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An atom with three electrons has:
A) one occupied orbital with three electrons.
B) two occupied orbitals, one of which has two electrons and the other has one.
C) three occupied orbitals, each of which contains one electron.
D) three energy shells, each of which contains one electron.
2. If an atom has three electrons, how many occupied orbitals will the atom have, and how
many electrons will be in each?
3. For an atom that is NOT an ion, which of the following must be TRUE?
A) The number of electrons equals the number of protons.
B) The number of electrons equals the number of neutrons.
C) The number of protons equals the number of neutrons.
4. Explain why an atom that is NOT an ion is electrically neutral.
5. Which of the following CORRECTLY pairs the particles of an atom with their physical
properties?
A) proton–positively charged; neutron–uncharged; electron–negatively charged
B) proton–negatively charged; neutron–uncharged; electron–positively charged
C) proton–positively charged; neutron–negatively charged; electron–uncharged
D) proton–uncharged; neutron–negatively charged; electron–positively charged
6. List the particles in an atom, and indicate whether each is positively charged, negatively
charged, or uncharged.
7. Sometimes, atoms gain or lose particles. The loss of which of the following results in a
change of atomic mass?
A) a neutron
B) a proton
C) an electron
D) a neutron and a proton
E) a proton and an electron
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8. Sometimes, atoms gain or lose particles. The loss of which of the following would result
in a change of overall electrical charge?
A) protons only
B) electrons only
C) neutrons only
D) protons or neutrons
E) protons or electrons
F) neutrons or electrons
9. The most common isotope of oxygen has 8 protons and an atomic mass of 16. How
many neutrons are present in the oxygen nucleus?
A) 2
B) 4
C) 6
D) 8
E) 10
10. The most common isotope of oxygen has 8 protons and an atomic mass of 16. How
many electrons are present in the orbitals around an atom of oxygen?
A) 2
B) 4
C) 6
D) 8
E) 10
11. The most common isotope of oxygen has an atomic mass of 16 (16O). An isotope with
an atomic mass of 18 (18O) is also stable. How many valence electrons are present in
18O?
A) fewer than in 16O
B) more than in 16O
C) the same as in 16O
D) None of the other answer options is correct.
12. 14C is an isotope of carbon that possesses:
A) 6 protons, 6 neutrons, and 2 electrons.
B) 6 protons, 8 neutrons, and 6 electrons.
C) 8 protons, 6 neutrons, and 2 electrons.
D) 6 protons, 2 neutrons, and 6 electrons.
E) 6 protons, 8 neutrons, and 2 electrons.
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13. Using the periodic table in Fig. 2.3, select the element that would be found in LEAST
abundance in a living cell.
A) hydrogen (H)
B) sodium (Na)
C) phosphorous (P)
D) zinc (Zn)
E) silicon (Si)
14. How many electron orbitals does a carbon atom possess?
A) 2
B) 4
C) 5
D) 6
E) 12
15. What differentiates isotopes of the same element?
A) protons
B) neutrons
C) electrons
D) charge
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16. You discover an isotope of an element that has 6 electrons in its second and outermost
shell, 8 protons, and 6 neutrons. What element is it?
A) fluorine (F)
B) carbon (C)
C) nitrogen (N)
D) oxygen (O)
17. What would happen to an atom’s atomic mass and electric charge if it gained or lost a
proton, a neutron, or an electron?
18. The atom:
A) is the basic unit of matter.
B) is the unit of composition for elements.
C) contains protons, neutrons, and electrons.
D) has negatively charged particles circling around a positively charged nucleus.
E) All of these choices are correct.
19. The designation of a magnesium ion as Mg2+ indicates an atom that has:
A) two more protons than neutrons.
B) lost two electrons and is negatively charged.
C) lost two electrons and is positively charged.
D) gained two protons and is positively charged.
E) gained two protons and is negatively charged.
20. The basic unit of matter is referred to as a(n) _____.
21. The negatively charged components of atoms are referred to as:
A) protons.
B) electrons.
C) anions.
D) neutrons.
E) cations.
22. For the first three rows of the periodic table, elements in the same row have the same
number and type of electron orbitals.
A) True
B) False
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23. Which one of the following pairs would be classified as isotopes of each other?
A) H and H+
B) Na +
and Cl–
C) C and Si
D) 12C and 13C
E) H and H+
, Na+
and Cl–
, C and Si, 12C and 13C
24. Nitrogen and phosphorus are in the same column of the periodic table. They have
similar properties in bonding with other molecules because they have the same number
of:
A) electrons.
