States of Water: Gas, Liquid and Solid

States of Water

Because water is extremely versatile, it can change states from a gas, liquid and solid. For example, when water is in a liquid state, it can evaporate into a gas or freeze into a solid.

If water is in a frozen state then you add heat, it melts and turns into a liquid again. When water vapor in the air condenses, it turns back into a liquid such as in the form of rain.

Finally, sublimation and deposition occur when water immediately turns into a gas or solid. This means that it skips the liquid phase going from solid to gas or vice versa.

Water transfers into phases with weak bonds continuously. So let’s talk about some of the amazing properties of water that makes this all happen.

The unique properties of water

Water H2O Molecule Partial Polarity

Water molecules are made of two hydrogen atoms and one oxygen atom. Thus, the chemical symbol for water is H2O.

But what’s important to know about water is that they are not symmetrical. Both the hydrogen atoms hang off the oxygen atom at angle.

Because of water has a positive side and a negative polar side, this is why H2O can dissolve other minerals. When it dissolves something, it makes it a solution.

Liquid water forms weak bonds with other atoms. It transfers into other phases with weak bonds continuously.

Evaporation: From liquid water to vapor

Hydrological Water Cycle

If you add enough energy from the sun, water evaporates into a gas from a liquid. In other words, it breaks the covalent bond of water.

When it evaporates, it isolates an individual molecule which flies off the surface as vapor. Because the water molecules absorb energy from heat, these energetic molecules stay farther apart from each other.

It takes a tremendous amount of energy to turn a liquid into a gas. For example, it requires 540 calories per gram for evaporation to occur. This is good because we don’t want all water on Earth to evaporate too rapidly.

71% of Earth is water so evaporation happens everywhere. But it happens most rapidly at the equator because it receives the most sunlight.

But in average, water resides in the atmosphere for only a short period of time. In fact, it spends less than a day in the atmosphere where it condenses and precipitates.

Condensation: From water vapor to liquid

States of Water

Condensation is essentially the opposite of evaporation. Instead of gaining heat, water molecules lose energy from a loss of heat during condensation. In turn, they bond together from a gas into a liquid state.

Condensation is the process of forming tiny water droplets. They surrounding a particle of dust or salt. Eventually, they become too heavy and fall as precipitation.

For example, liquid water drips down a chilled glass of lemonade on a hot day because of condensation. When the water vapor in the air comes in contact with the cold glass, it slows down the water molecules making them stick together and form a liquid.

Overall, the start of the hydrological cycle begins with evaporation at the surface of the ocean. Next, water condenses and precipitates back into the ocean, streams, glaciers or as groundwater. Eventually, it makes its way back to the ocean. And that’s the whole cycle.

Freezing, melting, deposition and sublimation

When temperature is lowered below its freezing point, water can freeze. When water freezes, it expands. In lakes and streams, the frozen ice is more buoyant and remains at the top. This unique property of water is important for life and the biosphere.

Melting is essentially the opposite of freezing. When temperature is increased to its melting point, water can melt. This is important to understand for the consequences of global warming. For example, if all glaciers melted right now, sea levels would rise about 30 meters.

Finally, the last two phases are deposition and sublimation which are complete opposites of each other. Sublimation is when a solid changes state to a gas, without going into the intermediate liquid phase. Whereas deposition is when a gas transforms into a solid state.


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