SCH3U – Review for Units 1-4.
Part A:
1. Draw structural diagrams (Lewis Diagrams) for the following (2 mark each, total of 4 marks):
a)
SiCl4
b)
PCl3
2. Five elements from the same period are found to have the following properties:
Element Atomic Radius (pm)
1st Ionization Energy (kJ/mol)
A
125
900
B
77
1086
C
134
520
D
69
2081
E
71
1681
a) Which of these elements is an alkali metal?
____________
(1 mark)
b) Which of these elements is an alkaline earth metal?
___________
(1 mark)
c) Which of these elements is a halogen?
____________
(1 mark)
d) Which of these elements is a noble gas?
____________
(1 mark)
3. In the space provided, write the name of the type of reaction for each of the following
(1 mark each, total of 3 marks):
a)
Mg (s) + 2HCl (aq)  H2 (g) + MgCl2 (aq)
_________________________
b)
CaCO3 (s)  CaO (s) + CO2 (g)
_________________________
c)
LiBr (aq) + AgNO3 (aq)  AgBr (s) + LiNO3 (aq)
_________________________
4. Write the correct formula for each of the following compounds (1 mark each, total of 4 marks):
a)
carbon monoxide
____________________
b)
potassium oxide
____________________
c)
iron (II) perchlorate
____________________
d)
lead (IV) phosphate
____________________
5. Write the correct IUPAC (written) name for each of the following compounds
(1 mark each, total of 4 marks)
a)
NO
____________________
b)
SF6
____________________
c)
SnF2
____________________
d)
H3PO4 (aq)
____________________
6. Calculate the pOH of a solution with a hydrogen ion content of 0.00075 mol/L. (3 marks)
7. Answer the following questions using the graph below:
a)
At what temperature does KClO3 become less soluble than
Ce2(SO4)3 ______________ (1 mark)
b)
How many grams of NH4Cl can be dissolved in 500 ml of water
at 70°C? Show your work. (3 marks)
c)
Which substances decrease in solubility as water temperature
increases? (1 mark)
8. If 4.45 grams of solid iron and 8.52 grams of chlorine gas chemically combine to form solid
iron (III) chloride:
a)
Write the BALANCED reaction for these two reactants in the space below. Include the phase symbols!
(1 mark)
b)
Identify the limiting reagent. SHOW YOUR WORK (3 marks)
c)
What mass of iron (III) chloride will be produced from the above quantities of reactants? Show your
calculations, and be certain to include units and the correct number of significant digits.
(3 marks)
d)
If 12.15 g of iron (III) chloride forms, calculate the percentage yield (2 marks).
9. Predict the products and write a balanced chemical equation for the following chemical reaction:
Copper wire is added to an aqueous solution of silver nitrate to recover the silver. (3 marks)
10. Calculate the number of moles of lead present in 8.6
17
atoms of Pb. (2 marks)
11. A compound was found to contain 10.06% C, 89.10% Cl, and 0.84% H, by mass. If the molar mass of the
compound is 119.6 g/mol, calculate its molecular formula. (3 marks)
Part B:
Answer all of the following questions by selecting the answer which is most correct.
(1 mark each)
1. Alkaline earth metals have the following number of valence electrons:
a)
1
b)
2
c)
3
d)
7
e)
8
2. During an experiment, a scientist gathers the following information: Mass of NaOH used = 1.507g,
volume of 0.103 mol/L HCl used: 149.76 mL, and final solution volume = 12.002 L. The FINAL ANSWER
should have how many significant digits?
a)
1
b)
2
c)
3
d)
4
e)
5
3. Which of the following elements has the largest atomic radius?
a)
F
b)
Al
c)
Mg
d)
Ca
e)
Rb
4. When magnesium ions and chloride ions combine, the formula of magnesium chloride will be:
a)
MgCl
b)
MgCl2
c)
Mg2Cl
d)
MgCh2
e)
MgCh
5. Which of the following reactions is a DOUBLE DISPLACEMENT reaction?
a)
CaO (s)  Ca (s) + O2 (g)
b)
CH4 (g) + 2O2 (g)  2H2O (g) + CO2 (g)
c)
BaCl2 (aq) + Na2CO3 (aq)  BaCO3 (s) + 2 NaCl (aq)
d)
2Al (s) + Fe2O3 (s)  2Fe (l) + Al2O3 (s)
e)
KOH (aq) + HCl (aq)  KCl (aq) + H2O (l)
