QQuestionChemistry
QuestionChemistry
Construct a Lewis structure for hydrogen peroxide, H^2O^2, in which each atom achieves a stable noble-gas electron configuration. Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons.
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Answer
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Step 1:I'll solve this Lewis structure problem step by step:
Step 2:: Determine the total number of valence electrons
- Total valence electrons: $$2 + 12 = 14$$ electrons
- Hydrogen (H): 1 electron × 2 atoms = 2 electrons - Oxygen (O): 6 electrons × 2 atoms = 12 electrons
Step 3:: Arrange atoms in the structure
\text{H-O-O-H}
- Connect the two oxygen atoms with a single bond - Attach hydrogen atoms to each oxygen atom
Step 4:: Distribute remaining electrons as lone pairs
- First, place single bonds between atoms - Remaining electrons go to oxygen atoms as lone pairs - Each oxygen atom needs 8 electrons to be stable
Step 5:: Complete the Lewis structure
- Place 3 lone pairs on each oxygen atom - Ensure each atom follows the octet rule - Final structure shows: * Single bond between oxygen atoms * Single bonds to hydrogen atoms * 3 lone pairs on each oxygen atom Final Lewis Structure: \begin{array}{c} \text{H} \ \quad \downarrow \ \text{:O:} - \text{:O:} \ \quad \uparrow \ \text{H} \end{array}
Final Answer
The Lewis structure of hydrogen peroxide (H₂O₂) consists of a single bond between oxygen atoms, single bonds to hydrogen atoms, and 3 lone pairs on each oxygen atom.
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