Question

Question 4
A)
Use the periodic table to answer the question.

An illustration shows the periodic table of elements. The elements in the periodic table are arranged in groups (columns numbered 1 through 18) and periods (rows numbered 1 through 7) such that the atomic number increases along a period from left to right. The elements are divided into the following categories: · Alkali metals · Alkaline earth metals · Transition metals · Post-transition metals · Lanthanides · Actinides · Metalloids · Nonmetals · Noble gases · Unknown The elements are also classified on the basis of their physical states as follows: · Solid · Liquid · Gas · Unknown The element sulfur is enlarged with the following properties. · Chemical symbol: S · Name: Sulfur · Atomic Number: 16 · Atomic mass: 32.06 · Common oxidation states: 6, 4, 2, negative 2 · Electronegativity: 2.58 · Ionization energies: 999.589 · Electron configuration: [Ne] 3s2 3p4

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

(1 point)
Responses

potassium (K) with a 1+
charge
potassium (K) with a 1 raised to the plus power charge

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

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

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

pick 1

Answer 1

To determine which ion has a stable valence electron configuration, we need to look for an ion that adopts a full outer electron shell, which is characteristic of the noble gases (group 18).

1. **Potassium (K)**: It typically loses one electron to form a K⁺ ion, achieving a configuration like argon (18 electrons). This configuration is stable.

2. **Fluorine (F)**: It typically gains one electron to form a F⁻ ion, achieving a configuration like neon (10 electrons). This is also stable.

3. **Magnesium (Mg)**: It typically loses two electrons to form a Mg²⁺ ion, which ends up with the same electron configuration as neon. That is stable as well.

4. **Sulfur (S)**: When sulfur gains two electrons, it becomes S²⁻, achieving a configuration similar to argon, which is considered stable.

Since all of these ions can achieve stable configurations by either gaining or losing electrons, the question may be asking for the one that is most common among them or perhaps the one that typically achieves a noble gas configuration through gaining rather than losing.

**Answer:** **fluorine (F) with a 1− charge** (F⁻) is a common choice since it gains an electron to achieve a stable noble gas configuration.