Download AVOGADRO EXAMS 1991 - 2002 PRACTICE BOOKLET

AVOGADRO EXAMS
1991 - 2002
PRACTICE BOOKLET
THE QUESTIONS CONTAINED IN THIS FILE ARE TAKEN FROM PAST
EXAM BOOKLETS. QUESTIONS DELETED FROM THE EXAMS HAVE
BEEN OMIITED FROM THIS FILE AND IN SOME CASES THE
QUESTIONS HAVE BEEN EDITED FROM THERE ORIGINAL FORMAT
Answer grids are found at the end of this booklet
1991
1.
In the metric system the multiple 1/102 is represented by the prefix
(a) milli (b) micro
(c) deci
(d) kilo
(e) centi
2.
During an experiment, five groups of students tried to measure the same electric current and
obtained the following results. Which group had the most precise results?
(a) Group A: 126 mA, 130 mA, 115 mA, 110 mA
(b) Group B: 131 mA, 129 mA, 130 mA, 130 mA
(c) Group C: 140 mA, 130 mA, 140 mA, 150 mA
(d) Group D: 120 mA, 115 mA, 140 mA, 150 mA
(e) Group E: 135 mA, 130 mA, 120 mA, 125 mA
3.
The vapor pressure of a liquid does not depend upon
(a) the purity of the liquid
(b) the temperature of the liquid
(c) the atmospheric pressure on the liquid
(d) the chemical composition of the liquid
(e) the extent of the hydrogen bonding in the liquid
4.
Which molecule or ion does NOT have the same shape as CH4?
+
-1
-1
-2
-1
(a) NH
(b) BF
(c) ClO
(d) SO
(e) PF
4
4
4
4
4
5.
Which molecule has the greatest bond dissociation energy?
(a) H2
(b) F2
(c) N2
(d) O2
(e) Cl2
6.
Compared to the electron, a neutron has
(a) the opposite charge and about the same mass
(b) the same charge and is much lighter
(c) the opposite charge and is much lighter
(d) the same charge and about the same mass
(e) no charge and is much heavier
7.
The figure below represents which molecule?(Non-bonding electron pairs are shown as two dots;
bonded atoms are connected by a solid line.)
(a) BrF3 (b) BF3
8.
(c) SO3
Chlorine in ClO2 has an oxidation number of
(a) 0
(b) +1
(c) +2
(d) +3
Last Revised by D Lougheed 00/7/3
(d) CHCl3
(e) XeO3
(e) +4
Page 2
9.
What volume does 11 kg of carbon dioxide occupy at standard temperature and pressure?
(a) 5.6 x 103 L (b) 246 m3
(c) 11 L
(d) 0.25 L
(e) 0.22 m3
10. In which closed container is the pressure greatest?
1 mol
Hydrogen
1 mol
Oxygen
1 mol
Argon
1 mol
Methane
CH
4
2 mol
Hydrogen
1L
273 K
1L
273 K
1L
273 K
2L
473 K
3L
373 K
Container A
Container B Container C
(a) Container A
(d) Container D
Container D
(b) Container B
(e) Container E
Container E
(c) Container C
11. The pressure of a gas is a direct measure of
(a) the hydrogen bonding between molecules
(b) the average speed of the molecules
(c) the force exerted per unit are on the walls of the container
(d) the shape of the molecules
(e) the size of the molecules
12. In the apparatus below(valve closed). 1/00 mol of oxygen is held at 100 kPa in a volume of 50.0 L.
As well, 2.00 mol of nitrogen at 200 kPa exists in a volume of 50.0 L. What is the total pressure
after the valve between the two containers is opened? The temperature is held constant.
1.00 mol
Oxygen
Nitrogen
50.0 L
50.0 L
100 kPa
(a) 67 kPa
2.00 mol
(b) 100 kPa
200 kPa
(c) 150 kPa
(d) 200 kPa
(e) 300 kPa
13. What is the correct formula of the stable compound that contains only calcium and phosphate ions?
(a) Ca2(PO 4)3 (b) CaPO4
(c) Ca(PO4)3 (d) Ca3(PO 4 )2
(e) Ca3PO 4
14. In a well insulated container, an endothermic chemical reaction takes place. When the reaction is
done, the temperature of the reaction will
(a) be higher than before the reaction began
(b) be higher or lower than at the start of the reaction, depending on the molecular masses involved
(c) be independent of the heat capacities of the substances involved
(d) be the same as before the reaction began
(e) be lower than before the reaction began
Last Revised by D Lougheed 00/7/3
Page 3
15. Which of the following oxides is the most basic?
(a) N2O5
(b) P4O10
(c) CaO
(d) CO2
(e) Cl2O7
16. An element occurring in nature as a metal(such as copper or gold) is likely to
(a) react readily with oxygen to from a protective oxide coating
(b) be at the high end of the activity series of metals
(c) cause strong acids to release hydrogen gas
(d) undergo oxidation only with difficulty
(e) lose some of its valence electron easily
17. Sodium thiosulphate(photographer’s hypo) reacts on film to
(a) coat the film with a protective layer to prevent further silver loss
(b) complex the sensitized silver bromide grains, thus fixing them in position
(c) dissolve silver bromide and remove it from the film
(d) precipitate black elemental silver form silver bromide
(e) reduce sensitized silver bromide to elemental silver, thus revealing the black image
18. Fission of a uranium-236 nucleus produces one krypton-92 nucleus and one barium-141 nucleus.
How many neutrons are also produced?
(a) zero (b) one
(c)O two
(d) three
(e) four
19. Three moles of ammonium nitrate contain how many moles of nitrogen atoms?
(a) three (b) six (c) nine
(d) eighteen (e) twenty-seven
20. Select the compound which contains the greatest percentage by mass of nitrogen
(a) HNO 3
(b) Mg3N2
(c) N2O5
(d) N2O
(e) NH3
21. A compound of sodium and oxygen alone has a composition of 59% sodium by mass. What is the
empirical formula for the compound?
(a) NaO
(b) NaO2
(c) Na2O
(d) Na2O2
(e) Na2O3
22. Hydrogen burns in oxygen and water is produced. If 4.0 mol of hydrogen is burned with 6.0 mol of
oxygen and the reaction is as complete as possible, how many moles of the excess, non-limiting
reactant are left at the end of the experiment?
(a) 2.0 mol
(b) 3.0 mol
(c) 4.0 mol
(d) 6.0 mol
(e) 10.0 mol
23. How many moles of barium hydroxide are in a sample that titrates to neutrality when 100 mL of
0.050 M HCl is added?
(a) 0.0025 mol (b) 0.0050 mol
(c) 0.0100 mol
(d) 0.0150 mol
(e) 0.200 mol
24. Lime juice is about 100,000 times more acidic than neutral water. What is the approximate pH of
lime juice?
(a) 1.0
(b) 2.1
(c) 3.2
(d) 4.0
(d) 5.5
Last Revised by D Lougheed 00/7/3
Page 4
25. Four different solid substances are observed in nearly saturated aqueous solutions:
- Substance 1 is more soluble in cold water than in hot water
- Substance 2 is more soluble in hot water than in cold water
- Dissolving substance 3 cools the solution
- Dissolving substance 4 warms the solution
Which substances dissolve endothermically?
(a) Substances 1 and 2 only
(b) Substances 2 and 3 only
(c) Substances 3 and 4 only
(d) Substances 1 and 3 only
(e) Substances 2 and 4 only
26. To 300 mL of 0.230 M magnesium nitrate solution, 200 mL of water is added. What is the final
concentration of the nitrate ions?
(a) 0.460 M
(b) 0.276 M (c) 0.184 M (d) 0.138 M (e) 0.092 M
27. Which substance is a non-electrolyte in aqueous solution?
(a) copper(II) sulphate (b) nitric acid (c) carbon dioxide
(d) sodium hydroxide (e) sucrose
28. Identify all the spectator ions in the following reaction;
Pb(NO 3)2(aq) + 2 KI (aq) → PbI2(s) + 2 KNO3(aq)
2+
(a) Pb (aq), NO 3-1(aq) and I-1(aq)
(b) Pb2+(aq) and I-1(aq)
(c) NO3-1(aq) and K+ (aq)
(d) K+(aq)
(e) Pb2+(aq) and K+ (aq)
29. What is the molarity of a solution prepared by dissolving 3.4 g of NH3 in enough water to make 2.0
L?
(a) 0.10 M
(b) 0.20 M
(c) 0.34 M
(d) 0.40 M
(e) 0.68 M
30. Is a sulphuric acid solution has a density of 1.29 g/mL and is 38% by mass sulphuric acid, what is
its molar concentration?
(a) 0.38 M
(b) 0.49 M
(c) 0.98 M
(d) 5.0 M
(e) 10.0 M
31. Avogadro’s Principle led to the idea that
(a) the average kinetic energy of all gases is the same at the same temperature
(b) volume depends upon the number of moles of gas present, when temperature and pressure are
constant
(c) pressure and volume of gases are inversely proportional at constant temperature
(d) the average velocity of gas molecules is proportional to the Kelvin temperature
(e) gaseous volume is directly proportional to molecular size, temperature and pressure being
constant
Last Revised by D Lougheed 00/7/3
Page 5
32. Which graph correctly displays the product PV as a function of T for one mole of an ideal gas?
0
0
T
0
0
0
(a)
T
(b)
0
T
0
(c)
0
0
T
0
(d)
T
(e)
33. As zinc metal reacts with dilute aqueous sulphuric acid, the products are
(a) aqueous zinc sulphate and oxygen gas
(b) zinc hydroxide and sulphur trioxide
(c) zinc hydride and sulphur dioxide
(d) aqueous zinc sulphate and hydrogen gas
(e) zinc sulphide and water
34. What is the anhydride of HNO3?
(a) N2
(b) NO
(c) NO2
(d) N25
(e) N2
1992
1.
One atom of the isotope
(a) ten
2.
(b) seven
7
Li contains how many neutrons?
3
(c) six (d) four
(e) three
Which of the following has the least ionic character?
(a) aluminum chloride
(b) calcium chloride
(d) magnesium chloride
(e) rubidium chloride
(c) sodium chloride
3.
Which of the following is the poorest electrical conductor?
(a) aqueous hydrogen chloride (b) graphite
(c) molten sodium bromide
(d) nickel metal
(e) anhydrous calcium chloride
4.
The relative atomic mass of 32S is 31.9721 u with a 95.02% abundance. Natural sulphur has a
relative atomic mass of 32.066 u. The other main isotope of sulphur has a mass number of
(a) 31
(b) 32
(c) 33
(d) 34
(e) 35
5.
Ionic peroxides contain the ion
+1
-1
(a) O2- (b) O-1 (c) O
(d) O
2
2
6.
(e) O
-2
2
The mass of 0.457 L of pure Br 2 at 25°C is 1.427 kg. What is the density of bromine?
(a) 0.3203 kg/L
(b) 0.652 kg/L
(c) 1.533 kg/L
(d) 3.123 kg/L
(e) 4.08 g/L
Last Revised by D Lougheed 00/7/3
Page 6
7.
Which of the following is not deflected in either a magnetic field or an electric field?
(a) an electron (b) a proton (c) an alpha particle (c) a beta particle
(e) a gamma ray
8.
Which molecule has no lone pairs of electrons on the underlined atom?
+1
(a) OF2
(b) H2S
(c) NH
(d) NCl3
(e) H3O+1
4
9.
Which electronic configuration for neutral atoms corresponds to a noble gas in its ground state?
(a) 1s2 2s2 2p 6 3s2
(b) 1s2 2s2 2p 6 3s1
(c) 1s 2 2s 2 2p 6
(d) 1s2 2s2 2p 5
(e) 1s2 2s2 2p 4
10. Which element is produced when the nucleus of a nitrogen atom emits an electron?
(a) boron
(b) carbon
(c) nitrogen (d) oxygen
(e) fluorine
11. Which one of the following does not occur in nature as the metal itself?
(a) iron
(b) copper
(c) gold
(d) silver
(e) zinc
12. Which one of the following is the principle cause of hardness in natural groundwater?
(a) calcium ions (b) iron ions (c) a pH less than 6 (d) sodium ions
(e) fluoride ions
13. Which processes are exothermic?
(i)
CO2(s) → CO2(g)
-1
(ii)
Cl(g) + e-1 → Cl
(g)
+
(iii)
Ca(s) → Ca
+ e-1
(g)
(iv)
Mg(l) → Mg(s)
(a) (i),(ii) and(iii) only
(b) (i) and(iii) only
(d) (iv) only
(e) (i) and(iv) only
14. The CO molecule is isoelectronic with
(i) CN-1
(ii) NO+
(iii) N2
(a) (i),(ii) and(iii) only
(b) (i) and(iii) only
(d) (iv) only
(e) (i) and(iv) only
(c) (ii) and(iv) only
(iv) NO-1
(c) (ii) and(iv) only
15. At standard temperature and pressure what is the volume of 8.0 g of O2(g)?
(a) 5.6 L (b) 11.2 L
(c) 22.4 L
(d) 45 L
(e) 90 L
16. Three successive elements, in order of increasing atomic number, have these first ionization energies:
1680 kJ/mol
2080 kJ/mol
494 kJ/mol
Which one of the following sets represents the three elements?
(a) N
O
F
(b) O F
Ne
(c) F Ne
Na
(d) Ne
Na
Mg
(e) Na Mg
Al
Last Revised by D Lougheed 00/7/3
Page 7
17. A graph shows heat of fusion for the elements plotted against(versus) atomic number as a series of
peaks and troughs. Which of the following sets of atomic numbers corresponds to peaks on such a
graph?
(a) 6, 14, 32
(b) 8, 16, 34
(c) 3, 11, 19
(d) 5, 13, 31
(e) 9, 17, 35
18. Consider one gram of each of the following gases at standard temperature and pressure. Which gas
will have the greatest volume?
(a) CO (b) CH4
(c) N2O
(d) NH 3
(e) N2
19. During the process
+
+ e-1
(g)
(a) Energy is released and the ion is larger than the atom
(b) Energy is gained and the ion is larger than the atom
(c) Energy is released but the atom and the ion have the same size
(d) Energy is gained and the ion is smaller than the atom
(e) Energy is released and the ion is smaller than the atom
Na(g) → Na
20. Which metal will not liberate hydrogen from concentrated sulphuric acid?
(a) iron
(b) magnesium(c) cobalt
(d) nickel
(e) copper
21. A mixture of nitrogen, oxygen and carbon dioxide contains a total of 3.0 mol of these gases and the
mole fraction of nitrogen is 0.40. What mass of nitrogen is present in this mixture?
(a) 17 g
(b) 28 g
(c) 34 g
(d) 104 g
(e) 125 g
22. A sample of helium at 300K and 100 kPa occupies 1.00 L. If the pressure is increased to 200 kPa, at
what temperature will the volume of the sample be 2.00L?
(a) 300K
(b) 600K
(c) 900K
(d) 1200K
(e) 2400K
23. What is the oxidation number of the halogen in Cl2O?
(a) -2
(b) -1
(c) 0
(d) +1
(e) +2
24. First ionization energies of three metals(P, Q and R) and three nonmetals(X, Y and Z) appear
below. Which compound will have the most ionic bond?
P
496 kJ/mol
X
348 kJ/mol
Q
419 kJ/mol
Y
423 kJ/mol
R
403 kJ/mol
Z
295 kJ/mol
(a) RX (b) RZ
(c) QY
(d) PX
(e) PZ
Last Revised by D Lougheed 00/7/3
Page 8
25. Assume that argon, at a constant temperature and pressure, behaves as an ideal gas. Which of the
following is correct?
