Chapter 2 Flashcards
1
Q
Proton
A
positively-charged subatomic particle
2
Q
center of an atom that contains protons and neutrons
A
nucleus
(chemistry)
3
Q
substance made up of atoms of more than one element
A
compound
4
Q
bond between charged ions
A
Ionic Bond
5
Q
positively-charged subatomic particle
A
Proton
6
Q
Base
A
substance that can accept hydrogen ion in solution
7
Q
heat of vaporization
A
energy required to convert liquid to a gas
8
Q
solution
A
solvent and dissolved solute mixture
9
Q
hydrophobic
A
uncharged, nonpolar groups of atoms/molecules that have no affinity for water
10
Q
- measure of a solution’s acidity/hydrogen ion concentration
- -log( [H+] )
A
pH
11
Q
hydrophillic
A
having an affinity for water; polar
12
Q
anion
A
negatively charged ion
13
Q
energy
A
capacity to do work or to accomplish change in physical or chemical systems
14
Q
orbital
A
region in space surrounding nucleus in which an electron is most likely to be found
15
Q
acid
A
substance that can release a proton in solution
16
Q
polar
A
having opposite electric charges at two ends
17
Q
molecule
A
chemical substance consisting of two or more atoms joined by bonds or attractions
18
Q
reactant
A
substance that enters into a chemical reaction
19
Q
solvent
A
liquid in which solutes are dissolved to form a solution
20
Q
Molecular Weight
A
sum of atomic weights in a molecule
21
Q
electron
(def)
A
negatively charged subatomic particle
22
Q
hydrogen bond
A
weak electrostatic bond between slightly-positive hydrogen atom and slightly-negative charge on a nearby atom
23
Q
ion
A
electrically charged particle that forms when atom gains or loses electron(s)
24
Q
van der Waals forces
A
weak attractions between atoms resulting from interactions between electons of one atom and the nucleus of another
25
van der Waals forces
| (strength)
bonds that are about 1/4 as strong as hydrogen bonds
26
neuton
* neutrally-charged subatomic particle located in the nuclei of atoms
* molecular weight of approx. 1 amu
27
reversible reaction
chemical change that can occur in both forward and reverse direction
28
electron shell
region in which electrons orbit; surrounding atomic nucleus at fixed energy level
29
sum of an atom's protons and neutrons
mass number
30
radioisotope
radioactive isotope
(e.g. carbon-14, hydrogen-3, tritium)
31
substance that can accept or release hydrogen ions to resist changes in pH
buffer
32
amount of energy required to raise 1 gram of a substance by 1 deg C
specific heat
33
isotope
atom containing same number of protons as shown in the periodic table, but differing in the number of neutrons within the nucleus
34
specific heat
amount of energy required to raise 1 gram of a substance by 1 deg C
35
compound
substance made up of atoms of more than one element
36
cohesion
tendency of molecules to stick together
37
element
substance that cannot be converted to a simpler substance
38
atomic number
* equivalent to the number of protons in an atom's nucleus (equal to electrons around atom)
* determines chemical properties of atom
39
electronegativity
affinity of an atom to attract electrons when it occurs as part of a compound
40
mole
avogadro's number of something
41
covalent bond
bond based on the (equal or unequal) sharing of electrons between two atoms
42
avogadro's number
6.022 x 10^23
43
chemical bond
attractive force linking two atoms
44
pH
* measure of a solution's acidity/hydrogen ion concentration
* -log( [H+] )
45
buffer
substance that can accept or release hydrogen ions to resist changes in pH
46
nucleus
| (chemistry)
center of an atom that contains protons and neutrons
47
substance that can accept hydrogen ion in solution
Base
48
energy required to convert liquid to a gas
heat of vaporization
49
solvent and dissolved solute mixture
solution
50
uncharged, nonpolar groups of atoms/molecules that have no affinity for water
hydrophobic
51
radioactive isotope
(e.g. carbon-14, hydrogen-3, tritium)
radioisotope
52
solute
substance dissolved in a liquid to form a solution
53
mass number
sum of an atom's protons and neutrons
54
having an affinity for water; polar
hydrophillic
55
negatively charged ion
anion
56
Ionic Bond
bond between charged ions
57
capacity to do work or to accomplish change in physical or chemical systems
energy
58
region in space surrounding nucleus in which an electron is most likely to be found
orbital
59
tendency of molecules to stick together
cohesion
60
substance that can release a proton in solution
acid
61
having opposite electric charges at two ends
polar
62
substance that cannot be converted to a simpler substance
element
63
chemical substance consisting of two or more atoms joined by bonds or attractions
molecule
64
substance that enters into a chemical reaction
reactant
65
