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(B) Step $1$: Determine the valency of element $A$. The configuration $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2$ shows $2$ electrons in the outermost shell. Thus

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$AB_2$

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(B) Step $1$: Determine the valency of element $A$. The configuration $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2$ shows $2$ electrons in the outermost shell. Thus, $A$ loses $2$ electrons to form $A^{2+}$ ion.Step $2$: Determine the valency of element $B$. The configuration $1s^2 2s^2 2p^6 3s^2 3p^5$ shows $7$ electrons in the outermost shell. Thus, $B$ gains $1$ electron to form $B^-$ ion.Step $3$: Determine the formula of the ionic compound. To balance the charges, one $A^{2+}$ ion reacts with two $B^-$ ions. The formula is $AB_2$.

The electronic configurations of elements are $A = 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2$ and $B = 1s^2 2s^2 2p^6 3s^2 3p^5$. Which of the following is the formula of the ionic compound that could be formed between these two elements $A$ and $B$?

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