Practicing Success
A divalent ion of 'V' (Atomic number- 23) in aqueous solution has magnetic moment of: |
\(\sqrt{24}BM\) \(\sqrt{15}BM\) \(\sqrt{12}BM\) \(\sqrt{3}BM\) |
\(\sqrt{15}BM\) |
The correct answer is option 2. \(\sqrt{15}BM\). The magnetic moment of an ion depends on the number of unpaired electrons it has. In the case of a divalent ion of vanadium (\(V^{2+}\)), we need to consider its electronic configuration to determine the number of unpaired electrons. The electron configuration of neutral vanadium (V) is: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^3 4s^2\). When vanadium loses two electrons to form \(V^{2+}\), its electronic configuration becomes: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^3\). So, the number of unpaired electrons, \(n = 3\) Hence, the magnetic moment, \(\mu = \sqrt{n(n + 2)}\) or, \(\mu = \sqrt{3(3 + 2)}\) or, \(\mu = \sqrt{3(5)}\) or, \(\mu = \sqrt{15} BM\) |