Preview j d lee concise inorganic chemistry for JEE (main advanced) by sudarsan guha , j d lee (2019)

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2020

For JEE (main & Advanced)
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Highlights of the Book


Chapter opener with an opening vignette related to
the topics, and contents of the chapter listed for an
overview.



Reorganization of chapters as per JEE syllabus flow
–Chemical Bonding combined to cover ionic, covalent
and metallic bonding together. Chapters on s-, p-, dand f- block elements combined to form single chapter
each, covering just the required topics.



Additional chapters on Hydrolysis, Metallurgy and
Qualitative Salt Analysis for complete coverage of JEE
syllabus.



Deletion of chapters not required as per syllabus –
Atomic Nucleus and Spectra



Assessment as per JEE comprising all question types –
Single correct choice, Multiple correct choice,
Comprehension type, Assertion-reasoning type,
Integer answer type and Matrix-match type.



Useful appendices with data on abundance of
elements, their melting and boiling points, densities,
electronic structure, bond energies, solubilities,
atomic weight and electrical resistivity.



Includes solved JEE Advanced 2018 Chemistry paper

About the Book
The book is an adaptation of the classic book Concise Inorganic
Chemistry by J.D. LEE (fifth edition), which is widely used by students
preparing for JEE. This adapted version provides a more concise and
relevant treatment of Inorganic Chemistry as per JEE syllabus
requirements. The concepts are explained in a simple and
straightforward manner. Yet the book provides a through grounding
of the subject, helping students approach the examination with
confidence.
New to this Edition
Chapter 8:
topics on which JEE questions are based.

Chapter 9:
Chapter 10:
ü Content more precise and better-organized under Groups
13 to 18
ü New question sets (all types) at the end of each group
ü Miscellaneous (Multi-concept) questions at the end of chapter
Exercises:
chapters
Includes
Solutions available at
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ISBN 978-81-265-9831-1

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J.D. Lee
Concise
Inorganic Chemistry
for JEE (Main & Advanced)

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J.D. Lee
Concise
Inorganic Chemistry
for JEE (Main & Advanced)

Adapted by

Sudarsan Guha


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J.D. Lee
Concise
Inorganic Chemistry
for JEE (Main & Advanced)
Copyright © 2019 by Wiley India Pvt. Ltd., 4436/7, Ansari Road, Daryaganj, New Delhi-110002.
All rights reserved. No part of this book may be reproduced, stored in a retrieval system, or transmitted in any form or by any
means, electronic, mechanical, photocopying, recording or scanning without the written permission of the publisher. This
book is an adaptation of Concise Inorganic Chemistry 5/e by J.D. Lee (ISBN: 978-81-265-1554-7). All rights remain with

respective holders.
Limits of Liability: While the publisher and the author have used their best efforts in preparing this book, Wiley and the
author make no representation or warranties with respect to the accuracy or completeness of the contents of this book, and
specifically disclaim any implied warranties of merchantability or fitness for any particular purpose. There are no warranties
which extend beyond the descriptions contained in this paragraph. No warranty may be created or extended by sales
representatives or written sales materials. The accuracy and completeness of the information provided herein and the
opinions stated herein are not guaranteed or warranted to produce any particular results, and the advice and strategies
contained herein may not be suitable for every individual. Neither Wiley India nor the author shall be liable for any loss of
profit or any other commercial damages, including but not limited to special, incidental, consequential, or other damages.
Disclaimer: The contents of this book have been checked for accuracy. Since deviations cannot be precluded entirely, Wiley
or its author cannot guarantee full agreement. As the book is intended for educational purpose, Wiley or its author shall not
be responsible for any errors, omissions or damages arising out of the use of the information contained in the book. This
publication is designed to provide accurate and authoritative information with regard to the subject matter covered. It is sold
on the understanding that the Publisher is not engaged in rendering professional services.
Trademarks: All brand names and product names used in this book are trademarks, registered trademarks, or trade names
of their respective holders. Wiley is not associated with any product or vendor mentioned in this book.
Other Wiley Editorial Offices:
John Wiley & Sons, Inc. 111 River Street, Hoboken, NJ 07030, USA
Wiley-VCH Verlag GmbH, Pappellaee 3, D-69469 Weinheim, Germany
John Wiley & Sons Australia Ltd, 42 McDougall Street, Milton, Queensland 4064, Australia
John Wiley & Sons (Asia) Pte Ltd, 1 Fusionopolis Walk #07-01 Solaris, South Tower, Singapore 138628
John Wiley & Sons Canada Ltd, 22 Worcester Road, Etobicoke, Ontario, Canada, M9W 1L1
Fourth Edition: 2017
Reprint: 2019
ISBN: 978-81-265-9831-1
www.wileyindia.com


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Preface
Concise Inorganic Chemistry by J.D. Lee is a book widely used by students reparing for
JEE as the most comprehensive and authentic text for understanding Inorganic Chemistry.
The purpose of adaptation of this book is to provide a complete textbook of Inorganic
Chemistry that covers the entire syllabus of JEE (Main and Advanced)in proper sequence
of topics and provides in-depth explanation of topics. The use of book should give confidence
to the students to apply their knowledge to problem-solving and attempting JEE.
In this new (fourth) edition, major changes have been made in the Chapter 8: Hydrogen,
where the concept of hydrogen bonding is now explained with specific examples relevant
to JEE. Chapter 9: The s-Block Elements has been made more concise with more focus on
topics required from JEE perspective. Major changes have been made in Chapter 10: The
p-Block Elements. It is now divided into six separate parts as Group 13, Group 14, Group
15, Group 16, Group 17 and Group 18 Elements. Each part is followed by a separate set
of exercises for that particular group. Miscellaneous questions based on multiple concepts
have been placed at the end of the chapter. Apart from this new questions have been
included in the exercises at the end of most of the chapters.
I would like to acknowledge my students for their intellectual doubts and my
colleagues for their valuable arguments in various aspects of the subject. This enhanced
my understanding of the subject and helped me to teach better. I am especially indebted to
my college Belur Ram Krishna Mission, Calcutta University for teaching me ‘How to read
and learn chemistry?’ and Bansal classes where I have got the opportunity to apply my
knowledge and teach chemistry. I am thankful to my promise to make this book as ‘only one
book for Inorganic Chemistry’ engineering aspirants.
For the future also, any suggestions for the improvement of this book are welcome by
the author.
Sudarsan Guha
M. Tech. (IIT-Kanpur)

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Note to the Student
The Joint Entrance Examination (JEE) comprises the Main and Advanced examinations,
which are essential stepping stones for all engineering aspirants. The JEE Main is focused
primarily on evaluating the conceptual strength of the students. The JEE Advanced would
further judge the ability of top performers in JEE Main to extend the conceptual strength
to application-based problem solving. For complete preparation of these prestigious
examinations, a book that is rich in conceptual strength and enriched with problem-solving
tools and assessment would serve as a one-stop solution!
Concise Inorganic Chemistry by J.D. Lee has been the definitive text for learning
Inorganic Chemistry since its first edition appeared about 45 years ago. The book captures
the fundamentals of the subject in a simple and logical framework of factual knowledge.
The description is long enough to cover the essentials, yet short enough to be interesting. Its
unparalleled approach to teaching Inorganic Chemistry is the reason why it is probably the
most favoured resource for an IIT aspirant like you today.
In collaboration with experts in JEE (Main & Advanced) coaching, the fifth edition of
the original book has now been adapted to give you the best book available in Inorganic
Chemistry for preparing for the toughest engineering entrance exam in India. This adaptation
offers the dual advantage of unmatched explanation of concepts as developed by “Master
teacher” and appropriate applications of the concepts to problem solving as developed by
an expert in this area.
Let’s walk through some of the special book features that will help you in your efforts
to take the JEE (Main & Advanced) with confidence.

A.

