Answer: The electronic configuration is given below.
Explanation:
Electronic configuration tells us about the number of electrons that are present in an atom. It also determines the atomic number of an element.
Phosphorus is the 15th element of the periodic table having 15 electrons.
The electronic configuration for the given element = [tex]1s^22s^22p^63s^23p^3[/tex]
This element require 3 electrons and thus carry a charge of -3 units.
So, the electronic configuration for the phosphide ion which is formed by gaining 3 electrons = [tex]1s^22s^22p^63s^23p^6[/tex]
Thus, the electronic configuration is given above.
The electron configuration of the phosphide ion (p3-) is 1S²2s²2p⁶3S²3p⁶.
The arrangement of electrons in different energy levels around the atom of a nucleus.
The s,p,d,f is the energy orbitals and energy levels.
When phosphorus becomes a phosphide ion, the atom gains three electrons, which are added to the 3p subshell.
Thus, the electron configuration of the phosphide ion (p3-) is 1S²2s²2p⁶3S²3p⁶.
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