Is the neon molecule Ne_2 possible? Why? | vedclass

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(B) The electronic configuration of $Ne$ $(Z=10)$ is $1s^2 2s^2 2p^6$. For $Ne_2$ molecule,the total number of electrons is $20$. The molecular orbita

Vedclass · Accepted Answer

No,it is unstable due to zero bond order.

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(B) The electronic configuration of $Ne$ $(Z=10)$ is $1s^2 2s^2 2p^6$. For $Ne_2$ molecule,the total number of electrons is $20$. The molecular orbital configuration is $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^2 = \pi^* 2p_y^2, \sigma^* 2p_z^2$. Bond order = $\frac{1}{2} (N_b - N_a) = \frac{1}{2} (10 - 10) = 0$. Since the bond order is $0$,the $Ne_2$ molecule is unstable and does not exist.

List-$I$ (Molecule)	List-$II$ (Number and types of bond/s between two carbon atoms)
$A.$ Ethane	$I.$ One $\sigma$-bond and two $\pi$-bonds
$B.$ Ethene	$II.$ Two $\pi$-bonds
$C.$ Carbon molecule,$C_2$	$III.$ One $\sigma$-bond
$D.$ Ethyne	$IV.$ One $\sigma$-bond and one $\pi$-bond

Is the neon molecule $Ne_2$ possible? Why?

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