QQuestionChemistry
QuestionChemistry
"The anion O^3− does not obey the octet rule.
Draw its Lewis structure.
State the type of octet-rule exception.
Indicate the values of nonzero formal charges.
Include lone pair electrons."
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Answer
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Step 1:: Draw the Lewis structure for the ozone anion (O^3−).
Start by placing the central oxygen atom and then add the two outer oxygen atoms around it. Place a single bond between the central and outer atoms: \mathrm{O}-\mathrm{O}=\mathrm{O}
Step 2:: Calculate the formal charge for each oxygen atom.
To calculate the formal charge, use the formula: For the central oxygen atom: - Valence electrons: 6 - Nonbonding electrons: 4 (two lone pairs) - Bonding electrons: 4 (two bonds) So, For each outer oxygen atom: - Valence electrons: 6 - Nonbonding electrons: 2 (one lone pair) - Bonding electrons: 4 (two bonds) So,
Step 3:: Identify the type of octet-rule exception.
In this case, the central oxygen atom has 6 electrons in its outer shell, which is an expanded octet. The two outer oxygen atoms have 7 electrons in their outer shell, which is also an expanded octet.
Step 4:: Indicate the values of nonzero formal charges.
The formal charge for each outer oxygen atom is + 1.
Step 5:: Include lone pair electrons.
Adding lone pair electrons to the Lewis structure: \mathrm{O}: \underline{\mathrm{O}}=\mathrm{O}:
Final Answer
The Lewis structure for the ozone anion (O^3−) is: \mathrm{O}: \underline{\mathrm{O}}=\mathrm{O}: The type of octet-rule exception is an expanded octet for the central and outer oxygen atoms. The nonzero formal charges are + 1 for each outer oxygen atom.
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