Question

When comparing H2, NH3, O2, and CH4, which of the following statements is correct?

a. CH4 has the highest boiling point because it experiences dipole-dipole forces.
b. H2 has the strongest intermolecular forces because it has the lowest mass.
c. NH3 has the highest boiling point because it experiences hydrogen bonding.
d. O2 has the strongest intermolecular force because it experiences London dispersion forces.

Answer 1

Answer:

c. NH3 has the highest boiling point because it experiences hydrogen bonding.

Explanation:

NH3 has three N-H polar covalent bonds with N and H having partial negative and positive charges respectively. The partial negative dipole of N from one NH3 molecule forms a hydrogen bond with the partial positive dipole of H from one NH3 molecule.  

δ- δ+   δ- δ+

N-H...N-H

Thus NH3 experiences hydrogen bonding and has the highest boiling point.  

The C-H bond in CH4 is nonpolar. Dipoles exist in polar covalent bonds. Hence option A is incorrect.  

Higher the molecular mass the greater is the intermocleuclar force of attraction. Hence option C is incorrect.  

London dispersion forces are weaker intermolecular forces than hydrogen bonding. Hence option D is incorrect.  

Answer 2

When comparing $H_2$, $NH_3$, $O_2$, and $CH_4$, the statement which is correct is: C. NH3 has the highest boiling point because it experiences hydrogen bonding.

A chemical bond refers to the forces of attraction that are existing between ions, crystals, atoms or molecules, and they are mainly responsible for the formation of chemical compounds.

Hence, a chemical bond is typically a force holding atoms together and binding ions, crystals, or molecules together, in order to form a chemical compound.

In Chemistry, there are three main types of chemical bonds and these include:

• Covalent bonds.

• Ionic bonds.

• Hydrogen bonds.

Hydrogen bond can be defined as a weak chemical bond existing between a partially positively charged hydrogen atom and an electronegative chemical atom.

Generally, a hydrogen bond has the strongest intermolecular force of attractions, but it is weaker than an ionic bond or covalent bond.

Since ammonia ($NH_3$) has a hydrogen bond, its boiling point would be very high, so as to break these strong intermolecular force of attractions between its atoms.

In conclusion,  $NH_3$ has the highest boiling point in comparison with $H_2$, $O_2$, and $CH_4$ because  it experiences hydrogen bonding.

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