Solution Manual For Essentials of General, Organic, and Biochemistry, 3rd Edition

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Solution Manual For Essentials of General, Organic, and Biochemistry, 3rd Edition helps you navigate your textbook with ease, offering answers to every question.

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Solutions Manual to accompany
Guinn’s Essentials of General, Organic, and
Biochemistry
Third Edition
Rachel C. Lum

2 Chapter 1
Chapter 1
Matter, Energy, and Measurement
37 Bone strength is assessed with a bone mineral density (BMD) measurement.
38 A strong bone has more bone mineral per volume than a weak one.
39 A DEXA (dual energy x-ray absorptiometry) scan is used to estimate BMD.
40 A T-score is assigned by how much a patient’s BMD deviates from the average BMD of healthy
people of the same gender and ethnicity.
41 The patient has osteopenia.
42 Her bone is normal.
43 The three physical states of matter are solid (s), liquid (l), and gas (g).
44 The particles interact with other particles in the liquid and solid states.
45 The particles are farther apart in the liquid and gas states.
46 Temperature is a measure of the average kinetic energy of particles.
47 Work is involved in moving an object.
48 A ball sitting at the top of a hill has stored energy, so it has potential energy.
49 A ball rolling downhill has kinetic energy.
50 a. kinetic energy (The water is moving.) b. potential energy (The skier is at the top of a hill.)
c. kinetic energy (The dancer is moving.) d. potential energy (The atoms in the sandwich have
stored energy in their bonds.)
51 a. kinetic energy (The biker is moving.) b. potential energy (The hiker is at the top of a mountain.)
c. kinetic energy (The helium atoms are moving within the balloon.)
d. potential energy (Energy is stored in the bonds of the molecules that make up candle wax.)
52 a. Molecules have the least amount of kinetic energy in the solid state.
53 c. Molecules have the greatest amount of kinetic energy in the gas state.
54 Steam. The water molecules are in the gas state.
55 a. A hospital is on the macroscopic scale. (You can see it.) b. A skin cell is on the microscopic
scale. (You need a microscope to see it.) c. DNA is on the atomic scale. (DNA is too small to be
seen.) d. A red blood cell is on the microscopic scale. (You need a microscope to see it.)
56 a. A lead atom is on the atomic scale. (It is too small to be seen.) b. The human body is on the
macroscopic scale. (You can see it.) c. A grain of sand is on the macroscopic scale. (You can
see it.) d. A virus is on the atomic scale. (It is too small to be seen.)
57 The SI system is an international system of units and was created by an international group of
scientists to establish a uniform set of units, selecting one standard metric unit for each quantity of
measurement.
58 the gram

Matter, Energy, and Measurement 3
59 mass and weight
60 length and distance
61 the liter
62 the second
63 pico (10 12 in a base unit); nano (10 9 in a base unit); micro (10 6 in a base unit); and kilo (10–3 in a
base unit)
64 milli (10 3 in a base unit); centi (10 2 in a base unit); deci (10 in a base unit); and giga (10−9 in a
base unit)
65 a. mm is a metric unit of length. b. in. is an English unit of length.
c. oz is an English unit of volume. d. g is a metric unit of mass.
66 a. kg is a metric unit of mass. b. lb is an English unit of mass.
c. mL is a metric unit of volume. d. ft is an English unit of length.
67 1 cm = 10–2 m
68 1 ps = 10−12 s
69
70 1 kW = 10 3 W
71
72 6.3 × 10−3 mm is smaller. The millimeter is a measure of length.
73 a graduated cylinder, a pipette, and a syringe
74 A meniscus is a curved surface of a liquid that forms when it is in a graduated cylinder.
75 c. at the bottom of the meniscus
76 Vlead = 16.5 mL – 15.0 mL = 1.5 mL
77 Vmetal = 203.5 mL – 200. mL = 3.5 mL
78 Volume = 24 cm × 24 cm ×24 cm = 14,000 cm3 = 14,000 mL
79 Volume = 5.21 cm × 5.21 cm × 5.21 cm = 141 cm3
80 a. 57,000 m measured value because it is a length; two significant figures
b. 4.60 mL measured value because it a volume; three significant figures
c. 0.00011 g measured value because it is a mass; two significant figures
d. 23,304.60 s measured value because it is time; seven significant figures
e. exact number because 256 nurses is a number obtained by counting the number of nurses
81 a. 304 mm measured value because it is a length; three significant figures; a zero between
nonzero digits is significant. b. exact number because 429 bees is a number obtained by
counting the number of bees c. 5,110 minutes measured value because it is time; three
significant figures d. 0.000330 kg measured value because it is a weight; three significant
figures; the zeros between the decimal and the first digit, 3, are not significant, they are
placeholders. The zero after the last digit, 3, is significant and the uncertain digit.
e. 5,000. g measured value because it is a weight; four significant figures
82 a. 2.31 μg b. 9,3100 mm c. 1.56 L d. 5680 s
83 a. 1.8 nm b. 4.3 mL c. 28 pg d. 360 m
84 c. 0.63
85 b. 79.88
1m =B 106 B
4 5. ×10 2 μg is larger. The microgram is a measure of mass.