(a) All argon atoms move with the same speed
(b) All argon atoms collide with the container walls with the same force
(c) Temperature is determined solely by the collision frequency of argon atoms
(d) All argon atoms have the same momentum
(e) Collisions between argon atoms are 100% efficient in energy transfer
26. An element classified as a metalloid(semi-metal) would be expected to have
(a) Ionic hydrides, polymeric covalent oxides and amphoteric oxides
(b) Covalent hydrides, ionic oxides and amphoteric oxides
(c) Covalent hydrides, molecular covalent oxides and acidic oxides
(d) Covalent hydrides, polymeric covalent oxides and amphoteric oxides
(e) Ionic hydrides, ionic oxides and basic oxides
27. If the coefficient of H+1 is 8, what is the value of “y” in the following reaction
-1
y [Fe(H2O)6]2+ + MnO + 8 H +1 → y [Fe(H2O)6]3+ Mn 2+ + 4 H 2O
4
(a) 2
(b) 3
(c) 4
(d) 5
(e) 6
28. Hydrogen may be prepared by mixing
(a) phosphorus and phosphoric acid
(c) manganese dioxide and hydrochloric acid
(e) water with sulphuric acid
(b) zinc and hydrochloric acid
(d) copper and nitric acid
29. Which salt has a pale green aqueous solution?
(a) Ni(NO3)2
(b) MgCl2
(c) K3PO 4
(d) NaBr
(e) CaCl2
30. What volume of sulphur dioxide at STP is produced as 38.0 g of carbon disulphide burns according
to
CS2(l) + 3 O 2(g) → CO2(g) + 2 SO2(g)
(a) 2.8 L (b) 5.6 L
(c) 11.2 L
(d) 22.4 L
(e) 44.8 L
31. If you’re careful about significant figures, the result of the following calculation
0.1000 x 0.010 is
(a) 0.001
(b) 0.0010
(c) 0.00100 (d) 0.001000
(e) 0.0010000
32. In a chemical reaction between the two substances, the limiting reagent must be the substance that
(a) has the lower mass
(b) has the smaller number of moles
(c) is used up first
(d) is present in excess
(e) evaporates most quickly
33. Which sulphate has the lowest solubility in water at 25°C?
(a) Na2SO4
(b) CuSO4
(c) CaSO4
(d)(NH 4)2SO4
Last Revised by D Lougheed 00/7/3
(e) Al2(SO4)3
Page 9
34. Calcium oxide is most soluble with or without reaction in
(a) ethanoic acid (b) water
(c) ethanol
(d) propanone(acetone)
(e) hexane
35. Which solution will have the highest vapor pressure at 25°C?
(a) 0.010 M NaCl
(b) 0.10 M HBr
(c) 0.050M Ca(NO3)2
(d) 0.10 M Na2CO3
(e) 0.020 M CuSO 4
36. What chemical(s) result(s) when NH3(g) reacts with HCl (g)?
(a) NH2Cl(g)
(b) NH 4Cl(s)
(c) NH4OH (aq) and HCl(g)
(d) NCl3(g) and H2(g)
(e) NH2OH (g) and HOCl(aq)
37. If an oxide of nitrogen contains 25.9% by mass of nitrogen, what is its empirical formula?
(a) NO (b) N2O
(c) NO2
(d) N2O4
(e) N2O5
38. To precipitate 99% of the silver ion from 0.50 L of 0.10 M AgNO3 solution will require a minimum
of
(a) 1.00 L of 0.040 M HCl
(b) 0.10 L of 0.20 M CaCl2
(c) 0.50 L of 0.10 M NaCl
(d) 0.25 L of 0.15 M NH4Cl
(e) 0.30 L of 0.20 M MgCl 2
39. To balance the following skeleton equation
HClO2 → ClO2 + HClO 3 + HCl + H 2O
Using whole number coefficients, the smallest coefficient for HClO2 is
(a) 5
(b) 4 (c) 3 (d) 2 (e) 1
40. Which equation is not balanced?
(a) 3 Pb + 8 HNO3 → 3 Pb(NO 3)2 + 2 NO + 4 H2O
(b) 2 C + SiO2 → Si + 2 CO
(c) 2 Mg2Sn + 8 H2O → 2 SnH4 + 4 Mg(OH)2
(d) H3CBr + Mg → H3CMgBr
(e) SnO2 + 2 NaOH → Na2SnO2 + H 2O
1993
1.
2.
Select the particle with the lowest mass;
(a) alpha
(b) beta
(c) helium atom
(d) neutron
(e) proton
All neutral atoms contain equal numbers of
(a) neutrons and electrons
(b) positrons and neutrons
(c) electrons and protons
(d) protons and neutrons
(e) electrons and positrons
Last Revised by D Lougheed 00/7/3
Page 10
3.
When alpha particles are shot at a gold foil(as in Rutherford’s experiment), most of the alpha
particles are not deflected. This experiment suggests that
(a) gold atoms are bonded to each other
(b) alpha particles bear a charged opposite to that of the nuclei of the gold atoms
(c) the mass of a gold atom is uniformly spread throughout its volume
(d) there is as much mass between the gold atoms as there is within them
(e) gold atoms are mostly empty space
4.
Which of the following forms the most basic oxide?
(a) bismuth
(b) antimony (c) arsenic
(d) phosphorus
(e) nitrogen
5.
If an atom has seven electrons in its valence shell, to which group of elements in the periodic table
does it belong?
(a) the Group headed by helium
(b) the Group headed by fluorine
(c) the Group headed by boron
(d) the Group headed by lithium
(e) the Group headed by nitrogen
6.
Which compound has the greatest ionic character in its bonds?
(a) BF3 (b) SF6 (c) PF3
(d) LiF
(e) OF2
7.
Of the following, what is the most abundant nitrogen containing pollutant in Earth’s lower
atmosphere?
(a) NaNO3
(b) Li3N
(c) NH3
(d) NO 2
(e) N2
8.
One litre of gaseous argon is compared to one litre of gaseous helium, both at 25°C and 100 kPa.
Select the correct statement:
(a) Argon and helium have the same average speed
(b) Argon atoms have greater average kinetic energy than the helium atoms do
(c) The average argon atom moves more slowly than the average helium atom
(d) Helium and argon atoms hit the walls of the containers with the same frequency
(e) The average helium atom hits the walls of its container with more force than the average argon
atom does in its container.
9.
What is the systematic IUPAC name for the compound Cr2O3?
(a) chromium(III) oxide
(b) chromium(II) oxide(III) (c) chromium trioxide
(d) chromium(0) oxide(0)
(e) trichromium dioxide
10. How many moles of pure NaOH must be used to prepare 1/00 L of 1.00 M NaOH?
(a) 2.00 mol
(b) 1.00 mol (c) 0.500 mol (d) 10.0 mol (e) 0.100 mol
11. Which metal can be isolated profitably from seawater?
(a) arsenic
(b) bromine (c) copper
(d) potassium (e) magnesium
Last Revised by D Lougheed 00/7/3
Page 11
12. When the following equation is balanced and the smallest whole number coefficients appear, what is
the coefficient of O2?
Cr2O3 + KOH + O2 → K2CrO4 + H 2O
(a) 2
(b) 3
(c) 4
(d) 6
(e) 8
13. Carbon monoxide can be made by the
(a) reaction of acids with carbonates
(c) complete combustion of methane
(e) action of steam on hot coke
(b) combustion of carbon dioxide
(d) heating a metal carbonate
14. ”A valence electron in a pure metal is not held by any specific atom, but all valence electrons are
used to hold together the atoms of the metal.” This statement is best classified as
(a) a specific experimental fact
(b) an opinion not based upon evidence
(c) a correct definition of a chemical term or expression, either in terms of experimental behaviour or
of sound scientific theory
(d) a scientific law expressing the directly observable results of many different experiments
(e) a scientific theory which, while it cannot be directly measured or observed, is in accord with and
explains the results of experiments
15. If equal volumes of 0.10 M NaOH and HCl are mixed, the total number of ions present will be
approximately
(a) 10-14 times as great as before mixing (b) 10-7 times as great as before mixing
(c) the same as before mixing
(d) half as great as before mixing
(e) twice as great as before mixing
16. Atoms of elements which exhibit highly metallic properties general have
(a) fewer than three valence electrons
(b) more than five valence electrons
(c) high electronegativity
(d) small atomic radii
(e) more protons than electrons
17. What volume of 6.00 M sulphuric acid would be required to make 2.00 L of 2.25 M sulphuric acid?
(a) 0.375 L
(b) 0.667 L (c) 0.750 L
(d) 1.33 L
(e) 6.75 L
Last Revised by D Lougheed 00/7/3
Page 12
18. One lire of aqueous 0.10 M NaNO 3 is mixed with one litre of aqueous 0.20 M Mg(NO3)2. The
resulting concentrations in mol/L are
-1
(a) 0.50 M Na+ , 0.10 M Mg2+ , 0.20 M NO
3
-1
(b) 0.50 M Na+ , 0.10 M Mg2+ , 0.25 M NO
3
-1
(c) 0.50 M Na+ , 0.20 M Mg2+ , 0.20 M NO
3
-1
(d) 0.50 M Na+ , 0.20 M Mg2+ , 0.40 M NO
3
-1
(e) 0.10 M Na+ , 0.10 M Mg2+ , 0.40 M NO
3
19. With due regard to significant figures, what is the value of the product
(1.01 x 102) x (1.0 x 10-4 + 10.1 x 10-5)?
(a) 0.02 (b) 0.020
(c) 0.0203
(d) 0.02030 (e) 0.020201
20. The vapor pressure of liquid water depends upon the
(a) atmospheric pressure
(b) partial pressure of nitrogen in the air
(c) volume of the container
(c) relative humidity of the air
(e) temperature
-3
-1
-2
21. Element E forms these stable compounds and ions: EH2, CE2, PE , CaE, NE and SE . What is
4
3
3
element E?
(a) boron
(b) oxygen
(c) fluorine
(d) sodium
(e) silicon
22. The percentage of water in a substance is determined by heating until it is believed all the water has
been driven off. In four different trials, students obtained these results:
10.128%
10.143%
10.140%
8.542%
What value would be reported for the percentage of water?
(a) 8.542%
(b) 9.738%
(c) 10.128% (d) 10.137% (e) 10.142%
23. Sodium hydroxide, NaOH, is added to a solution of ammonium nitrate, NH4NO 3, in water and the
solution is warmed. What gas is evolved?
(a) ammonia
(b) nitrogen (c) hydrogen (d) oxygen
(e) nitrogen monoxide
24. Which noble gas has the lowest boiling point?
(a) xenon (b) krypton (c) argon
(d) neon
(e) helium
25. Of the following, the substance most sensitive to light is
(a) silver bromide
(b) sodium nitrate
(v) potassium carbonate
(d) copper sulphate
(e) acetic acid
Last Revised by D Lougheed 00/7/3
Page 13
26. Select the largest ion
(a) Al3+
(b) Cl-1
(c) K+1
(d) S2-
(e) Ca2+
27. Which of these atoms is the most electronegative in its compounds?
(a) As
(b) Br
(c) Cl
(d) P
(e) Si
28. What is X in the following reaction
10
4
13
B + He →
N+X
5
2
7
(a) a neutron
(b) a proton (c) a positron (d) a deuteron (e) an electron
29. The oxidation number of sulfur is +4 in
(a) SF6 (b) SOBr2
(c) SO3
(d) H2S
(e) S2 Cl2
30. On the basis of group properties, what formula is expected for the binary compound of lanthanum
with selenium?
(a) LaSe (b) La2Se
(c) LaSe2
(d) La3Se2
(e) La2Se3
31. Which of the following has the highest first ionization energy?
(a) Al
(b) Ar (c) Cl (d) Mg(e) Na
32. Methanol, CH3OH, and glycerin, C3H5(OH) 3 are both non-electrolytes. Compare a solution of 10 g
of methanol in 10000 g of water with a solution of 10 g of glycerin in 1000g of water. Choose the
correct statement.
(a) the glycerin has a lower freezing point than the methanol solution
(b) the methanol has a lower freezing point than the glycerin solution
(c) both solutions freeze at 0°C
(d) both solutions freeze at the same temperature, which is above 0°C
(e) both solutions freeze at the same temperature, which is below 0°C
33. How many moles of SO3 can be produced from 3.00 mol of SO2 and 2.00 mol of O2?
(a) 1.00 mol
(b) 1.50 mol (c) 2.00 mol (d) 3.00 mol (e) 5.00 mol
34. A closed, 1.00 litre container of helium is at 20°C and 100 kPa pressure. If the container is heated to
200°C, what helium pressure is expected?
(a) 1000 kPa
(B) 181 kPa (c) 161 kPa (d) 62 kPa
(e) 20 kPa
35. Elemental analysis of a compound gives these results by mass:
Na
32.4%
H
0.71%
P
21.8%
O
45.1%
What is the simplest formula of the compound?
(a) NaHPO 3
(b) NaHP 2O4 (c) Na2H2P2O5
(d) Na2HPO 4 (e) NaH2PO 4
Last Revised by D Lougheed 00/7/3
Page 14
36. Why is it dangerous to dilute sulphuric acid by pouring water into the concentrated acid?
(a) the water may decompose
(b) a poisonous gas may be given off
(c) a fire may be started
(d) the heat evolved may rapidly convert the water into steam
(e) the acid could solidify and break the container
37. What is the value of ∆H for the reaction:
3 H2(g) + N 2(g) → 2 NH 3(g)
given the following bond energies?
H-H
535 kJ/mol
N-H
389 kJ/mol
N ≡ N 946 kJ/mol
(a) -83 kJ (b) -122 kJ
(c) +122 kJ (d) -1084 kJ
(e) -1770 kJ
38. Which of the following conduct’s electricity well?
(i) H2O (ii) NH3(g)
(iii) CH3OH (aq)
NaCl(aq)
(a)(i),(ii) and(iii) only
(b)(i) and(iii) only
(c)(ii) and(iv) only
(d)(iv) only
(e)(i) and(iv) only
39. What is the correct burette reading?
23
(a) 23 mL
(b) 23.3 mL
(c) 23.36 mL
(d) 23.64 mL
24
(e) 24.36 mL
40. An odorless, colorless, tasteless gas is thought to be oxygen. Which observation would support this
suggestion?
(a) burning the gas in air produces only water
(b) the gas extinguishes a flame
(c) the gas turns limewater milky
(d) a glowing splint bursts into flame in the gas
(e) the gas decolorizes a brown apple
1994
1.
Which of the following is not in the same group as neon?
(a) argon (b) boron
(c) krypton (d) radon
(e) xenon
Last Revised by D Lougheed 00/7/3
Page 15
2.
Which terms on the left correctly match the materials on the right?
Q Mechanical mixture
X salt water
R Solution
Y carbon dioxide
T Pure substance
Z washing detergent
(a) QX, RY, TZ
(b) QX, RZ, TY
(d) QZ, RX TY
(e) QZ, RY, TX
(c) QY, RX, TZ
3.
Two particles with equal numbers of positive charges repel each other with a force, F. If the
distance between the particles is doubled, the new repulsive force will be
(a) F/4 (b) F/2 (c) F (d) 2F (e) 4F
4.
In the periodic table, the elements are arranged in order of increasing
(a) number of neutrons
(b) number of protons
(c) ionization energy
(d) density
(e) electronegativity
5.
Select the element that is a typical nonmetal:
(a) silver
(b) calcium
(c) chromium
(d) sulphur
6.
Choose the element that is a solid at room temperature and pressure
(a) argon (b) bromine (c) chlorine (d) selenium (e) krypton
7.
Which molecule shows covalent bonding, with the least ionic character?
(a) F-Be-F
(b) F-Li
(c) F-Br
(d) F-F
(e) einsteinium
(e) F-O-F
8.
Which pair of characteristics applies to typical ionic solids?
(a) Good electrical conductivity and high ionization energy
(b) High melting point and malleability
(c) High melting point and crystalline structure
(d) Low melting point and high heat conductivity
(e) Low melting point and low aqueous solubility
9.
Which neutral halogen atom has the smallest ionization energy for the first electron removed?
(a) fluorine
(b) chlorine (c) bromine (d) iodine
(e) astatine
10. The following electronic configuration applies to a neutral atom or a cation:
1s2 2s2 2p 6 3s2 3p 6 4s1
The element or ion could be
(a) and argon ion
(b) a neutral potassium atom
(c) a chloride ion
(d) a neutral calcium atom
(e) a strontium ion
11. What volume of hydrogen will have nearly the same number of molecules as 1.00 L of nitrogen gas,
if both are measured at the same temperature and pressure?
(a) 0.500 K of hydrogen
(b) 1.00 L of hydrogen
(c) 2.00 L of hydrogen
(d) 14.0 L of hydrogen
(e) 28.0 L of hydrogen
Last Revised by D Lougheed 00/7/3
Page 16
12. At what temperature is the average kinetic energy of molecules in a gas twice as great as at 0°C?
(a) 1092 K
(b) 746 K
(c) 546 K
(d) 273 K
(e) 137 K
13. Pure oxygen in a closed container of fixed volume is heated until the average energy of the gas
molecules doubles. Which other aspect of this system is also doubled?
(a) the density of the oxygen
(b) the average velocity of the oxygen molecules
(c) the density of the oxygen gas
(d) the pressure in the container
(e) the volume occupied by each of the oxygen molecules
14. What volume of argon gas at 100 kPa and 25°C must be added to a 1.00 L glass flask containing
nitrogen gas at 70 kPa and 25°C to give a mixture of gases having a total pressure of 210 kPa at
25°C?
(a) 1.40 L(b) 1.70 L
(c) 2.00 L
(d) 2.86 L
(e) 3.10 L
15. In which of the following substances, all at 100 kPa, is the average transitional energy of the
molecules the greatest?
(a) iron at 150°C
(b) oxygen at 100°C
(c) liquid water at 80°C
(d) carbon dioxide at 70°C
(e) ice at 0°C
16. If the following equation is obeyed, how many moles of ammonia are needed to produce 801 mol of
hydrogen gas, H2?
