Introduction:
Pt(NH3)2Cl2 is a coordination complex in which a central platinum atom is surrounded by ammonia (NH3) and chloride (Cl) ligands. The magnetic properties of this complex arise from the presence of unpaired electrons in the d orbitals of the platinum atom.

Magnetic Properties:
- The magnetic behavior of Pt(NH3)2Cl2 can be explained using the concept of spin-only magnetic moment.
- The unpaired electrons in the d orbitals of the platinum atom result in a non-zero spin-only magnetic moment, indicating that the complex is paramagnetic.
- Paramagnetic substances are attracted to a magnetic field due to the presence of unpaired electrons that align with the external magnetic field.

Explanation:
- In Pt(NH3)2Cl2, the platinum atom has a d8 electronic configuration, with two unpaired electrons in its d orbitals.
- These unpaired electrons give rise to magnetic moments that align with an external magnetic field, causing the complex to be attracted to the field.
- The presence of the ammonia and chloride ligands does not significantly affect the magnetic properties of the complex, as the unpaired electrons are localized on the platinum atom.

Conclusion:
In conclusion, the magnetic behavior of Pt(NH3)2Cl2 can be attributed to the presence of unpaired electrons in the d orbitals of the platinum atom. This results in a spin-only magnetic moment, making the complex paramagnetic and attracted to external magnetic fields.