4
86 a. 3.2 × 8.54 = 27 b. 3.2 + 8.54 = 11.7
87 a. 2.26 + 8.1 = 10.4 b. 2.26 × 8.1 = 18
88 a. 56.33 cm × 2.50 cm = 140 cm2
b. 3.4 cm + 2.2 cm + 5.11 cm + 8.777 cm = 19.5 cm
c. = 0.852 g/mL
ଷଷ.ଶଶ ୥
ଷଽ.଴ ୫L
Chapter 1
89 a. 33,000. + 910. = 33,910. b. 0.333 × 0.22 = 0.073
c. (37.55 mL + 22.2 mL) × 5.666 = 339 mL
90 a. 50,000 ݉ × ଵ ୩୫
ଵ଴଴଴ ୫
b. = 6.6 ×10 5 μgଵ
ଵ μ୥
= 50 km
0.66 g × ଴షల ୥
91 a. . 6.0 L × ଵ ୫L
ଵ଴షయ L = 6.0 × 10 ଷ
ଵ୩୫
mL
b. 2.0 × 10଺m × ଵ଴଴଴ ୫ = 2.0 × 10ଷkm
92 c. 1,000 mm is equivalent to 1 m.
93 b. 0.001 kg is equivalent to 1 g.
94 1 m = 10−3 km
95 2.5 cm × ଵ଴షమ ୫
ଵ ୡ୫ = 0.025 m
96 200 mg × ଵ଴షయ ୥
ଵ ୫୥ = 0.2 g
97 500. mg × ଵ଴షయ ୥
ଵ ୫୥ = 0.500 g
0.500 g × ଵμ୥
ଵ଴షల ୥ = 5.00 × 10ହ μg
98 1 mm = 10−3 m and 1 pm = 10−15 m
99 75.6 μL × ଵ଴ షల L
ଵ μL × ଵ୫L
ଵ଴షయ L = 0.0756 mL
100 150 kg × ଶ.ଶ଴ହ ୪ୠ
ଵ ୩୥ = 330 lb
101 68.2 miles × ହଶ଼଴ ୤୲
ଵ ୫୧୪ୣ × ଵଶ ୧୬
ଵ ୤୲ × ଵ ୫
ଷଽ.ଷ଻ ୧୬ × ଵ ୩୫
ଵ଴య୫ = 110. km
102 86 gallons × ସ ୯୲
ଵ ୥ୟ୪୪୭୬ × ଵ L
ଵ.଴ହ଻ ୯୲ = 330 L
103 b. 26.7 mm × ଵ଴షయ ୫
ଵ ୫୫ × ଷଽ.ଷ଻ ୧୬.
ଵ ୫ = 1.05 in.
104 d. 14.3 cmଷ × ଵ଴షయ L
ଵ ୡ୫య = 0.0143 L
105 a.
b. 1 cm × ଵ଴ షమ ୫
ଵ
1 km × ଵ଴ య୫
ଵ ୩୫ × ଵ ୫୫
ଵ଴ షయ ୫ = 1 × 10଺ mm
ୡ୫ × ଵ ୫୫
ଵ଴ షయ ୫ = 10 mm
c. 1 dm × ଵ଴ షభ୫
ଵ ୢ ୫ × ଵ ୫୫
ଵ଴ షయ ୫ = 100 mm
d.1 nm × ଵ଴ షవ ୫
ଵ ୬୫ × ଵ ୫୫
ଵ଴ షయ ୫ = 1 × 10ି ଺ mm

