Question

question 32 (1 point)
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which statement accurately reflects a π bond between two carbon atoms?

a) it can be described by the overlap of unhybridized p atomic orbitals from each
atom.

b) it can be described by the overlap of sp² hybrid orbitals from each atom.

c) the region of high electron density lies along the bond axis connecting the nuclei of
the two atoms.

d) it can be described by the overlap of sp hybrid orbitals from each atom.

e) it can be described by the overlap of a p atomic orbital from one atom with an sp²
hybrid orbital from the other atom.

Explanation:

• Option a: $\pi$ bonds are formed by the lateral overlap of unhybridized $p$ atomic orbitals. For example, in ethylene ($C_2H_4$) with $sp^{2}$ hybridization, the unhybridized $p$ orbitals overlap sideways to form the $\pi$ bond.
• Option b: $sp^{2}$ hybrid orbitals form $\sigma$ bonds (e.g., $C - C$ and $C - H$ $\sigma$ bonds in ethylene).
• Option c: The region of high electron density in a $\pi$ bond is above and below the bond - axis, while for a $\sigma$ bond, the region of high electron density lies along the bond axis.
• Option d: $sp$ hybrid orbitals form $\sigma$ bonds (e.g., in acetylene $C_2H_2$, the $C - C$ $\sigma$ bond is formed by $sp - sp$ overlap).
• Option e: A combination of a $p$ orbital and an $sp^{2}$ hybrid orbital does not form a $\pi$ bond. A $\pi$ bond requires the overlap of two $p$ orbitals (or equivalent in terms of symmetry for lateral overlap).

Answer:

A. It can be described by the overlap of unhybridized $p$ atomic orbitals from each atom.