Question

identify the hybrid orbitals used by the inner atom of molecule whose lewis structure is below; enter superscripts in parentheses, e.g. enter sp³ as sp(3).

Explanation:

Step1: Determine the steric number

The steric number is calculated as the sum of the number of bonding pairs and lone pairs around the central atom. For the carbon atom in \(COCl_2\), it has 3 bonding pairs (one \(C = O\) double - bond and two \(C - Cl\) single - bonds, and double - bonds count as one region of electron density). The formula for steric number \(SN=\text{number of bonding regions}+\text{number of lone pairs}\). Here, \(SN = 3+0=3\).

Step2: Relate steric number to hybridization

If the steric number \(SN = 3\), the hybridization is \(sp^{2}\). According to the rule: \(SN = 2\) implies \(sp\) hybridization, \(SN=3\) implies \(sp^{2}\) hybridization, \(SN = 4\) implies \(sp^{3}\) hybridization, \(SN=5\) implies \(sp^{3}d\) hybridization and \(SN = 6\) implies \(sp^{3}d^{2}\) hybridization.

Answer:

\(sp(2)\)