Answer
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Step 1:I'll solve this step by step, focusing on molecular structure and polarity.
Step 2:: Understand the molecular structure of ammonia
- Ammonia (NH₃) has a central nitrogen atom bonded to three hydrogen atoms - The molecular geometry is trigonal pyramidal - Nitrogen has one lone pair of electrons
Step 3:: Analyze the electronegativity differences
- The difference is significant ($$3.04 - 2.20 = 0.84$$)
- Nitrogen's electronegativity: 3.04 - Hydrogen's electronegativity: 2.20
Step 4:: Determine bond polarity
- N-H bonds are polar due to the electronegativity difference - Each N-H bond has a partial negative charge on nitrogen and partial positive charge on hydrogen
Step 5:: Evaluate molecular symmetry
- The lone pair on nitrogen creates an asymmetric electron distribution - This asymmetry prevents complete cancellation of bond dipoles
Step 6:: Conclude molecular polarity
- Unequal charge distribution - Net dipole moment exists - Bonds are polar and do not cancel out
Final Answer
Ammonia (NH₃) is a POLAR molecule.
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