STRUCTURE OF THE BOOK

1. Structure of an Atom
2. Periodic Table and Periodic Properties
3. Chemical Bonding
4. Hydrolysis
5. Coordination Compounds
6. Metallurgy
7. Qualitative Salt Analysis
8. Hydrogen and its Hydrides
9. The s-Block Elements and their compounds
10. The p-Block Elements and their Compounds
11. The d-Block Elements and their Compounds
12. The f-Block Elements and their Compounds

The original book has been
reorganized in a manner to provide
more structured approach as per the
JEE (Main & Advanced) syllabus
requirement. The progression is from
basic concepts such as Structure of
an Atom, Periodic Table and Periodic
Properties and Chemical Bonding
to practical aspects of Metallurgy
and Qualitative Salt Analysis. This is
followed by description on Hydrogen
and its compounds and some
compounds and properties of s-, p- , dand f-block elements.

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B.

PEDAGOGY

CHAPTER OPENER
Each chapter starts with an
opening vignette related to the
topic, and listing of contents of
that chapter. This gives you an
overview of the chapter and
helps to identify the extent of
coverage.

CONCEPT EXPLANATION
Concepts are explained in a manner easy to read and understand.
They are descriptive to the extent
required and provide reasons for
the structure, properties and reactions of compounds. Many fascinating applications of inorganic
compounds are also explained.


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FIGURES
The text is sprinkled with
multiple figures which present two-dimensional representation of compounds

and their structures. This
visual representation enhances understanding and
helps the student visualize
what a molecule may look
like.

TABLES
A large number of tables
capture data on structure,
properties and other such
parameters. The tabular representation supports comparative study of properties and
draws out changing trends in
them. The trends of various
properties of elements along
the periodic table are also
amply illustrated.

C.

ASSESSMENT – AS PER JEE (MAIN & ADVANCED) PATTERN

Application of concepts to problem solving is the core of JEE (Main & Advanced),
so it is important to test our understanding of concepts. For the test to be effective,
the assessment technique should be comprehensive and in the context of this
book, also in resonance with the JEE Main and JEE Advanced paper pattern.
Each part of the assessment should be modeled on the actual paper pattern
because unless the student practices the JEE way, he/she will not be sufficiently
equipped to take the examination. Keeping this in mind, the assessment has been
divided into:

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SINGLE CORRECT CHOICE TYPE QUESTIONS
These are the regular multiple choice questions with
four choices provided. Only
one among the four choices
will be the correct answer.

MULTIPLE CORRECT CHOICE TYPE QUESTIONS
These are multiple choice
questions with four choices
provided. One or more of
the four choices provided
may be correct.

COMPREHENSION TYPE QUESTIONS
Comprehension-type
questions consist of a
small passage, followed
by three/four multiple
choice questions based
on it. The questions are
of single correct answer
type (with some exceptions).


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ASSERTION–REASONING TYPE QUESTIONS

These questions check the
analytical and reasoning
skills of the students. Two
statements are provided –
Statement I and Statement
II. The student is expected to
verify if (A) both statements
are true and if both are true,
verify if statement I follows
from statement II; (B) both
statements are true and if
both are true, verify if statement II is not the correct
reasoning for statement I;
(C), (D) which of the statements is untrue.

INTEGER ANSWER TYPE QUESTIONS
The questions in this section are numerical problems for which no choices
are provided. The students
are required to find the
exact answers to numerical problems which can
be one-digit or two-digit
numerals.

MATRIX–MATCH TYPE QUESTIONS
These questions are the
regular “Match the Following” variety. Two columns
each containing 4 subdivisions or first column with
four subdivisions and
second column with more
subdivisions are given and

the student should match
elements of column I to
that of column II. There can
be one or more matches.


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D.

USE OF SI UNITS

SI units for energy are used throughout this edition, thus making a comparison of thermodynamic properties easier. Ionization energies are quoted in kJ mol–1, rather than ionization
potentials in eV. Older data from other sources use eV and may be converted into SI units
(1 kcal = 4.184 kJ, and 1 eV = 23.06 × 4.184 kJ mol–1).
Meters are strictly the SI units for distance, and bond lengths are sometimes quoted in
nanometers (1 mm = 10–9 m). However Ångström units Å (10–10 m) are a permitted unit of
length, and are widely used by crystallographers because they give a convenient range of
numbers for bond lengths. Most bonds are between 1 and 2 Å (0.1 to 0.2 nm). Ångström
units are used throughout for bond lengths.
The positions of absorption peaks in spectra are quoted in wave numbers cm–1, because
instruments are calibrated in these units. It must be remembered that these are not SI units,
and should be multiplied by 100 to give SI units of m–1, or multiplied by 11.96 to give J mol–1.
The SI units of density are kg m–3, making the density of water 1000 kg m–3. This convention is not widely accepted, so the older units of g cm–3 are retained so water has a density
of 1 g cm–3.
In the section on magnetism both SI units and Debye units are given, and the relation
between the two is explained. For inorganic chemists who simply want to find the number
of unpaired electron spins in a transition metal ion, Debye units are much more convenient.

