Consider the following values of IE (eV) for | vedclass

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(B) For element $W$,the jump in $IE$ occurs between $IE_3$ and $IE_4$ ($24.9 \ eV$ to $79.8 \ eV$),indicating that $W$ has $3$ valence electrons. Thus

Vedclass · Accepted Answer

$b, c$

Vedclass · Answer

(B) For element $W$,the jump in $IE$ occurs between $IE_3$ and $IE_4$ ($24.9 \ eV$ to $79.8 \ eV$),indicating that $W$ has $3$ valence electrons. Thus,$W$ exhibits a valency of $+3$.For element $X$,the jump in $IE$ occurs between $IE_2$ and $IE_3$ ($14.8 \ eV$ to $78.9 \ eV$),indicating that $X$ has $2$ valence electrons. Thus,$X$ exhibits a valency of $+2$.Element $Y$ has configuration $ns^2 np^4$,requiring $2$ electrons to complete its octet,so its valency is $-2$.Element $Z$ has configuration $ns^2 np^5$,requiring $1$ electron to complete its octet,so its valency is $-1$.Possible compounds:$W$ $(+3)$ and $Y$ $(-2)$ form $W_2Y_3$.$X$ $(+2)$ and $Y$ $(-2)$ form $XY$.$W$ $(+3)$ and $Z$ $(-1)$ form $WZ_3$.$X$ $(+2)$ and $Z$ $(-1)$ form $XZ_2$.Comparing with the given options: $(a) W_2Y_3$ is possible,$(b) X_2Y_3$ is not possible,$(c) WZ_2$ is not possible,$(d) XZ_2$ is possible.Therefore,the compounds that are not possible are $(b)$ and $(c)$.

Element	$IE_1$	$IE_2$	$IE_3$	$IE_4$
$W$	$10.5$	$15.5$	$24.9$	$79.8$
$X$	$8$	$14.8$	$78.9$	$105.8$

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