddition and peroxide effect), ozonolysis, oxidation, mechanism of electrophilic addition.

Alkynes - Nomenclature, structure of triple bond (ethyne), physical properties. Methods of preparation,chemical reactions : acidic character of alkynes, addition reaction of hydrogen, halogens, hydrogen halidesand water.

Aromatic hydrocarbons : Introduction, IUPAC nomenclature; Benzene : resonance aromaticity ; chemicalproperties : mechanism of electrophilic substitution - nitration sulphonation, halogenation, Friedel Craft'salkylation and acylation : directive influence of functional group in monosubstituted benzene; carcinogenicityand toxicity.

Unit XIV : Environmental Chemistry 06 Periods

Environmental pollution - air, water and soil pollution, chemical reactions in atmosphere, smog, major atmosphericpollutants; acid rain, ozone and its reactions, effects of depletion of ozone layer, greenhouse effect and globalwarming - pollution due to industrial wastes; green chemistry as an alternative tool for reducing pollution,strategies for control of environmental pollution.

PRACTICALS

Evaluation Scheme for Examination Marks

Volumetric Analysis 08

Salt Analysis 08

Content Based Experiment 06

Project Work 04

Class record and viva 04

Total 30

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CHEMISTRY CLASS-XI, QUESTION PAPER DESIGN (CODE NO. 043) 2016-17

S. Typology of Questions Very Short Short Value Long Total %No. Short Answer Answer Based Answer Marks Weightage

Answer -I -II Quest- (LA)(VSA) (SA-I) (SA-II) ion

(1 mark) (2 mark) (3 mark) (4 mark) (5 mark)

1. Remembering- (Knowledge 2 1 1 – – 7 10% based Simple recallquestions, to know specificfacts, terms, concepts,principles, or theories,Identify, define,or recite,information)

2. Understanding- – 2 4 – 1 21 30%Comprehension -to befamiliar with meaning andto understand conceptually,interpret, compare, contrast,explain, paraphraseinformation)

3. Application (Use abstract – 2 4 – 1 21 30%information in concretesituation, to applyknowledge to new situations,Use given content tointerpret a situation, providean example, or solve aproblem)

4. High Order Thinking Skills 2 – 1 – 1 10 14%(Analysis & Synthesis-Classify, compare, contrast,or differentiate betweendifferent pieces ofinformation, Organize and/or integrate unique pieces ofinformation from a varietyof sources)

5. Evaluation - (Appraise, 1 – 2 1 – 11 16%judge, and/or justify thevalue or worth of a decisioncor outcome, or to predictoutcomes based on values)

TOTAL 5×1=5 5×2=10 12×3=36 1×4=4 3×5=15 70(26) 100%

QUESTION WISE BREAK UP

Type of Questions Mark per Question Total No. of Questions Total Marks

VSA 1 5 05SA-I 2 5 10SA-II 3 12 36VBQ 4 1 04LA 5 3 15

Total 26 70

1. Internal Choice : There is no overall choice in the paper. However, there is an internal choice in one question of 2marks weightage, one question of 3 marks weightage and all the three questions of 5 marks weightage.

2. The above template is only a sample. Suitable internal variations may be made for generating similar templateskeeping the overall weightage to different form of questions and typology of questions same.

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KENDRIYA VIDYALAYA SANGATHAN(AGRA REGION)

SESSION ENDING EXAMINATION 2015-16SUBJECT : CHEMISTRY

CLASS–XI(SOLVED PAPER)

Time : 3 Hrs. M.M. : 70

General Instructions : 1. All the questions are compulsory. 2. Q. No. 1 to 5 are very short answer questions and carry 1 mark each. 3. Q. No. 6 to 10 are short answer questions and carry 2 marks each. 4. Q. No. 11 to 22 are also short answer questions and carry 3 marks each. 5. Q. No. 23 is a value based question and carry 4 marks. 6. Q. No. 24 to 26 are long answer questions and carry 5 marks each. 7. Use log tables if necessary, use of calculators is not allowed.

1. How may significant figures exist in the value 0.01001 ? 1 2. Name the species which is isoelectronic with N3– ? 1 3. Complete the following equation : 1 CaC2 + H2O → ............. + ............. 4. What is the oxidation state of O in Na2O2 ? 1 5. Potassium carbonate cannot be prepared by Solvay process, why ? 1 6. A sample of drinking water was found to be severely contaminated with chloroform, CHCl3. Supposed to be

carcinogenic in nature. The level of contamination was 15 ppm (by mass). (i) Express this percent by mass, (ii) Determine the molality of chloroform in the water sample. 2 7. A hydrate of iron (III) thiocyanate [Fe(SCN)3. mH2O] was found to contain 19% water. Find out the value of m. 2 8. What is the total number of sigma and pi bond in the following molecules ? 2 (a) C6H6

(b) C2H4

OR Why is sigma bond stronger than pi bond ? Explain. 9. Complete the following equations :

(a) C3H8 + 3H2O catalyst∆→

(b) Zn + NaOH Heat→ 2

10. Write IUPAC names of the following :

(a)

Cl

(b)

H

11. (a) What will be the mass of one molecule of CO2 ? (b) Give the no. of electrons in the species He, He+, Li2+, H+

2. 3 12. (a) State Heisenberg uncertainty principle. (b) A microscope using suitable photons is employed to located an electron in an atom within distance of 0.1 A°.

What is the uncertainty involved in the measurement of its velocity ? 3 13. (a) Show by chemical reaction with water that Na2O is a basic oxide and Cl2O7 is an acidic oxide. (b) In terms of period and group where would you located the element with Z = 144 ? 3 14. What is Hybridisation ? Explain. What will be the state of the hybridization of the central atom in each of the

following species : CCl2F2, BF3, NF3, BeF2. 3 15. What is smog ? How is classical smog differ from photochemical smog ? What is meant by biological oxygen

demand (BOD) ? 3

continue

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