QQuestionChemistry
QuestionChemistry
"Draw the Lewis structure for the hydrazine N^2 H^4
molecule and determine the number of double bonds in the molecule."
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Answer
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Step 1:I'll solve this problem step by step, following the specified LaTeX and formatting guidelines:
Step 2:: Determine the total number of valence electrons
- Total valence electrons: $$2 \times 5 + 4 \times 1 = 14$$ valence electrons
- Nitrogen (N) has 5 valence electrons - Hydrogen (H) has 1 valence electron
Step 3:: Arrange the atoms in the molecule
- Place the two nitrogen atoms in the center - Attach hydrogen atoms to the nitrogen atoms
Step 4:: Connect atoms with single bonds
\begin{array}{c}
- First, connect the two nitrogen atoms with a single bond - Attach hydrogen atoms to each nitrogen H-N-N-H \ H \quad H \end{array}
Step 5:: Distribute remaining electrons as lone pairs
- Remaining electrons: $$14 - 4 = 10$$ electrons
- Initial single bonds used: 4 electrons - Add lone pairs to complete octets for both nitrogen atoms
Step 6:: Determine double bonds
\begin{array}{c}
- To satisfy the octet rule, one single bond between nitrogen atoms will become a double bond H-N=N-H \ H \quad H \end{array}
Final Answer
Key points: - Total valence electrons: 14 - Double bond count: 1 - Each nitrogen has 3 lone pairs - Each hydrogen is bonded with a single bond
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