Respuesta :
Answer:
[tex]1s^22s^22p^63s^23p^63d^{4}[/tex]
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 -
[tex]1s^22s^22p^63s^23p^63d^{5}4s^2[/tex]
To form [tex]Mn^{3+}[/tex], it will lose 3 electrons from the valence electrons and thus the configuration of the ion is:-
[tex]1s^22s^22p^63s^23p^63d^{4}[/tex]
The electronic configuration of [tex]\rm Mn^3^+[/tex] ion is [tex]\rm \bold{1s^2\;2s^2\;2p^6\;3s^2\;3p^6\;4s^2\;3d^2}[/tex].
The electronic configuration helps in filling the electrons in the atomic orbitals by following the rules for the electron address determination.
The elements in order to attain the stable noble gas configuration, gain or lose electrons. On losing the electrons a +ve charge has been imparted. On gaining the electrons, a -ve charge has been imparted.
The given element is [tex]\rm Mn^3^+[/tex] ion:
The ion has +3 charge. This indicates that it has lose 3 electrons.
The atomic number of Mn = 25. This states that it has 25 electrons.
The number of electrons in [tex]\rm Mn^3^+[/tex] ion = 25 - 3
The number of electrons in [tex]\rm Mn^3^+[/tex] ion = 22
Thus the electronic configuration for [tex]\rm Mn^3^+[/tex] ion = [tex]\rm 1s^2\;2s^2\;2p^6\;3s^2\;3p^6\;4s^2\;3d^2[/tex]
The electronic configuration of [tex]\rm Mn^3^+[/tex] ion is [tex]\rm \bold{1s^2\;2s^2\;2p^6\;3s^2\;3p^6\;4s^2\;3d^2}[/tex].
For more information about the electronic configuration, refer to the link:
https://brainly.com/question/21940070
