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The Most Accepted
CRASH COURSE
PROGRAMME
JEE Main
in
40 D AYS
CHEMISTRY
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The Most Accepted
CRASH COURSE
PROGRAMME
JEE Main
in
40 D AYS
CHEMISTRY
ARIHANT PRAKASHAN (Series), MEERUT
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Arihant Prakashan (Series), Meerut
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accuracy of any information published and the damages or loss suffered there upon.
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PREFACE
It is a fact that nearly 10 lacs students would be in the race with you in JEE Main, the gateway
to some of the prestigious engineering and technology institutions in the country, requires
that you take it seriously and head-on. A slight underestimation or wrong guidance will ruin
all your prospects. You have to earmark the topics in the syllabus and have to master them in
concept-driven-problem-solving ways, considering the thrust of the questions being asked in
JEE Main.
The book 40 Days JEE Main Chemistry serves the above cited purpose in perfect manner. At
whatever level of preparation you are before the exam, this book gives you an accelerated way
to master the whole JEE Main Physics Syllabus. It has been conceived keeping in mind the
latest trend of questions, and the level of different types of students.
The whole syllabus of Physics has been divided into day-wise-learning modules with clear
groundings into concepts and sufficient practice with solved and unsolved questions on that
day. After every few days you get a Unit Test based upon the topics covered before that day.
On last three days you get three full-length Mock Tests, making you ready to face the test. It is
not necessary that you start working with this book in 40 days just before the exam. You may
start and finish your preparation of JEE Main much in advance before the exam date. This will
only keep you in good frame of mind and relaxed, vital for success at this level.
Salient Features
Ÿ Concepts discussed clearly and directly without being superfluous. Only the required
material for JEE Main being described comprehensively to keep the students focussed.
Ÿ Exercises for each day give you the collection of only the Best Questions of the concept,
giving you the perfect practice in less time.
Ÿ Each day has two Exercises; Foundation Questions Exercise having Topically Arranged
Questions & Progressive Question Exercise having higher Difficulty Level Questions.
Ÿ All types of Objective Questions included in Daily Exercises (Single Option Correct,
Assertion & Reason, etc).
Ÿ Along with Daywise Exercises, there above also the Unit Tests & Full Length Mock Tests.
Ÿ At the end, there are all Online Solved Papers of JEE Main 2019; January & April attempts.
We are sure that 40 Days Physics for JEE Main will give you a fast way to prepare for Physics
without any other support or guidance.
Publisher
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CONTENTS
Preparing JEE Main 2020 Chemistry in 40 Days !
Day 1. Some Basic Concepts of Chemistry 1-11
Day 2. States of Matter 12-28
Day 3. Atomic Structure 29-42
Day 4. Chemical Bonding and Molecular Structure 43-56
Day 5. Unit Test 1 (General Chemistry) 57-62
Day 6. Chemical Thermodynamics 63-75
Day 7. Thermochemistry 76-85
Day 8. Solutions 86-99
Day 9. Physical and Chemical Equilibrium 100-112
Day 10. Ionic Equilibrium 113-124
Day 11. Unit Test 2 (Physical Chemistry-I) 125-131
Day 12. Redox Reactions 132-138
Day 13. Electrochemistry 139-152
Day 14. Chemical Kinetics 153-165
Day 15. Adsorption and Catalysis 166-173
Day 16. Colloidal State 174-181
Day 17. Unit Test 3 (Physical Chemistry-II) 182-188
Day 18. Classification and Periodicity of Elements 189-199
Day 19. General Principles and Processes of Isolation of Metals 200-209
Day 20. Hydrogen 210-218
Day 21. s-Block Elements 219-229
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Day 22. p-Block Elements (Group 13 to Group 18) 230-252
