Introduction To General, Organic And Biochemistry, 11th Edition Solution Manual

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Chapter 1: Matter, Energy, and Measurement1.1Multiplication:(a) 4.69105(b) 2.810-15Division:(a) 1.941018(b) 1.371051.2(a)oF = 95oC + 32 = 95 64.0oC + 32 = 147oF(b)oC = 59 (oF - 32) = 59 (47oF - 32) = 8.3oC1.38.55 mi1.609 km1 mi= 13.8 km1.4332 ms1 km1000 m1 mi1.609 km60 s1 min60 min1 hr= 743 mi/hr1.51.61.7d = m/V =56.8 g23.4 mL = 2.43 g/mL1.8The specific gravity of a substance is the density of this substance divided by the density ofwater, which is 1.000 g/mL.1.9Amount of heat = SHm(T2-T1) = 1.0 calggoC731 g()74−8()oC = 4.8104cal

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Chapter 1: Matter, Energy, and Measurement1.10100 g of iron may have been measured to one, two, or three significant figures (thezeros at the end of a number without a decimal point are called trailing zeros, areambiguous and may or may not be significant).If 100 g implied two or threesignificant figures, T2will be 46oC (the number of significant figures is determined bythe specific heat of iron, which is reported to two significant figures).One commonway to show that trailing zeros are significant is to place a decimal point after thezeros, for example 100. g (three significant figures).Zeros between a decimal and anon-zero digit are significant figures.This method is used often in the textbookproblems.The context of the problem suggests 100. g, therefore the solution willassume 100 g of iron was measured to three significant figures(100. g of iron).(T2-T1)oC = 21oCT2= 21oC + 25oC = 46oC1.11SH = Amount of heatm(T2-T1)=88.2 cal(13.4 g)(176-23)oC = 0.0430 cal / goC1.12A major reason for the increase of the average life expectancy of humans in the last 80years has been great progresses in medical science.Diseases that were once fatal haveeither been eradicated or cures developed.The causes and cures for many major diseasesare now better understood and treatments more effective.1.14Metals have low specific heats and organic compounds have higher specific heats.1.16(a)Chemical change: burning gasoline is converted to carbon dioxide and water.(b)Physical change:ice forming from liquid water is still H2O, just a different state ofmatter.(c)Physical change: boiling oil is still oil, just a different state of matter.(d)Physical change: melting lead remains lead, just a different state of matter.(e)Chemical change: elemental Fe has been converted to rust, Fe2O3.(f)Chemical change: nitrogen and hydrogen converted ammonia, NH3, involves a changein chemical composition.(g)Chemical change:the chemical components in food are converted to energy, carbondioxide, and water thus changing chemical composition.1.18(a) 403,000(b) 3,200(c) 0.0000713(d) 0.0000000005551.20(a) 2.101013(b) 1.07104(c) 2.9310-12(d) 8.4101(e) 1.3610-261.22(a) 7.74103(b) 8.80810-2(c) 1.3022102

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Chapter 1: Matter, Energy, and Measurement1.243.2510-101.26(a) 3(b) 2(c) 1(d) 4(e) 51.28(a) 2.5104(b) 4.1(c) 15.51.30(a) 10963.1(b) 244(c) 172.341.32(a) 1 kg = 1000 g(b) 1 mg = 0.001 g1.34(a) 100 cm(b) 230 mL(c) 75 kg(d) 15 mL(e) 50 mg(f)100 mm(g) 40 g1.36Temperature conversions:oC = 59 (oF - 32)andK = 273 +oC(a)59 (320oF - 32) = 160oC and 273 + 160oC = 433 K(b)59 (212oF - 32) = 100oC and 273 + 100oC = 373 K(c)59 (0oF - 32) = -18oC and 273 + (-18)oC = 255 K(d)59 (-250oF - 32) = -157oC and 273 + (-157)oC = 116 K1.38Unit conversions:(a) 42.6 kg2.205 lb1 kg= 93.9 lb(b) 1.62 lb453.6 g1 lb= 735 g(c) 34 in2.54 cm1 in= 86 cm(d) 37.2 km1 mi1.609 km= 23.1 mi(e) 2.73 gal3.785 L1 gal= 10.3 L(f) 62 g1 oz28.35 g= 2.2 oz(g) 33.61 qt1 L1.057 qt= 31.80 L(h) 43.7 L1 gal3.785 L= 11.5 gal(i) 1.1 mi1.609 km1 mi= 1.8 km(j) 34.9 mL1 fl oz29.57 mL= 1.18 fl oz1.40First, convert one of the bottle's units to the other.

