JEE

MAIN

COMPLETE

CHEMISTRY



JEE

MAIN

COMPLETE

CHEMISTRY
K.L. Kapoor
Formerly Associate Professor,
Hindu College,
University of Delhi, Delhi

McGraw Hill Education (India) Private Limited
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Complete Chemistry—JEE Main
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To Our Readers...
How to Crack the JEE


T

o help students preparing for the JEE Main, there was need for a book which included a variety of Multiple Choice
Questions (MCQs) designed on the basis of the prescribed syllabus for this examination. This book is an attempt
in this direction and will help students in developing a strong foundation and enough confidence to take the JEE Main.
The various topics of chemistry may be classified into three branches—Physical, Inorganic and Organic. The
book covers these three branches in 29 chapters. Each chapter starts with the synopsis of theory followed by MCQs
along with answers and hints and solutions to arrive at correct answers. Wherever needed, the chapter is divided into
sections to cover the subject in easily understandable portions to help in better grasping of the subject matter. Each
section/chapter ends with MCQs from the previous years' AIEEE and JEE Main. This will help students in getting an
idea about the types and levels of questions asked in this competitive examination. The answers and solutions to these
questions are provided separately, immediately after the questions.
The analyses of these papers (provided on the next page) reveals that in most of the cases, one question is asked
from each chapter and the entire syllabus is covered in the examination paper. This book provides extensive coverage
of the theory as well as the associated MCQs. The contents of each chapter are covered in various sections. At the end
of all the sections, more extensive MCQs based on the Entire Chapter along with their solutions are also included.
It will be beneficial for the students to adopt the present book as the reference book along with their main text book.
The MCQs included in this book should be attempted along with the class-room teaching of the subject matter. A regular
and periodical review of the theory and MCQs from this book will help students in gaining enough confidence to appear
in the JEE Main and enable them to face the challenge of successfully clearing this examination.
From the analyses of previous years’ question papers, a pattern of predominant topics emerges on which students
should pay more attention while preparing for the examination. These are:
Physical Chemistry—Entire portion
Inorganic Chemistry has been thoroughly revised and updated—Chemical families—perioidic properties,
structures of compounds containing Si, N, P, S, halogens and inert gases, d-block elements and coordination chemistry
Organic Chemistry—Stereoisomerism, SN1 and S22 Reactions, Reactions involving rearrangement, Chemistry of
typical reactions shown by phenols, aldehydes and ketones and amines, relative acidity/basicity of phenolic, Carboxylic
acids and amines, polymers, carbohydrates, stereochemistry involved in halogenation of alkenes and dehalogenation of
halogenated compounds to give alkene, reactions involving Grignard reagent and diazonium salt.


K.L. Kapoor



Trend Analysis
Physical Chemistry
  Chapter

1.
2.

3.
4.
5.
6.
7.

8.

9.
10.

Some Basic Concepts
States of Matter
Gaseous State
Liquid State
Solid State
Atomic Structure
Chemical Bonding
Solutions

Chemical Thermodynamics
Chemical and Ionic Equilibria
Chemical Equilibria
Ionic Equilibria
Redox Reactions and Electrochemistry
Redox Reactions
Electrolysis
Conduction
Galvanic Cells
Chemical Kinetics
Surface Chemistry
Total

2014
(offline)
1

I
1

2014
(online)
II
III
1
1

2015
2016
(offline) (offline)

IV
—

1

1
—
1
1

2
—
1
1

1
—
1
2

—
—
1
3

1
1
2
—


1
1
1

1
1
1

2
1
1

3
1
—

—
—
2

2
2
—

2

1
—

1

—

—
2

1
1

1
1

1
—
2
1
1
—
13

—
2
—
—
1
—
13

—
—
—

1
2
—
14

1
1
—
—
1
—
12

3
—
—
—
1
—
14

1
—
1
—
—
—
—
1
2

12

1

2017
(offline)
2

1

1

1

1
2

1
1
2

1
1
2

1
2
1

1

1
1
11

1
1
1
15

Inorganic Chemistry
Chapter

11.
12.
13.
14.

Chemical Families–Periodic properties
General Principles and
Processes of Isolation of Metals
Hydrogen
s-Block Elements

2014
(offline)
—

I
—


2014
(online)
II
III
1
2

IV
1

1

1

1
—
—

1
—
—

—
—
—

—
—
—


1
1
1

1

—
—
—

2015
2016
(offline) (offline)

2017
(offline)
1

1
(Contd...)


viii  Trend Analysis

  Chapter
15.
16.
17.
18.
19.


Study of p-Block Elements
(Groups 13, 14 and 15)
Study of p-Block Elements
(Groups 16, 17 and 18)
d– and f– Block Elements
Coordination Chemistry
and Organometallics
Nuclear Chemistry
Total

2014

2014 (online)

2015

1

1

2

1

2

2

2016

(offline)
1

2017

1

—

1

1

—

1

2

2

1

2

—

2

1


1

2

2
—
6

2
—
6

1
—
5

2
—
8

2
—
6

1
—
9

2


1

10

4

Organic Chemistry
  Chapter

2014
(offline)
I

20.
21.
22.

