Chemistry A Guided Inquiry, 7th Edition by Richard S. Moog (2017)

Chemistry A Guided Inquiry, 7th Edition by Richard S. Moog (2017) Chemistry A Guided Inquiry, 7th Edition by Richard S. Moog (2017) Chemistry A Guided Inquiry, 7th Edition by Richard S. Moog (2017) Chemistry A Guided Inquiry, 7th Edition by Richard S. Moog (2017) Chemistry A Guided Inquiry, 7th Edition by Richard S. Moog (2017)

CHEMISTRY A Guided Inquiry Richard S Moog Professor Franklin & Marshall College John J Farrell Professor Emeritus Franklin & Marshall College VP AND EDITORIAL DIRECTOR EDITORIAL DIRECTOR EDITORIAL MANAGER CONTENT MANAGEMENT DIRECTOR CONTENT MANAGER SENIOR CONTENT SPECIALIST PRODUCTION EDITOR COVER PHOTO CREDIT Petra Recter Sladjana Bruno Gladys Soto Lisa Wojcik Nichole Urban Nicole Repasky Bharathy Surya Prakash © The POGIL Project This book was set in 12/14 TimesNewRomanMTStd by SPi Global and printed and bound by Strategic Content Imaging Founded in 1807, John Wiley & Sons, Inc has been a valued source of knowledge and understanding for more than 200 years, helping people around the world meet their needs and fulfill their aspirations Our company is built on a foundation of principles that include responsibility to the communities we serve and where we live and work In 2008, we launched a Corporate Citizenship Initiative, a global effort to address the environmental, social, economic, and ethical challenges we face in our business Among the issues we are addressing are carbon impact, paper specifications and procurement, ethical conduct within our business and among our vendors, and community and charitable support For more information, please visit our website: www.wiley.com/go/ citizenship Copyright © 2017, 2015 John Wiley & Sons, Inc All rights reserved No part of this publication may be reproduced, stored in a retrieval system, or transmitted in any form or by any means, electronic, mechanical, photocopying, recording, scanning or otherwise, except as permitted under Sections 107 or 108 of the 1976 United States Copyright Act, without either the prior written permission of the Publisher, or authorization through payment of the appropriate per‐copy fee to the Copyright Clearance Center, Inc., 222 Rosewood Drive, Danvers, MA 01923 (Web site: www.copyright.com) Requests to the Publisher for permission should be addressed to the Permissions Department, John Wiley & Sons, Inc., 111 River Street, Hoboken, NJ 07030‐5774, (201) 748‐6011, fax (201) 748‐6008, or online at: www.wiley.com/go/permissions Evaluation copies are provided to qualified academics and professionals for review purposes only, for use in their courses during the next academic year These copies are licensed and may not be sold or transferred to a third party Upon completion of the review period, please return the evaluation copy to Wiley Return instructions and a free of charge return shipping label are available at: www.wiley.com/go/returnlabel If you have chosen to adopt this textbook for use in your course, please accept this book as your complimentary desk copy Outside of the United States, please contact your local sales representative ISBN: 978-1-119-11070-5 (PBK) ISBN: 978-1-119-29932-5 (EVALC) Library of Congress Cataloging‐in‐Publication Data Names: Moog, Richard Samuel, author | Farrell, John J (John Joseph), 1937author Title: Chemistry : a guided inquiry / Richard S Moog, professor, Franklin & Marshall College, John J Farrell, professor emeritus, Franklin & Marshall College Description: 7th edition | Hoboken, NJ : Wiley, [2017] Identifiers: LCCN 2017016358 (print) | LCCN 2017011474 (ebook) | ISBN 9781119110705 (pbk.) | ISBN 9781119299325 (evalc) | ISBN 9781119299400 (pdf) | ISBN 9781119299509 (epub) Subjects: LCSH: Chemistry | Chemistry—Problems, exercises, etc Classification: LCC QD42 M64 2017 (ebook) | LCC