Chemistry 11
Year End Review
Name;
Metric Conversions
Draw the metric conversion line. For each point give an exponent of 10, fraction or
decimal value, corresponding prefix and the symbol.
Do the indicated metric conversions
1. 3240 ng=
g
2. 0.06 kg=
cg
3. 0.3 ML=
kL
4. 426 L 
mL
5. 1mm=
nm
6. 14 hm=
mm
7. 273 cg=
g
8. 6 dag=
mg
9. 22 nL=
mL
10. 42 dL=
daL
11. 3000 g=
Mg
12. 346 g 
g
Convert these numbers from exponential notation to ordinary expanded notation
2
1. 10 =
4. 10
5
=
2. 10
2
=
6
5. 10 =
9
3. 10 =
6. 10
6
=
Convert these numbers from expanded notations to exponential.
1. 0.01=
2. 100 000 000=
3. 0.000 000 000 1=
4. 100 000=
5. 0.001=
6. 1 000 000=
Write the SI prefix for each of the following factors. For example, 10
"centi"
1. 10
4. 10
12
9
2. 0.001
3. 1000
5. 0.000 000 001
6. 10
2
corresponds to
1
List the basic SI unit and abbreviation for each of the following quantities.
Quantity
Length
SI Unit
Mass
Volume
Area
Density
Time
Velocity
Temperature
1. Please Define
a. Hypothesis
b. Theory
b. Model
2. What are the four physical states of matter?
Abbreviation
3. a. How is energy related to matter?
b. Give and example of energy.
4. What is the difference between kinetic and potential energy?
5. Fill in the blanks.
Math works in ___________________ but science works in _________________.
6. Fill in the chart using SI Units.
Quantity
Name
Abbreviation
Distance
Kilogram
,
s
Kelvin
7. Draw the symbol for
a. Danger - Poison
b. Caution - Flammable
c. Warning - Corrosive
d. Caution - Explosive
Chapter 2
1. 1.00 mole of nitrogen has a mass of 28.0 g. How many moles of nitrogen are in
10.0 g?
2. If concentrated hydrochloric acid has a concentration of 11.7 mol/L, what volume of
hydrochloric acid is required to have 0.45 moles of HCl?
3. Sugar costs $0.89/kg. 1 t = 1000 kg. How many tones (t) of sugar can you buy for
$250.00?
4. A 7.00 mL chunk of boron has a mass of 16.38 g. What is its density?
3
5. If the density of copper is 8.92x10 g / L and the density of magnesium is
1.74x103 g / L , what mass of magnesium occupies the same volume as 75.0 g of
copper?
6. An atomic clock measured a time interval as 39.492673. Give an example of a
measurement that would be:
a. not accurate, but precise
b. inaccurate and imprecise
c. not precise but accurate
d. accurate and precise
7.
Give
i. The difference between each numbered division.
ii. The difference between each unnumbered division.
iii. The reading at A______________
B______________
C______________
8. Write the following measurements and uncertainty in the correct form.
a. A balance gives a mass reading of 24.69, The balance has an uncertainty of 0.01g.
b. A measurement ranges from 365 to 371 cm.
c. Time range from 79.3 to 80.5 s.
9. What is the range of acceptable values for:
a. 16 .32  0.01mL
b. 2.69 x10
5
 0.03 x10 5 s
10. State the number of significant figures.
4
a. 4720
b. 36 .21x10
c. 32.510
d. 42 000 000
e. 0.00032 x10
4
f. 0.00890
11. Perform the operation, give answer with correct number of significant figures.
b. 3.2 x10  4 x10
a. 11 .2  0.50
c.
8
8.9
3
d.
