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(D) The electronic configuration of $X$ is $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2$. It has $2$ valence electrons in the $4s$ orbital,so it tends to lose $2$ e

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$XY_2$

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(D) The electronic configuration of $X$ is $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2$. It has $2$ valence electrons in the $4s$ orbital,so it tends to lose $2$ electrons to achieve a stable noble gas configuration,forming the $X^{2+}$ ion.The electronic configuration of $Y$ is $1s^2 2s^2 2p^6 3s^2 3p^5$. It has $7$ valence electrons,so it tends to gain $1$ electron to complete its octet,forming the $Y^{-}$ ion.To form a neutral compound,the charges must balance: $X^{2+} + 2Y^{-} \rightarrow XY_2$.Thus,$1$ atom of $X$ combines with $2$ atoms of $Y$ to form the compound $XY_2$.

Two elements $X$ and $Y$ have the following electron configurations:
$X = 1s^2, 2s^2 2p^6, 3s^2 3p^6, 4s^2$
$Y = 1s^2, 2s^2 2p^6, 3s^2 3p^5$
The compound formed by the combination of $X$ and $Y$ is:

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Two elements $X$ and $Y$ have the following electron configurations:$X = 1s^2, 2s^2 2p^6, 3s^2 3p^6, 4s^2$$Y = 1s^2, 2s^2 2p^6, 3s^2 3p^5$The compound formed by the combination of $X$ and $Y$ is: