Water molecules form bonds through a specific type of intermolecular attraction called hydrogen bonding.
Understanding Hydrogen Bonds in Water
The bonding between water molecules isn't about atoms sharing electrons directly, but about the attraction between molecules due to differences in electrical charge.
How Hydrogen Bonds Develop
- Polarity of Water: Water molecules are polar, meaning they have a slightly negative charge on the oxygen atom and a slightly positive charge on the hydrogen atoms. This charge difference arises from the unequal sharing of electrons between oxygen and hydrogen.
- Attraction: The slightly positive hydrogen atom of one water molecule is attracted to the slightly negative oxygen atom of a neighboring water molecule.
- Hydrogen Bond Formation: This attraction forms a hydrogen bond. It’s a weak bond compared to the covalent bonds within the water molecule itself (between the oxygen and hydrogen atoms), but it's strong enough to hold water molecules together.
Key Aspects of Hydrogen Bonds in Water
| Aspect | Description |
|---|---|
| Type of Bond | Intermolecular attraction (between molecules) |
| Mechanism | Attraction between a slightly positive hydrogen and a slightly negative oxygen |
| Strength | Weaker than covalent bonds, but significant in water's properties |
| Location | Occurs between neighboring water molecules |
Effects of Hydrogen Bonds
The hydrogen bonds between water molecules give water some of its special properties, including:
- High boiling point: More energy is needed to overcome hydrogen bonds.
- Surface tension: Water molecules are strongly attracted to each other at the surface.
- Capillary action: Water can move up narrow tubes because of these bonds.
In short, hydrogen bonds form between neighboring hydrogen and oxygen atoms of adjacent water molecules, as the reference notes. This attraction creates the bond between individual water molecules.