Day 23. The d-and f-Block Elements 253-264
Day 24. Coordination Compounds 265-278
Day 25. Unit Test 4 (Inorganic Chemistry) 279-283
Day 26. Environmental Chemistry 284-293
Day 27. General Organic Chemistry 294-310
Day 28. Hydrocarbons 311-327
Day 29. Organic Compounds Containing Halogens 328-343
Day 30. Organic Compounds Containing Oxygen 344-373
Day 31. Organic Compounds Containing Nitrogen 374-389
Day 32. Unit Test 5 (Organic Chemistry-I) 390-397
Day 33. Polymers 398-408
Day 34. Biomolecules 409-421
Day 35. Chemistry in Everyday Life 422-429
Day 36. Analytical Chemistry 430-443
Day 37. Unit Test 6 (Organic Chemistry-II) 444-448
Day 38. Mock Test 1 449-454
Day 39. Mock Test 2 455-459
Day 40. Mock Test 3 460-465
Online JEE Main Solved Papers 2019 1-32
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SYLLABUS
CHEMISTRY
SECTION- A (Physical Chemistry)
UNIT 1 models and their limitations; Nature of
Some Basic Concepts in Chemistry electromagnetic radiation, photoelectric effect;
spectrum of hydrogen atom, Bohr model of hydrogen
Matter and its nature, Dalton's atomic theory;
atom - its postulates, derivation of the relations for
Concept of atom, molecule, element and compound;
energy of the electron and radii of the different orbits,
Physical quantities and their measurements in
limitations of Bohr's model; dual nature of matter, de-
Chemistry, precision and accuracy, significant
Broglie's relationship, Heisenberg uncertainty
figures, S.I. Units, dimensional analysis; Laws of
principle.
chemical combination; Atomic and molecular
masses, mole concept, molar mass, percentage Elementary ideas of quantum mechanics, quantum
composition, empirical and molecular formulae; mechanical model of atom, its important features,
Chemical equations and stoichiometry. ψ and ψ2, concept of atomic orbitals as one electron
wave functions; Variation of ψ and ψ2 with r for 1s and
UNIT 2 States of Matter 2s orbitals; various quantum numbers (principal,
angular momentum and magnetic quantum numbers)
Classification of matter into solid, liquid and gaseous
and their significance; shapes of s, p and d - orbitals,
states.
electron spin and spin quantum number; rules for
Gaseous State Measurable properties of gases; Gas
filling electrons in orbitals – aufbau principle, Pauli's
laws - Boyle's law, Charle's law, Graham's law of
exclusion principle and Hund's rule, electronic
diffusion, Avogadro's law, Dalton's law of partial
configuration of elements, extra stability of half-filled
pressure; Concept of Absolute scale of
and completely filled orbitals.
temperature; Ideal gas equation, Kinetic theory of
gases (only postulates); Concept of average, root
UNIT 4 Chemical Bonding and
mean square and most probable velocities; Real
Molecular Structure
gases, deviation from Ideal behaviour,
compressibility factor, van der Waals’ Kossel Lewis approach to chemical bond formation,
concept of ionic and covalent bonds.
Equation, liquefaction of gases, critical constants.
Ionic Bonding Formation of ionic bonds, factors
Liquid State Properties of liquids - vapour pressure,
affecting the formation of ionic bonds; calculation of
viscosity and surface tension and effect of
lattice enthalpy.
temperature on them (qualitative treatment only).
Covalent Bonding Concept of electronegativity,
Solid State Classification of solids: molecular, ionic, Fajan's rule, dipole moment; Valence Shell Electron
covalent and metallic solids, amorphous and Pair Repulsion (VSEPR) theory and shapes of simple
crystalline solids (elementary idea); Bragg's Law and molecules.
its applications, Unit cell and lattices, packing in
Quantum mechanical approach to covalent
solids (fcc, bcc and hcp lattices), voids, calculations
bonding Valence bond theory - Its important features,
involving unit cell parameters, imperfection in
concept of hybridization involving s, p and d orbitals;
solids; electrical, magnetic and dielectric properties.
Resonance.
