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Solution Manual For Introductory Chemistry, 6th Edition

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

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

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    1 C HEM A CTIVITY 1A: A TOMS AND M OLECULES A NSWERS TO C RITICAL T HINKING Q UESTIONS 1. 2 2. 2 3. Only one circle 4. More than one atom 5. They have different atoms, They have different numbers of atoms, etc. 6. A molecule is composed of two or more atoms. 7. An observation 8. No-­‐-­‐-­‐laws are very general 9. 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 law 12. The law of conservation of mass 13. Theories explain why laws are true. 14. No. Laws summarize observations and theories explain laws.

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    2 C HEM A CTIVITY 2A: W RITING N UMBERS A NSWERS TO C RITICAL T HINKING Q UESTIONS 1. Statement 1 2. Statement 2 3. The one saying Statement 2. This scientist communicated more precision with more digits. 4. Statement 3 5. 0.6 °C 6. Their level of certainty. (The precision.) 7. 3 8. 10 3 9. 3 10. 10 -­‐3 11. The number of factors of 10 or 1/10 12. In the boxes starting in the top left blank… a. 10·∙10·∙10·∙10·∙10·∙10 b. 10 6 c. (1/10)·∙ (1/10)·∙ (1/10)·∙ (1/10)·∙ (1/10)·∙ (1/10)·∙ (1/10) d. 10 -­‐7 13. 5983 14. 5983 = 5.983 × 1000 15. 3 16. 0.00034 = 3.4 ÷ 10000 = 3.4 × (1/10) ×(1/10) ×(1/10) ×(1/10) = 3.4 × 10 -­‐4 17. a. Write the number as a number between 1 and 10 b. Determine how many factors of 10 or 1/10 are needed to make the number the same as the original c. Write those factors of 10 or 1/10 as the number 10 raised to an exponent 18. 1; 5 19. 3; 5.00 20. 1; 500 21. When a trailing zero is after a decimal point it is significant. 22. 2; 0.0051 23. Leading zeros are not significant 24. 4; 5.003 25. 1) after a decimal point, 2) between non-­‐zero digits 26. Whether the zeros are significant or not 27. Scientific notation 28. (see answer in model) 29. (see table)

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    3 5.02 × 89.665 × 0.10 = 45.01183 = 45 (final answer) 3 5 2 2 significant figures 2 3 2 0 # digits after dec. pt. s.f. # digits after decimal pt. 1. 74 3 2 11. 8231 6 4 + 12. 651 5 3 26. 2141 Final Answer  26. 21 4 2 30. number of significant figures 31. number of decimal places

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    4 C HEM A CTIVITY 2B: U NITS A NSWERS TO C RITICAL T HINKING Q UESTIONS 1. m, kg, K 2. kg 3. False. kg is a base unit, and it has a prefix. 4. (answers will vary) 5. m; c; M; n; G 6. mg; nm; ps; dm; μK 7. 2.54 8. 1 9. 1 because the numerator and denominator are equal 10. 1 11. no 12. no; you are multiplying by 1 13. yes; 26.2 cm 14. We wanted to cancel in and keep cm 15. 1) The top and bottom are equal; 2) The units you want are on the top and the units you want to cancel are on the bottom.

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    5 C HEM A CTIVITY 2C: M ORE WITH C ONVERSIONS A NSWERS TO C RITICAL T HINKING Q UESTIONS 1. 1 2. No 3. 5 . 4 ft × 12 in 𝟏 𝐟𝐭 × 𝟐 . 𝟓𝟒 𝐜𝐦 1 in = 𝟏𝟔𝟎 cm 4. in ; m 5. 3 ft/1 yd; 12 in/1 ft; 2.54 cm/1 in; 0.01 m/1 cm; 1 km/1000m 6. 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 km 7. A solution map shows the order in which units will be changed, starting with the units given and ending with the desired units. 8. yes; no 9. m 3 10. m/s 11. kg/m 3 12. 0.1 m 13. 0.001 14. no 15. no; 4.5 g = 1 cm 3 16. (1 cm 3 /4.5 g) and (4.5 g/1 cm 3 ) 17. 1590 g × (1 cm 3 /4.5 g) = 350 cm 3 18. 1.00 19. 1.00 in 3 20. 2.54 cm 21. 2.54 cm 22. (2.54 cm) 3 = 16.4 cm 3 23. 16.4 24. Circle both: ! in ! . !" cm ! ! in ! !" . ! cm ! 25. 10 26. 27. (1 m/10 dm) 3 = 1 m 3 /1000 dm = 1 m 3 /1000 L 28. 5 m × 8 m × 3 m = 120 m 3 29. 120 m 3 × (1000 L/1 m 3 ) = 1.2×10 5 L

