Chemistry Human Activity, Chemical Reactivity (International Edition by Paul Treichel - Test Bank

Chemistry Human Activity, Chemical Reactivity (International Edition by Paul Treichel – Test Bank

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Sample Questions Are Posted Below

Chapter 2—Building Blocks of Materials
TRUE/FALSE
1. In a liquid, the particles are vibrating with sufficient energy that they do not have fixed positions, but
not enough energy that they can fill any container.
ANS: T PTS: 1 REF: p. 21 BLM: Remember
2. One mole of dinitrogen tetroxide molecules, N2O4, contains the same number of atoms as one mole of
phosphorus pentachloride, PCl5.
ANS: T PTS: 1 REF: p. 26 BLM: Higher Order
3. All atoms of oxygen have the same mass.
ANS: F PTS: 1 REF: p. 29 BLM: Higher Order
4. Atoms with the same number of neutrons but a different number of protons are called isotopes of the
same element.
ANS: F PTS: 1 REF: p. 29 BLM: Remember
5. In the mass spectrometer, the high-energy electron beam gives particles of the vaporized sample a
negative charge.
ANS: F PTS: 1 REF: p. 33–34 BLM: Remember
MULTIPLE CHOICE
1. According to the kinetic-molecular model of matter, how are the particles in a gas arranged?
a. They are far apart from each other but confined to specific positions.
b. They are packed closely together but not confined to specific positions.
c. They vibrate back and forth in relation to a fixed position.
d. They are far apart from each other and move about randomly.
ANS: D PTS: 1 REF: p. 21 BLM: Remember
2. Which of the following phenomena cannot be accounted for using the kinetic-molecular model of
matter?
a. An ice cube will melt when it is heated to room temperature.
b. Vinegar and olive oil separate into two layers in a bottle of salad dressing.
c. The scent from a bunch of flowers diffuses in a room with no air currents.
d. The colour from a drop of blue food dye spreads in a glass of water.
ANS: B PTS: 1 REF: p. 21 BLM: Higher Order
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3. Which of the following is a most likely to be a homogeneous mixture?
a. butter
b. ethanol
c. gasoline
d. tomato soup
ANS: C PTS: 1 REF: p. 22 BLM: Higher Order
4. Which of the following is most likely to be a heterogeneous mixture?
a. blood
b. windshield washer fluid
c. sodium chloride dissolved in water
d. air trapped inside an inflated balloon
ANS: A PTS: 1 REF: p. 22 BLM: Higher Order
5. Suppose a lighted splint is used to ignite a test tube of hydrogen gas. Which statement about this
situation would be at the molecular level of operation?
a. A loud popping sound is heard by an observer when ignition occurs.
b. After the reaction, condensation appears on the inside surface of the test tube.
c. The provided energy breaks some covalent bonds, initiating a series of chemical reactions.
d. A chemical reaction occurs that releases heat energy to the surroundings.
ANS: C PTS: 1 REF: p. 23 BLM: Higher Order
6. Suppose a lighted splint is used to ignite a test tube of hydrogen gas. Which statement about this
situation would be at the symbolic level of operation?
a. The chemical equation for the reaction is 2H2(g) + O2(g) 2H2O(l).
b. After the reaction, condensation appears on the inside surface of the test tube.
c. The reaction of hydrogen and oxygen releases heat to the surroundings.
d. In the reaction, 1.0 g of hydrogen combines with 8.0 g of oxygen.
ANS: A PTS: 1 REF: p. 23 BLM: Higher Order
7. Which of the following elements exists as separate, individual atoms?
a. bromine
b. neon
c. phosphorus
d. zinc
ANS: B PTS: 1 REF: p. 24 BLM: Remember
8. Which of the following formulas represents an elemental substance?
a. C60
b. NO
c. HI
d. CS2
ANS: A PTS: 1 REF: p. 24 BLM: Higher Order
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9. What is the symbol for chromium?
a. Ch
b. Co
c. Cr
d. Cu
ANS: C PTS: 1 REF: p. 24–25 BLM: Remember
10. What is the symbol for silver?
a. Ag
b. Au
c. Se
d. Sr
ANS: A PTS: 1 REF: p. 24–25 BLM: Remember
11. What is the name of the element with the symbol Ar?
a. americium
b. argentum
c. argon
d. arsenic
ANS: C PTS: 1 REF: p. 24–25 BLM: Remember
12. What is the name of the element with the symbol W?
a. darmstadtium
b. hafnium
c. tungsten
d. wolfium
ANS: C PTS: 1 REF: p. 24–25 BLM: Remember
13. How is a mixture of iron and sulfur different from a compound of these elements?
a. A mixture has a fixed composition of iron and sulfur, but a compound does not.
b. A mixture is more difficult to separate into iron and sulfur than a compound.
c. A mixture is a homogeneous substance, but a compound is heterogeneous.
d. A mixture shows the properties of iron and sulfur, but a compound does not.