E.

NOMENCLATURE FOLLOWED IN THE PERIODIC TABLE

For a long time chemists have arranged the elements in groups within the periodic table in
order to relate the electronic structures of the elements to their properties, and to simplify
learning. There have been several methods of naming the groups.
A number of well known books name the main groups and the transition elements as A
and B subgroups, which dates back to the older Mendeleev periodic table of more than half
a century ago. Its disadvantages are that it may over emphasize slight similarities between
the A and B subgroups, and there are a large number of elements in Group VIII.
In earlier versions of this book the s-block and the p-block were numbered as Groups
I to VII and 0, depending on the number of electrons in the outer shell of the atoms, and
the transition elements were dealt with as triads of elements and named as the top element
in each group of three.
The IUPAC has recommended that the main groups and the transition metals should
be numbered from 1 to 18. This system has gained acceptance, and has now been adopted
throughout this book.

I
IA
H
Li
Na
K
Rb
Cs
1

II
IIA

Be
Mg
Ca
Sr
Ba
2

IIIB

Sc
Y
La
3

IVB

Ti
Zr
Hf
4

VB

V
Nb
Ta
5

VIB

Cr
Mo
W
6

VIIB

Mn
Tc
Re
7

<…VIIIB…>

Fe
Ru
Os
8

Co
Rh
Ir
9

Ni
Pd
Pt
10

IB

Cu
Ag
Au
11

IIB

III
IIIA

IV
IVA

V
VA

VI
VIA

VII
VIIA

Zn
Cd
Hg
12

B
Al

Ga
In
Tl
13

C
Si
Ge
Sn
Pb
14

N
P
As
Sb
Bi
15

O
S
Se
Te
Po
16

F
Cl
Br
I

At
17

F. APPENDICES
Appendix A: Abundance of the elements in the earth’s crust

0
VIIIA
He
Ne
Ar
Kr
Xe
Rn
18


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F.

APPENDICES

Appendix A

Abundance of the elements in the Earth’s crust

Appendix B

Melting points of the elements

Appendix C

Boiling points of the elements

Appendix D

Densities of solid and liquid elements

Appendix E

Electronic structures of the elements


Appendix F


Some average single bond energies and some double

Appendix G

Solubilities of main group compounds in water

Appendix H

Atomic weights based on 12C= 12.000

Appendix I

Values of some fundamental physical constants

Appendix J

Electrical resistivity of the elements at the stated temperature

Appendix K

Hardness of minerals — Mohs’ scale

and triple bond energies


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 Contents
Prefacev
Note to the Student
1. Structure of an Atom

1

1.1Atoms
1.2 Some Important Defnitions
1.3 Electronic Confguration of an Atom

Quantum numbers
Aufbau principle
Pauli exclusion principle
Hund’s rule
Stability of half-flled and fully-flled shells
Electronic confguration of ions
Nodal planes of different orbitals
Slater’s rule
Single Correct Choice Type Questions
Multiple Correct Choice Type Questions

Comprehension Type Questions

Assertion-Reasoning Type Questions

Integer Answer Type Questions

Matrix-Match Type Questions
Answers

1
2
3
4
6
8
9
13
13
15

15
17
20
21
23
23
24
25

2. Periodic Table and Periodic Properties

27



2.1 Periodic Table
Genesis of periodic classifcation
Moseley’s work
Modern periodic law
2.2 Classifcation of Elements Based on Electronic Confguration
Prediction of period and group number of an element from its electronic confguration
Neil Bohr’s classifcation
Naming of super heavy elements
2.3 Periodic Trends in Properties
Atomic radius
Ionic radius
Ionization energy
Applications of ionization energy
Electron affnity
Electronegativity

