REVIEW STATIONS
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PERIODIC TABLE & TRENDS
THE ATOM & BOHR/LEWIS DIAGRAMS
MOLECULAR/IONIC COMPOUNDS
NAMING - IONIC COMPOUNDS
NAMING MOLECULAR COMPOUNDS
BALANCING
LAW OF CONSERVATION OF MASS
PHYSICAL AND CHEMICAL CHANGE
TYPES OF REACTIONS - GENERAL
ACIDS AND BASES
PUTTING IT ALL TOGETHER - PART 1
PUTTING IT ALL TOGETHER - PART 2
PUTTING IT ALL TOGETHER - PART 3
STATION 1 - THE PERIODIC TABLE & TRENDS
Use the periodic tables provided to answer the
questions on your review handout.
STATION 2 - THE ATOM & BOHR & LEWIS
DIAGRAMS
1. Name the three sub-atomic particles of the atom. What charges do
they have?
2. What is meant by "valence electrons"?
3. Draw either a Bohr OR Lewis diagram for the following elements/ions
(note - Lewis diagram shows only the outermost shell, with valence
electrons only as opposed to Bohr diagrams which shows all the
shells, including the valence electrons)
a. Silicon atom
b.Magnesium ion
STATION 3 - MOLECULAR AND IONIC COMPOUNDS
1. What does "ion" mean? What does it mean if you see Al3+ or S2−?
2. How do you know if a compound is ionic or molecular?
3. Using NaF and CO2 as examples, draw either Bohr or Lewis
diagrams to show how their bonds are formed. What is the difference?
4. Why does magnesium chloride (MgCl2) have a weaker smell
compared to candle wax (C25H52)?
STATION 4 - NAMING IONIC COMPOUNDS
1. Complete the following chart by writing the correct chemical formula
or name in the space. Use the periodic tables provided. Remember to
take note of multivalent metals and polyatomic ions!
FORMULA
NAME
K2S
magnesium phosphide
tin(IV) oxide
CaCO3
copper(II) bicarbonate
Note: A periodic table will be provided to you on test day, including a
polyatomic ion chart as well as ionic charges for the elements. But no
names will be given on the periodic table. You are responsible for
knowing the names/symbols of the 40 elements that were discussed!
STATION 5 - NAMING MOLECULAR COMPOUNDS
1. Complete the following chart by writing the correct chemical formula
or name in the space. Use the periodic tables provided.
FORMULA
NAME
SO3
triphosphorus hexachloride
carbon monoxide
P2O5
dinitrogen tetroxide
Note: A periodic table will be provided to you on test day, including a
polyatomic ion chart as well as ionic charges for the elements. But no
names will be given on the periodic table. You are responsible for
knowing the names/symbols of the 40 elements that were discussed!
STATION 6 - BALANCING CHEMICAL EQUATIONS
Balance the 5 skeleton equations on your review
handout. Always double check your work by counting
the number of atoms of each element on both sides of
the arrow! Remember, do not put 1 as a coefficient!
STATION 7 - LAW OF CONSERVATION OF MASS
Is the Law of Conservation of Mass applicable to the following
scenarios? Justify your answers.
1. The mass of a rusty bicycle is found to be slightly greater than the
mass of the same bicycle before it rusted.
2. 0.51 g of aqueous solution of copper(II) chloride and 0.62 g of
sodium hydroxide were mixed in a test tube with a stopper. After the
reaction, the products were weighed to be a total of 1.10 g.
STATION 8 - PHYSICAL AND CHEMICAL CHANGE
Read the following scenarios. Identify whether a physical and/or
chemical change has occurred and how you know.
1. A student adds a piece of magnesium metal to a solution of sulphuric
acid (H2SO4). The test tube fizzes and is warmer at its base. The
student also puts a flaming split inside the test tube and hears a pop
sound.
2. A scoop of copper(II) chloride powder, which is light blue, is added to
distilled water. The result is a translucent blue homogeneous solution.
3. Aluminum foil is added to a beaker containing a solution of copper(II)
sulphate and heated up. After 15 minutes, the solution turns darker
and there are reddish flakes floating in the solution and deposited on
some pieces of the foil.
STATION 9 - TYPES OF CHEMICAL REACTIONS
1. Consider the six reaction types discussed in class. All involve
elements and compounds. Identify the type(s) of reaction that has the
following reactant(s) or product(s):
Reactant(s)
Two elements
An element
and a
compound
Product(s)
Water and a salt
Two
compounds
Only one
compound
Carbon dioxide
and water
Type of Reaction
STATION 10 - ACIDS AND BASES
1. Classify the compound as an ACID or a BASE or BOTH based on the
following properties:
a) pH = 4.0
d) litmus paper stays red
g) contain hydrogen ions
j) electrolyte in solution
(conducts electricity)
m) turns blue with
bromothymol blue (BTB)
b) reacts with carbonates
to produce CO2 gas
e) unreactive with metals
h) reacts with metals to
produce H2 gas
k) corrosive
c) slippery texture
n) sour tasting
o) phenolphthalein turns
pink
f) pH = 13.0
i) bitter tasting
l) contain hydroxide ions
2. Name or write the formulas for the following acids and bases:
a) HF
HNO2
b) magnesium hydroxide
hydroiodic acid
3. A scientist walked into a lab and discovered a clear puddle on the floor.
Taking precautions, he discovers from his analysis using different pH
indicators and equipment:
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Bromothymol blue: BLUE
Universal pH indicator paper: 11.0
Cabbage Juice: TURQUOISE
Electronic pH meter (see image): 11.4
a)What is meant by "pH"?
b)Is the chemical in the puddle acidic, basic or neutral?
c) How can he safely clean the spill up? What type of reaction is this?
STATION 11 – PUTTING IT ALL TOGETHER
PART 1
A student wishes to see the reaction between an aqueous solution of
phosphoric acid and an aqueous solution of magnesium hydroxide. One
of the products will be a solid compound that contains magnesium ions
as part of it.
a)Write a balanced chemical equation for this chemical reaction and
predict its products. Include the states of matter notations.
b)Classify this type of reaction.
STATION 12 - PUTTING IT ALL TOGETHER
PART 2
When a copper wire is placed in an aqueous solution of silver nitrate, a
solid layer appears on the copper wire and the solution turns blue due to
the Cu2+ ions and there are solids flaking off into the solution.
a)Write a balanced chemical equation for this chemical reaction and
predict its products. Include the states of matter notations.
b)Classify this type of reaction.
c) How do you know that a chemical change has occurred?
STATION 13 - PUTTING IT ALL TOGETHER
PART 3
A scientist reacts an aqueous solution of cobalt(II) chloride and an
aqueous solution of sodium carbonate. Only one of the products that
formed in this reaction will be a solid (see image) and it is a pink solid
that is due to the Co2+ ions present in the compound.
a)Write a balanced chemical equation for this chemical reaction and
predict its products. Include the states of matter notations.
b)Classify this type of reaction.