Physical chemistry (3rd ed), by gilbert w castellan@handu boyzz PDF

Preview

Summary

Download Physical chemistry (3rd ed), by gilbert w castellan@handu boyzz PDF

Description

STANDARD ATOMIC MASSES 1979 (Scaled to the relative atomic mass , A ,.(I2C) = 12) Name Actinium Aluminium Americium Antimony Argon Arsenic Astatine Barium Berkelium Beryllium Bismuth Boron Bromine Cadmium Caesium Calcium Californium Carbon Cerium Chlorine Chromium Cobalt Copper Curium Dysprosium Einsteinium Erbium Europium Fermium Fluorine Francium Gadolinium Gallium Germanium Gold Hafnium Helium Holmium Hydrogen Indium Iodine Iridium Iron Krypton Lanthanum Lawrencium Lead Lithium Lutetium Magnesium Manganese Mendelevium Mercury

Atomic Symbol number Ac 89 Al 13 Am 95 Sb 51 Ar 18 As 33 At 85 Ba 56 Bk 97 Be 4 Bi 83 B 5 Br 35 Cd 48 55 Cs Ca 20 Cf 98 C 6 Ce 58 Cl 17 Cr 24 Co 27 Cu 29 Cm 96 Dy 66 Es 99 Er 68 Eu 63 Fm 100 F 9 Fr 87 Gd 64 Ga 31 Ge 32 Au 79 Hf 72 He 2 Ho 67 H I In 49 I 53 Ir 77 Fe 26 Kr 36 La 57 Lr 103 Pb 82 Li 3 Lu 71 Mg 12 Mn 25 Md 101 Hg 80

Atomic mass 227.0278 26 .98154 (243) 121.75* 39 .948 74.9216 (210) 137 .33 (247) 9.01218 208.9804 10.81 79 .904 112.41 132 .9054 40 .08 (25 I) 12.011 140. 12 35.453 51.996 58 .9332 63 .546* (247) 162 .50* (252) 167.26* 151.96 (257) 18.998403 (223) 157.25 * 69.72 72 .59* 196.9665 178.49* 4.00260 164.9304 1.0079 114.82 126.9045 192 .22 * 55 .847* 83 .80 138.9055 * (260) 207 .2 6.941 * 174 .967 * 24.305 54.9380 (258) 200 .59*

Name Molybdenum Neodymium Neon Neptunium Nickel Niobium Nitrogen Nobelium Osmium Oxygen Palladium Phosphorus Platinum Plutonium Polonium Potassium Praseodymium Promethium Protactinium Radium Radon Rhenium Rhodium Rubidium Ruthenium Samarium Scandium Selenium Silicon Silver Sodium Strontium Sulfur Tantalum Technetium Tellurium Terbium Thallium Thorium Thulium Tin Titanium Tungsten (U nnilhexium) (Unnilpentium) (U nnilquadium) Uranium Vanadium Xenon Ytterbium Yttrium Zinc Zirconium

Atomic Symbol number Mo Nd Ne Np Ni Nb N No Os

0 Pd P Pt Pu Po K Pr Pm Pa Ra Rn Re Rh Rb Ru Sm Sc Se Si Ag Na Sr S Ta Tc Te Tb TI Th Tm Sn Ti

W (Unh) (Unp) (Unq) U V Xe Yb Y Zn Zr

42 60 10 93 28 41 7 102 76 8 46 15 78 94 84 19 59 61 91 88 86 75 45 37 44 62 21 34 14 47 II 38 16 73 43 52 65 81 90 69 50 22 74 106 105 104 92 23 54 70 39 30 40

Atomic mass 95.94 144.24* 20 . 179 237 .0482 58.69 92.9064 14 .0067 (259) 190.2 15 .9994* 106.42 30.97376 195.08* (244) (209) 39.0983 140.9077 (145) 231 .0359 226 .0254 (222) 186.207 102 .9055 85.4678 * 101.07* 150.36* 44.9559 78 .96* 28.0855 * 107 .868 22 .98977 87. 62 32 .06 180.9479 (98) 127.60* 158.9254 204 .383 232 .0381 168.9342 118 .69* 47 .88 * 183.85* (263) (262) (261) 238.0289 50.9415 131.29* 173 .04 * 88 .9059 65.38 91.22

Source: Pure and Applied Chemistry , 51, 405 (1979 ). By permission . Value s are considered reliable to ± I in the last digit or ± 3 when followed by an asterisk(*). Values in parentheses are used for radioactive elements whose atomic weight s cannot be quoted precisel y without knowledge of the origin of the elements; the value given is the atomic mass number of the isotope of th at element of longest known half-life.

