Part 2: Chemical Bonding
Lectures 9–14
Chemical bonding determines the structure, properties, and reactivity of all materials. This part covers the full hierarchy of bonding models — from simple Lewis structures through VSEPR geometry prediction to molecular orbital theory — and then examines the intermolecular forces that govern phases of matter.
Part Overview
Why do atoms bond? How can we predict molecular geometry? What determines whether a material is a gas, liquid, or solid at room temperature? This part answers these questions by developing increasingly sophisticated bonding models. We begin with Lewis dot structures and formal charge, progress to VSEPR theory for predicting 3D molecular shapes, and then develop molecular orbital theory for a quantum mechanical description of bonding. Finally, we examine the intermolecular forces that determine bulk material properties.
Key Topics
- • Lewis dot structures and formal charge
- • Octet rule and its exceptions
- • VSEPR theory and molecular geometry
- • Bond order, bond energy, and bond length
- • Electronegativity and bond polarity
- • LCAO-MO theory: bonding and antibonding orbitals
- • MO diagrams for homonuclear diatomics
- • Hybridization: sp, sp², sp³
- • Intermolecular forces: London, dipole-dipole, hydrogen bonding
- • Phase transitions and the Clausius-Clapeyron equation
2 topic pages | 6 lectures | Interactive simulations
Key Equations
Formal Charge
$$FC = V - L - \frac{B}{2}$$
Bond Order (MO Theory)
$$BO = \frac{n_b - n_a}{2}$$
Dipole Moment
$$\mu = q \cdot d$$
Clausius-Clapeyron
$$\ln\frac{P_2}{P_1} = -\frac{\Delta H_{vap}}{R}\left(\frac{1}{T_2} - \frac{1}{T_1}\right)$$
Topics
Chemical Bonding & Lewis Structures
Lewis dot structures, formal charge, octet rule and exceptions, VSEPR theory, bond properties, and electronegativity. Covers Lectures 9–11.
Molecular Orbital Theory & Intermolecular Forces
LCAO-MO theory, MO diagrams, hybridization, intermolecular forces, and phase transitions with the Clausius-Clapeyron equation. Covers Lectures 12–14.