Discuss the formation of the nickel ion with a 2+ oxidation number.
I would approach it this way.
I would write the electron configuration for the neutral Ni atom (1s2 2s2 2p6......etc), then explain that removing the last two electrons will make it Ni+2 ion.
To discuss the formation of the nickel ion with a 2+ oxidation number, we need to understand the electron configuration and the possible oxidation states of nickel (Ni).
First, let's determine the electron configuration of neutral nickel. In its ground state, nickel has the electron configuration [Ar] 3d8 4s2.
To form an ion with a 2+ oxidation number, nickel must lose two electrons. However, the 4s orbital is emptied before the 3d orbital due to the Aufbau principle. So, in the case of nickel, the two electrons removed will come from the 4s orbital, leaving the 3d orbital completely filled with 10 electrons.
After losing two electrons, the electron configuration of the nickel ion (Ni2+) becomes [Ar] 3d8. Notice that the 3d orbital is half-filled, which is a relatively stable configuration.
The formation of the nickel ion with a 2+ oxidation number can occur through various processes, such as oxidation reactions, where nickel loses two electrons, or by combining with ligands in coordination complexes. In these complexes, the 3d electrons may participate in bonding and being shared between the metal center (nickel) and the ligands.
Overall, the formation of the nickel ion with a 2+ oxidation number involves the loss of two electrons from the 4s orbital, resulting in a stable electron configuration with a half-filled 3d orbital.