Which molecule has the highest boiling point, primarily due to hydrogen bonding between molecules?

• A. Methane, $C_1{H}_4$
• B. Water, $H_{2}O$
• C. Hydrogen sulfide, $H_{2}S$
• D. Carbon dioxide, $C{O}_2$

Answer: (B)

Verified step by step guidance

1. Identify the key factor affecting boiling points in the given molecules, which is hydrogen bonding. Hydrogen bonding occurs when hydrogen is directly bonded to highly electronegative atoms like nitrogen (N), oxygen (O), or fluorine (F).
2. Examine each molecule to determine if it can form hydrogen bonds: Methane (CH\_4) has hydrogen bonded to carbon, which is not electronegative enough for hydrogen bonding; Hydrogen sulfide (H\_2S) has hydrogen bonded to sulfur, which is less electronegative and less likely to form strong hydrogen bonds; Carbon dioxide (CO\_2) is a linear molecule with no hydrogen atoms, so it cannot form hydrogen bonds; Water (H\_2O) has hydrogen bonded to oxygen, a highly electronegative atom, allowing strong hydrogen bonding.
3. Understand that hydrogen bonding significantly increases intermolecular forces, which raises the boiling point because more energy is required to separate the molecules during the phase change from liquid to gas.
4. Compare the ability of each molecule to engage in hydrogen bonding and predict that water, with strong hydrogen bonding, will have the highest boiling point among the options.
5. Conclude that the molecule with the highest boiling point due to hydrogen bonding is water (H\_2O).