Final answer:
Bond order affects both bond distance and bond dissociation enthalpy. As the bond order increases, the bond distance decreases, and the bond dissociation enthalpy increases.
Step-by-step explanation:
The bond order affects both bond distance and bond dissociation enthalpy. As the bond order increases, the bond distance decreases. This is because a higher bond order means more electron pairs between the atoms, resulting in a stronger attraction and a shorter distance between them. In terms of bond dissociation enthalpy, a higher bond order means a stronger bond, requiring more energy to break it, so the bond dissociation enthalpy also increases.