1.5  5.500
0.140
e. 9  3.4612
f. 16.2+86.92
g. 39.129+7.67324
h. 4.102 x10
i. 4 x10  5.972 x10
6
7
2
4
 3.49 x10 3
Chem 11 Review
Unit IIIA
Name:
Date:
1. Describe a measure of volume quantitatively and qualitatively.
/2
2. What it the difference between
a. observation and description
b. observation and interpretation
/2
3. Define
a. Hypothesis
b. Theory
c. Law
/6
4. Give an example of a
a. Hypothesis
b. Theory
c. Law
/3
/13
5. a. Give 2 examples of a chemical property
c. Give 2 examples of a physical property
/4
6. Define
a. Matter
b. Chemistry
/2
7. Which are intensive (I) and which are extensive (E)?
_____ Shape
_____ Melting point
_____ Malleability
_____ Hardness
/4
8. Describe the following in terms of volume, shape, flow and particles
Solid
Liquid
Gas
/6
/16
9. Define
a. Hardness
b. Malleability
c. Ductility
d. Lustre
e. Viscosity
f. Diffusion
g. Vapour
/7
10. Ice evaporates slowly. What do you know about its vapour pressure?
/1
11. Do p. 48 & 49
26. a.
b.
28.
29.a.
b.
/5
/13
12. Draw the chart for the divisions of matter. Give an example of each final division.
/6
13. Give an example of
a. Atom
b. Molecule
c. Ion
/3
14.
a. S
Classify the following as an atom, a molecule or an ion.
2
b. O2
c. Sb
d. S
e. Al
3
f. NH 3
/6
15. Classify each of the following as one of heterogeneous or homogeneous.
a. Salt
b. Cucumber
c. Duck Egg
d. Tea
/4
16.
Which of an element, compound, solution or mechanical mixture are possible
classifications for the following? (There may be more than one answer for each example)
a. A clear liquid which boils away to leave a white solid
b. A collection of solid particles, some of which are white and some of which are red.
c. A solid which melts at 170 degrees Celsius
d. A gas
e. A liquid
f. A liquid which boils away completely at 64 degrees Celsius but when heated in a
closed container produces a yellow gas and a black solid
/4
17. Which substance is the solute in the following?
a. Water with 8% acetic acid
b. a solution with 900 g of silver nitrate and 100 g of water
/2
18. Classify each of the following as a mixture or a compound
a. Methanol, CH 4
b. a pizza pop
c. Coke
d. Salt
/4
/29
Chem 11
Unit 3B REVIEW
Name:
Date:
1. Copy the two tables, A & B on page 58.
/10
2. Which separation method(s) could be used to separate
a. A mixture of rock, sugar and water
b. 2 immiscible liquids
c. A dry mixture of 3 water soluble dyes
/6
3. A single solvent extraction removes 80% of the desired chemical from a solution.
How much is left after 4 extractions?
/3
4. How would you separate a mixture of pennies, nails, a copper(II)sulphate aqueous
solution and trichloroethane (its density is greater than water). Carefully order the
steps and explain.
/6
5. Classify as a physical (P) or chemical (C) change.
a. drying cement
b. dissolving sugar
d. mixing blue and red dyes to make purple
c. frying potatoes
e. condensation forming on windows
/5
6. Please graph the cooling curve for water from 110oC to -10oC. Label the axes and
indicate phases present for each portion of the graph.
/5
7. Identify the 3 types of Kinetic Molecular Energy. Describe them and state where
they are the most crucial (play and important role)
Type
1.
2.
3.
/12
Description
When important
Ch 4
From text p. 75 15-65 and p. 76 66-160 - do every one divisible by 3.
Unit 5 – Part 1
WORKSHEET
Name:
Date:
1. Experimentally it is found that 2.0 L of gaseous sulphur reacts with 4.0 L of
oxygen. Suggest a possible formula and name for the compound if the gases are
at STP.
/2
2. If 1.5 L of an unknown gas Y contains 1.5x1023 molecules at a certain temperature
and pressure, how many molecules are present in 4.5 L of oxygen gas at the
same temperature and pressure?
/2
3. Calculate the molar mass of
a.
