Atoms that are ${\mathrm{sp}}^2$ hybridized form how many $\pi$ bonds?

• A. $3$
• B. $2$
• C. $1$
• D. $0$

Answer: (C)

Verified step by step guidance

1. Recall that an sp\textsuperscript{2} hybridized atom has three sp\textsuperscript{2} hybrid orbitals and one unhybridized p orbital.
2. The three sp\textsuperscript{2} hybrid orbitals form sigma (\sigma) bonds or hold lone pairs, depending on the atom's bonding environment.
3. The remaining unhybridized p orbital is oriented perpendicular to the plane of the sp\textsuperscript{2} orbitals and can overlap with another p orbital to form a pi (\pi) bond.
4. Therefore, an sp\textsuperscript{2} hybridized atom can form exactly one \pi bond due to the single unhybridized p orbital available for pi bonding.
5. Summarizing, the number of \pi bonds formed by an sp\textsuperscript{2} hybridized atom is 1.