QQuestionChemistry
QuestionChemistry
Draw the Lewis structure and determine the molecular geometry for NH^2 Cl.
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Answer
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Step 1:I'll solve this problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Determine the total number of valence electrons
Total valence electrons: $$5 + (1 \times 2) + 7 = 14$$ electrons
- Nitrogen (N): 5 valence electrons - Hydrogen (H): 1 valence electron × 2 - Chlorine (Cl): 7 valence electrons
Step 3:: Arrange atoms and connect with single bonds
\text{Cl} - \text{N} - \text{H}_{2}
- Place Cl as the central atom - Connect N and H atoms to Cl - Initial electron distribution:
Step 4:: Distribute remaining electrons as lone pairs
- Remaining electrons: $$14 - 2 = 12$$ electrons
- First, use 2 electrons for N-Cl bond - Place lone pairs on Cl and N - Ensure octet rule is satisfied
Step 5:: Draw Lewis structure
- N has one lone pair - Cl has three lone pairs - Two H atoms single-bonded to N
Step 6:: Determine molecular geometry
- Bond angle approximately $$109.5^{\circ}
- Central atom: N - Electron domain geometry: Trigonal pyramidal - Molecular geometry: Trigonal pyramidal
Final Answer
The Lewis structure for NH₂Cl shows a trigonal pyramidal molecular geometry with N as the central atom, two H atoms, one Cl atom, and one lone pair on N.
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