Solution Manual For Introductory Chemistry, 6th Edition

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iTABLE OFCONTENTSTable of Contents .................................................................................................................................... iChemActivity 1A: Atoms and Molecules .........................................................................................1ChemActivity 2A: Writing Numbers.................................................................................................2ChemActivity 2B: Units ........................................................................................................................4ChemActivity 2C: More with Conversions......................................................................................5ChemActivity 3A: Classifying Matter ...............................................................................................6ChemActivity 3B: Chemical Change .................................................................................................7ChemActivity 3C: Temperature and Heat ......................................................................................8ChemActivity 4A: Atoms and Elements (I) ....................................................................................9ChemActivity 4B: Atoms and Elements (II) ................................................................................ 10ChemActivity 4C: Ions, Isotopes, and Atomic Mass.................................................................. 11ChemActivity 5A: Combining Elements ....................................................................................... 13ChemActivity 5B: Types of Compounds....................................................................................... 14ChemActivity 5C: Naming Compounds ........................................................................................ 15ChemActivity 6A: Counting by Weighing .................................................................................... 17ChemActivity 6B: Counting by Weighing, Cont. ........................................................................ 18ChemActivity 6C: Mass Percent and Empirical Formula ....................................................... 19ChemActivity 7A: Chemical Equations......................................................................................... 20ChemActivity 7B: Solution Chemistry .......................................................................................... 22ChemActivity 7C: Classes of Chemical Reactions...................................................................... 24ChemActivity 8A: Pancakes and Molecules ................................................................................ 25ChemActivity 8B: How Much Can We Make?.............................................................................. 26ChemActivity 8C: Heat In or Heat Out? ........................................................................................ 27ChemActivity 9A: Waves and Light ............................................................................................... 28ChemActivity 9B: Orbits and Orbitals .......................................................................................... 29ChemActivity 9C: Electron Configurations ................................................................................. 30ChemActivity 9D: The Periodic Table .......................................................................................... 31ChemActivity 10A: Introduction to Bonding ............................................................................. 32ChemActivity 10B: Drawing Lewis Structures .......................................................................... 33

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iiChemActivity 10C: Molecular Shape and Polarity ................................................................... 34ChemActivity 11A: Pressure............................................................................................................ 35ChemActivity 11B: Gas Laws ........................................................................................................... 36ChemActivity 11C: Moles of Gas ..................................................................................................... 37ChemActivity 12A: Solids, Liquids, and Gases ........................................................................... 38ChemActivity 12B: Energetics of Boiling and Freezing .......................................................... 39ChemActivity 12C: Types of Intermolecular Forces................................................................ 40ChemActivity 13A: Solutions........................................................................................................... 41ChemActivity 13B: Concentration ................................................................................................. 42ChemActivity 13C: How is a Solution Different?....................................................................... 43ChemActivity 14A: Acids and Bases.............................................................................................. 44ChemActivity 14B: Chemistry of Acids and Bases.................................................................... 45ChemActivity 14C: Strong and Weak Acids and Bases ........................................................... 46ChemActivity 14D: pH and Buffers................................................................................................ 47ChemActivity 15A: Dynamic Equilibrium ................................................................................... 49ChemActivity 15B: Le Châtelier’s Principle ............................................................................... 51ChemActivity 15C: Solubility Products and Catalysts............................................................. 52ChemActivity 16A: Oxidation and Reduction ............................................................................ 53ChemActivity 16B: Balancing Redox Equations........................................................................ 55ChemActivity 16C: Electrochemical Cells ................................................................................... 58ChemActivity 17A: Nuclear Reactions.......................................................................................... 59ChemActivity 17B: Decay and Time.............................................................................................. 60ChemActivity 18A: Alkanes ............................................................................................................. 61ChemActivity 18B: Alkenes and Alkynes .................................................................................... 62ChemActivity 18C: Functional Groups ......................................................................................... 64ChemActivity 19A: Carbohydrates and Lipids .......................................................................... 65ChemActivity 19B: Proteins and DNA .......................................................................................... 66

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1CHEMACTIVITY1A:ATOMS ANDMOLECULESANSWERS TOCRITICALTHINKINGQUESTIONS1.22.23.Only one circle4.More than one atom5.They have different atoms, They have different numbers of atoms, etc.6.A molecule is composed of two or more atoms.7.An observation8.No-‐-‐-‐laws are very general9.Yes. One could observe something that contradicts a law and show that it is invalid.10.A law summarizes a large number of observations.11.Boyle’s law12.The law of conservation of mass13.Theories explain why laws are true.14.No. Laws summarize observations and theories explain laws.

