An element X has electronic configuration, $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} .$ What would be the expected formula of X with chloride.

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${XCl}_{3}$

${XCl}_{2}$

$XCl$

$X_{2} Cl$

answer is B.

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Detailed Solution

According to the given electronic configuration, total number of electrons present in X is 12, and it corresponds to Mg. It's a metal, and its outermost orbit has two electrons. As it is a metal, it can donate its two electrons and obtain the closest noble gas structure.

Valence electronic configuration of Cl is 3s² 3p⁵. This depicts that Cl needs only one electron to complete its octet. As a result, one Mg combined with 2Cl and forms MgCl₂. As a result, element X with chloride has the formula XCl₂.

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