Question

the lewis diagram for a neutral phosphorus atom is shown below.
p
complete the statement.
to produce a stable ion, a neutral phosphorus atom will
electron(s).
show periodic table

Explanation:

Step1: Recall Phosphorus' Electron Configuration

Phosphorus (P) has an atomic number of 15, so its electron configuration is \(1s^2 2s^2 2p^6 3s^2 3p^3\). The valence electrons are in the \(3s\) and \(3p\) orbitals, totaling 5 valence electrons (as seen in the Lewis diagram: 5 dots).

Step2: Determine Stable Ion Formation

To achieve a stable octet (8 valence electrons, like the nearest noble gas, argon), a phosphorus atom can gain 3 electrons (since it has 5 valence electrons; \(5 + 3 = 8\)). Gaining electrons means it will form an anion (\(P^{3-}\)). So the neutral P atom will gain 3 electrons.

Answer:

To produce a stable ion, a neutral phosphorus atom will $\boldsymbol{\text{gain}}$ $\boldsymbol{3}$ electron(s).