Which of the following is not correct w.r.t. covalent character of ionic bond? 

Cation polarises the anion.

For same size and charge of cation, the one with electronic configuration $\left(\mathrm{n}-1\right){\mathrm{d}}^{\mathrm{x}}{\mathrm{ns}}^0$ is more polarising than the cation having ${\mathrm{ns}}^2{\mathrm{np}}^6$ electronic configuration.

Electronic charge shifts towards cation to create covalent character.

Smaller the charge on cation and anion, greater is the covalent character.