|
Published:
April 17, 2017

Chemistry Workbook For Dummies with Online Practice

Overview

Take the confusion out of chemistry with hundreds of practice problems

Chemistry Workbook For Dummies is your ultimate companion for introductory chemistry at the high school or college level. Packed with hundreds of practice problems, this workbook gives you the practice you need to internalize the essential concepts that form the foundations of chemistry. From matter and molecules to moles and measurements, these problems cover the full spectrum of topics you'll see in class—and each section includes key concept review and full explanations for every problem to quickly get you on the right track. This new third edition includes access to an online test bank, where you'll find bonus chapter quizzes to help you test your understanding and pinpoint areas in need of review. Whether you're preparing for an exam or seeking a start-to-finish study aid, this

workbook is your ticket to acing basic chemistry.

Chemistry problems can look intimidating; it's a whole new language, with different rules, new symbols, and complex concepts. The good news is that practice makes perfect, and this book provides plenty of it—with easy-to-understand coaching every step of the way.

  • Delve deep into the parts of the periodic table
  • Get comfortable with units, scientific notation, and chemical equations
  • Work with states, phases, energy, and charges
  • Master nomenclature, acids, bases, titrations, redox reactions, and more

Understanding introductory chemistry is critical for your success in all science classes to follow; keeping up with the material now makes life much easier down the education road. Chemistry Workbook For Dummies gives you the practice you need to succeed!

Read More

About The Author

Christopher Hren is a high school chemistry teacher and former track and football coach. Peter J. Mikulecky, PhD, teaches biology and chemistry at Fusion Learning Center and Fusion Academy.

Sample Chapters

chemistry workbook for dummies with online practice

CHEAT SHEET

Getting through a chemistry class involves a range of science skills and procedures. You use exponential and scientific notation, analyze atomic structures, name compounds, convert to and from moles, and draw Lewis dot structures. Is there anything you don't do in chemistry?Basic exponential and scientific notation used in chemistryIn chemistry, you often use exponential notation, which is simply using exponents to express a number.

HAVE THIS BOOK?

