Download SCH4C: Chemistry, Grade 12, College Preparation

SCH4C – CAT
The CAT for this course is worth 5% of your final grade. Due Date: Exam Day (June 22, 2015) FYI Exam Sections:
Matter & Qualitative Analysis
Chemical Calculations
Organic Chemistry
Electrochemistry
Chemistry & The Environment
TOTAL:
37 marks
27 marks
32 marks
35 marks
18 marks
149 marks
Name: ____________________
37 minutes
27 minutes
32 minutes
35 minutes
19 minutes
150 minutes
Part A: Multiple Choice Questions
1. Which of the following is considered an inference from an observation?
a. The precipitate was yellow.
b. The metal sank in the water, it must be iron.
c. A gas was released when lithium was dropped into water.
d. Bubbles form from Alka-Seltzer tablets.
2. Which of the following is considered an observation?
a. The cloudy white liquid.
b. The man wore a hard hat so he must be a construction worker.
c. When copper metal is placed in a flame, it reacts with oxygen.
d. The flame colour of sodium is yellow.
3. The process by which an unknown substance is identified is called
a. quantitative analysis
c. deductive reasoning
b. qualitative analysis
d. spectroscopy
4. An element may have more than one atomic mass depending on which particular
isotope it is. This is due to:
a. varying numbers of protons
b. varying numbers of electrons
c. varying numbers of neutrons
d. heavier protons in the heavier isotopes
5. The line spectrum observed when an element is excited by flame or electricity is a result
of:
a. a quanta of energy released by moving electrons
b. electrons undergoing transitions
c. the absorption and release of energy
d. all of these
e. none of these
6. Which of the following is covalently bonded?
b. NaCl
a. NiF2
c. CH4
7. Which of the following is ionically bonded?
a. NaOH
b. Na metal
c. N2
d. CH4
8. What happened to aluminum to form Al
a. aluminum gained three protons
b. aluminum lost three protons
c. aluminum lost three electrons
d. aluminum gained three electrons
3+
d. NaOH
ion?
9. To which of the following elements will fluorine most likely form an ionic bond?
a. calcium
c. bromine
b. oxygen
d. boron
10. Which type of bond is present in CH4?
a. ionic
b. pure covalent
c. polar covalent
d. metallic
11. Which type of bond is present in BrCl5?
a. ionic
b. pure covalent
c. polar covalent
d. metallic
12. An atom will lose or gain electrons to become isoelectronic with a Noble gas and will be
stable. This is another way of stating which rule?
a. crisscross
c. octet rule
b. conservation of mass
d. There is no rule.
13. One reason that oxygen could not possibly be used as the backbone of organic
molecules is because:
a. It is so reactive; it forms double bonds with itself.
b. It is a solid at room temperature.
c. It has a low electronegativity.
d. It has seven valence electrons.
14. Carbon is the backbone of organic molecules because:
a. It forms four bonds.
b. It has a low electronegativity.
c. It is relatively stable.
d. It can form chains with itself and still have room for other atoms.
e. all of these
15. Which of the following functional groups would characterize a ketone?
16. Which of the following formulas would be an alkene?
c. C3H8
a. C3H6O
d. C3H6
b. C3H4
17. Which of the following would be an aldehyde?
18. Alkanes differ from alkenes in that alkenes are:
a. unsaturated
b. have only single bonds joining the carbon backbone together
c. have chlorine, fluorine, or bromine in their structure
d. have exactly 2n+2 hydrogens in any carbon backbone of length n
19. The combustion of 2-methyl-propanol will produce
a. alcohol and water
c. oxygen and water
b. carbon dioxide
d. carbon dioxide and water
20. The reaction between a carboxylic acid and an alcohol will produce
a. an ester
c. a polymer
b. an ether
d. an aldehyde
21. Which of the following is an alcohol?
a. 2-methylpropan-1-ol
b. 2-methylpropanal
22. A
a.
b.
c.
d.
c. 2- methylpropanal
d. 2-methylpropanoic acid
distillation is a lab technique used to:
separate solids based on melting points
separate gases by condensing them
separate liquids based on the energy required to overcome intermolecular forces
separate liquids based on their polarity
23. Which substance has gained three electrons?
a. Cu 2+
b. Al 3+
c. P 3d. F 1-
24. Which substance has lost 2 electrons?
a. Cu 2+
b. Al 3+
c. Al
d. Cl1-
25. Which substance is not an element?
a. Cu
b. Al 3+
c. H2
d. Cu
26. Which substance is not a compound?
a. CuCl2
b. O2
c. Na2O
d. CH4
27. Which substance is not considered a pure substance?
c. kool-aid
a. sugar (made up of C6H12O6)