23.
24.

25.
26.
27.
28.
29.

Purification and Characterization of
Organic Compounds
Some Basic Principles

Hydrocarbons
Alkanes
Alkenes
Alkynes
Benzene
Organic Compounds Containing
Halogens
Organic Compounds
Containing Oxygen
Alcohols
Phenols
Ethers
Aldehydes & Ketones
Carboxylic Acids
Organic Compounds
Containing Nitrogen
Synthetic & Natural Polymers
Biomolecules & Biological
Processes
Chemistry in Action
Principles Related
to Practical Chemistry
Total

2014
(online)
II
III

2015

2016
2017
(offline) (offline) (offline)
IV

1
—

—
1

—
2

—
1

—
1

1
2

—
—
—
—

—
—

—
—

—
1
1
—

1
1
—
—

—
—
1

—
—
—
1

2

2

1

—


1

—
2
—
1
1
2

1
—
1
2
—
1

—
1
—
2
—
1

2
—
—
—
2
1


1

2

—

1
—

—
—

—
11

1
11

1

2

1

2

1

1


1

—
2
1
—
1
1

—
—
—
—
—
1

1

1

1
1
1

—

1

1


1

1

—
1

1
1

1
—

—
2

1
2

1

1
11

—
10

—
10


—
9

9

1
11


About JEE Main
1.  Introduction and Scheme of Examination
The Joint Entrance Examination from the year 2013 for admission to the undergraduate programmes in Engineering
is being held in two parts, JEE-Main and JEE-Advanced. Only the top 1,50,000 candidates (including all categories)
based on performance in JEE Main will qualify to appear in the JEE Advanced examination. Admissions to IITs will be
based only on category-wise All India Rank (AIR) in JEE Advanced, subject to condition that such candidates are in the
top 20 percentile categories. Admission to NITs will be based on 40% weightage for performance in Class XII board
marks (normalized) and the remainder 60% weightage would be given to performance in JEE Main and a combined All
India Rank (AIR) would be decided accordingly.

In case any State opts to admit students in the engineering Colleges affiliated to state Universities where States
require separate merit list to be provided based on relative weightages adopted by the states, then the merit list shall be
prepared with such relative weightages as may be indicated by States.

2.  Eligibility Criteria and List of Qualifying Examinations for JEE(Main) Exam
The minimum academic qualification for appearing in JEE(Main) is that the candidate must have passed in final
examination of 10+2 (Class XII) or its equivalent referred to as the qualifying examination (see below).

However, admission criteria in the concerned institution/university will be followed as prescribed by concerned
university/institution and as per the guidelines & criteria prescribed by AICTE.


Qualifying Examinations
List of Qualifying Examinations
(i) The +2 level examination in the 10+2 pattern of examination of any recognized Central/State Board of Secondary
Examination, such as Central Board of Secondary Education, New Delhi, and Council for Indian School Certificate
Examination, New Delhi
(ii) Intermediate or two-year Pre-University Examination conducted by a recognized Board/University.
(iii) Final Examination of the two-year course of the Joint Services Wing of the National Defence Academy.
(iv) Any Public School/Board/University Examination in India or in foreign countries recognized by the Association
of Indian Universities as equivalent to 10+2 system.
(v) H.S.C. Vocational Examination.
(vi) A pass grade in the Senior Secondary School Examination conducted by the National Open School with a
minimum of five subjects.
(vii) 3 or 4-year diploma recognized by AICTE or a State Board of Technical Education.


x  About JEE Main

3.  Pattern of Examination
Subject combination for each paper and type of questions in each paper are given below:
Paper 1

Paper 2

Subjects
Physics, Chemistry & Mathematics

Mathematics – Part I
Aptitude Test – Part II &
Drawing Test – Part III


Type of Questions
Objective type questions with equal
weightage to Physics, Chemistry &
Mathematics
Objective type questions
Objective type questions
questions to test Drawing Aptitude

Duration
3 Hours

3 Hours

Requirement of papers for different courses is given in the table below:
Course
B.E/B.TECH
B.ARCH/B. PLANNING

Papers
Paper – 1
Paper – 2

Scoring and Negative Marking
There will be objective type questions with four options having single correct answer. For each incorrect response,
one fourth (1/4) of the total marks allotted to the question would be deducted. No deduction from the total score will,
however, be made if no response is indicated for an item in the answer sheet.


Syllabus
SECTION —A

Physical Chemistry
Unit 1  Some Basic Concepts in Chemistry
Matter and its nature, Dalton’s atomic theory; Concept of atom, molecule, element and compound; Physical quantities
and their measurements in Chemistry, precision and accuracy, significant figures, S.I. Units, dimensional analysis; Laws
of chemical combination; Atomic and molecular masses, mole concept, molar mass, percentage composition, empirical
and molecular formulae; Chemical equations and stoichiometry.