Articles from
the book

In real-life chemical reactions, not all of the reactants (substances present at the start of a chemical reaction) convert into product. More typically, one reagent (what is added to cause or test for a chemical reaction) is completely used up, and others are left in excess, perhaps to react another day. The reactant that is used up is the limiting reagent.
A solid understanding of molality helps you to calculate changes in boiling and freezing points. In the same way, a solid understanding of boiling point elevation and freezing point depression can help you determine the molecular mass of a mystery compound that's being added to a known quantity of solvent.Boiling point elevationrefers to the tendency of a solvent's boiling point to increase when an impurity (a solute) is added to it.
Getting through a chemistry class involves a range of science skills and procedures. You use exponential and scientific notation, analyze atomic structures, name compounds, convert to and from moles, and draw Lewis dot structures. Is there anything you don't do in chemistry?Basic exponential and scientific notation used in chemistryIn chemistry, you often use exponential notation, which is simply using exponents to express a number.
In the world of chemistry, not all acids and bases are created equally. Some have an innate ability to neutralize more effectively than others.Consider hydrochloric acid (HCl) and sulfuric acid (H2SO4), for example. If you mixed 1 M sodium hydroxide (NaOH) together with 1 M hydrochloric acid, you'd need to add equal amounts of each to create a neutral solution of sodium chloride (NaCl) and water (H2O).
In chemistry, you can add and subtract extreme numbers by using exponential notation, and expressing your numbers as coefficients of identical powers of 10. To wrestle your numbers into this form, you may need to use coefficients less than 1 or greater than 10. Adding with exponential notation To add two numbers by using exponential notation, you begin by expressing each number as a coefficient and a power of 10.
Chemists aren’t satisfied with measuring length, mass, temperature, and time alone. On the contrary, chemistry often deals in calculated quantities. These kinds of quantities are expressed with derived units, which are built from combinations of base units.Here are some examples: Area (for example, catalytic surface).
Real-life chemists in real-life labs don't make every solution from scratch. Instead, they make concentrated stock solutions and then make dilutions of those stocks as necessary for a given experiment.To make a dilution, you simply add a small quantity of a concentrated stock solution to an amount of pure solvent.
When gases mix, each individual gas within the mixture contributes a partial pressure, and adding the partial pressures yields the total pressure. This relationship is summarized by Dalton's law of partial pressures for a mixture of individual gases:This relationship makes sense if you think about pressure in terms of kinetic molecular theory.
Chemists have to be concerned with just how completely their reactants react to form products. To compare the amount of product obtained from a reaction with the amount that should have been obtained, they use percent yield. You determine percent yield of a chemical reaction with the following formula:That's nice and all, but what is an actual yield, and what is a theoretical yield?
If you don't know the empirical formula of a compound, you can analyze samples of the unknown compound to identify the percent composition. From there, you calculate the ratios of different types of atoms in the compound. You express these ratios as the empirical formula. An empirical formula represents the lowest whole-number ratio of elements in a compound.
A conversion factor uses your knowledge of the relationships between units to convert from one unit to another. For example, if you know that there are 2.54 centimeters in every inch (or 2.2 pounds in every kilogram or 101.3 kilopascals in every atmosphere), then converting between those units becomes simple algebra.
When doing math in chemistry, you need to follow some rules to make sure that your sums, differences, products, and quotients honestly reflect the amount of precision present in the original measurements. That’s where significant figures come in.You can be honest (and avoid the skeptical jeers of surly chemists) by taking things one calculation at a time, following a few simple rules.
Boiling point elevation refers to the tendency of a solvent's boiling point to increase when an impurity (a solute) is added to it. In fact, the more solute that is added, the greater the change in the boiling point.Boiling point elevations are directly proportional to the molality of a solution, but chemists have found that some solvents are more susceptible to this change than others.
An important property that you can calculate from molality is freezing point depression. When you add solute to a solvent, it lowers its freezing point. That's why you sprinkle salt on icy sidewalks. The salt mixes with the ice and lowers its freezing point.If this new freezing point is lower than the outside temperature, the ice melts, eliminating the spectacular wipeouts so common on salt-free sidewalks.
Many calculations that you make in chemistry will involve unit conversions (for example, between meters and millimeters, or between meters and inches). Fortunately, you don’t need to know all possible unit conversions.Instead of memorizing or looking up conversion factors between all types of units, you can memorize just a handful of conversion factors and use them one after another, letting the units guide you each step of the way.
For the chemist, Hess's law is a valuable tool for dissecting heat flow in complicated, multistep reactions. For the confused or disgruntled chemistry student, Hess's law is a breath of fresh air. In essence, the law confirms that heat behaves the way we'd like it to behave: predictably.Imagine that the product of one reaction serves as the reactant for another reaction.
To make it easier to work with extreme numbers, chemists turn to scientific notation, which is a special kind of exponential notation. A major benefit of presenting numbers in scientific notation is that it simplifies common arithmetic operations like multiplication and division. Multiplying in scientific notation To multiply two numbers written in scientific notation, you work out the coefficients and the exponents separately.
Different gases diffuse at different rates, depending on their molar masses. You can compare the rates at which two gases diffuse using Graham's law. Graham's law also applies to effusion, the process in which gas molecules flow through a small hole in a container. Diffusion is the movement of a substance from an area of higher concentration to an area of lower concentration.
Many compounds in nature are composed of atoms that occur in numbers that are multiples of their empirical formula. In other words, their empirical formulas don't reflect the actual numbers of atoms within them; instead, they reflect only the ratios of those atoms. What a pain!Fortunately, this is an old pain, so chemists have devised a means to deal with it.
Like the difference in their names, the practical difference between molarity and molality is subtle. Take a close look at their definitions, expressed next to one another in the following equations:The numerators in molarity and molality calculations are identical, but their denominators differ greatly. Molarity deals with liters of solution, while molality deals with kilograms of solvent.
https://cdn.prod.website-files.com/6630d85d73068bc09c7c436c/69195ee32d5c606051d9f433_4.%20All%20For%20You.mp3

Frequently Asked Questions

No items found.