What is the hybridization of the central atom in ${\mathrm{CO}}_2$?

• A. ${\mathrm{sp}}^3$
• B. $\mathrm{sp}$
• C. ${\mathrm{sp}}^{3}d$
• D. ${\mathrm{sp}}^2$

Answer: (B)

Verified step by step guidance

1. Identify the central atom in the molecule CO\_2, which is carbon (C).
2. Determine the number of regions of electron density (bonding and lone pairs) around the central atom. In CO\_2, carbon forms two double bonds with oxygen atoms and has no lone pairs.
3. Recall that the hybridization corresponds to the number of electron regions: 2 regions correspond to sp, 3 to sp\^2, and 4 to sp\^3 hybridization.
4. Since carbon in CO\_2 has two regions of electron density (two double bonds), its hybridization is sp.
5. Confirm this by considering the molecular geometry: CO\_2 is linear, which is consistent with sp hybridization.