2 NH 3(g) → N2(g) + 3 H 2(g)
(a) 2.00 mol
(b) 22.4 mol (c) 267 mol (d) 534 mol (e) 1203 mol
17. Hydrogen gas is a product in one of the following cases. Which one?
(a) aluminum turnings are heated with hot, concentrated potassium hydroxide solution
(b) aqueous hydrogen peroxide is added to an aqueous solution of iron(III) nitrate
(c) solid sodium carbonate is added to dilute aqueous hydrochloric acid
(d) copper is placed in dilute aqueous nitric acid
(e) calcium oxide is heated with ammonium chloride
18. Which atom or ion is formed as a result of the reduction in the following reaction?
2 KMnO4 + 16 HCl → 2 KCl + 2 MnCl2 + 5 Cl2 + 8 H 2O
(a) potassium in KCl
(b) manganese in MnCl2
(c) hydrogen in H2O
(d) chlorine in Cl2
(e) oxygen in H2O
19. What is the missing term, X, in the following equation?
238
234
U→
Th + X
92
90
(a) a positron
(b) a proton (c) a neutron (d) a helium nucleus (e) an electron
Last Revised by D Lougheed 00/7/3
Page 17
20. Which set of oxidation numbers is correct for K2Cr2O7?
(a) K
+1;
Cr
+2.5; O
-1
(a) K
+4;
Cr
+3;
O
-2
(a) K
+1;
Cr
+6;
O
-2
(a) K
+2;
Cr
+12; O
-14
(a) K
+1;
Cr
+7;
O
-2
21. The main gaseous product of the reaction of aqueous hydrochloric acid with manganese dioxide is
(a) permanganic acid
(b) hydrogen (c) chlorine (d) oxygen
(e) manganese chloride
22. Which of the following aqueous reagents will most effectively remove carbon dioxide from an air
sample?
(a) ammonium nitrate
(b) silica gel
(c) concentrated sulphuric acid
(d) sodium hydroxide
(e) sodium hydrogen carbonate
23. What products will result from adding solid barium oxide to water?
(a) a solution of barium hydroxide
(b) barium ions and hydrogen gas
(c) barium ions and oxygen gas
(d) barium metal and hydrogen gas
(e) no chemical change will take place
24. The general formula for the binary hydrogen compounds of the elements, E, of the nitrogen group of
the periodic table is
(a) EH5
(b) EH4
(c) EH3
(d) EH2
(e) E2H6
25. The percentage by mass of oxygen in pitchblende, U3O8 is
(a) 72.7%
(b) 35.0%
(c) 30.4%
(d) 17.9%
(e) 15.2%
26. How many moles of H 2O are there in 1.8 L of water?
(a) 111 mol
(b) 100 mol (c) 55.5 mol (d) 18 mol
(e) 1.8 mol
27. An oxide of nitrogen contains 30.4% of nitrogen by mass and its relative molecular mass is near 90.
What oxide of nitrogen is it?
(a) N2O5
(b) N2O4
(c) N3O3
(d) N4O2
(e) NH4NO 3
28. The relative molecular mass of a gas is 56.0 and its simplest formula is CH2. What is the correct
molecular formula for the gas?
(a) CH2 (b) C2H4
(c) C3H6
(d) C4H8
(e) C6H12
29. 40.0 mL of 0.0700 M HBr is titrated by the addition of 0.0500 M KOH. What is the hydrogen ion
concentration after 50.0 mL of KOH solution has been added?
(a) 6.5 x 10-3 M
(b) 3.3 x 10-3 M
(c) 0.0311 M
(d) 0.0200 M
(e) 0.0120 M
Last Revised by D Lougheed 00/7/3
Page 18
1
2
H, on earth became deuterium atoms, D, what
1
1
would be the new relative atomic mass for the element hydrogen? [ Relative atomic masses: H,
1.008: D, 2.014]
(a) 1.008
(b) 1.109
(c) 1.210
(d) 1.512
(e) 2.014
30. If, suddenly, 10.0% of the hydrogen atoms,
31. What mass of dry sodium chloride, NaCl, should one use to make 2.00 L of a 0.147 M Na+ ion
solution?
(a) 117 g
(b) 28.3 g
(c) 17.2 g
(d) 10.4 g
(e) 5.22 g
32. If 4.0 g of sodium hydroxide is dissolved in enough water to make 400 mL of solution, what is the
molar concentration of the solution>
(a) 10.0 M
(b) 0.40 M
(c) 0.25 M
(d) 0.040 M (e) 0.010 M
33. Sodium hypochlorite is prepared by the reaction
2 NaOH + Cl 2 → NaCl + NaClO + H 2O
If 71 g of chlorine is bubbled into a solution containing 50 g of sodium hydroxide, which component
limits the quantity of sodium hypochlorite formed?
(a) Cl2 (b) NaCl
(c) H2O
(d) NaOH
(e) NaClO
34. If one drop(0.05 mL) of 2.0 M HCl is added to 1.00 L of pure water, the hydrogen ion
concentration in the solution after mixing will be
(a) 1.0 x 10-2M
(b) 1.0 x 10-3 M
(c) 1.0 x 10-4 M
(d) 1.0 x 10-5 M
(e) 1.0 x 10-6 M
35. By addition to water, 30.0 mL of 6.0 M sulphuric acid is diluted to 150.0 mL. What is the
concentration of sulphuric acid after dilution?
(a) 1.20 M
(b) 1.50 M
(c) 2.40 M
(d) 3.00 M
(e) 4.80 M
36. AB2 is the salt of a strong acid and a strong base. A 0.020 M solution of this salt is a saturated
solution at 25°C What is the concentration of B -1 ions in solution?
(a) 1.0 x 10-7 M
(b) 4.0 x 10-4 M
(c) 1.0 x 10-3 M
(d) 2.0 x 10-2 M
(e) 4.0 x 10-2 M
37. Choose the one pair of salts whose aqueous solutions would, upon mixing, create a precipitate.
(a) Na2SO4 and(NH4)2S
(b) NaNO 3 and MgBr2
(c) Ag2SO4 and KNO 3
(d) CuSO4 and CaCl2
(e)(NH4)2CO3 and KNO 3
38. Which of the following is the most acidic?
(a) drinking water
ßßß(b) human saliva
(d) human gastric juice
(e) seawater
39. Select the one ion or molecule that is NOT tetrahedral
+
+
(a) NH (b) CH4
(c) SiCl4
(d) PCl
4
4
Last Revised by D Lougheed 00/7/3
(c) cow’s milk
+
(e) TeCl
4
Page 19
40. Which quantity of lead metal has the greatest mass?
(a) 22.4 mol
(b) 1.0 mL
(c) 207.2 g
(d) 6.0 x 1023 atoms
(e) one formula mass expressed in grams
1995
1.
Which two species have the same charge and mass number?
(a) a neutron and a hydrogen atom
(b) an electron and a proton
(c) an electron and a H-1 ion
(d) a proton and an electron
(e) a hydrogen atom and a H-1 ion
2.
Which gas has the greatest impact in the greenhouse effect?
(a) methane
(b) ozone
(c) nitric oxide, NO (d) sulphur dioxide
(e) carbon dioxide
3.
Which one of the following chemical equations is incorrect?
(a) Na + e-1 → Na+ + energy
(b) Mg + energy → Mg2+ + 2 e-1
(c) H2 + energy → 2 H+ + 2 e-1
(d) F + e-1 → F-1 + energy
(e) Ne+ + e-1 → Ne + energy
4.
Two particles with the same positive charge repel each other with a force Q. If the distance between
the particles is tripled, the repulsive force will be
(a) Q/9 (b) Q/6
(c) Q/3
(d) Q
(e) 9Q
5.
For which atom will the energy required to remove one electron be the greatest?
(a) K
(b) Kr
(c) Cs
(d) Br
(e) Ca
6.
Choose the substance that is solid at room temperature and pressure.
(a) CO2 (b) N2
(c) CH3CH2OH
(d) NaCl
(e) Br2
7.
In an aqueous solution, salt exists in the form of
(a) molecules
(b) dimers
(c) crystals
(d) ions
8.
(e) atoms
What products will result from adding a solid sodium oxide, Na2O, to water?
(a) a solution of sodium hydroxide
(b) sodium metal and oxygen gas
(c) sodium ions and oxygen gas
(d) sodium ions and hydrogen gas
(e) no chemical change will occur
Last Revised by D Lougheed 00/7/3
Page 20
9.
The region of the periodic table in which the elements of greatest density are found is the
(a) top right
(b) top left
(c) bottom right
(d) bottom left(e) bottom center
10. Which one of the following elements is NOT a halogen?
(a) fluorine
(b) bromine (c) sulphur
(d) iodine
(e) chlorine
11. Which compound is best described as an ionic compound?
(a) SiF4 (b) H2O
(c) NO
(d) N2O
(e) KNO 3
12. Exactly 1.00 L of an ideal gas is cooled from 100°C to 30°C. What is its new volume if the pressure
is kept constant?
(a) 18.1 L
(b) 1.23 L
(c) 0.90 L
(d) 0.81 L
(e) 0.30 L
13. What volume of oxygen will have nearly the same number of molecules as 1.00 L of hydrogen gas, if
both are measured at STP?
(a) 1.00 L
(b) 8.00 L
(c) 16.0 L
(d) 22.4 L
(e) 32.0 L
14. What is the “X” when the following equation is balanced with a “2” as the coefficient for NH3?
2 NH 3(g) + X O 2(g) → Y NO(g) + Z H2O(g)
(a) 5
(b) 1/5
(c) 5/4
(d) 5/3
(e) 5/2
15. What is the formula of potassium phosphide?
(a) KP3 (b) KP 2
(c) KP
(d) K2P
(e) K3P
16. How many moles of sodium peroxide, Na2O2(s) can be made from 1.0 mol of Na(s) and 2.0 mol of
O2(g)?
(a) 3.0 mol
(b) 2.0 mol
(c) 1.5 mol
(d) 1.0 mol
(e) 0.50 mol
17. When three moles of calcium hydroxide react completely with two moles of phosphoric acid, how
many moles of water are produced?
(a) six
(b) four
(c) three
(d) two
(e) one
18. Creative Chris wrote five different equations for the reaction of aqueous ammonia with aqueous
hydrochloric acid. Which one is right?
(a) NH3 + HCl → NH 2Cl + H2
+
(b) NH 3 + HCl → NH + Cl-1
4
(c) NH3 + 3 HCl → NCl3 + 3 H 2
+
(d) 2 NH 3 + HCl + 2 H 2O → NH + NOCl + OH-1
4
+
(e) 2 NH3 + 2 HCl → NH 2OH + NH + 2 Cl-1 + H +1
4
19. If one molecule of a virus has a mass of 10-18 g, approximately how many atoms are in it?
(a) 102 atoms
(b) 105 atoms
(c) 108 atoms
(d) 1011 atoms
(e) 1014 atoms
Last Revised by D Lougheed 00/7/3
Page 21
20. On earth, which one of these elements is found in elemental form?
(a) aluminum
(b) boron
(c) carbon
(d) fluorine (e) potassium
21. To melt 1.00 g of ice at 0°C requires 330 J. If 4.00 g of ice at 0°C is added to 100 g of water at
25°C, what is the final temperature?. Assume no heat loss or gain by the container. The specific
heat capacity of liquid water is 4.2 J·g-1 ·°C-1.
(a) 22.0°C
(b) 21.1°C
(c) 19.9°C
(d) 18.8°C
(e) 12.3°C
22. If the formula for yttrium chloride is YCl3, and that for sodium stannate is Na2SnO3, what formula
is expected for yttrium stannate?
(a) Y(SnO3)
(b) Y2(SnO3) (c) Y(SnO3)2 (d) Y2(SnO3)3 (e) Y3(SnO3)2
23. To 10.0 mL of 1.0 M HCl enough water is added to make one litre of solution. During this dilution,
the pH
(a) falls by about 2.0 pH units
(b) falls by about 0.5 pH units
(c) changes by less than 0.1 pH units
(d) rises by less than 0.1 pH unit
(e) rises by about 2 pH units
24. Analysis of an oxide of carbon, CxOy, shows a carbon content of 52.96% by mass. What is the
simplest formula for the compound?
(a) C5O2
(b) C3O2
(c) C2O3
(d) CO2
(e) CO
25. Select the one correct statement about a concentrated solution of a strong electrolyte in water.
(a) its boiling point is well below 100°C
(b) its freezing point is above 0°C
(c) it is a poorer conductor of electricity than pure water
(d) its vapor pressure is lower than that of pure water
(e) it contains a high proportion of neutral electrolyte molecules
26. The natural abundance of 2H is 0.015% and that of 18O is 0.20%. How many molecules of
2H 2(18O) are there in one mole of natural water?
(a) 1.4 x 1022 molecules
(b) 9 x 1019 molecules
16
(c) 1.4 x 10 molecules
(d) 3.6 x 1014 molecules
(e) 2.7 x 1013 molecules
27. What volume of 0.0400 M K 2SO4 will contain 0.02000 mol of potassium ions?
(a) 500 mL
(b) 400 mL (c) 250 mL
(d) 200 mL (e) 125 mL
28. If 100 g of MgCO3 is fully converted into MgO upon heating, what is the maximum mass of MgO
produced?
(a) 40.3 g
(b) 47.8 G
(c) 49.7 g
(d) 52.2 g
(e) 77.1 g
Last Revised by D Lougheed 00/7/3
Page 22
29. What hydrogen ion concentration results from mixing 145 mL of 0.186 M NaOH with 325 mL of
0.234 M HCl?
(A) 0.076 M
(b) 0.104 M (c) 0.151 M (d) 0.162 M (e) 0.219 M
30. Select the substance that is most soluble in water at 25°C.
(a) AgCl
(b) CH4
(c) Mg3(PO 4)2
(d) NH 4NO 3
(e) CuS
31. An oxide of phosphorus has the simplest formula P23 and a relative molecular mass of about 220.
The formula for one molecules of the oxide is
(a) P4O10
(b) P4O6
(c) P2O5
(d) P2O4
(e) P2O3
32. An unsaturated solution (180 g of KNO3 in 100 g of water) at 90°C is cooled to 25°C, where the
solubility is 40 g KNO 3 in 100 g of water. What mass of KNO3 precipitates, assuming the 25°C
solution is saturated?
(a) 240 g
(b) 180 g
(c) 140 g
(d) 40 g
(e) 1.4 g
33. 25.0 mL of 0.100 M Na 2SO4 and 350.0 mL of 0.150 M BaCl2 are mixed and diluted to exactly one litre
volume. What is the concentration of chloride ions in the final solution?
(a) 0.0515 M
(b) 0.105 M (c) 0.132 M (d) 0.150 M (e) 0.264 M
34. What volume of 0.0600 M NaOH must be added to 20.0 mL of 0.0400M H2SO4 to reach
neutrality?
(a) 60.0 mL
(b) 30.0 mL (c) 26.7 mL (d) 20.0 mL (e) 13.3. mL
35. Which one of the following does not show any significant hydrogen bonding?
(a) methane
(b) water
(c) methanol (d) ethanoic acid
(e) hydrogen fluoride
n
36. What charge is expected for the SiF ion?
6
(a) +2
(b) -1 (c) -2 (d) -3 (e) -4
37. At what temperature do the molecules of an ideal gas have twice the average kinetic energy that they
have at 100°C?
(a) 200 K (b) 373 K
(c) 473 K
(d) 546 K
(e) 746 K
38. In a water molecule the H-O-H angle is nearest to
(a) 60° (b) 90°
(c) 109°
(d) 120°
(e) 180°
39. (NH 4)2Fe(SO4)2 ·6H2O(50.0 g or 0.1276 mol) is heated and 9.2 g of water is lost. The product has
the formula(NH4)2Fe(SO4)2 ·yH2O. What is the value of y?
(a) 1
(b) 2
(c) 3
(d) 4
(e) 5
Last Revised by D Lougheed 00/7/3
Page 23
1996
1.
Which two species have the same charge and mass number?
(a) A hydrogen atom and a H- ion
(b) An electron and a proton
(c) An electron and a H- ion
(d) A proton and an electron
(e) A neutron and a hydrogen atom
2.
The Law of Definite Proportions states that elements always combine with each other, making a
compound,
(a) in a definite ratio by volume
(b) with the evolution of heat
(c) in the proportion, by mass, in which they were
(d) in a definite ratio by mass
(e) spontaneously
3.
A particle containing 6 protons, 5 electrons and 7 neutrons has approximately the same mass as
(a) 10 neutron
(b) 11 neutrons
(c) 12 neutrons
(d) 13 neutrons
(e) 18 neutrons
4.
Which isotope has the largest number of neutrons?
257
257
254
256
(a)
Unq
(b)
Lw (c)
No
(d)
Md
104
103
102
101
(e)
253
Es
99
290
300
Cn and
Cn, with relative
124
124
abundances of 25% and 75%, respectively. The relative atomic mass of canadium is
(a) 292.0 (b) 292.5
(c) 295.0
(d) 297.5
(e) 298.0
5.
The new element canadium has only two stable isotopes,
6.
How many valence electrons are there in one sulfide anion, S2-?
(a) Ten
(b) Eight
(c) Six
(d) Four
(e) Two
7.
Which set of elements is correctly arranged in order (left to right) of increasing first ionization
energy?
(a) F<Br<NecNa
(b) Br<F<Na<Ne
(c) Ne<F<Br<Na
(d) Na<F<Br<Ne
(e) Na< Br< F< Ne
8.
