Answer:
[tex]\boxed{\text{c) NH$_{3}$; hydrogen bonding}}[/tex]
Explanation:
For each of these molecules, you must determine their VSEPR structure and then identify the strongest intermolecular forces.
Remember that water is a highly polar molecule.
a) CH₄
Electron geometry: tetrahedral
Molecular geometry: tetrahedral
Bond polarity: C-H bond nonpolar
Molecular polarity: nonpolar
Strongest IMF: London dispersion forces
Solubility in water: low
A nonpolar molecule is insoluble in a polar solvent.
b) CCl₄
Electron geometry: tetrahedral
Molecular geometry: tetrahedral
Bond polarity: C-Cl bond nonpolar
Molecular polarity: nonpolar (symmetrical molecule. All bond dipoles cancel)
Strongest IMF: London dispersion forces
Solubility in water: low
A nonpolar molecule is insoluble in a polar solvent.
d) PH₃
Electron geometry: tetrahedral
Molecular geometry: trigonal pyramidal
Bond polarity: P-H bonds are polar
Molecular polarity: polar (all P-H bond dipoles point towards P)
Strongest IMF: dipole-dipole
Solubility in water: soluble
A polar molecule is soluble in a polar solvent.
c) NH₃
Electron geometry: tetrahedral
Molecular geometry: trigonal pyramidal
Bond polarity: N-H bonds are highly polar
Molecular polarity: highly polar (all N-H bond dipoles point towards N)
Strongest IMF: hydrogen bonding
Solubility in water: highly soluble
NH₃ is so polar that it can form hydrogen bonds with water.
[tex]\boxed{\textbf{The compound with the greatest solubility in water is NH$_{3}$}}[/tex]
