Answer:
9 p-electrons
Explanation:
Phosphorus is a reactive chemical element that belongs to the group 15 and period 3 of the periodic table. It is a p-block element having atomic number 15.
The electronic configuration of phosphorus in the ground state is 1s² 2s² 2p⁶ 3s² 3p³.
Since, 6 electrons are present in the 2p subshell and 3 electrons are present in the 3p subshell.
Therefore, there are total 9 p-electrons in a phosphorus atom present in its ground state.
The total number of p electrons present in phosphorus atom is 9
In Phosphorus electron configuration we the P atom has 15 electrons.
In writing the configuration, the 15 electrons are placed around the nucleus of the Phosphorus atom.
Since the atomic number of P is 15.
2 electrons can go into the 1s subshell, 2 electron also go into the 2s subshell,
6 electron do enter into the 2p subshell.
3 subshell has 2 electron while the last 3p subshell also contains 3 electron
Hence the total number of p electrons is 6+3=9.
Therefore, the total number of p electrons is 6+3=9.
Conclusively, the number of protons is also equal to number of electrons in a neutral atom.
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