Barron's Chemistry Practice Plus: 400+ Online Questions and Quick Study Review (2022)

Name: Barron's Chemistry Practice Plus: 400+ Online Questions and Quick Study Review (2022)
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Barron's Chemistry Practice Plus: 400+ Online Questions and Quick Study Review (2022) is your go-to practice exam, covering essential topics needed for your certification success.

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© Copyright 2022 by Kaplan North America, LLC, dba Barron’s Educational
Series
Content in this book was previously published in a different format under the
title SAT Subject Test in Chemistry.
All rights reserved under International and Pan-American Copyright
Conventions. By payment of the required fees, you have been granted the
non-exclusive, non-transferable right to access and read the text of this eBook
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without the express written permission of the publisher.
Published by Kaplan North America, LLC, dba Barron’s Educational Series
1515 W Cypress Creek Road
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www.barronseduc.com
ISBN: 978-1-5062-8151-3
10 9 8 7 6 5 4 3 2 1
Kaplan North America, LLC, dba Barron’s Educational Series print books are
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About the Authors
Mark Kernion, M.A.
Mark Kernion, M.A., taught AP, honors, and academic chemistry for 33
years at Mt. Lebanon High School in Pittsburgh, Pennsylvania, and currently
teaches an online AP Chemistry course through PA Homeschoolers and
Chemistry-Prep.com. He received the Yale Teaching Award in 2007, was
inducted into the Cum Laude Society (dedicated to honoring scholastic
achievement in secondary schools) in 2006, and holds a number of patents
related to his research.
Joe Mascetta, M.S., C.A.S.
Joe Mascetta, M.S., C.A.S., taught high school chemistry for 20 years. He
also served as the science department coordinator and principal of Mt.
Lebanon High School in Pittsburgh, Pennsylvania, a science consultant to the
area schools, and was a past president of the Western Pennsylvania
Association of Supervision and Curriculum Development (ASCD) and the
State Advisory Committee of ASCD.

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CONTENTS
How to Use This Book
CHAPTER 1: INTRODUCTION TO CHEMISTRY
Matter
Energy
Conservation of Mass and Energy
Scientific Method
Measurements and Calculations
CHAPTER 2: ATOMIC STRUCTURE AND THE PERIODIC
TABLE OF THE ELEMENTS
Early Atomic Models
Atomic Spectra
Nuclear Transformations and Stability
The Nature of Radioactive Emissions
Methods of Detection of Alpha, Beta, and Gamma Rays
Decay Series, Transmutations, and Half-Life
Nuclear Reactions

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The Wave-Mechanical Model
Electron Configuration
Transition Elements
Periodic Table of the Elements
Properties Related to the Periodic Table
CHAPTER 3: BONDING
Types of Chemical Bonds
Double and Triple Bonds
Resonance Structures
Molecular Geometry—VSEPR and Hybridization
Intermolecular Forces of Attraction
Metallic Bonds
Properties of Differently Bonded Substances
CHAPTER 4: CHEMICAL FORMULAS
Naming and Writing Chemical Formulas
Names and Formulas of Common Acids and Bases
Chemical Formulas: Their Meaning and Use
Laws of Definite Composition and Multiple Proportions
Writing and Balancing Simple Equations
Showing Phases in Chemical Equations
Writing Ionic Equations
CHAPTER 5: GASES AND THE GAS LAWS
General Characteristics of Gases
Gas Laws and Related Problems

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CHAPTER 6: STOICHIOMETRY (CHEMICAL CALCULATIONS)
AND THE MOLE CONCEPT
The Mole Concept
Molar Mass and Moles
Molar Mass and Gas Volumes
Using Molar Mass and Molar Volume
Density and Molar Mass
Stoichiometry: Mole-Mole Problems
Stoichiometry: Mass-Mass Problems
Stoichiometry: Volume-Volume Problems
Stoichiometry: Mass-Volume or Volume-Mass Problems
Problems with an Excess of One Reactant or a Limiting Reactant
Percent Yield of a Product
CHAPTER 7: LIQUIDS, SOLIDS, AND PHASE CHANGES
General Characteristics of Solids, Liquids, and Gases
Important Properties of Liquids
Important Properties of Solids
Types of Solids
Phase Diagrams
Solutions
Colligative Properties of Solutions
CHAPTER 8: CHEMICAL REACTIONS AND
THERMOCHEMISTRY
Thermochemistry
Predicting Reactions

