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Which of the following Lewis dot structures correctly represents the ion Cl^-?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Ions
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Which of the following best represents the Lewis dot structure for the ionic compound magnesium oxide (MgO)?
A
Mg with two dots and O with six dots
B
Mg^{+} with one dot and O^{-} with seven dots
C
Mg^{2+} with no dots and O^{2-} with eight dots (a full octet)
D
Mg with no dots and O with eight dots
Guida verificata passo dopo passo1
Step 1: Understand that magnesium oxide (MgO) is an ionic compound formed between magnesium (Mg) and oxygen (O). Magnesium tends to lose electrons to achieve a stable electron configuration, while oxygen tends to gain electrons.
Step 2: Recall that magnesium is in Group 2 of the periodic table, so it has 2 valence electrons. It will lose these 2 electrons to form a Mg^{2+} ion, resulting in no dots around Mg in the Lewis structure.
Step 3: Oxygen is in Group 16 and has 6 valence electrons. It will gain 2 electrons (to complete its octet) to form an O^{2-} ion, which means it will have 8 dots (representing 8 valence electrons) around it in the Lewis structure.
Step 4: The Lewis structure for MgO should show Mg^{2+} with no dots (since it lost its valence electrons) and O^{2-} with eight dots (a full octet), indicating the transfer of electrons and the formation of ions.
Step 5: Confirm that this representation matches the ionic nature of MgO, where Mg^{2+} and O^{2-} ions are held together by electrostatic attraction, which is characteristic of ionic compounds.
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