The highest boiling point is demonstrated by A. $$ \mathrm{CO}_{2} $$ B. $$ \mathrm{CH}_{4} $$ C. $$ \mathrm{NH}_{3} $$ D. $$ \mathrm{H}_{2} \mathrm{O} $$

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1. Identify the types of intermolecular forces for each substance:
   - For $$ \mathrm{CO}_{2} $$ and $$ \mathrm{CH}_{4} $$, the molecules are nonpolar; thus, they experience only London dispersion forces.
   - For $$ \mathrm{NH}_{3} $$ and $$ \mathrm{H}_{2}\mathrm{O} $$, the molecules are polar and have the ability to form hydrogen bonds.
   
2. Recognize that hydrogen bonding is generally stronger than London dispersion forces and dipole-dipole interactions, leading to higher boiling points.

3. Compare $$ \mathrm{NH}_{3} $$ and $$ \mathrm{H}_{2}\mathrm{O} $$:
   - Although both can hydrogen bond, $$ \mathrm{H}_{2}\mathrm{O} $$ has a bent molecular structure that allows each molecule to form up to four hydrogen bonds (two as a hydrogen donor and two as an acceptor), resulting in a very strong hydrogen bonding network.
   - $$ \mathrm{NH}_{3} $$ can also hydrogen bond, but its hydrogen bonding network is less extensive than that of water.

4. Therefore, $$ \mathrm{H}_{2}\mathrm{O} $$ has the highest boiling point among the given substances.

The correct answer is $$ \mathrm{H}_{2}\mathrm{O} $$.
$$ \mathrm{H}_{2}\mathrm{O} $$ has the highest boiling point.

The highest boiling point is demonstrated
by
A.
B.
C.
D.

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