Which type of intermolecular force is primarily responsible for the high boiling point of water compared to other group 16 hydrides?

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

Answer: (B)

Verified step by step guidance

1. Identify the molecules being compared: water (H\_2O) and other group 16 hydrides such as H\_2S, H\_2Se, and H\_2Te.
2. Recall that boiling point is influenced by the strength of intermolecular forces; stronger forces require more energy (higher temperature) to break.
3. Recognize the types of intermolecular forces present: London dispersion forces (present in all molecules), dipole-dipole interactions (in polar molecules), and hydrogen bonding (a special, stronger type of dipole-dipole interaction).
4. Note that water has hydrogen atoms bonded directly to a highly electronegative atom (oxygen), which allows it to form hydrogen bonds, a much stronger intermolecular force than dipole-dipole or London dispersion forces.
5. Conclude that the primary reason for water's unusually high boiling point compared to other group 16 hydrides is the presence of hydrogen bonding.