The electronic configuration of a metal ion in its complex is $[\mathrm{Ar}] 3 \mathrm{~d}^4$. For this…

The electronic configuration of a metal ion in its complex is $[\mathrm{Ar}] 3 \mathrm{~d}^4$. For this metal complex, $\Delta_0 < \mathrm{P}(\mathrm{P}=$ energy required for electron pairing in a single orbital). The distribution of electrons in the complex.
  1. $\left(\mathrm{t}_{2 \mathrm{~g}}\right)^3\left(\mathrm{e}_{\mathrm{g}}\right)^1$
  2. $\left(\mathrm{t}_{2 \mathrm{~g}}\right)^2\left(\mathrm{e}_g\right)^2$
  3. $\left(\mathrm{t}_{2 \mathrm{~g}}\right)^4\left(\mathrm{e}_{\mathrm{g}}\right)^0$
  4. $\left(t_{2 g}\right)^1\left(e_g\right)^3$

Solution

No solution. Refer to answer key.

Asked in: AP EAMCET 2017 (26 Apr Shift 2)

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