QQuestionChemistry
QuestionChemistry
Which of the following characteristics apply to NCl₃?
A. Polar bonds
B. Nonpolar molecule
C. Trigonal pyramidal molecular shape
D. sp³ hybridized
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Answer
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Step 1:Let's solve this step by step by analyzing the molecular structure and bonding of NCl₃.
Step 2:: Determine the Lewis structure
- Nitrogen (N) is the central atom - Chlorine (Cl) atoms are terminal atoms - Total valence electrons: 5 (N) + 3 × 7 (Cl) = 26 electrons - The Lewis structure shows three single bonds between N and Cl atoms
Step 3:: Analyze bond polarity
- $$\Delta\chi = |3.16 - 3.04| = 0.12
- Electronegativity difference between N (3.04) and Cl (3.16) - The difference is small but significant - This indicates polar covalent bonds
Step 4:: Determine molecular geometry
- Central N atom has four electron domains (3 bonds + 1 lone pair) - Molecular geometry is trigonal pyramidal - Lone pair causes slight deviation from perfect tetrahedral geometry
Step 5:: Hybridization analysis
- Central N atom uses sp³ hybridization - Four electron domains (3 bonds + 1 lone pair) require sp³ orbitals
Final Answer
NCl₃ has polar bonds, a trigonal pyramidal molecular shape, and is sp³ hybridized.
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