The incorrect statement is :

<p>To identify the incorrect statement, let&#39;s analyze each option :</p> <p>Option A : &quot;In manganate and permanganate ions, the π-bonding takes place by overlap of p-orbitals of oxygen and d-orbitals of manganese.&quot; This statement is true. In both manganate ${MnO}_4^{2-} $ and permanganate ${MnO}_4^- $ ions, the manganese atom is in a high oxidation state (+6 and +7, respectively) and forms bonds with oxygen atoms involving the overlap of p-orbitals of oxygen and d-orbitals of manganese.</p> <p>Option B : &quot;Manganate ion is green in colour and permanganate ion in purple in colour.&quot; This statement is true. Manganate ions are indeed green and permanganate ions are purple in aqueous solution.</p> <p>Option C : &quot;Manganate and permanganate ions are paramagnetic.&quot; This statement is incorrect. Both manganate and permanganate ions are diamagnetic, not paramagnetic. In these ions, manganese is in +6 and +7 oxidation states, respectively, and has no unpaired electrons.</p> Manganate($\mathop {Mn}\limits^{ + 6}$O₄ ^2–) , <br><br>Mn(25) = [Ar]3d⁶4s² <br><br>Mn⁺⁶(25) = [Ar]3d¹ $\to$ Paramagnetic <br><br>Permanganate ($\mathop {Mn}\limits^{ + 7}$O₄^-) <br><br>Mn(25) = [Ar]3d⁶4s² <br><br>Mn⁺⁷(25) = [Ar]3d⁰ $\to$ Diamagnetic <p>Option D : &quot;Manganate and permanganate ions are tetrahedral.&quot; This statement is true. Both manganate and permanganate ions have a tetrahedral geometry, with the manganese atom at the center and the four oxygen atoms surrounding it.</p> <p>Therefore, the incorrect statement is option C.</p>