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To understand the magnetic properties, we need to determine the electronic configuration of the Ni2+ ion in the complex. Nickel starts with eight d-electrons. But how do these electrons arrange themselves in the d orbitals when ammonia ligands surround the nickel ion? Ammonia is a strong-field ligand, which means it causes a large splitting of the d-orbitals. This means that the energy difference between the d-orbitals becomes significant, leading to the electrons pairing up in the lower-energy orbitals before occupying the higher-energy ones. Since the energy difference is considerable, the electrons will try to fill up the lower energy levels. The number of unpaired electrons directly affects the magnetic properties of the complex. The presence of unpaired electrons is the key to paramagnetism. This is because each unpaired electron acts like a tiny magnet, and these tiny magnets align when placed in an external magnetic field. The more unpaired electrons, the stronger the magnetic attraction.
