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Chemistry 11 Exam Review
 In most cases the emphasis is on ability to apply principles to problem solving not to
regurgitation of information.
 Tests, quizzes, labs and all classroom assignments/work can help guide you in preparing
for this exam.
 Differentiate between the following terms:
 Solid, liquid and gas See your notes
 Physical properties and chemical properties Make a chart to show these
 Physical change and chemical change See your notes
 Atoms, elements and compounds See your notes
 Describe the Law of conservation of mass and the Law of conservation of energy
 Law of conservation of mass - the mass of substances produced (products) by a chemical
reaction is always equal to the mass of the reacting substances (reactants).
 Law of conservation of energy - energy can be transformed (changed from one form to
another), but cannot be created or destroyed.
 Development of the theory of the atom
 Gas discharge tubes, Dalton, J.J. Thompson, Rutherford, Bohr – go over how each
developed their theories, main points of each theory and each model of the atom.
 Determination of atomic number, mass number, electrons, protons, neutrons and the
element symbol for both atoms and ions. Refer to charts that we have done for practice.
Name
Symbol
Atomic Mass
Atomic
Number
Number of
Protons
Number of
Neutrons
Number of
Electrons
Calcium
Neon
Krypton
Bromine
Iodine ion
Cadmium ion
Ca
Ne
Kr
Br
ICd2+
40
20
84
80
127
112
20
10
36
35
53
48
20
10
36
35
53
48
20
10
48
45
74
64
20
10
36
35
54
46




Isotopes and estimating average atomic masses
Isotopes are atoms that have the same number of protons but have different numbers of
neutrons and therefore differing masses.
Nitrogen has two isotopes – N14 and N15 . Nitrogen-14 exists with 99.632% abundance
and Nitrogen-15 occurs with 0.369% abundance. Find the average atomic mass of
nitrogen
14 x 0.99 = 13.86
15 x 0.01 = 0.15 .
14.01
Draw Bohr diagrams
7+

Draw energy level diagrams, and electron configuration diagrams
2
1s22s22p3
1 ___
s
___ ___ ___
px
py pz
 The Periodic Table and it’s trends
 Explain the concept of families and relate to oxidation numbers






Give the names of the families for groups 1, 2, 7, and 8
1-alkali metals, 2-alkaline earth metals, 7-halogens, 8-noble gasses
Characteristics of metals, nonmetals and metalloids
Describe the periodic trends in electron configurations
# of electons on valence orbital increase
# of orbitals increases
Draw electron dot diagrams for various elements
Give valence electrons for various elements and describe how the valence # is related to
the reactivity of elements.
S – 2s23p4
Li – 2s1
Kr – 4s24p6
Tends to gain 2e
Tends to lose 1e
Does not tend to react
Describe the periodic trends of
a) Atomic size
decreases
increases
b) Ionization energy
increases
decreases
c) Electron affinity
increases
decreases
d) Ionic Size
decreases but cations are smaller than anions
increases
 Chemical Bonding
 Ionic bonding – dot diagrams and equations
 Covalent bonding types
 Bond polarity


Molecular polarity
Molecular geometry
1. Draw the dot notation, and show the equations for ionic bonding for the following
combinations **I was unable to do the dot diagrams on here…sorry.
a) Sr & I
b) Al & S
c) K & P
+2
+3
Sr + energy
Sr + 2e 2Al + energy
2Al + 6e 3K + energy
3K+ + 3e2I + 2e2I- + energy 3S + 6e3S-2 + energy P + 3eP-3 + energy
+2
+3
-2
+
-3
Sr + 2I
SrI2 + energy 2Al + 3S
Al2S3 + energy 3K + P
K3P + energy
2. List some of the differences between ionic and covalent compounds
Ionic
Covalent
Hard
Relatively Soft
High melting point
Low melting point
Conduct electricity in
Poor conductors
molten and water solution
form
Soluble in water
Limited solubility in water
Strong forces of attraction
Weak forces of attraction
Have regular structures
Irregular structures
Relatively simple
Can create complex
compounds
compound formulae
3. give examples of
a) single covalent bonding
Cl-Cl
b) double covalent bonding
O=O
c) triple covalent bonding
N=N
d) polar covalent bonding
O-H
H
e) co-ordinate covalent bonding
H
H-N-H
H
4. Draw dot, Lewis, structural and orbital diagrams for the following compounds, indicate
the bond types (single, double or triple) and the bond polarities for each.
