SCH3U
Chapter 2 Test Review
This is not an extensive review of the concepts covered within the first chapter. Refer to the learning expectations
and the class wikispace for additional resources to assist you with your review.
1. Define the following terms, provide an example for each; See your notes and text
a.
single bond, double bond, triple bond
b.
polyatomic ion
c.
oxyacid
d.
octet rule
e.
empirical formula
2. Compare the following terms; (give a significant similarity, difference and examples for each term) See
your notes and text
a.
bonding pair and lone pair
b.
covalent bond and ionic bond
c.
non-polar covalent and polar covalent
d.
Lewis structure and structural formula
e.
hydrate and anhydrous salt
f.
London dispersion forces, dipole-dipole forces and hydrogen bonding
3. Use Lewis dot diagrams to predict the ratio of metal to non-metal ions in a compound formed by each pair
of elements. Give the chemical formula, and name the compound. See attached pdf
a.
magnesium and fluorine
b.
potassium and bromine
c.
rubidium and chlorine
d.
calcium and oxygen
4. Use Lewis dot diagrams to predict the ratio of metal to non-metal polyatomic ions in a compound formed
by each pair of elements. Give the chemical formula, and name the compound. See attached pdf
a.
sodium and hydroxide
b.
strontium and carbonate
5. Each of the following Lewis structures has an error in it.
State what the error is, and draw the correct Lewis structure. See attached pdf
A. The carbon attached to the oxygen has too many bonds.
B. Hydrogen has too many lone pairs.
C. Oxygen has too many lone pairs, carbon has too many
bonds.
6. Name each compound.
a.
MgCl
magnesium chloride
f.
Na2O
sodium oxide
b.
FeCl2
iron (II) chloride
g.
CuO
copper (II) oxide or cupric oxide
c.
Ba(ClO)2
barium chlorite
h.
NH4NO2
ammonium nitrite
d.
H2CrO4 (aq)
chromic acid
i.
H3PO4 (s)
hydrogen phosphate
e.
KOH
potassium hydroxide
j.
Cd(OH)2
cadmium hydroxide
7. Write the formula for each compound.
a. gold (III) chloride
AuCl3
g.
calcium oxide
CaO
b. lithium nitrite
LiNO2
h.
aqueous hydrogen sulfite
H2SO3 (aq)
c. calcium phosphide
Ca3P2
i.
sulphuric acid
H2SO4 (aq)
d. manganese (II) sulphide
MnS
j.
cobalt (II) hydroxide
Co(OH)2
e. magnesium oxide
MgO
k.
lithium hydroxide
LiOH
f. calcium hypochlorite
CaClO2
8. Name each compound
a. SO2 sulfur dioxide
d. Cl2O oxygen dichloride
b. N2O4 dinitrogen tetraoxide
c. CO carbon monoxide
e. C8H16 octene
9. Write the formula for each compound
a. dihydrogen monoxide H2O b. sulphur trioxide SO3
c. silicon tetrachloride SiCl4
d. methane CH4
10. Identify the errors in each phrase or statement, and rewrite it correctly.
a. four molecules of potassium bromide potassium bromide is ionic –compound not molecule
b. the compound NaHSO4 is sodium sulphate the compound is sodium hydrogen sulphate
c. the compound KNO2 is potassium nitrate the compound is potassium nitrite
11. Draw a structural formula based on the Lewis structure shown here. Explain, in detail, the relationship
between the two diagrams. See attached pdf
12. Determine whether or not the following molecules are polar or non-polar? See attached pdf
i. nitrogen triiodide
ii. sulfur dichloride
iii. carbon tetraiodide
iv. carbon dioxide
trigonal pyramidal -- polar
bent –polar
tetrahedral –non-polar
linear –non-polar
To determine this;
a) Show the electron tally for each molecule. Draw the Lewis Structure.
b) Show the structural formula, and name the shape of each compound.
c) Calculate the E.N.D. for each bond, add δ −and δ + symbols onto the structures if necessary.
d) Indicate with an arrow any net dipole in the molecule and then state whether each molecule is polar
or non-polar.
13. The melting points of three compounds are listed below. Predict the type of attractive forces between the
particles of each compound when the compound is in its solid form.
Compound
Scandium oxide
Nitrogen trichloride
Ethane
Melting Point (0C)
2489
-40
-182.79
Scandium oxide has strong ionic forces, thus in its solid form it will take a lot of energy to break apart the
crystal lattice structure.
Nitrogen trichloride is a polar molecule with dipole-dipole forces between molecules, making it a little
easier to create separation between molecules. There will also be the weaker VDW forces present between
molecules.
Ethane is normally a gas, and a non-polar molecule. London dispersion (VDW) forces are present between
molecules.
14. A classmate asks, “How could there possibly be any intermolecular forces between non-polar compounds?”
Answer your classmate’s question using a diagram to support your explanation.
Include discussion on instantaneous dipoles or induced dipoles within a non-polar
molecule.

Because electrons are moving around in atoms there will be instants when the
charge around an atom is not symmetrical. Resulting in an attraction between the nuclei
of one compound and the electrons of another compound.

May also be an attraction between temporary dipoles formed by the continuous
movement of electrons
E.g. Instantaneous dipoles :
Eventually electrons are situated so that tiny dipoles form
Induced Dipoles :
A dipole forms in one atom or molecule, inducing a
dipole in the other molecule
15. List the following compounds in the order of their boiling points, from lowest to highest without knowing
any exact boiling points. Explain your reasoning for your order, based upon the structures given.
Lowest chlorine gas –non-polar molecule,
VDW or London dispersion forces between
molecules.
Middle methanol –polar molecule due to the
O-H bond at one end. Hydrogen bonding will
exist between molecules, thus increasing the
energy demand for boiling point.
Highest potassium oxide –strong ionic forces
Textbook review: pg. 103-104 #1-21
Excellent review