Question

ionic charge
match each element to
the charge of the ion it
most commonly
forms.
sulfur
1+
iodine
1-
boron
2-
calcium
2+
potassium
3+

Explanation:

• Sulfur (\(S\)) is in Group 16 of the periodic table. Elements in Group 16 gain 2 electrons to achieve a stable electron configuration, so sulfur forms \(S^{2 -}\) ions.
• Iodine (\(I\)) is in Group 17. Elements in Group 17 gain 1 electron to get a stable electron configuration, so iodine forms \(I^{-}\) ions.
• Boron (\(B\)) is in Group 13. Elements in Group 13 lose 3 electrons to attain a stable electron configuration, so boron forms \(B^{3+}\) ions.
• Calcium (\(Ca\)) is in Group 2. Elements in Group 2 lose 2 electrons to achieve a stable electron configuration, so calcium forms \(Ca^{2+}\) ions.
• Potassium (\(K\)) is in Group 1. Elements in Group 1 lose 1 electron to get a stable electron configuration, so potassium forms \(K^{+}\) ions.

Answer:

• sulfur: \(2 -\)
• iodine: \(1 -\)
• boron: \(3+\)
• calcium: \(2+\)
• potassium: \(1+\)