Step 1: Understanding the Concept:
Hydrogen bonding is a strong dipole-dipole attraction that occurs when hydrogen is covalently bonded to highly electronegative atoms (N, O, or F). The extent of hydrogen bonding depends on the number of hydrogen atoms available and the number of lone pairs on the electronegative atom.
Step 2: Key Formula or Approach:
- \(\text{H}_2\text{O}\) has 2 hydrogen atoms and 2 lone pairs on the oxygen atom, allowing each molecule to participate in a 3D network of 4 hydrogen bonds.
- \(\text{HF}\) has only 1 hydrogen atom per molecule, limiting the network.
- \(\text{NH}_3\) has only 1 lone pair on nitrogen, which limits its ability to form extensive bonding networks compared to oxygen.
- \(\text{CH}_3\text{OH}\) has a large organic group that hinders the formation of a highly dense H-bonding network.
Step 3: Detailed Explanation:
Water (\(\text{H}_2\text{O}\)) is unique because it can act as both a double hydrogen-bond donor and a double hydrogen-bond acceptor. This leads to the formation of a highly extensive, three-dimensional tetrahedral hydrogen-bonded network in the liquid state, resulting in its unusually high boiling point and density properties compared to the other choices.
Step 4: Final Answer:
\(\text{H}_2\text{O}\) exhibits the maximum degree of hydrogen bonding.