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Determining Changes in Enthalpy
CHAPTER 9: RATES OF CHEMICAL REACTIONS
Factors Affecting Reaction Rates
Activation Energy
Reaction Rate Law
CHAPTER 10: CHEMICAL EQUILIBRIUM
Reversible Reactions and Equilibrium
Le Châtelier’s Principle
Equilibria in Heterogeneous Systems
Common Ion Effect
Driving Forces of Reactions
CHAPTER 11: ACIDS, BASES, AND SALTS
Definitions and Properties
Indicators
Titration-Volumetric Analysis
Buffer Solutions
Salts
Amphoteric Substances
CHAPTER 12: OXIDATION-REDUCTION
Oxidation States
Combustion Reactions
CHAPTER 13: CARBON AND ORGANIC CHEMISTRY
Forms of Carbon

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How to Use This Book
Barron’s Chemistry Practice Plus is designed to offer essential review of key
topics and loads of online practice to help you excel in chemistry.
Online Practice
Access more than 400 questions in online quizzes arranged by topic for
customized practice! All questions include answer explanations.
What Will You Learn in the Book?
Key review and topics are covered so you can study the essentials needed to
succeed.
Learning objectives are listed at the start of each chapter. This list of key
ideas will help guide your learning and study plan and allow you to easily
return to topics that you want to review again.
Examples are included to help support your learning of surrounding topics.
Tips are given throughout the book to offer helpful notes, reminders, and
strategies to improve your learning.

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CHAPTER 1
Introduction to Chemistry
Learning Objectives
In this chapter, you will learn how to:
Distinguish types of matter: i.e., elements, mixtures,
compounds, and pure substances.
Identify chemical and physical properties and changes.
Explain how energy is involved in these changes.
Identify and use the SI units of measurements.
Do mathematical calculations by using scientific notation,
dimensional analysis, and proper significant figures.
Chemistry is the study of matter and how it changes. Changes in matter are
always accompanied by changes in the energy associated with the matter that
is changing. Therefore, chemistry investigates matter and energy as well as
the changes they undergo as processes unfold. A good understanding of both
matter and energy is thus required to understand the world from a chemical
perspective.
Matter

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Matter is defined as anything that occupies space and has mass. Mass is the
quantity of matter that a substance possesses and, depending on the
gravitational force acting on it, has a unit of weight assigned to it. Its formula
is w = mg, where m is the mass of the substance and g is a gravitational
constant. Although weight can vary as the gravitational constant does, the
mass of the body is a constant and can be measured by its resistance to a
change of position or motion. This property of mass to resist a change of
position or motion is called inertia. Since matter does occupy space, we can
compare the masses of various substances that occupy a particular unit
volume. This relationship of mass to a unit volume is called the density of
the substance. It can be shown in a mathematical formula as . The unit
of mass (m) commonly used in chemistry is the gram (g), and of volume (V)
is the cubic centimeter (cm3), milliliter (mL), or liter (L).
TIP
Matter occupies space and has mass.
An example of how density varies can be shown by the difference in the
volumes occupied by 1 gram of a metal, such as gold, and 1 gram of
Styrofoam. Both have the same mass, 1 gram, but the volume occupied by
the Styrofoam is much larger. Therefore, the density of the gold is much
larger than that of the Styrofoam. In chemistry, the typical unit for the density
of solids is grams/cubic centimeter and for that of liquids is grams/milliliter.
Both of these are temperature dependent. The typical unit for the density of
gases is grams/liter at standard temperature and pressure. However, the
density of gases is usually much lower than the densities of solids and
liquids, which is the reason for the unit of liter in the denominator. This
ensures a reasonable amount of mass will be reported for gases. Density is an
important differentiating property of matter. It is a quantitative value that can
be assigned to all matter based on the definition of matter: anything that has
mass and volume.

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TIP
States of Matter
Matter occurs in three states: solid, liquid, and gas. A solid has both a definite
size and a definite shape. A liquid has a definite volume but takes the shape
of the container, and a gas has neither a definite shape nor a definite volume.
These states of matter can often be changed by the addition or subtraction of
heat energy. An example is ice changing to liquid water and finally steam.
Chemical and Physical Properties
Physical properties of matter are those properties that can usually be
observed with our senses. They include everything about a substance that can
be noted when no change is occurring in the type of structure that makes up
its smallest component. Some common examples are physical state, color,
odor, solubility in water, density, melting point, mass, and weight. All of the
properties just listed, except for mass and weight, are independent of the size
of the sample of matter being described and are referred to as intensive. The
intensive nature of a property does not preclude it from being quantitative,
however. Solubility, density, and melting point are examples of intensive
properties. They are measured properties and contain numbers in their
description. Mass and weight are also quantitative properties of matter but
depend on the size of the sample. These types of properties are referred to as
extensive.
Chemical properties are those properties that can be observed in regard to
whether or not a substance changes chemically, often as a result of reacting
with other substances. Some common examples are: iron rusts in moist air,
nitrogen does not burn, gold does not rust, sodium reacts with water, silver
does not react with water, and water can be decomposed by an electric
current.

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