Author: Ralph H. No part of this book may be reproduced, in any form or by any means, without permission in writing from the publisher. The deepest, without question, are to our wives, Sanny Chan and Cornelia Bica, not only for tolerating with good cheer our extended absences from the home during the twelve-month period over which the manual was prepared, but also for carefully poring over the chapters and finding errors that had eluded the authors and all of the other accuracy checkers.
Our wives, above all others, are glad to see the ordeal end and normal family life return. We must commend Dr. David Shim for the tremendous effort he put into thoroughly checking each and every solution in the manual. Put simply, David Shim's comments and corrections were invaluable to us. Also lending enormous assistance was Dr. Ralph Petrucci. During the course of the project, we asked Dr.
Petrucci innumerable questions, some of a highly complex nature, and, each and every time, he expeditiously fired us back a comprehensive answer. Hats off to you Ralph for a job well done! P Some help with proofreading and keying in corrections was provided by Dr. Dusan RisticPetrovic. We thank Dr. Geoff Hemng for providing us with a solution to Question 87 in Chapter Not sure? What mass of lithium chloride is formed? Argon is the heaviest atom. The heaviest element in group one is also the lightest element in period 3.
The lightest gaseous element is He. The heaviest gaseous element is Cl2. The heaviest element in group 18 is also the heaviest element in period 1. Which of the following statements is correct? H, Li and Na all have the same number of electrons. Bromine exists as a diatomic compound, ie. How many different Br2 molecules are possible and what are their masses?
The ion marked A is lighter than the ion marked B. The ion marked A is the lightest isotope of Hg. Given the diagram below, which of the following statements is incorrect? Without doing detailed calculations and using the periodic table to the right, which of the following samples contain the least number of atoms? Without using a calculator, estimate the number of Hg atoms in a mL sample. Given that naturally occurring diamond has density 0f 3.
Slide 60 of Then, we introduce atomic theory, including the periodic table, in Chapter 2. The periodic table is an extraordinarily useful tool, and presenting it early allows us to use the periodic table in different ways throughout the early chapters of the text. In Chapter 3, we introduce chemical compounds and their stoichiometry. Organic compounds are included in this presentation. The early introduction of organic compounds allows us to use organic examples throughout the book.
Chapters 4 and 5 introduce chemical reactions. We discuss gases in Chapter 6, partly because they are familiar to students which helps them build confidence , but also because some instructors prefer to cover this material early to better integrate their lecture and lab programs.
Chapter 6 can easily be deferred for coverage with the other states of matter, in Chapter In Chapter 7, we introduce thermochemistry and discuss the energy changes that accompany physical and chemical transformations. Chapter 8 introduces quantum mechanical concepts that are needed to understand the energy changes we encounter at the atomic level.
Collectively, Chapters 8 through 11 provide the conceptual basis for describing the electronic structure of atoms and molecules, and the physical and chemical properties of these entities.
The properties of atoms and molecules are then used in Chapter 12 to rationalize the properties of liquids and solids. Chapter 13 is a significant revision of Chapter 19 from the tenth edition. It introduces the concept of entropy, the criteria for predicting the direction of spontaneous change, and the thermodynamic equilibrium condition.
Moreover, many topics in these chapters can be covered selectively, without requiring the study of entire chapters. The text ends with comprehensive chapters on nuclear chemistry Chapter 25 and organic chemistry Chapters 26 and Please note that an additional chapter on biochemistry Chapter 28 is available online. Atomic mass intervals are recommended by the IUPAC because the isotopic abundances of these elements vary from one source to another, and therefore, their atomic masses cannot be considered constants of nature.
For example, standard enthalpies of reaction are represented by the symbol not and are expressed in kJ mol not kJ. We have added a molecular interpretation of specific heat capacities in Section and an introduction to entropy in Section Sections and of the previous edition have been combined and the material reorganized. This chapter includes a new section that focuses on the energy level diagram and spectrum of the hydrogen atom. The section entitled Interpreting and Representing the Orbitals of the Hydrogen Atom has been rewritten to include a discussion of the radial functions.
A new subsection describing the conceptual model for multielectron atoms has been added to the section entitled Multielectron Atoms.
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