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Chapter 1: Matter, Energy, and Measurement, which is less than 300. cc bottle1.42The key here is to first convert speed from mph to kph.Yes, you would reach Ottawawithin an hour.1.441.461.481.501.52combined volumes of IV solutions = 4102mL (rounded to one significant figure)1.54At low temperatures, most substances exist as solids.

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Chapter 1: Matter, Energy, and Measurement1.561.581.60Answer rounded to two significant figures:1.62(a)The densities of O2and CO2can be calculated as follows:dO2=10.00 g O26702 mL O21000 mL O21 L O2= 1.492 g/LdCO2=10.00 g CO25058 mL CO21000 mL CO21 L CO2= 1.977 g/L(b)Carbon dioxide (a gas that does not support combustion), being denser than oxygen,will sink to the level of the fire and temporarily displace the oxygen above it.Bycutting off the supply of oxygen (a fuel for the fire), the fire will be extinguished.1.64Matter-energy can neither be created nor destroyed (law of conservation of energy), solarpanels work by converting light energy into electrical energy.1.66

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Chapter 1: Matter, Energy, and Measurement1.681.70Assuming that the 200 lb man is measured to three significant figures:1.72Shivering generates heat for the body through muscular action.1.74(a) Volume(b) Volume(c) Mass(d) Energy(e) Density(f) Energy(g) Temperature(h) Velocity1.76Vroom= length x height x width = (5.3 m)(2.0 m)(4.2 m) = 45 m3mair= dairVair=1.2510-3gcm3(45 m3)100 cm1 m31 kg1000 g= 56 kg air1.78KE = 1/2(mv2)1.80Convert dollars/L into dollars/gal, then compare:Gasoline is less expensive in Potsdam ($3.93/gal) than in Montreal ($4.62/gal).

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Chapter 1: Matter, Energy, and Measurement1.82(a)Astronauts weigh less on the moon because of the moon’s reduced gravity will causethe astronaut to exert less force (weight) on the moon’s surface.(b)No, their masses were not different. Mass is independent of gravity, whereas weight isthe force that an object’s mass exerts on a surface under the influence of gravity.1.84Convert each quantity to a common unit, then compare:1.86In this problem, it is reasonable to assume that 100 g is measured to three significantfigures and that temperature is measured to two significant figures.(a)The heat required to raise the temperature of a substance is directly proportional to thespecific heat of that substance.Mercury, having the lowest specific heat, will requirethe least amount of energy to heat 100 g by 10oC.(b)If the heats and masses are equal, the combined equations can be expressed as:(c)If the heats andT are equal, the combined equations can be expressed as:SHunkmunk= SHFemFeidentify element by solving for SHunkSHunk= SHFemFemunk=0.107 cal/goC()1.6 g()1 g= 0.17 cal/goCThe unknown element is graphite1.88Compare products using common units.

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Chapter 1: Matter, Energy, and MeasurementMilk purchased by the quart ($0.80/qt) is a better buy than milk bought by the liter($0.81/qt).1.90Convert the quantities to common units (miles/hour) and then compare.The velocityexpressed in choice (c) is the fastest.(a)70 miles/hr(b)140 kmhr1 mi1.609 km= 87 mi/hr(c)4.5 kms1 mi1.609 km60 s1min60 minhr= 1.0104mi/hr(d)48 mimin60 minhr= 2.9103mi/hr1.92No, the solar cell cannot produce enough energy. First solve the problem quantitatively byconverting the solar cell energy production to kcal/hour for easy comparison. This revealsthat the solar cell only produces 1.20 x 102kcal/hr of energy, which is not enough tomaintain a temperature of 4oC in the refrigerator (250. kcal/hr required).1.94All of the substances in coffee are chemicals, including the water, caffeine, and the tracechemicals responsible for the coffee’s flavor.1.96You should purchase the 200. grams of cheese. Qualitatively, we can compare the massesof cheese with the masses of common items. The average mass of a human is about 70 kg;therefore, 200. kg of cheese is a lot of cheese.A single aspirin tablet contains 325 mg ofacetylsalicylic acid active ingredient; therefore, 200. mg of cheese would not even cover aslice of bread. A loaf of bread has a mass of about 500-600 grams, therefore, 200. grams ofcheese is a reasonable amount to compliment a loaf of bread.1.98Hydrometers measure the specific gravity of liquids.By comparing the hydrometerreadingofanunknownconcentrationofantifreezesolutionandcomparingitwithhydrometer readings from antifreeze solutions of standard concentrations, the unknownantifreeze concentration can be determined.