FUNDAMENTAL CONSTANTS (approximate values; best values are in Appendix IV)

!

,

Quantity

Symbol

Value

Gas constant Zero of the Celsius scale Standard atmosphere Standard molar volume of ideal gas A vogadro constant Boltzmann constant Standard acceleration of gravity Elementary charge Faraday constant Speed of light in vacuum Planck constant

R

8.314 J K- 1 mol-I

To

273.15 K 1.013 x 105 Pa 22.41 x 10- 3 m3 mol-I

Rest mass of electron Permittivity of vacuum

Bohr radius Hartree energy

Po

Vo

RTolpo

=

6.022 x 1023 mol I 1.381 x 10- 23 J K- 1 9.807 m s -2 e

F c Il Ii

=

=

NAe

h121T'

In

en

41T'eo 1/41T'eo ao = 41T'eoIi2/me2 Eh = el l41T'e oao

1.602 9.648 2.998 6.626 1.055 9.110 8.854 LIB 8.988 5.292 4.360

'>\.

X

x x X

X '>\.

X

x x x:

10 19 C 104 C mol-I lOR m s I 10 34 J s 10- 34 J s 10- 31 kg 10- 12 C2 N- 1 m 2 10- 10 C 2 N- I m -2 109 N m 2 C- 2 10 II m 10 I~ J

"-

CONVERSION FACTORS

i

I

1 L = 10- 3 m' (exactly) = 1 dm 3 I atm = 1.01325 Pa (exactly) I atm = 760 Torr (exactly) 1 Torr = 1.000 mmHg 1 cal = 4.184 J (exactly) 1 erg = 1 dyne cm = 10- 7 J (exactly) 1 eV = 96.48456 kJ/mol

1 A = 10 10 m = 0.1 nm = 100 pm I inch = 2.54 cm (exactly) 1 pound = 453.6 g I gallon = 3.785 L 1 Btu = 1.055 kJ I hp = 746 W

MATHEMATICAL DATA 1T =

e = 2.7182818 ...

3.14159265 ...

In x = 2.302585 ... log x

(all x) In I

+

x)

=x

-

Y~x"

+

x )-1

- X

(l -

x )-1

+

(I -

X)-"

+ 2x +

(l

+

X

+ +

IA\"3 -

Y4X 4

+

(x"

x" -

X3

+

(x~

<

X~

X3

+

(x"

< I)

+

3x~

+

4x 3

+ ...

(x"

< 1)

I)

<

1)

51 PREFIXES Submultiple

Prefix

Symbol

Multiple

Prefix

Symbol

10- [

deci

d

10

deca

da

10- 2

centi

c

10"

hecto

h

10- 3 10- 6

milli

m

10 3

kilo

k

mIcro

11..

106

mega

M

nano

1}

109

giga

G

pico

10 12

tera

T

femto

P f

10

peta

P

atto

a

10 18

exa

E

10- 9 10- [2 10 15 10 - IR

15

Physical Chemistry

Third Edition

Gilbert W. Castellan University of Maryland

"'

...

Addison-Wesley Publishing Company Reading, Massachusetts

Menlo Park, California

•

London

•

Amsterdam

•

Don Mills, Ontario

•

Sydney

To Joan and our family

Sponsoring Editor: Robert L. Rogers Production Editor: Margaret Pinette Copy Editor: Jerrold A. Moore Text Designer: Debbie Syrotchen Design Coordinator: Herb Caswell Illustrators: YAP International Communications, Ltd. Cover Designer: Richard Hannus, Hannus Design Associates Cover Photograph: The Image Bank, U. Schiller

Art Coordinator: Joseph K. Vetere

Production Manager: Herbert Nolan The text of this book was composed in Monophoto Times Roman by Composition House Limited.

