Question

Which of the following represents the ground state electron configuration for the Mn3+ ion? (Atomic number Mn = 25) 1s2 2s22p6 3s23p63d4

Answer 1

The ground state electron configuration for the Mn3+ ion is 1s2 2s2 2p6 3s2 3p6 3d4 after removing three electrons from the highest energy orbitals, which are the 4s and 3d in the case of manganese.

Step-by-step explanation:

The ground state electron configuration for the Mn3+ ion starts with the neutral manganese atom, which has an atomic number of 25. The neutral Mn atom would have an electron configuration of 1s2 2s2 2p6 3s2 3p6 3d5 4s2. However, for Mn3+, three electrons are removed to account for the +3 charge, typically from the outermost orbitals first which in this case are the 4s and 3d orbitals. Since the 4s electrons are generally removed before the 3d electrons, after losing two electrons from 4s and one electron from 3d, the configuration will be 1s2 2s2 2p6 3s2 3p6 3d4.

Answer 2

`1s^22s^22p^63s^23p^63d^(4)`

Step-by-step explanation:

Manganese is the element of group 7 and forth period. The atomic number of Manganese is 25 and the symbol of the element is Mn.

The electronic configuration of the element, manganese is -

`1s^22s^22p^63s^23p^63d^(5)4s^2`

To form
`Mn^(3+)`, it will lose 3 electrons from the valence electrons and thus the configuration of the ion is:-

`1s^22s^22p^63s^23p^63d^(4)`