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1.4 Crystal Lattices and Unit Cells
1.3 Classification of Crystalline Solids
1.2 Amorphous and Crystalline Solids
1.1 General Characteristics of Solid State
Unit 1 - The Solid State

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4.3 Bond Parameters

4.3 Bond Parameters

October 15, 2019April 21, 2020 Mounika

Bond parameters include Bond length, bond angle, bond enthalapy, bond order.

The following sections explain each in detail.

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4.2.1 Lattice Enthalpy

4.3.1 Bond Length

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Unit 1 – Some Basic Concepts Of Chemistry

1.1 Importance Of Chemistry

1.2 Nature Of Matter

1.2.1 States Of Matter
1.2.2. Classification of Matter

1.3 Properties Of Matter And Their Measurement

1.3.1 Physical And Chemical Properties
1.3.2 Measurement Of Physical Properties
1.3.3 The International System of Units (SI)

1.4 Uncertainty In Measurement

1.4.1 Scientific Notation
1.4.2 Significant Figures
1.4.3 Dimensional Analysis

1.5 Laws Of Chemical Combinations

1.6 Dalton’s Atomic Theory

1.7 Atomic And Molecular Masses

1.8 Mole Concept And Molar Masses

1.9 Percentage Composition

1.9.1 Empirical Formula for Molecular Formula

1.10 Stoichiometry And Stoichiometric Calculations

Unit 1 – Some Basic Concepts Of Chemistry – Summary

Class 11 – Chemistry Part 1 – Problems and Solutions

Unit 1 – Some Basic Concepts of Chemistry – Exercise

Unit-2 -Structure Of Atom

2.1 Discovery Of Sub-atomic Particles

2.2 Atomic Models

2.2.1 Thomson Model of Atom
2.2.2 Rutherford’s Nuclear Model of Atom
2.2.3 Atomic Number and Mass Number
2.2.4 Isobars and Isotopes
2.2.5 Drawbacks of Rutherford Model

2.3 Developments Leading To The Bohr’s Model Of Atom

2.3.1 Wave Nature of Electromagnetic Radiation
2.3.2 Particle Nature of Electromagnetic Radiation: Planck’s Quantum Theory
2.3.3 Evidence for the quantized* Electronic Energy Levels: Atomic spectra

2.4 Bohr’s Model For Hydrogen Atom

2.4.1 Explanation of Line Spectrum of Hydrogen

Unit – 3 Classification Of Elements And Periodicity In Properties

3.1 Why Do We Need To Classify Elements ?

3.2 Genesis Of Periodic Classification

3.3 Modern Periodic Law And The Present Form Of The Periodic Table

3.4 Nomenclature Of Elements With Atomic Numbers > 100

3.5 Electronic Configurations Of Elements And The Periodic Table

3.6 Electronic Configurations And Types Of Elements: S-, P-, D-, F- Blocks

3.7 Periodic Trends In Properties Of Elements

3.7.1 Trends in Physical Properties
3.7.2 Periodic Trends in Chemical Properties
3.7.3 Periodic Trends and Chemical Reactivity

Unit 3 – Classification Of Elements And Periodicity In Properties – Summary

Unit 4 – Chemical Bonding And Molecular Structure

4.1 Kössel-lewis Approach To Chemical Bonding

4.1.1 Octet Rule
4.1.2 Covalent Bond
4.1.3 Lewis Representation of Simple Molecules (the Lewis Structures)
4.1.4 Formal Charge
4.1.5 Limitations of the Octet Rule

4.2 Ionic Or Electrovalent Bond

4.2.1 Lattice Enthalpy

4.3 Bond Parameters

4.3.1 Bond Length
4.3.2 Bond Angle
4.3.3 Bond Enthalpy
4.3.4 Bond Order
4.3.5 Resonance Structures
4.3.6 Polarity of Bonds

4.4 The Valence Shell Electron Pair Repulsion (VSEPR) Theory

4.5 Valence Bond Theory

4.5.1 Orbital Overlap Concept
4.5.2 Directional Properties of Bonds
4.5.3 Overlapping of Atomic Orbitals
4.5.4 Types of Overlapping and Nature of Covalent Bonds
4.5.5 Strength of Sigma and pi Bonds

4.6 Hybridisation

4.6.1 Types of Hybridisation
4.6.2 Other Examples of sp3, sp2 and sp Hybridisation
4.6.3 Hybridisation of Elements involving d Orbitals

4.7 Molecular Orbital Theory

4.7.1 Formation of Molecular Orbitals Linear Combination of Atomic Orbitals (LCAO)
4.7.2 Conditions for the Combination of Atomic Orbitals
4.7.3 Types of Molecular Orbitals
4.7.4 Energy Level Diagram for Molecular Orbitals
4.7.5 Electronic Configuration and Molecular Behaviour

