Lab 4-A: Properties of Substances
Chemistry 12, McGraw Hill pg 164
1. Complete observation table (make sure to have a table title)
2. Identify the type of bonding each substance has (in another
3. Pick one substance (different than you lab partner’s).
Describe in detail how its structure determines the properties
Aluminium is a metallic solid making it hard, conductive and giving
it a high melting point. It also is not soluble in water.
Aluminium is a metallic solid, which means the metal cations are
arranged in a crystal lattice, held together by free electrons in the
empty spaces (electron sea). Because of the full charges, the
particles are strongly attracted to each other. This explains why Al
is a hard substance and has a high melting point. As seen in our
results, Al was the second highest in terms of hardness and did
not melt using the candle or Bunsen burner. Al is conductive as a
solid because its electrons are allowed to move from one place to
another creating a current. Al does not dissolve in water because
the Al3+ ions are more attracted to the free electrons than they are
to water because of the electron’s full one minus charges.