Unit 2  States of Matter
Classification of matter into solid, liquid and gaseous states.
Gaseous State: Measurable properties of gases; Gas laws—Boyle’s law, Charles’ law, Graham’s law of diffusion,
Avogadro’s law, Dalton’s law of partial pressure; Concept of Absolute scale of temperature; Ideal gas equation, Kinetic
theory of gases (only postulates); Concept of average, root mean square and most probable velocities; Real gases,
deviation from Ideal behaviour, compressibility factor, van der Waals equation, liquefaction of gases, critical constants.
Liquid State: Properties of liquids—vapour pressure, viscosity and surface tension and effect of temperature on
them (qualitative treatment only).
Solid State: Classification of solids: molecular, ionic, covalent and metallic solids, amorphous and crystalline solids
(elementary idea); Bragg’s Law and its applications, Unit cell and lattices, packing in solids (fcc, bcc and hcp lattices),
voids, calculations involving unit cell parameters, imperfection in solids; electrical, magnetic and dielectric properties.

Unit 3  Atomic Structure
Discovery of sub-atomic particles (electron, proton and neutron); Thomson and Rutherford atomic models and
their limitations; Nature of electromagnetic radiation, photoelectric effect; spectrum of hydrogen atom, Bohr model
of hydrogen atom—its postulates, derivation of the relations for energy of the electron and radii of the different
orbits, limitations of Bohr’s model; dual nature of matter, de-­Broglie’s relationship, Heisenberg uncertainty principle.
Elementary ideas of quantum mechanics, quantum mechanical model of atom, its important features, y and y2, concept
of atomic orbitals as one electron wave functions; Variation of y and y2 with r for 1s and 2s orbitals; various quantum
numbers (principal, angular momentum and magnetic quantum numbers) and their significance; shapes of s, p and
d—orbitals, electron spin and spin quantum number; rules for filling electrons in orbitals—aufbau principle, Pauli’s
exclusion principle and Hund’s rule, electronic configuration of elements, extra stability of half-filled and completely
filled orbitals.



xii  Syllabus

Unit 4  Chemical Bonding and Molecular Structure
Kossel: Lewis approach to chemical bond formation, concept of ionic and covalent bonds.
Ionic Bonding: Formation of ionic bonds, factors affecting the formation of ionic bonds; calculation of lattice
enthalpy.
Covalent Bonding: Concept of electronegativity, Fajan’s rule, dipole moment; Valence Shell Electron Pair Repulsion
(VSEPR) theory and shapes of simple molecules.
Quantum mechanical approach to covalent bonding: Valence bond theory—Its important features, concept of
hybridization involving s, p and d orbitals; Resonance.
Molecular Orbital Theory: Its important features, LCAOs, types of molecular orbitals (bonding, antibonding),
sigma and pi-bonds, molecular orbital electronic configurations of homonuclear diatomic molecules, concept of bond
order, bond length and bond energy.

Elementary idea of metallic bonding. Hydrogen bonding and its applications.

Unit 5  Chemical Thermodynamics
Fundamentals of Thermodynamics: System and surroundings, extensive and intensive properties, state functions,
types of processes.
First Law of Thermodynamics: Concept of work, heat, internal energy and enthalpy, heat capacity, molar heat
capacity, Hess’s law of constant heat summation; Enthalpies of bond dissociation, combustion, formation, atomization,
sublimation, phase transition, hydration, ionization and solution.
Second Law of Thermodynamics: Spontaneity of processes; DS of the universe and DG of the system as criteria
for spontaneity, DGo (Standard Gibbs energy change) and equilibrium constant.

Unit 6  Solutions
Different methods for expressing concentration of solution—molality, molarity, mole fraction, percentage (by volume
and mass both), vapour pressure of solutions and Raoult’s Law—Ideal and non-ideal solutions, vapour pressure—

composition plots for ideal and non-ideal solutions; Colligative properties of dilute solutions—relative lowering
of vapour pressure, depression of freezing point, elevation of boiling point and osmotic pressure; Determination of
molecular mass using colligative properties; Abnormal value of molar mass, van’t Hoff factor and its significance.

Unit 7  Equilibrium
Meaning of equilibrium, concept of dynamic equilibrium.
Equilibria Involving Physical Processes: Solid–liquid, liquid–gas and solid–gas equilibria, Henry’s law, general
characteristics of equilibrium involving physical processes.
Equilibria Involving Chemical Processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and
their significance, significance of DG and DGo in chemical equilibria, factors affecting equilibrium concentration,
pressure, temperature, effect of catalyst; Le­Chatelier’s principle.
Ionic Equilibrium: Weak and strong electrolytes, ionization of electrolytes, various concepts of acids and bases
(Arrhenius, Bronsted—Lowry and Lewis) and their ionization, acid—base equilibria (including multistage ionization)
and ionization constants, ionization of water, pH scale, common ion effect, hydrolysis of salts and pH of their solutions,
solubility of sparingly soluble salts and solubility products, buffer solutions.


