$X$ $ = 1{s^2},\,\,2{s^2}2{p^6},\,\,3{s^2}3{p^6},\,\,4{s^2}$
and $Y$ $ = 1{s^2},\,\,2{s^2}2{p^6},\,\,3{s^2}3{p^5}$
The compound formed by combination of $X$ and $Y$ is
$X =1 s ^2\, 2 s ^2\, 2 p ^6\, 3 s ^2 \,3 p ^6\, 4 s ^2$ has $2$ electrons more than stable configuration. So this can be written as $X ^{2+}$
after removing $2$ eletrcons.
Electronic configuration of $Y$ is:
$Y=1 s^2\, 2 s^2\, 2 p^6\, 3 s^2 \,3 p^5$ has $1$ electron less than stable configuration. So this can be written as $Y ^{-}$
after gaining $1$ electron
$X ^{2+}+2 Y ^{-}= XY _2$
$2$ ions of element $Y$ combine with $1$ ion $X$ to give $XY _2$.
The resulting molecule will be stable and will have no net charge.
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