6. In order to properly balance the following equation, what coefficients would be needed?
__C2H6 + __ O2  __ CO2 + __ H2O ?
a)
1, 2, 3, 3 respectively
b)
1, 3, 2, 3 respectively
d)
2, 5, 6, 8 respectively
e)
3, 6, 9, 12 respectively
c)
2, 7, 4, 6 respectively
7. What is the mass of 0.25 moles of hydrogen gas?
a)
0.25g
b)
0.50g
c)
1.0g
d)
2.0g
e)
4.0g
8. Nitrogen and oxygen combine to form nitrogen dioxide according to the following reaction:
N2 (g) + 2O2 (g) 2 NO2 (g)
If 14.0 g of nitrogen reacts with excess oxygen, and 40.0 g of NO2 are formed, what is the % yield?
a)
14.0%
b)
40.0%
c)
50.0%
d)
77.0%
e)
86.9%
9. If 0.135 moles of Na3PO4 are dissolved in 135.0 mL of water, what will be the molar concentration of the
solution?
a)
0.00100 mol/L
b)
0.0100 mol/L
c)
0.100 mol/L
d)
1.00 mol/L
e)
none of the above answers is correct
10. If 350 mL of a 0.50 mol/L solution of Ca(NO3)2 is added to 150 mL of water, what will be the final
concentration of the solution?
a)
3.5 x 10-5 mol/L
b)
3.5 x 10-4 mol/L
c)
3.5 x 10-3 mol/L
d)
3.5 x 10-2 mol/L
e)
3.5 x 10-1 mol/L
11. A compound has a molar mass of 170.0 g/mol and empirical formula of SiF3. The compound’s molecular
formula is
a)
SiF3
b)
Si4F12 c)
Si5F15
d)
Si3F9
e)
Si2F6
12. What is the molar concentration of 0.20 mol of potassium hydroxide in 0.75 L of solution?
a)
0.37 mol/L
b)
3.75 mol/L
c)
2.66 mol/L
d)
0.27 mol/L
e)
0.17 mol/L
13. Converting 153.0 g of Mg(CN)2 into moles yields approximately:
a)
0.98 mol
f)
2.00 mol
b)
1.49 mol
c)
2.53 mol
d)
3.06 mol
14. The number of valence electrons in a fluorine atom is
a)
`
1
b)
3
c)
5
d)
15. Examine the following 1st, 2nd, and 3rd ionization energies.
Element X
Element Y
Element Z
1st
(eV)
5.139
7.646
21.564
Element X is most likely a
a. Group 1 element
b. Group 2 element
c. transition metal
2nd
(eV)
47.286
15.035
40.962
3rd
(eV)
71.64
80.143
63.45
d. Group 17 element
e. noble gas
7
e)
9
16. Upon analysis in the lab, a compound is found to consist of 2.2% hydrogen, 26.7% carbon, and 71.1%
oxygen. The empirical formula for this compound is
a. H2C2O4
d. HCO2
b. HCO
e. HC2O2
c. HC2O
17. Based on the solubility rules, which of the following is insoluble?
a. CaCl2
d. (NH4)2CO3
b. Fe(NO3)3
e. PbBr2
c. LiBr
Part D:
Write the IUPAC name or the chemical formula for each compound
1. LiBr
16. aluminum nitride
2. SO2
17. sodium oxide
3. NH4Cl
18. phosphorus trifluoride
4. Na2SO4H20
19. water
5. Al2(CO3)3
20. ammonium phosphide
6. Mg(ClO3)2
21. calcium phosphate
7. N2O3
22. lithium sulphite
8. Cu(NO3)2
23. nickel (II) hydroxide
9. Ni(OH)3
24. lead (II) nitrite
10. BeCl2·H2O
25. sodium carbonate
11. Ca3(PO4)2
26. copper (II) nitride
12. FeCl3
27. potassium sulphate
13. BeCl2
28. barium oxide
14. CaC2
29. lead (IV) oxide
15. Cu(NO2)2
30. carbon monoxide