Which of the following molecules does not exi | vedclass

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(C) According to Molecular Orbital Theory,the bond order is calculated as: $Bond \ Order = \frac{1}{2} (N_b - N_a)$,where $N_b$ is the number of elect

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$He_2$

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(C) According to Molecular Orbital Theory,the bond order is calculated as: $Bond \ Order = \frac{1}{2} (N_b - N_a)$,where $N_b$ is the number of electrons in bonding orbitals and $N_a$ is the number of electrons in antibonding orbitals.For $He_2$,the electronic configuration is $\sigma 1s^2, \sigma^* 1s^2$.Bond order = $\frac{1}{2} (2 - 2) = 0$.Since the bond order is $0$,the molecule $He_2$ does not exist.

Which of the following molecules does not exist on the basis of Molecular Orbital Theory?

Similar Questions

Calculate the bond order for $NO, NO^+, CN, CN^-$ and $CO$.

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.

Which of the following pairs of species have the same bond order?

In dinitrogen tetroxide $(N_2O_4)$,there:

How many molecular orbitals filled with one or more electrons are present in $N_2^+$?

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