Molecular Geometry and Bonding Theories
by Wilson Mwonga
1. ---
2. Types of Chemical Bonds**
3. - **Ionic Bonds**
3.1. - Transfer of electrons
3.2. - Forms between metals and non-metals
3.3. - Examples: NaCl, MgO
4. - **Covalent Bonds**
4.1. - Sharing of electrons
4.2. - Can be polar or nonpolar
4.3. - Examples: H₂O (polar), CH₄ (nonpolar)
5. - **Metallic Bonds**
5.1. - Sea of electrons
5.2. - Explains properties like conductivity and malleability
6. : Lewis Symbols and Octet Rule**
7. - **Octet Rule**
7.1. - Atoms strive to complete 8 valence electrons
7.2. - Exceptions:
7.2.1. - Incomplete octets (e.g., Be, B compounds)
7.2.2. - Expanded octets (e.g., PCl₅, SF₆)
8. - **Lewis Symbols**
8.1. - Representation of valence electrons around atoms
9. : Bond Polarity and Electronegativity**
10. - **Electronegativity**
10.1. - Measure of an atom’s ability to attract shared electrons
10.2. - Trends: Increases across a period, decreases down a group
11. - **Bond Polarity**
11.1. - Determined by electronegativity difference
11.1.1. - Polar bonds (e.g., H-Cl)
11.1.2. - Nonpolar bonds (e.g., Cl-Cl)
12. Lewis Structures and Resonance Structures**
13. - **Drawing Lewis Structures**
13.1. - Show bonding and lone pairs
13.2. - Follow the octet rule (with exceptions)
14. - **Resonance Structures**
14.1. - Molecules with delocalized electrons
14.2. - Example: O₃ (ozone)
15. : Molecular Shapes and VSEPR Model**
16. - **VSEPR Model**
16.1. - Valence Shell Electron Pair Repulsion Theory
16.2. - Predicts 3D molecular geometry based on electron pair repulsion
16.3. - Examples:
16.3.1. - Linear: CO₂
16.3.2. - Bent: H₂O
16.3.3. - Tetrahedral: CH₄