Reprinted with corrections, November 1983

Copyright © 1 983 , 1 97 1 , 1 964 by Addison-Wesley Publishing Company, 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, or otherwise, without the prior written permission of the publisher. Printed in the United States of America. Published simultaneously in Canada. Library of Congress Catalog Card No. 82-74043 . ISBN 0-201-10386-9

BCDEFGHIJ -MA-89876543

m

Foreword to the Student

On most campuses the course in physical chemistry has a reputation for difficulty. It is not, nor should it be, the easiest course available; but to keep the matter in perspective it must be said that the IQ of a genius is not necessary for understanding the subject. The greatest stumbling block that can be erected in the path of learning physical chemistry is the notion that memorizing equations is a sensible way to proceed. Memory should be reserved for the fundamentals and important definitions. Equations are meant to be understood, not to be memorized. In physics and chemistry an equation is not a jumbled mass of symbols, but is a statement of a relation between physical quantities. As you study keep a pencil and scratch paper handy. Play with the final equation from a derivation. If it expresses pressure as a function of temperature, turn it around and express the temperature as a function of pressure. Sketch the functions so that you can "see" the variation. How does the sketch look if one of the parameters is changed? Read physical meaning into the various terms and the algebraic signs which appear in the equation. If a simplifying assumption has been made in the derivation, go back and see what would happen if that assumption were omitted. Apply the derivation to a different special case. Invent problems of your own involving this equation and solve them. Juggle the equation back and forth until you understand its meaning. In the first parts of the book much space is devoted to the meaning of equations; I hope that I have not been too long-winded about it, but it is important to be able to interpret the mathematical statement in terms of its physical content. By all means try to keep a good grasp on the fundamental principles that are being applied; memorize them and above all understand them. Take the time to understand the methods that are used to attack a problem. In Appendix I there is a brief recapitulation of some of the most important mathematical ideas and methods that are used. If any of these things are unfamiliar to you, take the time to review them in a mathematics text. Once the relations

vi

Foreword

between variables have been established, the algebra and calculus are simply mechanical devices, but they should be respected as precision tools. If problems baffle you, learn the technique of problem solving. The principles contained in

G. Polya's book,

How to Solve It, have helped many of my students.*

It is available as a paperback and is well worth studying. Work as many problems as possible. Numerical answers to all problems can be found in Appendix VII. Make up your own problems as often as possible. Watching your teacher perform will not make you into an actor; problem solving will. To aid in this, get a good "scientific" calculator (the serious student will want a programmable one with continuous memory) and learn how to use it to the limit of its capability. Reading the instructions will save you hundreds of hours! Finally, don't be put off by the reputation for difficulty. Many students have enjoyed learning physical chemistry. *

G . Polya,

How to Solve It.

Anchor Book No. 93. New York: Doubleday & Co . , 1 957.

Preface

An introductory course in physical chemistry must expose the fundamental principles that are applicable to all kinds of physicochemical systems. Beyond the exposition of fundamentals, the first course in physical chemistry takes as many directions as there are teachers. I have tried to cover the fundamentals and some applications in depth. The primary aim has been to write a book that the student can, with effort, read and understand; to provide the beginner with a reliable and understandable guide for study in the teacher's absence. I hope that this book is readable enough so that teachers may leave the side issues and the more elementary aspects for assigned reading while they use the lectures to illuminate the more difficult points. Chapters

1, 5, and 6, and most of Chapter 19 contain some general background

material and are intended exclusively for reading. Except where it would needlessly overburden the student, the subject is presented in a mathematically rigorous way. In spite of this, no mathematics beyond the elementary calculus is required. The justification for a rigorous treatment is pedagogical; it makes the subject simpler. The beginner may find it difficult at first to follow a lengthy derivation, but

can

follow it if it is rigorous and logical. Some "simplified"

derivations are not difficult to follow, but impossible.

CHANGES IN THIS EDITION There are several important differences between this edition and the earlier one. I am grateful to Professor James T. Hynes, University of Colorado, who kindly supplied the groups of questions at the end of each chapter. These are an important addition to the book. The questions range in difficulty; some are relatively simple while others challenge the student to take up a line of reasoning from the chapter and apply it beyond the topics that are discussed explicitly. Many new problems have been added; the total is over

750, about twice the number in the second edition. Answers to all

the problems are given in Appendix VII. More worked examples are included; these are now set apart from the text, while before they were sometimes hidden in the

viii

Preface

textual material. A separate solutions manual is in preparation in which representative problems are worked out in detail. Certain sections of the text are marked with a star. The star indicates that the material is either 0) an additional illustration of or a side issue related to the topic under discussion, or (2) a more advanced topic. In the treatment of thermodynamics, some errors have been corrected, some passages clarified, and a few new topics introduced. The emphasis on the laws of thermodynamics as generalizations from experience is maintained. The chapter on electrochemical cells has been revised and a discussion of electrochemical power sources has been added. The chapter on surface phenomena now includes sections on the BET isotherm and on the properties of very small particles. The chapters on the quantum mechanics of simple systems have been retained with only minor revisions, while the chapter on the covalent bond has been extended to include a description of molecular energy levels. The basic ideas of group theory are introduced here and illustrated by constructing symmetry-adapted molecular orbitals for simple molecules. There is a new chapter on atomic spectroscopy; the chapter on molecular spectroscopy has been expanded and reorganized. The treatment of statistical thermodynamics has been extended to include the calculation of equilibrium constants for simple chemical reactions. At the end of the book, new sections on photophysical kinetics, electrochemical kinetics, and a brief chapter on polymers have been added. TERMINOLOGY AND UNITS

