Answer
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Step 1:I'll solve this problem step by step, explaining why NH^3 (ammonia) is classified as a polar molecule:
Step 2:: Understand Molecular Structure
Ammonia (NH3) has a trigonal pyramidal molecular geometry. The central nitrogen atom is bonded to three hydrogen atoms, with one lone pair of electrons on the nitrogen.
Step 3:: Analyze Electronegativity
\text{Electronegativity difference} = 3.04 - 2.20 = 0.84
- Nitrogen has an electronegativity of 3.04 - Hydrogen has an electronegativity of 2.20
Step 4:: Examine Bond Polarity
Nitrogen, being more electronegative, pulls the electron density towards itself, creating a partial negative charge ($$\delta^{-}$$) on nitrogen and partial positive charges ($$\delta^{+}$$) on the hydrogen atoms.
The difference in electronegativity creates polar N-H bonds.
Step 5:: Consider Molecular Geometry
Due to the lone pair on nitrogen, the molecule is not symmetrically balanced. This asymmetry prevents the bond dipoles from canceling out.
Step 6:: Determine Net Dipole Moment
The unequal distribution of charge creates a net dipole moment, with the negative charge concentrated toward the nitrogen atom.
Final Answer
1. It has polar N-H bonds 2. Its trigonal pyramidal geometry is asymmetric 3. The lone pair on nitrogen creates an uneven charge distribution 4. These factors result in a net dipole moment, making NH^3 a polar molecule.
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