B) paired electrons.
C) valence electrons.
D) electron shells.
25. What percentage of carbon’s orbitals is spherical in conformation?
A) 0%
B) 20%
C) 40%
D) 80%
E) 100%
26. Which one of the following contributes to the measurement referred to as atomic mass?
A) protons and electrons
B) electrons and neutrons
C) protons, electrons, and neutrons
D) protons and neutrons
E) neutrons only
27. Which component of an atom has the SMALLEST mass?
A) proton
B) neutron
C) electron
D) isotope
E) isomer
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28. Two elements within the same group:
A) occupy the same row on the periodic table of elements.
B) occupy the same column on the periodic table of elements.
C) have the same number of electrons in their outermost shell.
D) have different numbers of electrons in their outermost shell.
E) occupy the same column on the periodic table and have the same number of
electrons in their outermost shell.
29. Consider two carbon atoms, one represented as 14C and the other as 12C. Which of the
following statements is TRUE regarding these two atoms?
A) These carbon atoms have the same number of protons.
B) These carbon atoms have the same number of neutrons.
C) These carbon atoms have different numbers of electrons.
D) These carbon atoms have different numbers of protons.
30. Which of the following statements is TRUE regarding elements?
A) Elements are composed of several different types of atoms.
B) Elements are only found in nature and cannot be created by humans.
C) Elements are still categorized according to Aristotle’s early classifications.
D) Elements are composed of only one type of atom.
E) Elements are only found in inorganic substances and not in living organisms.
31. Which of the following statements is TRUE regarding atomic mass?
A) The atomic mass is defined as the sum of electrons and neutrons in an atom.
B) The atomic mass can be used to differentiate between different isotopes of the
same element.
C) The atomic mass is synonymous with the atomic number.
D) The atomic mass is calculated by adding the total number of electrons, protons, and
neutrons in an atom.
32. Imagine that you have two different carbon atoms, one identified as 14C and the other as
13C. These two carbon atoms:
A) are two different carbon isotopes.
B) have a different number of neutrons.
C) have a different number of protons.
D) are two different carbon isotopes and have a different number of protons.
E) are two different carbon isotopes and have a different number of neutrons.
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33. Where is the highest-energy electron found in an atom of hydrogen?
A) in the spherical orbital closest to the nucleus
B) in the second spherical orbital, a little farther from the nucleus
C) in the dumbbell-shaped orbital of the y-axis
D) in the dumbbell-shaped orbital of the x-axis
E) in the dumbbell-shaped orbital of the z-axis
34. Consider the two elements, sodium (Na) and magnesium (Mg), which occupy the same
row in the periodic table of elements. Sodium and magnesium atoms have:
A) a different number of orbitals.
B) the same atomic number.
C) different atomic masses.
D) the same number of electrons in their outermost orbitals.
E) different atomic masses and the same number of electrons in their outermost
orbitals.
35. Which of the following bonds rely on the attraction of positive and negative charges?
A) ionic bonds
B) covalent bonds
C) hydrogen bonds
D) ionic bonds and hydrogen bonds
E) ionic bonds and covalent bonds
Page 8
36. Refer to the periodic table, and decide which of the following molecules is held together
by ionic bonds.
A) NH3
B) CO2
C) KCl
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37. Refer to the periodic table, and decide which of the following molecules is held together
by polar covalent bonds.
A) NH3
B) CO2
C) KCl
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38. Refer to the periodic table, and decide which of the following molecules is held together
by nonpolar covalent bonds.
A) NH3
B) CO2
C) KCl
39. Of the following types of bonds between atoms, which is the STRONGEST?
A) ionic bond
B) hydrogen bond
C) covalent bond
D) van der Waals forces
40. A pair of atoms joined by a polar covalent bond:
A) has the charge spread evenly across both atoms.
B) has a slight positive charge on one atom and a slight negative charge on the other.
C) is unlikely to form hydrogen bonds with water.
D) mixes well with nonpolar solvents.
41. The ability of atoms to form bonds is due largely to electrons farthest from the nucleus.
These electrons are called _____ electrons.
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42. Which one of the following elements would MOST likely have bonding properties
similar to nitrogen (N)? Consult the periodic table in Fig. 2.3 if necessary.