* equivalent to the number of protons in an atom's nucleus (equal to electrons around atom)
* determines chemical properties of atom
atomic number
66
liquid in which solutes are dissolved to form a solution
solvent
67
substance dissolved in a liquid to form a solution
solute
68
affinity of an atom to attract electrons when it occurs as part of a compound
electronegativity
69
sum of atomic weights in a molecule
Molecular Weight
70
avogadro's number of something
mole
71
negatively charged subatomic particle
electron
| (def)
72
bond based on the (equal or unequal) sharing of electrons between two atoms
covalent bond
73
weak electrostatic bond between slightly-positive hydrogen atom and slightly-negative charge on a nearby atom
hydrogen bond
74
positively charged ion
cation
75
electrically charged particle that forms when atom gains or loses electron(s)
ion
76
6.022 x 10^23
avogadro's number
77
weak attractions between atoms resulting from interactions between electons of one atom and the nucleus of another
van der Waals forces
78
attractive force linking two atoms
chemical bond
79
bonds that are about 1/4 as strong as hydrogen bonds
van der Waals forces
| (strength)
80
* neutrally-charged subatomic particle located in the nuclei of atoms
* molecular weight of approx. 1 amu
neuton
81
cation
positively charged ion
82
chemical change that can occur in both forward and reverse direction
reversible reaction
83
region in which electrons orbit; surrounding atomic nucleus at fixed energy level
electron shell
84
the (weighted) average mass numbers of a sample of atoms
atomic weight
85
atom containing same number of protons as shown in the periodic table, but differing in the number of neutrons within the nucleus
isotope
86
atomic weight
the (weighted) average mass numbers of a sample of atoms
87
Phosphorus has an atomic number of 15 and an atomic mass of 31. How many neutrons does phosphorus have?
A. 5
B. 16
C. 30
D. 31
E. 47
B
88
Particles having a net negative charge are called
A. electronegative
B. cations
C. anions
D. acids
E. bases
C
89
Which of the following correctly states an unusual property of water?
A. Water will not react with other atoms
B. Water's solid state is denser than its liquid state.
C. Energy is not required to change water from a wolid to a liquid.
D. Little heat energy is needed to raise the temperature of water.
E. The hydrogen bonds between water molecules continually form and break.
E
90
Polar molecules
A. have bonds with an overall positive charge.
B. have bonds with an unequal distribution of electric charge.
C. must form ions in water solution.
D. have bonds with an equal distribution of electrical charge.
E. have bonds with an overall negative charge.
B
91
Covalent bond formation depends ont eh ability of atoms to
A. share electrons with other atoms.
B. donate electrons to other atoms.
C. receive electrons from other atoms.
D. both a and b
E. all of the above
A
92
The element with which of the following atomic numbers would be most stable?
A. 1
B. 3
C. 12
D. 15
E. 18
E
93
The role of a buffer is to
A. allow the pH of a solution to vary widely.
B. make a solution basic.
C. maintain pH homeostasis.
D. disrupt pH homeostasis.
E. make a solution more acidic.
C
94
Based on the symbol for iron (Fe) shown here, select the correct list of characteristics for iron.
A. Number of protons = 26; number of electrons = 29; number of neutrons = 29
B. Number of protons = 29; number of electrons = 26; number of neutrons = 26
C. Number of protons = 26; number of electrons = 26; number of neutrons = 55
D. Number of protons = 26; number of electrons = 26; number of neutrons = 29
E. Number of protons = 55; number of electrons = 55; number of neutrons = 26
D
95
The graph shown depicts a pH scale with the pH values of several substances indicated. Which of the following statements is false?
A. Distilled water (pH 7.0) has an equal concentration of H+ and OH– ions.
B. Baking soda (pH 9.0) has a higher concentration of H+ ions than black coffee (pH 5.0).
C. Milk of magnesia (pH 10.0) has a higher concentration of OH– ions than seawater (pH 8.0)
D. A solution with a lower pH has a higher concentration of H+ ions than a solution with a higher pH.
E. A solution with a higher pH has a higher concentration of OH– ions than a solution with a lower pH.
B
96
Which example shown (A–E) depicts the correct distribution of charge and hydrogen bonding between two water molecules?
A
B
C
D
E
A
97
The accompanying figure demonstrates the process of salt dissolving in water. Which of the following is not depicted?
A. Cations and anions
B. Ionic bonding
C. Hydrogen bonding
D. Solute dissolving in water
E. Hydrophobic interactions
E
98
In comparing solid water (ice) and liquid water, select the false statement from the following choices.
