NIRBHAY SHARMA CHEMICAL BONDING
CHEMICAL BONDING
A Comprehensive Textbook for Classes 11 & 12
Table of Contents
PART I: FOUNDATIONS OF CHEMICAL BONDING (Class 11)
• Chapter 1: Introduction to Chemical Bonding
• Chapter 2: Ionic Bonding
• Chapter 3: Covalent Bonding
• Chapter 4: Metallic Bonding
• Chapter 5: Intermolecular Forces
PART II: ADVANCED CONCEPTS (Class 12)
• Chapter 6: Valence Bond Theory
• Chapter 7: Molecular Orbital Theory
• Chapter 8: Coordination Compounds and Bonding
• Chapter 9: Crystal Field Theory
• Chapter 10: Special Topics and Applications
PART I: FOUNDATIONS OF CHEMICAL BONDING
Chapter 1: Introduction to Chemical Bonding
1.1 What is a Chemical Bond?
A chemical bond is the attractive force that holds atoms together in molecules and
compounds. The formation of chemical bonds is driven by the tendency of atoms to
achieve a more stable electronic configuration, typically resembling the nearest noble gas
configuration.
1
, NIRBHAY SHARMA CHEMICAL BONDING
1.2 Types of Chemical Bonds
Chemical bonds are primarily classified into three main types:
1. Ionic Bonds - Formed by complete transfer of electrons
2. Covalent Bonds - Formed by sharing of electrons
3. Metallic Bonds - Formed by delocalized electrons in metals
1.3 Octet Rule
The octet rule states that atoms tend to gain, lose, or share electrons to achieve eight
electrons in their outermost shell (valence shell). This rule explains the formation of most
chemical bonds.
Exceptions to Octet Rule:
• Hydrogen (duplet rule - 2 electrons)
• Elements with less than 8 electrons (like BF₃)
• Elements with more than 8 electrons (like SF₆)
1.4 Lewis Dot Structures
Lewis structures represent the valence electrons of atoms as dots around the chemical
symbol. They help visualize how electrons are arranged in molecules and predict bonding
patterns.
Steps to draw Lewis structures:
1. Count total valence electrons
2. Arrange atoms (least electronegative in center)
3. Connect atoms with single bonds
4. Distribute remaining electrons to satisfy octet rule
5. Form multiple bonds if necessary
2
CHEMICAL BONDING
A Comprehensive Textbook for Classes 11 & 12
Table of Contents
PART I: FOUNDATIONS OF CHEMICAL BONDING (Class 11)
• Chapter 1: Introduction to Chemical Bonding
• Chapter 2: Ionic Bonding
• Chapter 3: Covalent Bonding
• Chapter 4: Metallic Bonding
• Chapter 5: Intermolecular Forces
PART II: ADVANCED CONCEPTS (Class 12)
• Chapter 6: Valence Bond Theory
• Chapter 7: Molecular Orbital Theory
• Chapter 8: Coordination Compounds and Bonding
• Chapter 9: Crystal Field Theory
• Chapter 10: Special Topics and Applications
PART I: FOUNDATIONS OF CHEMICAL BONDING
Chapter 1: Introduction to Chemical Bonding
1.1 What is a Chemical Bond?
A chemical bond is the attractive force that holds atoms together in molecules and
compounds. The formation of chemical bonds is driven by the tendency of atoms to
achieve a more stable electronic configuration, typically resembling the nearest noble gas
configuration.
1
, NIRBHAY SHARMA CHEMICAL BONDING
1.2 Types of Chemical Bonds
Chemical bonds are primarily classified into three main types:
1. Ionic Bonds - Formed by complete transfer of electrons
2. Covalent Bonds - Formed by sharing of electrons
3. Metallic Bonds - Formed by delocalized electrons in metals
1.3 Octet Rule
The octet rule states that atoms tend to gain, lose, or share electrons to achieve eight
electrons in their outermost shell (valence shell). This rule explains the formation of most
chemical bonds.
Exceptions to Octet Rule:
• Hydrogen (duplet rule - 2 electrons)
• Elements with less than 8 electrons (like BF₃)
• Elements with more than 8 electrons (like SF₆)
1.4 Lewis Dot Structures
Lewis structures represent the valence electrons of atoms as dots around the chemical
symbol. They help visualize how electrons are arranged in molecules and predict bonding
patterns.
Steps to draw Lewis structures:
1. Count total valence electrons
2. Arrange atoms (least electronegative in center)
3. Connect atoms with single bonds
4. Distribute remaining electrons to satisfy octet rule
5. Form multiple bonds if necessary
2
