Question

the diagram above shows two resonance structures for a molecule of c₆h₆. the phenomenon shown in the diagram best supports which of the following claims about the bonding in c₆h₆?
a in the c₆h₆ molecule, all the bonds between the carbon atoms have the same length.
b because of variable bonding between its carbon atoms, c₆h₆ is a good conductor of electricity.
c the bonds between carbon atoms in c₆h₆ are unstable, and the compound decomposes quickly.
d the c₆h₆ molecule contains three single bonds between carbon atoms and three double bonds between carbon atoms.

Explanation:

Resonance structures imply that the actual bonding in a molecule is a hybrid of the resonance forms. In benzene (\(C_6H_6\)), resonance leads to all \(C - C\) bonds having the same length. This is because the electrons are delocalized, and each \(C - C\) bond has a bond order of \(1.5\) (a blend of single and double - bond character).

• Option B: Benzene (\(C_6H_6\)) is not a good conductor of electricity. It is a non - polar covalent compound with no free - moving charged particles (like ions or free electrons) to conduct electricity.
• Option C: Benzene is a stable compound. The delocalized \(\pi\) - electrons (due to resonance) give it aromatic stability. It does not decompose quickly under normal conditions.
• Option D: In the resonance hybrid of benzene, there are no distinct single and double bonds. All \(C - C\) bonds are equivalent.

Answer:

A. In the \(C_6H_6\) molecule, all the bonds between the carbon atoms have the same length.