Types of
Solids
·
Try some
practice worksheets
An overview of the different
types of solids, how they differ from each other, and where you can find them. Where appropriate, I’ve put
handy-dandy links to other parts of the site that might help you out.
What’s a solid? “Solid”
refers to the state of matter in which the particles are locked into place
without much freedom of movement. They
can be locked into crystal lattices or just kind of stuck together with
intermolecular forces so tightly that they can’t really move around. As we’ll see, it depends on the type of
solid we’re talking about. Solids
differ from liquids in that the particles in liquids, while still stuck together, do have some freedom of motion. Solids differ from gases in that gas
molecules really don’t interact with each other much, flying all over the
place. |
What are the different
types of solids? Ionic solids: Ionic solids are solids in which anions and
cations (negatively and positively charged atoms or groups of atoms,
respectively) stick together via “electrostatic attraction.” By “electrostatic attraction”, I basically mean
that the opposite charges just like to stick to each other. When they do this, they form great big
crystals in which each ion is surrounded by ions with the opposite charge. Such crystal lattices (as they’re called)
are really stable, requiring lots of energy (called the “lattice energy”) to
pull apart. Examples of ionic solids
include sodium chloride (table salt) and Epsom salts (magnesium sulfate
heptahydrate). For more info, click here. Metallic solids: Metallic solids are solids in which the
positively charged nuclei are held together by a bunch of valence electrons
that kind of bind the whole mess together.
These electrons are referred to as being “delocalized” because they
don’t stay between two atoms as they do in covalent bonds – instead, they
travel throughout the solid. This
allows the atoms in solids to move around, as the bonding electrons can move
around with them. A phrase commonly
used to describe metallic bonding is “electron sea theory”, which describes
the positive metal nuclei as floating around in an ocean of negative
electrons that hold them together.
Just about anything you know of that’s a metal does this kind of
bonding. Network atomic solids: Network atomic solids are great big
crystals in which all of the atoms are stuck together using covalent
bonds. Because the atoms are all
locked into place, these solids usually have properties very similar to that
of ionic compounds (high melting and boiling point, hard, brittle, and so
forth) with the exception that they don’t conduct electricity if you melt
them. Typically, gemstones (such as
amethyst, diamond, and ruby) are network atomic solids. Molecular solids: Molecular solids occur when covalent
molecules are held together by intermolecular forces. In this type of bonding, which occurs in
ice, the intermolecular forces between the molecules are strong enough to
keep the molecules locked into place.
Typically, these types of solids have much lower melting and boiling
points than metallic, network atomic, or ionic solids, because the
intermolecular forces holding the molecules together are much weaker than
those of the bonds in the other compounds.
My tutorial on covalent
compounds deals mostly with the properties and behavior of this type of
solid. Atomic solids: Atomic solids occur when noble gases are
cooled to really low temperatures and lock themselves in place using very
weak Amorphous solids: Amorphous solids, unlike the rest of these
solids, have no particular crystal structure.
In an amorphous solid, the particles are just kind of stuck all over
the place, with no regular bonding pattern.
Some amorphous solids are soft and rubbery (such as plastic and
rubber) because they consist of long molecules which are just kind of tangled
together and bound with intermolecular forces. Other molecular solids (called glassy
solids) are a lot more like network atomic solids because they consist of
atoms stuck together in an irregular fashion using covalent bonds. It won’t be much of a surprise to find that
glass is an example of such a solid! |
Questions? Comments?
Email them to me at misterguch@chemfiesta.com