The Liquid State

How can water molecules in a gas state be moving slower than water molecules in a liquid state? Remember, the state that a molecule is in does not just depend on the speed of the molecule; it also depends on the strength of the attraction between molecules. If a molecule is by itself, it does not matter how slow it is moving… it will be in a gas state because the molecule will be moving freely.

When two water molecules come close together, they are attracted to each other just like magnets. The strength, or force, of the attraction depends on the distance between them. The two water molecules on the left in the simulation below are attracted to each other. Notice how they are constantly drawn toward each other when they are close together, but “ignore” each other when they are farther apart. On the other hand, the two water molecules on the right in the simulation are not attracted to each other at all. Notice how they move independently and do not interact, except when they bounce off of each other like hard spheres.

It is actually very difficult for two water molecules to enter a liquid state all by themselves. If the two water molecules on the left in the simulation above were not trapped in a small box together, chances are, they would eventually drift apart and never come close to each other again. The force of attraction between them would only be strong enough to hold them together if they were moving very, very, very, very slowly. Meanwhile, the two water molecules on the right will never enter a liquid state because they are not attracted to each other at all and will always move independently.

But if we pack more water molecules into the small box, we can see how the water molecules clump up together. The water molecules in the center of the clump are held together for a short period of time, while the water molecules on the edges of the clump are constantly breaking away and rejoining. These water molecules are not moving independently of each other. However, it is important to note that, even when molecules are strongly attracted to each other, this attraction does not slow them down… they continue moving and bouncing off of each other. This is because the water molecules still have kinetic energy, which means they are still moving. The only way for the water molecules to slow down is if they lose kinetic energy, which would mean cooling down the box and removing heat from the system.

Increasing the number of water molecules again and including the presence of gravity makes the simulation even more realistic. Now the water molecules are forming what almost looks like a water drop on top of a penny. Notice how the water molecules on the edge of the water drop are attracted by and pulled back toward the other water molecules in the center of the drop.

In order to simulate water molecules in a drop of water, we had to cheat a little bit by keeping the speed of the molecules extremely slow. Increasing the speed of the water molecules causes the water drop to break apart and the water molecules to enter something that looks much more like a gas state (the water molecules would certainly fly apart and enter a full gas state if they were not trapped in the box together).

So how does a drop of water stay together when the average speed of a water molecule at room temperature is approximately 590 m/s? Well, in real life, a drop of water does not consist of just 36 water molecules surrounded by a vacuum (empty space); it consists of over 1,000,000,000,000,000,000,000 water molecules surrounded by air.