Syllabus  xiii

Unit 8  Redox Reactions and Electrochemistry
Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation
number, balancing of redox reactions.
Eectrolytic and metallic conduction, conductance in electrolytic solutions, specific and molar conductivities and their
variation with concentration: Kohlrausch’s law and its applications.
Electrochemical cells—Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including
standard electrode potential, half-cell and cell reactions, emf of a Galvanic cell and its measurement; Nemst equation
and its applications; Relationship between cell potential and Gibbs’ energy change; Dry cell and lead accumulator; Fuel
cells; Corrosion and its prevention.

Unit 9  Chemical Kinetics

Rate of a chemical reaction, factors affecting the rate of reactions c­ oncentration, temperature, pressure and catalyst;
elementary and complex reactions, order and molecularity of reactions, rate law, rate constant and its units, differential
and integral forms of zero and first order reactions, their characteristics and half-lives, effect of temperature on rate of
reactions—Arrhenius theory, activation energy and its calculation, collision theory of bimolecular gaseous reactions
(no derivation).

Unit 10  Surface Chemistry
Adsorption: Physisorption and chemisorption and their characteristics, factors affecting adsorption of gases on
solids—Freundlich and Langmuir adsorption isotherms, adsorption from solutions.
Catalysis: Homogeneous and heterogeneous, activity and selectivity of solid catalysts, enzyme catalysis and its
mechanism.
Colloidal state: Distinction among true solutions, colloids and suspensions, classification of colloids—lyophilic,
lyophobic; multi molecular, macro-molecular and associated colloids (micelles), preparation and properties of
colloids—Tyndall effect, Brownian movement, electrophoresis, dialysis, coagulation and flocculation; Emulsions and
their characteristics.

SECTION — B
Inorganic Chemistry
Unit 11  Classificaton of Elements and Periodicity in Properties
Modem periodic law and present form of the periodic table, s, p, d and f block elements, periodic trends in properties
of elements­atomic and ionic radii, ionization enthalpy, electron gain enthalpy, valence, oxidation states and chemical
reactivity.

Unit 12  General Principles and Processes of Isolation of Metals
Modes of occurrence of elements in nature, minerals, ores; steps involved in the extraction of metals — concentration,
reduction (chemical. and electrolytic methods) and refining with special reference to the extraction of Al, Cu, Zn and
Fe; Thermodynamic and electrochemical principles involved in the extraction of metals.

Unit 13  Hydrogen
Position of hydrogen in periodic table, isotopes, preparation, properties and uses of hydrogen; physical and chemical

properties of water and heavy water; Structure, preparation, reactions and uses of hydrogen peroxide; Classification of
hydrides—ionic, covalent and interstitial; Hydrogen as a fuel.


xiv  Syllabus

Unit 14  s-Block Elements (Alkali and Alkaline Earth Metals)
Group - 1 and 2 Elements
General introduction, electronic configuration and general trends in physical and chemical properties of elements,
anomalous properties of the first element of each group, diagonal relationships.

Preparation and properties of some important compounds—sodium carbonate, sodium chloride, sodium
hydroxide and sodium hydrogen carbonate; Industrial uses of lime, limestone, Plaster of Paris and cement; Biological
significance of Na, K, Mg and Ca.

Unit 15  p-Block Elements
Group-13 to Group-18 Elements
General Introduction: Electronic configuration and general trends in physical and chemical properties of elements
across the periods and down the groups; unique behaviour of the first element in each group.
Groupwise study of the p-block elements
Group-13
Preparation, properties and uses of boron and aluminium; structure, properties and uses of borax, boric acid, diborane,
boron trifluoride, aluminium chloride and alums.
Group-14
Tendency for catenation; Structure, properties and uses of allotropes and oxides of carbon, silicon tetrachloride,
silicates, zeolites and silicones.
Group-15
Properties and uses of nitrogen and phosphorus; Allotrophic forms of phosphorus; Preparation, properties, structure
and uses of ammonia nitric acid, phosphine and phosphorus halides, (PCl3, PCl5); Structures of oxides and oxoacids of
nitrogen and phosphorus.

Group-16
Preparation, properties, structures and uses of dioxygen and ozone; Allotropic forms of sulphur; Preparation,
properties, structures and uses of sulphur dioxide, sulphuric acid (including its industrial preparation); Structures of
oxoacids of sulphur.
Group-17
Preparation, properties and uses of chlorine and hydrochloric acid; Trends in the acidic nature of hydrogen halides;
Structures of Interhalogen compounds and oxides and oxoacids of halogens.
Group-18
Occurrence and uses of noble gases; Structures of fluorides and oxides of xenon.

Unit 16  d – and f – Block Elements
Transition Elements
General introduction, electronic configuration, occurrence and characteristics, general trends in properties of the
first row transition elements—physical properties, ionization enthalpy, oxidation states, atomic radii, colour, catalytic
behaviour, magnetic properties, complex formation, interstitial compounds, alloy formation; Preparation, properties
and uses of K2 Cr2 O7 and KMnO4.


