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The boiling point of water is surprisingly high when compared to other small molecules like hydrogen sulfide (Hâ‚‚S). This is primarily due to the hydrogen bonds that exist between water molecules. When you heat water, energy is required to break these hydrogen bonds before the water molecules can transition into a gaseous state.
This is why water boils at 100°C, which is significantly higher than one might expect given its molecular weight.
Understanding this can help explain why water can remain a liquid over a wide temperature range, which is essential for life as we know it.

• Hydrogen bonds result in cohesive forces that increase water's boiling point.
• Boiling involves breaking these bonds so that molecules can enter the gas phase.

In comparison, substances with weaker intermolecular forces require less energy to convert to a gas, and therefore, have lower boiling points.

Water is known as the "universal solvent," but there are exceptions to its dissolving power, particularly when it comes to nonpolar substances. Water molecules are polar, meaning they have partial positive and negative charges. This allows them to easily interact with other polar molecules and ions. Nonpolar substances, however, have no charge that can interact with water's partial charges, which makes them hard to dissolve in water.
This principle is often remembered by the phrase "like dissolves like," meaning polar solvents best dissolve polar solutes, and nonpolar solvents dissolve nonpolar solutes.

• Water's polarity does not match with nonpolar substances like oil or fats.
• Due to their mismatched polarities, nonpolar substances cannot mix well with water.
• Hydrophobic interactions are typical of nonpolar substances, causing them to separate in water.

This characteristic of water has significant implications in many areas, including biology and environmental science, where the separation of molecules plays a critical role.

Surface tension is a fascinating property of water that you might have observed if you've ever seen a small insect like a water strider walking on its surface. This effect is a result of hydrogen bonding. Molecules at the surface of water form stronger bonds with each other than with the air, creating a "skin" effect.
This cohesion between molecules results in water having a higher surface tension than many other liquids.
The consequences of high surface tension are far-reaching, affecting everything from the formation of droplets to the ability of plants to draw water from their roots upward through a phenomenon known as capillary action.

• Hydrogen bonds pull water molecules close together at the surface.
• This creates a "film" that makes it difficult to break through the surface.
• Surface tension affects how liquids spread over surfaces and the ability of certain objects to float.

This property is critical in many natural processes and has practical implications in various technologies and industries.