Chemistry, 29.06.2019 22:20, kodak0531

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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answered: skyler1muir

The correct answer is $NH_{3}$ .

Explanation:

The electron geometry of the $NH_{3}$ is tetrahedral and the molecular geometry is a trigonal pyramid.

The $NH_{3}$ 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, $NH_{3}$ has the greatest solubility.

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On the basis of molecular structure and bond polarity, which of the following compounds is most like

answered: kryoung08

$\boxed{\text{c) NH$_{3}$; hydrogen bonding}}$

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.

$\boxed{\textbf{The compound with the greatest solubility in water is NH$_{3}$}}$

answered: Guest

50.23 i believe is correct but don't quote me on that.

answered: Guest

Electrons are emitted

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On the basis of molecular structure and bond polarity, which of the following compounds is most like...