The Foundations of Chemistry

C. Valence Bond Theory

Sulfur atoms can use one 3s, three 3p, and two 3dorbitals to form six hybrid orbitals that

accommodate six electron pairs:

Se and Te, in the same group, form
analogous compounds. O cannot do so,
for the same reasons as discussed
earlier for N (see Section 8-11).

336 CHAPTER 8: Molecular Structure and Covalent Bonding Theories

3 p

3 d^3 d

sp^3 d^2

3 s

S[Ne] hybridize S[Ne]

The six sp^3 d^2 hybrid orbitalsare directed toward the corners of a regular octahedron.

Each sp^3 d^2 hybrid orbital is overlapped by a half-filled 2porbital from fluorine, to form a

total of six covalent bonds.

An analogous picture could be drawn for the PF 6 
ion.

sp^3 d^2 Hybridization occurs at the central atom whenever there are six regions of

high electron density around the central atom. AB 6 molecules and ions with no lone

pairs on the central atom have octahedral electronic geometry, octahedral molec-

ular geometry, and sp^3 d^2 hybridization on the central atom.

S

F

F sp^3 d^2 hybrid orbitals on S

p orbitals on F

F

F

F

F