The electronic configuration of three element | vedclass

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(B) Element $C$ has the electronic configuration $1s^2, 2s^2, 2p^6, 3s^2, 3p^5$,which corresponds to Chlorine $(Cl)$.Chlorine is a halogen with $7$ va

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$C_2$

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(B) Element $C$ has the electronic configuration $1s^2, 2s^2, 2p^6, 3s^2, 3p^5$,which corresponds to Chlorine $(Cl)$.Chlorine is a halogen with $7$ valence electrons and requires $1$ electron to complete its octet.Therefore,two Chlorine atoms share one electron each to form a stable diatomic molecule,$Cl_2$ (or $C_2$ in this context).The molecular orbital configuration for $C_2$ (if $C$ were Carbon) would be $KK [\sigma_{2s}]^2 [\sigma_{2s}^*]^2 [\pi_{2px}]^2 [\pi_{2py}]^2$,but here $C$ represents a halogen,so it forms a stable diatomic molecule $C_2$.

The electronic configuration of three elements $A$,$B$ and $C$ are given below. Stable form of $C$ may be represented by the formula
$A : 1s^2, 2s^2, 2p^6$
$B : 1s^2, 2s^2, 2p^6, 3s^2, 3p^3$
$C : 1s^2, 2s^2, 2p^6, 3s^2, 3p^5$

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The electronic configuration of three elements $A$,$B$ and $C$ are given below. Stable form of $C$ may be represented by the formula$A : 1s^2, 2s^2, 2p^6$$B : 1s^2, 2s^2, 2p^6, 3s^2, 3p^3$$C : 1s^2, 2s^2, 2p^6, 3s^2, 3p^5$