b. lead piping
d. oxygen
28. Which of the following would be considered a solution?
a. brass
c. sand
b. vinegar and oil salad dressing
d. copper wire
29. The name of CuHSO3 is:
a. cuprous hydrogen sulphite
b. cupric sulphate
c. cuprous hydrogen persulphite
d. copper (I) hydrogen sulphate
30. The name of Fe2(C2O4)3 is
a. ferrous carbonate
b. iron (II) oxalate
c. iron (III) oxalate
d. ferrous oxalate
31. The name of P2O7 is:
a. phosphorous heptoxide
b. diphosphorous heptoxide
c. phosphorous hexoxide
d. diphosphorous oxide
32. The formula for cobalt (II) chlorate is:
a. Co2(ClO4)3
b. Co2(ClO3)3
c. Co(ClO2)3
d. Co(ClO3)2
33. The number 6.02 x 10 23 describes which of the following:
a. the number of grams in a mole
b. the number of moles in a reaction
c. the number of anything in a mole
d. the number of atoms in a molecule
34. The mass of Na = 23.0 g. This is
a. sodium’s atomic mass
b. sodium’s molar mass
35. To
a.
b.
c.
c. sodium’s formula mass
d. sodium’s density
which family of organic compounds does CH3COCH2CH2CH3 belong?
alcohol
d. ketone
aldehyde
e. carboxylic acid
alkyne
36. Name the following compound:
a. 4-ethyl-3-methylheptane
b. 4-methyl-3-propylhexane
c. 3-propyl-4-methylhexane
d. 4-ethyl-3-methylhexene
e. 3-ethyl-4-propylheptane
37. Which of the following is not considered a pollutant?
a. sulphur dioxide
c. nitrogen dioxide
b. nitrogen
d. VOCs
38. Which class of organic compounds does not contain a carbon-oxygen double bond?
a. esters
c. alcohols
b. ketones
d. carboxylic acids
39. Which molecule is polar?
a. carbon dioxide
b. ethanol
c. propane
40. Which organic compound is unsaturated?
a. methylcyclopentane
b. 2-methyl-3-ethylpentyne
d. carbon tetrachloride
e. butane
c. 1,1-dimethylhexane
d. cyclohexane
41. What does the boiling point of a hydrocarbon family do with increasing carbon length?
a. The boiling point increases.
b. The boiling point remains relatively the same.
c. The number of intermolecular attractions increases.
d. The boiling point decreases.
42. Which of the following molecules would you expect to be a liquid at room temperature?
c. C2H5OH
a. C29H58
d. Cl2
b. C2H6
Part B: Matching - you may not use all options!
Complete the sets of matching questions.
1. Match each term with its correct definition shown below.
1. cannot be broken down further _____
2. can be separated by physical properties _____
3. the number of electrons in the outer shell _____
4. does not dissolve in water _____
5. the ability to attract electrons _____
6. the equal sharing of electrons _____
7. conducts electricity _____
8. the temperature where a liquid turns to a gas _____
a. electronegativity b. insoluble c. soluble d. electrolyte e. boiling point f. element
g. valence electrons h. covalent bonding i. ionic bonding j. mechanical mixture
2. Match each term with its correct definition shown below.
1.
2.
3.
4.
5.
6.
7.
8.
relatively small quantity of solute per unit volume of solution _____
forces that hold molecules close to one another _____
specific attraction within a molecule (ionic or covalent bonds) _____
separation of ions as an ionic compound dissolves in water _____
relatively large quantity of solute per unit volume of solution _____
bonds that have a slightly positive and negative charged end _____
compounds that don’t mix with water _____
compounds that will mix with water _____
a. intramolecular b. intermolecular
dissociation g. dilute h. ionic
c. polar
d. nonpolar
e. concentrated
f.
3. Match each term with its correct definition shown below.
1.
2.
3.
4.
5.
6.
7.
8.
quantity of a given solute in a solution _____
substance doing the dissolving _____
measures moles of hydrogen per litre _____
unit used for very low concentrations _____
amount of solute, in moles, dissolved in one litre of solution _____
mass of solute in volume of solution _____
concentration expressed as solute volume in solvent volume _____
substance being dissolved _____
a. % V/V b. solvent c. % M/V d. concentration e. molar concentration f. pH g.
solute h. ppm
Part C: Short Answer
1. Draw Bohr-Rutherford or Lewis atomic structures for the following atoms and state the
number of bonds each atom can form.
a. Cl
b. P
2. Draw the Lewis molecular structure for each of the following.
b. CS2
c. CCl4
a. NH3
3. Complete the following table by writing the name or formula for the substance and
identifying the type of substance.
Name
1
2
3
4
5
6
7
8
nickel (II) phosphate
chlorine
dinitrogen tetroxide
Formula
S3Br6
NaHCO3
Type: ionic or covalent
MgF2
Al2(C2O4)3
Fe(OH)3
4. Balance the following equation and state the type of reaction
a. __ H2C2O4 + ___ NaOH
b. ___Bi2O3 + ___ H2
___Na2C2O4 + ___ H2O
___ Bi + ___ H2O
c. __ Al2(SO4)3 + ____ NH3 + ___ H2O
____ Al(OH)3 + ___ (NH4)2SO4
Type:
Type:
Type:
d. List the types of reactions not covered in this question and provide examples!