Syllabus  xv

Inner Transition Elements
Lanthanoids — Electronic configuration, oxidation states, chemical reactivity and lanthanoid contraction.
Actinoids — Electronic configuration and oxidation states.

Unit 17  Co-ordination Compounds
Introduction to co-ordination compounds, Werner’s theory; ligands, co-ordination number, denticity, chelation;
IUPAC nomenclature of mononuclear co-ordination compounds, isomerism; Bonding ­Valence bond approach and basic
ideas of Crystal field theory, colour and magnetic properties; importance of co-ordination compounds (in qualitative
analysis, extraction of metals and in biological systems).


Unit 18  Environmental Chemistry
Environmental Pollution: Atmospheric, water and soil.
Atmospheric Pollution: Tropospheric and stratospheric. .
Tropospheric Pollutants: Gaseous pollutants: Oxides of carbon, nitrogen and sulphur, hydrocarbons; their sources,
harmful effects and prevention; Green house effect and Global warming; Acid rain;
Particulate Pollutants: Smoke, dust, smog, fumes, mist; their sources, harmful effects and prevention.
Stratospheric Pollution: Formation and breakdown of ozone, depletion of ozone layer—its mechanism and effects.
Water Pollution: Major pollutants such as pathogens, organic wastes and chemical pollutants; their harmful effects
and prevention.
Soil Pollution: Major pollutants such as Pesticides (insecticides,. herbicides and fungicides), their harmful effects
and prevention.
Strategies to control environmental pollution.

SECTION—C
Organic Chemistry
Unit 19  Purification and Characterisation of Organic Compounds
Purification: Crystallization, sublimation, distillation, differential extraction and chromatography—principles and
their applications.
Qualitative Analysis: Detection of nitrogen, sulphur, phosphorus and halogens.
Quantitative Analysis (basic principles only) Estimation of carbon, hydrogen, nitrogen, halogens, sulphur,
phosphorus.

Calculations of empirical formulae and molecular formulae; Numerical problems in organic quantitative
analysis.

Unit 20  Some Basic Principles of Organic Chemistry
Tetravalency of carbon; Shapes of simple molecules—hybridization (s and p); Classification of organic compounds
based on functional groups: - C = C - , - C = C - and those containing halogens, oxygen, nitrogen and sulphur,
Homologous series; Isomerism - structural and stereoisomerism.
Nomenclature (Trivial and IUPAC)



xvi  Syllabus

Covalent Bond Fission—Homolytic and heterolytic: free radicals, carbocations and carbanions; stability of
carbocations and free radicals, electrophiles and nucleophiles.
Electronic Displacement in a Covalent Bond: Inductive effect, electromeric effect, resonance and hyperconjugation.
Common Types of Organic Reactions: Substitution, addition, elimination and rearrangement.

Unit 21  Hydrocarbons
Classification, isomerism, IUPAC nomenclature, general methods of preparation, properties and reactions.
Alkanes: Conformations: Sawhorse and Newman projections (of ethane); Mechanism of halogenation of alkanes.
Alkenes: Geometrical isomerism; Mechanism of electrophilic addition: addition of hydrogen, halogens, water,
hydrogen halides (Markownikoff’s and peroxide effect); Ozonolysis, oxidation, and polymerization.
Alkynes: acidic character; addition of hydrogen, halogens, water and hydrogen halides; polymerization.
Aromatic hydrocarbons: Nomenclature, benzene—structure and aromaticity; Mechanism of electrophilic
substitution: halogenation, nitration, Friedel–Craft’s alkylation and acylation, directive influence of functional group in
mono-substituted benzene.

Unit 22  Organic Compounds Containing Halogens
General methods of preparation, properties and reactions; Nature of C-X bond; Mechanisms of substitution reactions.

Uses/environmental effects of chloroform, iodoform, freons and DDT.

Unit 23  Organic Compounds Containing Oxygen
General methods of preparation, properties, reactions and uses.
Alcohols, Phenols and Ethers
Alcohols: Identification of primary, secondary and tertiary alcohols; mechanism of dehydration.
Phenols: Acidic nature, electrophilic substitution reactions: halogenation, nitration and sulphonation, Reimer Tiemann reaction.
Ethers: Structure.

Aldehyde and Ketones: Nature of carbonyl group; Nucleophilic addition to >C=O group, relative reactivities of
aldehydes and ketones; Important reactions such as—Nucleophilic addition reactions (addition of HCN, NH3 and its
derivatives), Grignard reagent; oxidation; reduction (Wolff Kishner and Clemmensen); acidity of a - hydrogen, aldol
condensation, Cannizzaro reaction, Haloform reaction; Chemical tests to distinguish between aldehydes and Ketones.
Carboxylic Acids: Acidic strength and factors affecting it.

Unit 24  Organic Compounds Containing Nitrogen
General methods of preparation, properties, reactions and uses.
Amines: Nomenclature, classification, structure basic character and identi-fication of primary, secondary and tertiary
amines and their basic character.
Diazonium Salts: Importance in synthetic organic chemistry.