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    6 C HEM A CTIVITY 3A: C LASSIFYING M ATTER A NSWERS TO C RITICAL T HINKING Q UESTIONS 1. No 2. No 3. Yes (a little) 4. gas 5. Something is compressible if it can be made smaller by squeezing it. 6. stay about the same 7. a lot bigger 8. gas 9. Solid and liquid. Because the gas is much bigger but the same amount of solid and liquid are about the same size. 10. liquid and gas 11. Because solids don’t flow, the molecules must not be free to move around each other. 12. Similar to Fig. 3.4 in Introductory Chemistry 13. copper pipe 14. copper pipe, sugar 15. copper pipe, sugar 16. 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 dressing 19. 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; dressing 21. Answers will vary

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    7 C HEM A CTIVITY 3B: C HEMICAL C HANGE A NSWERS TO C RITICAL T HINKING Q UESTIONS 1. physical 2. physical 3. physical; melting point is listed in the table as physical, and boiling is a similar process 4. chemical 5. Chemical properties refer to reactivity, while physical properties do not. 6. physical 7. no 8. chemical 9. yes 10. In chemical change a new compound is formed. 11. chemical; a new compound is formed 12. 58 g butane, 208 g oxygen 13. 176 g carbon dioxide; 90 g water 14. 266 g 15. 266 g 16. the compounds present 17. the mass 18. 4.184 19. 4184 20. 3.60×10 6 21. J < cal < Cal < kWh 22. (4.184 J/1 cal) 23. 115 Cal × (1000 cal/1 Cal) × (4.184 J/1 cal) = 4.31×10 5 J 24. Energy moves from the car to the air as heat. 25. reactants 26. given off 27. given off 28. absorbing 29. the product it goes uphill by absorbing energy 30. Similar to the second part of figure 3.16 in Introductory Chemistry

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    8 C HEM A CTIVITY 3C: T EMPERATURE AND H EAT A NSWERS TO C RITICAL T HINKING Q UESTIONS 1. 180 ° 2. 100 ° 3. 100 ° 4. Celsius and Kelvin 5. A degree Celsius because there are fewer of them between freezing and boiling, so each one must be bigger 6. Yes, they are just shifted by 273 7. K = °C + 273.15 = 100 + 273.15 = 373.15 °C. Yes, it is consistent. 8. °C = (°F-­‐32)/1.8 9. (212 °F-­‐32)/1.8 = 100 °C 10. (70 °F -­‐32)/1.8 = 21.1 °C 11. °F = 1.8 ×°C + 32 12. (1.8)(21.1) + 32 = 69.98 °F 13. Twice as much material should take twice as much heat. 4.184 × 2 = 8.368 J 14. Temperature change is 17 times greater, so it should take 17 times as much heat 4.184 × 17 = 71.13 J 15. Both have doubled so it should take four times as much heat 4.184 × 2 × 2 = 16.74 J 16. 37 times the temperature and 250 times the amount… 4.184 × 37 × 250 = 38.7 kJ 17. q ; m ; C ; Δ T 18. 4.184 J/g °C 19. q = (2 g)(4.184 J/g °C)(2 °C) = 16.74 J 20. yes 21. yes 22. q = (2 g)(0.903 J/g °C)(2 °C) = 3.612 J 23. aluminium; it takes less heat to warm it by 1 °C, so the same amount of heat will warm it more 24. It is the ability of a substance to absorb heat without changing temperature.

