According to Molecular Orbital Theory,

($A$) $\mathrm{C}_2^{2-}$ is expected to be diamagnetic

($B$) $\mathrm{O}_2{ }^{2+}$ is expected to have a longer bond length than $\mathrm{O}_2$

($C$) $\mathrm{N}_2^{+}$and $\mathrm{N}_2^{-}$have the same bond order

($D$) $\mathrm{He}_2^{+}$has the same energy as two isolated He atoms

Bond energies in $NO,\,N{O^ + }$ and $N{O^ - }$ are such as

Assertion : $B_2$ molecule is diamagnetic.
Reason : The highest occupied molecular orbital is of $\sigma $ type.

Which one of the following molecules is expected to exhibit diamagnetic behaviour ?

The correct order of the  $O-O$  bond length in  $O_2, H_2O_2$  and  $O_3$  is

For $F_2$ and $OF$ molecules consider the following statements 
$(a)$ Bond order for both is one
$(b)$ $OF$ is paramagnetic but $F_2$ is diamagnetic
$(c)$ $F_2$ is more likely to dissociate into atoms than $OF$
$(d)$ Both have greater number of electrons in $BMO$ than that in $ABMO$
Which of the following statements are true $(T)$ or false $(F)$ respectively