Did you know that the way water molecules interact with each other caused the sinking of the Titanic? And the unique chemical properties of this miracle liquid that cause icebergs to float also cause the surface of water to stick together with enough force that the Basilisk or “Jesus” lizard can walk on water.
Water, critical to our survival, behaves differently from any other substance on Earth. The unique chemical properties of water are presented in this module. The module explains how the dipole across the water molecule leads to hydrogen bonding, making water molecules act like little magnets. Also explored are surface tension and water’s properties as a solvent.
- bonding = the act of fastening two atoms together
- covalent = a type of bond that involves the sharing of electron pairs between atoms to achieve chemical stability, as in the hydrogen and oxygen atoms that make up a water molecule
- solvent = the substance present in the greatest amount within a solution
In many ways, water is a miracle liquid. It is essential for all living things (on this planet at least), and it is often referred to as a universal solvent because many substances dissolve in it. These unique properties of water result from the ways in which individual H2O molecules interact with each other.
In the Chemical Bonding lesson we discussed the dipole that forms across the water molecule as a result of the polar covalent bonding between hydrogen and oxygen (see our Chemical Bonding module for more information). Because the bonding electrons are shared unequally by the hydrogen and oxygen atoms, a partial negative charge (ð-) forms at the oxygen end of the water molecule, and a partial positive charge (ð+) forms at the hydrogen ends (Figure 1). Since the hydrogen and oxygen atoms in the molecule carry opposite (though partial) charges, nearby water molecules are attracted to each other like tiny little magnets. The electrostatic attraction between the ð+ hydrogen and the ð- oxygen in adjacent molecules is called hydrogen bonding (Figure 2).
Hydrogen bonding makes water molecules "stick" together. While hydrogen bonds are relatively weak compared to other types of bonds, they are strong enough to give water many unique properties. For example, hydrogen bonds sank the Titanic, and hydrogen bonds allow the Basilisk lizard to walk on water (as a result, the Basilisk has earned the nickname "Jesus" lizard).
Just how does hydrogen bonding do this? Well, let's start with the Titanic. The Titanic sank because it hit an iceberg – a chunk of ice floating on the surface of the ocean. The reason ice floats is because of hydrogen bonding. In water's liquid form, hydrogen bonding pulls water molecules together. As a result, liquid water has a relatively compact, dense structure. The animation below illustrates this idea.
Water molecules are attracted to each other because of
As we just discussed, neighboring water molecules are attracted to one another. Molecules at the surface of liquid water have fewer neighbors and, as a result, have a greater attraction to the few water molecules that are nearby. This enhanced attraction is called surface tension. It makes the surface of the liquid slightly more difficult to break through than the interior.
When a small object that would normally sink in water is placed carefully on the surface, it can remain suspended on the surface due to surface tension. The Basilisk lizard makes use of the high surface tension of water to accomplish the incredible feat of walking on water's surface. The Basilisk can't actually walk on water; rather, it runs on water, moving its feet before they break through the surface. Take a look:
The "Jesus" Lizard (11M movie)
From the article: Minetti A, Ivanenko Y, Cappellini G, Dominici N, Lacquaniti F. "Humans Running in Place on Water at Simulated Reduced Gravity". PLOS ONE. DOI:10.1371/journal.pon
In liquid water, which molecules have a stronger attraction to each other?
Water as a solvent
The partial charge that develops across the water molecule helps make it an excellent solvent. Water dissolves many substances by surrounding charged particles and "pulling" them into solution. For example, common table salt, sodium chloride, is an ionic substance that contains alternating sodium and chlorine ions (see Figure 3).
When table salt is added to water, the partial charges on the water molecule are attracted to the Na+ and Cl- ions. The water molecules work their way into the crystal structure and between the individual ions, surrounding them and slowly dissolving the salt. The water molecules will actually line up differently depending on which ions are being pulled into solution. The negative oxygen ends of water molecules will surround the positive sodium ions; the positive hydrogen ends will surround the negative chlorine ions, as shown in Figure 4.
In a similar fashion, any substance that carries a net electrical charge, including both ionic compounds and polar covalent molecules (those that have a dipole), can dissolve in water. This idea also explains why some substances do not dissolve in water. Oil, for example, is a nonpolar molecule. Because there is no net electrical charge across an oil molecule, it is not attracted to water molecules and therefore does not dissolve in water.