A) carbon (C)
B) silicon (Si)
C) phosphorus (P)
D) sulfur (S)
E) oxygen (O)
43. Which of the following accurately describes a polar covalent bond?
A) the interaction of a hydrogen atom connected to an atom with a high
electronegativity, and an electronegative atom of another molecule
B) the interaction of an atom with very high electronegativity, and an atom with very
low electronegativity
C) the unequal sharing of electrons between an atom with a partial positive charge,
and an atom with a partial negative charge
D) the equal sharing of electrons between atoms of identical or similar
electronegativities
E) None of the other answer options is correct.
44. Which one of the following is maintained during a chemical reaction?
A) the number of atoms present in the reactants
B) the identity of the atoms present in the reactants
C) the arrangement of chemical bonds present in the reactants
D) the number and identity of the atoms present in the reactants
E) the number and identity of the atoms, and the arrangement of chemical bonds
present in the reactants.
45. A pair of shared valence electrons is referred to as a(n):
A) ionic bond.
B) hydrogen bond.
C) van der Waals interaction.
D) covalent bond.
E) hydrophobic effect.
46. The ability of atoms to attract electrons is referred to as:
A) van der Waals attraction.
B) potential energy.
C) hydrophobicity.
D) cohesion.
E) electronegativity.
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47. An ionic interaction, such as the interaction between Na+
and Cl–
, is considered a
covalent bond.
A) True
B) False
48. A(n) _____ is a substance composed of two or more atoms.
49. The valence electrons of an atom are at the lowest energy level because their increased
distance from the nucleus reduces their attraction to the atom’s protons.
A) True
B) False
50. The _____ of a chemical reaction are transformed into different molecules called _____.
A) reactants; products
B) reactants; isomers
C) products; compounds
D) products; reactants
E) compounds; products
51. A polar bond is due to:
A) equal sharing of valence electrons.
B) an attraction of opposite charges.
C) uneven sharing of electrons in a covalent bond.
D) the interaction between an ion and a non-ionic atom.
E) None of the other answer options is correct
52. Hydrogen bonding is ultimately due to differences in _____ between two atoms.
53. Which one of the following elements is likely to form exactly three non-ionic
interactions with hydrogen?
A) phosphorus
B) oxygen
C) carbon
D) sulfur
E) chlorine
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54. The structural formula for hydrogen gas (H2) is represented as HH. Here, the dash
() represents a(n):
A) product.
B) reactant.
C) chemical reaction.
D) chemical bond.
E) electronegative bond.
55. Which of the following statements regarding an atom with high electronegativity is
TRUE?
A) It will have fewer protons than an atom with low electronegativity.
B) It will have a tendency not to attract electrons.
C) It will most likely be located on the left-most side of the periodic table of elements.
D) None of the other answer options is correct.
56. When two atoms form a covalent bond, they share electrons from all of their orbitals.
All of their orbitals, in turn, combine to form a single molecular orbital.
A) True
B) False
57. A young girl is staring at the raindrops running down her window. She notices that the
raindrops remain more or less intact, even as they cascade down the windowpane. This
is a result of:
A) covalent bonds between water molecules.
B) oxygen bonds between water molecules.
C) polar covalent bonds between water molecules.
D) hydrogen bonds between water molecules.
E) ionic bonds between water molecules.
58. Which of the following is an example of a hydrogen bond?
A) the bond that forms between a hydrogen and oxygen atom within the same water
molecule
B) the bond that forms between two hydrogen atoms within the same water molecule
C) the bond that forms between hydrogen and oxygen atoms within different water
molecules
D) the bond that forms between two hydrogen atoms within different water molecules
E) the bond that forms between two oxygen atoms within different water molecules
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59. A molecule of common table salt, or NaCl, is the result of _____ bond forming between
a sodium (Na) atom and a chlorine (Cl) atom.
A) an ionic
B) a covalent
C) a polar covalent
D) a hydrogen
E) either an ionic or a polar covalent
60. An ionic bond is really a modified polar covalent bond, because two atoms ―share‖
electrons when one atom steals a valence electron from the other.
A) True
B) False
61. A woman’s doctor tells her to gargle with salt water. She stirs a tablespoon of salt into a
cup of warm water and watches it dissolve. Why does the salt dissolve in water?
A) The positive hydrogen atoms in water molecules are attracted to chlorine ions.
B) The positive hydrogen atoms in water molecules are attracted to sodium ions.
C) The negative oxygen atoms in water molecules are attracted to chlorine ions.
D) The negative oxygen atoms in water molecules are attracted to sodium ions.