Matter, Energy, and Measurement 5
106 a. 1 g × ଵ ୩୥
ଵ଴ య ୥ = 1 × 10ି ଷ kg
b. 1 ng × ଵ଴ షవ ୥
ଵ ୬୥ × ଵ ୩୥
ଵ଴ య ୥ = 1 × 10ି ଵଶ kg
c. 100 mcg × ଵ଴ షల୥
ଵ୫ୡ୥ × ଵ ୩୥
ଵ଴ య ୥ = 1 × 10ି ଻ kg
d. 10 μg × ଵ଴ షల ୥
ଵ μ୥ × ଵ ୩୥
ଵ଴ య ୥ = 1 × 10ି଼ kg
107 a. 5 mL × ଵ଴ షయL
ଵ ୫L × ଵ μL
ଵ଴ షల L = 5 × 10ଷ μL
b. 0.5 L × ଵ μL
ଵ଴ షల L = 5 × 10ହ μL
c. 250 cm ଷ × ଵ଴ షయ L
ଵ ୡ୫య × ଵ μL
ଵ଴ షల L = 2.5 × 10 ହ μL
d. 80 dL × ଵ଴ షభL
ଵ ୢ L × ଵ μL
ଵ଴ షల L = 8 × 10଺ μL
108 c. 150 μg is equivalent to 1.5 ×10−7 kg.
109 density = ଽ.ଶଶ ୥଼
.଻ ୫L = 1.1 g/mL
110 density = ଷ.଼ ୥
ଶ.଴ ୡ୫ య × ଵୡ୫య
ଵ ୫L = 1.9 g/mL
111 Water has a density of 1.0 g/mL.
112 A liquid with a density greater than 1.0 g/mL will sink in water.
113 volume = 2.3 mL
2.3 mL × ଵଽ.ଷଶ ୥
ଵ ୫L = 44 g
114 volume = (length of side) 3
volume = (2.20 cm) 3
volume = 10.6 cm3
10.6 cmଷ × ଵଽ.ଷଶ ୥
ଵୡ୫య = 205 g
115 specific gravity = ଵ.଴ଶହ ୥/୫L
ଵ.଴ ୥/୫L = 1.025
Yes, the specific gravity is within the normal range.
116 specific gravity = ଵ.଴ଷ଻ ୥/୫L
ଵ.଴ ୥/୫L = 1.037
No, the specific gravity is not within the normal range.
117 density of urine = 1.014 × 1.0 g⁄mL = 1.014 g/mL
The specific gravity of the urine sample is within the normal range.
118 density of urine = 0.997 × 1.0 g⁄mL = 0.997 g/mL
The specific gravity of the urine sample is not within the normal range.
119 The abbreviation q.d. indicates that Accupril should be administered once a day. 10 mg should be
given at every administration.
120 The abbreviation b.i.d. indicates that Retrovir should be administered twice a day. 300 mg should
be given at every administration.
121 34 lb × ଵ ୩୥
ଶ.ଶ଴ହ ୪ୠ × ଶହ ୫୥
୩୥∙ୢୟ୷ = 390 ୫୥ୢ
ୟ୷
122 27 kg × ଶ.ଶ଴ହ ୪ୠ
ଵ ୩୥ ୪ୠ∙ୢୟ୷ୢ ୟ୷
× ଵ ୫୥ = 60 ୫୥

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6
123 12 lb × ଵ ୩୥
Chapter 1
ଶ.ଶ଴ହ ୪ୠ × ଶ଴ ୫୥
୩୥∙ୢୟ୷ × ଵ ୢ ୟ୷
ଷ ୢ ୭ୱୣ = 36 mg/dose
124 Tamiflu should be administered twice a day.
16 lb × ଵ ୩୥
ଶ.ଶ଴ହ ୪ୠ × ଷ ୫୥
୩୥∙ୢୟ୷ × ଵ ୢ ୟ୷
ଶ ୢ ୭ୱୣ = 11 mg/dose
125 The freezing point of water is 0 C° and 32 °F .
126 Normal body temperature is 37 °C and 98.6 °F.
127 b. in the refrigerator (1.8 × 2 ℃) + 32 = 36 ℉
(1.8 × 8 ℃) + 32 = 46 ℉
128 c. in a medicine cabinet (1.8 × 15 ℃) + 32 = 59 ℉
(1.8 × 30 ℃) + 32 = 90 ℉
129 18 ℃ + 273.15 = 291 K
(1.8 × 18 ℃) + 32 = 64 ℉
31 ℃ + 273.15 = 304 K
(1.8 × 31 ℃) + 32 = 88 ℉
You are wearing summer clothes.
(ଵ଴ହ.ଶ ℉ ି ଷଶ)
(଼଻.ସ ℉ ି ଷଶ)
ଵ.଼
You are wearing summer clothes.
130
131 = 40.7 ℃
132 ଵ.଼ = 30.8 ℃
133 (1.8 × 33 ℃) + 32 = 91 ℉
The patient has hypothermia.
134 2.7 K − 273.15 = −270.4 ℃
(1.8 × (−270.4 ℃)) + 32 = −454.7 ℉
135 −78 ℃ + 273.15 = 195 K
(1.8 × (−78 ℃)) + 32 = −110 ℉
136 77 K − 273.15 = −196 ℃
(1.8 × (−196 ℃)) + 32 = −321 ℉
137 Carbohydrates and fats provide us most of our energy.
138 Glucose is the most important source of energy for the body.
139 The body will convert muscle into glucose to produce energy.
140 Glucose is a high in potential energy.
141 Carbon dioxide is low in potential energy.
142 2 cm volume = length × width × height = 8 cm3 = 2√8
య
143 Convert all measurements to a common unit.
5,000 μL × ଵ଴షల L
ଵ μL × ଵ ୫L
ଵ଴షయ L = 5 mL
0.5000 L × ଵ ୫L
ଵ଴షయ L = 500.0 mL
8.000 cm ଷ = 8.000 mL
Largest to smallest: 0.5000 L, 50.00 mL, 8.000 cm3 , 5,000 μL
144 a. 10 m b. the same length c. the same length d. 1 nm
145 a. 1 ng b. 100 mg c. the same mass d. 50 mcg

