This page details the various types of hybridization and their corresponding molecular shapes. Each hybridization type results in specific molecular geometries and bond angles.

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.

The final page demonstrates practical applications through specific molecular examples, showing how to determine hybridization and predict molecular geometry.

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.

The first page introduces the concept of hybrydyzacja orbitali atomowych as a process of orbital mixing. The hybridization process creates new hybrid orbitals with different shapes, spatial distributions, and energies compared to the original atomic orbitals.

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.