A. Liquid water is less dense than solid water.
B. Solid water has a crystalline structure.
C. Hydrogen bonds hold water molecules in a rigid state in solid water.
D. In solid water, each water molecule can be hydrogen-bonded to four other water molecules.
E. Hydrogen bonds continue to break and re-form in liquid water.
A
99
Consider the accompanying figure showing a hydrogen bond between two water molecules. Which of the following properties of water is not caused by this interaction?
A. High surface tension
B. Great cohesive strength
C. Low specific heat
D. Excellence as a solvent
E. High heat of evaporation
C
99
Consider the carbonic acid (H2CO3) buffer system depicted in the graph shown. In this system, the following reaction (H2CO3 → HCO3– + H+) is utilized to reduce the effect of adding acid. From the following choices, select the one that makes the following statement true: In this buffer system, HCO3– is \_\_\_\_\_\_\_, H2CO3 is \_\_\_\_\_\_\_, and _______ would predominate in the system, receiving zero units of base.
A. a base; an acid; HCO3–
B. a base; an acid; H2CO3
C. an acid; a base; HCO3–
D. an acid; a base; H2CO3
E. basic; acidic; H2CO3
100
This figure shows the radioisotope tritium. Which of the following statements regarding radioisotopes is false?
A. Radioisotopes differ from other isotopes in that they give off energy.
B. Radioisotopes can be used as a molecular “tag” for medical diagnostic purposes.
C. Radioisotopes are unstable because they contain more protons than nonradioactive forms of the same element.
D. Radioisotopes can be damaging to cells.
E. During the process of radioactive decay, radioisotopes can release energy in the form of alpha radiation.
C
101
The part of the atom that determines how the atom behaves chemically is the
A. proton.
B. election.
C. neutron.
D. innermost shell.
E. nucleus.
B
103
Which of the following statements about chemcial reactions is false?
A. They occur when atoms combine or change their bonding partners.
B. Reactions may go to completion.
C. The products of a chemica reaction are formed from the reactants.
D. Energy may be created or destroyed in a chemical reaction.
E. Changes in forms of energy may accompany chemical reactions.
D
104
Refer to the periodic table. Which of the following has the same number of outer-shell (valence) electrons as oxygen?
A. S
B. N
C. F
D. Na
E. Ca
A
105
Covalent Bonds: Given the shell configurations of hydrogen, carbon, and sulfur (shown), select a molecule from the list below that could not be formed
A. CH4
B. H–C=C–H
C. H3C–CH3
D. H–S–H
E. S=S
B
106
Oxygen forms ___ covalent bond(s), carbon forms \_\_\_, and hydrogen forms \_\_\_.
A. 1, 4, 1
B. 4, 4, 4
C. 2, 4, 0
D. 2, 4, 1
E. 2, 2, 2
D
107
The four most common elements in organisms are
A. Ca, Fe, H, O
B. H2O, C, H, O
C. C, O, H, N
D. N, C, Fe, H
E. P, H2O, C, O
C
108
Atomic and Mass Numbers I: This figure shows an atom of helium. Which of the following characteristics is true for helium?
A. Mass number = 4; atomic number = 2; net charge = 0
B. Mass number = 4; atomic number = 4; net charge = 0
C. Mass number = 4; atomic number = 2; net charge = +2
D. Mass number = 6; atomic number = 2; net charge = 0
E. Mass number = 6; atomic number = 2; net charge = +1
A
109
Chemical Reactions: Which of the following statements about the chemical reaction in the figure shown is false?
A. The reactants are to the left of the arrow.
B. The arrow represents the direction of the chemical reaction.
C. There is more potential chemical energy in the products than in the reactants.
D. The energy associated with this reaction could be measured in calories.
E. The difference in potential chemical energy in this reaction is released as heat and light.
C
110
A basic solution contains
A. more OH- ions than H+ ions.
B. more H+ ions than OH- ions.
C. the same number of OH- ions and H+ ions.
D. no OH- ions.
E. none of the above
A
111
Ions: Given the electron shell configuration and mass and atomic numbers for the sodium ion (Na+) shown here, select the correct choice below to complete the following sentence: The sodium ion has _______ protons in its nucleus, _______ electrons in its outermost shell, and it is a(n) \_\_\_\_\_\_\_.
A. 10; 0; anion
B. 11; 8; anion
C. 11; 0; anion
D. 10; 0; cation
E. 11; 8; cation
E
112
Given the electron shell configuration for sulfur (S) shown, select the correct choice below to complete the following sentence: Sulfur has _______ protons in its nucleus and requires _______ more electrons to complete its outer shell.
