Give reasons:
(i) Mn shows the highest oxidation state of +7 with oxygen but with fluorine it shows the highest oxidation state of +4 .
(ii) Transition metals show variable oxidation states.
(iii) Actinoids show irregularities in their electronic configurations.

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Solution

$(i)$ $M n$ do not show $+ 7$ oxidation with fluorine as it does not have the ability to form multiple bonds with $M n$ . If seven fluorine atoms are attracted to $M n$ , then $δ +$ at $M n$ will be too high and compound will be unstable.
$(i i)$ Transition metal when forms compounds, the electrons present in $n_{s}$ and $(n - 1) d$ orbitals can participate in bonding due to almost similar energies.
$(i i i)$ Because the energy difference between $5 f, 6 d$ and $7 s$ subshell of the actinoids is very small due to Actinoids contraction hence electrons could be accommodated in any of them.

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\begin{matrix} (i) & 2 M n O_{2} & + & 4 K O H & + & O_{2} & △ - \to (i i) & C r_{2} O_{7}^{2 -} & + & 14 H^{+} & + & 6 I^{-} & - \to \end{matrix}

\begin{matrix} (i) & 2 M n O_{2} & + & 4 K O H & + & O_{2} & △ - \to (i i) & C r_{2} O_{7}^{2 -} & + & 14 H^{+} & + & 6 I^{-} & - \to \end{matrix}

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