ANS: D PTS: 1 REF: p. 25 BLM: Remember
14. Which of the following formulas represents a chemical compound?
a. Cl2
b. CO
c. Co
d. O3
ANS: B PTS: 1 REF: p. 26 BLM: Higher Order
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15. Which of the following is a chemical property?
a. the flammability of phosphorus
b. the electrical conductivity of aluminum
c. the malleability of gold
d. the viscosity of antifreeze
ANS: A PTS: 1 REF: p. 27 BLM: Higher Order
16. Which of the following is an example of a chemical change?
a. Sodium chloride melts at 801 ºC.
b. The density of water decreases when it changes from a liquid to a solid.
c. Silver cutlery tarnishes after a few weeks.
d. Steam condenses on a cold surface.
ANS: C PTS: 1 REF: p. 27 BLM: Higher Order
17. When ethanol undergoes complete combustion, the reaction equation is
C2H5OH(l) + 3 O2(g) 2 CO2(g) + 3 H2O(g).
What information does this equation provide?
a. The chemical reaction releases heat energy.
b. This reaction takes place in the gas phase.
c. The number of molecules in the reaction vessel changes.
d. The redistribution of atoms represents a spontaneous reaction.
ANS: C PTS: 1 REF: p. 27 BLM: Higher Order
18. Iron metal is produced from iron oxide by reacting iron oxide with carbon monoxide. Which of the
following equations represents this reaction?
a. Fe2O3(s) + 3 CO(g) 2 Fe(s) + 3 CO2(g)
b. Fe2O3(s) + 3 C(s) 2 Fe(s) + 3 CO(g)
c. 3 Fe2O3(s) + CO(g) 2 Fe3O4(s) + CO2(g)
d. 2 Fe2O3(s) 4 Fe(s) + 3 O2(g)
ANS: A PTS: 1 REF: p. 27 BLM: Higher Order
19. Which of the following is NOT a physical property?
a. the viscosity of motor oil at minus 20 ºC
b. the flash point of alcohol
c. the melting point of gold
d. the electrical conductivity of copper wire
ANS: B PTS: 1 REF: p. 28 BLM: Higher Order
20. How many protons, neutrons, and electrons are in an yttrium-89 atom?
a. 39 protons, 50 neutrons, 39 electrons
b. 39 protons, 89 neutrons, 39 electrons
c. 50 protons, 39 neutrons, 50 electrons
d. 39 protons, 11 neutrons, 39 electrons
ANS: A PTS: 1 REF: p. 29 BLM: Higher Order
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21. Which two of the following atoms are isotopes?
, , ,
a. and
b. and
c. and
d. and
ANS: D PTS: 1 REF: p. 29 BLM: Higher Order
22. What is the atomic symbol for an element with 38 protons and 50 neutrons?
a.
b.
c.
d.
ANS: B PTS: 1 REF: p. 29–30 BLM: Higher Order
23. Which two of the atoms below have the same number of neutrons?
, , ,
a. and
b. and
c. and
d. and
ANS: A PTS: 1 REF: p. 29–30 BLM: Higher Order
24. How is an atomic mass unit (u) defined?
a. the mass of one hydrogen-1 atom
b. 1/12 the mass of one carbon-12 atom
c. 1/16 the mass of one oxygen-16 atom
d. the mass of one proton
ANS: B PTS: 1 REF: p. 32 BLM: Remember
25. What is the role of the magnets in a mass spectrometer?
a. to ionize the vaporized sample
b. to accelerate the ionized particles of the sample
c. to deflect the ionized particles of the sample
d. to focus the ionized particles into a narrow beam
ANS: C PTS: 1 REF: p. 33 BLM: Remember
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26. What properties are used to separate particles in a mass spectrometer?
