Look up and compare the normal boiling points and normal melting points of H2O and H2S. Based on these physical properties, which substance has stronger intermolecular forces? What kinds of intermolecular forces exist for each molecule?

Verified step by step guidance

Step 1: Identify the normal boiling and melting points of H2O and H2S. H2O has a boiling point of 100°C and a melting point of 0°C, while H2S has a boiling point of -60°C and a melting point of -85°C.

Step 2: Compare the boiling and melting points of H2O and H2S. Notice that H2O has significantly higher boiling and melting points than H2S.

Step 3: Determine the types of intermolecular forces present in each molecule. H2O exhibits hydrogen bonding, dipole-dipole interactions, and London dispersion forces. H2S primarily exhibits dipole-dipole interactions and London dispersion forces.

Step 4: Analyze the strength of intermolecular forces based on boiling and melting points. Higher boiling and melting points in H2O suggest stronger intermolecular forces compared to H2S.

Step 5: Conclude that H2O has stronger intermolecular forces due to the presence of hydrogen bonding, which is absent in H2S, leading to higher boiling and melting points.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Intermolecular Forces

Intermolecular forces are the attractive forces between molecules that influence their physical properties, such as boiling and melting points. The main types include hydrogen bonding, dipole-dipole interactions, and London dispersion forces. Stronger intermolecular forces typically result in higher boiling and melting points, as more energy is required to overcome these attractions.

Hydrogen Bonding

Hydrogen bonding is a specific type of strong dipole-dipole interaction that occurs when hydrogen is bonded to highly electronegative atoms like oxygen, nitrogen, or fluorine. In the case of water (H2O), hydrogen bonds significantly increase its boiling and melting points compared to substances that do not exhibit hydrogen bonding, such as hydrogen sulfide (H2S), which primarily experiences weaker dipole-dipole interactions.

Boiling and Melting Points

Boiling and melting points are physical properties that indicate the temperatures at which a substance transitions between solid, liquid, and gas phases. These points are influenced by the strength of intermolecular forces; substances with stronger forces will have higher boiling and melting points. Comparing the boiling and melting points of H2O and H2S reveals insights into the relative strength of their intermolecular forces.

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