QQuestionChemistry
QuestionChemistry
Draw the Lewis dot structure for the following ions:
Al³⁺, Mg²⁺, Se²⁻, N³⁻
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Answer
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Step 1:I'll solve this Lewis dot structure problem step by step, following the specified formatting guidelines:
Step 2:: Understanding Lewis Dot Structures
- Lewis dot structures represent the valence electrons of atoms - For ions, we need to account for the charge by adding or removing electrons - The goal is to show the electron configuration around each ion
Step 3:: Al³⁺ (Aluminum Ion)
- Aluminum's ground state electron configuration: $$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{1}
- Valence electrons: 3 - Loses 3 electrons to become Al³⁺ - Lewis dot structure: No dots (all valence electrons removed)
Step 4:: Mg²⁺ (Magnesium Ion)
- Magnesium's ground state electron configuration: $$1s^{2} 2s^{2} 2p^{6} 3s^{2}
- Valence electrons: 2 - Loses 2 electrons to become Mg²⁺ - Lewis dot structure: No dots (all valence electrons removed)
Step 5:: Se²⁻ (Selenide Ion)
\ddot{Se}\ddot{}
- Valence electrons: 6 - Gains 2 electrons to become Se²⁻ - Lewis dot structure: 8 dots around Se (full octet)
Step 6:: N³⁻ (Nitride Ion)
\ddot{N}\ddot{}
- Valence electrons: 5 - Gains 3 electrons to become N³⁻ - Lewis dot structure: 8 dots around N (full octet)
Final Answer
- Al³⁺: No dots - Mg²⁺: No dots - Se²⁻: \ddot{Se}\ddot{} (8 dots) - N³⁻: \ddot{N}\ddot{} (8 dots)
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