a) C2I2
b) H2CS
c) PF3
d) SF2
5. Predict the shapes of the compounds above.
 Chemical Naming and formula writing
 Determine the oxidation numbers for atoms of a compound
 Writing chemical formulas and naming of compounds for compounds containing
a) a metal and a nonmetal
b) hydrogen and another element
c) two nonmetals
d) compounds containing one or more polyatomic ions
e) acids
6. Name the following compounds indicating the oxidation number of the underlined
elements
CuSO4- Copper II sulfate Mg2C Magnesium carbide N2O3 dinitrogen trioxide
KMnO4 Potassium permanganate AlF3 Aluminum fluoride NaC2H3O2 sodium acetate
OF2 oxygen difluoride Hg3PO4 mercury III phosphate Ni2O3 Nickel III oxide
CF4 Carbon tetrafluoride (NH4)3P ammonium phosphide
Ca(ClO3)2 calciumchlorate
Au2S3 gold III sulfide
Fe(OH)3 Iron III hydroxide
HI Hyroiodic acid
H2SO3 sulfurous acid
Sn(S2O3)2 tin II thiosulfate
7. Write formulas for the following chemicals
Silver sulfide Ag2S
Barium phosphate Ba3PO4 Tin IV oxide SnO2
Mercury I acetate HgC2H3O2 Phosphoric acid H3PO4 Potassium nitride K3N
Lead II chromate PbCrO4 Dichlorine monoxide Cl2O Calcium carbide Ca2C
Aluminum fluoride AlF3 Bromine trichloride BrCl3 Copper II hydride CuH2
 Equations
 Balancing equations
 Chemical reaction types
8. For each of the following, complete the equation where necessary, balance the equation
and state the type of reaction.
a) Silver nitrate + zinc
?
2AgNO3 + Zn
2Ag + Zn(NO3)2
single replacement
∆
b) Magnesium chlorate
Magnesium chloride + oxygen
Mg(ClO3)2 ∆ MgCl2 + O2
decomposition
c) Ammonium sulfide + gold III nitride
?
3(NH4)2S + 2AuN
2(NH4)3N + Au2S3 double replacement
d) Magnesium Nitride + water
Magnesium hydroxide + ammonia
Mg3N2 + 6H2O
Mg(OH)2 + NH3
double replacement
e) Strontium + Phosphorus
?
3Sr + 2P
Sr3P2
Synthesis
f) Si4H10 + O2
SiO2 + H2O
2Si4H10 + 13O2
8SiO2 + 10H2O
double replacement
g) C7H6O3 + oxygen
water + carbon dioxide
C7H6O3 + 7O2
3H2O + 7CO2
Combustion
h) HbrO3 + HBr
H2O + Br2
HbrO3 + 5HBr
H2O + Br2
Double replacement
 The Mole Concept
 Mole mass determination
 Avogadro’s number
 Conversion between each of the following: grams – moles – molecules – atoms
 Percent composition
 Determination of empirical formula and molecular formula
9. Calculate the number of atoms of antimony in an ingot with a mass of 600.0g.
2.9655x1024 atoms
10. Calculate the mass of silver in a bar of silver that has 4.5 x 1022 atoms of silver.
8.07g
11. Determine the mass of 0.82 moles of aluminum chloride.
109.47g
12. How many molecules of benzene (C6H6) would be contained in a bottle holding 230g?
1.77x1024 molecules
13. The chemical formula for Rolaids is NaAlH2CO4. If you swallowed 8.3 x 1021 molecules
of Rolaids, how many grams of Rolaids would that be?
1.77g
14. How many atoms of oxygen is in the above sample?
3.32x1022 atoms
15. The chemical stimulant caffeine has the formula C8H10N4O2. In a cup of coffee that
contains 3.5g of caffeine, how many grams of nitrogen would the cup hold?