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Matter, Energy, and Measurement 7
146 2.5 in.× ଶ.ହସ ୡ୫
ଵ ୧୬. = 6.4 cm
volume = length × width × height = 6.4 cm × 6.4 cm × 6.4 cm = 262 cm3
mass = density × volume = 7.87 ୥
ୡ୫య × 262 cmଷ = 2.06 × 10ଷg
2.06 × 10ଷ g × ଵ ୫୥
ଵ଴ షయ ୥ = 2.06 × 10଺ mg
147 a. twice daily
b. two times a day
c. 62 lb × ଵ ୩୥
ଶ.ଶ଴ହ ୪ୠ × ଶହ ୫୥
୩୥∙ୢୟ୷ × ଵ ୢ ୟ୷
ଶ ୢ ୭ୱୣ = 350 mg/dose
d. (1.8 × 20 ℃) + 32 = 68 ℉ It should be stored in the refrigerator.
e. The particles in the tablet are close together since they are in the solid state.
148 3.2 mm × ଵ଴ షయ୫
ଵ ୫୫ × ଵ ୡ୫
ଵ଴ షమ ୫ = 0.32 cm
volume = length × width × height = 0.32 cm × 0.32 cm × 0.32 cm = 0.033 cm3 = 0.033 mL
149 volume = length × width × height = 147cm3 య
√147
5.27 cm × ଵ ୧୬.
ଶ.ହସ ୡ୫ = 2.07 in.
= 5.27cm

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8 Chapter 2
Chapter 2
Atomic Structure and Radioisotopes
41 Iodine is concentrated in the thyroid gland.
42 The common sources of iodine in foods are dried seaweed, yogurt, turkey breast, tuna, eggs,
potatoes, strawberries, and cranberries.
43 The symptoms of an iodine deficiency in an adult are an enlarged thyroid or goiter. Severe iodine
deficiency is linked to high infant mortality and physical and learning disabilities.
44 Iron requires a daily intake of 8–18 mg.
45 Hemoglobin is a substance in red blood cells that transports oxygen.
46 Iron is found in red meat, pork, poultry, beans, seafood, dark green leafy vegetables, dried fruit,
and cereal.
47 A person is anemic when they have a diminished number of red blood cells produced.
48 Fluoride builds strong bones and tooth enamel. Fluoride is found in fluoridated water.
49 Zinc is necessary for wound healing and fighting infection. Zinc is found in oysters, breakfast
cereal, beef, pork, chicken, yogurt, baked beans, and nuts.
50 The smallest stable component of matter is an atom.
51 Protons, neutrons, and electrons are three subatomic particles found in an atom. The protons and
neutrons are found in the nucleus, whereas the electrons are found in electron orbitals.
52 A proton has a +1 charge; a neutron has no charge; and an electron has a −1 charge.
53 the proton and the neutron
54 the proton and the neutron
55 the electron
56 The heavier particles (the protons and the neutrons) are concentrated in the small volume of the
nucleus. Therefore, the nucleus is extremely dense.
57 The mass of a proton is 1.007 amu and 1 6. ×726 10−24 g.
58 The atomic number represents the number of protons in an atom.
59 a. Sb, antimony b. As, arsenic c. Al, aluminum d. Ra, radium
60 a. Mg, magnesium b. Si, silicon c. Ba, barium d. Se, selenium
61 a. carbon, C b. thallium, Tl c. uranium, U d. platinum, Pt e. cobalt, Co
62 a. Beryllium, Be b. Manganese, Mn c. Palladium, Pd d. Thorium, Th e. Seaborgium, Sg
63 Lead is located between thallium and bismuth. Lead has 82 protons; thallium has 81 protons;
bismuth has 83 protons.
64 Titanium is located between scandium and vanadium.
65 a. boron, B, atomic number 5, 5 protons and 5 electrons b. cesium, Cs, atomic number 55, 55
protons and 55 electrons c. gallium, Ga, atomic number 31, 31 protons and 31 electrons
d. strontium, Sr, atomic number 38, 38 protons and 38 electrons
66 a. rubidium, Rb, atomic number 37, 37 protons and 37 electrons b. argon, Ar, atomic number
18, 18 protons and 18 electrons c. helium, He, atomic number 2, 2 protons and 2 electrons
d. cadmium, Cd, atomic number 48, 48 protons and 48 electrons