QD42 (print) | DDC 540—dc23 LC record available at https://lccn.loc.gov/2017016358 The inside back cover will contain printing identification and country of origin if omitted from this page In addition, if the ISBN on the back cover differs from the ISBN on this page, the one on the back cover is correct To the Instructor The activities in this book are written according to the principles of Process Oriented Guided Inquiry Learning (POGIL), a student-centered, team-based, active-learning pedagogy based on research on how students learn best POGIL activities are designed to be used by students as active participants in learning teams There are many written materials available on-line to help instructors use this particular collection of POGIL activities effectively Please contact your Wiley representative for information on how to obtain access to these materials, or visit the web site at: http://www.wiley.com/college/moog In addition, The POGIL Project supports the dissemination and implementation of these types of materials for high school chemistry courses at the first-year and AP levels and for most of the undergraduate chemistry curriculum (including organic, physical, analytical and biochemistry.) POGIL materials are also available for other STEM disciplines including biology and anatomy and physiology, materials engineering, computer science, and mathematics Information about The POGIL Project, a not-for-profit 501(c)(3) organization, and its activities (including additional materials, workshops, and other professional development opportunities) can be found at http://www.pogil.org New for this edition This 7th edition of Chemistry: A Guided Inquiry is the result of the most substantial changes that we have made to these activities since they were first published over twenty years ago Over the past several years, substantial gains have been made by a variety of colleagues in The POGIL Project – and others – in understanding how to create activities that produce the most learning and the greatest gains in the development of key learning skills such as teamwork, critical thinking, and problem solving We have tried to incorporate as much of these new insights into the structure and organization of these materials as we can Below we list some of the major changes and highlights for this new edition: • Several activities have been restructured to better incorporate a learning cycle structure of exploration, concept invention, and application • Many of the activities now begin with a “Warm-Up” section that students may complete before coming to class In many cases, the activity has been reorganized so that much of the text is now in this “Warm-Up” section, enabling students to read some introductory material before coming to class and reserving more class time for working on the activities with their teammates Instructors may choose to use the “Warm-Up” sections in this way, or they may choose to have the students complete the “Warm-Up” sections as part of the team work during class time • The amount of text has been reduced and restructured to make it easier for students to read and process • Student responses to Critical Thinking Questions are more frequently organized into tables to facilitate analysis and interpretation • The content dealing with electronegativity, partial charge, and dipole moments has been reorganized to reduce repetition and get to the concept of electronegativity sooner The concept of Average Valence Electron Energy is still introduced (in ChemActivity 19) but its relationship to electronegativity is then established directly • Based on research on how students respond to the wording of prompts in these types of activities, we have included more prompts that directly require the students to explain their reasoning and/or analysis We have also included