Describe hydrogen bonding as it occurs in water in terms of the location of the bond, the particles involved, the strength of the bond, and the effects this type of bonding has on physical properties.

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Hydrogen bonding in water occurs between the hydrogen atom of one water molecule and the oxygen atom of a neighboring water molecule. The hydrogen bond forms as a result of the partially positive charge on the hydrogen atom and the partially negative charge on the oxygen atom. This unequal sharing of electron density creates a dipole-dipole interaction.

The strength of the hydrogen bond is relatively weaker than a covalent or ionic bond but stronger than van der Waals forces. It is around 5-10% the strength of a covalent bond.

The effects of hydrogen bonding on the physical properties of water are significant. For instance:

1. High boiling point: Hydrogen bonding causes water to have a higher boiling point compared to other substances of similar molecular weight. This is due to the extra energy needed to break the hydrogen bonds between water molecules.

2. Cohesion and surface tension: Hydrogen bonding gives water strong cohesive properties, meaning water molecules tend to stick together. This cohesion results in high surface tension, allowing certain insects, like water striders, to walk on the water surface.

3. Density anomalies: Unlike most compounds, water exhibits an unusual density anomaly. As the temperature decreases, water molecules form a crystalline lattice and lock into a hexagonal structure, causing an expansion of volume and a decrease in density. This is why ice floats on water, as it is less dense.

4. High specific heat capacity: Hydrogen bonding in water contributes to its high heat capacity, meaning it can absorb a large amount of heat energy without a significant change in temperature. This property helps to stabilize temperatures in aquatic environments and regulate the Earth's climate.

In summary, hydrogen bonding in water occurs between the hydrogen and oxygen atoms of neighboring water molecules. These bonds are relatively weaker than covalent bonds but stronger than van der Waals forces. They significantly influence water's physical properties, including its boiling point, cohesion, surface tension, density anomalies, and high specific heat capacity.