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    9 C HEM A CTIVITY 4A: A TOMS AND E LEMENTS (I) A NSWERS TO C RITICAL T HINKING Q UESTIONS 1. It seems continuous. No matter how small of a drop, it is still water. 2. Greek philosophers 3. atoms 4. John Dalton 5. 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 with the wooden rods. 11. evenly distributed 12. More like tissue paper because it is evenly distributed across the room. 13. alpha particles 14. Most pass through with no deflection 15. 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 few small concentrated locations. 18. proton and neutron 19. electron 20. 1.0073 amu/0.00055 amu= 1831 (electrons per proton are the actual units for this) 21. proton and electron 22. one 23. They are the same because the cancel each other out 24. protons and neutrons

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    10 C HEM A CTIVITY 4B: A TOMS AND E LEMENTS (II) A NSWERS TO C RITICAL T HINKING Q UESTIONS 1. Si 2. P 3. K 4. 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. Antimony 8. 14; 79 9. The number of protons is in the periodic table above the symbol. 10. 19; 51 11. oxygen 12. proton 13. This must be nitrogen, not carbon, because the number of protons determines the identity of the element. 14. See Fig. 4.12 in Introductory Chemistry 15. Metals. See Fig. 4.12 in Introductory Chemistry 16. See Fig. 4.12 in Introductory Chemistry 17. See Fig. 4.12 in Introductory Chemistry 18. See the figure on p. 104 of Introductory Chemistry 19. a. rubidium: alkali metals b. vanadium: transition metal c. bromine: halogen d. neon: noble gas e. strontium: alkaline earth metal

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    11 C HEM A CTIVITY 4C: I ONS , I SOTOPES , AND A TOMIC M ASS A NSWERS TO C RITICAL T HINKING Q UESTIONS 1. 12; 12 2. +12 3. -­‐10 4. There are two more protons than electrons, so the total charge is 2+. 5. 9 6. It must have the same number of electrons as protons: 9. 7. 9 8. It must have one more electron than protons: 10. 9. Neutral atoms have the same number of protons and electrons. Ions have unequal number. 10. An ion is an atom with an unequal number of protons and electrons, and therefore a non-­‐zero charge. 11. A superscript to the right of the symbol. 12. Ion charge = N P -­‐ N e 13. The charge is 1+. The symbol is Na + . 14. Li + 15. K + 16. Na + 17. O 2-­‐ , F -­‐ , Mg 2+ 18. (add Ne to the right of F) 19. 10 20. 10 21. They are the same 22. 10 23. They are the same 24. Ions have the charges they do because atoms tend to form ions with the same number of electrons as the nearest noble gas. 25. 6 26. 1 amu 27. 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 significant difference. 29. the neutron! 30. 6 amu 31. 6 32. 7 33. 1,000 34. 11,868 amu

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    12 35. 143 amu 36. 12,011 amu 37. 12.011 amu 38. 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 weigh exactly this amount.

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    13 C HEM A CTIVITY 5A: C OMBINING E LEMENTS A NSWERS TO C RITICAL T HINKING Q UESTIONS 1. (answers in table) 2. Total = 4.5; Ratios both = 8.0 3. mass of H, mass of O, total mass 4. The ratio mass O/mass H 5. 80 g 6. 2 Hs, 1 O 7. H 2 O 8. No. The 2 should be subscript. 9. hydrogen peroxide, H 2 O 2 10. Hydrogen peroxide has two atoms of oxygen and water has only one. 11. 1 12. Yes. One of each and no subscripts. 13. CO 2 14. 12 Cs, 22 Hs, 11 Os 15. 1 16. 2 17. subscript 2 18. 2 19. subscript 2 20. O and H are in parentheses. The 2 applies to both. 21. 2 22. 6 23. 2 24. Yes. The subscript on the parentheses. 25. Parentheses indicate a group of atoms that can all be multiplied by a subscript. 26. 8 Two NH 4 units with four H atoms in each unit. 2x4=8. 27. 500: one for each H 28. Only the ratio of atoms 29. H 2 O 2 30. 2 Hs, 2 Os 31. 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 not communicate the actual number of atoms in one molecule. H 2 O 2 also says how many atoms are in one molecule. 33. CH 2 O

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