Syllabus  xvii

Unit 25  Polymers
General introduction and classification of polymers, general methods of polymerization - addition and condensation,
copolymerization; Natural and synthetic rubber and vulcanization; some important polymers with emphasis on their
monomers and uses - polythene, nylon, polyester and bakelite.

Unit 26  Biomolecules
General introduction and importance of biomolecules.
Carbohydrates: Classification: aldoses and ketoses; monosaccharides (glucose and fructose), constituent
monosaccharides of oligosacchorides (sucrose, lactose, maltose) and polysaccharides (starch, cellulose, glycogen).
Proteins: Elementary Idea of a - amino acids, peptide bond, polypeptides; proteins: primary, secondary, tertiary and
quaternary structure (qualitative idea only), denaturation of proteins, enzymes.
Vitamins: Classification and functions.
Nucleic Acids: Chemical constitution of DNA and RNA.
Biological functions of Nucleic acids.


Unit 27  Chemistry in Everyday Life
Chemicals in Medicines: Analgesics, tranquilizers, antiseptics, disinfectants, antimicrobials, antifertility drugs,
antibiotics, antacids, antihistamins-their meaning and common examples.
Chemicals in Food: Preservatives, artificial sweetening agents-common examples.
Cleansing Agents: Soaps and detergents, cleansing action.

Unit 28  Principles Related to Practical Chemistry
∑ Detection of extra elements (N,S, halogens) in organic compounds; Detection of the following functional groups:
hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketone), carboxyl and amino groups in organic
compounds.
∑ Chemistry involved in the preparation of the following:
Inorganic compounds: Mohr’s salt, potash alum.
Organic compounds: Acetanilide, p-nitroacetanilide, aniline yellow, iodoform.
∑ Chemistry involved in the titrimetric excercises - Acids bases and the use of indicators, oxalic-acid vs KMnO4,
Mohr’s salt vs KMnO4.
∑ Chemical principles involved in the qualitative salt analysis:
Cations:Pb2+, Cu2+, AI3+, Fe3+, Zn2+, Ni2+, Ca2+, Ba2+, Mg2+, NH4+.
Anions:CO32–, S2–, SO42–, NO2– , NO3– , CI – , Br–, I– .


(Insoluble salts excluded).

∑ Chemical principles involved in the following experiments:


1. Enthalpy of solution of CuSO4



2. Enthalpy of neutralization of strong acid and strong base.




3. Preparation of lyophilic and lyophobic sols.



4. Kinetic study of reaction of iodide ion with hydrogen peroxide at room temperature.



Contents

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About JEE Main
Syllabus
1. Some Basic Concepts of Chemistry
Section-1 Physical Quantities  1.1

v
vii
ix
xi
1.1–1.35

Section-2 Significant Figures (or Digits)  1.7
Section-3 Atomic and Molecular Masses  1.9
Section-4 Laws of Chemical Combination  1.14
Section-5 Composition of a Solution  1.19

2. States of Matter
Gaseous State  2.1
Unit-1

2.1–2.90

Section-1 Ideal Gases  2.1
Section-2 Kinetic-Molecular Theory of Gases  2.7
Section-3 Real Gases  2.12
Unit-2

Liquid State  2.37

Unit-3

Solid State  2.43

Section-1 Crystal Systems  2.43
Section-2 Closest Packings of Atoms  2.54
Section-3 Structures of Ionic Compounds  2.64
Section-4 Imperfection in Solids  2.74
3. Atomic Structure
Section-1 Development of Structure of Atom  3.1

3.1–3.39

Section-2 Quantum-Mechanical Model of Atom  3.8
4. Chemical Bonding and Molecular Structure
Section-1 Bond Formation and VSEPR Theory  4.1


4.1–4.42

Section-2 VB and MO Theories 4.13
5.Solutions
Section-1 Composition of a Solution  5.1

5.1–5.42

Section-2 Liquid Solutions  5.7
Section-3 Colligative Properties  5.16
6. Chemical Thermodynamics
Section-1 Basic Definitions and First Law of Thermodynamics  6.1

6.1–6.45


xx  Contents

Section-2 Thermochemistry 6.9
Section-3 Criteria of Spontaneity  6.17
7. Chemical and Ionic Equilibria
Chemical Equilibrium  7.1
Unit-1
unit-2

7.1–7.75

Ionic Equilibrium  7.27

Section-1 Concepts of Acids and Bases  7.27

Section-2 The pH Scale and pH of Acid and Base Solutions  7.32
Section-3 Hydrolysis of Salts  7.39
Section-4 Buffer Solutions  7.44
Section-5 Solubility Product  7.48
Section-6 Acid-Base Indicators  7.53
8. Redox Reactions and Electrochemistry
Redox Reactions and Electrolysis  8.1
Unit-1