more explicit prompts for students to engage as a team in addressing the questions that are posed Acknowledgments This book is the result of innumerable interactions that we have had with a large number of stimulating and thoughtful people • We greatly appreciate the support and encouragement of the many members of The POGIL Project and the Middle Atlantic Discovery Chemistry Project, who have provided us with an opportunity to discuss our ideas with interested, stimulating, and dedicated colleagues Over the past several years, our colleagues in The POGIL Project have helped us learn a great deal about how to construct more effective and impactful activities; much of what we have learned from them is reflected in the substantially revised activities in this edition • Thanks to the numerous colleagues who used our previous editions in their classrooms Many provided us with insightful comments and suggestions for which we are grateful We are particularly indebted to Professor Gail Webster, Guilford College, who provided us with feedback on every activity in this edition Her thoughtful insights and suggestions had a significant impact on the final product • Many thanks to Jim Spencer, Professor Emeritus, Franklin & Marshall College, for his helpful and insightful discussions, comments, and corrections • A great debt of thanks is due our students in General Chemistry at Franklin & Marshall College over the past two decades Their enthusiasm for this approach, patience with our errors, and helpful and insightful comments have inspired us to continue to develop as instructors, and have helped us to improve these materials immeasurably In particular, RSM thanks the students in his CHM 111 class at Franklin & Marshall College who used the penultimate draft of this book during the fall, 2016 semester Their thoughtful comments and keen eye for typographic errors helped improve this edition and their patience and good humor was greatly appreciated • Thanks to the National Science Foundation (Grants DUE-0231120, 0618746, 0618758, and 0618800) for its initial support of The POGIL Project, a not-for-profit organization that fosters the development and dissemination of guided-inquiry materials and encourages faculty to develop and use student-centered approaches in their classrooms • Special thanks to Dan Apple, Pacific Crest Software, for starting us on this previously untraveled path The Pacific Crest Teaching Institute we attended in 1994 provided us with the initial insights and inspiration to convert our classrooms into fully student-centered learning environments vi • RSM would also like to thank Mark McDaniel, Gina Frey, and all of the staff of the Center for Integrative Research on Cognition, Learning, and Education at Washington University in St Louis A more stimulating sabbatical year could not be imagined, and many of the insights gained from that year were invaluable in improving this edition Contents Chem Topic Activity To the Student Page 1 10 11 Atomic Structure The Nuclear Atom Atomic Number and Atomic Mass Coulombic Potential Energy The Shell Model (I) The Shell Model (II) Atomic Size Electromagnetic Radiation Photoelectron Spectroscopy The Shell Model (III) Electron Configurations and the Periodic Table Electron Spin 12 13 14 15 16 17 18 19 20 21 Molecular Structure Lewis Structures (I) Bond Characteristics Lewis Structures (II) Lewis Structures (III) Lewis Structures (IV) Molecular Shapes Hybrid Orbitals Electronegativity Partial Charge Covalent Bonds and Dipole Moments 75 82 90 96 102 107 117 120 126 132 22 23 24 25 Solids and Liquids The Ionic Bond Metals The Bond-Type Triangle Intermolecular Forces 140 148 152 157 26 27 28 29 30 Stoichiometry The Mole Concept Chemical Equations Limiting Reagent Empirical Formula Molarity 164 170 176 182 188 31 Gases The Ideal Gas Law 196 