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.

$\left(i\right)$ $Mn$ do not show $+7$ oxidation with fluorine as it does not have the ability to form multiple bonds with $Mn$. If seven fluorine atoms are attracted to $Mn$, then $\delta +$ at $Mn$ will be too high and compound will be unstable.

$\left(ii\right)$ 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.

$\left(iii\right)$ Because the energy difference between $5f,6d$ and $7s$ subshell of the actinoids is very small due to Actinoids contraction hence electrons could be accommodated in any of them.