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Atomic Structure and Radioisotopes 9
67 a. oxygen, atomic number 8
.
b. sodium, atomic number 11 c. copper, atomic number 29
d. tin, atomic number 50 e ruthenium, atomic number 44 f. tungsten, atomic number 74
g. europium, atomic number 63.
68 a. fluorine, atomic number 9 b. radium, atomic number 88 c. osmium, atomic number 76
d. silver, atomic number 47 e. mercury, atomic number 80 f. americium, atomic number 95
g. molybdenum atomic number 42
69 a. Oxygen has 8 protons and 8 electrons. b. Chromium has 24 protons and 24 electrons.
c. Phosphorus has 15 protons and 15 electrons.
70 a. Vanadium has 23 protons and 23 electrons. b. Sulfur has 16 protons and 16 electrons.
c. Magnesium has 12 protons and 12 electrons.
71 The mass number of an isotope represents the sum of the protons and neutrons.
72 Isotopes are atoms that have the same number of protons but a different number of neutrons.
Isotopes of an element differ in the number of neutrons they contain. Isotopes of an element have
the same number of protons and electrons.
73
74 Tc-99 has 43 protons, 43 electrons, and 56 neutrons. ସଷ
ଽଽ
Tc
75
Isotope Atomic Number Number of Protons Number of Neutrons Mass Number
Sulfur-32 16 16 16 32
Sulfur-33 16 16 17 33
Sulfur-34 16 16 18 34
Sulfur-36 16 16 20 36
76 All the sulfur isotopes have the same number of protons and the same number of electrons.
77 Sulfur-32 has the smallest mass.
78 The natural abundance and the mass of each isotope are used to calculate a weighted average,
which is the atomic mass.
79 a. The atomic number for both isotopes is 35. b. The mass numbers are 79 and 81.
c. One of the isotopes has two more neutrons than the other one. d. The average atomic mass is
79.90. Yes, it does. e. There are roughly equal amounts of both isotopes present in bromine.
80 a. iron-54 b. iron-58 c. iron-56 d. iron-54 e. Iron-56 is present in the greatest amount,
but there are three other isotopes of iron that contribute to the mass of iron.
81 A family or group of elements has elements in the same column in the periodic table.
82 Group 1A (alkali metals), group 2A (alkaline earth metals), group 3A, group 4A, group 5A, group
6A, group 7A (halogens), and group 8A (noble gases) are the groups of the main group elements.
The transition metal elements are located between group 2A and group 3A. The inner transition
metal elements are located between group 3B and 4B.
83 Elements within a group exhibit similar physical and chemical properties.
84 a period
16 17 18
8 8O O, , 8 O

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10
85 a. group 2A, alkaline earth metal b. group 8A, noble gases c. group 7A, halogens
d. group 1A, alkali metals e. group 7A, halogens
86 a. group 1A, alkali metals b. group 4A c. group 8B d. group 3A
e. group 8A, noble gases
87 Nonmetals are dull; can exist as solids, liquids, or gases at room temperature; are poor conductors
of electricity; and can be brittle, hard, or soft. Metals are shiny, exist as solids at room temperature
(except for mercury), are good conductors of electricity, and are malleable.
88 a. nonmetal b. metalloid c. nonmetal d. metal
89 a. metal b. nonmetal c. metalloid d. metal e. nonmetal
90 a. potassium b. radon
91 a. palladium b. uranium
92 The macronutrients are Na, K, Mg, Ca, P, S, and Cl.
93 The micronutrients are V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Si, Se, F, and I.
94 the electron
95 less energy
96 more energy
97 The group number equals the number of valence electrons for the elements in that group.
98
Element
Name
Atomic
Symbol
Atomic
Number
Group
Number
Period
Number
Number of Electrons
n = 1 n = 2 n = 3
a. boron B 5 3A 2 2 3 0
b. phosphorus P 15 5A 3 2 8 5
c. sodium Na 11 1A 3 2 8 1
d. sulfur S 16 6A 3 2 8 6
Chapter 2
99
Element
Name
Atomic
Symbol
Atomic
Number
Group
Number
Period
Number
Number of Electrons
n = 1 n = 2 n = 3
a. oxygen O 8 6A 2 2 6 0
b. beryllium Be 4 2A 2 2 2 0
c. argon Ar 18 8A 3 2 8 8
d. fluorine F 9 7A 2 2 7 0
100 halogens, group 7A
101 group 4A
102 noble gases, group 8A
103 Boron has three valence electrons in the n = 2 level; aluminum has three valence electrons in the
n = 3 level.
104 eight electrons