A. 8; 2
B. 8; 6
C. 16; 2
D. 16; 6
E. 16; 8
C
113
What determines if a molecule is polar, nonpolar, or ionic?
A. the number of protons
B. the bond distances
C. the differences in the electronegativities of the atoms
D. the ionic charges
E. the distance of the electrons from the nucleus
C
114
The three most abundant elements in a human skin cell are
A. calcium, carbon, and oxygen.
B. carbon, hydrogen, and oxygen.
C. carbon, hydrogen, and sodium.
D. carbon, nitrogen, and potassium.
E. nitrogen, hydrogen, and argon.
B
115
Which of the following statements about the isotopes of an element is not true?
A. They all have the same atomic number.
B. They all have the same number of protons.
C. They all have the same number of neutrons.
D. They all have the same number of electrons.
E. They all have identical chemical properties.
C
116
The atomic weight (atomic mass) of an element
A. equals the number of neutrons in an atom.
B. equals the number of protons in an atom.
C. equals the number of electrons in an atom.
D. equals the number of neutrons plus the number of protons.
E. depends on the relative abundances of its electrons and neutrons.
D
117
The atomic number of an element
A. equals the number of neutrons in an atom.
B. equals the number of protons in an atom.
C. equals the number of protons minus the number of neutrons.
D. equals the number of neutrons plus the number of protons.
E. depends on the isotope.
B
118
When table salt (NaCl) is added to water,
A. a covalent bond is broken.
B. an acidic solution is formed.
C. the Na+ and Cl− ions are separated.
D. the Na+ ions are attracted to the hydrogen atoms of water.
E. water molecules surround the Na+ (but not Cl−) ions.
C
119
Hydrophobic interactions
A. are stronger than hydrogen bonds.
B. are stronger than covalent bonds.
C. can hold two ions together.
D. can hold two nonpolar molecules together.
E. are responsible for the surface tension of water.
D
121
The reaction HCl → H+ + Cl− in the human stomach is an example of the
A. cleavage of a hydrophobic bond.
B. formation of a hydrogen bond.
C. elevation of the pH of the stomach.
D. formation of ions by dissolving an acid.
E. formation of polar covalent bonds.
D
122
Which of the following statements about water is not true?
A. It releases a large amount of heat when changing from liquid into vapor.
B. Its solid form is less dense than its liquid form.
C. It is the most effective solvent for polar molecules.
D. It is typically the most abundant substance in a living organism.
E. It takes part in some important chemical reactions.
A
123
The hydrogen bond between two water molecules arises because water is
A. polar.
B. nonpolar.
C. a liquid.
D. small.
E. hydrophobic
A
124
Which of the following statements about covalent bonds is not true?
A. A covalent bond is stronger than a hydrogen bond.
B. A covalent bond can form between atoms of the same element.
Cc. Only a single covalent bond can form between two atoms.
D. A covalent bond results from the sharing of electrons by two atoms.
E. A covalent bond can form between atoms of different elements.
C
125
positively-charged subatomic particle
Proton
126
nucleus
| (chemistry)
center of an atom that contains protons and neutrons
127
compound
substance made up of atoms of more than one element
128
Ionic Bond
bond between charged ions
129
Proton
positively-charged subatomic particle
130
substance that can accept hydrogen ion in solution
Base
131
energy required to convert liquid to a gas
heat of vaporization
132
solvent and dissolved solute mixture
solution
133
uncharged, nonpolar groups of atoms/molecules that have no affinity for water
hydrophobic
134
pH
* measure of a solution's acidity/hydrogen ion concentration
* -log( [H+] )
135
having an affinity for water; polar
hydrophillic
136
negatively charged ion
anion
137
capacity to do work or to accomplish change in physical or chemical systems
energy
138
region in space surrounding nucleus in which an electron is most likely to be found
orbital
139
substance that can release a proton in solution
acid
140
having opposite electric charges at two ends
polar
141
chemical substance consisting of two or more atoms joined by bonds or attractions
molecule
142
substance that enters into a chemical reaction
reactant
143
liquid in which solutes are dissolved to form a solution
solvent
144
sum of atomic weights in a molecule
Molecular Weight
145
negatively charged subatomic particle
electron
| (def)
146
weak electrostatic bond between slightly-positive hydrogen atom and slightly-negative charge on a nearby atom
hydrogen bond
147
electrically charged particle that forms when atom gains or loses electron(s)
ion
148
weak attractions between atoms resulting from interactions between electons of one atom and the nucleus of another
van der Waals forces
149
