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

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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    BARRON'S Chemistr Sy Practice Plus WITH QUICK REVIEW GUIDE B \ FA \ | nN & \ MARK C. KERNION, M.A., axp JOSEPH A. MASCETTA, MS. + StudyXY

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    Downloaded from StudyXY.com ® + StudyXY Sd Ye. o> \ | iF ’ pr E \ 3 S Stu dy Anything This ContentHas been Posted On StudyXY.com as supplementary learning material. StudyXY does not endrose any university, college or publisher. Allmaterials posted are under the liability of the contributors. wv 8) www.studyxy.com

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    Scan how = Lied to access practice included with this book, or goto online.barronsbooks.com BARRON'S

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    Chemistry Practice Plus

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    Dedication To my wife, Patty; children, Emily, Sam, and Ben; granddaughters, Stella and Clare; grandson, Nate; son-in-law, Rob; and daughter-in-law, Aly —M. Kernion To my wife, Jean; daughters, Lisa, Linda, and Lori; and their families, who supported my efforts throughout the years —J. Mascetta

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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 on screen. No part of this text may be reproduced, transmitted, downloaded, decompiled, reverse engineered, or stored in or introduced into any information storage and retrieval system, in any form or by any means, whether electronic or mechanical, now known or hereinafter invented, without the express written permission of the publisher. Published by Kaplan North America, LLC, dba Barron’s Educational Series 1515 W Cypress Creek Road Fort Lauderdale, FL 33309 www.barronseduc.com ISBN: 978-1-5062-8151-3 10987654321 Kaplan North America, LLC, dba Barron’s Educational Series print books are available at special quantity discounts to use for sales promotions, employee premiums, or educational purposes. For more information or to purchase books, please call the Simon & Schuster special sales department at 866-506- 1949.

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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 Chatelier’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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    Organic Chemistry Hydrocarbons Hydrocarbon Derivatives CHAPTER 14: THE LABORATORY The Ten Commandments of Lab Safety Some Basic Setups

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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: o Distinguish types of matter: i.e., elements, mixtures, compounds, and pure substances. o Identify chemical and physical properties and changes. o Explain how energy is involved in these changes. o Identify and use the SI units of measurements. o 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 D = c 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 oo, Mass Densfty.= Volume States of Matter Matter occurs in three states: solid, liquid, and gas. A selid 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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