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2CHEMACTIVITY2A:WRITINGNUMBERSANSWERS TOCRITICALTHINKINGQUESTIONS1.Statement 12.Statement 23.The one saying Statement 2. This scientist communicated more precision with moredigits.4.Statement 35.0.6 °C6.Their level of certainty. (The precision.)7.38.1039.310.10-‐311.The number of factors of 10 or 1/1012.In the boxes starting in the top left blank…a.10·∙10·∙10·∙10·∙10·∙10b.106c.(1/10)·∙ (1/10)·∙ (1/10)·∙ (1/10)·∙ (1/10)·∙ (1/10)·∙ (1/10)d.10-‐713.598314.5983 = 5.983 × 100015.316.0.00034 =3.4÷ 10000 =3.4× (1/10) ×(1/10) ×(1/10) ×(1/10) =3.4× 10-‐417.a.Write the number as a number between 1 and 10b.Determine how many factors of 10 or 1/10 are needed to make the number thesame as the originalc.Write those factors of 10 or 1/10 as the number 10 raised to an exponent18.1; 519.3; 5.0020.1; 50021.When a trailing zero is after a decimal point it is significant.22.2; 0.005123.Leading zeros are not significant24.4; 5.00325.1) after a decimal point, 2) between non-‐zero digits26.Whether the zeros are significant or not27.Scientific notation28.(see answer in model)29.(see table)

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35.02× 89.665× 0.10= 45.01183=45(final answer)3522significant figures2320# digits after dec. pt.s.f.# digits afterdecimal pt.1.743211.823164+12.6515326.2141Final Answer26.214230.number of significant figures31.number of decimal places

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4CHEMACTIVITY2B:UNITSANSWERS TOCRITICALTHINKINGQUESTIONS1.m, kg, K2.kg3.False. kg is a base unit, and it has a prefix.4.(answers will vary)5.m; c; M; n; G6.mg; nm; ps; dm; μK7.2.548.19.1 because the numerator and denominator are equal10.111.no12.no; you are multiplying by 113.yes; 26.2 cm14.We wanted to cancel in and keep cm15.1) The top and bottom are equal; 2) The units you want are on the top and the units youwant to cancel are on the bottom.

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5CHEMACTIVITY2C:MORE WITHCONVERSIONSANSWERS TOCRITICALTHINKINGQUESTIONS1.12.No3.5.4ft×12in𝟏𝐟𝐭×𝟐.𝟓𝟒𝐜𝐦1in=𝟏𝟔𝟎cm4.in ; m5.3 ft/1 yd; 12 in/1 ft; 2.54 cm/1 in; 0.01 m/1 cm; 1 km/1000m6.100 yd×(3 ft/1 yd)×( 12 in/1 ft)×(2.54 cm/1 in)×(0.01 m/1 cm)×(1 km/1000m)=0.0914 km7.A solution map shows the order in which units will be changed, starting with the unitsgiven and ending with the desired units.8.yes; no9.m310.m/s11.kg/m312.0.1 m13.0.00114.no15.no; 4.5 g = 1 cm316.(1 cm3/4.5 g) and (4.5 g/1 cm3)17.1590 g × (1 cm3/4.5 g) = 350 cm318.1.0019.1.00 in320.2.54 cm21.2.54 cm22.(2.54 cm)3= 16.4 cm323.16.424.Circle both:!in!.!"cm!!in!!".!cm!25.1026.27.(1 m/10 dm)3= 1 m3/1000 dm = 1 m3/1000 L28.5 m × 8 m × 3 m = 120 m329.120 m3× (1000 L/1 m3) = 1.2×105L

