Given below are two statements: Statement I: | vedclass

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(B) Statement $I$: $A$ molecule with a bond order of $0$ implies that the number of bonding electrons equals the number of antibonding electrons,makin

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Both Statement $I$ and Statement $II$ are false.

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(B) Statement $I$: $A$ molecule with a bond order of $0$ implies that the number of bonding electrons equals the number of antibonding electrons,making the molecule unstable or non-existent (e.g.,$He_2$,$Be_2$,$Ne_2$). Thus,Statement $I$ is false.Statement $II$: According to Molecular Orbital Theory,bond order is inversely proportional to bond length $(	ext{Bond order} \propto \frac{1}{	ext{Bond length}})$. Therefore,as bond order increases,bond length decreases. Thus,Statement $II$ is false.

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.

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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.