32 33 Thermochemistry Enthalpy of Atom Combination Enthalpy Changes in Chemical Reactions 200 207 16 22 28 40 44 48 56 62 70 viii 34 35 36 37 38 39 Equilibrium Rates of Chemical Reactions (I) Equilibrium (I) Equilibrium (II) The Equilibrium Constant (I) The Reaction Quotient The Solubility Product 213 217 223 228 236 246 40 41 42 43 44 45 Acids and Bases Acids and Bases Acid Strength Weak Acid/Base Dissociation pH Relative Acid Strength Acid/Base Strength of Conjugate Pairs 256 261 270 278 283 290 46 47 48 49 Oxidation-Reduction Redox Reactions Oxidation Numbers The Electrochemical Cell The Cell Voltage 297 302 306 312 50 51 52 53 54 Thermodynamics Entropy (I) Entropy (II) Entropy Changes in Chemical Reactions The Equilibrium Constant (II) The Equilibrium Constant (III) 316 322 326 332 337 55 56 57 58 59 60 Kinetics Rates of Chemical Reactions (II) Integrated Rate Laws Reaction Mechanisms (I) Reaction Mechanisms (II) Reaction Mechanisms (III) Temperature Dependence of Rate Constants 342 352 360 365 375 380 Appendix TABLE A.1 Values of Selected Fundamental Constants TABLE A.2 Selected Conversion Factors TABLE A.3 Standard-State Enthalpies, Free Energies, and Entropies of Atom Combination 383 383 384 59 Ch hemActivity Reaction n Mechanism ms (III) 37 79 Exe ercise diagram (draawn in the absence of a Modify thee following reaction co oordinate d catalyst) fo or the presen nce of a cata alyst Prob blem At 1000 °C C, the reactiion HI(g) kJ/mol and d ΔH° = 9.5 kJ/mole has Ea (forrward) = 1883 I2(gg) + H2(g) h a) nate) for this Dra aw a reactio on coordinatte diagram (H vs reacttion coordin ke some atteempt to scalle reacction Graph paper is not n necessarry, but mak he prop perly Clearrly indicatee Ea (forwaard), Ea (revverse), and ΔH° on th diag gram b) Dettermine the value of Ea (reverse) c) o 58 kJ/molee A platinum p cattalyst is add ded and Ea ((forward) iss reduced to What is the vallue of ΔH° when w the caatalyst is preesent? ChemActivity 60 Temperature Dependence of Rate Constants (What Role Does Activation Energy Play?) Model: The Arrhenius Equation The rate of a reaction depends on the temperature because the magnitude of the rate constant, k, is typically a function of the temperature In general, the relationship between k and T is found to be Ea ln k = ln A – RT (1) Here, A is the frequency factor, Ea is the activation energy in units of joules per mole, T is the absolute temperature in Kelvin, and R is the gas constant (8.314 J/mol K) Both A and Ea are characteristic of the particular reaction being studied If the rate constant for a given reaction is examined at two temperatures, T1 and T2, and if the observed rate constants at those temperatures are k1 and k2, respectively, then equation can be used to derive the following relationship: ln º k1 Ea ª = R ôT T ằ 1ẳ k2 (2) Critical Thinking Questions According to equation 1, if the temperature increases, does the rate constant increase or decrease? Explain At how many different temperatures must the rate constant be determined in order to evaluate the activation energy for a reaction? A student is studying a reaction in detail and uses experimental data to calculate that at a given temperature, T, k > A for the reaction Explain why it must be that the student has made an error ChemActivity 60 Temperature Dependence of Rate Constants 381 This same student has determined the value of the rate constant, k, for the reaction at a number of different temperatures She decides to use her data to make a plot of ln k vs 1/T in order to obtain important parameters related to this reaction Based on equation 1, what information can she gain from this plot? Explain your reasoning According to equation 1, if the activation energy for some reaction, Q, is greater than the activation energy for a different reaction, W, which has the