Chemistry
Description
Master the fundamentals of chemistry with this fast and easy guide. Chemistry is a fundamental science that touches all other sciences, including biology, physics, electronics, environmental studies, astronomy, and more. Thousands of students have successfully used the previous editions of Chemistry: Concepts and Problems, A Self-Teaching Guide to learn chemistry, either independently, as a refresher, or in parallel with a college chemistry course. This newly revised edition includes updates and additions to improve your success in learning chemistry.
This book uses an interactive, self-teaching method including frequent questions and study problems, increasing both the speed of learning and retention. Monitor your progress with self-tests, and master chemistry quickly. This revised Third Edition provides a fresh, step-by-step approach to learning that requires no prerequisites, lets you work at your own pace, and reinforces what you learn, ensuring lifelong mastery.
* Master the science of basic chemistry with this innovative, self-paced study guide
* Teach yourself chemistry, refresh your knowledge in preparation for medical studies or other coursework, or enhance your college chemistry course
* Use self-study features including review questions and quizzes to ensure that you're really learning the material
* Prepare for a career in the sciences, medicine, or engineering with the core content in this user-friendly guide
Authored by expert postsecondary educators, this unique book gently leads students to deeper levels and concepts with practice, critical thinking, problem solving, and self-assessment at every stage.
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CHAD SNYDER is Professor of Chemistry at Liberty University where he teaches organic, inorganic, general, and forensic chemistry. He authors end-of-chapter problems and test bank questions for a variety of chemistry titles and frequently serves as a subject matter expert in chemistry.
CLIFFORD HOUK was Professor of Health Science at Ohio University. He held a doctoral degree in inorganic chemistry, and was a fellow of the American Industrial Hygiene Association (AIHA). Dr. Houk co-authored the first two editions of Chemistry: A Self-Teaching Guide.
Content
Introduction xi
Acknowledgments xiii
How to Use This Book xvi
1 Atomic Structure, Periodic Table, Electronic Structure 1
2 Atomic Weights 27
3 Periodic Properties and Chemical Bonding 47
4 Molecular and Formula Weights 79
5 Nomenclature 105
6 Chemical Equations 129
7 Mole Concept 155
8 Gases 167
9 Solids 203
10 Liquids 223
11 Solutions and Their Properties 245
12 Chemical Equilibrium 277
13 Acids and Bases 317
14 Organic Chemistry 355
Appendix
Table of Atomic Weights 400
Periodic Table of the Elements 401
Table of Four-Place Logarithms 402
Index 405
1
Atomic Structure, Periodic Table, Electronic Structure
There is a smallest unit of substance. This smallest unit may be only a single atom or a group of atoms chemically joined together.
This chapter deals with the structure of the atom, which is the very backbone of chemistry. In this chapter we introduce the three basic subatomic particles in an atom, their arrangement in the atom, and the similarities of this arrangement revealed by the position of the elements in the periodic table. A clear understanding of this chapter will give you a sound basis for learning chemistry.
OBJECTIVES
After completing this chapter, you will be able to
- define, describe, or illustrate: proton, neutron, electron, atom, nucleus, atomic number, shell, orbital, subshell, alkali metal, noble gas, halogen, alkaline earth, period, group, family, oxide, ductile, malleable, metal, nonmetal, metalloid, and Bohr model of an atom;
- determine the numbers of protons, neutrons, and electrons in a neutral atom when given its mass number and atomic number;
- compare and contrast the three fundamental particles in an atom according to mass and charge;
- determine the maximum number of electrons any given shell can hold;
- determine the maximum number of orbitals in any given shell;
- write the electron configuration for any element;
- determine what element is represented when given its electron configuration;
- use the periodic table to locate different families of elements and determine whether an element is a metal, nonmetal, or metalloid.
An atom, the smallest unit of an element, is composed primarily of three fundamental particles: electrons, protons, and neutrons. The combination of these particles in an atom is distinct for each element. An atom of the element radon is composed primarily of a specific combination of what three basic particles?_____________
Answer: electrons, protons, neutrons (any order)
Let's forget about neutrons for the moment and consider just electrons and protons. Each atom of the same element has the same combination of protons and electrons. An atom of the element hydrogen in outer space has (the same, a different) __________ combination of electrons and protons as that of an atom of hydrogen on earth.
Answer: the same
Each element has a unique combination of protons and electrons in its atoms. The combination of electrons and protons in an atom of one element is different from that in an atom of any other element. Since each element has a known unique number of protons and electrons in its atoms, would it be possible to identify an element if you know the number of protons and electrons in its atoms? __________
Answer: yes (if you could compare the number of electrons and protons in your unknown atom with a list of the electrons and protons in atoms of each known element)
Protons are particles with a positive (plus) charge. Electrons are particles with a negative (minus) charge. Unless otherwise stated, an atom is assumed to be neutral, with the positive and negative charges being equal. In any neutral atom, the number of electrons (having a negative charge) is always equal to the number of protons (having a positive charge).
