CONTENTS
•Syllabus
v - viii
•
Solved Paper (KVS), 2016 Agra region
•
Solved Paper (KVS), 2016 Guwahati region
17 - 24
•
Solved Paper (KVS), 2016 Mumbai region
25 - 32
•On Tips Notes



9 - 16
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

( iii )
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
Unit I
Some Basic Concepts of Chemistry
12
Unit II
Structure of Atom
14
Unit III
Classification of Elements and Periodicity in Properties
08
Unit IV
Chemical Bonding and Molecular Structure
14
Unit V
States of Matter: Gases and Liquids
12
Unit VI
Chemical Thermodynamics
16
Unit VII
Equilibrium
14
Unit VIII
Redox Reactions
06
Unit IX
Hydrogen
08
Unit X
s -Block Elements
10
Unit XI
Some p -Block Elements
14
Unit XII
Organic Chemistry: Some basic Principles and Techniques
14
Unit XIII
Hydrocarbons
12
Unit XIV
Environmental Chemistry
06
Total
160
Marks
11
04
21
16
18
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 atomic
number 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)
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
ijh{kk lEcU/kh vko';d tkudkjh
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 importance
of Sodium and Potassium.
Calcium Oxide and Calcium Carbonate and their industrial uses, biological importance of Magnesium and
Calcium.
Unit XI : Some p-Block Elements
General Introduction to p-Block Elements
14 Periods
( vi )
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, Boronphysical 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. Important
compounds 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 IUPAC
nomenclature of organic compounds. Electronic displacements in a covalent bond : inductive effect, electromeric
effect, 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), physical
properties, chemical reactions including free radical mechanism or halogenation, combustion and pyrolysis.
Alkenes - Nomenclature, structure of double bond (ethene) geometrical isomerism, physical properties, methods
of preparation; chemical reactions : addition of hydrogen, halogen, water, hydrogen halides (Markownikov's
addition 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 halides
and water.
Aromatic hydrocarbons : Introduction, IUPAC nomenclature; Benzene : resonance aromaticity ; chemical
properties : mechanism of electrophilic substitution - nitration sulphonation, halogenation, Friedel Craft's
alkylation and acylation : directive influence of functional group in monosubstituted benzene; carcinogenicity
and toxicity.
Unit XIV : Environmental Chemistry
06 Periods
Environmental pollution - air, water and soil pollution, chemical reactions in atmosphere, smog, major atmospheric
pollutants; acid rain, ozone and its reactions, effects of depletion of ozone layer, greenhouse effect and global
warming - 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
Volumetric Analysis
Salt Analysis
Content Based Experiment
Project Work
Class record and viva
Marks
08
08
06
04
04
30
Total
( vii )
CHEMISTRY CLASS-XI, QUESTION PAPER DESIGN (CODE NO. 043) 2016-17
S. Typology of Questions
No.
Short
Answer
-II
(SA-II)
(3 mark)
Value
Based
Question
(4 mark)
Long
Answer
(LA)
(5 mark)
Total
Marks
%
Weightage
Remembering- (Knowledge
based Simple recall
questions, to know specific
facts, terms, concepts,
principles, or theories,
Identify, define,or recite,
information)
2
1
1
–
–
7
10%
2.
UnderstandingComprehension -to be
familiar with meaning and
to understand conceptually,
interpret, compare, contrast,
explain, paraphrase
information)
–
2
4
–
1
21
30%
3.
Application (Use abstract
information in concrete
situation, to apply
knowledge to new situations,
Use given content to
interpret a situation, provide
an example, or solve a
problem)
–
2
4
–
1
21
30%
4.
High Order Thinking Skills
(Analysis & SynthesisClassify, compare, contrast,
or differentiate between
different pieces of
information, Organize and/
or integrate unique pieces of
information from a variety
of sources)
2
–
1
–
1
10
14%
5.
Evaluation - (Appraise,
judge, and/or justify the
value or worth of a decisionc
or outcome, or to predict
outcomes based on values)
1
–
2
1
–
11
16%
5×1=5
5×2=10
12×3=36
1×4=4
3×5=15
70(26)
100%
Type of Questions
VSA
SA-I
SA-II
VBQ
LA
Total
2.
Short
Answer
-I
(SA-I)
(2 mark)
1.
TOTAL
1.
Very
Short
Answer
(VSA)
(1 mark)
QUESTION WISE BREAK UP
Mark per Question
Total No. of Questions
1
5
2
5
3
12
4
1
5
3
26
Total Marks
05
10
36
04
15
70
Internal Choice : There is no overall choice in the paper. However, there is an internal choice in one question of 2
marks weightage, one question of 3 marks weightage and all the three questions of 5 marks weightage.
The above template is only a sample. Suitable internal variations may be made for generating similar templates
keeping the overall weightage to different form of questions and typology of questions same.
( viii )
KENDRIYA VIDYALAYA SANGATHAN
(AGRA REGION)
SESSION ENDING EXAMINATION 2015-16
SUBJECT : CHEMISTRY
CLASS–XI
(SOLVED PAPER)
Time : 3 Hrs.
M.M. : 70
General Instructions :
1.
2.
3.
4.
5.
6.
7.
ll the questions are compulsory.
A
Q. No. 1 to 5 are very short answer questions and carry 1 mark each.
Q. No. 6 to 10 are short answer questions and carry 2 marks each.
Q. No. 11 to 22 are also short answer questions and carry 3 marks each.
Q. No. 23 is a value based question and carry 4 marks.
Q. No. 24 to 26 are long answer questions and carry 5 marks each.
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 :
∆ catalyst
(a)C3H8 + 3H2O 
→
Heat
(b) Zn + NaOH → 2
10.
Write IUPAC names of the following :
(b)
(a) Cl
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
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