What may be the stable oxidation states of the transition elements with the following $d$ electron configurations in the ground state of their atoms: $3d^3$,$3d^5$,$3d^8$,and $3d^4$?
(N/A) The stable oxidation states depend on the electronic configuration and the stability of the resulting ions.
| Electronic configuration in ground state | Stable oxidation states |
| $(i)$ $3d^3$ (e.g.,$V$) | $+2, +3, +4, +5$ |
| $(ii)$ $3d^5$ (e.g.,$Cr$ or $Mn$) | For $Cr$: $+3, +6$; For $Mn$: $+2, +4, +6, +7$ |
| $(iii)$ $3d^8$ (e.g.,$Ni$) | $+2, +3$ |
| $(iv)$ $3d^4$ | There is no transition element with a $3d^4$ configuration in the ground state (as $Cr$ is $3d^5 4s^1$). |
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