Given below are two statements, one is labelled as Assertion A and...

$[ Fe ( {H}_{2}O{)}_{6}{]}^{3 +}$ has magnetic moment value of $5 . 92BM$ because ${H}_{2}O$ is a weak ligand and pairing will not occur. It involves ${sp}^{3}{d}^{2}$ hybridisation with five unpaired electrons (because magnetic moment is equal to $5 . 92BM$) and outer orbital complex is formed. Magnetic moment can be calculated by the formula ${\mu}_{m} = \sqrt{n ( n + 2 )}$ $BM$ where, ${\mu}_{m} =$magnetic moment, $n =$number of unpaired electron(s).

${\mu}_{m} = 1 . 74BM, n = 1{\mu}_{m} = 5 . 92BM, n = 5$

In $[ Fe ( CN{)}_{6}{]}^{3 –}$complex ${CN}^{-}$ is stronger ligand than ${H}_{2}O$ according to spectrochemical series. Hence, four electrons will pair itself. It involves ${d}^{2}{sp}^{3}$hybridisation with one unpaired electron and inner orbital complex is formed and has a value of only $1 . 74BM$.

In Bothe the complexes the oxidation state of iron is +3.