Lattice energy
Hydration energy
Ionic mobility
Single Correct Choice Type Questions
Multiple Correct Choice Type Questions

Comprehension Type Questions

Assertion–Reasoning Type Questions

Integer Answer Type Questions

Matrix–Match Type Questions
Answers

TOC.indd 15

vii

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27
32
32
33
34
34
34
35
35
38

39
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41
43
46
46
47
48
51
52
55
55
56
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xvi

Contents

3. Chemical Bonding

59

3.1Attainment of a Stable ­Confguration
60
3.2 Types of Bonds
60
3.3 Transitions Between the Main Types of Bonding
61
Ionic bonds
61
Covalent bonds
62
Oxidation numbers
63
Coordinate bonds
63
Double and triple bonds
64
Metallic bonds and metallic structures
64
3.4 The Covalent Bond
64
The Lewis theory
64
Sidgwick–Powell theory
66

3.5 Valence Bond Theory
66
What is the essence of hybridization?

66
Features of hybrid orbitals 
67
Calculation of steric number
68
3.6Valence Shell Electron Pair Repulsion (Vsepr) ­Theory
69
Effect of lone pair
69
Effect of double bond
73
Effect of electronegativity
73
Back bonding
75
3.7The Extent of d Orbital Participation in Molecular Bonding
79
3.8 Types of Covalent Bonds (Sigma (s ) and Pi (p ) Bonds)
80
Bridge bonding
83
3.9 Molecular Orbital Method
85
3.10
Lcao Method
85
s–s combinations of orbitals
86
s–p combinations of orbitals
87

p–p combinations of orbitals
88
p–d combinations of orbitals
89
d–d combinations of orbitals
89
Non-bonding combinations of orbitals
89
3.11 Rules for Linear Combination of Atomic Orbitals
90
3.12Examples of Molecular Orbital Treatment for Homonuclear Diatomic Molecules
92
H+2 molecule ion
93
H2 molecule
93
+
He2  molecule ion
93
He2 molecule
94
Li2 molecule
94
Be2 molecule
94
B2 molecule
94
C2 molecule
94
N2 molecule

95
O2 molecule
95
O-2 ion
95
F2 molecule
96
3.13Examples of Molecular Orbital Treatment for ­Heteronuclear Diatomic Molecules
96
NO molecule
97
CO molecule
97
3.14 Dipole Moment
98
Application of dipole moment
100
Some special cases102

TOC.indd 16

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Contents

TOC.indd 17

xvii

3.15 The Ionic Bond

104
Radius ratio rules
104
Calculation of some limiting radius ratio values
105
3.16 Close Packing
106
3.17 Ionic Compounds of the Type AX (ZnS, NaCl, CsCl)
108
Structures of zinc sulphide
108
Sodium chloride structure
108
Caesium chloride structure
108
3.18 Ionic Compounds of the Type AX2 (CaF2, TiO2, SiO2)109
Calcium fuoride (fuorite) structure
109
Rutile structure
109
b-cristobalite (silica) structure
110
3.19 Layer Structures (Cdi2, Cdcl2, [NiAs])
110
Cadmium iodide structure
110
Cadmium chloride structure
111
Nickel arsenide structure
111

3.20 Lattice Energy
111
3.21 Stoichiometric Defects
114
Schottky defects
115
Frenkel defects
115
3.22 Nonstoichiometric Defects
116
Metal excess
116
Metal defciency
117
3.23 Born–Haber Cycle 
118
3.24Polarizing Power and Polarizability – Fajans’ Rules
119
Properties of ionic compounds affected by polarization
120
3.25 Melting Point of Ionic Compounds
121
3.26 Solubility of Ionic Compounds
123
Prediction of solubility order in ionic compounds 
124
3.27 Electrical Conductivity and Colour
126
3.28 Acidic Nature of Oxides
127