E) The positive hydrogen atoms in water molecules are attracted to chlorine ions, and
the negative oxygen atoms in water molecules are attracted to sodium ions.
62. Part of the reason why salt dissolves in water is that hydrogen bonds form between
water molecules and chlorine ions.
A) True
B) False
63. What is the chemical basis for water’s role as the universal solvent?
A) Because water is polar, it disrupts most covalent bonds.
B) Because water is polar, it disrupts hydrogen bonds.
C) Because water is polar, it disrupts ionic bonds.
D) Because water is polar, it disrupts both covalent and hydrogen bonds.
E) Because water is polar, it disrupts both hydrogen and ionic bonds.
64. What is the chemical basis for water’s role as the universal solvent?
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65. Several chemical properties make water uniquely suited for its role as a central
―molecule of life.‖ Which of the following is FALSE?
A) Hydrogen bonding leads to high cohesiveness between water molecules.
B) Water resists temperature changes.
C) Water molecules are always polar.
D) The structure of a water molecule is stabilized by hydrogen bonds.
E) Water is a good solvent of polar molecules and ions.
66. Describe three chemical properties of water that make it uniquely suited for its role as a
central ―molecule of life.‖
67. The association of individual water molecules with other water molecules is called
_____ and occurs through _____ bonds between water molecules.
A) adhesion; polar covalent
B) cohesion; polar covalent
C) cohesion; hydrogen bonds
D) adhesion; hydrogen bonds
68. The unique properties of water are due to the _____ of water molecules and the ability
of water to form _____ with other water molecules and with other polar molecules.
A) electronegativity; polar covalent bonds
B) polarity; polar covalent bonds
C) polarity; hydrogen bonds
D) hydrophobicity; hydrogen bonds
69. You have an aqueous solution with a pH of exactly 7.0. What would you add to make
the solution more acidic?
A) hydrogen chloride (HCl)
B) sodium hydroxide (NaOH)
C) sodium chloride (NaCl)
D) deionized water (dH2O)
70. You have an aqueous solution with a pH of 6.0. What would you add to make the
solution more basic?
A) Hydrogen chloride (HCl)
B) Sodium hydroxide (NaOH)
C) Sodium chloride (NaCl)
D) Deionized water (dH2O)
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71. You have an aqueous solution with a pH of 8.0. You add sodium chloride to a
concentration of 1 gram per 100 milliliters. What happens to the pH?
A) It goes up.
B) It goes down.
C) It stays the same.
D) It depends on the temperature.
72. Complete the matching exercise below by choosing the CORRECT description of each
bond type in aqueous solution.
1. covalent bond
2. hydrogen bond
3. ionic bond
A. an interaction of a hydrogen atom and an electronegative atom
B. an interaction between oppositely charged ions
C. electrons shared by atoms
73. Complete the matching exercise below by choosing the CORRECT strength of each
bond type in aqueous solution. Responses may be used once, more than once, or not at
all.
1. covalent bond in aqueous solution
2. hydrogen bond in aqueous solution
3. ionic bond in aqueous solution
A. weak
B. strong
74. Which of the following is NOT a property of water?
A) contracts during freezing
B) floats when solid
C) is a good solvent
D) adheres to polar compounds
E) is a polar molecule
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75. Which statement BEST describes an effect of the low density of frozen water in a lake?
A) When water freezes, it contracts, decreasing the water level in the lake.
B) Water in a lake freezes from the bottom up, killing most aquatic organisms.
C) When water in a lake freezes, it floats, providing insulation for organisms below
the ice.
D) Water removes thermal energy from the land around a lake, causing the lake to
freeze.
76. Which one of the following represents the pH of a solution with the HIGHEST
concentration of hydrogen ions?
A) 1.0
B) 4.5
C) 7.0
D) 9.1
E) 11.5
77. In a solution that has pH = 7.0, the ratio of protons (H+
) to hydroxide ions (OH–
) equals
A) 70
B) 7
C) 1
D) 1/7
E) 1/70
78. A water molecule contains what type of bond?
A) hydrogen
B) ionic
C) polar covalent
D) van der Waals interactions
79. Which of the following statements about water is CORRECT?
A) Water is the most abundant molecule in living cells.
B) Water is a polar molecule.
C) Water has good solvent properties.
D) Water molecules form hydrogen bonds with other polar molecules.
E) All of these choices are correct.