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Atomic Structure and Radioisotopes 11
105 two electrons
106 a. n = 4, two valence electrons b. n = 3, one valence electron c. n = 5, eight valence electrons
d. n = 2, six valence electrons e. n = 1, one valence electron
107 Radioisotopes are unstable isotopes of an element. They have an imbalance in the ratio of neutrons
to protons in the nucleus.
108 Radioactive decay occurs when an unstable radioisotope produces a more stable nucleus by
releasing radiation.
109 α and β particles. The nuclear symbols are respectively.ଶ
ସ α and ି ଵ ଴
β,
110 a. 213 209 4
83 Bi → 81Tl 2 α+ b. The daughter nuclide is thallium-209.
111 a. 211 207 4
85 At → 83 Bi 2 α+ b. The daughter nuclide is bismuth-207.
112 a. 153 153 0
62 Sm → 63 Eu −1β+ b. The daughter nuclide is europium-153.
113 a. 32 32 0
15 P S→ +16 −1β b. The daughter nuclide is sulfur-32.
114 a. 26 26 0
11 Na → 12 Mg −1β+ b. 232 228 4
81Tl → 79 Au 2 α+
115 a. 225 221 4
89 Ac → 87 Fr 2 α+ b. 107 107 0
46 Pd → 47 Ag −1β+
116 16 g (initial amount), 8 g (one half-life), 4 g (two half-lives); 4 g remains after 156 hours or two
half-lives.
117 18.0 g (initial amount), 9.0 g (one half-life), 4.5 g (two half-lives), 2.25 g (three half-lives), 1.125g
(four half-lives); 1.125 g remains after 32 days or four half-lives.
118 28 g (initial amount), 14 g (one half-life), 7 g (two half-lives), 3.5 g (three half-lives), 1.75 g (four
half-lives)
44 days
4 half lives × 176 days
1 half life =
It takes 4 half-lives or 176 days for 28 g of iron-59 to decay to 1.75 g.
119 It has a very short half-life and won’t remain in the body for a long time.
120 1 half-life
24 days × = 3 half-lives
8 days
25.0 mg (initial amount), 12.5 mg (one half-life), 6.25 mg (two half-lives), 3.125 mg (three half-
lives)
3.125 mg will remain after 24 days.
121 66 hours
122 Electromagnetic radiation is a form of energy that travels through space, as a wave, at the speed of
light.
123 light
124 gamma rays, x-rays, ultraviolet, visible, infrared, microwave, and radio waves
125 a. radio waves b. x-ray c. visible
126 a. visible b. ultraviolet light c. γ-rays
127 α particles, neutrons, and β particles
128 When a daughter nuclide is an “exited state,” it has excess energy in the nucleus. The letter m after
the mass number is used to denote the metastable state.

