Given the molecule ${\mathrm{CH}}_2={\mathrm{CH}}_2$ (ethene), what is the hybridization of each carbon atom?

• A. Both carbons are unhybridized
• B. $\mathrm{sp}$
• C. ${\mathrm{sp}}^3$
• D. ${\mathrm{sp}}^2$

Answer: (D)

Verified step by step guidance

1. Identify the bonding environment of each carbon atom in ethene (CH\_2=CH\_2). Each carbon forms three sigma bonds: two with hydrogen atoms and one with the other carbon atom.
2. Recall that the hybridization state depends on the number of sigma bonds and lone pairs around the atom. For carbon atoms with three sigma bonds and no lone pairs, the hybridization is typically sp\^2.
3. Recognize that the double bond between the two carbons consists of one sigma bond and one pi bond. The sigma bond is formed by the overlap of sp\^2 hybrid orbitals, while the pi bond is formed by the side-to-side overlap of unhybridized p orbitals.
4. Conclude that each carbon in ethene is sp\^2 hybridized because it forms three sigma bonds and has one unhybridized p orbital involved in the pi bond.
5. Summarize that the correct hybridization for each carbon atom in ethene is sp\^2, which explains the planar structure and bond angles of approximately 120 degrees around each carbon.