bonds that are about 1/4 as strong as hydrogen bonds
van der Waals forces
| (strength)
150
* neutrally-charged subatomic particle located in the nuclei of atoms
* molecular weight of approx. 1 amu
neuton
151
chemical change that can occur in both forward and reverse direction
reversible reaction
152
region in which electrons orbit; surrounding atomic nucleus at fixed energy level
electron shell
153
mass number
sum of an atom's protons and neutrons
154
radioactive isotope
(e.g. carbon-14, hydrogen-3, tritium)
radioisotope
155
buffer
substance that can accept or release hydrogen ions to resist changes in pH
156
specific heat
amount of energy required to raise 1 gram of a substance by 1 deg C
157
atom containing same number of protons as shown in the periodic table, but differing in the number of neutrons within the nucleus
isotope
158
amount of energy required to raise 1 gram of a substance by 1 deg C
specific heat
159
substance made up of atoms of more than one element
compound
160
tendency of molecules to stick together
cohesion
161
substance that cannot be converted to a simpler substance
element
162
* equivalent to the number of protons in an atom's nucleus (equal to electrons around atom)
* determines chemical properties of atom
atomic number
163
affinity of an atom to attract electrons when it occurs as part of a compound
electronegativity
164
avogadro's number of something
mole
165
bond based on the (equal or unequal) sharing of electrons between two atoms
covalent bond
166
6.022 x 10^23
avogadro's number
167
attractive force linking two atoms
chemical bond
168
* measure of a solution's acidity/hydrogen ion concentration
* -log( [H+] )
pH
169
substance that can accept or release hydrogen ions to resist changes in pH
buffer
170
center of an atom that contains protons and neutrons
nucleus
| (chemistry)
171
Base
substance that can accept hydrogen ion in solution
172
heat of vaporization
energy required to convert liquid to a gas
173
solution
solvent and dissolved solute mixture
174
hydrophobic
uncharged, nonpolar groups of atoms/molecules that have no affinity for water
175
radioisotope
radioactive isotope
(e.g. carbon-14, hydrogen-3, tritium)
176
substance dissolved in a liquid to form a solution
solute
177
sum of an atom's protons and neutrons
mass number
178
hydrophillic
having an affinity for water; polar
179
anion
negatively charged ion
180
bond between charged ions
Ionic Bond
181
energy
capacity to do work or to accomplish change in physical or chemical systems
182
orbital
region in space surrounding nucleus in which an electron is most likely to be found
183
cohesion
tendency of molecules to stick together
184
acid
substance that can release a proton in solution
185
polar
having opposite electric charges at two ends
186
element
substance that cannot be converted to a simpler substance
187
molecule
chemical substance consisting of two or more atoms joined by bonds or attractions
188
reactant
substance that enters into a chemical reaction
189
atomic number
* equivalent to the number of protons in an atom's nucleus (equal to electrons around atom)
* determines chemical properties of atom
190
solvent
liquid in which solutes are dissolved to form a solution
191
solute
substance dissolved in a liquid to form a solution
192
electronegativity
affinity of an atom to attract electrons when it occurs as part of a compound
193
Molecular Weight
sum of atomic weights in a molecule
194
mole
avogadro's number of something
195
electron
| (def)
negatively charged subatomic particle
196
covalent bond
bond based on the (equal or unequal) sharing of electrons between two atoms
197
hydrogen bond
weak electrostatic bond between slightly-positive hydrogen atom and slightly-negative charge on a nearby atom
198
cation
positively charged ion
199
ion
electrically charged particle that forms when atom gains or loses electron(s)
200
avogadro's number
6.022 x 10^23
201
van der Waals forces
weak attractions between atoms resulting from interactions between electons of one atom and the nucleus of another
202
chemical bond
attractive force linking two atoms
203
van der Waals forces
| (strength)
bonds that are about 1/4 as strong as hydrogen bonds
204
neuton
* neutrally-charged subatomic particle located in the nuclei of atoms
* molecular weight of approx. 1 amu
205
positively charged ion
cation
206
reversible reaction
chemical change that can occur in both forward and reverse direction
207
electron shell
region in which electrons orbit; surrounding atomic nucleus at fixed energy level
208
atomic weight
the (weighted) average mass numbers of a sample of atoms
209
isotope
atom containing same number of protons as shown in the periodic table, but differing in the number of neutrons within the nucleus
210
the (weighted) average mass numbers of a sample of atoms
atomic weight
