This NBC Learn video explains how the molecular structure of H2O changes as it reaches its freezing point, and turns from a liquid to a less dense solid crystal lattice.
Chemistry of Ice
BETH NISSEN, reporting:
A riddle to start things off. What never gets tired, no matter how long it runs? Water! H20. One of the great riddles in chemistry and the natural world. It’s the only natural substance on Earth found in all three common states of matter: liquid, gas or vapor, and solid (ice). Which is another riddle. Unlike ice, almost all other substances behave like steel. When in liquid form, like molten steel, they’re less dense than when in solid form. As steel changes from liquid, cooling into a solid (say a steel beam) it condenses, concentrates, gets more compact.
JON WILKER (Chemist, Purdue University): Atoms come in closer to each other, and overall the material becomes more dense, becomes more heavy for a given volume.
NISSEN: Drop the steel beam into the molten steel, and it will sink. But drop a piece of solid water, ice, into liquid water and whether it’s ice cubes in your water glass or icebergs in the Arctic, it floats. In solid form, H20 is less dense, lighter than the same amount of H20 in liquid form. Because as you’re about to see, when water freezes, it doesn’t contract, it expands. To puzzle out the riddle of ice, look at the H20 molecule itself: two smaller atoms of hydrogen, bonded to one larger atom of oxygen. H20 is a polar molecule, the same way our planet has two opposite poles, the H20 molecule has two polar opposite sides. One side has a slight positive charge, the other a slight negative charge. You’ve probably heard that opposites attract, so the slightly positive hydrogen side of every H20 molecule is going to attract, and be attracted to, all the slightly negative oxygen sides of other H20 molecules in all directions. These bonds, called hydrogen bonds, are what hold water together. And as you know, water flows easily. In liquid state, the H20 molecules are making and breaking those bonds constantly. Imagine massive numbers of H20 molecules in a hot dance club, dancing so closely and wildly that they’re constantly making and breaking contact with each other.
WILKER: There is a lot of motion, there is a lot of energy, and they are not able to lock on to each other very well.
NISSEN: But watch what happens if the temperature drops. The energy level does, too. The H20 molecules move more slowly, space further apart, as if at arm’s length. This is the water expanding as it freezes, which is at 0 degrees Celsius, or at 32 degrees Fahrenheit. That’s water’s freezing point, the temperature at which liquid water becomes solid water, ice. As the mass of H20 stops “slam-dancing” and starts doing more of a molecular “minuet,” the water molecules are able to make longer-lasting connections, hydrogen bonds, with each other. The molecules freeze in place, “arms,” locked, in six sided, or hexagonal, groups that connect to form a 3-D network called a crystal lattice.
WILKER: Chemists will sometimes work weeks and months and years to get a single crystal of their compound or maybe a protein. And then, you go by a frozen puddle and you can see one crystal of ice that might be two feet long and it’s just amazing.
NISSEN: This crystal lattice structure explains why H20 is less dense in solid than in liquid form. This is called water’s density anomaly, by the way.
WILKER: As you lock one water molecule to the next and the next and the next, you build up this network that actually has a lot of empty space.
NISSEN: All that empty space means there are far fewer H20 molecules in, say, a cup of ice than in a cup of water. Fewer molecules means it’s less dense, which is why ice floats. But ice is no lightweight when it comes to strength. The Titanic only brushed past an iceberg on its fateful voyage in 1912, but that was enough to open fatal slits in the ship’s steel hull. Water as it freezes expands with enough force to crack rock, burst pipes. Cutting through layers of ice can require axes, chainsaws, 3,000 ton icebreakers. As much as researchers know about ice, there are still unsolved riddles about what really happens on the surface of water and ice, about ice on other planets, moons, and asteroids. Think of this story as just the tip of the floating mass of H20 in solid form.
They say that no two snowflakes are the same. That may be true, but snowflakes share some striking similarities. Take a look at these snowflakes:
Ice, Water, H2O Liquid, Solid, Density, Density Anomaly, Dense, Condense, Volume, Contract, Expand, Hydrogen, Oxygen, Polar, Polar Molecule, Charge, Electrical, Positive, Negative, Bonds, Hydrogen Bonds, Energy, Freezing Point, Crystal, Crystal Lattice, Hexagon, Hexagonal, Titanic, Ice-Breaker, Chemistry Now