Which of the following statements about hybrid orbitals is or are true? (i) After an atom undergoes sp hybridization, there is one unhybridized p orbital on the atom, (ii) Under sp2 hybridization, the large lobes point to the vertices of an equilateral triangle, and (iii) The angle between the large lobes of sp3 hybrids is 109.5°.

Key Concepts

Hybridization

Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. These hybrid orbitals have different shapes and energies than the original atomic orbitals, allowing for the formation of covalent bonds in molecules. The type of hybridization (sp, sp2, sp3) depends on the number of atomic orbitals mixed and the geometry of the resulting molecular structure.

Geometry of Hybrid Orbitals

The geometry of hybrid orbitals is determined by the arrangement of the hybrid orbitals around the central atom. For example, sp hybridization results in a linear geometry with a bond angle of 180°, sp2 hybridization leads to a trigonal planar arrangement with 120° bond angles, and sp3 hybridization results in a tetrahedral geometry with bond angles of approximately 109.5°. Understanding these geometries is crucial for predicting molecular shapes and bond angles.

Unhybridized Orbitals

Unhybridized orbitals are atomic orbitals that remain unchanged during the hybridization process. For instance, in sp hybridization, one p orbital remains unhybridized, while in sp2 hybridization, one p orbital is also unhybridized. These unhybridized orbitals can participate in π bonding, which is essential for the formation of double and triple bonds in molecules, influencing their reactivity and properties.