Question

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

Answer 1

Answer:

$1s^22s^22p^63s^23p^63d^{4}$

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:-

$1s^22s^22p^63s^23p^63d^{4}$

Answer 2

Answer:

1s2 2s22p6 3s23p63d4

Explanation:

A total of 22 electrons  which is right for Mn3+  as At No. of Mn is 25.