Valence bond theory and hydrogen

Covalent Bonds

Formed by sharing electrons between atoms to achieve a stable octet, works for simple molecules like methane.

Molecular Orbitals (MOs)

Result from the combination of atomic orbitals (AOs) in molecules, with different shapes and energies than AOs.

Linear Combination of Atomic Orbitals (LCAO)

Approach to combine atomic orbitals in a linear way to find solutions for molecular orbitals.

Bonding and Anti-bonding Orbitals

Result from constructive and destructive interference of combined atomic orbitals, affecting bond strength and stability.

Bond Order

Calculated as 1/2 (Number of Electrons in Bonding Orbitals - Number of Electrons in Anti-bonding Orbitals), predicts bond strength.

Orbital Overlap

Stronger bonding occurs with better spatial and energy overlap between orbitals, influencing bond strength.

Nuclear-Nuclear Repulsion

Repulsive interaction between atomic nuclei in a diatomic molecule, affects bond length and geometry.

Rules of LCAO

Guidelines for combining atomic orbitals to form molecular orbitals, including conservation of orbitals and energy considerations.