3.29 Thermal Stability of Ionic Compounds
128
3.30 Weak Forces 
128
Attractive intermolecular forces 
128
Repulsive intermolecuar forces 
131
Lennard–Jones potential 
131
3.31Interactions between Ions and Covalent ­Molecules 
131
3.32 The Metallic Bond
132
Conductivity
132
Lustre
133
Malleability and cohesive force
133
Crystal structures of metals
135
Bond lengths
136
3.33 Theories of Bonding in Metals
137
Free electron theory
137
Valence bond theory
137

Molecular orbital or band theory
137
3.34 Conductors, Insulators and Semiconductors
139
Single Correct Choice Type Questions
140
Multiple Correct Choice Type Questions 
144
Comprehension Type Questions
147
Assertion–Reasoning Type Questions
151
Integer Answer Type Questions
152
Matrix–Match Type Questions
153
Answers154

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xviii

Contents

4.Hydrolysis

157

4.1
introduction157

4.2Hydrolysis Through SN1 Mechanism157

4.3 Hydrolysis Through SN2 Mechanism158

4.4Hydrolysis Through Addition–Elimination Mechanism
162

4.5 Hydrolysis Through Addition Mechanism
163

4.6 Hydrolysis Through Redox Reaction
163

4.7 Hydrolysis Through Push–Pull Mechanism
163

4.8 Hydrolysis Through Mixed Mechanism
164
Single Correct Choice Type Questions
166
Multiple Correct Choice Type Questions
167
Comprehension Type Questions
167
Assertion–Reasoning Type Questions
168

Integer Answer Type Questions
169
Matrix–Match Type Questions
169
Answers170

5.Coordination Compounds171


5.1Double Salts and ­Coordination Compounds 
5.2Werner’s Work 
5.3More Recent Methods of Studying Complexes 
5.4Classifcation of Ligands 
5.5Effective Atomic Number (EAN) 
Sidgwick EAN rule

5.6Shapes of d Orbitals 
5.7Bonding in Transition Metal Complexes 
Valence bond theory
Crystal feld theory
Molecular orbital theory

5.8Valence Bond Theory 

5.9Crystal Field Theory 
Octahedral complexes
5.10Effects of Crystal Field Splitting 
5.11Tetragonal Distortion of Octahedral Complexes (Jahn-Teller Distortion) 

5.12Square Planar Arrangements 

5.13Tetrahedral Complexes 

5.14Magnetism 
5.15Extension of the Crystal Field Theory to Allow for Some Covalency 
5.16Nomenclature of Coordination Compounds 

5.17Isomerism 
Polymerization isomerism
Ionization isomerism
Hydrate isomerism
Linkage isomerism
Coordination isomerism
Coordination position isomerism
Geometrical isomerism and optical isomerism
Single Correct Choice Type Questions
Multiple Correct Choice Type Questions

Comprehension Type Questions

Assertion–Reasoning Type Questions

Integer Answer Type Questions

Matrix–Match Type Questions
Answers


TOC.indd 18

171
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181
181
181
181
182
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189
191
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201
206

209
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211
212
212
214

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Contents

6.Metallurgy

TOC.indd 19

6.1 Types of Ores  
6.2Principal Steps in the Recovery of a Metal from its Ore  
6.3 Concentration or Dressing of Ore 
Gravity separation or levigation
Magnetic separation
Froth foatation or oil foatation
Chemical method of separation: leaching
6.4 Conversion of Concentrated Ore into its Oxide
Calcination
Roasting
6.5 Different Reduction Processes  
Carbon reduction
Self reduction
Thermite reduction (or Goldschmidt-Thermite process)
Metal replacement method (Hydrometallurgy)
Electrolytic reduction

Thermal decomposition method
6.6 Purifcation or Refning of Metal 
Thermal refning
Electrorefning
6.7 Thermodynamics of Reduction Process 
6.8 Alloys and Amalgams 
Classifcation of alloys
Characteristics of alloys
Preparation of alloys
Amalgam
6.9 Different Types of Furnaces Used in Metallurgy 
6.10 Extraction of Silver  
Refning of Ag
6.11 Extraction of Gold by Cyanide Process 
Refning of Au
6.12 Extraction of Tin 
Refning of Sn
6.13 Extraction of Magnesium 
Electrolytic reduction
Carbon reduction process
Other processes
6.14 Extraction of Aluminium 
Benefciation of bauxite
Electrolytic reduction of pure Al2O3
Electrorefning of aluminium
6.15 Extraction of Lead 
Carbon reduction
Self reduction process
Refning of lead
6.16 Extraction of Copper 

