General Chemistry: Periodic Table and Bonding Theory

These flashcards cover key vocabulary and concepts from general chemistry focused on the periodic table and bonding theories.

Valence Bond Theory

A theory that explains the formation of covalent bonds through the overlap of atomic orbitals.

Hybridization

The mixing of atomic orbitals to generate new sets of equivalent orbitals for covalent bonding.

σ Bond

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

π Bond

A bond formed by the side-to-side overlap of atomic orbitals, existing above and below the bonding axis.

Bond Order

The number of bonds that exist between two atoms, calculated as the difference in the number of electrons in bonding and antibonding orbitals.

Molecular Orbital Theory

A theory that describes the formation of molecular orbitals from the wave functions of atomic orbitals.

Paramagnetism

The property of a substance that has unpaired electrons, causing it to be attracted to magnetic fields.

Diamagnetism

The property of a substance that has all paired electrons, causing it to be repelled by magnetic fields.

Hybrid Orbital

An orbital that results from the combination of atomic orbitals and is used for bonding.

Multiple Bonding

The presence of more than one bond between two atoms, involving multiple atomic orbital overlaps.

Molecular Geometry

The three-dimensional arrangement of atoms in a molecule, which can be predicted using the VSEPR model.

Hybridization Types

The classification of hybrid orbitals based on the number of atomic orbitals mixed, such as sp, sp2, sp3.

Electrons in Bonding Orbitals

Electrons that contribute to the bond between two atoms, resulting in bond formation.