Atoms of element X, having two valence electrons each, combine with atoms of element Y, having
six valence electrons each. The compound formed is expected to have the formula
(a) XY
(b) X3Y
(c) XY3
(d) X2Y
(e) XY2
9.
The region of the periodic table in which the elements of greatest density are found is the
(a) top, right
(b) top, left (c) bottom, right
(d) bottom, left
(e) bottom, centre
10. In the periodic table, the elements are arranged in order of increasing
(a) Number of neutrons
(b) lonization energy
(c) Number of protons
(d) Density
(e) Electronegativity
Last Revised by D Lougheed 00/7/3
Page 24
11. Which of these elements forms the most basic oxide?
(a) Bismuth
(b) Antimony (c) Arsenic
(d) Phosphorus
(e) Nitrogen
12. If an atom has five electrons in its valence shell, to which group of elements in the periodic table
does it belong?
(a) Group headed by helium
(b) Group headed by fluorine
(c) Group headed by boron
(d) Group headed by lithium
(e) Group headed by nitrogen
13. Which element is produced when the nucleus of a nitrogen atom emits an electron?
(a) Boron(b) Carbon
(c) Nitrogen (d) Oxygen (e) Fluorine
14. Which molecule has the greatest bond dissociation energy?
(a) H2
(b) F2
(c) N2
(d) O2
(e) Cl2
15. The Sl unit of pressure has the dimensions
(a) kg m s-2
(b) kg m2 S-2 (c) kg m-1 S-2 (d) kg m s-1
(e) mol °C m~3
16. Which statement embodies Avogadro’s hypothesis about gases?
(a) At the same temperature, the average kinetic energy of all gases is the same
(b) At constant temperature, pressure and volume are directly proportional
(c) The volume of a gas is directly proportional to the volume of its molecules
(d) At the same temperature, all gases exert the same pressure on the walls of their containers
(e) The volume is proportional to the number of moles present, if temperature and pressure are
constant
17. Properties of four different elements are listed below. Which two should be located in the same
group(column) in the periodic table?
Element Compound
One of its
Formula of
with most
oxygen
an oxyacid
hydrogen
compounds
J
JH 3
JO
HJO 3
R
RH4
RO2
H4RO4
X
XH 4
XO
H2XO 3
Z
Z 2H6
Z 2O3
H3ZO 3
(a) Elements J and R
(b) Elements J and X
(c) Elements J and Z
(d) Elements R and X
(e) Elements R and Z
18. Exactly 1.00 L of an ideal gas is cooled from 1 00°C to 30°(c) What is its new volume if the
pressure is kept constant?
(a) 18.1 L
(b) 1.23 L
(c) 0.90L
(d) 0.81 L
(e) 0.30L
Last Revised by D Lougheed 00/7/3
Page 25
19. What volume of hydrogen will have nearly the same number of molecules as 1.00 L of nitrogen gas,
if both are measured at the same temperature and pressure?
(a) 0.500 L hydrogen
(b) 1.00 L hydrogen
(c) 2.00 L hydrogen
(d) 14.0 L hydrogen
(e) 28.0 L hydrogen
20. If one molecule of a virus has a mass of 10-18 g, approximately how many atoms are in it?(Choose
the nearest estimate).
(a) 102 atoms
(b) 105 atoms (c) 108 atoms (d) 1011 atoms (e) 1014 atoms
21. When this equation is balanced and the smallest whole-number coefficients appear what is the
coefficient of O2?
? Cr2O3 + ? KOH + ? O2 → ? K2CrO4 + ? H2O
(a) 2
(b) 3 (c) 4 (d) 6 (e) 8
22. Which processes are exothermic?
(1 ) CO2(s) → C02(g)
(2) Cl(g) + e~ → Cl-(g)
(3) Ca(g) → Ca+ (g) + e~
(4) Mg(liquid) → Mg(s)
(a)(1),(2) and(3) only
(b)(1) and(3) only
(d)(4) only
(e)(1) and(4) only
(c)(2) and(4) only
23. Sulfur has three natural isotopes of relative masses 32.0, 33.0 and 34.0. If the relative atomic mass
of sulfur is 32.07, which one of the following statements must be correct?
(a) 32S is less abundant than 34S
(b) 34S is more abundant than 33S
(c) 32S is more abundant than either 33S or 34S
(d) 33S is the most common isotope
(e) another natural isotope of lesser mass must exist
24. How many moles of methane, CH4, are in 16.0 9 of methane? Relative atomic masses are H, 1.01;
C, 12.01
(a) 1.0 mol
(b) 0.75 mol (c) 0.68 mol (d) 0.33 mol (e) 1.25 mol
25. What is the percentage by mass of oxygen in carbon dioxide? Relative atomic masses are: C, 12.01;
O, 16.00
(a) 73%
(b) 67%
(c) 61%
(d) 36%
(e) 27%
26. In a water molecule, the H-O-H angle is nearest
(a) 180° (b) 120°
(c) 109°
(d) 90°
27. Water is a good solvent for
(a) Ammonia gas
(d) Copper metal
Last Revised by D Lougheed 00/7/3
(b) Methane gas
(e) Liquid octane
(e) 60°
(c) Solid calcium carbonate
Page 26
28. As Cl207 is added to water, what is formed?
(a) HOCI
(b) HCI and O2
(c) HCIO3
(d) HCIO 4
(e) ClO2 and O2
29. What volume of 0.123 mol/L aqueous HCI is needed to neutralize 40.0 mL of 0.175 mol/L aqueous
NaOH?
(a) 17.6 mL
(b) 28.1 mL (c) 35.6 mL (d) 40.0 mL (e) 56.9 mL
30. In which of the following substances, all at100 kPa, is the average translational energy of the
molecules the greatest?
(a) Iron at 150°C
(b) Oxygen at 1 00°C
(c) Liquid water at 80°C
(d) Carbon dioxide at 70°C
(e) Ice at 0°C
31. If 100 9 MgCO 3 is fully converted into MgO upon heating, what is the maximum mass of MgO
produced? Relative atomic masses: C, 12.01; O, 16.00; Mg, 24.32
(a) 40.39
(b) 47.8 9
(c) 49.7 9
(d) 52.2 9
(e) 77.1 9
32. Lime juice is about 100,000 times more acidic than neutral water. What is the approximate pH of
lime juice?
(a) 1.0
(b) 2.1
(c) 3.2
(d) 4.0
(e) 5.5
33. Hydrogen may be prepared by mixing
(a) Phosphorus and phosphoric acid
(c) Manganese dioxide and hydroiodic acid
(e) Sulfuric acid with water
(b) Zinc and hydrochloric acid
(d) Copper and nitric acid
34. Which solution will have the highest vapour pressure at 25°C?
(a) 0.010 mol/L NaCl(aq)
(b) 0.10 mol/L HBr(aq)
(c) 0.050 mol/L Ca(NO3)2(aq)
(d) 0.10 mol/L Na2CO3(aq)
(e) 0.020 mol/L CuSO4(aq)
35. According to the Arrhenius definition, HNO3 in water is a
(a) weak base
(b) strong base
(c) weak acid (d) strong acid (e) nonelectrolyte
36.
"A valence electron in a pure metal is not held by any specific atom, but all valence electrons are
used to hold together the atoms of the metal". This statement is best classified as
(a) A specific experimental fact
(b) An opinion not based on evidence
(c) A correct definition of a chemical term or expression, either in terms of experimental behaviour
or of sound scientific theory
(d) A scientific law expressing the directly observable results of many different experiments
(e) A scientific theory which, while it cannot be directly measured or observed, is in accord with and
explains the results of experiments
Last Revised by D Lougheed 00/7/3
Page 27
37. Sodium hydroxide, NaOH, is added to a solution of ammonium nitrate, NH4N03, in water, and the
solution is warmed. What gas is evolved?
(a) Ammonia
(b) Nitrogen (c) Hydrogen (d) Oxygen (e) Nitrogen monoxide
38. Select the largest ion:
(a) Al3+
(b) Cl-1
(c) K+
(d) S2-
(e) Ca2+
39. If 4.0 9 of sodium hydroxide is dissolved in enough water to make 400 mL of solution, wha is the
molar concentration of sodium ions in the solution?
Relative atomic masses:
H, 1.01; O, 16.0; Na, 23.0
(a) 10.0 mol/L
(b) 0.40 mol/L
(c) 0.25 mol/L
(d) 0.040 mol/L
(e) 0.010 mol/L
40. How many moles of SO3 can be produced from 3.00 mol SO2 and 2.00 mol O2?
(a) 1.00 mol SO3
(b) 1.50 mol SO3
(c) 2.00 mol SO3
(d) 3.00 mol SO3
(e) 5.00 mol SO3
1997
1.
The letter Z represents any one of several atoms. Choose the one correct statement:
11
(a) Neutral atoms of Z have 16 electrons.
5
12
13
(b)
Z and
Z are isotopes of the same element.
6
6
4
(c) Z means that Z has atomic number 4 and mass number 2.
2
7
(d) The number of neutrons in Z is 3.
3
4
(e) The number of protons in Z is 4.
2
2.
Compared to an electron, a proton has
(a) the opposite charge and much less mass (b) the opposite charge and a much greater mass
(c) no charge and much less mass
(d) the same charge but a much greater mass
(e) the same charge and about the same mass
Last Revised by D Lougheed 00/7/3
Page 28
3.
Rutherford's alpha-particle bombardment of gold foil helped develop our current model of the
atom by
(a) finding the mass of the electron.
(b) showing the existence of the neutron.
(c) showing that the atom has a concentrated region of positive charge.
(d) showing that the electron carries a negative charge.
(e) showing the existence of the proton.
4.
In terms of Bohr's K, L, M,... shells, what is the distribution of electrons in an atom of selenium in
its lowest energy state?
(a) 2, 8, 16
(b) 2, 8, 10, 16
(c) 2, 18, 8, 6
(d) 2, 8, 18, 4
(e) 2,
8, 18, 6
5.
Which one of the following has the least ionic character?
(a) Sodium fluoride
(b) Phosphorus fluoride
(d) Rubidium fluoride
(e) Zinc fluoride
6.
(c) Aluminum fluoride
Which of the following is the correct Lewis structure for carbon dioxide:
O
C
O
(a)
O
C
O
(b)
O
C
O
(c)
(d)
O
C
O
C
O
O
(e)
7.
Which one of the following has the highest boiling point?
(a) H2Te
(b) H2Se
(c) H2S
(d) H4C
(e) H2O
8.
In what region of the periodic table are the atoms with smallest covalent atomic radii found?
(a) Lower left
(b) Lower right
(c) Lower centre
(d) Upper centre
(e) Upper right
9.
Which one of the following statements is true of aluminum?
(a) It is the most abundant element in the earth's crust.
(b) The metal forms a protective oxide coating when exposed to air.
(c) It occurs in nature as the free metal.
(d) It has a high tensile strength.
(e) It is one of the hardest elements.
10.
Which ion has the largest radius?
(a) O2(b) F(c) Cl-
11.
(d) S2-
(e) P3-
Which one of the following compounds is the largest contributor to the greenhouse effect?
(a) CO2
(b) C6H6
(c) CH4
(d) H3CCO2H
(e) CaCO3
Last Revised by D Lougheed 00/7/3
Page 29
12.
Four of these processes normally consume oxygen. Which one does not?
(a) combustion
(b) rusting of iron
(c) respiration in animals
(d) photosynthesis in plants
(e) operation of an acetylene torch
13.
The catalytic converter in an automobile oxidizes carbon monoxide, CO, to carbon dioxide, CO2,
2CO + O 2 → 2CO2
How many litres of oxygen are needed to oxidize 100 L of carbon monoxide at constant
temperature and pressure?
(a) 18 L
(b) 36 L
(c) 50 L
(d) 100 L
(e) 200 L
14.
What volume of argon gas at 200 kPa and 25°C must be added to a 1.00-litre glass flask containing
nitrogen gas at 140 kPa and 25°C to give a mixture of gases having a total pressure of 420 kPa at
25°C?
(a) 1.40 L
(b) 1.70 L
(c) 2.00 L
(d) 2.86 L
(e) 3.10 L
15.
Gases are most effectively liquefied by
(a) raising the temperature and lowering the pressure.
(b) raising the pressure and lowering the temperature.
(c) lowering both the temperature and pressure.
(d) raising both the temperature and pressure.
(e) lowering the temperature and keeping the pressure unchanged.
16.
If the temperature and pressure are the same, one gram of hydrogen gas has about the same number
of atoms as
Atomic Molar Masses
H
1.0 g⋅mol-1
N
14.0 g⋅mol-1
(a) 1 g of nitrogen gas.
(b) 2 g of nitrogen gas.
(c) 7 g of nitrogen gas.
(d) 14 g of nitrogen gas.
(e) 28 g of nitrogen gas.
17.
According to the Avogadro Principle, one litre of gaseous hydrogen and one litre of gaseous
ammonia contain the same number of
(a) atoms at standard conditions.
(b) molecules at all conditions.
(c) molecules at standard conditions only.
(d) atoms if conditions in both containers are the same.
(e) molecules if conditions in both containers are the same.
Last Revised by D Lougheed 00/7/3
Page 30
18.
One litre of gaseous krypton is compared to one litre of gaseous neon, both at standard
temperature and pressure. Select the correct statement.
(a) The average neon atom hits the walls of its container with more force than the average krypton
atom does in its container.
(b) The average krypton atom moves more slowly than the average neon atom.
(c) Krypton and neon atoms have the same average speed.
(d) Krypton atoms have a greater average kinetic energy than the neon atoms do.
(e) Neon and krypton atoms hit the walls of the containers with the same frequency.
19.
Which temperature on the Celsius scale corresponds to 257 K on the Kelvin scale?
(a) -16°C
(b) -26°C
(c) 273°C
(d) 347°C
(e) 520°C
20.
When the following equation is balanced, what is the coefficient of oxygen, O2?
2C4H10(g) + ? O2(g) → ? CO2(g) + ? H2O(g)
(a) 7
(b) 9
(c) 13
(d) 15
(e) 18
21.
Which one of the following procedures is the least hazardous?
(a) Adding water to concentrated sulfuric acid.
(b) Adding concentrated sulfuric acid to water.
(c) Adding finely-divided calcium metal powder to acid.
(d) Adding a large piece of sodium metal to water.
(e) Burning potassium metal wire in fluorine gas.
22.
The correctly-matched names and formulas below are
1- Sodium sulfite
X- Na2SO4
2- Sodium sulfate
Y- Na2S
3- Sodium sulfide
Z- Na 2SO3
(a) 1X, 2Y, 3Z
(b) 1X, 2Z, 3Y
(d) 1Z, 2Y, 3X
(e) 1Z, 2X, 3Y
23.
24.
The analysis by mass of a pure white powder is:
H 5.61%
C 5.60%
O 67.29%
Na 21.50%
Which formula is consistent with this analysis?
Atomic Molar Masses
H 1.01 g·mol-1
C 10.8 g·mol-1
O 16.0 g·mol-1
Na 22.99 g·mol-1
(a) Na2CO3·10H2O
(b) Na2CO3·NaOH
(d) Na2CO3·6H2O
(e) NaHCO3
(c) 1Y, 2X, 3Z
(c) Na2CO3·NaHCO 3
If X represents any of the elements of the carbon family, then the general formula for the hydrogen
compound of X is
(a) XH5
(b) X2H3
(c) XH
(d) XH 2
(e) XH4
Last Revised by D Lougheed 00/7/3
Page 31
25.
Which processes are endothermic?
(1) Mg(s) → Mg(liquid)
(2) Ca+ (g) + e- → Ca(g)
(3) Cl-(g) → Cl(g) + e(4) CO2(g) → CO2(s)
(a) (1) only
(b) (1) and(3) only
(d) (2) and(4) only
(e) (2),(3) and(4) only
(c) (1) and(4) only
26.
Approximately how many molecules are in 11 g of carbon dioxide, CO2, gas?
Atomic Molar Masses
C 12.0 g·mol-1
O 16.0 g·mol-1
(a) 1.5 x 1023
(b) 3.0 x 1023 (c) 6.0 x 1023 (d) 2.4 x 1023 (e) 1.2 x 1023
27.
Hydrogen gas is a product in one of the following cases. Which one?
(a) Calcium oxide is warmed with ammonium chloride.
(b) Aqueous hydrogen peroxide is added to an aqueous solution of iron(III) nitrate.
(c) Aluminum turnings are heated with hot, concentrated potassium hydroxide solution.
(d) Copper is placed in dilute, aqueous nitric acid.
(e) Solid sodium carbonate is added to dilute, aqueous hydrochloric acid.
28.
Diborane, B2H6, has been used as a rocket fuel. It reacts with liquid oxygen according to the
equation
B2H6 + 3O 2 → B2O3 + 3H 2O
What mass of oxygen is required to react with 1.00 g of diborane?
Atomic Molar Masses
B 10.8 g·mol-1
H 1.01 g·mol-1
O 16.0 g·mol-1
(a) 1.16 g
(b) 1.74 g
(c) 3.47 g
(d) 6.94 g
(e) 10.4 g
29.
