The electronic configuration of a metal M is | vedclass

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(B) The electronic configuration of metal $M$ is $1s^2 \, 2s^2 \, 2p^6 \, 3s^1$. This indicates that the metal $M$ has $1$ valence electron in its out

Vedclass · Accepted Answer

$M_2O$

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(B) The electronic configuration of metal $M$ is $1s^2 \, 2s^2 \, 2p^6 \, 3s^1$. This indicates that the metal $M$ has $1$ valence electron in its outermost shell $(3s^1)$. Therefore,the valency of metal $M$ is $+1$. Oxygen $(O)$ has an electronic configuration of $1s^2 \, 2s^2 \, 2p^4$,meaning it needs $2$ electrons to complete its octet,so its valency is $-2$. By the criss-cross method,the formula of the oxide is formed by combining $M^+$ and $O^{2-}$,which results in $M_2O$.

The electronic configuration of a metal $M$ is $1s^2 \, 2s^2 \, 2p^6 \, 3s^1$. What will be the formula of its oxide?

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