Which of the following is the type of intermolecular force present between molecules of water (H_2O) in a beaker of water?

• A. London dispersion forces
• B. Hydrogen bonding
• C. Covalent bonding
• D. Ionic bonding

Answer: (B)

Verified step by step guidance

1. Identify the types of intermolecular forces that can exist between molecules: London dispersion forces, dipole-dipole interactions, hydrogen bonding, and ionic interactions.
2. Recognize that water (H\_2O) is a polar molecule with a bent shape, where the oxygen atom is more electronegative than hydrogen atoms, creating partial positive and negative charges.
3. Understand that hydrogen bonding occurs when hydrogen is covalently bonded to highly electronegative atoms like oxygen, nitrogen, or fluorine, and this hydrogen interacts with lone pairs on another electronegative atom.
4. Since water molecules have O-H bonds and lone pairs on oxygen, they can form hydrogen bonds with each other, which are stronger than London dispersion forces and dipole-dipole interactions.
5. Conclude that the dominant intermolecular force between water molecules in liquid water is hydrogen bonding, not covalent or ionic bonding, which are intramolecular or different types of interactions.