Sodium hypochlorite, NaClO, is prepared by the following reaction:
2 NaOH + Cl 2 → NaCl + NaClO + H 2O
If 65 g of chlorine, Cl2, is bubbled into a solution containing 80 g of sodium hydroxide, which
component limits the quantity of sodium hypochlorite formed?
Atomic Molar Masses
H 1.01 g·mol-1
Na 23.0 g·mol-1
O 16.0 g·mol-1
Cl 35.5 g·mol-1
(a) Cl2
(b) NaCl
(c) H2O
(d) NaOH
(e) NaClO
Last Revised by D Lougheed 00/7/3
Page 32
30.
When 40 g of copper is heated with 4 g of sulfur, all of the sulfur is converted to Cu2S according to
the reaction:
2Cu + S → Cu2S
Approximately how many grams of copper remain uncombined?
Atomic Molar Masses
Cu 63.5 g·mol-1
S 32 g·mol-1
(a) 4 g
(b) 8 g
(c) 16 g
(d) 24 g
(e) 32 g
31.
How many litres of oxygen gas, O2, measured at STP, will be required to burn 1.00 mol of
acetylene gas, C2H2?
C2H2(g) + 5/2O2(g) → 2CO2(g) + H2O(g)
(a) 8.90 (b) 56.0
(c) 67.2
(d) 89.0
(e) 112
32.
A sample of pure strontium metal, Sr, weighing 1.350 g was quantitatively converted to 1.597 g of
pure SrO. If the atomic weight of oxygen is taken to be 16.0, what is the atomic weight of
strontium?
(a) 13.5 (b) 16.0
(c) 18.9
(d) 87.4
(e) 100.9
33.
If one mole of an acid neutralizes two moles of a base, then
(a) the acid is twice as concentrated as the base.
(b) the base is twice as concentrated as the acid.
(c) one mole of acid supplies one-half mole of hydrogen ions.
(d) one mole of acid supplies one mole of hydrogen ions.
(e) one mole of acid supplies two moles of hydrogen ions.
34.
In going through the three physical states water would normally undergo
(a) changes in mass.
(b) no energy changes.
(c) changes in weight.
(d) changes in density.
(e) changes in composition.
35.
As acetic acid is slowly added to a solution of ammonium hydroxide, the conductivity increases
because
(a) a soluble compound is formed.
(b) acetic acid dissociates readily.
(c) the pH of the solution changes.
(d) the number of ions in solution increases. (e) neutralization is an exothermic reaction.
36.
Assuming that 1 L of HCl solution contains two times the Avogadro number of ions, the molarity
of HCl in this solution is
(a) 1.0
(b) 2.0
(c) 3.0
(d) 6.0
(e) 0.5
37.
AB2 is the salt of a strong acid and a weak base. A 0.02 mol/L solution of this salt is a saturated
solution at 25°C What is the concentration of B- ions in solution?
(a) 1.0 x 10-7 mol/L
(b) 4.0 x 10-4 mol/L
(c) 1.0 x 10-3 mol/L
(d) 2.0 x 10-2 mol/L
(e) 4.0 x 10-2 mol/L
Last Revised by D Lougheed 00/7/3
Page 33
38.
Identify all the spectator ions in the following reaction:
Pb(NO 3)2(aq) + 2NaI(aq) → Pbl2(s) + 2NaNO3(aq)
(1) Pb2+ (aq)
(2) NO 3-(aq)
(3) Na+ (aq)
(4) I-(aq)
(a)(3) only
(b)(1) and(3) only
(c)(1) and(4) only
(d)(2) and(3) only
(e)(1),(2) and(4) only
39.
Which one of the following oxides is the most basic?
(a) CaO (b) CO2
(c) Cl2O7
(d) P4O10
(e) N2O5
1998
1.
A beta particle is
(a) the nucleus of a helium atom.
(c) also called a photon.
(e) a negatively-charged hydrogen ion.
(b) negatively-charged and has mass number zero.
(d) a pair of electrons.
2.
Here is one method of separating and isolating the components of a mechanical mixture of 0.1 mm
diameter glass beads, iron filings, iodine, and table salt:
(i) In a fume hood, gently heat the mixture in a tall beaker covered by a watch glass, then carefully
lift off the watch glass and remove component(1) which is attached to its underside.
(ii) To the cooled residue in the beaker add warm water and stir. This dissolves component(2).
(iii) Filter the solution plus undissolved material, and wash with warm water. This leaves
component(3) &(4) on the filter paper.
(iv) Evaporate the filtrate to recover component(2).
(v) Spread the residue that was on the filter paper on a glass plate and repeatedly pass a magnet
over the mixture. This removes component(3), which is attached to the magnet.
Which is the only correct identification of the components?
(a) (1) iodine,(2) iron filings,(3) salt,(4) glass beads
(b) (1) iodine,(2) glass beads,(3) iron filings,(4) salt
(c) (1) glass beads,(2) iodine,(3) salt,(4) iron filings
(d) (1) salt(2) iodine,(3) iron filings,(4) glass beads
(e) (1) iodine(2) salt,(3) iron filings,(4) glass beads
3.
An element, X, has only two isotopes, of relative masses 24.01 and 26.01, and the relative atomic
mass of a natural sample of the element is 24.31. What is the percentage abundance of atoms of the
heavier isotope?
(a) 7%
(b) 15%
(c) 30%
(d) 60%
(e) 85%
4.
Which molecule has no lone pairs of electrons on the underlined atom?
(a) OF2
(b) H3P
(c) NF3
(d) CH4
Last Revised by D Lougheed 00/7/3
(e) HCl
Page 34
5.
The N 2 molecule is isoelectronic with
(1) O2
(2) NO +
(3) CO
(4) NO (a)(1) and(3) only
(b)(2) and(4) only
(d)(2) and(3) only
(e)(2),(3) and(4) only
(c)(3) only
6.
In which one of the following compounds do the bond(s) have the greatest ionic character?
(a) PCl5
(b) CCl4
(c) AlCl3
(d) Cl2
(e) NaCl
7.
When two atoms share a pair of electrons, the bond formed is
(a) ionic
(b) double
(c) covalent
(d) bivalent
(e) electrovalent
8.
Since sodium and potassium are both members of Group 1A in the periodic table, a sodium and a
potassium atom have the same
(a) atomic mass.
(b) number of protons in their nuclei.
(c) atomic number and the same nuclear charge.
(d) characteristic of losing one electron per atom to form an ion.
(e) total number of electrons around the nucleus.
9.
Which molecule has the greatest bond dissociation energy?
(a) O2
(b) Cl2
(c) H2
(d) N2
(e) F2
Which of these metals combines most readily with oxygen?
(a) zinc
(b) iron
(c) copper
(d) sodium
10.
(e) aluminum
11.
According to Avogadro's law, at the same temperature and pressure, which sample of gas contains
the same number of particles as one litre of oxygen, O2?
(a) 1 litre of helium, He
(b) 2 litres of neon, Ne
(c) 3 litres of carbon dioxide, CO2
(d) 2 litres of hydrogen, H2
(e) 2.5 litres of methane, CH4
12.
One litre of a certain gas has a mass of 4 g at STP. Given that the molar volume of an ideal gas
under standard conditions is 22.4 L, which one of the following statements is correct?
(a) The gas is helium.
(b) The molar mass of the gas is 4 g/mol.
(c) The molar mass of the gas is 89.6 g/ mol. (d) 6 x 1023 molecules of the gas have a mass of 4 g.
(e) There are two atoms in each molecule of the gas.
13.
A gas occupies a 1.5 L container at 25°C and 2.0 atm. What pressure would be expected if the gas
is tranferred to a 3.0 L container at the same temperature?
(a) 1.0 atm
(b) 2.0 atm
(c) 3.0 atm
(d) 4.0 atm
(e) 5.0 atm
14.
An ideal gas is one in which the molecules
(a) are all monatomic.
(b) have an absolute temperature of 0°C.
(c) do not interact with each other.
(d) can be liquefied above absolute zero.
(e) tend to stick to the walls of the container.
Last Revised by D Lougheed 00/7/3
Page 35
15.
Which graph represents the relationship between the volume of an ideal gas and its temperature(in
Kelvin) at constant pressure?
(a)
(b)
(c)
(d)
(e)
16.
At what temperature is the average kinetic energy of the molecules in a gas twice as great as at
100°C?
(a) 137 K
(b) 273 K
(c) 373 K
(d) 546 K
(e) 746 K
17.
The Haber process for the industrial production of ammonia is:
N2 + 3 H 2 → 2 NH 3
This reaction is an example of
(a) a substitution reaction.
(b) a displacement reaction.
(c) a combination reaction.
(d) a decomposition reaction.
(e) an elimination reaction.
18.
An oxide of nitrogen contains 36.4% oxygen by mass, and its relative molecular mass is near 90.
Which oxide of nitrogen is it?
Relative Atomic Mass
H 1.0
N 14.0
O 16.0
(a) NH4NO 3
(b) N3O3
(c) N4O2
(d) N2O4
(e) N2O5
19.
What substance is a nonelectrolyte in an aqueous solution?
(a) ammonia
(b) ethanoic(acetic) acid
(d) carbon tetrachloride
(e) calcium hydroxide
(c) hydrogen fluoride
20.
Which equation is not balanced?
(a) 2 C + SiO2 → Si + 2 CO
(b) 2 Mg2Sn + 8 H2O → 2 SnH4 + 4 Mg(OH)2
(c) H3CBr + Mg → H3CMgBr
(d) 3 Pb + 8 HNO3 → 3 Pb(NO 3)2 + 3 NO + 4 H2O
(e) 2 NaOH + Cl2 → NaCl + NaClO + H 2O
21.
In which one of the following reactions(all occur in pure water) would a precipitate be most likely
to form?
(a) KOH(aq) + H 2O(l) ?
(b) Ag(NO3)(aq) + NaCl(aq) ?
(c) KOH(aq) + HBr(aq) ?
(d) Na2SO4(aq) + KNO 3(aq) ?
(e) NaNO 3(aq) + HBr(aq) ?
22.
Consider the unbalanced expression:
? Cu(s) + ? NO 3-(aq) + ? H+ (aq) →? Cu2+ (aq) + ? NO(g) + ? H2O(l)
Which set of coefficients correctly balances the equation?
(a) 4, 5, 3, 8, 2, 3
(b) 3, 2, 8, 7, 2, 4
(c) 2, 4, 3, 8, 3, 3
(d) 3, 1, 8, 7, 4, 2
(e) 3, 2, 8, 3, 2, 4
Last Revised by D Lougheed 00/7/3
Page 36
23.
Which processes are exothermic ?
(1) condensing steam on a cool surface
(2) converting solid carbon dioxide to gaseous carbon dioxide in cold, dry air
(3) dissolving KOH in water
(4) expanding a gas
(a) (1),(3) and(4) only
(b) (1) and(3) only
(c) (2) and(4) only
(d) (4) only
(e) (1) and(4) only
24.
Which procedure could be used to determine whether a solution is saturated?
(a) measure the volume
(b) evaporate the solution
(c) cool the solution slowly
(d) warm the solution slowly
(e) add a crystal of the solute
25.
Since sodium is an active metal it
(a) occurs free in nature.
(b) forms ions readily.
(c) gains electrons readily.
(d) forms unstable compounds.
(e) liberates oxygen when it reacts with water.
26.
Copper oxide(CuO) reacts with hydrogen(H2) and produces copper(Cu) and water(H2O). How
many moles of water can 240 g of CuO produce?
Atomic Molar Mass
Cu 63.5 g/mol
H 1.0 g/mol
O 16.0 g/mol
(a) 1.0 mol
(b) 6.0 mol
(c) 3.0 mol
(d) 18 mol
(e) 54 mol
27.
How many moles of H 2O are there in 0.6 L of water?(The density of water is 1.00 g/mL and its
concentration is 55.5 M at 25°C)
(a) 0.6 mol
(b) 6.0 mol
(c) 19 mol
(d) 33 mol
(e) 37 mol
28.
For the following reaction:
2 NaOH + H2SO4 → Na2SO4 + 2 H 2O,
how many millilitres of 0.10 M sodium hydroxide solution exactly neutralize 10 mL of 0.20 M
sulfuric acid?
(a) 2.0
(b) 4.0
(c) 10
(d) 20
(e) 40
29.
Gaseous hydrogen burns in gaseous oxygen and water is produced. If 6.0 mol of hydrogen is
burned with 4.0 mol oxygen and the reaction is as complete as possible, how many moles of the
excess, non limiting reactant are left at the end of the experiment?
(a) 1.0 mol
(b) 2.0 mol
(c) 3.0 mol
(d) 4.0 mol
(e) 6.0 mol
Last Revised by D Lougheed 00/7/3
Page 37
30.
If 4.0 g of sodium hydroxide is dissolved in enough water to make 400 mL of solution, what is the
molar concentration of the solution?
Relative Atomic Mass
Hydrogen 1.0
Oxygen 16.0
Sodium 23.0
(a) 0.010 mol/L (b) 0.040 mol/L
(c) 0.25 mol/L
(d) 0.40 mol/L
(e) 10 mol/L
31.
At 25°C, vinegar is about 300 times more acidic than pure water, which has a pH of 7.0. What is
the approximate pH of vinegar?
(a) 1.0
(b) 2.5
(c) 3.1
(d) 4.0
(e) 4.5
32.
If a sulfuric acid solution has a density of 1.29 g/mL and is 38% by mass sulfuric acid, what is the
molar concentration of sulfuric acid?
Relative Atomic Mass
Hydrogen 1.0
Oxygen 16.0
Sulfur 32.0
(a) 10 mol/L
(b) 5.0 mol/L (c) 0.98 mol/L (d) 0.49 mol/L (e) 0.38 mol/L
33.
A small amount of solid calcium hydroxide is gently swirled in a test tube almost full of water until
no further change occurs. Most of the solid does not dissolve. The resulting solution is
(a) dilute and supersaturated.
(b) dilute and saturated.
(c) dilute and unsaturated.
(d) concentrated and unsaturated.
(e) concentrated and saturated.
34.
Why is it dangerous to dilute sulphuric acid by pouring water into the concentrated acid?
(a) The heat evolved may rapidly convert the water into steam.
(b) A fire may be started.
(c) A poisonous gas may be given off.
(d) The water may decompose.
(e) The acid could solidify and break the container.
35.
Glucose(C6H12O6) and glycerol(C3H8O3) are both nonelectrolytes. Compare a solution of 10 g of
glucose in 1000 g water with a solution of 10 g of glycerol in 1000 g water. Choose the correct
statement:
(a) Both solutions freeze at 0°C.
(b) Both solutions freeze at the same temperature, which is above 0°C.
(c) Both solutions freeze at the same temperature, which is below 0°C.
(d) The glycerol solution has a lower freezing point than the glucose solution.
(e) The glucose solution has a lower freezing point than the glycerol solution.
36.
In an aqueous solution, salts exist in the form of
(a) crystals
(b) molecules (c) atoms
(d) ions
Last Revised by D Lougheed 00/7/3
(e) dimers
Page 38
37.
When 20 g of the compound XY is dissolved in water to make 250 mL of a solution, a 0.500 M
solution is obtained. What is the molar mass of XY?
(a) 20.0 g
(b) 40.0 g
(c) 80.0 g
(d) 100 g
(e) 160 g
38.
For the following reaction:
2 As(s) + 3 NaOH(aq) → Na3AsO 3(aq) + AsH 3(g),
what volume of arsine gas(AsH3), measured at STP, would be produced if 25 g of arsenic reacts
with excess NaOH?(The molar volume of an ideal gas under standard conditions is 22.4 L)
Atomic Molar Mass
As 74.9 g/mol
(a) 3.7 L (b) 7.5 L
(c) 11 L
(d) 15 L
(e) 22 L
39.
What hydrogen ion concentration results from mixing 25 mL of 0.023 mol/L Ba(OH)2 solution with
125 mL of 0.014 mol/L HBr solution?
(a) 0.0092 mol/L
(b) 0.0078 mol/L
(c) 0.0020 mol/L
(d) 0.0040 mol/L
(e) 0.0063 mol/L
1999
1.
The letter Z represents any one of several atoms. Choose the one correct statement:
(a) The number of protons in 14
(b) The number of neutrons in
6 Z is 8.
(c)
(d)
13
6 Z means that Z has atomic number 6 and
12
12
6 Z and 6 Z are isotopes of one element.
13
6 Z
is 13.
mass number 7.
(e) Neutral atoms of
12
6 Z have
2.
Which two species have the same charge and mass number?
(a) a neutron and a hydrogen atom
(b) an electron and a positron
(c) an electron and a H ion
(d) a positron and an electron
(e) a hydrogen atom and a positron
3.
How many valence electrons are there in Cl- ?
(a) 7
(b) 8
(c) 17
(d) 6
6 electrons.
(e) 18
4.
Which one of the following has the most ionic character?
(a) CsF (b) Rb2S
(c) KCI
(d) NaBr
(e) LiI
5.
The second ionization energy of an element, M, in the gaseous state, is the energy required to
remove one mole of electrons from
(a) one-half of a mole of M atoms.
