Chemical Bonding II: Advanced Concepts

Flashcards covering advanced concepts in chemical bonding, including VSEPR theory, molecular geometries, and types of chemical bonds.

VSEPR Theory

Valence Shell Electron Pair Repulsion theory predicts the shape of a molecule based on the repulsion between electron pairs.

Sigma Bond

A covalent bond formed by the direct overlap of atomic orbitals along the internuclear axis.

Pi Bond

A covalent bond formed by the side-by-side overlap of p orbitals.

Electrostatic Repulsion

The repulsive force between charged particles, which influences the geometry of molecules according to VSEPR theory.

Hybridization

The mixing of atomic orbitals to form new hybrid orbitals that determine molecular geometry.

Diatomic Molecules

Molecules composed of two atoms, which can be of the same or different elements.

Bond Order

A measure of the number of chemical bonds between a pair of atoms, calculated as the difference between the number of bonding and antibonding electrons.

Lewis Structure

A diagram that represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist.

Molecular Orbital Theory

A theory that describes the electronic structure of molecules using quantum mechanics, which involves the combination of atomic orbitals to form molecular orbitals.

Covalent Bond

A chemical bond formed by the sharing of one or more pairs of electrons between atoms.

Valence Bond Theory

A theory that describes the electron pairs that are shared between atoms through the overlap of atomic orbitals.

Dipole Moment

A measure of the separation of positive and negative charge in a system, which determines the polarity of a molecule.

Intermolecular Forces

Forces of attraction or repulsion which act between neighboring particles (molecules, atoms, or ions).

Hydrogen Bonding

A strong type of dipole-dipole attraction that occurs when hydrogen is bonded to electronegative atoms like nitrogen, oxygen, or fluorine.

Lone Pair

A pair of valence electrons that are not shared with another atom.

Electronegativity

A measure of the tendency of an atom to attract a bonding pair of electrons.

London Dispersion Forces

Weak intermolecular forces arising from temporary dipoles in atoms or molecules.

Dipole-Dipole Interaction

An attractive force between the positive end of one polar molecule and the negative end of another polar molecule.

Ion-Dipole Interaction

The attractive force between an ion and a polar molecule.

Surface Tension

The cohesive force at the surface of a liquid that makes it behave like a stretched elastic membrane.