Exam Info + Review

SCH4C1 Chemistry Exam Review
Exam Breakdown:
-
Wednesday, January 21, 2015
15% of your final mark
2 hours long (8:30-10:30)
Category:
Knowledge and Understanding
Thinking and Investigation
Communication
Application
Category Weighting:
25%
35%
15%
25%
Question Type:
Multiple Choice
Short Answer
Short Answer
Short Answer
Total Marks
Marks:
/20
/30
/15
/20
/85
What to bring:
-
Periodic table, solubility table
Nomenclature Summary
Calculator
Pens and pencils
1 page, 1 side formula sheet
o You may use 1 regular sized piece of paper (blank or lined – 8.5” x 11”)
o You can ONLY write on ONE SIDE
o There are no restrictions to what you may include – write whatever you find helpful
** you will not be given any formulas ON the exam.
o Must be your own original work only – no computer scans, photocopies, etc
o If it violates any of these rules, you will not be allowed to use it!
Topics to Review:
-
-
Energy levels and the Bohr atom
Ionic and molecular bonding diagrams
Ionic and molecular nomenclature
Reaction types and balancing
How to use solubility table
Precipitate reactions, total and net ionic equations, spectator ions
Counting atoms and molecules
The mole
Molar mass
Avogadro’s number
Stoichiometry
Limiting reagent
Concentration
Hydrocarbon naming and drawing
Hydrocarbon reactions
Hydrocarbon derivatives and functional groups
Arrhenius theory and modified theory
Acids and bases – strong vs weak
pH scale
pH indicators
pH and [H+] calculations
Oxidation vs reduction
Half reactions
Galvanic cells
Also Review:
-
all tests and quizzes (cover up your answers and redo them)
Sample Exam Questions:
1. Fill in the blanks.
Element
Atomic Number
# of protons
# of electrons
Atomic Mass
# of neutrons
C – 12
C – 14
Na – 23
Sn - 119
2. What is the difference between ionic and molecular compounds in terms of:
a. electrical conductivity
b. state
c. composition
d. how to name and write formulas
3. Complete the following chart.
Type of
Elements
Compound
Type of Bonding
Bonding Diagram
Chemical
Formula
Ca and Cl
H and O
Mg and P
C and O
4. Name the following compounds:
a. NaCl ______________________________
b. Mg3(PO4)2 __________________________
f. Hg2SO4 ____________________________
g. CCl4 ______________________________
c. CaF2 ______________________________
h. Fe(OH)2 ___________________________
d. Sr(ClO3)2 ___________________________
i. (NH4)2O ___________________________
e. P2O5 ______________________________
5. Write the chemical formula for the following compounds:
a. Calcium nitrite _______________________
e. Lead (II) nitrate _____________________
b. Iron (III) chloride _____________________
f.
Potassium iodide____________________
c. Sulphur trioxide _____________________
g. Chlorine Gas ________________________
d. Gold (I) phosphate ___________________
h. Ammonia __________________________
6. For each of the examples below indicate the type of reaction and balance the equation.
a. _____ Mg(OH)2 → _____ MgO + _____H2O
Type of Reaction: ____________________
b. _____ Cl2 + _____NaBr → _____Br2 + _____NaCl
Type of Reaction: _____________________
c. _____Al(NO3)3 + ______Li2CO3 →______ Al2(CO3)3 + ______ LiNO3
Type of Reaction: _____________________
d. _____C7H12 + _____O2 → _____CO2 + _____H2O
e. _____N2 + _____H2 → _____NH3
Type of Reaction: _____________________
Type of Reaction: _____________________
7. Explain the differences between acids and bases:
Property
Acids
Bases
Ion that is present in solution
Reactivity with metals
Reactivity with tissue (skin)
Electrical conductivity
Taste
Feel
pH range
Chemical indicators:
Colour with Phenolphthalein
Colour with Litmus paper
8. What is a mole? What is an organic compound? How would you describe these concepts to a 10 year
old?
9. What is the limiting reagent? How does the limiting reagent affect the reaction?
10. What is the excess reagent? How does the extra excess reagent affect the reaction?
11. What is the percent yield? Is it possible to have a percent yield over 100%? What would this mean?
12. Define an acid and a base according to the Arrhenius theory and the modified Arrhenius theory.
13. Draw the following organic compounds:
a. 3-methylbut-2-ene b. hept-3-yne
c. propyne
d. 4-ethyloctane
14. Predict the organic product of the following reactions:
a. But-2-yne + HBr (excess)
b. Propane + H2SO4
c. Carboxylic acid + alcohol
15. The structure of citric acid is shown to the right. Identify and name
the functional groups.
16. Consider a galvanic cell constructed using the following components:
electrodes  copper and tin
electrolytes  copper(II) nitrate and tin(II) chloride.
In the ensuing redox reaction, tin gets oxidized to tin 2+ ions and copper 2+ gets reduced to copper
atoms.
Use this information to write the two half-reactions taking place in the cell.
17. Determine the states (solid or aqueous) of the following compounds:
a) AgCl
b) CaSO4
c) Na3PO4
d) Mg(OH)2 e) NaNO3
18. Predict the products of the reactions below. Include states. Balance.
a) AlBr3(aq)
+
KOH(aq)

b) CuNO3 (aq) + (NH4)3PO4 (aq) 
c) Li2CO3 (aq) + BaCl2 (aq)

19. Write the total ionic and net ionic equations for the reactions above. Identify the spectator ions.
20. Calculate the pH of the following solutions:
a. [H+] = 1 x 10-4
b. [H+] = 3.64 x 10-9
c. A solution that contains a 2.4 x 10-5 M of H3PO4
21. Calculate [H+]
a. pH = 2.5
c. pH = 7.0
b. pH = 11.9
22. Convert to Moles:
a. 3.01 x 1023 atoms Cl
d. 156.3 grams of lead
b. 12.04 x 1023 atoms Mg
e. 19 000 molecules of KI
23. Convert to Mass in grams
a. 5.0 mol Li
b. 7.5 mol Co
d. 2.67 mol of aluminum oxide
c. 48 grams of aluminum
f. 56.2 grams of Ca(ClO3)2
c. 0.3 mol of bromine gas
e. 7.0 mol NH3
f. 1.8 mol Na2CO3
24. In the following reaction
C3H8 + 5 O2  4 H2O + 3 CO2
a) 17 moles of C3H8 makes how many moles of H2O?
b) 17 moles of H2O are made, how many moles of C3H8 reacted?
c) 3.41 moles of O2 makes how many moles of CO2?
d) 15.9 moles of H2O are made, how many moles of O2 reacted?
e) 142 moles of CO2 are made, how many moles of H2O are made?
f) 1 mole of C3H8 makes how many moles of H2O?
25. Carbon dioxide reacts with lithium hydroxide to produce lithium carbonate and water. What mass of
lithium hydroxide do you need to react with 23 g of carbon dioxide?
26. Lithium nitride reacts with water to form ammonia and lithium hydroxide. If 3.92 g of lithium nitride
reacts with 4.7 g of water, how many grams of ammonia will be created? (You must find the limiting
reagent).
27. Hydrogen peroxide (H2O2) decomposes into hydrogen gas and oxygen gas. If 12.4 g of hydrogen
peroxide is reacted, what is the theoretical yield of oxygen? What is the % yield if 4.5 g of oxygen is
actually produced?
28. Ammonia is created by reacting nitrogen gas with hydrogen gas. During an experiment, 40 g of nitrogen
was reacted with 500 g of hydrogen to produce an actual yield of 0.74 g of ammonia. What is the
percentage yield of the reaction?
29. Determine the concentration of the following solutions:
a. 2 mol of sodium chloride in 1.5 L of water.
b. 15 g of sodium chloride in 0.75 L of water
c. 3 g of magnesium fluoride in a 200 mL aqueous solution
30. Determine the number of moles present in the following solutions:
a. 2 L of 0.5 mol/L CaCl2(aq)
b. 300 mL of 0.4 mol/L Na2(SO4)
31. A stock solution of HCl has a concentration of 12 mol/L. If one were to take 15 mL of stock solution and
make a 500 mL solution, what would the concentration of the solution be?
32. A stock solution of H2SO4 has a concentration of 18 mol/L. How many milliliters of stock solution does
one need to make 250 mL of a 0.4 mol/L solution?
Calculation Solutions:
20a. pH = 4 b. pH = 8.44 c. pH = 4.62
21a. 0.00316 mol/L b. 1.26 x 10-12 mol/L c. 1.0 x 10-7 mol/L
22a. 0.5 mol b. 2 mol c. 1.7791 mol d. 0.7543 mol e. 3.16 x 10-20 f. 0.2715 mol
23a. 34.7g b. 441.98 g c. 47.94 g d. 288.25 g e. 119.28 g f. 107.79 g
24a. 68 mol b. 4.25 mol c. 2.046 mol d. 19.875 mol e. 189.33 mol f. 4 mol
25. 25.04 g
26. 1.482 g
27. 5.83 g, 77%
28. 48.67 g, 1.52 %
29a. 1.33 mol/L b. 0.342 mol/L c. 1576 mol/L
30a. 1 mol b. 0.12 mol
31. 0.36 mol/L
32. 2.56 mL