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12 Chapter 2
129 Irradiating fruits and vegetables destroys disease-causing microorganisms and reduces spoilage
caused by bacteria. When food is irradiated, only the energy from electromagnetic radiation
emitted, not the radioisotope itself, comes in contact with the food.
130 Ionizing radiation has sufficient energy to dislodge a valence electron from an atom.
131 Ionizing radiation can kill cells. It can also cause gene mutations in the cells.
132 The mutations that ionizing radiation causes are passed when a cell reproduces, which can be the
beginning of cancer.
133 Ionizing radiation affects rapidly dividing cells such as lymphocytes (white blood cells), blood-
producing cells, and cancer cells.
134 the energy and penetrating power of the radiation
135 X-rays have more penetrating power than radio waves. Therefore, when you go to the dentist you
need to wear a lead apron.
136 An α particle is high in energy and very destructive to human tissue. If you swallow an α emitter,
the high energy is close to the tissue. An α particle is also heavy and slow moving, so it has little
penetrating power. It can be stopped by a piece of paper.
137 The lead apron protects your neck and chest from the penetrating power of the x-rays.
138 a. γ-rays b. α particles c. β particles
139 a. β particles b. γ-rays c. γ-rays
140 An α particle has the highest amount of energy, but the least penetrating power.
141 α particles, β particles, and x-rays
142 An absorbed dose measures the energy of radiation absorbed per mass of tissue but does not take
into account the penetrating power of the radiation. The effective dose takes into account both the
penetrating power of radiation and the amount of energy to give a biological effect. The unit for
absorbed dose used in medicine is the Gray. The effective dose in medicine is measured in
Sieverts.
143 a. chronic exposure b. acute exposure c. chronic exposure d. acute exposure
144 You can expect loss of hair all over the body, fatigue, general illness, and a high risk of infection
for an exposure to 2.4 Sv of radiation.
145 An LD50 indicates a level of exposure that would result in death in 50% of the population in 30
days. An effective dose of 3–4 Sv is LD50 for radiation exposure.
146 Radiation-based diagnostic techniques allow medical professionals to “see” internal organs and
systems for the purpose of diagnosis. Imaging techniques can eliminate the need for exploratory
surgery.
147 X-ray imaging and CT scans. X-rays are high-energy forms of electromagnetic radiation.
148 The detectors in a CT are arranged in a circular array that surrounds the body.
149 The quarter is higher in density than the tissue in the esophagus. The quarter absorbed more x-rays
and is lighter in color than the tissue of the esophagus.
150 A CT scan can be used to detect a brain hemorrhage. A regular x-ray can be used to detect a simple
fracture.

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Atomic Structure and Radioisotopes 13
151 The building block elements make up the structure of the majority of compounds found in living
organisms. They are carbon, 4 valence electrons; hydrogen, 1 valence electron; nitrogen, 5 valence
electrons; oxygen, 6 valence electrons; phosphorus, 5 valence electrons; and sulfur, 6 valence electrons.
152 Astatine has seven valence electrons. They are in the = 6 energy level.n
153 A helium atom has the smaller diameter and volume because it has fewer electrons. As the number
of electrons increases, the outermost electrons spend more of their time in larger orbitals that
extend farther from the nucleus, thereby increasing the diameter of the atom. The helium atom
would be lighter since it only has 2 protons, whereas gold has 79 protons.
154 A selenium atom has the larger diameter because it has more electrons, which take up more space
around the nucleus.
155 average atomic mass = (78.9183)(. 5069) + (80.9163)(. 4931) = 79.904
157 The danger of nuclear waste is that some of the radioisotopes have very long half-lives. Yes,
hospitals produce nuclear waste, but the half-lives of the radioisotopes used in hospitals range
from a few hours to a few days, not thousands of years.
158 a. γ-ray has more penetrating power and can cause more damage to biological tissue.
b. Ultraviolet light is higher in energy than visible light and can cause more damage.
159 α decay and β decay
160 a.
.
210 206 4
86 Rn → 84 Po + 2 α b. 90 90 0
39Y Z→ +40 r −1β
Lu177 177 0
71 → 72 Hf + −1β161 a
b.
.
.
.
.
92
7
Hf-177
c A high-energy β particle and a small amount of electromagnetic radiation (γ-rays) are released.
162 a technetium b. atomic number 43 c. 43 protons and 43 electrons d. 10 mCi e. γ-rays
e Tc-99 The daughter nuclide is not metastable.
163 a atomic number 77 b. 77 protons 192 − 77 = 115 neutrons c. 192 → 192m
77 Ir 78 Pt 0
−1β
1 m 192 0
8 Pt → 78 Pt 0 γ
+
+ d. a thick lead apron
164 I-131 is probably responsible for thyroid cancer.
156
0
10
20
30
40
50
60
70
80
90
0 1 2 3 4 5 6 7
AMOUNT OF RADIOISOTOPE (G)
NUMBER OF HALF‐LIVES
8

