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Phosphorus has 5 valence electron. It forms anion by gaining 3 electrons.
Phosphorus in is 3rd period. So it has 3 electron shells.
Zero. First n=3; second l = 0; third m = 0.
Bohr's model explains how electron transitions cause hydrogen's atomic emission spectra. The quantum model is a 3-d view of the atom, which shows an electron's energy levels and sublevels and the probability of an electron's location, proven with complex mathematics.
In the third period.
3
n=3
Phosphorus has 5 valence electron. It forms anion by gaining 3 electrons.
The principal quantum number n = 3 and the azimuthal or orbital angular momentum quantum number would be l =1 .l = 1
Phosphorus in is 3rd period. So it has 3 electron shells.
Phosphorus, like all atoms, tries to achieve a full electron shell. For Phosphorus to achieve its full shell and obtain an electron configuration that is isoelectronic with Argon, it must gain 3 electrons. Therefore, Phosphorus forms a -3 anion.
Zero. First n=3; second l = 0; third m = 0.
n=3
The valence electrons are the outermost (highest energy) s and p sublevels. There are 5 valence electrons in a phosphorus atom, and it is in period 3, so its valence electron configuration is 3s23p3.
A 3s electron
All of the elements in Period 3, excluding group 18/VIIIA, have the same inside electron arrangement as phosphorus. They all have the electron configuration of neon as their inside arrangement of electrons.
Phosphorus ion (P³⁻) typically gains three electrons to achieve a stable electron configuration. As a result, it carries a charge of -3 and has a full outer electron shell.