Refning of blister copper
6.17 Extraction of Zinc 
6.18 Extraction of Iron 
Purifcation of iron or preparation of wrought iron
Steel making
Single Correct Choice Type Questions
Multiple Correct Choice Type Questions

xix

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218
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219
220
220
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223
224
224
225
225
226
226
226

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Contents


Comprehension Type Questions

Assertion–Reasoning Type Questions

Integer Answer Type Questions

Matrix–Match Type Questions
Answers

7. Qualitative Salt Analysis

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Tests for Acid Radicals
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7.1 Action of Dilute Acids
264
7.2 Tests for CO32-/Hco3- and SO32-/Hso3- Radicals

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Distinction between carbonate and bicarbonate
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Detection of carbonate and bicarbonate when both are present ­together
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Distinction between sulphite and bisulphite
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Some other tests for SO32- ions
270
7.3 Tests for Sulphide (S2-) Radical
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7.4 Tests for Thiosulphate (S2o2273
3 ) Radical
7.5 Tests for Nitrite (No-2) Radical
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7.6 Tests for Acetate, Formate and Oxalate Radicals
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Specifc test for acetate (cacodyl oxide test)
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Specifc test for formate (mercury (II) formate test)
279
Specifc tests for oxalate
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7.7 Tests for Halide (Cl-, Br-, I-) Radicals280
Specifc test for Cl - (chromyl chloride test)
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Specifc test for Br- and I - (layer test)
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Other test for Br−
282

Other tests for I −
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7.8 Tests for Nitrate (No-3) Radical
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7.9 Tests for Sulphate (So42-) Radical
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7.10 Tests for Borate (Bo33- ) Radical
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7.11 Tests for Phosphate (Po43-) Radical
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7.12Tests for Chromate (Cro42-) and Dichromate (Cr 2o72-) Radicals
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7.13Tests for Permanganate (Mno-4) and Manganate (Mno42-) Radicals
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Tests for Basic Radicals
7.14 Dry Tests for Basic Radicals
Heating effects on the dry sample
Flame test
Borax bead test
Sodium carbonate bead test
7.15 Wet Tests for Basic Radicals
Classifcation of cations (group analysis)
7.16 Some General Tests for Cations
Tests for group V cations
Tests for group vi and zero group cations
7.17 Specifc Tests for Some Cations

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eating Effects
H
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Single Correct Choice Type Questions
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Multiple Correct Choice Type Questions
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Comprehension Type Questions
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Assertion–Reasoning Type Questions
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Integer Answer Type Questions
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Matrix–Match Type Questions
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Answers319

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8. Hydrogen and the Hydrides

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321


8.1
8.2

8.3

8.4

8.5

Electronic Structure
321
Position in the Periodic Table
322
Abundance of Hydrogen
322
Preparation of Hydrogen
322

Properties of Molecular Hydrogen
323
Physical properties
323
Chemical properties
323
Use of hydrogen as fuel
324

8.6 Isotopes of Hydrogen
325
8.7Ortho and Para Hydrogen
326

8.8Hydrides
327
Ionic or salt-like hydrides
327
Covalent hydrides
328
Metallic (or interstitial) hydrides
329
Intermediate hydrides
330

8.9 The Hydrogen Ion
330

8.10 Hydrogen Bonding
330

Intermolecular hydrogen bonding
331
Intramolecular hydrogen bonding
334
Strength of hydrogen bonding
337
Extent of hydrogen bonding
338
Special cases of hydrogen bonding
338
Single Correct Choice Type Questions
339
Multiple Correct Choice Type Questions
340
Comprehension Type Questions
340
Assertion–Reasoning Type Questions
341
Integer Answer Type Questions
342
Matrix–Match Type Questions
342
Answers343

9.The s-Block Elements and their Compounds

345

roup 1 – The Alkali Metals
G

9.1 General Properties
Electronic structure
Size of atoms and ions
Density
Ionization energy
Electronegativity and bond type

