The electronic configurations of four element | vedclass

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(C) Element $A$ $(1s^2)$ is Helium,a noble gas,which is chemically inert.Element $B$ $(1s^2, 2s^2 2p^2)$ has $4$ valence electrons and typically forms

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$C: 1s^2, 2s^2 2p^5$

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(C) Element $A$ $(1s^2)$ is Helium,a noble gas,which is chemically inert.Element $B$ $(1s^2, 2s^2 2p^2)$ has $4$ valence electrons and typically forms covalent bonds.Element $C$ $(1s^2, 2s^2 2p^5)$ has $7$ valence electrons. It requires $1$ electron to complete its octet,readily forming an anion $(C^-)$,which facilitates the formation of an electrovalent (ionic) bond.Element $D$ $(1s^2, 2s^2 2p^6)$ is Neon,a noble gas,which is chemically inert.Therefore,element $C$ is the most likely to form an electrovalent bond.

The electronic configurations of four elements $A, B, C, D$ are given below. Which of these elements is most likely to form an electrovalent (ionic) bond?

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