Based on patterns in the periodic table, which ion has a stable valence electron configuration?

Question

(1 point)
Responses

fluorine (F) with a
1
+
charge
fluorine (F) with a 1 raised to the plus power charge

sulfur (S) with a
1
−
charge
sulfur (S) with a 1 raised to the negative power charge

magnesium (Mg) with a
1
−
charge
magnesium (Mg) with a 1 raised to the negative power charge

potassium (K) with a
1
+
charge

Answer 1

To determine which ion has a stable valence electron configuration, we can look for ions that achieve a noble gas electron configuration, which is typically associated with stability.

1. Fluorine (F) with a +1 charge: This would only have 6 valence electrons (since it starts with 7 and loses one) and does not achieve a stable configuration.
2. Sulfur (S) with a -1 charge: This would have 7 valence electrons (since it starts with 6 and gains one) and does not achieve a stable configuration.
3. Magnesium (Mg) with a -1 charge: This is not common; magnesium typically loses 2 electrons to achieve a +2 charge and does not gain electrons to have a -1 charge.
4. Potassium (K) with a +1 charge: Potassium loses one electron, achieving the stable electron configuration of the noble gas argon (18 electrons, with a full outer shell).

The only ion that achieves a stable valence electron configuration is potassium (K) with a +1 charge.