The magnetic moment of a transition metal compound has been calculated to be $3.87$ $B.M.$ The metal ion is

  • [JEE MAIN 2023]
  • A

    $Cr ^{2+}$

  • B

    $Mn ^{2+}$

  • C

    $V ^{2+}$

  • D

    $Ti ^{2+}$

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How would you account for the following:

$(i)$ of the $d^{4}$ species, $Cr ^{2+}$ is strongly reducing while manganese $(III)$ is strongly oxidising.

$(ii)$ Cobalt $(II)$ is stable in aqueous solution but in the presence of complexing reagents it is easily oxidised.

$(iii)$ The $d^{1}$ configuration is very unstable in ions.

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