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Chapter 1: Matter, Energy, and Measurement1.100Aspirin tablets that contain 325 mg of aspirin contain more aspirin than 81 mg tablets.The 325 mg dose of aspirin is usually taken for pain, while the 81 mg daily dose of aspirinis usually taken to help prevent heart attacks.1.102Water reaches its maximum density at 4oC, therefore freshwater lakes freeze from the topon down.1.104First, it is important to know exactly what the treatment involves and the mechanism ofaction.Also, did the study compare the treatment group with a control group consistingof ear infection patients that didn’t receive the treatment?Finally, did the scientist testthe treatment for safety?1.106The quantity of a solid is most easily measured by its mass; therefore, the mass of urea ismeasured using a balance.The quantity of a liquid is easily measured by its volume ormass.The volume of pure ethanol can be measured using a volumetric pipette or agraduated cylinder.The advantage of measuring the volume of ethanol is that the massof ethanol can be calculated using its volume and density.1.108The molecular structure and arrangement of atoms in chemical substances are importantto their reactivity and biological activity.New medications are going to mimic naturalmolecules involved in biochemical processes, therefore, the new medicines would beexpected to have similar characteristics to the natural biomolecules that are comparable inmolecular structure and atomic arrangement.1.1101.112(a) Dose (in milligrams) of Tylenol calculated to two significant figures:(b) Dose in milliliters of Tylenol solution calculated to two significant figures:

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Chapter 2: Atoms2.1(a)NaClO3(b) AlF32.2(a)The mass number is 15 + 16 = 31.(b)The mass number is 86 + 136 = 222.2.3(a)The element has 15 protons, making it phosphorus (P); its symbol is.(b)The element has 86 protons, making it radon (Rn); its symbol is.2.4(a)The atomic number of mercury (Hg) is 80; that of lead (Pb) is 82.(b)An atom of Hg has 80 protons; an atom of Pb has 82 protons.(c)The mass number of this isotope of Hg is 80 + 120 = 200; the mass number for thisisotope of Pb is 82 + 120 = 202.(d)The symbols of these isotopes areand.2.5The atomic number of iodine (I) is 53. The number of neutrons in each isotope is 125-53= 72 for iodine-125 and 131-53 = 78 for iodine-131. The symbols for these two isotopesareand.2.6The atomic weight is 6.941 amu, which is nearer to 7 amu than 6 amu. Therefore, lithium-7 is the more abundant isotope. The relative abundances for these two isotopes are 92.50percent for lithium-7 and 7.50 percent for lithium-6.2.7This element has 13 electrons and, therefore, 13 protons. The element with atomic number13 is Aluminum (Al).2.8Both Democritus and Dalton believed that matter was composed of tiny indivisibleparticles referred to as atoms. The major difference between Democritus and Dalton is thatDalton based his theory on evidence rather than belief.2.10(a)Oxygen-an element(b)Table salt-a compound(c)Sea water-a mixture(d)Wine-a mixture(e)Air-a mixture(f)Silver-an element(g)Diamond-an element(h)A pebble-a mixture(i)Gasoline-a mixture(j)Milk-a mixture(k)Carbon dioxide-a compound(l)Bronze-a mixture

