The calculated spin-only magnetic moment of C | vedclass

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(C) The electronic configuration of $Cr$ is $[Ar] 3d^5 4s^1$.For $Cr^{2+}$ ion,two electrons are removed,resulting in the configuration $[Ar] 3d^4$.Th

Vedclass · Accepted Answer

$4.90$

Vedclass · Answer

(C) The electronic configuration of $Cr$ is $[Ar] 3d^5 4s^1$.For $Cr^{2+}$ ion,two electrons are removed,resulting in the configuration $[Ar] 3d^4$.This means there are $n = 4$ unpaired electrons.The spin-only magnetic moment is calculated using the formula $\mu = \sqrt{n(n+2)} \ B.M.$Substituting $n = 4$:$\mu = \sqrt{4(4+2)} \ B.M. = \sqrt{4 	imes 6} \ B.M. = \sqrt{24} \ B.M. \approx 4.90 \ B.M.$

The calculated spin-only magnetic moment of $Cr^{2+}$ ion is......$B.M.$

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