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What is the electronic configuration of Hg2+ ?

Answer
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Hint : Hg2+ ion is formed when an Hg atom loses two electrons. When losing electrons, the electrons in the outermost (valence) shells are lost first. But while filling up the orbitals we have to follow the Aufbau principle and other rules.

Complete Step By Step Answer:
Well, we know that the atomic number of mercury is 80 . We will find the electronic configuration of its ground state 80Hg first using the Aufbau’s principle, Pauli’s exclusion principle and Hund’s rule. We can easily find its electronic configuration to be 1s22s22p63s23p64s23d104p65s24d105p66s24f145d10 . We know that the ionic species Hg2+ is formed when it loses two electrons. We have to remember that an element loses electrons from its outermost or valence shell. Here, the valence electrons are in the 6s orbital. So, the two electrons of 6s orbital are lost. Hence, the electronic configuration of Hg2+ is 1s22s22p63s23p64s23d104p65s24d105p66s04f145d10 . Now re-arranging it we get the electronic configuration to be 1s22s22p63s23p63d104s24p64d104f145s25p65d106s0 . It is easy to observe the noble gas configuration of 80Hg to be [Xe]4f145d106s2 and so that of Hg2+ as [Xe]4f145d10 .

Note :
It is common to get confused and remove the electrons from the 5d orbital instead of removing from 6s orbital as 5d orbitals are filled up last. Always keep in mind that while filling up orbitals we have to use the Aufbau’s principle and fill up the less energy orbitals first. But in case of removing electrons, the electrons in the valence shells are easy to lose, so we have to remove them from the valence shells first, and then the pen-ultimate shells and so on.