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(B) The spin-only magnetic moment $(\mu_{spin})$ is calculated using the formula $\mu_{spin} = \sqrt{n(n+2)} 	ext{ BM}$,where $n$ is the number of un

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$3d^5$

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(B) The spin-only magnetic moment $(\mu_{spin})$ is calculated using the formula $\mu_{spin} = \sqrt{n(n+2)} 	ext{ BM}$,where $n$ is the number of unpaired electrons.
| Electronic Configuration | No. of Unpaired Electrons $(n)$ | Magnetic Moment $(\mu_{spin})$ |
| $3d^7$ | $3$ | $\sqrt{3(3+2)} = \sqrt{15} 	ext{ BM}$ |
| $3d^5$ | $5$ | $\sqrt{5(5+2)} = \sqrt{35} 	ext{ BM}$ |
| $3d^8$ | $2$ | $\sqrt{2(2+2)} = \sqrt{8} = 2\sqrt{2} 	ext{ BM}$ |
| $3d^2$ | $2$ | $\sqrt{2(2+2)} = \sqrt{8} = 2\sqrt{2} 	ext{ BM}$ |
Comparing the values,the $3d^5$ configuration has the highest number of unpaired electrons $(n=5)$,resulting in the highest magnetic moment of $\sqrt{35} 	ext{ BM}$.

$I. \ Zn^{2+}$	$(i) \ d^8 \ \text{configuration}$
$II. \ Cu^{2+}$	$(ii) \ \text{Colourless}$
$III. \ Ni^{2+}$	$(iii) \ \mu = 1.73 \ \text{BM}$

The magnetic nature of elements depends on the presence of unpaired electrons. Identify the configuration of transition elements which shows the highest magnetic moment.

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Match the following:
$I. \ Zn^{2+}$ $(i) \ d^8 \ \text{configuration}$
$II. \ Cu^{2+}$ $(ii) \ \text{Colourless}$
$III. \ Ni^{2+}$ $(iii) \ \mu = 1.73 \ \text{BM}$

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