Which of the following intermolecular forces are most significant in determining the physical properties of water (H2O)?

• A. Hydrogen bonding
• B. Ionic bonding
• C. London dispersion forces only
• D. Dipole-dipole interactions only

Answer: (A)

Verified step by step guidance

1. Identify the types of intermolecular forces present in water (H\_2O). Water is a polar molecule with a bent shape, which means it has a permanent dipole moment.
2. Recall that water molecules can form hydrogen bonds because the hydrogen atoms are bonded to a highly electronegative atom (oxygen), and there are lone pairs on the oxygen atom.
3. Understand that hydrogen bonding is a special, strong type of dipole-dipole interaction that occurs when hydrogen is bonded to N, O, or F, making it stronger than regular dipole-dipole forces.
4. Compare hydrogen bonding to other intermolecular forces: London dispersion forces are present in all molecules but are weaker, and ionic bonding is not relevant here because water is a molecular compound, not ionic.
5. Conclude that hydrogen bonding is the most significant intermolecular force affecting water's physical properties such as its high boiling point, surface tension, and heat capacity.