(b) one mole of M atoms.
(c) one mole of M+ ions.
(d) one mole of M2+ ions.
(e) one mole of M3+ ions.
6.
In a water molecule the H-O-H angle is nearest to
(a) 1 80°. (b) 1 20°.
(c) 109°
(d) 90°.
Last Revised by D Lougheed 00/7/3
(e) 60°.
Page 39
7.
The N 2 molecule is isoelectronic with
(1 ) O2
(2) NO +
(3) CO
(4) NO
(a) (1) and (3) only.
(b) (2) and (4) only.
(c) (3) only.
(d) (2) and (3) only.
(e) (2), (3) and (4) only.
8.
The region of the periodic table (see the cover of this exam) in which the elements of greatest
density are found is the
(a) top, right.
(b) top, left. (c) bottom, right.
(d) bottom, left.
(e) bottom, centre.
9.
The electron dot diagram for PH3(g) is
H
(a)
P
H
H
P
H
H
P
H
H
(b)
10. Which compound has no covalent bonds?
(a) Na2S04
(b) HCI03
(c) CH3CI
H
(c)
(d) NaN03
H
H
(d)
P
H
H
(e) KCI
11. Exactly 2.00 L of an ideal gas is cooled from 100°C to 30°C. What is the new volume of the gas if
the pressure is kept constant?
(a) 0.60 L
(b) 1.62 L
(c) 1.80 L
(d) 2.46L
(e) 36.2 L
12. What temperature is half as hot as 0°C?
(a) 50 K (b) 137K
(c) 100K
(d) 273 K
(e) 546 K
13. In a mixture of N2 and O2 gases, the N2 molecules and the O2 molecules have the same
(a) average velocity.
(b) average momentum.
(c) molecular mass.
(d) average kinetic energy.
(e) partial pressure.
14. Which statement correctly describes Avogadro's hypothesis about gases?
(a) At the same temperature, the average kinetic energy of all gases is the same.
(b) At constant temperature, pressure and volume are directly proportional.
(c) The volume of a gas is directly proportional to the volume of its molecules.
(d) At the same temperature, all gases exert the same pressure on the walls of their containers.
(e) The volume is proportional to the number of moles present, if temperature and pressure are
constant.
15. A balloon of volume 5.0 L at 27°C contains helium at a pressure of 120 kPa. How much helium is
in the balloon?
(a) 5.0 mol
(b) 1.2 mol (c) 0.17 mol (d) 0.21 mol (e) 0.24 mol
Last Revised by D Lougheed 00/7/3
Page 40
16. Select the one incorrect statement about ideal gases.
(a) The total pressure of a mixture of non-reacting gases is equal to the sum of the partial pressures
of all the gases in the mixture.
(b) The volumes of gases used or produced in a chemical reaction, and measured at the same
temperature and pressure, can be expressed as the ratios of small, whole numbers.
(c) A plot of V against P will pass through the pointP=0, V=0.
(d) A plot of V against T extrapolated to V = 0 for a gas will cross the T-axis at absolute zero.
(e) Equal volumes of two gases contain the same number of molecules, provided the pressure and
temperature are the same.
17. Phantasy Phil wrote five different equations for the reaction of aqueous ammonia with aqueous
hydrochloric acid. Which one is correct?
(a) NH3 + HCI → NH 2CI + H 2
(b) NH 3 + HCI → NH 4+ + Cl
(c) NH3 + 3HCI → NC13 + 3H 2
(d) 2NH 3 + HCI + 2H20 → NH 4+ + NOCI + OH- 3H2
(e) 2NH3 + 2HCI → NH 2OH + NH4+ + 2CI- + H +
18. Which processes are endothermic?
(1 ) CO2(s) → C02(g)
(2) Cl(g) + e- → Cl-(g)
(3) Ca(g) → Ca+ (g) + e(4) Mg(liquid) → Mg(s)
(a) (2), (3) and (4) only
(b) (1) and (3) only
(d) (1 ) only
(e) (1) and (4) only
(c) (2) and (4) only
19. The reaction,
2 Na(s) + O 2(g) → Na2O2(s),
(a) a displacement.
(d) a synthesis.
(b) a decomposition .
(e) a substitution .
is best described as
(c) an elimination .
20. When this equation is balanced and the smallest whole-number coefficients appear, what is the
coefficient of 02?
?Cr2O3 + ? KOH + ?O2 → ? K2CrO4 + ?H20
(a) 2
(b) 3
(c) 4
(d) 6
(e) 8
21. Three moles of ammonium nitrate contain how many moles of nitrogen atoms?
(a) Three
(b) Six
(c) Nine
(d) Eighteen (e) Twenty-seven
22. Amixture of nitrogen, oxygen and carbon dioxide contains a total of 6.0 mol of these gases, and the
mole fraction of nitrogen is 0.40. What mass of nitrogen is present in this mixture?
(a) 34 g (b) 56 g
(c) 67 g
(d) 208 g
(e) 250 g
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Page 41
23. In a chemical reaction between two substances, the limiting reagent must be the substance that
(a) has the lower mass.
(b) has the smaller number of moles.
(c) is used up most slowly.
(d) is present in excess.
(e) is used up first.
24. What is the formula for ferric sulfate?
(a) Fe2(SO4)3
(b) Fe3(SO4)2
(c) Fe2(SO3)3
25. In which pair of anions do both names end in '-ate'?
(a) Cl-1, Cl03-1
(b) Cl03-1, NO 3-1
-1
-1
(d) HS , HSO4
(e) Cl02-1, NO 2-1
(d) Fe3SO4
(e) FeSO4
(c) NO2-1, NO 3-1
26. How many moles of rubidium peroxide, Rb2O2(s) can be made from 1.0 mol of Rb(s) and 2.0 mol of
02(g)?
(a) 3.0 mol
(b) 2.0 mol (c) 1.5 mol
(d) 1.0 mol
(e) 0.50 mol
27. Apure white powder was found to have the following composition (percent by mass):
Carbon 14.29% Hydrogen 1.19% Sodium 27.38% Oxygen 57.14%
Which formula is consistent with this analysis?
(a) NaHCO3
(b) Na2CO3⋅6H2O
(c) Na2CO3⋅NaHCO 3
(d) Na2CO3⋅NaOH
(e) Na2CO3⋅10H20
28. If 50.0 g MgCO3 is fully converted into MgO upon heating, what is the maximum mass of MgO
produced?
(a) 20.2 g(b) 23.9 g
(c) 24.9 g
(d) 26.6g
e) 37.6g
29. What is the value of ∆H for the reaction
3 H2(g) + N2(g) → 2 NH 3(g)
H-H
435 kJ/mol
(a) -83 kJ(b) -122 kJ
given the following bond energies?
N-H
389 kJ/mol N-N
946 kJ/mol
(c) +122kJ
(d) -1084 kJ (e) -1770 kJ
30. Aluminum chloride forms a hydrate with the formula Al2CI6⋅nH2O. The substance was analyzed to
determine the percentage water in the hydrate. In the analysis the crucible and the sample of
aluminum chloride were heated to constant mass.
Mass of crucible
23.40 g
Mass of crucible and hydrate
31.44 g
Mass of crucible and residue after heating
27.84 g
The percentage of water in the hydrate is
(a) 31.4%
(b) 36.0%
(c) 44.8%
(d) 55.2%
(e) 67.9%
Last Revised by D Lougheed 00/7/3
Page 42
31. Water is added to 50 mL of 2.0 mol/L aqueous hydrochloric acid to make one litre of solution.
During this dilution, the pH
(a) changes by less than 0.1 pH unit.
(b) rises by about 0.3 pH unit.
(c) rises by about 1 pH unit.
(d) falls by about 1 pH unit.
(e) falls by about 0.3 pH unit.
32. Select the one correct statement about a concentrated solution of a strong electrolyte in water.
(a) Its boiling point is below 100°C.
(b) Its freezing point is above 0°C.
(c) It is a poorer conductor of electricity than pure water.
(d) Its vapour pressure is lower than that of pure water at the same temperature.
(e) It contains a high proportion of neutral electrolyte molecules.
33. What minimum volume of 0.123 mol/L aqueous HCI is needed to neutralize 20.0 mL of 0.175
mol/L aqueous NaOH?
(a) 56.3 mL
(b) 40.0 mL (c) 35.6 mL (d) 28.5 mL (e) 17.6 mL
34. Potassium hydroxide, KOH, is added to a solution of ammonium nitrate, NH4NO 3, in water, and
the solution is warmed. What gas is evolved?
(a) Ammonia
(b) Nitrogen
(c) Hydrogen
(d) Oxygen (e) Nitrogen monoxide
35. Four different solid substances are observed in nearly saturated aqueous solutions:
• substance (1) is more soluble in cold than in hot water
• substance (2) is more soluble in hot than
• dissolving substance (3) cools the solution
• dissolving substance (4) warms the solution
Which substances dissolve endothermically?
(a) Substances (1) and (2) only
(b) Substances (2) and (3) only
(c) Substances (3) and (4) only
(d) Substances (1) and (3) only
(e) Substances (2) and (4) only
36. Identify all the spectator ions in the following reaction:
Pb(NO 3)2(aq) + 2 Kl(aq) → Pbl2(s) + 2 KNO3(aq)
2+
(1) Pb (aq)
(2) NO3-1(aq)
(3) I-1(aq)
(4) K+ (aq)
(a) (1), (2) and (3) only
(b) (1) and (3) only
(c) (2) and (4) only
(d) (4) only
(e) (1) and (4) only
37. Which gas when present in the air we breathe causes physical discomfort to humans, even at low
concentration?
(a) Nitrogen
(b) Argon
(c) Helium
(d) Sulfur dioxide
(e) Carbon dioxide
Last Revised by D Lougheed 00/7/3
Page 43
38. An odorless, colourless, tasteless gas is thought to be oxygen. Which observation would support
this suggestion?
(a) Burning the gas in air produces only water. (b) The gas extinguishes a flame.
(c) The gas turns limewater milky.
(d) A glowing splint bursts into flame in the gas.
(e) The gas decolorizes a brown apple.
39. Of the following, what is the most abundant nitrogen-containing pollutant in the Earth's lower
atmosphere?
(a) NO2 (b) Li3N
(c) NH4CI
(d) N2O
(e) N2
2000
1.
What volume of F2(g) must react with excess Br2(g) to give 2.46 L of BrF5(g)?
(a) 2.46 L
(b) 6.15 L
(c) 0.984 L
(d) 12.3 L
(e) 0.492 L
2.
In which one of the following compounds is the oxidation state of chlorine the most positive?
(a) HCl
(b) Cl2
(c) NaCl
(d) HClO3
(e) BrCl
3.
A compound contains only C, H, and N. Analysis shows that the compound is 75.9% C by mass
and 17.7% N by mass. What is the empirical formula of the compound?
(a) C3H4N
(b) C4H4N
(c) C5H5N
(d)
C6H6N2
(e)
C10H7N2
4.
A mixture of BaCl2 and Ba(NO3)2, with a total mass of 2.00 g, is dissolved in water and treated
with excess AgNO3 solution. The precipitate (AgCl) is dried and found to weigh 0.688 g. How
much BaCl2 was in the original mixture?
(a) 1.00 g
(b) 0.500 g
(c) 2.00 g
(d) 0.688 g
(e) 1.33 g
5.
Which of the following involves a chemical change?
(1) evaporation (3) oxidation
(2) neutralization
(a) (1), (2), (3), and (4)
(b) (1) and (3)
(d) (1) only
(e) (2), (3), and (4)
6.
7.
What value of x is required to balance the reaction
Be3N2 + x H2O → 3 Be(OH)2 + 2 NH 3 ?
(a) 1
(b) 3
(c) 5
(d) 6
(4) sublimation
(c) (2) and (3)
(e) 12
Suppose 6.0 mot N2O and 8.0 mol O2 react via
2 N2O + 3 O 2 → 4 N O 2
to produce as much N 2O as possible. Which one of the following statements is correct?
(a) 0.33 mol O2 remains
(b) 0.67 mol O2 remains
(c) 0.33 mol N2O remains
(d) 0.67 mol N2O remains
(e) 4.0 mol N2O and 5.0 mol O2 remain
Last Revised by D Lougheed 00/7/3
Page 44
8.
Which one of the following reactions, when carried out in aqueous solution, produces a precipitate?
(a) H2SO4 + 2 KOH →
(b) CaCl2 + Na2CO3 →
(c) 2 NH4Cl + K2SO4 →
(d) HNO3 + NaOH →
(e) 2 NaOH + H 2S →
9.
In the reaction
AgNO3(aq) + HCl(aq) → HNO3(aq) + AgCl(s),
the spectator ions are
(a) Ag+ and NO3(b) H+ and Cl(d) Ag+ and Cl(e) NO3- and Cl-
(c) H+ and NO3-
10. Identify the element X from the following information.
(i) At 25°C and 101 kPa, it is a liquid.
(ii) The formula of its sodium salt is NaX
(iii) Its gas phase molecules have the formula X2
The element X could be,
(a) mercury
(b) hydrogen (c) nitrogen (d) sulfur
(e) bromine
11. The correct formula for sodium nitrate is
(a) Na3N
(b) NaN
(c) NaNO
(e) NaNO
(d) NaNO 3
12. Copper(ll) oxide reacts with hydrogen gas, producing copper metal and water. What is the correct
chemical equation for this reaction?
(a) Cu2O2(s) + 2 H 2(g) → 2 Cu(s) + 2 H 2O(l)
(b) CuO(s) + H2(g) → C(s) + H 2O(l)
(c) Cu2O(S) + 2 H(g) → 2 Cu(s) + H 2O(l)
(d) CuO(s) + 2 H(g) → Cu(s) + H 2O(l)
(e) CuO2(s) + 2 H 2(g) → Cu(s) + 2 H 2O(l)
13. The space shuttle maneuvers in outer space using thrusters that obtain their energy from the
reaction between hydrazine (N 2H4) and dinitrogen tetroxide (N2O4). The equation for the reaction is
3 N2H4(l) + N2O4(l) → 4 N2(g) + 4 H2O(g) + 2H2(g)
and ∆H is -1310 kJ per mole of N 2O4. How much energy is produced per mole of hydrazine?
(a) 13.6 kJ
(b) 40.9 kJ (c) 437 kJ
(d) 1310 kJ (e) 3930 kJ
14. A gas in a flask has a pressure of 193 kPa at 0°C. What is the pressure at 300°C if the volume of
the flask remains constant?
(a) 405 kPa
(b) 92.0 kPa (c) 493 kPa (d) 223 kPa (e) 2509 kPa
15. What is the ratio of oxygen atoms to hydrogen atoms in the mineral cacoxenite,
Fe4(PO 4)3(OH) 3·12H2O?
(a) 1: 1
(b) 5:1
(c) 19:27
(d) 27:15
(e) 15:27
16. An 11.3 g sample of gas occupies a volume of 3.56 L at STP. The molar mass of this gas is
Last Revised by D Lougheed 00/7/3
Page 45
(a) 3.17 g/mol
(d) 71.1 g/mol
(b)11.3 g/mol
(e) 79.7 g/mol
(c) 40.2 g/mol
17. Which of the following statements are true?
(i) At a given temperature, He atoms move faster than Ar atoms.
(ii) The volume of 1.00 mol O2 gas is only two thirds the volume of 1.00 mol O3 gas, at the
same temperature and pressure.
(iii) The volume of 1.00 mol of ideal gas is always 22.4 L.
(iv) In an equimolar mixture of He and Ar gases, helium and argon exert the same pressure.
(a) (i) and (ii)
(b) (i) and (iii)
(c) (ii) and (iv)
(d) (ii) and (iii)
(e) (i) and (iv)
18. What mass of solid sodium hydroxide is required to prepare 2.00 L of a 3.00 M solution?
(a) 40 g (b) 80g
(c) 240 g
(d) 480 g
(e)
667 g
19. A sample of water containing "temporary hardness" was boiled for a few minutes, then cooled and
filtered. The formula of the compound left on the filter paper is most likely
(a) CaCO3
(b) Ca(HCO3)2
(c) CaSO4
(d) CaCl2
(e) Mg(HCO 3)2
20. An aqueous solution was thought to contain a high concentration of chloride ions. To confirm the
presence of chloride ions a chemist would probably add a solution of
(a)barium chloride
(b)sodium nitrate
(c) sodium sulfate
(d) silver chloride
(e) silver nitrate
21. Which of the following metals will react readily with each of (i) cold water (ii) oxygen (iii) dilute
acid?
(a) Na
(b) Mg
(c) Pb
(d) Au
(e) Ti
22. Sulfide ores are one of the principal sources of industrial metals. Which of the following metals does
not occur in substantial quantities as a sulfide ore?
(a) copper
(b) nickel
(c) magnesium
(d) mercury
(e) zinc
23. An aqueous solution of pH 0.0 at 25°C is
(a) slightly acidic.
(b) strongly acidic.
basic.
(c) neutral.
(d) slightly basic.