a. mass and size
b. mass and charge
c. mass and reactivity
d. mass and density
ANS: B PTS: 1 REF: p. 33 BLM: Remember
27. Suppose an element consists of two isotopes. The abundance of one isotope is 60.1%, and its atomic
mass is 68.9 u. The atomic mass of the second isotope is 70.9 u. What is the average atomic mass of
the element?
a. 69.5 u
b. 69.7 u
c. 69.9 u
d. 70.1 u
ANS: B PTS: 1 REF: p. 33–34 BLM: Higher Order
28. Cesium has only one stable isotope. What is the atomic mass of this isotope?
a. 131.90643431
b. 132.90545196
c. 133.90671857
d. 134.90597703
ANS: B PTS: 1 REF: p. 33–34 BLM: Higher Order
29. Antimony consists of two stable isotopes. The lighter isotope, Sb-121, has atomic mass 120.904 u. The
heavier isotope, Sb-123 has atomic mass 122.904 u. What is the percent natural abundance of the
lighter stable isotope of antimony?
a. 39.0%
b. 42.8%
c. 57.2%
d. 61.0%
ANS: C PTS: 1 REF: p. 34 BLM: Higher Order
30. Consider the following data.
1 mol Al
2 mol O2
3 mol C
4 mol H2
Which sample has the greatest number of atoms?
a. Al
b. O2
c. C
d. H2
ANS: D PTS: 1 REF: p. 35 BLM: Higher Order
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31. Consider the following data.
1 mol Al
2 mol O2
3 mol C
4 mol H2
Which sample has the greatest mass?
a. Al
b. O2
c. C
d. H2
ANS: B PTS: 1 REF: p. 35 BLM: Higher Order
32. Lithium metal has a density of 0.535 g/mL. How many moles of lithium atoms are present in a cube of
the metal with sides of 2.00 cm?
a. 0.154 mol
b. 0.539 mol
c. 0.617 mol
d. 2.15 mol
ANS: C PTS: 1 REF: p. 36–37 BLM: Higher Order
33. What is the mass of tin that contains the same number of atoms as there are in 100.0 g of lead?
a. 57.29 g
b. 60.97 g
c. 164.0 g
d. 174.6 g
ANS: A PTS: 1 REF: p. 36–37 BLM: Higher Order
34. What is the mass of 2.41×1022 atoms of the element boron?
a. 0.432 g
b. 4.32 g
c. 27.0 g
d. 270 g
ANS: A PTS: 1 REF: p. 36–37 BLM: Higher Order
35. What type of elements are found in the upper-right corner of the periodic table?
a. main group metals
b. transition metals
c. metalloids
d. non-metals
ANS: D PTS: 1 REF: p. 38 BLM: Remember
36. Which group in the periodic table contains metallic, non-metallic, and metalloid elements?
a. 11
b. 13
c. 15
d. 17
ANS: C PTS: 1 REF: p. 38 BLM: Remember
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37. Which of the following did Mendeleev NOT do when he constructed his version of the periodic table?
a. leave gaps for undiscovered elements
b. place elements with similar properties in the same horizontal row
c. order the elements on the basis of increasing atomic mass
d. correctly predict the properties of some undiscovered elements
ANS: B PTS: 1 REF: p. 39 BLM: Remember
38. In which of the following groups are the three elements likely to have similar chemical and physical
properties?
a. boron, silicon, and germanium
b. sodium, magnesium, and aluminum
c. magnesium, calcium, and strontium
d. carbon, nitrogen, and oxygen
ANS: C PTS: 1 REF: p. 39 BLM: Higher Order
COMPLETION
1. Homogeneous mixtures can also be referred to as ____________________.
ANS: solutions
PTS: 1 REF: p. 22 BLM: Remember
2. Since the composition of a mixture can vary, it is impossible to assign a mixture a chemical
____________________.
ANS: formula
PTS: 1 REF: p. 26 BLM: Remember
3. For an atom of an element, the symbol Z represents the number of ____________________.
ANS: protons
PTS: 1 REF: p. 29 BLM: Remember
4. The atomic weight of an element is the average relative atomic mass of a representative sample of its
atoms, taking into account the ____________________.
ANS: relative abundances of its isotopes
PTS: 1 REF: p. 29 BLM: Remember