An oxygen atom contains eight protons. We assume the atom to be neutral. How many electrons must it have? _________
Answer: eight
An atom contains 10 electrons. How many protons does it contain? _________
Answer: 10
Each element has a unique number of electrons and protons in its atoms. Since the number of electrons in a neutral atom is equal to the number of protons, do you think we can identify an element if we know just the number of protons in its atoms? _________
Answer: yes (if we could compare the number of protons in an atom of the unknown element with a list or table of the number of protons in atoms of every known element)
The periodic table is a very useful table describing the atoms of every known element. A complete periodic table is included in Appendix (see page 399) of this book. Each box in the periodic table represents an element. The one- or two-letter symbol in each box is a shorthand notation used to represent a neutral atom of an element. The symbol "C" represents a neutral atom of the element carbon. The symbol "He" represents a neutral atom of the element helium.
The number of protons in an atom is listed above each symbol. (Ignore the number underneath the symbol, called the "atomic weight," for the time being as you will get this information from the periodic table. More on that to come.)
An atom of carbon has six protons. How many protons does an atom of helium have? _________
Answer: two
Note: The table of atomic weights, located in the Appendix along with the periodic table, lists all the elements alphabetically and gives the symbol for each. (Ignore the atomic weights for now.) You'll be using the periodic table and the table of atomic weights throughout this book.
The number of protons in an atom of an element is called its atomic number. What is the atomic number of the element helium (He)? ___________
Answer: 2
The element iron (Fe) has an atomic number of 26. How many protons does an atom of iron contain? _______
Answer: 26
A neutral atom of iron contains how many electrons? _________
Answer: 26 (the same as the number of protons)
Using the periodic table, determine the number of electrons in a neutral atom of zinc (Zn). _______
Answer: 30 (the same as the number of protons)
BOHR ATOMIC MODEL
A Danish physicist, Niels Bohr, came up with a model that pictured the atom with a nucleus of protons in the center and electrons spinning in an orbit around it (similar to the movement of the planets around the sun). The following Bohr model contains one orbiting electron and a nucleus of one proton.
What is the atomic number of the element represented? _________
What element is represented? _________
Answer: 1 (The atomic number equals the number of protons.); hydrogen (H)
An electron always carries a negative charge. A proton carries a charge exactly opposite that of the electron. A proton must therefore have a (negative, positive, neutral) ___________ charge.
Answer: positive
An electron has very little mass when compared to a proton. It takes about 1836 electrons to equal the weight of just one proton. In a hydrogen atom consisting of just one proton and one electron, the greatest proportion by weight is accounted for by the (electron, proton) _________.
Answer: proton (The proton accounts for about 99.95% of the weight of a hydrogen atom and the electron 0.05%.)
The element helium (He), represented by the Bohr model below, has an atomic number of _______.
Answer: 2
The neutralatom of He contains how many protons? _______
How many electrons? _______
Answer: two; two
The weight of an atom of helium is not totally accounted for by the protons and electrons. A third subatomic particle, the neutron, is responsible for the additional weight. The neutral atoms of all elements except the most common form of the element hydrogen have one or more neutrons in the nucleus of their atoms. The diagram below shows the neutrons in the corrected Bohr model of helium.
Since a neutral atom contains equal numbers of negatively charged electrons and positively charged protons, what type of electrical charge do you think is possessed by a neutron? ____________ (negative, positive, no charge)
Answer: no charge (The name neutron means a neutral particle.)
A neutron is slightly heavier than a proton. Of the primary fundamental particles in an atom:
- which is the lightest in weight? _________
- which is the heaviest? _________
- which is between the other two in weight? _________
Answer: (a) the electron; (b) the neutron; (c) the proton
In the Bohr model of a lithium atom shown below, which subatomic particle(s) is (are) represented by the circular orbits shown by the larger circles? _________
Which particle(s) make(s) up the nucleus or center of the atom? _________
Answer: electrons; protons and neutrons
If the negative charge of an electron is represented by -1, the charge on the proton would be (-1, +1, neutral) _______ and the charge on the neutron would be (-1, +1, neutral) _______.
Answer: +1; neutral
Neutrons can be found in all atoms of all elements except the most common form of the simplest element. Identify that element. _______ (Hint: If you don't remember, reread frame 17.)
Answer: hydrogen
You have just learned the names, charges, and relative sizes of the fundamental particles that constitute an atom. You have also been shown one model representing the arrangement of these particles in an atom.
We have referred you to the periodic table and hinted that...
