Question

directions: fill in the missing information for a given element.

1. ** phosphorus p
2. ** potassium k
3. * fluorine f
4. neon ne
5. sulfur s

Explanation:

Step1: Determine the preferred charge of Phosphorus

Phosphorus has 5 valence electrons. It gains 3 electrons to achieve a stable octet. So its preferred charge is \(P^{3 -}\).

Step2: Determine the preferred charge of Potassium

Potassium has 1 valence electron. It loses 1 electron to achieve a stable octet. So its preferred charge is \(K^{+}\).

Step3: Determine the preferred charge of Fluorine

Fluorine has 7 valence electrons. It gains 1 electron to achieve a stable octet. So its preferred charge is \(F^{-}\).

Step4: Determine the preferred charge of Neon

Neon is a noble gas. It has a full - filled valence shell (8 electrons). So its preferred charge is \(Ne\) (no charge, \(0\) charge).

Step5: Determine the preferred charge of Sulfur

Sulfur has 6 valence electrons. It gains 2 electrons to achieve a stable octet. So its preferred charge is \(S^{2 -}\).

Answer:

1. \(P^{3 -}\)
2. \(K^{+}\)
3. \(F^{-}\)
4. \(0\) (or \(Ne\) with no charge symbolically)
5. \(S^{2 -}\)