The incorrect statement is:

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(C) $1$) Manganate ion $(MnO_{4}^{2-})$ has $Mn$ in $+6$ oxidation state $(3d^1)$,which is paramagnetic due to one unpaired electron.$2$) Permanganate

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Manganate and permanganate ions are paramagnetic.

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(C) $1$) Manganate ion $(MnO_{4}^{2-})$ has $Mn$ in $+6$ oxidation state $(3d^1)$,which is paramagnetic due to one unpaired electron.$2$) Permanganate ion $(MnO_{4}^{-})$ has $Mn$ in $+7$ oxidation state $(3d^0)$,which is diamagnetic due to no unpaired electrons.$3$) Therefore,the statement that both are paramagnetic is incorrect.$4$) Both ions exhibit $d^3s$ hybridization (often described as $sp^3$ in simpler models) and possess a tetrahedral geometry.$5$) The $\pi$-bonding involves the overlap of $2p$-orbitals of oxygen with $3d$-orbitals of manganese.$6$) Manganate is green and permanganate is purple.

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