With only a few exceptions I have followed the recommendations of the International Union of Pure and Applied Chemistry (IUPAC) for symbols and terminology. I have retained the traditional name, "advancement of the reaction" for the parameter �, rather than''extent of reaction," which is recommended by IUPAC. The connotation in English of the words "advancement" and "advance" when applied to chemical reactions allow a variety of expression that "extent" and its derivatives do not. For thermodynamic work I have retained the sign convention used in the earlier edition. I attempted (unsuccessfully, I thought) to write a clear discussion of the Carnot cycle and its consequences using the alternate sign convention. Then, after examining some other recent books that use the alternate sign convention, I came to the opinion that their discussions of the second law are not distinguished by their clarity. It seems to me that if the subterfuges used in some of these books are· needed for clarity, then the game is not worth the candle. The SI has been used almost exclusively throughout the book. Except for the thermodynamic equations that involve 1 atm or 1 mol/L as standard states (and a few other equations that explicitly involve non-SI units), all the equations in this book have been written in the S1, so that if the values of all the physical quantities are expressed in the correct SI unit, the quantity desired will be obtained in the correct SI unit. The net result is that the calculations of physical chemistry are not just simplified, they are e normously simplified. The student no longer has to assemble and store all the mental clutter that was formerly needed to use many of the equations of physical chemistry. One of the great blessings conferred on the student by the SI is that there is only one numerical value of the gas constant, R. The systematic value of R is the only one used and the only one printed in this book. To those who wish to use any other value, I leave the opportunity to muddle the situation and suffer the consequences.

Preface

ix

ACKNOWLEDGMENTS

In this third edition my aim has been to preserve the best parts of the earlier editions and to improve the others, hoping all the while for the wisdom to know which is which. I have been aided in this by the following individuals who reviewed either the �ntire manuscript or major parts of it. My best thanks go to Professors Irving Epstein, Brandeis University; James T. Hynes, University of Colorado; Paul J. Karol, Carnegie-Mellon University; Lawrence Lohr, University of Michigan; Alden C. Mead, University of Minnesota; Earl Mortenson, Cleveland State University. These reviews were thorough and constructive; the final book owes much to them. I am particularly grateful for their willingness to review a manuscript that was not always in a neat and clean form. My thanks are due to earlier authors in physical chemistry who have shaped my thoughts on various topics. Most particular thanks are due to my first teachers in the subject, Professors Karl F. Herzfeld, Walter J. Moore, and Francis O. Rice. In addition, I am deeply indebted to Professor James A. Beattie for his kind permission to reprint definitions from his book, Lectures on Elementary Chemical Thermody namics. I believe that the influence of this remarkably clear exposition may be noticeable throughout the material on thermodynamics in this book. Chapter 8 , the introduction to the second law, is particularly indebted to Professor Beattie's Lectures. I am grateful to all my colleagues at the University of Maryland who have made suggestions, pointed out errors, responded to my questions, and helped in other ways. Particular thanks go to Professors Raj Khanna and Paul Mazzocchi, who supplied laboratory spectra for illustrations; to Professor Robert J. Munn, who wrote the computer program to construct the index; to Professors Isadore Adler and James M. Stewart, who read and commented on the sections dealing with x-ray spectroscopy and x-ray diffraction; and to Professor E. C. Lingafelter, University of Washington, who was kind enough to write detailed comments on the chapter on x-ray diffraction. Thanks to them a number of errors have been corrected and several passages clarified. Donald D. Wagman and David Garvin of the thermochemistry section of The National Bureau of Standards were most helpful and patient in answering my questions and kindly arranged for me to see a copy of NBS Technical Note 270-8 almost before the ink was dry. Professor D. H. Whiffen, The University, Newcastle-upon-Tyne, was most helpful in correspondence on the use of SI units in quantum mechanics. I wish to express my appreciation to all the teachers, students, and casual readers who have taken the time to write letters with questions, criticisms, and suggestions. The book is much improved as a result of their comments. I �lso wish to thank the editors and producti...