Question

which of the following arranges the bonds in order of decreasing bond length? choose 1 answer: a c≡o > c=s > c=o b c=o > c=s > c≡o c c=s > c=o > c≡o d c≡o > c=o > c=s

Explanation:

Step1: Recall bond - length rule

Bond length is inversely related to bond order. A triple - bond has a higher bond order than a double - bond, so a triple - bond is shorter. Also, for the same bond order, the bond length increases with the size of the atoms involved.

Step2: Analyze bond orders

The $C\equiv O$ is a triple - bond, and $C = O$ and $C = S$ are double - bonds. The triple - bond $C\equiv O$ is the shortest among them.

Step3: Compare double - bonds

Among $C = O$ and $C = S$, sulfur is larger than oxygen. Since the size of the atom affects the bond length (larger atom leads to longer bond for the same bond order), the $C = S$ bond is longer than the $C = O$ bond.

Answer:

C. $C = S>C = O>C\equiv O$