(e) strongly
24. Complete neutralization of 60 mL of 1.0 M hydrochloric acid solution requires 80 mL of sodium
hydroxide solution. What is the molar concentration of the sodium hydroxide solution?
(a) 1.0 mol/L
(b) 1.5 mol/L
(c) 1.3 mol/L
(d) 0.75 mol/L
(e) 2.7 mol/L
Last Revised by D Lougheed 00/7/3
Page 46
25. Water is a liquid at room temperature, whereas hydrogen sulfide is a gas. This is because
(a) the O—H bond is stronger than the S—H bond.
(b) the H 2O molecule has a permanent dipole moment but the H2S molecule does not.
(c) the hybridization of O in the H2O molecule is different from that of S in the H2S molecule.
(d) the high electronegativity of O leads to strong hydrogen bonding.
(e) oxygen has a smaller ionic radius.
26. When two elements unite to form an ionic crystal, what is the principal force that holds the
particles together?
(a) electrostatic attraction
(b)Van der Waals forces
(c) metallic bonding
(d) covalent attraction
(e) resonance
27. Which one of the following groups forms an isoelectronic series?
(a) V2+ , V3+ , V4+
(b) S2-, Cl-, Ar
(c) F-,Cl-,Br2+
2+
2+
3+
3+
3+
(d) Co , Ni , Zn
(e) Al ,Si , P
28. Which of the following represents the ground state electron configuration of an alkali metal?
(a) 1s22s22p 5
(b)1s2 2s2 2p 6
(c) 1s2 2sl 2p 6 3sl
2
2
6
l
2
2
6
(d) 1s 2s 2p 3s
(e)1s 2s 2p 3s2
29. Which of the following has the greatest bond energy?
(a) HF
(b) HCl
(c) HBr
(d) HI
(e) HAt
30. What is the electron dot diagram for the nitrogen atom?
(a)
N
(b)
N
N
(c)
N
N
(d)
(e)
31. The ground state electron configuration of Cr2+ is
(a) 1s2 2s2 2p 6 3s2 3p 3
(b) 1s2 2s2 2p 6 3s2 3p 6 3d4
(c) 1s2 2s2 2p 6 3s2 3p 6 3d4 4sl
(d) 1s2 2s2 2p 6 3s2 3p 6 3d5 4sl
(e) 1s2 2s2 2p 6 3s2 3p 6 4s2 4p 2
32. Electronegativity is a measure of
(a) the electron affinity of an atom, ion or molecule.
(b) the electromotive force developed between an element and a solution of its salt.
(c) the energy acquired or released in the formation of an anion.
(d) the affinity between the neutrons and electrons.
(e) the power of an atom in a molecule to attract electrons.
33. For the reaction
2 H+ +2 IO 3- + 5 SO32- → 3 I2 + 5 SO42- + H 2O
the reducing agent is
(a) H+
(b) IO3(c) SO32(d) I2
(e) SO42
Last Revised by D Lougheed 00/7/3
Page 47
34. Which describes the atomic structure of 358181Br-1
(a) 35 protons, 81 neutrons, 36 electrons
(c) 46 protons, 35 neutrons, 47 electrons
(e) 35 protons, 46 neutrons, 36 electrons
(b) 36 protons, 45 neutrons, 37 electrons
(d) 35 protons, 46 neutrons, 34 electrons
35. Isotopes of an element have
(a) different atomic numbers.
(b) different numbers of electrons.
(c) the same atomic number and mass number.
(d) the same mass numbers but different atomic numbers.
(e) the same atomic numbers but different mass numbers.
36. The electron dot diagram for carbon dioxide is
O
C
C
O
(a)
O
O
(b)
O
C
O
O
(d)
(c)
C
O
C
O
O
(e)
37. The decomposition of PCl 5 is described by the chemical equation
PCl5 → PCl3 + Cl2
In an experiment, 1.5 grams of Cl2 was obtained from 5.0 grams of PCl5. What was the percent
yield?
(a) less than 5% (b) 6.8%
(c) 30%
(d) 88%
(e) greater than 90%
38. The chemical properties of element 19 will most closely resemble those of
(a) element 9. (b) element 11.
(c) element 18.
(d) element 20.
39. The percent by mass of fluorine in calcium fluoride is
(a) 64.32%
(b) 48.67%
(c) 32.16%
19.16%
Last Revised by D Lougheed 00/7/3
(d) 24.33%
(e) element 36.
(e)
Page 48
AVOGADRO EXAM 2001
UNIVERSITY OF WATERLOO
DEPARTMENT OF CHEMISTRY
17 MAY 2001
TIME: 75 MINUTES
This exam is being written by several thousand students. Please be sure that you follow the instructions below.
We'll send you a report on your performance. Top performers are eligible for a prize.
1. Print your name here:
4. Print your name (last name, first name and optional
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Also fill in the corresponding circles below your
2. Print your school name and city on your STUDENT
RESPONSE sheet.
printed name.
3. Select, and enter on the STUDENT RESPONSE
sheet, one of the following CODE numbers:
5. Now answer the exam questions. Indicate your
choice on the STUDENT RESPONSE sheet by
Code 1
Ontario, now studying grade 11 Chemistry in
a nonsemestered school
Code 2
Ontario, now studying grade 11 Chemistry in
a semestered school
Code 3
marking one letter beside the question number.
•Mark only one answer for each question.
•Questions are all of the same value.
•There is a penalty (1/4 off) for each incorrect
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Ontario, grade 11 Chemistry already
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•Questions are not in order of difficulty.
Code 5
Manitoba or Saskatchewan high school
student
Code 6
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just filling the oval.
Code 8
Alberta or British Columbia high school
student
Be careful that any erasures are complete—make
Code 9
New Brunswick, Newfoundland, Nova
Scotia or Prince Edward Island high school
student
6. Take care that you make firm, black pencil marks,
the sheet white again.
Code 10 Northwest Territories, Nunavut, or Yukon
high school student
Code 11 High school student outside Canada
Code 12 Teacher
H
He
Li
Be
B
C
N
O
F
Ne
Na
Mg
Al
Si
P
S
Cl
Ar
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
Cs
Ba
La*
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
Fr
Ra
Ac**
* Lanthanides
** Actinides
AVOGADRO EXAM 2001 - ANSWERS
1
How many mm3 are there in one m3 ?
A
B
C
2
4
10+6
Al3+
B
B3+
C
N3-
D
V3+
E
Ne3-
10+3
10-3
E
10-9
Two students made independent measurements of
the mass of an object using four different balances.
Their results are shown below.
Student A:
51.6 g, 50.8 g, 53.4 g, 49.3 g
Average value: 51.3 g
Student B:
50.1 g, 49.6 g, 51.0 g, 49.4 g
Average value: 50.0 g
5
The true mass is exactly 51 g. Which statement is
correct?
A
The results of Student A are more accurate but
less precise.
B
The results of Student A are more accurate and
more precise.
C
The results of Student B are more accurate and
more precise.
D
The results of Student B are more accurate and
less precise.
6
How many neutrons are there in one
A
37
B
17
C
18
D
20
E
54
37Cl
atom?
In what region of the periodic table are the atoms with
the smallest covalent atomic radii found?
A
upper left
B
lower left
C
upper right
D
lower right
E
upper centre
None of the above statements is true.
7
3
A
10+9
D
E
Which monatomic ion has an atomic number of 13
and 10 electrons?
The nucleus of any atom, except hydrogen, is made
up of
A
only neutrons.
B
only protons.
C
equal numbers of electrons and protons.
D
equal numbers of protons and neutrons.
E
neutrons and protons.
The first ionization energy of an isolated atom, X(g), is
A
the minimum energy required to remove an
electron from X(g).
B
the maximum energy required to remove an
electron from X(g).
C
the energy released when X acquires an electron
to form X-(g).
D
the minimum energy required to remove an
electron from X-(g)
E
the maximum energy required to remove an
electron from X-(g).
 2001 UNIVERSITY OF WATERLOO AVOGADRO EXAM /2
8
Which one of the following elements would you
expect to be the most similar in chemical properties to
oxygen?
12 A U-tube mercury manometer is open on the right
arm and connected to a gas sample at the other arm
as shown below. The atmospheric pressure is 101
kPa and the difference in levels of mercury is 20 cm.
What is the pressure of the gas in the bulb?
A
carbon
B
nitrogen
A
121 kPa
C
fluorine
B
104 kPa
D
neon
C
94 kPa
E
sulfur
D
98 kPa
E
128 kPa
760 mm Hg = 101 kPa
gas
20 cm
9
Which of the following is not a mixture?
A
brass
B
sodium chloride
C
air
D
seawater
E
stainless steel
13 A 140-g sample of nitrogen gas in a rigid container
exerts a pressure of 203 kPa at 127oC. What is the
volume of the container?
10 Noble gases are usually unreactive but a few
compounds of the noble gases have been
synthesized. Which one of the following chemical
bonds is least likely to form?
A
82 L
B
26 L
R = 8.3145 kPa L K-1 mol-1
C
110 L
N, 14.01 g mol-1
D
160 L
0oC = 273.15 K
E
52 L
A
Xe-O
B
Xe-F
C
Xe-N
D
Kr-F
A
16 g mol 1
E
Ar-F
B
19 g mol 1
C
40 g mol 1
D
80 g mol
E
none of the above
14 A 7.20-L flask contains 20.0 g of an unknown gas at a
pressure of 104 kPa and a temperature of 87oC.
What is the molar mass of the gas?
11 Which compound contains both covalent and ionic
bonds?
A
HClO4
B
CsCl
C
graphite
D
KCN
E
water
Note: Some teachers commented that
HClO4 has ionic and covalent bonds. To the
best of our knowledge, pure HClO4 is a
liquid comprised of molecules with no ionic
bonds. The monohydrate, HClO4$H2O,
+
however, is an ionic solid comprised of H3O
−
and ClO4 ions.
-
-1
 2001 UNIVERSITY OF WATERLOO AVOGADRO EXAM /3
15 What is the total pressure in a 4.55-L container if it
contains 0.0410 mol O2, 0.173 mol N2 and 0.056 mol
He, at a temperature of 167oC?
19 Which of the following has the lowest melting point?
A
CaO(s)
B
Si(s)
C
C6H12O6(s)
A
250 kPa
B
82.4 kPa
C
217 kPa
D
NaNO3(s)
D
0.0232 kPa
E
SiO2(s)
E
2.14 kPa
R = 8.3145 kPa L K-1 mol-1
0oC = 273.15 K
16 Which of the following gaseous compounds behaves
most like an ideal gas at 298 K and 101 kPa?
20 What is the maximum mass of iron that can be
recovered from 1.06 L of 0.20 M Fe2(SO4)3 solution?
A
12 g
Fe, 55.85
B
24 g
S, 32.07
A
NO
B
H2S
C
6.0 g
C
HF
D
80 g
D
N2
E
40 g
E
SO3
17 What is the correct formula of the stable compound
that contains only aluminum and sulfate ions?
A
B
21 A compound of sulfur and phosphorus contains
72.13% sulfur by mass. What is the empirical formula
of this compound?
A
P2S5
B
P2S3
C
PS3
D
P2S
E
PS2
Al2S3
AlSO4
C
Al3S2
D
Al3(SO4)2
E
Al2(SO4)3
18 Which of the following molecules is not planar? (The
central atom is underlined and all other atoms are
bonded to it.)
O, 16.00
S, 32.07
P, 30.97
22 Magnesium burns in oxygen to produce magnesium
oxide, MgO. If 5.0 moles of magnesium and 4.0
moles of oxygen react to produce as much MgO as
possible, how much of the excess reactant remains?
A
SF4
A
1.0 mol Mg
B
BrF3
B
1.0 mol O2
C
SO3
C
1.5 mol O2
D
H2CO
D
3.0 mol Mg
E
AlF3
E
0.5 mol Mg
 2001 UNIVERSITY OF WATERLOO AVOGADRO EXAM /4
23 What volume of 12 M HCl(aq) solution is required for
the preparation of 7.50 L of 0.10 M HCl(aq)?
A
6.3 L
B
63 mL
C
0.16 L
D
0.90 L
E
9.0 mL
26 Gastric fluid in the human stomach has a pH of 1.2.
What is [H+] in gastric fluid?
A
1.2 mol L-1
B
0.12 mol L-1
C
12 mol L-1
D
15.8 mol L-1
E
0.063 mol L-1
24 Consider the unbalanced equation
KMnO4 + HCl → KCl + MnCl2 + Cl2 + H2O.
If the coefficient of KMnO4 in the balanced equation is
taken to be 2, what is the coefficient of HCl ?
A
8
B
16
C
4
D
2
E
5
27 Which of the following is the poorest conductor of
electricity?
A
1.0 M HCl(aq)
B
a saturated, aqueous solution of CCl4
C
molten sodium chloride
D
1.0 M NH3(aq)
E
solid platinum
28 Diamond and graphite are
25 What products result from adding solid calcium oxide
to water?
A
calcium hydroxide
B
calcium hydroxide and hydrogen gas
C
calcium hydride and oxygen gas
D
calcium hydride and calcium hydroxide
E
calcium metal, hydrogen gas, and oxygen gas
A
stereoisomers.
B
enantiomers.
C
allotropes.
D
isotopes.
E
structural isomers.
29 In which reaction does a precipitate form?
A
AgNO3(aq) + NH4NO3(aq) →
B
NH4Cl(aq) + NaOH(aq) →
C
CuSO4(aq) + HNO3(aq) →
D
HNO3(aq) + KOH(aq) →
E
Fe(NO3)2(aq) + Na2S(aq) →
 2001 UNIVERSITY OF WATERLOO AVOGADRO EXAM /5
30 What is the systematic, IUPAC name for Fe2O3 ?
A
B
34 What is the approximate bond angle in the H2O
molecule? (Choose the closest value.)
iron(III) oxide
A
60o
B
90o
C
109o
D
120o
E
180o
iron oxide
C
iron(II) oxide
D
iron (II) trioxide
E
iron trioxide
31 What is the oxidation number of chlorine in HClO2 ?
A
+5
B
+3
C
+7
D
-1
E
0
35 What is the net ionic equation for the reaction that
occurs when aqueous barium chloride reacts with
aqueous sulfuric acid?
32 In the reaction,
A
BaCl2(aq) + H2SO4(aq) → BaSO4(s) + 2HCl(aq)
B
H+(aq) + Cl-(aq) → HCl(g)
C
Ba2+(aq) + SO 4 (aq) → BaSO4(s)
D
Br2(l) + 2OH-(aq) → OBr-(aq) + Br-(aq) + H2O(l)
the reducing agent and the oxidizing agent are,
respectively
A
Br2 and OH-
B
Br2 and Br-
C
OH- and Br2
D
Br2 and Br2
E Br2 and OBr-
E
2-
2Ba2+(aq) + 2Cl-(aq) + 2H+(aq) + SO 4 (aq)
→ BaSO4(aq) + 2HCl(g)
2-
Ba2+(aq) + SO 4 (aq) → BaS(s) + 2O2(g)
36 The addition of HCl to C2H4 produces C2H5Cl. In a
certain experiment, 5.61 grams of C2H4 reacts with
excess HCl and 4.83 grams of C2H5Cl is recovered.
What is the percent yield for the experiment?
A
86.1%
B
37.4%
C, 12.01
C
20.0%
Cl, 35.45
D
16.1%
E
13.9%
H, 1.01
33 Which molecule has a triple bond?
A
C2H2
B
C2H4
C
O2
D
CO2
E
N2H2
 2001 UNIVERSITY OF WATERLOO AVOGADRO EXAM /6
40 A sample of water, initially at 25oC, was heated at a
constant rate of 1.00 kJ per second until the
temperature was 110oC. Which of the following
graphs of temperature versus time best depicts the
variation of temperature with time?
37 Which of the following is not endothermic?
A
CO2(s) → CO2(g)
B
Br2(l) → Br2(g)
C
O(g) + e- → O-(g)
D
H2(g) → 2H(g)
A
E LiF(s) → Li (g) + Cl-(g)
+
38 Which of the following represents the ground
electronic configuration of an isolated halogen atom?
2
1
A
1s 2s
B
1s 2s 2p
C
1s 2s 2p
D
1s 2s 2p 3s 3p 4s 3d
E
1s 2s 2p 3s 3p
B
2
2
4
2
2
6
2
2
6
2
6
2
2
6
2
5
2
5
C
39 What is [Na+] when 35.0 mL of 0.284 M Na2SO4(aq)
and 45.0 mL of 0.196 M NaNO3(aq) are mixed?
Assume the final volume is 80.0 mL.
A
0.234 mol L-1
B
0.172 mol L-1
C
0.248 mol L-1
D
0.359 mol L-1
E
0.382 mol L-1
D
E
 2001 UNIVERSITY OF WATERLOO AVOGADRO EXAM /7
AVOGADRO EXAM 2002
UNIVERSITY OF WATERLOO
DEPARTMENT OF CHEMISTRY
16 MAY 2002
TIME: 75 MINUTES
This exam is being written by several thousand students. Please be sure that you follow the instructions below.
We'll send you a report on your performance. Top performers are eligible for a prize.