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80. Which one of the following properties of water is primarily responsible for the ability of
trees to draw water up from the roots to the leaves?
A) polarity
B) density
C) solvent capability
D) cohesion
E) pH neutrality
81. Water is able to dissolve many compounds as a result of which of the following?
A) the fact that water molecules are polar
B) the fact that water molecules are nonpolar
C) the fact that the hydrogen atoms in water molecules have a slight negative charge
D) the fact that most nonwater molecules are hydrophobic
E) the fact that water molecules are polar, and that the hydrogen atoms in water
molecules have a slight negative charge
82. Which of the following statements about water is CORRECT?
A) Ice is less dense than liquid water.
B) Ice forms on top and sinks to the bottom of lakes and rivers.
C) Ice is more dense than liquid water.
D) Bodies of water freeze from the bottom up.
E) Water molecules in ice demonstrate a disorganized, non-lattice arrangement.
83. Water is neither hydrophilic nor hydrophobic, because these terms only define the
interaction of other molecules with water molecules.
A) True
B) False
84. Which of the following statements is TRUE regarding a polar molecule?
A) A polar molecule is hydrophobic.
B) A polar molecule is hydrophilic.
C) A polar molecule will dissolve in water.
D) A polar molecule will not dissolve in water.
E) A polar molecule is hydrophilic and it will dissolve in water.
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85. Imagine you are looking at a bottle of salad dressing containing oil, vinegar, and water.
You notice that the oil sits on ―top‖ of the other liquids. This is due, in part, to the fact
that:
A) water is hydrophobic.
B) oil is hydrophilic.
C) vinegar is hydrophobic.
D) oil is hydrophobic.
E) water is hydrophobic and oil is hydrophilic.
86. A researcher has measured the pH of a solution, and found that the pH is 10. This
solution is _____, and has more _____ compared with _____.
A) basic; protons; hydroxide ions
B) basic; hydroxide ions; protons
C) acidic; protons; hydroxide ions
D) acidic; hydroxide ions; protons
E) neutral; hydroxide ions; protons
87. Evidence exists that atmospheric CO2 has increased over the last several decades due to
human activities. How do increased CO2 levels affect the pH of Earth’s waters?
A) It does not affect the pH of Earth’s waters, because atmospheric CO2 is not located
in oceans.
B) Due to the formation of carbonic acid, increased CO2 levels decrease the pH of
Earth’s waters.
C) Due to the formation of carbonic acid, increased CO2 levels increase the pH of
Earth’s waters.
D) Due to the formation of carbonic acid, increased CO2 levels cause Earth’s waters to
become neutral.
88. A man heats water in a teakettle while drinking a glass of water at room temperature.
The water molecules in the teakettle are moving _____ the water molecules in the glass.
A) faster than
B) slower than
C) at the same speed as
89. As water is heated, the temperature rises before any hydrogen bonds between water
molecules are broken.
A) True
B) False
Page 20
90. A man has ordered a glass of soda in a restaurant. When his drink arrives, he notices
that quite a bit of ice is floating at the top of the glass. Why does the ice float?
A) The water molecules in ice are arranged in a lattice pattern, causing ice to float.
B) The water molecules in the soda are arranged in a lattice pattern, providing a ―net‖
on which ice can sit.
C) The water molecules in the soda are more densely packed compared to the water
molecules in the ice.
D) The water molecules in the ice are more densely packed compared to the water
molecules in the soda.
E) The water molecules in ice are arranged in a lattice pattern, and the water
molecules in the soda are more densely packed compared to the water molecules in
the ice, causing ice to float.
91. If hydrogen bonds between water molecules were, collectively, not as strong as they are,
how would this affect plant height?
A) As hydrogen bonds impede the movement of water through plant vasculature,
plants would be able to grow taller.
B) As hydrogen bonds are responsible for the movement of water through plant
vasculature, plants would be shorter.
C) As plants actively transport water through their vasculature, weaker hydrogen
bonds would have no effect on plant height.
D) As hydrogen bonds cause water to stick to the sides of plant vasculature, plants
would be able to grow taller.
E) As hydrogen bonds increase the amount of sugar that plants can transport through
their vasculature, plants would be able to grow taller.
92. Water readily dissolves compounds that are referred to as:
A) hydrophobic.
B) solvent.
C) nonpolar.
D) hydrophilic.
E) aqueous.
93. The tendency of nonpolar molecules to self-associate in water instead of dissolve
individually is called the hydrophobic effect.
A) True
B) False