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6CHEMACTIVITY3A:CLASSIFYINGMATTERANSWERS TOCRITICALTHINKINGQUESTIONS1.No2.No3.Yes (a little)4.gas5.Something is compressible if it can be made smaller by squeezing it.6.stay about the same7.a lot bigger8.gas9.Solid and liquid. Because the gas is much bigger but the same amount of solid and liquidare about the same size.10.liquid and gas11.Because solids don’t flow, the molecules must not be free to move around each other.12.Similar to Fig. 3.4 inIntroductory Chemistry13.copper pipe14.copper pipe, sugar15.copper pipe, sugar16.No. Sugar has more than one element, but they are all in one molecule.17.sugar; yes, in the tea contents, etc.18.tea and vinaigrette dressing19.Answers will vary. (E.g.The vinaigrette dressing has oil on top and water on the bottom.It also has other stuff in it.)20.tea; dressing21.Answers will vary

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7CHEMACTIVITY3B:CHEMICALCHANGEANSWERS TOCRITICALTHINKINGQUESTIONS1.physical2.physical3.physical; melting point is listed in the table as physical, and boiling is a similar process4.chemical5.Chemical properties refer to reactivity, while physical properties do not.6.physical7.no8.chemical9.yes10.In chemical change a new compound is formed.11.chemical; a new compound is formed12.58 g butane, 208 g oxygen13.176 g carbon dioxide; 90 g water14.266 g15.266 g16.the compounds present17.the mass18.4.18419.418420.3.60×10621.J < cal < Cal < kWh22.(4.184 J/1 cal)23.115 Cal × (1000 cal/1 Cal) × (4.184 J/1 cal) = 4.31×105J24.Energy moves from the car to the air as heat.25.reactants26.given off27.given off28.absorbing29.the product it goes uphill by absorbing energy30.Similar to the second part of figure 3.16 inIntroductory Chemistry

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8CHEMACTIVITY3C:TEMPERATURE ANDHEATANSWERS TOCRITICALTHINKINGQUESTIONS1.180 °2.100 °3.100 °4.Celsius and Kelvin5.A degree Celsius because there are fewer of them between freezing and boiling, so eachone must be bigger6.Yes, they are just shifted by 2737.K = °C + 273.15 = 100 + 273.15 = 373.15 °C. Yes, it is consistent.8.°C = (°F-‐32)/1.89.(212 °F-‐32)/1.8 = 100 °C10.(70 °F -‐32)/1.8 = 21.1 °C11.°F = 1.8 ×°C + 3212.(1.8)(21.1) + 32 = 69.98 °F13.Twice as much material should take twice as much heat. 4.184 × 2 = 8.368 J14.Temperature change is 17 times greater, so it should take 17 times as much heat 4.184 ×17 = 71.13 J15.Both have doubled so it should take four times as much heat 4.184 × 2 × 2 = 16.74 J16.37 times the temperature and 250 times the amount… 4.184 × 37 × 250 = 38.7 kJ17.q;m;C; ΔT18.4.184 J/g °C19.q = (2 g)(4.184 J/g °C)(2 °C) = 16.74 J20.yes21.yes22.q = (2 g)(0.903 J/g °C)(2 °C) = 3.612 J23.aluminium; it takes less heat to warm it by 1 °C, so the same amount of heat will warm itmore24.It is the ability of a substance to absorb heat without changing temperature.