BaS
b. PtCl4
c. Ba HS 2  4H2O
e. Al CLO4 3
f. Pt 2O3  3H2O
/6
d. C3S2
/6
/16
g. CH3COOH
h. MgSO4  7H2O
i. CH 3CH 2CH 3
/6
4. Calculate the mass of
a. 1.36 mol of NH 4Cl
b. 6.23x10-2 mol of NaOH
/6
c. 2.75 mol of PCl3
d. 6.79x102 mol of NH3
/6
5. Calculate the number of moles in
a. 29.7 g of H 2SO4
b. 45.7 mg of O2
/6
/24
c. 96.7 g of sulphur dioxide
d. 327 kg of potassium permanganate
/8
6. Calculate the molar mass of the following
a. a 0.125 mol sample of methane that has a mass of 2.00 g
/2
b. a 6.88x10-5 mol sample of a protein that has a mass of 149.6 g
/2
7. Calculate the volume at STP of
a. 6.92 mol of NH3 g 
b. 1.75 mol of HClg 
/4
8. Calculate the number of moles in the following at STP.
a. 46.7 L of H2g 
/4
b. 490 mL of O2g 
/20
9. How many atoms in 1 molecule of the following?
a. Na2B4O7  10H2O
b. Ca OH 2
c. Cu3 OH 2 CO3 2
/6
10. Find the mass in grams of
a. 1.4x1014 CO molecules
/3
b. 7.92 L of O2g  at STP
/3
c. 367 Ne atoms
/3
11. How many atoms in the following?
a. 2.5 mol of NH 4F
/3
b. 3.2 L of N2g  at STP
/3
/21
c. 56.7 g of NaCl
/3
12. a. What is the density of CO(g) at STP?
/3
c. What is the volume of 1.5 mol of SiO2 (d=2.64 g/mL)?
/3
/9
Chem 11
Review Ch 5 Part 2
Name:
Date:
1. What is the molarity if 232.9 mg of K2CrO4 is dissolved in enough water to make
325 mL?
/3
2. What is the actual experimental procedure you should use to make 350.0 mL of
0.823 M KBr, starting with solid KBr?
/4
3. What is the concentration produced when 140.0 mL of 2.55 M FeCl3 is mixed with
450.0 mL of 1.27 M FeCl3?
/5
/12
4. 75.0 Ml of 0.275 M HCl is mixed with 52.0 mL of 0.472 M HCl. What is the final
concentration?
/5
5. What is the molarity if 2.25 M of 325.0 mL of HNO3 is boiled down to 200.0 mL?
/3
6. What is the molarity if 125.0 mL of 0.275 M SnCl2 is mixed with 275.0 mL of 0.527
M SnCl2 and then boiled down to 227.0 mL?
/5
7. What mass of the solid solute is in 0.56 L of 1.25 M NaCl?
/4
/17
8. What is the molarity of CH3COCH3, d = 789.9 g/L?
/3
9. What is the density of S2Cl2, with a molarity of 12.73 M?
/3
10. What volume of 0.350 M FeCl3 can be made from 50.0 mL of 3.00 M FeCl3?
/3
11. How many moles of CaCl2 are in 1.32 M CaCl2 if you have 567 mL?
/3
/12
12. What concentration of KOH is made by diluting 50.0mL of 2.32 M KOH to 300.0
mL?
/3
13. What concentration is produced when 50.0 Ml of 0.125 M HCl is mixed with 75.0
mL of 0.250 HCl?
/3
14. What volume of 0.450 M BaCl2 contains 45.0 g of BaCl2?
/3
15. What is the percent composition of BaCl2?
/3
/12
16. Calculate the percentage of water in CaCl 2  2H 2O .
/3
17. Find the empirical formula if the percent composition is
24.4% C, 3.39% H, 72.2% Cl
/3
18. A gas has the percentage composition of 30.4% N and 69.6% O. If the density of
the gas is 4.11 g/L at STP, what is the molecular formula of the gas?
/4
/10
Chem 11
Ch. 6 Review
Name:
Date:
1. Balance the following chemical equations:
______K
+ _____Cl2
 ______KCl
______Na
+ ______O2
 ______Na2O
______Sr
+ ______N2  ______Sr3N2
______K
+ ______H2O  ______KOH
______NH4Cl + ______Ca(OH)2
______FeS2
 ______NH3 + ______H2O + ______ CaCl2
+ ______O2  ______Fe2O3
______Mg(ClO3)2
+ ______H2
 ______MgCl2
+ ______SO2
+ ______O2
______C6H14 + ______O2  ______CO2
+ ______H2O
______K2CO3(s) + ______H3PO4(aq)  ______K3PO4(aq) + ______H2O(l)
/18
+ ______CO2(g)
2. Write the chemical formulas with subscripts and balance the equation.
a. magnesium chloride decomposes to give metal magnesium and chlorine gas
/3
b. sulfuric acid reacts with calcium hydroxide to form water and calcium sulphate.
