Chemistry Molecules: Valence Bond Theory

Flashcards covering key concepts of hybridization and molecular shapes in valence bond theory.

Hybridization

The mixing of atomic orbitals to form new hybrid orbitals.

sp Hybridization

Involves 2 sigma bonds and 0 non-bonding pairs, creating a linear molecular shape with bond angles of 180°, e.g., BeH2.

sp2 Hybridization

Involves 3 sigma bonds and 0 non-bonding pairs, leading to a trigonal planar molecular shape with bond angles of 120°, e.g., SO3.

sp3 Hybridization

Involves 4 sigma bonds, resulting in a tetrahedral molecular shape and bond angles of 109.5°, e.g., CH4.

Trigonal pyramidal

A molecular shape resulting from sp3 hybridization with 3 sigma bonds and 1 non-bonding pair, having bond angles of <109.5°, e.g., NH3.

Angular shape

Also known as bent shape, resulting from sp2 or sp3 hybridization with non-bonding pairs, e.g., H2O.

Trigonal bipyramidal

A molecular structure with 5 sigma bonds arranged with bond angles of 120° and 90°, e.g., PF5.

Seesaw shape

A molecular shape in sp3d hybridization with 4 sigma bonds and 1 non-bonding pair, with bond angles of <120° and <90°, e.g., SF4.

T-shaped

A molecular configuration with 3 sigma bonds and 2 non-bonding pairs from sp3d hybridization, having bond angles of <90°, e.g., ClF3.

Octahedral

A molecular shape with 6 sigma bonds and bond angles of 90°, e.g., SF6.