Chemistry An Atoms Focused Approach 3rd Edition PDF Free Download

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Chemistry An Atoms Focused Approach 3rd Edition PDF Free Download Free download contains the content in its entirety. Chemistry An Atoms Focused Approach 3rd Edition PDF ebook was not written to impress you but to help you understand the fundamentals of chemistry easily. This book is a complete course that can help you learn chemistry very quickly.

Chemistry An Atoms Focused Approach 3rd Edition is a book that offers the highest quality content. It is written in a manner that facilitates understanding for both students and instructors. Chemistry An Atoms Focused Approach 3rd Edition contains careful reading from cover to cover and offers engaging material in which readers can find real meaning regarding their daily life.

Chemistry An Atoms Focused Approach 3rd Edition PDF Free Download

Chemistry An Atoms Focused Approach 3rd Edition is a book written by Edward R. Gillespie, David R. Shoenberg and Susan E. DeLong. This book has been published by Pearson Prentice Hall in 2011. The book has 13 chapters with the total number of pages being 856. Chemistry An Atoms Focused Approach 3rd Edition provides the reader with a thorough and in-depth understanding of chemical principles that have been applied to everyday life. The book also provides readers with an opportunity to learn about chemical reactions that occur within various systems, including living organisms and non-living matter.

The book starts by introducing readers to different types of atoms, including carbon atoms as well as hydrogen atoms. It then goes on to explain how these atoms are made up of smaller subatomic particles such as protons, neutrons and electrons. The second chapter discusses how these particles can join together to form molecules while offering examples of different types of molecules such as water molecules which consist of two hydrogen atoms bonded together with one oxygen atom (H2O).

Chemistry An Atoms Focused Approach 3rd Edition PDF Free Download

Introduction

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Chemistry An Atoms First Approach

Chemistry An Atoms First Approach is a comprehensive text that uses the concept of “atoms” as the fundamental building block of matter to introduce basic concepts such as chemical formulas, stoichiometry, periodic trends and bonding. The book begins with an introduction to atoms, ions and electron configurations. It then covers atomic structure including protons, neutrons and electrons, electron orbitals and shells; covalent bonding including ionic vs covalent bonds; molecular geometry including VSEPR theory and Lewis structures; Lewis diagrams; chemical bonding using orbital hybridization; acid-base reactions involving proton transfer; oxidation-reduction reactions involving electron transfer between molecules or atoms (the most common type of redox reaction); thermochemistry including enthalpy changes under various conditions such as standard state at 25°C (298 K), pressure at 1 atmosphere (101 kPa), molar heat capacity at constant volume (ΔHvap), molar heat capacity at constant pressure (ΔHconstp) and entropy change for pure substances undergoing these types of reactions

About the Author

Thomas Holme is a professor at Iowa State University, where he has taught chemistry for more than 35 years. He received his B.S. in chemical engineering from Caltech and his Ph.D. in physical chemistry from Stanford University under the direction of Professor Richard Zare. Dr. Holme is an associate editor for the Journal of Chemical Education, a fellow of the American Chemical Society and served on its Council from 1993-1995; he was also president of The Midwest Section (1997) and chairperson of the national awards program that same year (ACS Divisional Award). Dr. Holme has published over 100 journal articles, but this one stands out as one that students often ask him about: “Chemistry An Atom Focused Approach.”

What Is New In The Third Edition?

The third edition of Chemistry: An Atoms Focused Approach is available in three formats: hardcover, ebook, and PDF. The book was published in 2018 by Cengage Learning and is written in English. It was first published in 2010 as a second edition but has been revised and updated for this third edition. It is part of the Chemistry series, which also includes other books such as Chemistry: An Introduction to General Organic and Biochemistry 13th Edition (Cengage Learning).

Table of Contents

  • Chapter 1 The Atom
  • Chapter 2 Chemical Nomenclature and Formulas
  • Chapter 3 Chemical Reactions
  • Chapter 4 Stoichiometry
  • Chapter 5 Gas Laws and Their Role in Chemistry
  • Chapter 6 Modern Atomic Theory & the Periodic Table with Electrons in Atoms

Chapter 1 The Atom

The atom is the smallest particle of an element that exists. It consists of three subatomic particles: protons, neutrons, and electrons.

The number of protons in an atom’s nucleus defines its atomic number; the more protons an atom has, the higher its atomic number will be. The total number of protons and neutrons defines an element’s mass; atoms with equal numbers of protons but differing numbers of neutrons are called isotopes. Isotope notation uses superscripts to indicate how many times heavier or lighter than normal a given isotope is compared to carbon-12 (the reference standard). For example, carbon-12 has six protons and six neutrons; methane contains one carbon atom with four neutrons and four hydrogen atoms each having one proton—CH4

Chapter 2 Chemical Nomenclature and Formulas

  • 1 Naming simple ionic compounds
  • 2 Naming simple molecular compounds
  • 3 Formulas of simple ionic compounds and their charges, identity and valence electrons, electronegativities of atoms, and number of valence electrons
  • 4 Formulas of simple molecular compounds, molecular mass, molecular formula mass and the molar mass (molarity)

Chapter 3 Chemical Reactions

The mole is used in stoichiometry to express, relate and compare the amounts of substances involved in a reaction. For example, if:

  • The molecular formula for sodium chloride, Nacl, is NaCl
  • The percentage by mass of sodium (Na) in Nacl is 23%

then:

  • When 0.5 mole of NaCl reacts with excess water to form liquid sodium hydroxide (lye), the amount of product formed will be 0.5 mole of lye and 0.5 mole of solid (sodium hydroxide).
  • If we want to calculate how many moles are consumed when 0.1 mole of Nacl reacts with excess water to form liquid sodium hydroxide (lye), then:

Chapter 4 Stoichiometry

In this chapter, you will learn about the definitions of stoichiometry and stoichiometric calculations. You will also be able to calculate reactant amounts from product amounts, or vice versa. You can then use these methods to solve problems involving solutions and mixtures with varying amounts of dissolved substances.

