Questions: Answer the following questions pertaining to Lewis dot structures. Select the single best Lewis electron-dot symbol for the ion formed from Mg: [Mg]^+ [Mg]^2+ [Mg]^2- [Mg]^3+

Solution Steps

Magnesium (Mg) is an element in Group 2 of the periodic table, which means it has two valence electrons. When forming ions, magnesium tends to lose these two valence electrons to achieve a stable electron configuration similar to the nearest noble gas, neon (Ne).

We need to determine which of the given options correctly represents the ion formed by magnesium:

• \( [\mathbf{Mg}]^{+} \)
• \( [\mathbf{Mg}]^{2+} \)
• \( [\mathrm{Mg}]^{2-} \)
• \( [\mathbf{Mg}]^{3+} \)

Since magnesium loses two electrons to achieve a stable electron configuration, the correct ion formed is \( [\mathbf{Mg}]^{2+} \).

Final Answer