Question

this carbon atom has...
options: sp³ hybridization (yellow), sp² hybridization (blue), sp hybridization (orange)
molecular structure image (e.g., hco-related) shown

Explanation:

To determine the hybridization of the carbon atom in the given molecule (formaldehyde, \( \text{H}_2\text{CO} \)):

Step 1: Analyze the bonding of the carbon atom

In formaldehyde, the carbon atom is bonded to two hydrogen atoms and one oxygen atom via a double bond (C=O) and two single bonds (C-H). The carbon atom forms 3 sigma bonds (2 with H, 1 with O) and 1 pi bond (with O in the double bond).

Step 2: Determine the hybridization based on electron domains

The number of electron domains (regions of electron density) around the carbon atom is 3 (2 single bonds + 1 double bond; a double bond counts as one electron domain for hybridization). For 3 electron domains, the hybridization is \( \boldsymbol{sp^2} \) (since \( sp^2 \) hybridization corresponds to 3 hybrid orbitals, allowing trigonal planar geometry, which matches the bonding in formaldehyde).

Answer:

The carbon atom has \( \boldsymbol{sp^2} \) hybridization (corresponding to the "sp² hybridization" option).