Question

Discuss the bond angle(s) in SF4. Explain the hybridization involved in the C2H4 molecule.

A) SF4 has a tetrahedral bond angle; C2H4 has sp3 hybridization.
B) SF4 has a trigonal bipyramidal bond angle; C2H4 has sp2 hybridization.
C) SF4 has a linear bond angle; C2H4 has sp hybridization.
D) Can't be determined

Answer 1

The bond angles in SF4 are not tetrahedral but seesaw-shaped, due to trigonal bipyramidal electronic geometry affected by one lone pair. C2H4 has carbon atoms that are sp2 hybridized, leading to a trigonal planar geometry with a bond angle of about 120°.

Step-by-step explanation:

The bond angles in SF4 relate to its molecular geometry, which differs from a perfect tetrahedral due to the presence of a lone pair of electrons. SF4 exhibits a trigonal bipyramidal arrangement, although with one position occupied by a lone pair, resulting in a seesaw structure. This means the bond angles are approximately 120° in the plane and 90° or 180° for axial positions. For the molecule C2H4 (ethylene), the central carbon atoms are sp2 hybridized, meaning each carbon forms three sp2 hybrid orbitals and one p orbital, which results in a trigonal planar shape around each carbon atom with bond angles of about 120°. This configuration allows for the formation of a sigma bond between the carbons and pi bonding above and below the plane of the molecules.