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Water is a remarkable substance with several unusual properties that set it apart from many other liquids. These unusual characteristics are essential to support life as we know it. Hydrogen bonding plays an instrumental role in endowing water with these unique properties. For instance, consider water's ability to achieve high surface tension and a high specific heat capacity. Another intriguing property of water is its density anomaly when frozen into ice. Water also acts as an exceptional solvent for a wide variety of substances, which further emphasizes its uniqueness among liquids.

The high surface tension of water is mainly due to hydrogen bonding, which creates a strong 'skin' on the water's surface. Water molecules at the surface are pulled inwards by hydrogen bonds with other water molecules below. This inward pull makes the surface compact and resistant to external forces.

Because of this effect, water can form droplets on surfaces, and insects such as water striders can stand on water without sinking. This is why water can hold onto leaves, forming beautiful dew drops in the morning. Water's high surface tension is crucial for many biological processes, including transporting nutrients in plants and performing certain animal activities.

One of the most intriguing properties of water is its behavior upon freezing. Unlike most substances, water expands when it freezes due to the hydrogen bonds forming a lattice structure. In ice, each water molecule forms hydrogen bonds with others, resulting in a hexagonal lattice that takes up more space than when water is in its liquid state.

This structure makes ice less dense than liquid water, allowing it to float. This floating ice creates an insulating layer on bodies of water, protecting aquatic life during freezing temperatures. It is essential for maintaining ecosystems in cold environments by preventing bodies of water from freezing solid. This anomaly also affects global sea levels and climate systems.

Water is often referred to as the 'universal solvent' because of its remarkable ability to dissolve a wide range of substances. This ability stems from water's polar nature and its ability to form hydrogen bonds with various molecules. Water molecules can surround and interact with charged particles, such as ions, or other polar molecules, effectively dissolving them.

This property is vital for life on Earth as it allows water to carry nutrients, minerals, and gases, which are essential for biological processes in living organisms. In the human body, for example, blood utilizes water to transport oxygen, nutrients, and waste products to and from cells. Water's solvent properties also play a crucial role in Earth's climate and weather systems, by sustaining the water cycle and influencing both weather patterns and climate stability.