STATION 1
Label bond type as metallic, ionic, covalent, or both:
1. NH3
2. NH4Cl
3. SeH2
4. NaBr
5. Fe
6. MgI
7. CO2
8. HBr
9. CaCO3
10. H2O
11. Mg(NO3)2
12. Cu
Station 2
Label bond type as metallic ionic, covalent, or both:
1. good conductor of electricity
2. usually a gas/liquid
3. high melting point
4. brittle
5. conducts electricity in the aqueous or liquid phases, only
6. dissolves in polar solvents
7. dissolves in nonpolar solvents
8. malleable/ductile
9. usually a solid
10. electrons are shared to complete valence shell
11. electrons are transferred to complete valance shell
12. electrons move freely around the atoms of the element
13. can never conduct electricity
STATION 3
a. Label as metallic, ionic, or covalent
b. Explain conductivity for each: when would they
conduct and WHY?
1.
2.
3.
STATION 4
Label the following MOLECULES (not bonds) as polar or nonpolar, and
state the IMF associated with it.
1. HCl
2. H2
3. H2O
4. CO2
5. CCl4
6. CCl3H
STATION 5
1. Atoms become ________________ stable since bonding
______________ energy. This is known as an ________________
process.
2. Upon bonding, the valence shell will usually have ____ electrons.
One exception is hydrogen which will have ______ valence electrons
after bonding to other atoms.
3. Ionic bonds_____________ electrons from the ____________ to
the ________________ atom. Covalent bonds ____________
electrons between two _______________ atoms.
4. Polar bonds share electrons _________________. This is because
there is a difference in ________________________. The atom
with a _______________ electronegativity will pull the electrons
___________, giving it a partially _______________ charge. The
less electronegative atom will then have a partially _______________
charge.
STATION 6
Match the following substances to the properties described below
(read the entire passage to get the most out of this station!):
a. CaBr2
b. CO2
c. Cu
d. MgO
e. F2
1. It has the weakest of the three bond types and therefore is
brittle and has a low melting point. It cannot conduct electricity no
matter the phase because it can never have mobile charges. It can
only occur as a solid under very high pressure. This substance is also
known as a molecule.
2. This substance is a solid and has a very high melting and
boiling point. It can conduct electricity in any phase since the valence
electrons are free to move around the nuclei of the element’s atoms.
It can be hammered into sheets (malleable) or spread into wires
(ductile).
3. This substance is very hard and has a high melting point. It
exists in a crystal lattice structure. It is referred to as a salt. This
substance can conduct electricity, but only if it is melted or if it is
dissolved in water.
4. Draw the Lewis dot structures for F2 and MgO