Definition: sp hybridization results in linear molecules with 180° bond angles.

Example: sp² hybridization creates trigonal planar molecules with 120° bond angles when there are no lone pairs.

Highlight: sp³ hybridization forms tetrahedral structures with ideal bond angles of 109.5°.

Vocabulary: Sigma bonds (σ) - direct head-on overlap between atomic orbitals.

Example: BH₃ molecule demonstrates sp² hybridization with a trigonal planar shape.

Highlight: NH₃ exhibits sp³ hybridization with a pyramidal shape due to the presence of a lone pair.

Definition: The total number of electron domains (bonding and non-bonding) determines the hybridization type.

Vocabulary: Lone pair - a pair of valence electrons not involved in bonding.

Definition: Hybridization is the process of mixing atomic orbitals to form an equal number of hybrid orbitals with different spatial arrangements.

Example: Beryllium in BeH₂ undergoes sp hybridization, where one s orbital and one p orbital combine to form two hybrid orbitals.

Highlight: Hybridization is only determined for the central atom in a covalent molecule.

Vocabulary: Orbital - a region in an atom where electrons are likely to be found.