9.2Structures of the Metals, Hardness and Cohesive Energy
Melting and boiling points

9.3 Flame Colours and Spectra

9.4 Colour of Compounds

9.5 Chemical Properties
Reaction with water
Reaction with air
Reaction with dinitrogen

9.6 Oxides, Hydroxides, Peroxides and Superoxides
Reaction with air
Normal oxides – monoxides
Hydroxides
Peroxides and superoxides
9.7Sulphides

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9.8  Oxosalts – Carbonates, Bicarbonates, Nitrates, Nitrites and Sulphates
9.9  Halides and Polyhalides
9.10Hydrides

9.11 Solubility and Hydration

9.12 Solutions of Metals in Liquid Ammonia

9.13 Compounds with Carbon

9.14 Complexes, Crowns and Crypts

9.15 Biological Importance

9.16Differences between Lithium and the Other Group 1 Elements

9.17 Preparation of Sodium Hydroxide

9.18 Electrolytic Processes
Diaphragm cell
Mercury cathode cell

9.19 Preparation of Sodium Carbonate

9.20 The Solvay (or Ammonia – Soda) Process

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Group 2 – The Alkaline Earth Elements
365
9.21 General Properties
366
Electronic structure
366
Size of atoms and ions
366
Ionization energy
367
Electronegativity
367
Hydration energies
367
Solubility and lattice energy
368
Solutions of the metals in liquid ammonia

368

9.22 Anomalous Behaviour of Beryllium
369

9.23 Chemical Properties
370
Reaction with water
370
9.24Hydroxides
371

9.25 Hardness of Water
371

9.26 Reaction with Acids and Bases
372

9.27 Oxides and Peroxides
372
9.28Sulphates
374
9.29Nitrates
374
9.30Hydrides
375
9.31Halides
375
9.32Nitrides
376

9.33 Carbides
376
9.34Complexes
377

9.35 Biological Role of Mg2+ and Ca2+379

9.36Differences between Beryllium and the Other Group 2 Elements
379
Single Correct Choice Type Questions
380
Multiple Correct Choice Type Questions
381
Comprehension Type Questions
382
Assertion–Reasoning Type Questions
383
Integer Answer Type Questions
383
Matrix–Match Type Questions384
Answers384


10.  The p-Block Elements and their Compounds


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Part 1: The Group 13 Elements

10.1 Oxidation States and Types of Bonds
The (+III) oxidation state
The (+I) oxidation state – the ‘inert pair effect’
10.2  General Properties
Melting points, boiling points and structures

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Size of atoms and ions
Electropositive character
Ionization energy

10.3 Preparation of Boron

10.4 Reactions of Boron

10.5 Reactions of the Other Elements

Reaction with water and air
Reaction with acids and alkalis
Reaction with dioxygen
Reaction with the halogens and sulphate
Alums
Cement

10.6 Compounds of Boron and Oxygen
Boron sesquioxide and the borates
Acidic properties of H3BO3 or B(OH)3
Structures of borates
Borax
Sodium peroxoborate
Qualitative analysis of boron compounds
Fluoboric acid

10.7 The Other Group 13 Oxides
Preparation of Al2O3
Amphoteric behaviour – aluminates

10.8 Tetrahydridoborates (Borohydrides)
10.9Halides
Trihalides
Dihalides
        10.10 Complexes

10.11 Differences Between Boron and the Other ­Elements (Anomalous Behaviour of Boron)

10.12 Boron Hydrides
Compounds known

Preparation

10.13 Reactions of the Boranes
Hydroboration
Reaction with ammonia
Some other reactions of boranes

10.14 Structures of the Boranes

10.15Organometallic Compounds
Single Correct Choice Type Questions
Multiple Correct Choice Type Questions
Comprehension Type Questions
Assertion–Reasoning Type Questions
Integer Answer Type Questions
Matrix–Match Type Questions
Answers






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Part 2: The Group 14 Elements
10.16 Structure and Allotropy of the Elements
10.17Differences Between Carbon, Silicon and the ­Remaining Elements
10.18 Physical Properties
Covalent radii

Ionization energy
Melting points
Metallic and non-metallic character
Four-covalent compounds
10.19 Chemical Reactivity

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