QQuestionChemistry
QuestionChemistry
Draw a Lewis structure for H^3O+ . Show all unshared electrons and the formal charges, if any. Assume that bonding follows the octet rule.
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Answer
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Step 1:I'll solve this step-by-step, following the LaTeX formatting guidelines precisely:
Step 2:: Identify the Atoms and Valence Electrons
- Hydrogen (H): 1 valence electron × 3 = 3 electrons - Oxygen (O): 6 valence electrons - Total valence electrons: 3 + 6 = 9 electrons
Step 3:: Arrange the Central Atom and Hydrogens
- Oxygen will be the central atom - Arrange three hydrogen atoms around the oxygen
Step 4:: Connect Atoms with Single Bonds
\begin{array}{c} \text{H} \ \downarrow \ \text{O} \leftarrow \text{H} \ \uparrow \ \text{H} \end{array}
Step 5:: Distribute Remaining Electrons
- 9 total valence electrons - 3 single bonds use 6 electrons - Remaining 3 electrons go as lone pairs on oxygen
Step 6:: Calculate Formal Charges
- Hydrogens: \frac{1 - 0 - 1}{2} = 0 Final Lewis Structure: \begin{array}{c} \text{H}^{\delta-} \ \downarrow \ \text{O}^{+} \leftarrow \text{H} \ \uparrow \ \text{H}^{\delta-} \end{array}
Final Answer
The Lewis structure shows a central oxygen with three single bonds to hydrogen atoms, a lone pair on oxygen, and a + 1 formal charge on the oxygen atom.
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