The best way to think about stoichiometry is as a set of rules that govern how reactions occur (and what happens when they do). These rules are built on mathematical equations that help predict whether or not different compounds will mix together in certain ratios based on their relative masses or volumes. Strictly speaking, these equations apply only to reactions that happen at constant temperature and pressure—meaning you’ll need some basic thermodynamics knowledge before diving into them too deeply!

Chapter 5 Gas Laws and Their Role in Chemistry

This chapter introduces gas laws and their role in chemistry. Gas laws are used to describe the behavior of gases under different conditions, such as changes in temperature or pressure. The first two chapters have taught you how to calculate the number of moles and grams (mass) of a substance from its atomic mass unit (amu). In this chapter, you will use your knowledge of the mole concept to understand how gases behave under different conditions.

The three most basic gas laws are Boyle’s law, Charles’ law, and the ideal gas law. These three laws can be combined into an equation called the ideal gas law that offers a precise description o f many aspects o f gas behavior over wide ranges o f pressure, temperature and volume changes at constant concentration. However , it is important to note that real gases do not obey all these rules exactly; they only approximate them well enough for us t o approximate certain physical phenomena with accuracy sufficient for everyday life needs .

In addition to being very useful in understanding various chemical processes , knowing some common relationships between variables like pressure or volume can help you solve problems quickly when it comes time for test day!

Chapter 6 Modern Atomic Theory

Chapter 6: Modern Atomic Theory

The goal of this chapter is to discuss the atomic theory in terms of quantum mechanics. In this section, you will learn about the experiments that led to modern atomic theory and how they were used to explain atoms. You will also learn about some important concepts such as quantum numbers, sublevels and electron spin that are important for understanding atoms.

Quantum numbers—the three quantum numbers used for labeling orbitals; principal quantum number (n), azimuthal quantum number (ℓ), magnetic quantum number (m)

Sublevels—different subshells/sublevels with different energies and corresponding orbital configurations

Electron spin—spin ½ fermions with two possible spin states; up or down

Chapter 7 The Periodic Table, Periodicity, and Electrons in Atoms

Chapter 7: The Periodic Table, Periodicity, and Electrons in Atoms

The periodic table of the elements is a chart that organizes all known chemical elements into a neat grid. Each row of the table contains one group (column) of elements with similar properties. In this chapter you will learn how the periodic table is arranged and what periodicity means. You will also learn about electrons and how they are arranged in atoms to make an atom complete (neutral). Finally we’ll look at atomic number and its relationship to mass, charge, electron configuration, characteristic properties and valence shell electrons (the number of outermost electrons).

Chapter 8 Ionic Bonding and Simple Ionic Compounds

In this chapter, you will learn about the bonding of ions and simple ionic compounds. You will learn about the electron arrangements in atoms that make up an ion and how those arrangements can be represented with Lewis structures. You can see examples of electron configurations for some common ions in Figure 8-1. An important concept related to electrons is the octet rule: Atoms tend to gain or lose electrons until they have eight valence electrons (or valence shells) filled around their nuclei; this reduces their overall energy by stabilizing their outermost electrons with fewer bonds between them. The most common way atoms achieve this goal is through covalent bonding rather than ionic bonding, but there are exceptions: some elements form polyatomic ions because they require more than eight valence electrons to complete their outermost shell!**END OF SECTION

Chapter 9 Covalent Bonding and Simple Molecular Compounds

Covalent Bonding and Simple Molecular Compounds

In this chapter, we will focus on covalent bonding in which nonmetals share electrons. In addition to carbon compounds, you will study the bonding of hydrogen and oxygen in water.

Chapter 10 Quantitative Information from Chemical Equations – Thermochemistry

In this chapter, we will learn about the quantitative information that can be obtained from chemical equations. The first part of the chapter is devoted to thermochemistry, which is a branch of chemistry that deals with heat and its relationship to chemical reactions. Thermochemistry covers topics such as:

  • Theories of chemical reactions
  • Theories of heat (the First Law)
  • Calorimetry – A method for determining the amount of energy released or absorbed during a reaction by measuring temperature changes in a system at constant pressure.
  • Hess’ Law – States that when two similar chemical species are involved in the same reaction at different concentrations, their enthalpies change by the same amount per mole regardless of how much each contributes to the overall enthalpy change for the overall system

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Conclusion

This book is for students who have been away from chemistry for some time and may not remember much about it. It is also suitable for those who are currently taking their first course in chemistry or are looking to refresh their understanding of the subject. I hope that this book will be of use to you no matter what your background is, but if you want something more advanced then this might not be the right choice.

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