1. Print your name here:
4. Print your name (last name, first name and optional
middle initial) on the STUDENT RESPONSE sheet.
Also fill in the corresponding circles below your
2. Print your school name and city on your STUDENT
RESPONSE sheet.
printed name.
3. Select, and enter on the STUDENT RESPONSE
sheet, one of the following CODE numbers:
5. Now answer the exam questions. Indicate your
choice on the STUDENT RESPONSE sheet by
Code 1
Ontario, now studying grade 11 Chemistry in
a nonsemestered school
Code 2
Ontario, now studying grade 11 Chemistry in
a semestered school
Code 3
marking one letter beside the question number.
• Mark only one answer for each question.
• Questions are all of the same value.
• There is a penalty (1/4 off) for each incorrect
answer, but no penalty if you do not answer.
Ontario, grade 11 Chemistry already
completed
• Questions are not in order of difficulty.
Code 5
Manitoba or Saskatchewan high school
student
Code 6
Québec high school student
just filling the oval.
Code 8
Alberta or British Columbia high school
student
Be careful that any erasures are complete—make
Code 9
New Brunswick, Newfoundland, Nova
Scotia or Prince Edward Island high school
student
6. Take care that you make firm, black pencil marks,
the sheet white again.
Code 10 Northwest Territories, Nunavut, or Yukon
high school student
Code 11 High school student outside Canada
Code 12 Teacher
H
He
Li
Be
B
C
N
O
F
Ne
Na
Mg
Al
Si
P
S
Cl
Ar
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
Cs
Ba
La*
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
Fr
Ra
Ac**
* Lanthanides
** Actinides
1
2
One isotope of iron has the symbol 56Fe. How many
protons, neutrons and electrons are there in one atom
of this isotope?
neutrons
26
4
electrons
26
What is the formula of the ionic compound that
contains only magnesium and phosphate ions?
A
MgPO4
B
Mg(PO4)3
A
protons
26
B
26
30
30
C
Mg3PO4
C
26
30
26
D
Mg2(PO4)3
D
30
26
30
E
Mg3(PO4)2
E
56
30
30
There are two naturally occurring isotopes of lithium:
6
Li and 7Li. Assume that the masses of these isotopes
are 6 u and 7 u, respectively. If the average atomic
mass of lithium in nature is 6.941 u, what is the
percent abundance of 7Li in a naturally occurring
sample?
5
Lewis symbols for the atoms of two different
elements, X and Y, are shown below.
X
Y
Which of the following correctly describes the binary
compound that these two elements form?
3
A
99.2%
B
1 u = 1 atomic mass unit
A
a covalent compound with formula X2Y
94.1%
B
a covalent compound with formula XY2
C
70.0%
C
an ionic compound comprised of X+ and Y2- ions
D
48.6%
D
an ionic compound comprised of X- and Y2+ ions
E
9.41%
E
a covalent compound with formula X6Y7
Which one of the following elements exists as a liquid
at room temperature and normal atmospheric
pressure?
6
For elements in the same group, which one of the
following quantities decreases as the atomic number
increases?
A
chlorine
A
atomic mass
B
xenon
B
melting point
C
iodine
C
atomic radius
D
bromine
D
first ionization energy
E
silicon
E
density
 2002 UNIVERSITY OF WATERLOO AVOGADRO EXAM /2
7
Consider the unbalanced chemical equation
10 Zinc and sulfur react according to the chemical
equation
CH3CH2CHO(l) + O2(g) → CO2(g) + H2O(g).
Zn(s) + S(s) → ZnS(s).
Which set of coefficients balances the equation?
8
9
A
2, 8, 3, 6
B
3, 8, 6, 6
C
1, 4, 3, 2
D
1, 8, 3, 3
E
1, 4, 3, 3
In an experiment, 50 grams of zinc and 60 grams of
sulfur were heated in a reaction vessel. At the end of
the experiment, 70 grams of ZnS were obtained.
What was the percentage yield of ZnS for this
experiment?
Which of the following salts produces a gas when it is
treated with hydrochloric acid, HCl(aq)?
A
32%
B
44%
C
64%
D
75%
E
94%
Atomic masses:
S, 32.1
Zn, 65.4
A
CaS
B
Na2SO4
C
Mg(NO3)2
D
NaCl(aq)
is an example of
E
Zn(NO3)2
A
a neutralization reaction
B
a combustion reaction
C
a precipitation reaction
D
a displacement reaction
E
a decomposition reaction
11 The reaction
Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq)
What is percentage by mass of aluminum in Al2O3?
A
23%
B
53%
C
36%
D
64%
E
40%
Atomic masses:
Al, 27.0
O, 16.0
12 Hydroquinone is 65.4% carbon, 5.5% hydrogen and
29.1% oxygen by mass. What is the empirical formula
of this hydrocarbon?
A
CHO
B
C2H2O
C
C2H2O3
D
C3H3O2
E
C3H3O
Atomic masses:
H, 1.0
C, 12.0
O, 16.0
 2002 UNIVERSITY OF WATERLOO AVOGADRO EXAM /3
13 What is the mass of one molecule of acetylsalicylic
acid, C9H8O4?
A
180 g
B
3.31×1021 g
C
2.99×10-22 g
D
3.45×10-22 g
E
6.90×10-22 g
Atomic masses:
H, 1.01
C, 12.0
O, 16.0
Avogadro constant:
NA = 6.022×1023 mol-1
14 If a 50.0 mL sample of Ba(OH)2(aq) requires
44.23 mL of 0.2245 mol L-1 HCl(aq) to reach the
equivalence point in a titration, what is the
concentration of the Ba(OH)2 solution?
16 Which of the following aqueous solutions is the best
conductor of an electric current at room temperature?
A
0.10 mol L-1 CH3COOH(aq)
B
0.10 mol L-1 H2SO4(aq)
C
0.10 mol L-1 HCl(aq)
D
0.10 mol L-1 NaCl(aq)
E
0.10 mol L-1 H3PO4(aq)
17 A precipitate forms when an aqueous solution of
carbonic acid, H2CO3, is added to an aqueous
solution of
A
Ba(OH)2
A
0.09930 mol L-1
B
(NH4)2S
B
0.1986 mol L-1
C
Na2SO4
C
0.3972 mol L-1
D
KNO3
0.1269 mol L-1
E
D
H2SO3
E
0.2538 mol L-1
15 A concentrated sulfuric acid solution is 74.0% H2SO4
by mass and it has a density of 1.66 g mL-1 at 20oC.
What is the concentration of this H2SO4 solution?
A
18 What is the net ionic equation for the reaction that
occurs between nitrous acid, HNO2, and lithium
hydroxide, LiOH?
A
HNO2(aq) + LiOH(aq) → LiNO2(aq) + H2O(l)
B
H+(aq) + OH-(aq) → H2O(l)
C
HNO2(aq) + OH-(aq) → NO2 (aq) + H2O(l)
D
+
Li (aq) + NO2 (aq) → LiNO2(s)
E
H+(aq) + NO2 (aq) + Li+(aq) + OH-(aq)
2.3 mol L-1
B
6.7 mol L-1
C
7.6 mol L-1
D
12.5 mol L-1
E
16.9 mol L-1
Molar mass of H2SO4:
98.0 g mol-1
→ LiNO2(aq) + H2O(l)
 2002 UNIVERSITY OF WATERLOO AVOGADRO EXAM /4
19 Which bromine compound is the most soluble in the
solvent hexane, C6H14(l)?
A
LiBr
B
AgBr
C
NaBr
D
MgBr2
E
22 A sample of seawater has a pH of 8.10. What is [H+ ]
in the sample?
A
1.0×10-8 mol L-1
B
8.0×10-1 mol L-1
C
7.9×10-9 mol L-1
D
1.3×10-8 mol L-1
E
0.91 mol L-1
IBr
20 For which of the following does the solubility increase
if the solution is heated gently?
23 If 0.200 L of 0.15 mol L-1 HCl(aq) is mixed with
0.300 L of 0.090 mol L-1 NaOH(aq), what is the pH of
the solution that results?
A
a gaseous solute
B
a nonionic solute that dissolves without
appreciable solvation
A
1.22
C
a salt that dissolves endothermically
B
2.22
D
a salt that dissolves exothermically
C
2.52
E
a liquid that dissolves exothermically
D
0.52
E
7.00
21 In the reaction
- → NH + HS3
H2S + NH2
ammonia, NH3, is
-
A
the conjugate acid of NH2
B
the conjugate base of NH2
C
the conjugate acid of HS-
D
the conjugate base of HS-
E
the conjugate acid of H2S
-
24 Which one of the following is not consistent with the
postulates of the kinetic-molecular theory of gases?
A
collisions between molecules are elastic
B
gas molecules are in constant motion
C
a gas molecule moves along a straight line until it
collides with another molecule or a wall of the
container
D
the volume of any molecule is negligible
compared with the volume of the container
E
all the molecules move with the same speed
 2002 UNIVERSITY OF WATERLOO AVOGADRO EXAM /5
25 The behaviour of HCl(g) is most likely to approach
ideal behaviour at
28 The chemical equation for the combustion of glucose,
C6H12O6, is
C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(g).
A
10 atm and 100oC
B
1 atm and 0oC
C
0.10 atm and –100oC
What volume of O2, measured at standard
temperature and pressure, is required to oxidize
1.50 g of glucose?
D
1 atm and 100oC
A
E
0.10 atm and 100oC
B
0.37 L
C
1.1 L
D
11 L
E
134 L
0.19 L
R = 0.08206
26 How many molecules are there in a 1.0-mL sample of
gas if the temperature is 200 K and the pressure is
1.0×10-3 mm Hg?
A
4.8×1013 molecules
B
4.0×1012 molecules
1 atm = 760 mm Hg
C
1.6×1016 molecules
NA = 6.022×1023
D
7.9×1020 molecules
E
7.9×1017 molecules
R = 0.08206
one quarter of the helium
B
one third of the helium
C
one half of the helium
D
two thirds of the helium
E
three quarters of the helium
Molar mass of glucose,
180.2 g mol-1
atm L
mol K
29 At 0oC and 1 atm, a 3.56-L sample of a particular gas
weighs 11.3 g. What is the molar mass of the gas?
27 A 5.0-L container of He(g) at 1 atm is heated from
300 K to 450 K. The volume of the container does not
change. How much helium must be released from the
container to restore the pressure to 1 atm, assuming
that the temperature does not change as the gas is
released?
A
atm L
mol K
A
3.17 g mol-1
B
11.3 g mol-1
C
40.2 g mol-1
D
71.1 g mol-1
E
79.7 g mol-1
30 What is the partial pressure of helium gas in a mixture
that contains 48 grams of He(g) and 48 grams of
O2(g) if the total pressure is 675 mmHg?
A
135 mm Hg
B
295 mm Hg
C
338 mm Hg
D
540 mm Hg
E
600 mm Hg
1 atm = 760 mm Hg
Atomic masses:
He,
4.0
O,
16.0
 2002 UNIVERSITY OF WATERLOO AVOGADRO EXAM /6
31 What is the IUPAC name of the alkane shown below?
CH3
CH3 CH2 CH2 CH2 C
CH3
CH2 CH3
A
2-ethyl-2-methyl-hexane
B
1,1-dimethyl-1-ethylpentane
C
3,3-dimethylheptane
D
2-methyl-2-butylbutane
E
nonane
34 A 0.91-g sample of sucrose, C12H22O11, was burned
completely in excess oxygen in a constant volume
calorimeter. The temperature of the calorimeter rose
by 3.50oC. If the heat capacity of the calorimeter and
its contents was 4250 J (oC)-1, what is the constant
volume heat of combustion of sucrose?
A
14.9 kJ mol-1
B
14 900 kJ mol-1
C
184 kJ mol-1
D
5090 kJ mol-1
E
5590 kJ mol-1
Molar mass of C12H22O11:
342 g mol-1
32 How many structural isomers of C4H10 are there?
A
one
B
two
C
three
D
four
E
five
35 For which of the following compounds are cis-trans
isomers possible?
CH3CH=CH2
(i)
33 What are the ideal values for the H-C-H and H-C-C
bond angles in ethane, C2H6?
A
(i) and (ii)
B
(ii) and (iii)
C
(i) and (iii)
D
(ii) only
E
(i), (ii) and (iii)
CH3CH=CHCl
(ii)
CHCl=CHBr
(iii)
36 Which one of the following hydrocarbons has the
highest boiling temperature?
A
60o
B
72o
C
90o
D
109.5
E
120o
A
CH3CH2CH2CH3
B
H2C=CH2
C
HC≡CH
D
CH3CH3
E
CH4
o
 2002 UNIVERSITY OF WATERLOO AVOGADRO EXAM /7
37 The thermochemical equation for the combustion of
C3H6(g) is
C3H6(g) +
9
2
O2(g) → 3CO2(g) + 3H2O(l) + 2061 kJ.
What is the maximum quantity of heat that can be
obtained if a mixture containing 5 moles each of C3H6
and O2 is ignited?
A
40 When zinc metal is placed in contact with iron metal
in an aqueous environment, the iron does not rust.
Why does zinc metal prevent iron metal from rusting
in water?
A
Zinc loses electrons more readily than iron.
B
Zinc gains electrons more readily than iron.
C
Zn2+ ions gain electrons more readily than Fe2+
ions
10 320 kJ
B
2290 kJ
C
20 610 kJ
D
Zinc catalyzes the decomposition of rust.
D
9275 kJ
E
Zinc accepts protons from water molecules more
readily than iron.
E
46 370 kJ
38 Which of the following structures is the correct Lewis
(i.e. electron dot) structure for the HCN molecule?
A
H
C
N
B
H
C
N
C
H
C
N
D
H
C
N
E
H
C
N
39 Which set of coefficients balances the equation
x Cu (aq) + y Al(s) → n Cu(s) + m Al (aq)?
2+
3+
A
x
1
y
1
n
1
m
1
B
1
2
3
1
C
2
3
2
3
D
3
2
3
2
E
2
1
1
3
 2002 UNIVERSITY OF WATERLOO AVOGADRO EXAM /8
ANSWER GRIDS BY YEAR
1991
E
C
A
B
B
C
C
A
C
D
A
D
E
E
B
D
C
C
B
E
D
B
C
C
E
E
D
C
A
B
A
B
E
D
A
A
D
C
E
C
D
C
D
A
A
A
E
A
E
D
D
C
D
B
E
D
A
E
C
B
B
C
C
C
A
B
D
E
D
E
C
B
D
B
E
E
A
D
A
E
E
C
B
D
A
D
D
A
D
D
D
C
C
A
C
B
A
D
A
B
B
C
B
E
E
D
D
C
D
C
A
D
A
D
B
A
C
C
D
B
E
A
D
D
B
E
D
A
B
D
C
B
D
D
E
D
B
E
B
C
B
A
E
D
D
C
A
A
E
B
A
E
B
C
B
E
D
A
A
E
E
C
D
A
C
E
A
B
B
C
E
B
B
B
C
C
A
D
E
C
B
D
D
C
B
D
C
A
A
D
C
A
D
B
E
C
E
E
D
A
A
A
D
D
D
E
B
E
C
C
B
B
D
1992
D
E
C
B
1993
B
E
B
B
1994
B
B
C
C
1995
A
E
B
B
1996
E
A
E
B
Last Revised by D Lougheed 00/7/3
Page 49
1997
B
A
B
B
B
D
E
D
C
C
D
E
E
A
E
D
B
B
B
D
D
D
A
A
E
E
C
E
E
B
C
D
B
A
A
A
E
C
D
E
C
E
B
B
A
B
B
D
D
E
A
D
B
B
D
E
E
C
D
C
C
D
E
D
C
E
A
D
D
A
D
D
D
A
A
D
C
D
B
D
E
D
A
E
A
A
C
E
B
B
C
C
E
C
D
B
A
D
E
B
B
D
C
D
A
A
E
B
C
D
B
C
E
C
C
B
C
B
A
D
E
C
A
D
E
D
D
A
A
D
E
B
D
B
C
D
B
C
A
A
B
E
E
D
1998
B
A
E
E
1999
E
B
B
C
2000
B
D
A
B
Last Revised by D Lougheed 00/7/3
Page 50
2002 AVOGADRO EXAM ANSWERS
1. C
2. B
3. D
4. E
5. A
6. D
7. E
8. A
9. B
10. E
11. D
12. E
13. C
14. A
15. D
16. B
17. A
18. C
19. E
20. C
21. A
22. C
23. B
24. E
25. E
26. A
27. B
28. C
29. D
30. E
31. C
32. B
33. D
34. E
35. B
36. A
37. B
38. D
39. D
40. A
2001 AVOGADRO EXAM ANSWERS
1. B
2. A
3. E
4. A
5. D
6. C
7. A
8. E
9. B
10. E
11. D
12. E
13. A
14. D
15. C
16. D
17. E
18. A
19. C
20. B
21. A
22. C
23. B
24. B
25. A
26. E
27. B
28. C
29. E
30. A
31. B
32. D
33. A
34. C
35. C
36. B
37. C
38. E
39. D
40. D