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

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

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    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

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    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 V lead = 16.5 mL – 15.0 mL = 1.5 mL 77 V metal = 203.5 mL – 200. mL = 3.5 mL 78 Volume = 24 cm × 24 cm ×24 cm = 14,000 cm 3 = 14,000 mL 79 Volume = 5.21 cm × 5.21 cm × 5.21 cm = 141 cm 3 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 μ g 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 10 6 B 4 5 . × 10 2 μ g is larger. The microgram is a measure of mass.

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    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 cm 2 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 μ g ଵ 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 × 1 0 ଷ km 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 × 10 ହ 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଴ య ୫ = 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 cm ଷ × ଵ଴ షయ L ଵ ୡ୫ య = 0 .0143 L 105 a. b. 1 cm × ଵ଴ షమ ୫ ଵ 1 km × ଵ଴ య ୫ ଵ ୩୫ × ଵ ୫୫ ଵ଴ షయ ୫ = 1 × 1 0 ଺ mm ୡ୫ × ଵ ୫୫ ଵ଴ షయ ୫ = 10 mm c. 1 dm × ଵ଴ షభ ୫ ଵ ୢ ୫ × ଵ ୫୫ ଵ଴ షయ ୫ = 100 mm d . 1 nm × ଵ଴ షవ ୫ ଵ ୬୫ × ଵ ୫୫ ଵ଴ షయ ୫ = 1 × 1 0 ି ଺ mm

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    Matter, Energy, and Measurement 5 106 a . 1 g × ଵ ୩ ୥ ଵ଴ య ୥ = 1 × 1 0 ି ଷ kg b. 1 ng × ଵ଴ షవ ୥ ଵ ୬୥ × ଵ ୩୥ ଵ଴ య ୥ = 1 × 1 0 ି ଵଶ kg c. 100 mcg × ଵ଴ షల ୥ ଵ୫ୡ୥ × ଵ ୩୥ ଵ଴ య ୥ = 1 × 1 0 ି ଻ kg d. 10 μg × ଵ଴ షల ୥ ଵ μ୥ × ଵ ୩୥ ଵ଴ య ୥ = 1 × 10ି଼ kg 107 a. 5 mL × ଵ଴ షయ L ଵ ୫L × ଵ μL ଵ଴ షల L = 5 × 1 0 ଷ μL b. 0.5 L × ଵ μL ଵ଴ షల L = 5 × 1 0 ହ μL c. 250 cm ଷ × ଵ଴ షయ L ଵ ୡ୫ య × ଵ μL ଵ଴ షల L = 2.5 × 10 ହ μL d. 80 dL × ଵ଴ షభ L ଵ ୢ L × ଵ μ L ଵ଴ షల L = 8 × 1 0 ଺ μL 108 c. 150 μ g is equivalent to 1.5 ×10 − 7 kg. 109 density = ଽ.ଶଶ ୥ ଼ .଻ ୫L = 1 .1 g/mL 110 density = ଷ.଼ ୥ ଶ.଴ ୡ୫ య × ଵୡ୫ య 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 volum e = 2.3 m L 2.3 mL × ଵଽ.ଷଶ ୥ ଵ ୫L = 44 g 114 volume = (length of side) 3 volume = (2.20 cm) 3 volume = 10.6 cm 3 10.6 cm ଷ × ଵଽ.ଷଶ ୥ ଵୡ୫ య = 205 g 115 specific gr a vity = ଵ.଴ଶହ ୥/ ୫L ଵ.଴ ୥/୫L = 1.025 Yes, the specific gravity is within the normal range. 116 specific gr a vity = 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∙ୢୟ୷ ୢ ୟ୷ × ଵ ୫୥ = 6 0 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 cm 3 = 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 m L 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 cm 3 , 5,000 μ L 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 ୧ ୬ . = 6 . 4 c m volum e = length × width × height = 6.4 cm × 6.4 cm × 6.4 c m = 262 c m 3 mass = density × volume = 7.87 ୥ ୡ୫ య × 262 cm ଷ = 2 . 0 6 × 1 0 ଷ g 2.06 × 10 ଷ g × ଵ ୫୥ ଵ଴ షయ ୥ = 2 . 0 6 × 1 0 ଺ 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଴ షయ ୫ 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 cm 3 = 0.033 mL 149 volume = length × width × height = 147cm 3 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 8 O 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 → 81 Tl 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 − 1 β + b. The daughter nuclide is europium-153. 113 a. 32 32 0 15 P S → + 16 − 1 β b. The daughter nuclide is sulfur-32. 114 a. 26 26 0 11 Na → 12 Mg − 1 β + b. 232 228 4 81 Tl → 79 Au 2 α + 115 a. 225 221 4 89 Ac → 87 Fr 2 α + b. 107 107 0 46 Pd → 47 Ag − 1 β + 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 LD 50 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 LD 50 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 39 Y Z → + 40 r − 1 β Lu 177 177 0 71 → 72 Hf + − 1 β 161 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 → 192 m 77 Ir 78 Pt 0 − 1 β 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, P 3 − 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, N 3– 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 O 2 − 8 8 10 − 2 35 a. K + , potassium ion, charge +1, Br − ; bromide ion, charge − 1 b. Mg 2+ , magnesium ion, charge +2; Cl − , chloride ion, charge − 1 c. K + , potassium ion, charge +1; I − , iodide ion, charge − 1 d. Ba 2+ , 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; O 2 − , oxide ion, charge − 2 b. Cu 2+ , copper (II) ion, charge +2; O 2 − , oxide ion, charge − 2 c. Ag + , silver ion, charge +1; Cl − , chloride ion, charge − 1 d. Zn 2+ , zinc ion, charge +2; S 2 − , sulfide ion, charge − 2 e. Ga 3+ , gallium ion, charge +3; As 3 − , arsenide ion, charge − 3 37 a. LiI b. RbF c. CaBr 2 d. BaI 2 e. CoCl 2 f. Al 2 3 O 38 a. SrCl 2 b. Cr 2 O 3 c FeO d. ZnBr 2 e. PtF 4 f. Ag 2 O . . . 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 PO 4 b. NH 4 Cl c. Mg(OH) 2 d. NaHCO 3 49 a. CaCO 3 b. K 2 HPO 4 c. Ca(HCO 3 ) 2 d. MgHPO 4 50 Pb 3 (PO 4 ) 2 51 Ca 3 (PO 4 ) 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 3 CO

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