/3
c. solid iron reacts with oxygen to form iron (II)oxide
/3
d. chlorine replaces iodine in calcium iodide
/3
e. barium chlorate, when heated forms barium chloride and oxygen
/3
/15
3. Complete each equation, balance it and identify the type of reaction.
TYPE
a. ______Ni(s) + ______FeSO4(aq) 
/3
b. ______C4H8(l) + ______O2(g) 
/3
c. ______H3PO4(aq) + ______Al(OH)3(aq) 
/3
d. ______Pb(NO3)2(aq) + ______NaCl(aq) 
/3
e. ______CoBr2(s) 
/3
f. ______AlCl3(aq) + ______Pb(NO3)2(aq) 
/3
4. Draw an energy diagram having H  42kJ
/2
5. H  75 kJ , for the reaction A  B. Rewrite this equation to show the 75 kJ properly on
the reactant or product side.
/2
/22
6.
If a reaction releases 35 kJ of heat, what is the H for the reaction?
/1
7. Name
a. An exothermic reaction
/1
b. An endothermic reaction
/1
8. If C + 28 kJ  D
a. What is H for the reaction?
b. Which has more energy, the reactants or the products?
c. Is it exo- or endo- thermic?
/3
9. Translate each of the following chemical reactions into a complete, balanced
chemical equation using international symbols and including states of matter.
a. The reaction of magnesium and oxygen to form magnesium oxide is used to produce light
in disposable flash bulbs.
/3
b. Chlorine gas reacts with an aqueous solution of sodium iodide. Experimental evidence
indicates that the products are solid iodine and aqueous sodium chloride.
/3
/12
c. Solid sodium sulphate reacts with carbon to form solid sodium sulphide (used to produce
synthetic fabrics) and carbon dioxide.
./3
d. sulfuric acid, spilled from a battery, reacts with baking soda to produce aqueous sodium
sulfate, carbon dioxide gas, and water.
/3
e. The roasting of zinc sulfide ore in a smelter involves the heating of the ore in the presence
of oxygen to produce zinc oxide and sulfur dioxide gas.
/3
f. Once the protective oxide coating is removed, aluminum metal reacts readily with water to
form hydrogen and aluminum hydroxide.
/3
/12
10. Balance the following equations by inspection.
a. ___ Ni ( s )  ___ HCl( aq )  ___ NiCl2( aq )  ___ H 2( g )
b. ___ Ca(OH ) 2( s )  ___ HCl( aq )  ___ CaCl2( aq )  ___ HOH( l )
c. ___ Cl 2( g )  ___ NaBr( aq )  ___ Br2  ___ NaClaq 
d. ___ Cr2O3s   ___ Crs   ___ O2g 
e. ___ Fes   ___ HCl aq   ___ FeCl3aq   ___ H 2g 
f. ___ C3 H 6g   ___ O2g   ___ CO2g   ___ H 2Og 
g. ___ P4s   ___ F2g   ___ PF3l 
h. ___ Ca NO 3 2aq   ___ KOH aq   ___ Ca OH 2s   ___ KNO 3 aq 
i. ___ KHCO3s   ___ K 2CO3s   ___ H 2Ol   ___ CO2g 
j. ___ H 3 PO4aq   ___ NaOHaq   ___ Na3 PO4aq   ___ HOHl 
k. ___ Ca NO 3 2aq   ___ Na 3 PO 4aq   ___ Ca 3 PO 4 2s   ___ NaNO 3aq 
l.
___ Cu s   ___ HNO 3aq   ___ Cu NO 3 2aq   ___ NO 2g   ___ H 2Ol 
/24
Chemistry 11
Unit 7
Name:
Date:
1. Given: 4NH3g   5O2g   6H 2Og   4NOg 
a. What mass of NO is produced when 64.7 g of oxygen react?
/3
b. If 36.7 L of NH 3 reacts, how many grams of water are produced at STP?
/3
c. If 46.4 L of water is produced, what volume of oxygen reacted at STP?
/3
2. 4CH3NO2l   3O2g   4CO2g   6H 2Ol   2N2g 
a. What mass of water is produced when 2.34 g of CH 3 NO2 is burned?
