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hayleyharding013
29.06.2019 •
Chemistry
On the basis of molecular structure and bond polarity, which of the following compounds is most likely to have the greatest solubility in water and why? a)ch4 b)ccl4 c)nh3 d)ph3
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Ответ:
The correct answer is
.
Explanation:
The electron geometry of the
is tetrahedral and the molecular geometry is a trigonal pyramid.
The
has the strongest intramolecular hydrogen bond, which makes them a highly polar molecule.
The polarity is directly proportional to the solubility of the compound in the water.
Therefore,
has the greatest solubility.
For more information, refer to the link:-
link
Ответ:
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.
Ответ:
c
Explanation: