Download chemistry- sch4u - final exam

CHEMISTRY- SCH4U - FINAL EXAM
Length: 2 hours
Teacher: Mr. Smiley
Total Marks: 110
Student Name:
Instructions:
1. This examination has 7 pages and is divided into 3 parts
2. Initial here_________ to indicate that all 7 pages have been received
3. Pages are double sided make sure that you answer all parts
4. Calculators may be used but not shared
5. A periodic table, Activity series reference, Solubility guidelines, Equilibrium constants and
answer sheet are also provided separate to this exam.
6. Follow all instructions given for each part
Part A: Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question. When finished
Part A, transfer answers to the Answer sheet provided.
____
____
____
____
1. An amine is characterized by what functional group?
a. -CO2CH3
d. -CHO
b. -NH2
e. -CONH2
c. -CO2H
2. When two alcohols undergo a self condensation, what is formed?
a. liquid alcohol
d. an aldehyde
b. a ketone
e. an ether
c. an ester
3.
The correct name for the compound given above is which of the following?
a. 2-methyl-1-butene
d. 3-methyl-2-butene
b. Pentene
e. 2-ethyl-1-pentene
c. 2-ethyl-1-propene
4. Which of the following is a secondary alcohol?
a.
d. CH3OH
b.
c.
e. CH3CH2OH
____
____
5. What results when a primary alcohol is oxidized?
a. an aldehyde
d. an acid
b. an amine
e. no reaction
c. a ketone
6.
The correct name for compound above is which of the following?
a. chloropropylbenzene
c. 1-chloro-3-phenyl-3-propene
b. 3-phenyl-1-choloropropyne
d. 3-chloro-1-phenyl-1-propene
____
____
7.
The correct name for the compound given above is which of the following?
a. 1,3-cyclopentadiene
c. 1,4-cyclopentene
b. 1,4-cyclopentadiene
d. 1,3-cyclopentene
8. The correct structure for 1-methyl-2,4,6-trinitrobenzene(TNT) is which of the following?
a.
c.
b.
____
d.
9. The formula for methyl ethanoate is which of the following?
a.
c.
b.
d.
____ 10. Which type of reaction will an alkene not undergo?
a. Addition
d. dehydration
b. Polymerization
e. hydration
c. Oxidation
____ 11. Which of the following classes of organic compounds does not contain oxygen?
a. Aldehydes
d. ethers
b. Amines
e. amides
c. amino acids
____ 12. The following is an example of what type of reaction?
CH3CH2-CH2-OH
+ HOOC-CH2-CH2CH3 –> CH3CH2CH2-O-COCH2CH2CH3 + H20
a) condensation
b) reduction
c) hydrogenation
d) addition
____ 13. Butane and fluorine gas would react by which of the following?
a. Addition
c. substitution
b. Combustion
d. single displacement
____ 14. The synthesis sequence shown here is best described as which of the following?
1.
2.
3.
a. (1) Dehydration; (2) halogenation; (3) hydrogenation
b. (1) Hydrogenation; (2) dehydration; (3) halogenation
c. (1) Hydrogenation; (2) halogenation; (3) dehydration
d. (1) Halogenation; (2) hydrogenation; (3) dehydration
e. (1) Dehydration; (2) hydrogenation; (3) halogenation
____ 15. In order to determine the identity of an alcohol, a chemist reacts it with excess sulphuric acid, then reacts it
with HCl, and then finally with benzene. A gas chromatograph (an analytical test) determines that
isopropylbenzene has been produced. The identity of the alcohol was most likely which of the following?
a.
c.
b.
d.
____ 16. Amines will not react with which of the following?
a. alkyl halides
c.
b. carboxylic acids
d.
____ 17. The 3p atomic orbital has the shape of
a. a sphere
d.
b. a torus
e.
c. a dumb-bell
Ketones
hydrogen chloride
two perpendicular dumb-bells
an egg
____ 18. In the reaction
+
+
+
+
Which of the following statements is correct?
a.
hydrogen is oxidized and
is the oxidizing agent
b.
hydrogen is oxidized and
is the oxidizing agent
c.
carbon is oxidized and
is the oxidizing agent
d.
manganese is oxidized and
is the oxidizing agent
e.
carbon is oxidized and
is the oxidizing agent
____ 19. Which of the following statements are true for the redox reaction:
+
+
I. the oxidation number of
II.
+
+
changes from +7 to +3
is the oxidizing agent
III.
is oxidized to
IV.
is the reducing agent
V. the oxidation number of
changes from +1 to 0
a. II and IV
d. IV and V
b. I and III
e. III and V
c. II and III
____ 20. Why do energy levels exist in atoms?
a. electrons are negatively charged
b. electrons are attracted to certain numbers of neutrons
c. electrons are able to possess any range of energy
d. electrons will only display certain colours
e. electrons are only able to possess quanta of energy
____ 21. "A region of space in which there is a high probability of finding an electron" is the definition of
a. orbital
d. photon
b. absorption spectrum
e. dipole
c. quantum
____ 22. Which of the following is the electron configuration for the valence shell of oxygen?
a.
d.
b.
c.
e.
____ 23. Which of the following is the electron configuration for magnesium?
a. 1s22s22p8
d. 1s32s32p33s2
3 3
4 2
b. 1s 2s 2p 3s
e. 1s22s22p63s2
2 2
7 1
c. 1s 2s 2p 3s
____ 24. Which of the following is always true of all electrons in the same principal energy level.
a. they possess the same energy
d. all of the above
b. they have opposite spins
e. none of the above
c. they are in identical orbitals
____ 25. Which of the following are properties of alkali metals?
I. They have one valence electron.
II. They have high first ionization energies.
III. They are very reactive.
IV. Their most easily removed electron is in an s orbital.
a. I and II only
d. III only
b. I and IV only
e. I only
c. I, III and IV only
____ 26. Which of the following equations does not represent an oxidation-reduction reaction?
a.
+
+
b.
+
c.
+
d.
+
e.
+
+
+
____ 27. Which atoms could have the valence electron configuration shown below?


 
s
p
a. N3d. Cl12b. O
e. all of the above
c. Ar
____ 28. Which shape and bond angle are predicted by VSEPR theory for H2O?
a. linear, 180o
d. bent, 109.5o
o
b. bent, 120
e. bent, less than 109.5o
o
c. bent, less than 120
____ 29. Experiments were performed with four strips of metals , , , and , and their corresponding nitrate
solutions
,
,
, and
. The following observations were obtained:
A
no reaction
no reaction
no reaction
no reaction
precipitate
no reaction
precipitate
precipitate
precipitate
no reaction
no reaction
no reaction
precipitate
no reaction
precipitate
no reaction
Which of the following is the correct list of the metal ions in order of decreasing strength as oxidizing agents
(strongest oxidizing agent first)?
a.
d.
b.
e.
c.
____ 30. According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as
possible?
a. pairs of valence electrons
d. mobile electrons
b. inner shell electrons
e. lone pairs of electrons
c. bonding pairs of electrons
____ 31. Four pairs of electrons surrounding a central atom will be arranged
a. pyramidally
d. linearly
b. spherically
e. trigonally
c. tetrahedrally
____ 32. What is the correct order of bond polarity of the bonds F-F, H-F and O-F beginning with the least polar?
a. F-F, O-F, H-F
d. H-F, F-F, O-F
b. F-F, H-F, O-F
e. O-F, H-F, F-F
c. H-F, O-F, F-F
____ 33. Which of the molecules, CO2, H2O, NH3, and BF3, will be polar?
a. CO2, NH3 and BF3
d. CO2, H2O and NH3
b. H2O and NH3
e. CO2 and BF3
c. H2O and BF3
____ 34. The following two half-reactions are involved in a galvanic cell:
At standard conditions, what species are produced at each electrode?
a.
is produced at the cathode and
at the anode
b.
is produced at the cathode and
at the anode
c.
is produced at the anode and
at the cathode
d.
is produced at the cathode and
at the anode
e.
is produced at the cathode and
at the anode
____ 35. What would be the shape of a molecule containing a central atom attached to two other atoms with one lone
pair of electrons?
a. linear
d. tetrahedral
b. bent
e. trigonal bipyramidal
c. trigonal planar
____ 36. What would be the shape of a molecule containing a central atom attached to two other atoms with no lone
pairs of electrons?
a. linear
d. trigonal planar
b. bent
e. see-saw
c. trigonal pyramidal
____ 37. What would be the shape of a molecule containing a central atom attached to four other atoms with two lone
pairs of electrons?
a. trigonal planar
d. square pyramidal
b. trigonal pyramidal
e. octahedral
c. square planar
____ 38. In the electrochemical cell above, the left half cell is set up with a zinc electrode in contact with 1.0 mol/L
and the right half-cell is set up with a silver electrode in contact with 1.0 mol/L
.
The relevant reduction potentials are
Which of the following statements is false?
a. the silver electrode is the cathode
b. the zinc electrode is the cathode
c. electrons in the external circuit will flow from zinc to silver
d. the standard cell potential for this cell is 1.56 V
e. the zinc electrode is the anode
____ 39. Which forces exist between amines, R-NH2, molecules?
I. Van der Waals
II. metallic bonding
III. hydrogen bonding
IV. dipole
a. I only
d. I, III and IV only
b. I and IV only
e. I, II and III only
c. I and II only
____ 40. An exothermic reaction is one where
a. heat is transferred from the surroundings into a system
b. heat is transferred from a system into the surroundings
c. kinetic energy is transformed into potential energy
d. there is no transfer of heat
e. none of the above
____ 41. A chemical system in which matter cannot flow into or out of a system is described as
a. a closed system
d. a chemical system
b. an open system
e. none of the above
c. an isolated system
____ 42. Polar covalent bonds occur between
a. atoms which both have equally high electronegativities
b. atoms which have high but unequal electronegativities
c. atoms which both have equally low electronegativities
d. atoms which both have equally low ionization energies
e. atoms which have low but unequal ionization energies
____ 43. Markonikov’s Rule states that when an alkene or alkyne reacts with either a hydrohalide or with water that:
a. the carbon that already had the most H
d. the carbon that has the fewest H atoms
atoms receives the H atom
receives the H atom
b. the H atoms are lost as H2 gas
e. the H atoms combine with O to form
water
c. Markonikov’s Rule does not apply to this
situation
____ 44. In a calorimeter, a 1.0 g sample of magnesium is burned to form MgO. In doing so, 25.5 kJ of energy are
released. What is the Heat of Combustion in kJ/mol of magnesium?
a. 306.2
d. 25.5
25
b. 1.54  10
e. 620
c. 0.0392
____ 45. Which statement concerning the accompanying diagram is true?
a.
b.
c.
d.
e.
H is positive
the system is endothermic
the system releases heat to the surroundings
the heat content of the reactants is less than the heat content of the products
the enthalpy of the products is greater than the enthalpy of reactants
____ 46. When a 'target' reaction can be expressed as the sum of other reactions, the heat of the 'target' reaction is the
sum of the enthalpy changes of the other reactions. This statement is referred to as
a. Smiley’s Law
d. Priestly's Law
b. Law of Conservation of Energy
e. Boyle's Law
c. Hess's Law
____ 47. Given the following thermochemical data:
1. C2H2(g) + 5/2 O2(g)  2CO2(g) + H2O(l) H = –1.30  103 kJ
2. C2H6(g) + 7/2 O2(g)  2CO2(g) + 3H2O(l) H = –1.56  103 kJ
3. H2(g) + 1/2 O2(g)  H2O(l) H = –2.86  102 kJ
What is ΔH for the following reaction?
C2H2(g) + 2H2(g)  C2H6(g)
a. –2.60  101 kJ
d. –5.46  103 kJ
2
b. –3.12  10 kJ
e. 2.60  101 kJ
2
c. –5.72  10 kJ
____ 48. Consider the following equation for the combustion of hydrogen:
H2(g) + 1/2 O2(g)  H2O(g) + 243 kJ
____ 49.
____ 50.
____ 51.
____ 52.
In order to produce 1215 kJ of heat, how many grams of H2 must burn?
a. 12.0 g
d. 0.250 g
b. 0.100 g
e. 8.00 g
c. 10.0 g
The following property can be measured to determine the rate of the reaction
a. change in mass
b. change in colour
c. change in volume
d. change in pressure
e. all of the above depending on the reaction
In the reaction, N2(g) + O2(g)  2NO2(g) , if the concentration changes from 0.45 mol/L to 1.00 mol/L in 2
minutes, what is the overall rate of production of nitrogen dioxide in the system?
a. 3.64 mol/(L·min)
d. 12.6 mol/(L·min)
b. 0.275 mol/(L·min)
e. 0.333 mol/(L·min)
c. 0.137 mol/(L·min)
Which of the following is not a factor that controls the rate of the reaction
a. chemical nature of the reactants
d. surface area
b. concentration of the reactants
e. temperature
c. the number of products formed
The presence of a catalyst is thought to increase the rate of a reaction by
a. changing the products that are formed in the reaction
b. decreasing the enthalpy change of the reaction
c. increasing the enthalpy change of the reaction
d. decreasing the activation energy of the reaction
e. increasing the activation energy of the reaction
____ 53. If for the reaction
, the rate law is determined to be
a. the order of the reaction is 0
b. increasing the concentration of Y will have no effect on the rate
c. increasing the concentration of X will have no effect on the rate
d. increasing the concentration of Y will increase the rate of the reaction
e. there is no way to determine the value of k
, then
____ 54. If for the reaction
, the rate law is determined to be
, then
a. doubling the concentration of Y will double the rate of the reaction
b. halving the concentration of Y will double the rate of the reaction
c. doubling the concentration of X will double the rate of the reaction
d. halving the concentration of X will double the rate of the reaction
e. only changes to the concentration of Y will affect the rate of the reaction
____ 55. Rates of reaction can be explained by
a. atomic theory
d. rate theory
b. collision theory
e. all of the above
c. kinetic molecular theory
____ 56. In the following diagram, the letter which represents the position of the activated complex is:
a. A
d. D
b. B
e. E
c. C
____ 57. If a reaction can be broken down into a reaction mechanism, then the steps of the reaction mechanism are
known as
a. stages of reaction
d. elementary steps
b. activated complexes
e. primary equations
c. reaction progress
____ 58. Consider the above reaction mechanism. The rate-determining step of this reaction is
a. elementary step 1
b. elementary step 2
c. elementary step 3
d. elementary steps 2 and 3
e. impossible to tell from this information
____ 59. Consider the above reaction mechanism. The reaction intermediates are formed in
a. elementary step 1
b. elementary step 2
c. elementary step 3
d. elementary steps 1 and 2
e. impossible to tell from this information
____ 60. Consider the above reaction mechanism. The rate-law equation from this reaction would be
a.
d.
b.
e. impossible to tell from this information
c.
____ 61. The theoretical effect of an increase in the initial concentration of a reactant can be explained in terms of
collision theory because it affects
I. the collision geometry involved in the reaction
II. the total number of collisions that occur
III. the fraction of collisions that are effective
IV. the required activation energy for a reaction
a. both I and IV
d. both III and IV
b. I, II and III are true
e. II only
c. both II and III
____ 62. 1.6 mol of CH3OH(g) are injected into a 4.0 L container and the following equilibrium becomes established.
2H2(g) + CO(g) <=====> CH3OH(g) + 92 kJ
If at equilibrium 0.80 mol of CH3OH is still in the container the Ke must be which of the following?
a. 0.78
d. 0.16
b. 25
e. 6.25
c. 5.0
____ 63. For the equilibrium system below, which of the following would result in a decrease in the quantity of PCl5(g)?
PCl3(g) + Cl2(g) <=====> PCl5(g) + 45 kJ
a. increasing temperature
d. decreasing the size of the container
b. adding some Cl2(g)
e. injecting some He gas
c. decreasing temperature
____ 64. The function of the salt bridge in a galvanic cell is
a. to act as a nonelectrolyte
b. to provide an external circuit for the flow of electrons from one half-cell to the other
c. to provide a path for the migration of ions from one half-cell to the other
d. to allow the solution in each half-cell to become electrically charged
e. to provide a path for the flow of electrons internally from one half-cell to the other
____ 65. Which equilibrium shows an increase in [products] when the volume decreases?
I. 2H2(g) + O2(g) <====> 2H2O(g)
II. Cl2(g) + PCl3(g) <====> PCl5 (g)
III. H2(g) + I2(g) <====> 2HI(g)
IV. 2NH3(g) <====> N2(g) + 3H2(g)
a. I
d. III and IV
b. I and II
e. II
c. IV
____ 66. A concentrated weak acid is best described as which of the following?
a. a solution with a low pH
b. a solution where the concentration of undissociated acid particles is low compared to the
concentration of hydronium ions
c. a solution where the concentration of hydronium ions is large compared to the
concentration of undissociated acid particles
d. a solution with a high pH
e. a solution where the concentration of undissociated acid particles is high and the relative
quantity of hydronium ions is small
____ 67. The Ksp for a substance A2B is 1.2  10-12. The [B] must be which of the following?
a. 4.0  10-11
d. 1.3  10-4
-12
b. 3.6  10
e. 2.6  10-4
-5
c. 6.7  10
____ 68. Which of the following salts acts like an acid when added to water?
a. ammonium nitrate
d. both a and b
b. potassium nitrite
e. both a and c
c. iron(III) nitrate
____ 69. In the reaction
+
+
+
+
Which of the following statements is correct?
a.
is the reducing agent, and
is the oxidizing agent
b.
is the reducing agent, and
is the oxidizing agent
c.
is the reducing agent, and
is the oxidizing agent
d.
is the reducing agent, and
is the oxidizing agent
e.
is the reducing agent, and
is the oxidizing agent
____ 70. The oxidation number of chromium (
a. +2
b. +4
c. +6
) in the dichromate ion (
d. +7
e.
) is
Please answer the following on the foolscap provided.
Part B: Short Answer (11 marks)
71. Using Quantum Theory to explain give the stable ions that Zn and Pb can form. (4)
72. Explain the following lab results. (3)
Alcohol
Butanol
2-butanol
2-methyl-2-propanol
Reaction with KMnO4
Reaction
Reaction
No Reaction
73. Using ethane, ethene, and ethyne as example molecules state the order of their reactivity and state reasons for
the order that you have given. (4)
Part C: Problems (29 marks)
74.
Balance the following redox reaction that takes place in a basic solution using the half-reaction method: (5)
NO3-1 (aq) + Al (s)  NH3(aq) + Al(OH)4-1(aq)
75. Barbituric acid, (H-Bar), was discovered by Adolph von Baeyer and named after a friend Barbara. It is the
parent compound of a widely used sleeping drug, the barbituates. It is a weak acid with a Ka of 9.7 x 10-5.
What is the [H+], the pH, and the [OH-] of a 0.05 mol/L solution of H-Bar? (6)
76. Write the balanced chemical equation for the double displacement reaction of calcium nitrate and sodium
carbonate. Predict the concentration of calcium and carbonate ions at equilibrium. (6)
77. Use the following data to calculate the reaction rate law and the rate law constant for the system (6)
Experiment
NO (mol/L)
H2 (mol/L)
Initial Rate of Reaction (mol/(L·s))
1
0.001
0.004
0.002
2
0.002
0.004
0.008
3
0.003
0.004
0.018
4
0.004
0.001
0.008
5
0.004
0.002
0.016
6
0.004
0.003
0.024
78. Design a reaction pathway to produce N-methyl butanamide from methane and butanol using any catalysts
and inorganic materials that you would like. (6)