Review for Final Exam
Unit 2
REVIEW: Chemical Reactions
1. Definitions Matching: (2.2 to 2.11 and 4.1 to 4.3)
a) A charged particle (the number of protons and
electrons will be different).
______ Base
b) One way to change the speeds of a reaction, this
one involves adding more reactants.
______ Covalent
c) The symbol we use when a reactant or product is a
solid
______ Ionic
d) A particle that has the same number of protons as
electrons.
______ Atom
e) The type of compound formed between a positive
metal and a negative non-metal.
______ Ion
f) The type of compound formed when two nonmetals share, which creates a bond.
______ Indicator
______ (aq)
g) A substance that will have extra H+ ions when you
add it to water.
______ (s)
______ Acid
h) A substance that will have extra OH1- ions when
added to water.
______ Surface Area
i) By changing the size of the reacting particles, this
is changed.
______ Concentration
j) A chemical such as phenolphthalein that lets you
know if you have an acid or a base.
k) The symbol we use when a solute is dissolved in
water.
2. Complete the following table, which shows atoms and ions of various elements:
Symbol (with charge)
Atomic Number
# of electrons
72
68
2+
Ni
Sc
I1-
P3-
3. Identify the following symbols, and explain one hazard this symbol represents. (section 2.1)
Identify Symbol
One Hazard
A
B
C
D
E
F
G
H
4. Draw Bohr diagrams for these to show how the compounds form. (section 2.2)
a) LiF
b) F2
5. Draw Lewis diagrams for the following, in order to show how
the compounds form. (section 2.2)
a) NaCl, sodium chloride
b) NH3, ammonia gas
6. Determine the metal and it’s charge in each of the following. (section 2.3)
a) FeCO3
metal is __________________, charge is ________________
b) Pd(SO4)2
metal is __________________, charge is ________________
7. Name these compounds. Include an “I” for ionic and a “C” for covalent compounds.
(section 2.4)
I or C?
Name
a) P2S3
b) Be(CN)2
c) MgSO4
d) SrCl2
e) Ag2SO4
f) Mn(OH)3
8. Identify the following atoms (no ions are shown below) given their Bohr diagrams.
(section 2.2)
a)
___________________
b)
___________________
c)
___________________
d)
___________________
9. Write formulas for the following compounds. Include an “I” for ionic and “C” for covalent
compounds. [REMEMBER to use the ‘metal/non-metal table’ for ionic compounds]
(section 2.3)
I or C?
a) Potassium arsenide
b) Sodium sulfate
c) Barium cyanide
d) Titanium (III) oxide
e) Tricarbon tetraiodide
Chemical Formula
f) Aluminum carbonate
g) Dinitrogen monoxide
h) Radium acetate
i) Ammonium phosphate
10. Balance the following equations. (section 2.6)
a) ______ Al + ______ F2 → ______ AlF3
b) ______Mn + ______ I2 → ______ MnI4
c) ______ PbCl4 + ______ K3PO4 → ______ KCl + ______ Pb3(PO4)4
d) ______ Ca(OH)2 + ______ HCl → ______ CaCl2 + ______ H2O
e) ______ Na2CO3 + ______ Cr(NO3)3 → ______ NaNO3 + ______ Cr2(CO3)3
11. Write a skeleton equation for these word equations. You don’t need to balance them.
(section 2.6)
a) Aluminum hydroxide + hydrogen fluoride → aluminum fluoride + water
b) Barium sulfate + sodium hydroxide → sodium sulfate + barium hydroxide
12. Identify the type of reaction for each of these. (section 2.8)
a) ZnS + 2 HCl → ZnCl2 + H2S
_________________________________
b) 2 H2 + O2 → 2 H2O
_________________________________
c) C5H12 + 8 O2 → 5 CO2 + 6 H2O
_________________________________
d) 8 Al + 3 Fe3O4 → 4 Al2O3 + 9 Fe
_________________________________
e) CaO + CO2 → CaCO3
_________________________________
f) HNO3 + NaOH → NaNO3 + H2O
_________________________________
g) 2 Al2O3 → 4 Al + 3 O2
_________________________________
13. Complete the following table, which shows the important aspects of acids and bases.
(section 2.9)
Have What Ion?
Have What pH?
Turn phenolphthalein
what colour?
3 Physical Properties?
Acids
Bases
14. Describe a chemical test to check for the presence of “hydrogen gas” or “carbon dioxide gas”
(section 2.2)
15. Explain how an indicator helps you find out… (section 2.9 and 2.10)
a) if you have an acid or a base
b) if the acid/base you have is strong or weak
16. List the four factors that affect the rate of a chemical reaction, and explain how you could
change each to slow down a reaction. (section 4.1)
17. According to the collision theory, what two things must happen for a reaction to occur?
(section 4.1)