Sure, let's analyze the molecule of ammonia ([tex]\(\text{NH}_3\)[/tex]) in detail based on its properties.
### Step-by-Step Solution:
1. Electronegativity of Nitrogen and Hydrogen:
- The electronegativity of Nitrogen ([tex]\(N\)[/tex]) is [tex]\(3.04\)[/tex].
- The electronegativity of Hydrogen ([tex]\(H\)[/tex]) is [tex]\(2.20\)[/tex].
2. Bond Polarity:
- Bond polarity is determined by the difference in electronegativities between the two atoms in a bond.
- For the Nitrogen-Hydrogen ([tex]\(N-H\)[/tex]) bond:
[tex]\[
\text{Bond Polarity} = 3.04 - 2.20 = 0.84
\][/tex]
3. Molecular Shape:
- The molecular shape of [tex]\(\text{NH}_3\)[/tex] is determined by its Lewis structure, which reveals that the nitrogen atom is bonded to three hydrogen atoms and has one lone pair of electrons.
- This arrangement leads to a trigonal pyramidal geometry to minimize repulsion between electron pairs as predicted by the VSEPR (Valence Shell Electron Pair Repulsion) theory.
4. Molecule Polarity:
- A molecule is polar if it has a net dipole moment, which depends on both the bond polarity and the geometry of the molecule.
- The [tex]\(\text{NH}_3\)[/tex] molecule, with its trigonal pyramidal shape, has a net dipole moment due to the lone pair pushing the N-H bonds slightly downward, creating an overall dipole pointing towards the lone pair of electrons.
- Therefore, [tex]\(\text{NH}_3\)[/tex] is a polar molecule.
### Final Characteristics:
- The bond polarities are [tex]\(0.84\)[/tex].
- The molecular shape is trigonal pyramidal.
- The molecule is polar.
By assembling these detailed analyses, we can describe the characteristics of an ammonia ([tex]\(\text{NH}_3\)[/tex]) molecule comprehensively.
