The electronic configuration of Mg 2+ is

The electronic configuration of Mg2+ is: Is2 2s2 2p6. This configuration can be determined by first looking at the electron configuration of a neutral magnesium atom, which is 1s2 2s2 2p6 3s2. When magnesium loses two electrons to become Mg2+, the two electrons that are removed come from the 3s orbital, leaving behind the completely filled 2p orbital. Thus, the electronic configuration of Mg2+ is 1s2 2s2 2p6, which can be abbreviated as Is2 2s2 2p6. To understand this configuration, we can break it down into the following parts: - "Is2" represents the completely filled 1s orbital, which contains two electrons. - "2s2" represents the completely filled 2s orbital, which also contains two electrons. - "2p6" represents the completely filled 2p orbital, which contains six electrons. Overall, the electronic configuration of Mg2+ has a total of 12 electrons, with all the lower energy orbitals completely filled and the 2p orbital partially filled with six electrons.