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Chapter 2: Atoms2.12Given here is the element, its symbol, and its atomic number:(a)Bohrium (Bh, 107)(b)Curium (Cm, 96)(c)Einsteinium (Es, 99)(d)Fermium (Fm, 100)(e)Lawrencium (Lr, 103)(f)Meitnerium (Mt, 109)(g)Mendelevium (Md, 101)(h)Nobelium (No, 102)(i)Rutherfordium (Rf, 104)(j)Seaborgium (Sg, 106)2.14The three elements named for planets are mercury (Hg, 80), uranium (U, 92), andneptunium (Np, 93).2.16(a) NaHCO3(b) C2H6O(c) KMnO42.18The law of conservation of mass2.20Mass percent of H and O in:H2O:18.015 g/molH: 11.2%O: 88.8%H2O2:34.014 g/molH:5.9%O: 94.1%2.22(a)Protons are located in the nucleus.(b)Electrons are outside the nucleus.(c)Neutrons are in the nucleus.2.24(a)Mass number = 22 protons + 26 neutrons = 48(b)Mass number = 76 protons + 114 neutrons = 190(c)Mass number = 34 protons + 45 neutrons = 79(d)Mass number = 94 protons + 150 neutrons = 2442.26An element is identified by its atomic number, which is mass number-number of neutrons.(a)45-24 = 21 protons. The element is scandium (Sc), and its symbol is.(b)48-26 = 22 protons. The element is titanium (Ti), and its symbol is.(c)107-60 = 47 protons. The element is silver (Ag), and its symbol is.(d)246-156 = 90 protons. The element is thorium (Th) and its symbol is.(e)36-18 = 18 protons. The element is argon (Ar) and its symbol is.2.28The number of neutrons is equal to the mass number-atomic number (number of protons).(a) 13-6 = 7 neutrons(b) 73-32 = 41 neutrons(c) 188-76 = 112 neutrons(d) 195-78 = 117 neutrons

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Chapter 2: Atoms2.30(a)Neon-22 has 10 protons and 22-10 = 12 neutrons(b)Palladium-104 has 46 protons and 104-46 = 58 neutrons(c)Chlorine-35 has 17 protons and 35-17 = 18 neutrons(d)Tellurium-128 has 52 protons and 128-52 = 76 neutrons(e)Lithium-7 has 3 protons and 7-3 = 4 neutrons(f)Uranium-238 has 92 protons and 238-92 = 146 neutrons2.32The atomic number is the number of protons in the nucleus of an element. The massnumber is the number of protons and neutrons in the nucleus.2.34The atomic weight (121.75 amu) is nearer to that of antimony-121 (120.90 amu) than it isto antimony-123 (122.90 amu). Therefore, antimony-121 has the greater naturalabundance. The observed abundances are 57.3 percent antimony-121, and 42.7 percentantimony-123.2.36Carbon-14 has 6 protons, 6 electrons, and 8 neutrons.2.38Fluorine-18 has 9 protons, 9 electrons, and 9 neutrons.Nitrogen-13 has 7 protons, 7 electrons, and 6 neutrons.Oxygen-15 has 8 protons, 8 electrons, and 7 neutrons.2.40Rubidium-87 has 37 protons, 37 electrons, and 50 neutrons.Strontium-87 has 38 protons, 38 electrons, and 49 neutrons.2.42In period 3, there are three metals (Na, Mg, and Al), one metalloid (Si) and four nonmetals(P, S, Cl, and Ar).2.44Periods 1-3 contain more nonmetals than metals. Periods 4-7 contain more metals thannonmetals.2.46Palladium (Pd), cobalt (Co), and chromium (Cr) are transition elements. Cerium (Ce) is aninner transition element; K and Br are main group elements.2.48(a)Argon is a nonmetal(b)Boron is a metalloid(c)Lead is a metal(d)Arsenic is a metalloid(e)Potassium is a metal(f)Silicon is a metalloid(g)Iodine is a nonmetal(h)Antimony is a metalloid(i)Vanadium is a metal(j)Sulfur is a nonmetal(k)Nitrogen is a nonmetal

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Chapter 2: Atoms2.50Only Period 1 has two elements. Periods 2 and 3 have eight elements. Periods 4 and 5have 18 elements and Period 6 has 32 elements. Period 7 is filling with recently discoveredelements, and upon confirmation, will contain its full capacity of 32 elements.2.52The group number tells the number of Lewis dots to be placed around the symbol of theelement.(a)(b)(c)(d)(e)(f)CSiOSAlBr:: :::::::..:.. ......2.54Following are Lewis dot structures for each element in Problem 2.49:(a)(b)(c)(d)(e)LiN eC..::Be: .Mg::::2.56Following are Lewis dot structures for each element in Problem 2.55:(a)(b)(c)(d)(e)N aP.Cl:.: .H e:.::.H.2.58In the ground state, 3sand 3porbitals are occupied by four valence electrons.2.60(a)Rb(37): 1s22s22p63s23p64s23d104p65s1(b)Sr(38): 1s22s22p63s23p64s23d104p65s2(c)Br(35): 1s22s22p63s23p64s23d104p52.62The properties are similar because all of them have the same outer-shell electronconfiguration. They are not identical because each has a different number of filled innershells.2.64Going from left to right within a period, increasing positive charge holds onto the outerelectrons more tightly, thus decreasing the atomic radius and increasing the ionizationenergy. So, for the following atoms B, C, and N:(a)Boron has the largest atomic radius.(b)Nitrogen has the smallest atomic radius.(c)Nitrogen has the largest ionization energy.(d)Boron has the lowest ionization energy.2.66Ionization energy generally increases from left to right within a period in the PeriodicTable and from bottom to top within a column:(a) K < Na < Li(b) C < N < Ne(c) C < O < F(d) Br < Cl < F

