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Science 9
1.
Chemistry Review Worksheet 2o11
Define the following terms:
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
k.
WHMIS
Matter
mixture
heterogenous mixture
suspension
colloids
homogeneous mixture
pure substance
elements
physical properties
chemical properties
l.
m.
n.
o.
p.
q.
r.
s.
t.
u.
v.
atomic mass
mass number
atomic number
compound
ionic compound
molecular compound
ion and ion charge
chemical reaction
exothermic reaction
endothermic reaction
law of conservation of mass
2.
What is the difference between physical and chemical properties?
3.
Complete a chart, like the one below, indicating the atomic theories of the following scientists.
Scientist
Theory
Diagram
Dalton
JJ Thomson
Nagaoka
Bohr
Rutherford
4.
On a Periodic Table, where would you find the following:
a.
metals and non-metals
b.
families and periods
c.
alkali metals, alkali-earth metals, halogens, and noble gases
5.
Diagram an atom of oxygen according to Bohr, and label all the subatomic particles.
6.
Explain the term ion and explain how an ion gets an ionic charge.
7.
What is a polyatomic ion? (see p146)
8.
What are the properties of ionic compounds? (list 2 properties, and what ionic compounds are made of)
9.
Name the following ionic compounds:
a.
b.
c.
g.
LiCl (s)
Al2S3 (s)
AgF (s)
K2CO3 (s)
d.
e.
f.
Fe2O3 (s)
CuSO4 (s)
NaOH (s)
1
10.
Write the chemical formulas for the following ionic compounds:
a.
b.
c.
d.
sodium chloride
cesium bromide
calcium chloride
strontium sulfide
11.
What are the properties of molecular compounds?
12.
Name the following molecular compounds:
a.
b.
c.
d.
13.
e.
f.
g.
h.
sodium nitride
copper (II) chloride
lead (II) iodide
lithium phosphide
(2 properties and what elements they are made of.)
SiO2 (g)
OF2 (g)
CCl4 (g)
CH4 (g)
e.
f.
h.
C6H12O6 (s)
CO2 (g)
N2O5 (g)
S2F4 (g)
c.
d.
trinitrogen pentafluoride
oxygen dichloride
g.
Write the formulas for the following molecular compounds:
a.
b.
sulfur trioxide
diphosphorus tetraoxide
14.
What is a chemical reaction?
15.
What are the 4 evidences that a chemical reaction has occurred?
16.
What is the difference between chemical and physical changes?
17.
What is a chemical word equation?
18.
Re-write the following as chemical word equations:
a.
a solid piece of sodium metal is placed in water, and it reacts explosively to produce sodium
hydroxide and hydrogen gas
b.
hydrogen peroxide is placed in sunlight and reacts slowly to produce oxygen and water.
c.
iron (III) chloride is formed when iron and chlorine gas are mixed.
d.
when aluminium is exposed to oxygen, it forms aluminium oxide
19.
For reactions a), and c) above, write the chemical formula equation.
20.
How is a chemical formula equation different from a word equation?
21.
What are the two types of reactions that involve a gain or a release of energy? Explain each type.
22.
Define combustion and corrosion.
23.
What do the reactions in # 22 have in common?
24.
List the four factors that can affect reaction rates.
25.
Define catalyst and enzyme. What is the difference between the two.
26.
Explain how cutting up a piece of wood would increase the rate at which it burns.
2
27.
What is the Law of Conservation of Mass? Explain what it means in terms of chemical reactions.
28.
In the following examples, calculate the mass of the unknown product:
29.
a.
how much water is produced when a spark creates an explosion between 4 g of hydrogen and
32 g of oxygen?
b.
in a 100-g beaker, a student added 25 g of lead (II) nitrate to 15 g of sodium iodide.
In her notebook, the student recorded the final mass of the products, it was 140 g. Did this
reaction conserve mass? Explain your answer.
Write the chemical name of the following substances. Remember to use Roman Numerals where
necessary (hint – first figure out if it’s a molecular or ionic compound):
a.
b.
c.
MgBr2 (s)
Ba3N2 (s)
FeP (s)
d.
e.
30.
Explain how to calculate the number of neutrons in an atom.
31.
Complete the following chart:
Element
H
Atomic Number
Mass Number
Protons
PbI4 (s)
Cu2S (s)
Electrons
(assume a
neutral atom)
Neutrons
1
207
Ca
40
Ag
108
82
92
4
20
2
10
3