Question

use the periodic table to answer the question
based on patterns in the periodic table, which ion has a stable valence electron configuration?
(1 point)
magnesium (mg) with a 1 - charge
sulfur (s) with a 1 - charge
potassium (k) with a 1+ charge
fluorine (f) with a 1+ charge

Explanation:

Step1: Recall stable electron configuration

Atoms gain or lose electrons to achieve a stable electron configuration similar to noble gases (full valence shell).

Step2: Analyze each option

• Magnesium (\(Mg\)) with \(1^{-}\) charge:

Magnesium has an atomic number of \(12\). Its electron configuration is \([Ne]3s^{2}\). If it gains one electron (\(Mg^{-}\)), it does not have a noble - gas - like configuration.

• Sulfur (\(S\)) with \(1^{-}\) charge:

Sulfur has an atomic number of \(16\). Its electron configuration is \([Ne]3s^{2}3p^{4}\). If it gains one electron (\(S^{-}\)), \(3s^{2}3p^{5}\), not a noble - gas - like configuration.

• Potassium (\(K\)) with \(1^{+}\) charge:

Potassium has an atomic number of \(19\). Its electron configuration is \([Ar]4s^{1}\). When it loses one electron (\(K^{+}\)), its electron configuration is \([Ar]\), which is the electron configuration of argon (a noble gas).

• Fluorine (\(F\)) with \(1^{+}\) charge:

Fluorine has an atomic number of \(9\). Its electron configuration is \([He]2s^{2}2p^{5}\). If it loses one electron (\(F^{+}\)), \(2s^{2}2p^{4}\), not a noble - gas - like configuration.

Answer:

potassium (\(K\)) with a \(1^{+}\) charge