Reasons why PtCl4 2- does not conduct electricity like K4Fe(CN)6

Chemical Structure:
- PtCl4 2- contains a central platinum atom surrounded by four chloride ions, resulting in a covalent molecular structure.
- K4Fe(CN)6, on the other hand, consists of a potassium cation complexed with a hexacyanoferrate anion, which forms an ionic lattice structure.

Bonding Nature:
- PtCl4 2- has covalent bonds between the platinum and chlorine atoms, leading to a lack of mobile charge carriers necessary for conductivity.
- In K4Fe(CN)6, the ionic bonds between potassium and the hexacyanoferrate complex allow for the movement of ions, facilitating conductivity.

Charge Carriers:
- The absence of free ions in PtCl4 2- limits its ability to conduct electricity, as there are no charged particles available to carry the current.
- K4Fe(CN)6, being an ionic compound, contains mobile ions that can move and carry electric current when a potential difference is applied.

Diamagnetic Properties:
- Both PtCl4 2- and K4Fe(CN)6 are diamagnetic, meaning they exhibit weak repulsion in the presence of a magnetic field. However, this property does not directly influence their conductivity.

Conclusion:
- In summary, the difference in chemical structure, bonding nature, and presence of charge carriers between PtCl4 2- and K4Fe(CN)6 determine their conductivity properties. While both compounds may be diamagnetic, their ability to conduct electricity varies based on their unique characteristics.