UNIT 3 Atomic Structure Molecular Orbital Theory Its important features,
LCAOs, types of molecular orbitals (bonding,
Discovery of sub-atomic particles (electron, proton
antibonding), sigma and pi-bonds, molecular orbital
and neutron); Thomson and Rutherford atomic
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electronic configurations of homonuclear diatomic multistage ionization) and ionization constants,
molecules, concept of bond order, bond length and ionization of water, pH scale, common ion effect,
bond energy. hydrolysis of salts and pH of their solutions, solubility
Elementary idea of metallic bonding. Hydrogen of sparingly soluble salts and solubility products,
bonding and its applications. buffer solutions.
UNIT 5 Chemical Thermodynamics UNIT 8
Redox Reactions and Electrochemistry
Fundamentals of thermodynamics System and
surroundings, extensive and intensive properties, Electronic concepts of oxidation and reduction, redox
state functions, types of processes. reactions, oxidation number, rules for assigning
First law of thermodynamics Concept of work, heat oxidation number, balancing of redox reactions.
internal energy and enthalpy, heat capacity, molar Eectrolytic and metallic conduction, conductance in
heat capacity, Hess's law of constant heat summation; electrolytic solutions, specific and molar
Enthalpies of bond dissociation, combustion, conductivities and their variation with
formation, atomization, sublimation, phase transition, concentration: Kohlrausch's law and its applications.
hydration, ionization and solution.
Electrochemical cells - Electrolytic and Galvanic cells,
Second law of thermodynamics Spontaneity of different types of electrodes, electrode potentials
processes; ΔS of the universe and ΔG of the system as including standard electrode potential, half - cell and
criteria for spontaneity, ΔGo (Standard Gibb's energy cell reactions, emf of a Galvanic cell and its
change) and equilibrium constant. measurement; Nernst equation and its applications;
Relationship between cell potential and Gibbs’ energy
UNIT 6 Solutions change; Dry cell and lead accumulator; Fuel cells;
Different methods for expressing concentration of Corrosion and its prevention.
solution - molality, molarity, mole fraction,
UNIT 9 Chemical Kinetics
percentage (by volume and mass both), vapour
pressure of solutions and Raoult's Law - Ideal and Rate of a chemical reaction, factors affecting the rate
non-ideal solutions, vapour pressure - composition of reactions concentration, temperature, pressure and
plots for ideal and non-ideal solutions. catalyst; elementary and complex reactions, order
Colligative properties of dilute solutions - relative and molecularity of reactions, rate law, rate constant
lowering of vapour pressure, depression of freezing and its units, differential and integral forms of zero
point, elevation of boiling point and osmotic and first order reactions, their characteristics and
pressure; Determination of molecular mass using half - lives, effect of temperature on rate of reactions -
colligative properties; Abnormal value of molar mass, Arrhenius theory, activation energy and its
van’t Hoff factor and its significance. calculation, collision theory of bimolecular gaseous
reactions (no derivation).
UNIT 7 Equilibrium
UNIT 10 Surface Chemistry
Meaning of equilibrium, concept of dynamic
equilibrium. Adsorption Physisorption and chemisorption and
their characteristics, factors affecting adsorption of
Equilibria involving physical processes
gases on solids- Freundlich and Langmuir
Solid -liquid, liquid - gas and solid - gas equilibria,
adsorption isotherms, adsorption from solutions.
Henry’s law, general characteristics of equilibrium
involving physical processes. Catalysis Homogeneous and heterogeneous, activity
and selectivity of solid catalysts, enzyme catalysis and
Equilibria involving chemical processes Law of
its mechanism.
chemical equilibrium, equilibrium constants
(K and K) and their significance, significance of ΔG and Colloidal state distinction among true solutions,
ΔGo in chemical equilibria, factors affecting colloids and suspensions, classification of
equilibrium concentration, pressure, temperature, colloids: - lyophilic, lyophobic; multi molecular,
effect of catalyst; Le -Chatelier’s principle. macromole-cular and associated colloids
(micelles), preparation and properties of colloids
Ionic equilibrium Weak and strong electrolytes,
Tyndall effect, Brownian movement,
ionization of electrolytes, various concepts of acids
electrophoresis, dialysis, coagulation and
and bases (Arrhenius, Bronsted - Lowry and Lewis)
flocculation; Emulsions and their characteristics.
and their ionization, acid-base equilibria (including
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