4.8 Bonding In Some Homonuclear Diatomic Molecules

4.9 Hydrogen Bonding

4.9.1 Cause of Formation of Hydrogen Bond
4.9.2 Types of H-Bonds

Unit 4 – Chemical Bonding And Molecular Structure – Summary

Unit 5 – States Of Matter

5.1 Intermolecular Forces

5.1.1 Dispersion Forces or London Forces
5.1.2 Dipole – Dipole Forces
5.1.3 Dipole–Induced Dipole Forces
5.1.4 Hydrogen bond

5.2 Thermal Energy

5.3 Intermolecular Forces Vs Thermal Interactions

5.4 The Gaseous State

5.5 The Gas Laws

5.5.1 Boyle’s Law (Pressure – Volume Relationship)
5.5.2 Charles’ Law (Temperature – Volume Relationship)
5.5.3 Gay Lussac’s Law (Pressure-Temperature Relationship)
5.5.4 Avogadro Law (Volume – Amount Relationship)

5.6 Ideal Gas Equation

5.6.1 Density and Molar Mass of a Gaseous Substance
5.6.2 Dalton’s Law of Partial Pressures

5.7 Kinetic Energy And Molecular Speeds

5.8 Kinetic Molecular Theory Of Gases

5.9 Behaviour Of Real Gases: Deviation From Ideal Gas Behaviour

5.10 Liquifaction Of Gases

5.11 Liquid State

5.11.1 Vapour Pressure
5.11.2 Surface Tension
5.11.3 Viscosity

Unit 5 – States Of Matter – Summary

Unit 6 – Thermodynamics

6.1 Thermodynamic Terms

6.1.1 The System and the Surroundings
6.1.2 Types of the System
6.1.3 The State of the System
6.1.4 The Internal Energy as a State Function

6.2 Applications

6.2.1 Work
6.2.2 Enthalpy, H

6.3 Measurement Of Du And Dh: Calorimetry

6.4 Enthalpy Change, ∆rh Of A Reaction – Reaction Enthalpy

6.5 Enthalpies For Different Types Of Reactions

6.6 Spontaneity

6.7 Gibbs Energy Change And Equilibrium

Unit 6- Thermodynamics -Summary

Unit 7 – Equilibrium

7.1 Equilibrium In Physical Processes

7.1.1 Solid-Liquid Equilibrium
7.1.2 Liquid-Vapour Equilibrium
7.1.3 Solid – Vapour Equilibrium
7.1.4 Equilibrium Involving Dissolution of Solid or Gases in Liquids
7.1.5 General Characteristics of Equilibria Involving Physical Processes

7.2 Equilibrium In Chemical Processes – Dynamic Equilibrium

7.2.1 Dynamic Equilibrium – A Student’s Activity

7.3 Law of Chemical Equilibrium And Equilibrium Constant

7.4 Homogeneous Equilibria

7.4.1 Equilibrium Constant in Gaseous Systems

7.5 Heterogeneous Equilibria

7.6 Applications Of Equilibrium Constants

7.6.1 Predicting the Extent of a Reaction
7.6.2 Predicting the Direction of the Reaction
7.6.3 Calculating Equilibrium Concentrations

7.7 Relationship Between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G

7.8 Factors Affecting Equilibria

7.8.1 Effect of Concentration Change
7.8.2 Effect of Pressure Change
7.8.3 Effect of Inert Gas Addition
7.8.4 Effect of Temperature Change
7.8.5 Effect of a Catalyst

7.9 Ionic Equilibrium In Solution

7.10 Acids, Bases And Salts

7.10.1 Arrhenius Concept of Acids and Bases
7.10.2 The Brönsted-Lowry Acids and Bases
7.10.3 Lewis Acids and Bases

7.11 Ionization of Acids And Bases

7.11.1 The Ionization Constant of Water and its Ionic Product
7.11.2 The pH Scale
7.11.3 Ionization Constants of Weak Acids
7.11.4 Ionization of Weak Bases
7.11.5 Relation between Ka and Kb
7.11.6 Di- and Polybasic Acids and Di- and Polyacidic Bases
7.11.7 Factors Affecting Acid Strength
7.11.8 Common Ion Effect in the Ionization of Acids and Bases
7.11.9 Hydrolysis of Salts and the pH of their Solutions

7.12 Buffer Solutions

7.12.1 Designing Buffer Solution

7.13 Solubility Equilibria Of Sparingly Soluble Salts

7.13.1 Solubility Product Constant
7.13.2 Common Ion Effect on Solubility of Ionic Salts

Unit 7 – Equilibrium – Summary

Unit 8 – Redox Reactions

8.1 Classical Idea Of Redox Reactions – Oxidation And Reduction Reactions

8.2 Redox Reactions In Terms Of Electron Transfer Reactions

8.2.1 Competitive Electron Transfer Reactions

8.3 Oxidation Number

8.3.1 Types of Redox Reactions
8.3.2 Balancing of Redox Reactions
8.3.3 Redox Reactions as the Basis for Titrations
8.3.4 Limitations of Concept of Oxidation Number

