Which of the following electronic configuration would be associated with the highest magnetic moment?

<p>The magnetic moment of an atom or ion with unpaired electrons is given by the formula $\mu = \sqrt{n(n+2)}$ Bohr magnetons (BM), where $n$ is the number of unpaired electrons. The magnetic moment depends on the number of unpaired electrons: more unpaired electrons lead to a higher magnetic moment.</p> <p>Looking at the given options with respect to their electron configurations and calculating their respective magnetic moments based on their unpaired electrons: </p><ul><li>$[\mathrm{Ar}] 3 \mathrm{~d}^7$ has 3 unpaired electrons, yielding a magnetic moment of $\sqrt{15}$ BM.</li><li>$[\mathrm{Ar}] 3 \mathrm{~d}^8$ has 2 unpaired electrons, for a magnetic moment of $\sqrt{8}$ BM.</li><li>$[\mathrm{Ar}] 3 \mathrm{~d}^3$ also has 3 unpaired electrons, similar to $3 \mathrm{~d}^7$, so its magnetic moment is likewise $\sqrt{15}$ BM.</li><li>Finally, $[\mathrm{Ar}] 3 \mathrm{~d}^6$ has 4 unpaired electrons, resulting in the highest magnetic moment among the options, $\sqrt{24}$ BM.</li></ul> <p>Hence, the electron configuration associated with the highest magnetic moment is $[\mathrm{Ar}] 3 \mathrm{~d}^6$.</p>