The molecule ICl4 (Iodine tetrachloride) is considered nonpolar. To understand why, we need to look at its molecular geometry and the electronegativity of the atoms involved.
ICl4 has a central iodine atom bonded to four chlorine atoms. The molecular geometry of ICl4 is square planar. In a square planar arrangement, the polar bonds (I-Cl) effectively cancel each other out because they are symmetrically arranged around the central iodine atom.
Even though the I-Cl bonds are polar due to the difference in electronegativity between iodine and chlorine, the symmetrical shape means that the dipole moments point in opposite directions, resulting in a net dipole moment of zero. Thus, the overall structure of ICl4 is nonpolar.