8.1–8.58

Section-1 Redox Reactions  8.1
Section-2 Electrolytic Cell  8.8
Unit-2

Electrolytic Conduction  8.18

Unit-3

Galvanic Cells  8.30

9. Chemical Kinetics

9.1–9.33

10. Surface Chemistry

10.1–10.9

11. Chemical Families–Periodic Properties


11.1–11.19

12. General Principles and Processes of Isolation of Metals

12.1–12.8

13. Hydrogen

13.1–13.7

14. S-Block Elements (Alkali and Alkaline Earth Metals)

14.1–14.25


The Group 1 Elements – Alkali Metals  14.1
The Group 2 Element – Alkaline Earth Metals  14.12
15. Study of the p-Block Elements (Groups 13, 14 and 15)

15.1–15.60

The Group 13 Elements – Boron Family  15.1
The Group 14 Elements – Carbon Family  15.16
The Group 15 Elements  15.35
16. Study of the p-Block Elements (Groups 16, 17 and 18)

16.1–16.48

The Group 16 Elements  16.1

The Group 17 Elements  16.22
The Group 18 Elements  16.41
17. d– and f–Block Elements

17.1–17.28

18. Coordination Chemistry and Organometallics

18.1–18.26

19. Nuclear Chemistry

19.1–19.8

20. Purification and Characterization of Organic Compounds

20.1–20.9

21. Some Basic Principles

21.1–21.46


Contents  xxi

22. Hydrocarbons
Section-1 Alkanes   22.1

22.1–22.61


Section-2 Alkenes   22.13
Section-3 Alkynes   22.31
Section-4 Benzene 22.43
Section-5 Sources of Hydrocarbons  22.58
23. Organic Compounds Containing Halogens (Haloalkanes and Haloarenes)
Section-1 Haloalkanes 23.1
Section-2 Haloarenes 23.5
24. Organic Compounds Containing Oxygen (Alcohols, Phenols, Ethers, Aldehydes,
Ketones, Carboxylic Acids and their Derivatives)
Section-1 Alcohols 24.1

23.1–23.14

24.1–24.73

Section-2 Phenols 24.16
Section-3 Ethers 24.31
Section-4 Aldehydes and Ketones  24.34
Section-5 Carboxylic Acids  24.55
25. Organic Compounds Containing Nitrogen (Cyanides, Isocyanides,
Nitrocompounds and Amines)

25.1–25.24

Section-1 Cyanides and Isocyanides  25.1
Section-2 Nitro Compounds  25.2
Section-3 Amines 25.4
26. Synthetic and Natural Polymers

26.1–26.14


27. Biomolecules and Biological Processes

27.1–27.24

28. Chemistry in Action

28.1–28.13

29. Principles Related to Practical Chemistry

29.1–29.15

Annexure
Practice Test Paper–I
Practice Test Paper–II
Practice Test Paper–III
Practice Test Paper–IV
Practice Test Paper–V
JEE (Main) ChemistryOffline Solved Paper—2017

JEE (Main) ChemistryOnline Solved Paper 1—2017
JEE (Main) ChemistryOnline Solved Paper 2—2017

AN.1–AN.15
PI.1–PI.3
PII.1–PII.4
PIII.1–PIII.5
PIV.1–PIV.4
PV.1–PV.4

JEEC.1-JEEC.8
JEEC.1-JEEC.8
JEEC.1-JEEC.9



1
Some Basic Concepts of
Chemistry
Section 1

Physical Quantities

In physical sciences, we commonly deal with quantities such as pressure, volume, mass, temperature, current, etc. These
quantities are known as physical quantities. A physical quantity has two components, namely, numerical value and its
unit, and is written as
Physical quantity = (Numerical value) (Unit)
The International Union of Pure and Applied Chemistry (IUPAC) has
recommended the use of seven physical quantities having their own dimensions. Their dimensions are completely
independent of one another and it is for this reason, these are known as dimensionally independent physical quantities.
These physical quantities along with their recommended symbols are given in Table 1.
Seven Base Physical Quantities
Physical quantity

Symbol

Length

l


Mass

m

Time

t

Electric current

I

Thermodynamic temperature

T

Amount of substance

n

Luminous intensity

Iv

Of the seven physical quantities, luminous intensity is not needed in physical chemistry. It is used in optical
photometry and is, therefore, included here, only for the sake of completeness.

International System of Units, commonly abbreviated as SI. The SI units of seven base physical quantities are listed
in Table 2.