1.01g
16. The formula for an organic compound is C10H8O. If a person drinks 3.0 x 10 molecules
of the compound, what mass of hydrogen would that person consume?
0.040g
21
17. What is the % iron in the compound Fe3(PO4)2?
46.8%
18. An organic compound contains 30.3% carbon, 1.7% hydrogen, and 68% bromine. If the
molar mass of the compound is 236 g/mol, what is the correct molecular formula?
C6H4Br2
19. The analysis of a 10g sample of a sodium compound shows that in addition to sodium,
the compound contains 5.38g of oxygen and 2.69g of sulfur. If the molar mass is
238g/mol, calculate the correct chemical formula.
Na2O8S2
20. A sample of organic compound contains 0.225 moles of carbon, 0.328g of hydrogen, and
1.50 x 1022 atoms of nitrogen per 1.5 x 1022 molecules of compound. What is the
chemical formula of the compound?
C9H13N
 Chemical Stoichiometry
 Stoichiometric calculations
 Double Reactions
 Limiter reactions
21. How many grams of hydrogen can be produced from a reaction involving 4.5g of zinc
and an excess of hydrochloric acid?
Zn + 2HCl
ZnCl2 + H2
Mass of H2 = 0.139g
22. How many grams of water is produced from the following reaction if 5.00g of SiF4 is
reacted with 2.00g of NaOH?
SiF4 + 6 NaOH
Na2SiO3 + 4NaF + 3H2O
NaOH is the limiter
Mass of H2O =0.45g
23. What mass of sodium nitride can be produced form the following double reaction using
∆
3.4 x 1022 molecules of N2O5? N2O5
N2 + O2
Na + N2
Na3N
Mass of Na3N = 9.38g
24. If 34.0g of gold III nitrate reacts with 23.7g of barium chloride, what mass of gold III
chloride is formed in this reaction?
2Au(NO3)3 + 3BaCl2
2AuCl3 + 3Ba(NO3)2
BaCl2 is the limiter.
Mass of AuCl3 = 23.07g
 Organic Chemistry
 Name and draw structural formula for the hydrocarbon families including
a) alkanes
b) alkenes
c) alkynes
d) substituent branches
e) cyclo groups
f) benzenes
g) various functional groups
 Describe and draw structural formula for isomers
 Identify and write balanced equations for hydrocarbon reactions.
25. Name the following organic compounds:
a) CH3-CH-CH2-CH3
b) CH3-CH2-CH-CH=CH2
CH3-CH-CH2-CH3
3,4-dimethylhexane
CH2- CH3
Cl
3-chloro-1-pentene
c) CH3-C=C-CH-CH-CH3
d) CH3-CH2-CH
CH3
3-ethyl-3-methyl-4-hexyne
CH2
CH2
CH2 CH2
ethylcyclopentane
26. Draw structural formulas for the following:
a) 3-cloro-2,2,5-trimethylheptane
CH3
CH3-C-CH2- CH2-CH-CH2-CH3
CH3 Cl
CH3
b) 4-bromo-2,3-diethyl -1nonene
CH3=C-CH- CH-CH2-CH2-CH2-CH2-CH3
CH2CH2 Br
CH3 CH3
c) Bromocyclopropane
Br
CH
CH2
CH2
d) 2,6-dimethyl-3-octyne
CH3-CH-C = C-CH2-CH-CH2-CH3
CH3
CH3
27. Draw and name three structural isomers of the compound C6H10
CH3-CH2-CH2-CH2-C=CH
CH3-CH2-C=C-CH2-CH3
1-hexyne
3-hexyne
CH3
CH=C-C-CH3
CH3
2,2-dimethyl-3-butyne
28. Write balanced equations for each of the following:
a) Combustion of 2,3-dimethyl-3-ethyl-pentane
C9H20 + 14O2
9H2O + 10CO2
b) Reaction between 5-ethyl-3,3-dimethyloctane and bromine.
C12H26 + Br2
C12H25Br + HBr