GRADE 12 COLLEGE CHEMISTRY
EXAM REVIEW
Unit 1 – Matter and Qualitative Analysis
Words to know
Preservatives
Additives
Qualitative observations
Quantitative observations
Inference
Theory
Electromagnetic spectrum
Continuos spectrum
Line spectrum
Ionic bond
Covalent bond (non/polar)
Dissociation
Soluble
1. Convert the following:
(a) 0.0030 km to m
(b) 4.82 mm to m
(c) 1423 Pa to kPa
proton
electron
neutron
valence shell
valence electrons
atomic number
spectroscope
ground state
excited state
E.N.
types of reactions
insoluble
precipitate
atomic mass
isotope
ion (cat/anion)
Lewis diagram
Bohr model
energy level
frequency
wavelength
element
skeletal equation
balanced equation
ionic equation
net ionic equation
(d) 584 mL to L
(e) 1234 g to kg
(f) 6.203 L to mL
2. How many protons, electrons, and neutrons do each of the following contain?
(a) Co60
(b) Li7
(c) Na23
(d)
O16
(e) He4
3. Draw Bohr-Rutherford diagrams for: B
4. Draw Lewis/electron dot diagrams for: Al
C
O2-
K
O
5. How many electrons can each energy level hold?
H
I
Ba
Be2+
Fr
S
6. Why do elements emit colour when heated?
7.
(a) show the E.N. difference between the two elements
(b) state whether they bond ionic, polar or nonpolar covalent
(c) if ionic – show the transfer diagram, molecular formula, and its name
(d) if covalent – Lewis formula, structural formula, and molecular formula
(e) if polar covalent don’t forget to include ∂+ and ∂-
Te and Cl
Li and O
C and Br
8. Write the chemical formula for the following:
(a) potassium chloride
(i) copper(I) phosphate
(b) aluminum oxide
(j) carbon dioxide
(c) barium sulfate
(k) lead (II) chlorate
(d) carbon tetrachloride
(l) barium cyanide
(e) sodium acetate
(m) lithium sulfide
(f) ammonium hydroxide
(n) dinitrogen pentoxide
(g) magnesium fluoride
(o) ozone
(h) iron (III) carbonate
(p) ammonia
9. Give the correct names for the following:
(a) PbSO4
(i) HgCl2
(b) Fe(OH)3
(j) NaNO3
(c) CO
(k) CuSO4
(d) H2O
(l) CCl5
(e) N3Cl4
(m) MgS
(f) Sn(ClO3)2
(n) Ba3(PO4)2
(g) CaCO3
(o) NH4CH3COO
(h) KCN
(p) SO3
10. Write word equations, balanced chemical equations, and state the type of reaction for:
(a) Mercury (II) oxide is prepared from its elements
(b) Aluminum metal reacts with Zinc (II) sulfate
(c) Barium chloride reacts with sodium carbonate to produce barium carbonate and sodium
chloride
(d) Water is decomposed into hydrogen and oxygen gas
11. Balance the following and state the type of reaction observed:
(a)
K3PO4
(b)
K
(c)
N2
+
+
+
HCl

KCl
+
H3PO4
NaNO3

Na
+
KNO3
O2

NO2
12. Precipitate reactions – Use the solubility table to:
(a) write the balanced molecular equation (include if the products are soluble (aq) or insoluble
(s)
(b) write the ionic equation, and
(c) the net ionic equation (if there is no reaction, write NR)
Calcium chloride and ammonium hydroxide produces calcium hydroxide and ammonium chloride
Lead (II) nitrate and sodium sulfide
Ammonium carbonate and magnesium chloride
Unit 2 – Chemical Calculations
Words to know
The mole
Avogadro’s number
Molar mass
Mass
n = m/MM
solvent
C = n/V
1.
empirical formula
molecular formula
percentage composition
stoichiometery
mole ratio
solution
C1V1 = C2V2
limiting reagent
excess reagent
percentage yield
concentration
solute
dilution
1 mole of bananas = ___________________________ bananas
2. 2.5 mole of pencils = __________________________ pencils
3. 8.75 x 1025 atoms of sodium = ___________________ mole Na
4. Calculate the molar mass of the following:
(a) H2O
(b) FeCl3
(c) O2
(d) NaNO3
(e)
Ca(ClO3)2
5. Find the number of moles for the following compounds:
(a) 100g of CaCO3
(c) 50g of C6H12O6
(b) 15.57g of Bi(OH)3
(d) 4.11 kg of K3PO4
6. Find the mass of the following (in grams):
(a) 1 mol of HC2H3O2
(c) 2387 mol of Lithium hydroxide
(b) 0.5 mol of Ca(ClO3)2
(d) 3.5 x 1027 molecules of NaCl
7. Calculate the percentage composition of each atom in:
(a) KNO3
(b) H2O
8. Determine the empirical formula for a compound containing 80% C, and 20% H
9. Calculate the molecular formula for the following:
(a) Molecular mass 400.5g ; Al = 20.2% Cl = 79.8%
(b) Molecular mass 357g ; Sn = 66.4% C = 6.7% O = 26.9%
10. Consider the following reaction:
2H2
+
O2

