Explanation of Dipole Moment in PtCl4 2-
PtCl4 2- is a square planar complex ion with a coordination number of 4. The dipole moment of a molecule or ion is the measure of the separation of positive and negative charges within the molecule or ion. In the case of PtCl4 2-, the dipole moment is zero due to the symmetrical arrangement of the chloride ions around the central platinum atom.

Geometry of PtCl4 2-
- PtCl4 2- has a square planar geometry with the platinum atom at the center and four chloride ions surrounding it.
- The chloride ions are arranged symmetrically around the platinum atom, with two chloride ions lying in the plane and the other two lying above and below the plane.

Symmetry of PtCl4 2-
- Due to the symmetrical arrangement of the chloride ions, the dipole moments of the individual Pt-Cl bonds cancel each other out.
- The dipole moment is a vector quantity, and in PtCl4 2-, the individual dipole moments of the Pt-Cl bonds point in opposite directions and have equal magnitudes, resulting in a net dipole moment of zero.

Effect of Symmetry on Dipole Moment
- In molecules or ions with high symmetry, such as PtCl4 2-, the dipole moment is often zero due to the cancelation of dipole moments from individual bonds.
- The symmetry of the molecule or ion plays a crucial role in determining the overall dipole moment.
In conclusion, the dipole moment of PtCl4 2- is zero due to the symmetrical arrangement of chloride ions around the central platinum atom, which results in the cancelation of dipole moments from individual Pt-Cl bonds.