In which of the following pairs,both the elem | vedclass

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(D) The general electronic configuration for the elements in the given groups is $(n-1)d^{10} ns^2$.$Zn$ $([Ar] 3d^{10} 4s^2)$,$Cd$ $([Kr] 4d^{10} 5s^

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$Ag, Cu$

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(D) The general electronic configuration for the elements in the given groups is $(n-1)d^{10} ns^2$.$Zn$ $([Ar] 3d^{10} 4s^2)$,$Cd$ $([Kr] 4d^{10} 5s^2)$,and $Hg$ $([Xe] 4f^{14} 5d^{10} 6s^2)$ follow this configuration.$Cu$ has the configuration $[Ar] 3d^{10} 4s^1$.$Ag$ has the configuration $[Kr] 4d^{10} 5s^1$.In the pair $Cu, Zn$,$Cu$ does not have the $(n-1)d^{10} ns^2$ configuration.In the pair $Ag, Cu$,neither element has the $(n-1)d^{10} ns^2$ configuration.However,the question asks for the pair where both elements do not have this configuration. Since $Ag$ and $Cu$ both have $ns^1$ instead of $ns^2$,this is the correct pair.

column-$I$ $(\text{Property})$	column-$II$ $(\text{Metal})$
$i$. An element which can show $+8$ oxidation state	$a$. $Mn$
$ii$. $3d$ series element that can show upto $+7$ oxidation state	$b$. $Cr$
$iii$. $3d$ series element with highest melting point	$c$. $Os$

In which of the following pairs,both the elements do not have $(n-1)d^{10} ns^2$ configuration?

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