2H2O
(a) How many moles of water can be produced by 6 moles of hydrogen? (use mole ratios)
(b) How many moles of hydrogen are required if 5.5 moles of oxygen are used?
11. What mass of oxygen will react with nitrogen monoxide to form 3.68g of nitrogen dioxide?
12. How much ammonium hydroxide is needed to react completely with 75g of copper (I) nitrate
in a double displacement reaction?
13. How many grams of CO2 will be produced when 8.50g of methane (CH4) reacts with 15.9g of
oxygen gas? This is a limiting/excess reagent question. (10.9g)
14. A solution containing 5.0g of Na3PO4 is mixed with a solution containing 10.90g of Ba(NO3)2.
If 7.69g of barium phosphate (actual yield) are recovered from the reaction, what is the
percentage yield? (91.8%)
15. Calculate the concentration of a solution that contains 7.91 mol of solute in 2.53 L of
solvent.
16. How many moles are contained in 750 mL of a 3.64 mol/L solution?
17. What is the mass of 3.96 L of a 0.628 M solution?
18. A solution contains 8.50 g of calcium chloride (CaCl2) dissolved in 3.33 L of water. What is
the concentration of this solution?
19. Water is added to 0.20 L of 2.40 M NH3 cleaning solution until the final volume is 1.0 L. Find
the new concentration of this diluted solution.
Unit 3 – Organic Chemistry
Words to know
Hydrocarbon
Alkane
Alkene
Alkyne
Fractional distillation
Cracking
1.
functional group
alcohol (hydroxy group)
ether
aldehyde (carbonyl group)
ketone (carbonyl group)
carboxylic acid (carboxyl group)
ester
organic solvent
flammable
combustible
polymer
un/saturated
Name the following compounds:
2. Draw (any method) the following organic compounds:
Propane
methanol
2-pentene
ethoxy hexane
3-octyne
2-pentanone
butanal
methyl propanoate
ethanoic acid
2-butyne
3. Complete, balance, and name the following organic reactions. (don’t forget catalysts!)
Unit 4 – Electrochemistry
Words to know
LEO says GER
Redox
Oxidation
Reduction
Oxidation numbers
1.
activity series
galvanic cells
RED CAT and an OX
electrolytic cell
anode
cathode
primary cell
salt bridge
secondary cell
electrolyte
corrosion
half-cell
electroplating
half-cell reactions electrorefining
What is the oxidation number for the underlined element?
H2
NaNO3
SO42-
MgO
HPO42-
CO2
2. Use oxidation numbers to determine if the following are redox reactions. If it is, identify
which element is oxidized and which is reduced.
K
H2
+
+
HCl
+
Na2CO3
O2


Na
H2O
+
+
K2CO3
H 2O
NaHCO3

CO2
+
NaCl
3. Use the activity series to determine if a reaction will occur:
Cu
+
ZnSO4
Li
+
Pb(NO3)2


4. Draw a completely labeled galvanic cell using magnesium and silver electrodes.
(include the anode, cathode half-cell reactions and the overall reaction)
5. Define corrosion and state the four factors that affect the rate of corrosion.
6. State two main differences between galvanic and electrolytic cells.
Unit 5 – Chemistry in the Environment
Words to know
Hard water
Soft water
Acid
Base
Strong acid
Weak acid
1.
dilute concentration
concentrated solution
pH
hydrogen ion conc.
hydroxide ion conc.
neutralization reaction
titration
volume (L)
standard solution
Boyle’s Law
endpoint
Charle’s Law
Kinetic molecular theory Dalton’s Law
Pressure (kPa)
temperature (K)
Draw a fully label a basic pH scale.
2. List three main properties of acids and bases.
3. What are the products of a neutralization reaction and show a typical reaction.
4. In an acid-base titration, 15.0 mL of carbonic acid H2CO3 were neutralized completely by
18.25 mL of 0.18 M potassium hydroxide. Calculate the concentration of the carbonic acid.
(0.110 M)
5. What volume of 0.525 M HCl must combine exactly with 40.5 mL of an aqueous sodium
hydroxide solution with a concentration of 0.375 M?
6. Outline the procedure (and all lab equipment) for performing an acid-base titration.
7. What is the final pressure of a 2.5 L gas that initially was at 122 kPa and 5.5 L?
7. Calculate the initial temperature of a 5.5 L gas that ends up with a volume of 7.2 L and a
final temperature of 22 oC.
8. If a gas at standard pressure is added to another nonreactive gas at 35 kPa, what is
the new pressure?