Chemical Bonding

Flashcards covering key concepts in chemical bonding, including Lewis theory, quantum mechanics, and molecular orbital theory.

Lewis Theory

Works reasonably well for light atoms in main-group compounds, emphasizing the electron pair bond and octets.

Schrödinger Equation

A mathematical equation that describes the energy of a given state with potential and kinetic energy terms; useful for tackling chemical bonding.

Wavefunction

A solution to the Schrödinger equation that describes the behavior of an electron; squaring the wavefunction gives a probability distribution.

Atomic Orbitals

Characterized by quantum numbers including principal (n), angular momentum (l), magnetic (ml), and spin (ms). Phase is important.

Pauli Exclusion Principle

No two electrons can have the same four quantum numbers.

Molecular Orbital Theory

A delocalized view of chemical bonding.

Valence Bond Theory

A localized view of chemical bonding.

Molecular Orbitals

Solutions to the molecular problem, formed by combining atomic orbitals.

Symmetry

Molecular orbitals must have the same symmetry to combine.

Sigma (σ) symmetry

Symmetric with respect to rotation about the bond axis.

Pi (π) symmetry

Antisymmetric with respect to rotation about the bond axis.