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1. Introduction to Chemical Bonding

Chemical bonding explains how and why atoms combine to form molecules and compounds. Atoms bond to achieve stability, usually by attaining octet configuration (noble gas structure).

🔑 Key Points:

Atoms interact through electrons

Bond formation lowers potential energy

Stability is the main driving force

🔹 2. Kossel–Lewis Approach to Chemical Bonding

This theory explains bonding using electron transfer or sharing.

Types of Bonds:

Ionic Bond – Transfer of electrons

Covalent Bond – Sharing of electrons

📌 Example:

NaCl → Ionic

H₂O → Covalent

🔹 3. Ionic Bonding

Formed between metal and non-metal atoms due to large electronegativity difference.

Characteristics:

High melting & boiling point

Soluble in water

Conduct electricity in molten or aqueous state

Factors Affecting Ionic Bond Formation:

Low ionization energy

High electron affinity

High lattice energy

🔹 4. Covalent Bonding

Formed by mutual sharing of electrons.

Types of Covalent Bonds:

Single bond (σ)

Double bond (σ + π)

Triple bond (σ + 2π)

Bond Parameters:

Bond Length

Bond Angle

Bond Energy

🔹 5. Lewis Structures

Lewis structures show valence electrons as dots.

Rules:

Total valence electrons are counted

Octet rule is applied (except H, B, expanded octet elements)

📌 Exceptions:

Incomplete octet → BF₃

Expanded octet → SF₆

Odd-electron molecules → NO

🔹 6. Formal Charge

Formal charge helps determine the most stable structure.

Formula:

Formal Charge = Valence e⁻ − Non-bonding e⁻ − ½ (Bonding e⁻)

🔹 7. VSEPR Theory

Valence Shell Electron Pair Repulsion theory predicts molecular shape.

Basic Principle:

Electron pairs repel each other and arrange to minimize repulsion.

Common Shapes:
Electron Pairs Shape
2 Linear
3 Trigonal planar
4 Tetrahedral
5 Trigonal bipyramidal
6 Octahedral

📌 Lone pairs distort geometry.

🔹 8. Valence Bond Theory (VBT)

Explains bonding through orbital overlap.

Types of Overlap:

σ bond – head-on overlap

π bond – side-wise overlap

Hybridization:
Hybridization Shape Example
sp Linear BeCl₂
sp² Trigonal planar BF₃
sp³ Tetrahedral CH₄
sp³d Trigonal bipyramidal PCl₅
sp³d² Octahedral SF₆
🔹 9. Molecular Orbital Theory (MOT)

Atomic orbitals combine to form molecular orbitals.

Types:

Bonding MO

Antibonding MO

Bond Order:

Bond Order = (Bonding e⁻ − Antibonding e⁻) / 2

📌 Higher bond order → stronger bond

🔹 10. Hydrogen Bonding

A weak bond between H attached to highly electronegative atoms (F, O, N).

Types:

Intermolecular (between molecules)

Intramolecular (within a molecule)

📌 Responsible for:

High boiling point of water

Structure of DNA

Protein stability

🔹 11. Polarity of Molecules

Depends on:

Electronegativity difference

Molecular geometry

📌 Example:

CO₂ → Non-polar

H₂O → Polar

🔹 12. Importance of Chemical Bonding

Explains shape & properties of molecules

Essential for biochemistry & materials science

Basis of reaction mechanisms

📌 EXAM FOCUS (NEET/JEE/BOARDS)

✔ VSEPR shapes
✔ Hybridization
✔ Bond order
✔ MOT energy diagrams
✔ Hydrogen bonding


Chemical Bonding Notes, Molecular Structure Class 11, VSEPR Theory, Hybridization Chart, Covalent Bonding, Ionic Bonding, Molecular Orbital Theory, Hydrogen Bonding, NEET Chemistry Notes, JEE Chemical Bonding

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