Question

Identify a hydride with highest boiling point from following?

• A. \(\text{H}_{2}\text{O}\)
• B. \(\text{H}_{2}\text{S}\)
• C. \(\text{H}_{2}\text{Se}\)
• D. \(\text{H}_{2}\text{Te}\)

Hint:

Water forms extensive hydrogen bonds, which the heavier group 16 hydrides cannot.

Answer 1

The Correct Option is A

Step 1: Understanding the Concept
Among group 16 hydrides, boiling point normally rises with molar mass because van der Waals forces increase.

Step 2: Anomaly of water
Oxygen is small and highly electronegative, so water molecules form strong intermolecular hydrogen bonds.

Step 3: Result
Because of hydrogen bonding, water boils at 373 K, far above \(\text{H}_{2}\text{S}\), \(\text{H}_{2}\text{Se}\) and \(\text{H}_{2}\text{Te}\).

Final Answer:
Water has the highest boiling point. \[ \boxed{\text{(A) }\text{H}_{2}\text{O}} \]