Which statement is correct about ${\mathrm{ICl}}_3$ molecule?

Iodine trichloride all adjacent bond angles are equal
Additionally, not all $\mathrm{I}-\mathrm{Cl}$ bonds are the same. Some bonds are axial or analogous bonds.
Iodine trichloride is the formal name of the ${\mathrm{ICl}}_3$ molecule. Iodine and chlorine combine to form this interhalogen substance.
Each chlorine atom contributes one electron, making a total of five pairs, whereas iodine possesses seven electrons.
These five pairs of electrons align and create a trigonal bipyramidal structure. Iodine trichloride is supposed to take on a T-shape according to the valence shell electron pair repulsion (VSEPR) hypothesis, yet its initial shape was trigonal bipyramidal.
The difference between the electronegativity of iodine and chlorine causes the molecule ${\mathrm{ICl}}_3$ to have a net dipole moment that is greater than zero, making it polar and non-planar.
Axial $\mathrm{I}-\mathrm{Cl}$ bonds have less s-character than equatorial $\mathrm{I}-\mathrm{Cl}$ bonds do. So,

$(\mathrm{I}-\mathrm{Cl}{)}_{\mathrm{a}}>(\mathrm{I}-\mathrm{Cl}{)}_{\mathrm{e}}(\mathrm{B}.\mathrm{L})$

Molecule is polar and planar

Hence, correct option is c.