5. Write balanced chemical equations for each of the following reactions. [10 marks]
a. Complete combustion of butane (C4H10)
b. Sulphuric acid + potassium hydroxide Æ
6. Complete the equation. Use the solubility rules to determine if a precipitate forms.
Then complete a-c:
+ ____KI (aq) Æ
____Pb(NO3) 2 (aq)
a. Total ionic equation:
b. Spectator ions _________________________________________
c. Net ionic equation
7. Draw structures or provide names for following molecules.
a. 3-methylheptane
b. 4,4-dibromo-1-chloropentan-2-one
c. 3,3-dichloro-2-methylnon-4-ene
d. 3-ethyl-3-methyl-pentanal
e. 2-chloro-5,5-diethyloctan-4-ol
f.
3,4-dimethyl hexy-1-ne
g. 3-methylhxanoic acid
h. methyl ethyl ether (methoxy ethane)
i.
ethyl butanoate
O
O
OH
O
O
OH
Cl
O
O
8. What are the two types of polymers? What are the similarities and differences? What
are crosslinks and how do they help with the strength of polymers?
9. Discuss the following:
a. Organic solvents; their use and the dangers of their use
b. The pH scale and the properties of acids and bases
c. Corrosion and the 4 factors that affect it.
d. Why plastics are bad for the environment
e. Applications of electrochemistry
Part D: Calculations
1. Determine the molar mass of Ca3(PO4) 2.
2. Determine the molar mass of CaCO3.
3. Determine the number of moles in each of the following:
a. 100.0 g of NaCl
b. 8.43 x 10
22
molecules of chlorine
4. Determine the number of molecules present in each of the following:
a. 45.0 g of sodium phosphate
b. 525 molecules of ethane
5. A solution of cupric sulphate is used at blood donor clinics to test donor blood for low
iron. Calculate the molar concentration of this solution, if 125 g of CuSO4 crystals are
dissolved in 900.0 mL of water.
6. D5W is an intravenous solution used as a fluid and nutrient replenisher for patients and
is basically just sugar and water mixed together. As a hospital pharmacist, you need to
make 750 mL of this solution with a concentration of 0.30 mol/L. What mass of
glucose, C6H12O6, will you need to dissolve in water?
7. Determine the % concentration (be sure to state the type w/w, w/v, v/v)
a. 5 g of silver in 25 g of iron
b. 6.7 mL of vinegar in 108.5 mL of water
c. 44.5 g of salt in 130 mL of water
8. Determine the concentration in ppm for 116 grams of KF is dissolved in enough water to
make 4 L of solution.
9.
a. What volume of a 17.4 mol/L acetic acid stock solution is required to make 2.0 L
of a 1.5 mol/L acetic acid solution?
b. What is the pH of the initial solution if the [H+] concentration is 1.77 x 10-2
mol/L?
c. What is the pH of the diluted solution if the [H+] concentration is 5.2 x 10-3
mol/L?
10. If 74.5 g of ammonium nitrate was the actual amount obtained in a reaction for which
the theoretical yield was 88.0 g, determine the percentage yield.
11. When 30.0 g of sodium hydroxide is mixed with excess magnesium nitrate according to
the equation: Mg(NO3)2 + 2NaOH Æ Mg(OH)2 + 2NaNO3
a. Determine the theortetical yield of Mg(OH)2
b. Determine the percent yield of the reaction if 16.0 g of magnesium hydroxide is
collected.
12. A sugar contains 39.95% C, 6.71% H, and 53.34% O, by mass.
a) Determine its Empirical Formula
b) If the molar mass of glucose was found experimentally to have a molar mass of 180.0 g/mol,
calculate its Molecular Formula.
13. Redox Reactions:
a. Assign oxidation numbers to ALL elements in the following compounds:
i. CuOH
iii. CaBr2
ii. Na2SO4
iv. CO32-
b. Which of the following are redox reactions? Explain how you know.
i. CuCl2(aq) + Al(s) Æ Cu(s) + AlCl3(aq)
ii. H2O(l) + CO2(g) Æ H2CO3(aq)
c. Classify the following half-reactions as either oxidation or reduction reactions.
EXPLAIN your answer
i. 2 Cl
Æ Cl2(g) + 2 e-
ii. Sn4+ + 2 e- Æ Sn2+
d. Balance the following redox reactions using the half reaction method:
2+
3+
i. Mn
+ BiO3 Æ MnO4 + Bi
ii. P + Cu
2+
Æ Cu + H2PO4
–
iii. PH3 + I2 Æ H3PO2
-
+ I
-