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9CHEMACTIVITY4A:ATOMS ANDELEMENTS(I)ANSWERS TOCRITICALTHINKINGQUESTIONS1.It seems continuous. No matter how small of a drop, it is still water.2.Greek philosophers3.atoms4.John Dalton5.Atoms are indivisible. There is no such thing as “half an oxygen atom”.6.Water is formed when one oxygen atom combines with two hydrogen atoms.7.No. It will go through the paper.8.It will go out the back of the room.9.There must be a wooden rod in that room.10.Throw lots of balls into each room. If any come back, that room must be the one withthe wooden rods.11.evenly distributed12.More like tissue paper because it is evenly distributed across the room.13.alpha particles14.Most pass through with no deflection15.No. A few are deflected at large angles.16.More like wooden rods because some particles bounced back.17.Rutherford proposed a model for the atom in which the matter is distributed in a fewsmall concentrated locations.18.proton and neutron19.electron20.1.0073 amu/0.00055 amu= 1831 (electrons per proton are the actual units for this)21.proton and electron22.one23.They are the same because the cancel each other out24.protons and neutrons

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10CHEMACTIVITY4B:ATOMS ANDELEMENTS(II)ANSWERS TOCRITICALTHINKINGQUESTIONS1.Si2.P3.K4.Some symbols are clearly abbreviations, but not all.5.No. They are not capitalized in CTQ 1-‐3 above.6.The first letter in a symbol is capitalized. If there is another letter, it is not capitalized.7.Antimony8.14; 799.The number of protons is in the periodic table above the symbol.10.19; 5111.oxygen12.proton13.This must be nitrogen, not carbon, because the number of protons determines theidentity of the element.14.See Fig. 4.12 in Introductory Chemistry15.Metals. See Fig. 4.12 in Introductory Chemistry16.See Fig. 4.12 in Introductory Chemistry17.See Fig. 4.12 in Introductory Chemistry18.See the figure on p. 104 of Introductory Chemistry19.a.rubidium: alkali metalsb.vanadium: transition metalc.bromine: halogend.neon: noble gase.strontium: alkaline earth metal

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11CHEMACTIVITY4C:IONS,ISOTOPES,ANDATOMICMASSANSWERS TOCRITICALTHINKINGQUESTIONS1.12; 122.+123.-‐104.There are two more protons than electrons, so the total charge is 2+.5.96.It must have the same number of electrons as protons: 9.7.98.It must have one more electron than protons: 10.9.Neutral atoms have the same number of protons and electrons. Ions have unequalnumber.10.An ion is an atom with an unequal number of protons and electrons, and therefore anon-‐zero charge.11.A superscript to the right of the symbol.12.Ion charge =NP-‐Ne13.The charge is 1+. The symbol is Na+.14.Li+15.K+16.Na+17.O2-‐, F-‐, Mg2+18.(add Ne to the right of F)19.1020.1021.They are the same22.1023.They are the same24.Ions have the charges they do because atoms tend to form ions with the same numberof electrons as the nearest noble gas.25.626.1 amu27.If it had more protons, it would not be carbon but some other element.28.Electrons have so little mass that more electrons would not make a significantdifference.29.the neutron!30.6 amu31.632.733.1,00034.11,868 amu

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1235.143 amu36.12,011 amu37.12.011 amu38.Yes. It is under the symbol for carbon.39.It means that the average of all the atoms is 35.45 amu. It may be that no atoms weighexactly this amount.

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13CHEMACTIVITY5A:COMBININGELEMENTSANSWERS TOCRITICALTHINKINGQUESTIONS1.(answers in table)2.Total = 4.5; Ratios both = 8.03.mass of H, mass of O, total mass4.The ratio mass O/mass H5.80 g6.2 Hs, 1 O7.H2O8.No. The 2 should be subscript.9.hydrogen peroxide, H2O210.Hydrogen peroxide has two atoms of oxygen and water has only one.11.112.Yes. One of each and no subscripts.13.CO214.12 Cs, 22 Hs, 11 Os15.116.217.subscript 218.219.subscript 220.O and H are in parentheses. The 2 applies to both.21.222.623.224.Yes. The subscript on the parentheses.25.Parentheses indicate a group of atoms that can all be multiplied by a subscript.26.8 Two NH4units with four H atoms in each unit. 2x4=8.27.500: one for each H28.Only the ratio of atoms29.H2O230.2 Hs, 2 Os31.Yes. There is one H for each O in the compound.32.HO correctly communicates the ratio of atoms in the compound, but it does notcommunicate the actual number of atoms in one molecule. H2O2also says how manyatoms are in one molecule.33.CH2O

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