Video Transcript
A 𝜎 bond is created when specific
combinations of atomic orbitals overlap. Which of the following occurrences
does not result in the formation of a 𝜎 bond? (A) A hybrid sp orbital overlapping
with another hybrid sp orbital, (B) an s orbital overlapping with a p orbital, (C) a
p orbital overlapping with another p orbital side-by-side, (D) an s orbital
overlapping with another s orbital, (E) a p orbital overlapping with another p
orbital end-to-end.
Sigma bonds, often noted with the
lowercase Greek letter, are formed by the end-to-end overlap of orbitals. It doesn’t matter which two
orbitals are overlapping as long as they overlap end-to-end. Two s orbitals overlapping can
create a 𝜎 bond or an s orbital can overlap with a p orbital. A 𝜎 bond results from the s
orbital overlapping any of the hybrid orbitals. 𝜎 bonds also result from p
orbitals overlapping end-to-end or a p orbital overlapping with any of the hybrid
orbitals. Any of the hybrid orbitals can also
overlap with each other end-to-end.
Any combination of two orbitals
that overlap end-to-end such as these will result in a 𝜎 bond. But if we have two orbitals
overlapping side-by-side, like these two p orbitals, the resulting bond is a 𝜋
bond, not a 𝜎 bond. So answer choice (C), a p orbital
overlapping with another p orbital side-by-side, would result in the formation of a
𝜋 bond not a 𝜎 bond. So it’s the correct answer.
