Chemistry

Question Analysis
This question involves distinguishing between bond polarity and molecular polarity by analyzing electronegativity differences and molecular geometry. The main focus is on understanding how symmetric geometry cancels bond dipoles.

Key Concept Explanation
A molecule with polar bonds can be nonpolar if its geometry is symmetric, causing bond dipoles to cancel each other out. Polar bonds form when ΔEN > 0; molecular polarity depends on both bond polarity and shape.

Step-by-Step Solution
1. Identify bond polarity for each molecule (calculate ΔEN):
All options have polar bonds (ΔEN > 0 for H–O, N–H, C–O, H–Cl)
2. Analyze molecular geometry:
A. H₂O: Bent geometry → dipoles do not cancel → polar molecule
B. NH₃: Trigonal pyramidal → dipoles do not cancel → polar molecule
C. CO...