Question

evaluate understanding what did i learn? bond length and energy comparing the length of carbon - carbon covalent bonds c - c c = c c ≡ c 147 pm 134 pm 120 pm 347 kj/mol⁻¹ 614 kj/mol⁻¹ 839 kj/mol⁻¹ as the bond order increases between two atoms (e.g., from a single bond to a double or triple bond), the bond length typically: a) increases b) decreases c) remains the same d) becomes unpredictable

Explanation:

Bond order refers to the number of chemical bonds between two atoms. A single bond (\(C - C\)) has a bond order of \(1\), a double bond (\(C = C\)) has a bond order of \(2\), and a triple bond (\(C\equiv C\)) has a bond order of \(3\). As shown in the image, the bond length for \(C - C\) is \(147\ pm\), for \(C = C\) is \(134\ pm\), and for \(C\equiv C\) is \(120\ pm\). As the bond order increases from \(1\) (single bond) to \(2\) (double bond) to \(3\) (triple bond), the bond length decreases. This is because a higher - order bond has more electron density between the two atoms, pulling the atoms closer together.

Answer:

B. Decreases