Which of the following is not paramagnetic?

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(C) To determine if a species is paramagnetic,we check for the presence of unpaired electrons.$1$. $Be^-$ ($4 + 1 = 5$ electrons): $1s^2 2s^2 2p^1$ (U

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$Cl^-$

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(C) To determine if a species is paramagnetic,we check for the presence of unpaired electrons.$1$. $Be^-$ ($4 + 1 = 5$ electrons): $1s^2 2s^2 2p^1$ (Unpaired electron present,paramagnetic).$2$. $Ne^{2+}$ ($10 - 2 = 8$ electrons): $1s^2 2s^2 2p^4$ (Unpaired electrons present,paramagnetic).$3$. $Cl^-$ ($17 + 1 = 18$ electrons): $1s^2 2s^2 2p^6 3s^2 3p^6$ (All electrons are paired,diamagnetic).$4$. $As^+$ ($33 - 1 = 32$ electrons): The electronic configuration ends in $4p^2$,which has unpaired electrons (paramagnetic).Therefore,$Cl^-$ is not paramagnetic.

Column-$I$	Column-$II$
$A$. The orbital which has two angular nodes	$P$. $4d_{x^2-y^2}$
$B$. The $d$ orbital with zero nodal plane	$Q$. $3d_{z^2}$
$C$. The orbital with two radial nodes	$R$. $4f$
$D$. The orbital with three angular nodes	$S$. $3s$

Similar Questions

Which of the following is not a permissible arrangement of electrons in an atom?

In $Sr$ $(Z=38)$, the number of electrons with $l=0$ is $x$, and the number of electrons with $l=2$ is $y$. The value of $(x-y)$ is equal to:
($l=$ Azimuthal quantum number)

Match the column:

Column-$I$ Column-$II$

$A$. The orbital which has two angular nodes $P$. $4d_{x^2-y^2}$

$B$. The $d$ orbital with zero nodal plane $Q$. $3d_{z^2}$

$C$. The orbital with two radial nodes $R$. $4f$

$D$. The orbital with three angular nodes $S$. $3s$

Correct match will be $:-$

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