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14 Chapter 3
Chapter 3
Ionic and Covalent Compounds
17 Caffeine is a compound.
18 When adenosine binds to the adenosine receptor, a signal is sent to the cell to slow its activity and
prepare for sleep.
19 Caffeine has a shape that is similar to adenosine, so it can also bind the receptor.
20 When caffeine binds to the adenosine receptor, the receptor cannot perform its normal signaling
function, and brain cells remain alert.
21 Epinephrine is the hormone produced in the fight-or-flight response.
22 dopamine
23 An element is made up of one type of atom. A compound is composed of two or more different
types of atoms.
24 The two types of chemical bonds are ionic and covalent bonds. Ionic bonds are formed when
valence electrons are transferred from one atom to another atom, whereas covalent bonds are
formed when valence electrons are shared between atoms.
25 Ionic compounds are formed when a metal atom transfers one or more valence electrons to a
nonmetal atom.
26 The two types of ions are monoatomic anions and monoatomic cations. Metals form monoatomic
anions.
27 A cation is positively charged; an anion is negatively charged. Metal elements form monatomic cations.
28 An ionic bond is formed between a monoatomic cation and a monoatomic anion.
29 An ionic bond is strong because opposite charges attract.
30 a. cation, one electron lost, Li+ b. anion, three electrons gained, P3−
c. anion, one electron gained, I− d. cation, five electrons lost, V 5+
31 a. cation, two electrons lost, Ca 2+ b. cation, two or three electrons lost, Cr 2+ or Cr 3+
c. anion, three electrons gained, N3– d. cation, one electron lost, Ag+
32 Group 8A elements have no partially filled energy levels. They are stable.
33
Atomic Number of Number of
Name of Ion Symbol Number Protons Electrons Charge
a. cesium ion Cs + 55 55 54 +1
b. silver ion Ag + 47 47 46 +1
c. chromium (III) ion Cr 3+ 24 24 21 +3
d. selenide ion Se 2– 34 34 36 −2
e. bromide ion Br – 35 35 36 −1

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Ionic and Covalent Compounds 15
34
Atomic Number of Number of
Name of Ion Symbol Number Protons Electrons Charge
a. Magnesium ion Mg 2+ 12 12 10 +2
b. Mercury (II) ion Hg 2+ 80 80 78 +2
c. Chloride ion Cl− 17 17 18 −1
d. Fluoride ion F− 9 9 10 −1
e. Oxide ion O2− 8 8 10 −2
35 a. K+, potassium ion, charge +1, Br−; bromide ion, charge −1 b. Mg2+, magnesium ion, charge
+2; Cl−, chloride ion, charge −1 c. K+, potassium ion, charge +1; I−, iodide ion, charge −1
d. Ba2+, barium cation, charge +2; Cl−, chloride ion, charge −1 e. Na+, sodium ion, charge +1; F−,
fluoride ion, charge −1
36 a. Na +, sodium ion, charge +1; O2−, oxide ion, charge −2 b. Cu 2+, copper (II) ion, charge +2;
O2−, oxide ion, charge −2 c. Ag +, silver ion, charge +1; Cl−, chloride ion, charge −1
d. Zn2+, zinc ion, charge +2; S2−, sulfide ion, charge −2 e. Ga 3+, gallium ion, charge +3; As3−,
arsenide ion, charge −3
37 a. LiI b. RbF c. CaBr2 d. BaI 2 e. CoCl 2 f. Al 2 3O
38 a. SrCl2 b. Cr2O3 c FeO d. ZnBr2 e. PtF4 f. Ag2O
.
.
.
39 a strontium oxide b. potassium iodide c. sodium iodide d. zinc chloride e. gallium oxide
40 a magnesium bromide b. lithium fluoride c. cesium chloride d. zinc oxide
e. silver iodide
41 b and d. Polyatomic ions are molecules that have lost or gained electrons, and there are covalent
bonds between the atoms in the polyatomic ion.
42 a. monatomic b. polyatomic c. monatomic d. polyatomic e. polyatomic
43 a. polyatomic b. polyatomic c. monatomic d. monatomic e. polyatomic
44 a. barium sulfate b. lithium carbonate c. magnesium sulfate
d. potassium dihydrogen phosphate e. sodium nitrite
45 a. calcium sulfate b. ammonium hydrogen carbonate c. aluminum carbonate
d. silver nitrate e. iron(III) oxide
46 b. potassium hydrogen phosphate
47 d.
48 a. Na 3 PO4 b. NH4 Cl c. Mg(OH) 2 d. NaHCO3
49 a. CaCO3 b. K2 HPO4 c. Ca(HCO3 ) 2 d. MgHPO4
50 Pb 3 (PO4 ) 2
51 Ca 3 (PO4 ) 2
52 When atoms come together to form a molecule, the valance energy levels are filled. This
arrangement is more stable than the isolated atoms as elements.
53 A molecule is a discrete entity composed of two or more nonmetal atoms held together by
covalent bonds.
Na 2 3CO

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Solution Manual For Essentials of General, Organic, and Biochemistry, 3rd Edition

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