greater rate constant—reaction Q or reaction W (assuming that the value of A, the frequency factor, is identical in both reactions)? Explain Exercises A chemist's "rule of thumb" is that the rate of a chemical reaction doubles for every 10 °C increase in temperature Use equation to demonstrate this rule of thumb (assume that a typical chemical reaction has an activation energy of 50 J kJ/mol) Recall that R = 8.314 K mol (Hint: a typical chemical reaction occurs at a typical temperature.) A great Martian chemist enunciated the following chemical principle: The rate of a chemical reaction doubles for every °C increase in temperature Assume that the average temperature on Mars is –40 °C, and determine if the Martian chemist was correct or not Indicate whether the following statement is true or false and explain your reasoning In general, the higher the activation energy, the faster a reaction occurs at a given temperature 382 ChemActivity 60 Temperature Dependence of Rate Constants Problems H2(g) + I2(g) HI(g) The rate constant for the above reaction at two temperatures was determined: Temperature (K) 400 500 Rate Constant (M–1 sec–1) 0.0234 0.750 Determine the rate constant at 400 K for the reverse reaction HI(g) H2(g) + I2(g) as precisely as you can, assuming that A = × 105 M–1 s–1 for the reverse reaction Consider a generic reaction: AB (g) + CD (g) AC (g) + BD (g) a) Construct a reaction coordinate diagram for this reaction assuming that it has a large equilibrium constant, but that it reaches equilibrium very slowly Explain your reasoning clearly b) Indicate how the addition of a catalyst would change the reaction coordinate diagram from part a, and describe what effect this would have on the equilibrium constant and the rate at which equilibrium is reached Appendix TABLE A.1 Values of Selected Fundamental Constants Speed of light in a vacuum (c) c = 2.99792458 x 108 m/s Charge on an electron (qe) qe = 1.6021892 x 10–19 C Rest mass of an electron (me) me = 9.109534 x 10–28 g me = 5.4858026 x 10–4 amu Rest mass of a proton (mp) mp = 1.6726485 x 10–24 g mp = 1.00727647 amu mn = 1.6749543 x 10–24 g Rest mass of a neutron (mn) mn = 1.008665012 amu Faraday's constant (F) F = 96,484.56 C/mol Planck's constant (h) h = 6.626176 x 10–34 J s Ideal gas constant (R) R = 0.0820568 L-atm/mol-K R = 8.31441 J/mol-K Atomic mass unit (amu) amu = 1.6605655 x 10–24 g Boltzmann's constant (k) k = 1.380662 x 10–23 J/K Avogadro's constant (N) N = 6.022045 x 1023 mol–1 Rydberg constant (RH) RH = 1.09737318 x 107 m–1 = 1.09737318 x 10–2 nm–1 Heat capacity of water C = 75.376 J/mol-K TABLE A.2 Energy Selected Conversion Factors J = 0.2390 cal = 107 erg = volt•coulomb cal = 4.184 J (by definition) ev/atom = 1.6021892 x 10–19 J/atom = 96.484 kJ/mol Temperature K = °C + 273.15 °C = (5/9)(°F – 32) °F = (9/5)(°C) + 32 Pressure atm = 760 mm Hg = 760 torr = 101.325 kPa Mass kg = 2.2046 lb lb = 453.59 g = 0.45359 kg oz = 0.06250 lb = 28.350 g ton = 2000 lb = 907.185 kg tonne (metric) = 1000 kg = 2204.62 lb Volume mL = 0.001 L = cm3 (by definition) oz (fluid) = 0.031250 qt = 0.029573 L qt = 0.946326 L L = 1.05672 qt m = 39.370 in mi = 1.60934 km in = 2.54 cm (by definition) Length 384 TABLE A.3 Standard-State Enthalpies, Free Energies, and Entropies of Atom Combination ΔHac ° ΔGac ° ΔSac ° Substance (kJ/mol) (kJ/mol) (J/mol-K) Aluminum Al(s) –326.4 –285.7 –136.21 Al(g) 0 Al+3(aq) –857 –77.1 –486.2 Al2O3(s) –3076.0 –2848.9 –761.33 AlCl3(s) –1395.6 –1231.5 –549.46 –2067.5 –1896.4 –574.36 AlF3(s) Al2(SO4)3(s) –7920.1 –7166.9 –2525.9 Ba(s) Ba(g) Ba+2(aq) BaO(s) Ba(OH)2.8H2O(s) BaCl2(s) BaCl2(aq) BaSO4(s) Ba(NO3)2(s) Ba(NO3)2(aq) Barium –180 –146 0 –718 –707 –983 –903 –9931.6 –8915 –1282 –1168 –1295 –1181 –2929 –2673 –3612 –3217 –3573 –3231 Be(s) Be(g) Be+2(aq) BeO(s) BeCl2(s) Beryllium –324.3 –286.6 0 –707.1 –666.3 –1183.1 –1026.6 –1058.1 –943.6 –126.77 –266.0 –283.18 –383.99 Bi(s) Bi(g) Bi2O3(s) BiCl3(s) BiCl3(g) Bi2S3(s) Bismuth –207.1 –168.2 0 –1735.6 –1525.3 –951.2 –800.2 –837.8 –741.2 –1393.7 –1191.8 –130.31 –705.8 –505.6 –323.79 –677.2 B(s) B(g) B2O3(s) B2H6(g) B5H9( ) B10H14(s) Boron –562.7 –518.8 0 –3145.7 –2926.4 –2395.7 –2170.4 –4729.7 –4251.4 –8719.3 –7841.2 (continued) –107.4 –160.6 –260.88 –3419 –376.96 –378.04 –850.1 –1229.4 –1140.7 –147.59 –736.10 –763.07 –1615.45 –2963.92 385 TABLE A.3 Substance H3BO3(s) BF3(g) BCl3( ) B3N3H6( ) B3N3H6(g) Standard-State Enthalpies, Free Energies, and Entropies of Atom Combination (continued) ΔHac ° ΔGac ° ΔSac ° (kJ/mol) (kJ/mol) (J/mol-K) –3057.5 –2792.7 –891.92 –1936.7 –1824.9 –375.59 –1354.9 –1223.2 –442.7 –4953.1 –4535.4 –1408.9 –4923.9 –4532.8 –1319.84 Br2( ) Br2(g) Br(g) HBr(g) HBr(aq) BrF(g) BrF3(g) BrF5(g) Bromine –223.768 –164.792 –192.86 –161.68 0 –365.93 –339.09 –451.08 –389.60 –284.72 –253.49 –604.45 –497.56 –935.73 –742.6 Ca(s) Ca(g) Ca+2(aq) CaO(s) Ca(OH)2(s) CaCl2(s) CaSO4(s) CaSO4.2H2O(s) Ca(NO3)2(s) CaCO3(s) Ca3(PO4)2(s) Calcium –178.2 –144.3 0 –721.0 –697.9 –1062.5 –980.1 –2097.9 –1912.7 –1217.4 –1103.8 –2887.8 –2631.3 –4256.7 –4383.2 –3557.0 –3189.0 –2849.3 –2639.5 –7278.0 –6727.9 C(graphite) C(diamond) C(g) CO(g) CO2(g) COCl2(g) CH4(g) HCHO(g) H2CO3(aq) HCO3–(aq) CO3–2(aq) CH3OH( ) CH3OH(g) CCl4( ) CCl4(g) CHCl3( ) Carbon –716.682 –671.257 –714.787 –668.357 0 –1076.377 –1040.156 –1608.531 –1529.078 –1428.0 –1318.9 –1662.09 –1535.00 –1509.72 –1412.01 –2599.14 –2396.02 –2373.83 –2156.47 –2141.33 –1894.26 –2075.11 –1882.25 –2037.11 –1877.94 –1338.84 –1159.19 –1306.3 –1154.57 –1433.84 –1265.20 –197.813 –104.58 –91.040 –207.3 –104.81 –358.75 –648.60 –113.46 –208.0 –276.19 –623.03 –380.7 –860.3 –1553.8 –1234.5 –703.2 –1843.5 –152.36 –155.719 –121.477 –266.47 –366.02 –430.68 –329.81 –683.3 –664.8 –698.16 –651.2 –538.19 –602.49 –509.04 –567.3 386 TABLE A.3 Standard-State Enthalpies, Free Energies, and Entropies of Atom Combination (continued) ΔHac ° ΔGac ° ΔSac ° Substance (kJ/mol) (kJ/mol) (J/mol-K) CHCl3(g) –1402.51 –1261.88 –472.69 CH2Cl2( ) –1516.80 –1356.37 –540.1 –1487.81 –1354.98 –447.69 CH2Cl2(g) CH3Cl(g) –1572.15 –1444.08 –432.9 CS2( ) –1184.59 –1082.49 –342.40 CS2(g) –1156.93 –1080.64 –255.90 HCN(g) –1271.9 –1205.43 –224.33 CH3NO2( ) –2453.77 –2214.51 –805.89 C2H2(g) –1641.93 –1539.81 –344.68 –2251.70 –2087.35 –555.48 C2H4(g) C2H6(g) –2823.94 –2594.82 –774.87 CH3CHO( ) –2745.43 –2515.35 –775.9 –3286.8 –3008.86 –937.4 CH3CO2H( ) CH3CO2H(g) –3234.55 –2992.96 –814.7 –3288.06 –3015.42 –918.5 CH3CO2H(aq) –3070.66 –2785.03 –895.8 CH3CO2–(aq) CH3CH2OH( ) –3266.12 –2968.51 –1004.8 –3223.53 –2962.22 –882.82 CH3CH2OH(g) CH3CH2OH(aq) –3276.7 –2975.37 –1017.0 C6H6( ) –5556.96 –5122.52 –1464.1 C6H6(g) –5523.07 –5117.36 –1367.7 Cl2(g) Cl(g) Cl–(aq) ClO2(g) Cl2O(g) Cl2O7( ) HCl(g) HCl(aq) ClF(g) Chlorine –243.358 –211.360 0 –288.838 –236.908 –517.5 –448.6 –412.2 –345.2 –1750 –431.64 –404.226 –506.49 –440.155 –255.15 –223.53 Cr(s) Cr(g) CrO3(s) CrO4–2(aq) Cr2O3(s) Cr2O7-2(aq) (NH4)2Cr2O7(s) PbCrO4(s) Chromium –396.6 –351.8 0 –1733.6 –2274.4 –2006.47 –2680.4 –2456.89 –4027.7 –3626.8 –7030.7 –2519.2 - Co(s) Co(g) Cobalt –424.7 –380.3 0 (continued) –107.330 –108.7 –230.47 –225.24 –93.003 –223.4 –106.06 –150.73 –768.51 –751.0 –1214.5 - –149.475 387 TABLE A.3 Standard-State Enthalpies, Free Energies, and Entropies of Atom Combination (continued) ΔHac ° ΔGac ° ΔSac ° Substance (kJ/mol) (kJ/mol) (J/mol-K) Co+2(aq) –482.9 –434.7 –293 Co+3(aq) –333 –246.3 –485 CoO(s) –911.8 –826.2 –287.60 –3162 –2842 –1080.3 Co3O4(s) Co(NH3)6+3(aq) –7763.5 –6929.5 –3018 Cu(s) Cu(g) Cu+(aq) Cu+2(aq) CuO(s) Cu2O(s) CuCl2(s) CuS(s) Cu2S(s) CuSO4(s) Cu(NH3)4+2(aq) Copper –338.32 –298.58 0 –266.65 –248.60 –273.55 –233.09 –744.8 –660.0 –1094.4 –974.9 –807.8 –685.6 –670.2 –590.4 –1304.9 –921.6 –2385.17 –1530.44 –5189.4 –4671.13 –133.23 –125.8 –266.0 –284.81 –400.68 –388.71 –267.7 –379.7 –869 –1882.5 Fluorine –157.98 –123.82 0 –411.62 –340.70 –567.7 –538.4 –616.72 –561.98 –114.73 –172.6 –99.688 –184.8 H2(g) H(g) H+(aq) OH–(aq) H2O( ) H2O(g) H2O2( ) H2O2(aq) Hydrogen –435.30 –406.494 0 –217.65 –203.247 –696.81 –592.222 –970.30 –875.354 –926.29 –866.797 –1121.42 –990.31 –1124.81 –1003.99 –98.742 –114.713 –286.52 –320.57 –202.23 –441.9 –407.6 I2(s) I2(g) I(g) HI(g) IF(g) IF5(g) IF7(g) ICl(g) IBr(g) Iodine –213.676 –141.00 –151.238 –121.67 0 –298.01 –272.05 –281.48 –250.92 –1324.28 –1131.78 –1603.7 –1322.17 –210.74 –181.64 –177.88 –149.21 –245.447 –100.89 –88.910 –103.38 –646.9 –945.6 –98.438 –97.040 F2(g) F(g) F–(aq) HF(g) HF(aq) 388 TABLE A.3 Substance Fe(s) Fe(g) Fe+2(aq) Fe+3(aq) Fe2O3(s) Fe3O4(s) Fe(OH)2(s) Fe(OH)3(s) FeCl3(s) FeS2(s) Fe(CO)5( ) Fe(CO)5(g) Standard-State Enthalpies, Free Energies, and Entropies of Atom Combination (continued) ΔHac ° ΔGac ° ΔSac ° (kJ/mol) (kJ/mol) (J/mol-K) Iron –416.3 –370.7 –153.21 0 –505.4 –449.6 –318.2 –464.8 –375.4 –496.4 –2404.3 –2178.8 –756.75 –3364.0 –3054.4 –1039.3 –1918.9 –1727.2 –644 –2639.8 –2372.1 –901.1 –1180.8 –1021.7 –533.8 –1152.1 –1014.1 –463.2 –6019.6 –5590.9 –1438.1 –5979.5 –5582.9 –1330.9 Pb(s) Pb(g) Pb+2(aq) PbO(s) PbO2(s) PbCl2(s) PbCl4( ) PbS(s) PbSO4(s) Pb(NO3)2(s) PbCO3(s) Lead –195.0 –161.9 0 –196.7 –186.3 –661.5 –581.5 –970.7 –842.7 –797.8 –687.4 –1011.0 –574.2 –498.9 –2390.4 –2140.2 –3087.3 –2358.3 –2153.8 –110.56 –164.9 –267.7 –428.9 –369.8 –252.0 –838.84 –685.6 Li(s) Li(g) Li+(aq) LiH(s) LiOH(s) LiF(s) LiCl(s) LiBr(s) LiI(s) LiAlH4(s) LiBH4(s) Lithium –159.37 –126.66 0 –437.86 –419.97 –467.56 –398.26 –1111.12 –1000.59 –854.33 –784.28 –689.66 –616.71 –622.48 –551.06 –536.62 –467.45 –1472.7 –1270.0 –1401.9 –1333.4 –109.65 –125.4 –233.40 –371.74 –261.87 –244.64 –239.52 –232.78 –683.42 –675.21 Mg(s) Mg(g) Mg+2(aq) MgO(s) MgH2(s) Magnesium –147.70 –113.10 0 –614.55 –567.9 –998.57 –914.26 –658.3 –555.5 (continued) –115.97 –286.8 –282.76 –346.99 389 TABLE A.3 Substance Mg(OH)2(s) MgCl2(s) MgCO3(s) MgSO4(s) Mn(s) Mn(g) Mn+2(aq) MnO(s) MnO2(s) Mn2O3(s) Mn3O4(s) KMnO4(s) MnS(s) Hg( ) Hg(g) Hg+2(aq) HgO(s) HgCl2(s) Hg2Cl2(s) HgS(s) N2(g) N(g) NO(g) NO2(g) N2O(g) N2O3(g) N2O4(g) N2O5(g) NO3–(aq) NOCl(g) NO2Cl(g) HNO2(aq) HNO3(g) HNO3(aq) NH3(g) NH3(aq) NH4+(aq) NH4NO3(s) NH4NO3(aq) Standard-State Enthalpies, Free Energies, and Entropies of Atom Combination (continued) ΔHac ° ΔGac ° ΔSac ° (kJ/mol) (kJ/mol) (J/mol-K) –2005.88 –1816.64 –637.01 –1032.38 –916.25 –389.43 –2707.7 –2491.7 –724.2 –2708.1 –2448.9 –869.1 Manganese –280.7 –238.5 0 –501.5 –466.6 –915.1 –833.1 –1299.1 –1167.1 –2267.9 –2053.3 –3226.6 –2925.6 –2203.8 –1963.6 –773.7 –695.2 Mercury –61.317 –31.820 0 +109.8 +132.58 –401.32 –322.090 –529.0 –421.8 –631.21 –485.745 –398.3 –320.67 Nitrogen –945.408 –911.26 0 –631.62 –600.81 –937.86 –867.78 –1112.53 –1038.79 –1609.20 –1466.99 –1932.93 –1740.29 –2179.91 –1954.8 –1425.2 –1259.56 –791.84 –726.96 –1080.12 –970.4 –1307.9 –1172.9 –1572.92 –1428.79 –1645.22 –1465.32 –1171.76 –1081.82 –1205.94 –1091.87 –1475.81 –1347.93 –2929.08 –2603.31 –2903.39 –2610.00 –141.69 –247.3 –275.05 –442.76 –720.1 –1009.7 –806.50 –263.3 –98.94 –207.2 –265.73 –359.4 –487.8 –260.4 –114.99 –103.592 –235.35 –247.80 –477.48 –646.53 –756.2 –490.1 –217.86 –368.46 –454.5 –484.80 –604.8 –304.99 –386.1 –498.8 –1097.53 –988.8 390 TABLE A.3 Substance NH4Cl(s) N2H4( ) N2H4(g) HN3(g) O2(g) O(g) O3(g) Standard-State Enthalpies, Free Energies, and Entropies of Atom Combination (continued) ΔHac ° ΔGac ° ΔSac ° (kJ/mol) (kJ/mol) (J/mol-K) –1779.41 –1578.17 –682.7 –1765.38 –1574.91 –644.24 –1720.61 –1564.90 –526.98 –1341.7 –1242.0 –335.37 Oxygen –498.340 –463.462 0 –604.8 –532.0 –116.972 –244.24 