Ice floats in water.
Ice is less dense than water. Ice
has a more open structure than water.
What in
the world does all that mean aside from making my summer beverage more
refreshing?
I’m
going to tell you. No! Wait.
I’m going to show you.
Let’s
start at Figure 24.4 from my Play Ball!
post (GO
PHILLIES!). It shows how atoms/molecules/ions (blue circles in the figure) line up in the
solid, liquid and gas phases. You’ll
notice that the atoms/molecules/ions are very close together in the solid
phase, move further apart in the liquid phase and are further apart still in
the gaseous phase. This is generally how close atoms in each phase
can be described. Key word: generally.
Now let’s discuss density.
Sure, we all learned the equation in third grade – mass divided my
volume – but what does that mean in real words?
Mass is directly related to the number of atoms/molecules/ions (also called particles) present. So, if you look at the same volume of a
solid, liquid or a gas, how many particles can you find there? Figure 69.1
shows that for a particular volume (orange square) the solid has 9 particles; the
liquid has 4 and the gas has 1. The solid’s
density is greatest (most amount of atoms/molecules/ions in the volume), the
gas’s density is least and liquid is in the middle. This means that if we had a cube of solid
nitrogen and a glass of liquid nitrogen (brr!) and we dropped the cube in the liquid,
the cube would sink to the bottom.
Why? Because the cube is MORE
dense than the liquid. Again, this is generally true for most substances.
When particles come together to form
a solid, many things need to be considered such as the size and charge of the
particles. The atoms/molecules/ions need
to align themselves as close together as possible in the solid form, but without
ticking each other off. For example, two
positive charges close together would be repulsive and unfavorable. How do particles deal with this balancing act?
To
explain this, I’m going to show you two examples: solid NaCl (table salt)
and solid water (ice).
NaCl: Solid NaCl
is ions of sodium and chloride all packed very closely together. A sodium ion is positively charged while a
chloride ion is negative charged.
Obviously two chlorides aren’t packing directly next to each other because
they both have the same charge. Instead,
the ions arrange themselves such that a chloride ion is surrounded by sodium
ions in a very ordered array. This way,
the negatively charged chlorides are pacified by the positively charged sodiums
enough such that the ions can pack close together (Figure
69.2).
Water: I’ve discussed water and its fun properties a
few times on this blog: Soap! and What Does Water Look Like? come to mind so
you should be familiar with what a molecule of water looks like and how parts
of it are positively and negative charged (Figure
69.3). Similar to NaCl, water
must not place two positive or negative charges too close together in the solid
form. Water’s shape, however, is quite
different than ions of Na+ and Cl- so its shape comes
into play when ordering itself in the solid phase. Figure 69.4
shows how water molecules line up when forming ice. Compare it to solid NaCl (Figure 69.2) and the generic example of solids I
showed in Figure 24.4. Do you notice the differences?
Water molecules adopt a very open conformation. Yes, the water molecules are close together,
but there’s a lot of room between the molecules, which is not true in
NaCl. This kind of arrangement minimizes
the steric and charge clashing of water molecules the most so it is the most
favorable way that water molecules can pack together. It is not air between those water molecules,
it is empty space (I discussed air
and its properties in my Play Ball! Post).
If we
now return the idea of Figure 69.2, but redraw the
solid phase so it more accurately represents water, we can see that liquid water,
not solid water, has the most molecules per volume.
As the ice is warmed to form water, the lovely ordered structure
falls apart. Instead of being
held in an array, the molecules fall into a disordered jumble which
results in more water molecules being present in a particular volume than would
be true for ice.
More water molecules in the same volume of space means a higher density
(Figure 69.5). Solid water is LESS dense than liquid water
and therefore floats in it.
Exceptions
exist for every rule and, in the case of decreasing density from solid to
liquid to gas, water is the exception.
Ions: Atoms that have
either more or less electrons than the number of protons in their nuclei.
Density: the measure of
how much mass is present per unit volume.
Less dense items float in more dense items.
Particles: an alternative
name for atoms, molecules, or ions
REFERENCES
Zumdahl, Steven S. “Chemical Principles, 4th Edition”
(2002) Houghton Mifflin Company, Boston, MA.