8.4 Redox Reactions And Electrode Processes

Unit 9 – Hydrogen

9.1 Position Of Hydrogen In The Periodic Table

9.2 Dihydrogen, H2

9.3 Preparation Of Dihydrogen, H2

9.4 Properties Of Dihydrogen

9.5 Hydrides

9.6.1 Physical Properties of Water
9.6.2 Structure of Water
9.6.3 Structure of Ice
9.6.4 Chemical Properties of Water
9.6.5 Hard and Soft Water
9.6.6 Temporary Hardness
9.6.7 Permanent Hardness

9.7 Hydrogen Peroxide (H2O2)

9.7.1 Preparation
9.7.2 Physical Properties
9.7.3 Structure
9.7.4 Chemical Properties
9.7.5 Storage
9.7.6 Uses

9.8 Heavy Water, D2O

9.9 Dihydrogen as a Fuel

Chapter 9 – Hydrogen – Summary

Unit 10 – The s-Block Elements

10.1 Group 1 Elements: Alkali Metals
10.2 General Characteristics Of The Compounds Of The Alkali Metals
10.3 Anomalous Properties Of Lithium
10.4 Some Important Compounds Of Sodium
10.5 Biological Importance Of Sodium And Potassium
10.6 Group 2 Elements : Alkaline Earth Metals
10.7 General Characteristics Of Compounds Of The Alkaline Earth Metals
10.8 Anomalous Behaviour Of Beryllium
10.9 Some Important Compounds Of Calcium
10.10 Biological Importance Of Magnesium And Calcium
Chapter 10 – The s-Block Elements – summary

Unit 11 – The p-block Elements

11.1 Group 13 Elements: The Boron Family
11.2 Important Trends And Anomalous Properties Of Boron
11.3 Some Important Compounds Of Boron
11.4 Uses Of Boron And Aluminium And Their Compounds
11.5 Group 14 Elements: The Carbon Family
11.6 Important Trends And Anomalous Behaviour Of Carbon
11.7 Allotropes Of Carbon
11.8 Some Important Compounds Of Carbon And Silicon
Unit 11 – The p-block Elements – Summary

Unit 12 – Organic Chemistry – Some Basic Principles And Techniques

12.1 General Introduction

12.2 Tetravalence Of Carbon: Shapes Of Organic Compounds

12.3 Structural Representations Of Organic Compounds

12.4 Classification Of Organic Compounds

12.5 Nomenclature Of Organic Compounds

12.6 Isomerism

12.7 Fundamental Concepts In Organic Reaction Mechanism

12.7.1 Fission of a Covalent Bond
12.7.2 Substrate and Reagent
12.7.3 Electron Movement in Organic Reactions
12.7.4 Electron Displacement Effects in Covalent Bonds
12.7.5 Inductive Effect
12.7.6 Resonance Structure
12.7.7 Resonance Effect
12.7.8 Electromeric Effect (E effect)
12.7.9 Hyperconjugation
12.7.10 Types of Organic Reactions and Mechanisms

12.8 Methods Of Purification Of Organic Compounds

12.8.1 Sublimation
12.8.2 Crystallisation
12.8.3 Distillation
12.8.4 Differential Extraction
12.8.5 Chromatography

12.9 Qualitative Analysis Of Organic Compounds

12.10 Quantitative Analysis

Unit 12 – Organic Chemistry – Summary

Unit 13 – Hydrocarbons

13.1 Classification

13.2 Alkanes

13.2.1 Nomenclature and Isomerism
13.2.2 Preparation
13.2.3 Properties
13.2.4 Conformations

13.3 Alkenes

13.3.1 Structure of Double Bond
13.3.2 Nomenclature
13.3.3 Isomerism
13.3.4 Preparation
13.3.5 Properties

13.4 Alkynes

13.4.1 Nomenclature and Isomerism
13.4.2 Structure of Triple Bond
13.4.3 Preparation
13.4.4 Properties

13.5 Aromatic Hydrocarbon

13.5.1 Nomenclature and Isomerism
13.5.2 Structure of Benzene
13.5.3 Aromaticity
13.5.4 Preparation of Benzene
13.5.5 Properties
13.5.6 Directive influence of a functional group in monosubstituted benzene

13.6 Carcinogenicity And Toxicity

Unit 13 – Hydrocarbons – Summary

Unit 14 – Environmental Chemistry

14.1 Environmental Pollution

14.2 Atmospheric Pollution

14.2.1 Tropospheric Pollution
14.2.2 Stratospheric Pollution

14.3 Water Pollution

14.4 Soil Pollution

14.5 Industrial Waste

14.6 Strategies To Control Environmental Pollution

14.7 Green Chemistry

Unit 14 – Environmental Chemistry – summary

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