/3
b. What combined volume of gas at STP is produced if 4.79 g of CH 3 NO2 burns?
/3
c. What volume of oxygen gas at STP is required to produce 32.74 g of carbon dioxide gas?
/3
3. NaOHaq   HClaq   H 2Ol   NaCl
a. What volume of 2.50 M sodium hydroxide is required to neutralize 31.2 mL of 0.249 M
HCl?
/3
b. If 49.7 mL of acid neutralizes 25.7 mL of 2.96 M NaOH, what is the concentration of the
HCl?
/3
c. If 63.2 mL of NaOH is neutralized by 34.7 mL of 0.264 M HCl, what is the concentration
of the HCl?
/3
4. a. Write a balanced chemical equation for calcium hydroxide reacting with sulphuric acid.
Ch. 8 – Atoms & the Periodic Table
REVIEW
Name:
1.
Date:
Fill in the table. Show both atomic # and atomic mass of the particle.
27
13 Al
138
2
56 Ba
X 3 
Cd 2
/8
2.
Calculate the expected molar mass of the following isotopes
69
a)
Ga = 60.0% ; 71Ga = 40.0%
/2
b)
/2
12
C = 98.90% ;
13
C = 1.10%
8R-2
3.
Write the electron configurations of: (may use core notation)
a) Be
b) Ne
c) Cd
d) Fr
e) O-2
f) Ti+4
g) Clh) Pb+4
i) Ca+2
/10
j) As-3
4.
How many valence electrons do these contain?
a) O
b) Kr
c) Al
d) Ca
e) Hg
f) Br-
g) O+3
h) Ge+4
/8
5.
/8
State the Chemical family/group the following belong to
a) Mo
b) Sr
c) K
d) Ce
e) I
f) Pa
g) Xe
h) Dy
8R-3
6.
Which member in the pair is more metallic?
a) Ca or S
b) K or Fr
c) Zn or Al
d) Au or Cu
/4
7.
Which member in the pair has better electrical conductivity?
a) Ra or Mg
b) Cr or Zn
c) Ba or Cl
d) Cs or Fr
/4
8.
Please indicate the number of valence electrons and the valence and the electron dot
structure.
/9
9.
a)
Why are the ionization energies of Ne & Ar so high?
b)
Why does ionization energy increase going from K to Kr?
/2
/2
8R-4
10.
Consider
/12
11.
Which have open shells?
a) I-
b) Li+
c) Cu
d) Ne
/5
12.
/2
Name 2 atom pairs that would form ionic bonds?
e) Pb+2
13. Nuclear size.
a) Explain why Ca+2 is smaller than Ca?
/2
8R-5
b) Is O larger or smaller than O? Why?
-2
/2
14.
What happens to the strength of a London Force between identical atoms going
a) down a column?
/1
b) across a row?
/1
c) why?
/2
15.
What type of bond do you expect to form between
a) H & N
/4
b) Na & I
c) Cl & F
d) Mg & Mg
Organic Chemistry
I.
Alkanes
A. Give the following IUPAC name for each of the following:
1.
H
H
H
H
H
C
C
C
C
H
H
H
H
2.
H
H
H
C
H
H
H
H
C
H
C
C
C
C
C H
H
H
H
H
H
H
H C
H
H
H
3.
H
H
H
C
H
C
C
C
H
H
H
H
4.
H
H
H
H
C
C
H
H
H
H
H
H
C
H
C
C
C
H
H
H
C
H
H
H
H
C
H
H
C
H
H
C
H
H
5.
6.
H
H C H
H
H C H
H C HH C H
H
H
H
H C H
H C H
H
H
H
C
C
C
C
C
C
C
H
H
H C H
H
H
H
H
H
H
H C
C
H
H
H
H
H
H
H
H
H
C
H C
C
C
C
H
H
H
H
H C
H
H
H
C
C
C
H
H
H
C
H
H C
H
H
H
H
B. Write the structural formula for each of the following:
1. 2,3,4-trimethyloctane
2. 2,3-dimethylbutane
3. 4-ethyl-2,4-dimethylheptane
4. 1,3-dipropyl decane
C. Name the all the compounds in this reaction.
1.
D. Identify the circled functional groups in these compounds.
2.