Complete Chemistry—JEE Main

Seven Base Physical Quantities
Physical quantity
Length
Mass
Time
Electric current
Thermodynamic temperature
Amount of substance
Luminous intensity

Name of SI unit
metre
kilogram
second
ampere
kelvin
mole
candela

Symbol for SI unit
m
kg
s
A
K
mol
cd


The SI base units stated in Table 2 have been precisely
The metre is the length of path travelled by light in vacuum during a time interval of 1/299 792 458 of a second.
The kilogram is the unit of mass; it is equal to the mass of the international prototype of the kilogram.
This prototype is a polished cylinder of platinum-iridium alloy which was chosen for its durability and resistance to
corrosion. The cylinder is kept at the International Bureau of Weights and Measures in a suburb of Paris, France.
The second is the duration of 9 192 631 770 periods of the radiation corresponding to the transition between

of negligible cross-section, and placed 1 metre apart in vacuum, would produce between these conductors a force equal
to 2 ¥ 10–7 newton per metre of length.
The kelvin, unit of thermodynamic temperature, is the fraction 1/273.16 of the thermodynamic temperature
of the triple point of water.
The mole is the amount of substance of a system which contains as many elementary entities as there are atoms
in 0.012 kilogram of carbon-12.
The candela is the luminous intensity, in a give direction, of a source that emits monochromatic radiation of
frequency 540 ¥ 1012 hertz and that has a radiant intensity in that direction of (1/683) watt per steradian.
Of the seven base physical quantities, it is worth highlighting the physical
quantity ‘amount of substance’ along with its unit ‘mol’. This is because a basic change in our conventional way of
referring to this quantity is required. Suppose we have 0.5 mol of a substance (say, hydrogen). Conventionally, we
speak or write it as
Number of moles of hydrogen = 0.5
(or moles of hydrogen = 0.5 mol)
Now suppose we have 1 kg of hydrogen. We never speak or write it as
Number of kg of hydrogen = 1
since we are not accustomed to speak or write it like this. Instead, we say
Mass of hydrogen = 1 kg
Many such examples can be cited. For example, we never say
Number of kg of apples = 1
Number of litre of milk = 1
Number of dozen of apples = 1

Number of metre of a line = 1
A mole of a substance is a collection of 6.022 ¥ 1023 particles of that substance. It is like a dozen which is a collection
of 12 articles. When we do not refer to a collection of 12 articles as
Number of dozen of articles = 1
why should we refer to a collection of 6.022 ¥ 1023 articles as
Number of moles of articles =1?
So, some inconsistency has arisen in referring to these two quantities which basically belong to the same category.
To avoid this, IUPAC has recommended the use of the phrase ‘amount of substance’ for a physical quantity whose unit
is ‘mol’. More precisely, the word ‘amount’ is exclusively reserved whenever the quantity is to be expressed in terms
of moles. It is like using the words mass for kg, volume for m3 (or L) and length for metre. Thus, the use of the phrase
‘number of moles equal to 0.5’ should be completely replaced by ‘amount of substance equal to 0.5 mol’. It may be
mentioned that to write
Amount of substance = 0.5 g
is not acceptable as the word ‘amount’ is exclusively reserved for the unit ‘mol’ and not for ‘g’.


Some Basic Concepts of Chemistry

entities of that substance. The proportionality factor is the same for all substances and is equal to l/NA, where NA is
Avogadro constant which has a value of
NA = 6.022 ¥ 1023 mol–1
(
Earlier, NA was commonly referred to as Avogadro number. But it is not a pure number as it has both a
numerical value as well as a unit. So, It is a physical quantity and is called Avogadro constant.)
Mathematically, the amount of substance is given as
n = N / NA
NA is Avogadro constant. For example, 3.011.5 ¥ 1023

where N
molecules of dihydrogen will contain


Amount of dihydrogen = 3.011 ¥ 1023 / (6.022 ¥ 1023 mol–1) = 0.5 mol

Physical quantities other than base physical quantities are known as derived physical quantities. These may be expressed
in terms of base physical quantities by multiplication and division. Table 3 records some of the derived physical
quantities.
SI derived units of a few physical quantities
Physical quantity

SI unit

Symbol for SI unit

area

(length)2

square metre

m2

volume

(length)3

cubic metre

m3

density


mass/volume

kilogram per cubic metre

speed

distance/time

metre per second

m s–1

acceleration

speed/time

metre per square second

m s–2

heat capacity

Dq/Dt

—

J K–1

(l/m)(Dq/Dt)


—

J kg–1 K–1

molar heat capacity

(l/n)(Dq/Dt)

—

J K–1 mol–1

amount concentration

amount of substance/volume of solution

mole per cubic metre

mol m–3

molality

amount of substance/mass of solvent

mole per kilogram

mol kg–1

kg m–3


Some physical quantities have been assigned special names and symbols. These are described in Table 4.
Special names and symbols for certain SI derived units
Physical quantity
frequency
force

Name of SI unit Symbol for SI unit
—
mass ¥ accleration

Hertz

Hz

s–1

Newton

N

kg m s–2
kg m–1 s–2 (=N m–2)

pressure

force/(length)2

Pascal


Pa

energy

force ¥ length

Joule

J

kg m2 s–2 (= N m)

power

energy/time

Watt

W

kg m2 s–3 (= J s–1)

Coulomb

C

As

electric charge


current ¥ time

electric potential difference

—

Volt

V

kg m2 s–3 A–1 (= J A–1 s–1)

electric resistance

—

Ohm

W

kg m2 s–3 A–2 (= V A–1)

electric conductance

—

Siemens

S


kg–1 m–2 s3 A2 (= A V–1 = W–1)

—

Tesla

T

kg s–2 A–1