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Chapter 2: Atoms2.68Following are the ground-state electron configurations of Mg atom, Mg+, Mg2+, and Mg3+.The first electron is removed from the 3s orbital. The removal of each subsequent electronrequires more energy because, after the first electron is removed, each subsequent electronis removed from a positive ion, which strongly attracts the remaining electrons. The thirdionization energy is especially large because the electron is removed from the filled secondprincipal energy level, meaning that it is removed from an ion that has the same electronconfiguration as neon.2.70The most abundant elements by weight (a) in the Earth's crust are oxygen and silicon, and(b) in the human body they are oxygen and carbon.2.72Bronze is an alloy of copper and tin.2.74(a) 1s(b) 2s, 2p(c) 3s, 3p, 3d(d) 4s, 4p, 4d, 4f2.76(a)The atomic radius decreases going from left to right across a period in the PeriodicTable. Although the principal quantum number of the outermost orbital remains thesame, as each successive electron is added, the nuclear charge also increases by theaddition of one proton. The resulting increased attraction between nucleus andelectrons is somewhat stronger than the increasing repulsion between electrons, whichcauses the atomic radius to decrease.(b)To pull a valence electron from an atom, energy is required to overcome the attractiveforces on the electron from the positively charged nucleus.2.78(a)s2p1(b)s2p5(c)s2p3

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Chapter 2: Atoms2.80(a)Carbon-12 has 6 protons and 6 neutrons. Neutrons contribute 50% of its mass.(b)Calcium-40 has 20 protons and 20 neutrons. Neutrons contribute 50% of its mass.(c)Iron-55 has 26 protons and 29 neutrons. Neutrons contribute 53% of its mass.(d)Bromine-79 has 35 protons and 44 neutrons. Neutrons contribute 56% of its mass.(e)Platinum-195 has 78 protons and 117 neutrons. Neutrons contribute 60% of its mass.(f)Uranium-238 has 92 protons and 146 neutrons. Neutrons contribute 61% of its mass.2.82(a) P(b) K(c) Na(d) N(e) Br(f) Ag(g) Ca(h) C(i) Sn(j) Zn2.84(a)Silicon is in Group 4A. It has four outer-shell electrons.(b)Bromine is in Group 7A. It has seven outer-shell electrons.(c)Phosphorus is in Group 5A. It has five outer-shell electrons.(d)Potassium is in Group 1A. It has one outer-shell electron.(e)Helium is in Group 8A. It has two outer-shell electrons.(f)Calcium is in Group 2A. It has two outer-shell electrons.(g)Krypton is in Group 8A. It has eight outer-shell electrons.(h)Lead is in Group 4A. It has four outer-shell electrons.(i)Selenium is in Group 6A. It has six outer-shell electrons.(j)Oxygen is in Group 6A. It has six outer-shell electrons.2.86(a)An electron has a charge of-1, a proton a charge of +1, and a neutron has no charge.(b)An electron has a mass of 0.0005 amu; both protons and neutrons have masses of 1amu.2.88Xenon (Xe) will have the highest ionization energy. Ionization energy increases from leftto right going across the periodic table.2.90Going from left to right across a period in the Periodic Table, protons are being added tothe nucleus and electrons are added to the valence shell. For elements in the same period,the principal energy level remains the same (for example, the valence electrons of allsecond period elements occupy the second principal energy level). But in going from oneelement to the next across a period, one more proton is added to the nucleus, thusincreasing the nuclear charge by one unit for each step from left to right. The result is thatthe nucleus exerts an increasingly stronger pull on the valence electrons and atomic radiusdecreases.2.92The O2-has a larger radius than F and F-for several reasons. The most important beingthat O2-has two (-) charged electrons in excess of the positively charged nucleus. Thisincreases the amount of electron-electron repulsions, expanding the electron cloud relativeto F and F-. Another factor is that oxygen is less electronegative than fluorine, therefore,oxygen holds on to its electrons less tightly.

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