Question

what is the hybridization of the central atom in the sulfur hexabromide (sbr6) molecule?

Explanation:

Step1: Determine the number of electron - groups around the central atom

In $SBr_6$, sulfur (S) is the central atom. Sulfur has 6 valence electrons and forms 6 single bonds with bromine (Br) atoms. The number of electron - groups (bonding pairs + lone pairs) around the central sulfur atom is 6 (since there are 6 S - Br bonds and 0 lone pairs on S).

Step2: Use the electron - group number to determine hybridization

The relationship between the number of electron - groups (n) and hybridization is as follows:

• If n = 2, hybridization is $sp$.
• If n = 3, hybridization is $sp^2$.
• If n = 4, hybridization is $sp^3$.
• If n = 5, hybridization is $sp^3d$.
• If n = 6, hybridization is $sp^3d^2$.

Since the number of electron - groups around S in $SBr_6$ is 6, the hybridization of the central sulfur atom is $sp^3d^2$.

Answer:

$sp^3d^2$