What is the total number of electrons present | vedclass

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(C) The atomic number of fluorine $(F)$ is $9$. Therefore, an $F_2$ molecule has $9 	imes 2 = 18$ electrons.The molecular orbital configuration for $

Vedclass · Accepted Answer

Bonding - $10$, Antibonding - $8$

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(C) The atomic number of fluorine $(F)$ is $9$. Therefore, an $F_2$ molecule has $9 	imes 2 = 18$ electrons.The molecular orbital configuration for $F_2$ is: $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2, \pi 2p_y^2, \pi^* 2p_x^2, \pi^* 2p_y^2$.Bonding electrons are those in orbitals without an asterisk $(*)$. Total bonding electrons = $2 (\sigma 1s) + 2 (\sigma 2s) + 2 (\sigma 2p_z) + 2 (\pi 2p_x) + 2 (\pi 2p_y) = 10$.Antibonding electrons are those in orbitals with an asterisk $(*)$. Total antibonding electrons = $2 (\sigma^* 1s) + 2 (\sigma^* 2s) + 2 (\pi^* 2p_x) + 2 (\pi^* 2p_y) = 8$.Thus, bonding electrons are $10$ and antibonding electrons are $8$.

What is the total number of electrons present in bonding and antibonding molecular orbitals respectively in an $F_2$ molecule according to molecular orbital $(MO)$ theory?

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