Given below are two statements:
Statement I: A hypothetical diatomic molecule with bond order zero is quite stable.
Statement II: As bond order increases, the bond length increases.
In the light of the above statements, choose the most appropriate answer from the options given below:

In Molecular Orbital Theory, a bond order of zero indicates that bonding electrons equal antibonding electrons, meaning no net attractive bonding exists and the molecule is completely unstable/does not exist (Statement I is false). As bond order increases, atoms are pulled closer by stronger shared electron density, so bond length decreases (Statement II is false). Hence, both statements are false.