P(white) P4(g) P2(g) P(g) PH3(g) P4O6(s) P4O10(s) PO43-(aq) PF3(g) PF5(g) PCl3( ) PCl3(g) PCl5(g) H3PO4(s) H3PO4(aq) Phosphorus –314.64 –278.25 –1199.65 –1088.6 –485.0 –452.8 0 –962.2 –874.6 –4393.7 –6734.3 –6128.0 –2588.7 –2223.9 –1470.4 –1361.5 –2305.4 –999.4 –867.6 –966.7 –863.1 –1297.9 –1111.6 –3243.3 –2934.0 –3241.7 –2833.6 –122.10 –372.79 –108.257 –297.10 –2034.46 –1029 –366.22 –441.7 –347.01 –624.60 –1041.05 –1374 K(s) K(g) K+(aq) KOH(s) KCl(s) KNO3(s) K2Cr2O7(s) KMnO4(s) Potassium –89.24 –60.59 0 –341.62 –343.86 –980.82 –874.65 –647.67 –575.41 –1804.08 –1606.27 –4777.4 –4328.7 –2203.8 –1963.6 –96.16 –57.8 –357.2 –242.94 –663.75 –1505.9 –806.50 Si(s) Si(g) SiO2(s) SiH4(g) SiF4(g) SiCl4( ) SiCl4(g) Silicon –455.6 –411.3 0 –1864.9 –1731.4 –1291.9 –1167.4 –2386.5 –2231.6 –1629.3 –1453.9 –1599.3 –1451.0 (continued) –149.14 –448.24 –422.20 –520.50 –589 –498.03 391 TABLE A.3 Substance Standard-State Enthalpies, Free Energies, and Entropies of Atom Combination (continued) ΔHac ° ΔGac ° ΔSac ° (kJ/mol) (kJ/mol) (J/mol-K) Ag(s) Ag(g) Ag+(aq) Ag(NH3)2+(aq) Ag2O(s) AgCl(s) AgBr(s) AgI(s) Silver –284.55 –178.97 –2647.15 –849.32 –533.30 –496.80 –453.23 Na(s) Na(g) Na+(aq) NaH(s) NaOH(s) NaOH(aq) NaCl(s) NaCl(g) NaCl(aq) NaNO3(s) Na3PO4(s) Na2SO3(s) Na2SO4(s) Na2CO3(s) NaHCO3(s) NaCH3CO2(s) Na2CrO4(s) Na2Cr2O7(s) Sodium –107.32 –76.761 –102.50 0 –374.45 –338.666 –94.7 –3811.25 –313.47 –228.409 –999.75 –891.233 –365.025 –1044.25 –930.889 –381.4 –640.15 –566.579 –246.78 –405.65 –379.10 –89.10 –636.27 –575.574 –203.4 –1795.38 –1594.58 –673.66 –3550.68 –3224.26 –1094.75 –2363.96 –2115.0 –803 –2877.20 –2588.86 –969.89 –2809.51 –2564.41 –813.70 –2739.97 –2497.5 –808.0 –3400.78 –3099.66 –1013.2 –2950.1 –2667.18 –949.53 –4730.6 - S8(s) S8(g) S(g) S2-(aq) SO2(g) SO3(s) SO3( ) SO3(g) SO42-(aq) SOCl2(g) SO2Cl2(g) H2S(g) Sulfur –2230.440 –2128.14 –245.7 –1073.975 –1480.82 –1467.36 –1422.04 –2184.76 –983.8 –1384.5 –734.74 –245.65 –168.54 –2393.51 –734.23 –461.12 –424.95 –382.34 –130.42 –100.29 –922.6 –385.7 –242.0 –240.9 –238.3 –1906.000 –1310.77 –1856.37 –911.59 0 –152.4 –182.4 –1001.906 –241.71 –1307.65 –580.3 –1307.19 –537.2 –1304.50 –394.23 –1909.70 –791.9 –879.6 –349.50 –1233.1 –508.39 –678.30 –191.46 392 TABLE A.3 Substance H2SO3(aq) H2SO4(aq) SF4(g) SF6(g) SCN–(aq) Standard-State Enthalpies, Free Energies, and Entropies of Atom Combination (continued) ΔHac ° ΔGac ° ΔSac ° (kJ/mol) (kJ/mol) (J/mol-K) –2070.43 –1877.75 –648.2 –2620.06 –2316.20 –1021.4 –1369.66 –1217.2 –510.81 –1962 –1715.0 –828.53 –1391.75 –1272.43 –334.9 Sn(s) Sn(g) SnO(s) SnO2(s) SnCl2(s) SnCl4( ) SnCl4(g) Tin –302.1 –837.1 –1381.1 –870.6 –1300.1 –1260.3 Ti(s) Ti(g) TiO(s) TiO2(s) TiCl4( ) TiCl4(g) Titanium –469.9 –425.1 0 –1238.8 –1151.8 –1913.0 –1778.1 –1760.8 –1585.0 –1719.8 –1574.6 –149.6 –306.5 –452.0 –588.7 –486.2 W(s) W(g) WO3(s) Tungsten –849.4 –807.1 0 –2439.8 –2266.4 –141.31 –581.22 Zn(s) Zn(g) Zn2+(aq) ZnO(s) ZnCl2(s) ZnS(s) ZnSO4(s) Zinc –130.729 –95.145 0 –284.62 –242.21 –728.18 –645.18 –789.14 –675.90 –615.51 –534.69 –2389.0 –2131.8 –119.35 –273.1 –278.40 –379.92 –271.1 –862.5 –267.3 –755.9 –1250.5 –249.8 –1122.2 –124.35 –273.0 –438.3 –570.7 –463.5 WILEY END USER LICENSE AGREEMENT Go to www.wiley.com/go/eula to access Wiley’s ebook EULA ... marbles have a mass of 5.00 g and 75% of the marbles have a mass of 7.00 g The average mass of a marble can be determined by dividing the total mass of the marbles by the total number of marbles: average... in Model have the same mass as the average mass? For a large number of marbles (assume that the actual number of marbles is unknown), 37.2% have a mass of 10.0 g and 62.8% have a mass of 12.00... chemistry courses at the first-year and AP levels and for most of the undergraduate chemistry curriculum (including organic, physical, analytical and biochemistry.) POGIL materials are also available