Valence Bond Theory and Hybridization Overview

Valence bond theory

Describes how molecules form bonds and the types of bonding in molecules.

Valence electrons

Electrons in the outermost shell of an atom involved in bonding.

Formal charge

Describes the difference in electrons around an atom in a given structure.

Polar molecule

Molecule with positive and negative charges on different sides.

Functional groups

Groups of atoms attached to a molecule determining its properties.

Atomic orbitals

Describe the probability of finding an electron around an atom.

Molecular orbitals

Formed by the combination of atomic orbitals, can be bonding or antibonding.

Bonding molecular orbitals

Formed by constructive combination of atomic orbitals, lower energy.

Antibonding molecular orbitals

Formed by destructive combination of atomic orbitals, higher energy.

Energy diagrams

Show the relationship between atomic and molecular orbitals.

Electron configuration

Describes the arrangement of electrons in an atom.

Carbene

Unstable structure of methane with 2 bonds to hydrogen and a lone pair on carbon.

Hybridization

The mixing of atomic orbitals to form new hybrid orbitals.

Atomic Orbitals

Probability functions describing electron distribution within an atom

sp³ Hybrid Orbitals

Result from combining s and p orbitals in carbon, with energy closer to p orbitals

Sigma Bonds

Form between hybrid orbitals or hybrid orbitals and hydrogen atoms, requiring s characteristic

Pi Bonds

Form between unhybridized p orbitals, with a dumbbell-shaped overlap

Ethylene

Molecule where carbon atoms form a double bond with one sigma and one pi bond

Constructive Interference

Orbitals overlapping in phase to form a bonding molecular orbital

Destructive Interference

Orbitals overlapping out of phase to form an antibonding molecular orbital

Triple Bonds

Consist of one sigma bond and two pi bonds, with pi bonds from unhybridized p orbitals

Rotation Around Single Bonds

Can rotate freely

Rotation Around Double Bonds

Cannot rotate freely due to disruptive pi bond overlap