Identify all the species that do not exist: H | vedclass

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(B) According to Molecular Orbital Theory,a species does not exist if its Bond Order $(B.O.)$ is $0$.$B.O. = \frac{1}{2} (N_b - N_a)$,where $N_b$ is t

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$Li_2^{2-}, Ne_2, He_2$ only

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(B) According to Molecular Orbital Theory,a species does not exist if its Bond Order $(B.O.)$ is $0$.$B.O. = \frac{1}{2} (N_b - N_a)$,where $N_b$ is the number of bonding electrons and $N_a$ is the number of antibonding electrons.$1$. $H_2^{+} (1e^-): \sigma 1s^1, B.O. = 0.5$ (Exists)$2$. $He_2^{2+} (2e^-): \sigma 1s^2, B.O. = 1$ (Exists)$3$. $Li_2^{2-} (8e^-): \sigma 1s^2 \sigma^* 1s^2 \sigma 2s^2 \sigma^* 2s^2, B.O. = \frac{1}{2}(4-4) = 0$ (Does not exist)$4$. $Ne_2 (20e^-): \sigma 1s^2 \sigma^* 1s^2 \sigma 2s^2 \sigma^* 2s^2 \sigma 2pz^2 \pi 2px^2 \pi 2py^2 \pi^* 2px^2 \pi^* 2py^2 \sigma^* 2pz^2, B.O. = \frac{1}{2}(10-10) = 0$ (Does not exist)$5$. $Be_2^{-} (9e^-): \sigma 1s^2 \sigma^* 1s^2 \sigma 2s^2 \sigma^* 2s^2 \sigma 2pz^1, B.O. = 0.5$ (Exists)$6$. $He_2 (4e^-): \sigma 1s^2 \sigma^* 1s^2, B.O. = \frac{1}{2}(2-2) = 0$ (Does not exist)Thus,$Li_2^{2-}, Ne_2,$ and $He_2$ do not exist.

Column $I$	Column $II$
$(A)$ $B_2$	$(p)$ Paramagnetic
$(B)$ $N_2$	$(q)$ Undergoes oxidation
$(C)$ $O_2^{-}$	$(r)$ Undergoes reduction
$(D)$ $O_2$	$(s)$ Bond order $\geq 2$
	$(t)$ Mixing of '$s$' and '$p$' orbitals

Identify all the species that do not exist: $H_2^{+}, He_2^{2+}, Li_2^{2-}, Ne_2, Be_2^{-}, He_2$.

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