Explanation of Magnetism in Pt(NH3)2Cl2
Pt(NH3)2Cl2 is a coordination complex consisting of platinum metal ion coordinated with ammine ligands (NH3) and chloride ions (Cl). The magnetism exhibited by this complex can be explained by considering the electronic configuration of the metal ion and the ligand field theory.

Electronic Configuration
- Platinum (Pt) is a transition metal with an electronic configuration of [Xe] 4f14 5d9 6s1.
- In Pt(NH3)2Cl2, the Pt(II) ion loses one electron to form a +2 oxidation state, resulting in a d8 configuration.

Ligand Field Theory
- The ammine ligands and chloride ions act as ligands that create a ligand field around the Pt(II) ion.
- The ligand field splits the d orbitals of the metal ion into higher energy and lower energy levels.

Magnetic Behavior
- In the case of Pt(NH3)2Cl2, the d8 configuration corresponds to a diamagnetic species.
- Diamagnetic substances are repelled by a magnetic field as they contain all paired electrons, resulting in a net magnetic moment of zero.

Conclusion
- Therefore, Pt(NH3)2Cl2 exhibits diamagnetic behavior due to the presence of paired electrons in the d orbitals of the Pt(II) ion.