Chemistry, 2nd Edition

In this first episode, Professor Cardulla explains how any student can find success in chemistry by cultivating a meaningful understanding of the concepts and quantitative thinking operations that underlie this often challenging area of study.

Introductory chemistry is not mysterious: It requires simple quantitative reasoning that comes naturally to most students. You learn about the types of numbers involved in chemistry and how to solve problems commonly encountered in high school chemistry.

Only a handful of important ideas must be mastered in order to be successful at solving chemistry problems. In this episode, you review some basic guidelines for approaching any chemistry problem and try out your skills on a few sample problems that demonstrate how you can use everyday reasoning in your chemistry class.

Building on the ideas explored in the first three episodes, you examine a fundamental quantitative measurement in chemistry, density, and explore the real-world meaning of this measurement. You then solidify your understanding of this concept by working some basic density problems.

Continue to lay a strong foundation for your understanding of chemistry by learning about one of the key tools you'll be using: the International System of Units (SI), or the metric system. This episode explains why this system is so useful to scientists and lays out the prefixes and units of measurement that make up the metric system.

Now that you have established an understanding of the SI system, put your knowledge to work as you practice converting units from one system of measurement to another. You hone your conversion skills by working several sample problems.

In this episode, examine the basic building blocks of matter, elements and the atoms that constitute them, and you learn how to interpret the information about elements presented in the periodic table.

Learn about protons, electrons, and neutrons; how ions are formed from atoms; how these ions can combine to form compounds; and how you can determine the formulas of these compounds. Some molecular substances are discussed and you are introduced to the final number associated with every element: its atomic weight.

Discover how isotopes, which are different atoms of the same element, can actually differ in their weight because they contain different numbers of neutrons in their nuclei. Also, learn how different kinds of elements are grouped into both general categories (such as metals and nonmetals) as well as specific chemical families, which then are arranged into the periodic table.

One of the most important concepts to master in an introductory chemistry course is the concept of the mole, which provides chemists with a way to "count" atoms and molecules. Learn how scientists use the mole and explore the quantitative definition of this basic unit.

In this episode, refine the quantitative techniques introduced in earlier episodes while increasing your familiarity with this important chemical value of mole.

After mastering the mole, move on to a related concept: the "molar volume," or the amount of space occupied by one mole. Apply this understanding of molar volume as you examine Avogadro's Hypothesis, a principle concerning the molar volume of gases.

In this episode, you encounter two "classic" types of chemistry problems and learn the basic characteristics of each. The episode concludes with several practice problems to help you master the skill of solving percent composition problems.

Here, continue your consideration of "classic" chemistry problems with a look at empirical formulas, and examine how empirical formulas relate to molecular formulas.

What happens when you combine two or more elements? Through a variety of practice problems, learn to identify when a chemical reaction has occurred, how to write chemical equations, and how to "balance" equations to conserve the atoms.

What are the quantitative relationships between the substances in a chemical reaction? The study of stoichiometry shows you how to apply your ability to balance equations to solve problems involving chemical reactions.

In this episode, extend your study of stoichiometry to consider more complex problems involving volume, molecules, and energy.

As you move on to more advanced stoichiometry problems, see that they can be solved using a very simple approach. You'll encounter three terms often applied to chemical reactions: theoretical yields, actual yields, and percent yields.

One important idea to master in any introductory chemistry course is the concept of concentration of a solution. Here, you explore this concept; the components that make up a solution; and learn about a basic unit of measurement for concentration, molarity.

Extend your understanding of molarity by solving some typical problems encountered in the high school chemistry classroom. To foster your understanding of these problems, you are asked to draw upon the quantitative reasoning skills you previously used.

Take the concepts you learned about molarity in the last two episodes and apply them to a number of unfamiliar problems. These problems offer an opportunity to test your comprehension of the concepts you've been exploring.

Continue your study of chemical reactions by examining an important new concept: the equilibrium system. Start by looking carefully at the difference between reactions that "go to completion" and those that are "reversible."

By tracking and graphing a hypothetical reaction as it approaches a state of equilibrium, gain a deeper understanding of the essential characteristics of equilibrium systems. Then, you're introduced to the single most important expression used to solve equilibrium problems: the equilibrium constant.

Your examination of the equilibrium constant continues in this episode. Learn exactly what the numerical value for an equilibrium constant tells and doesn't tell you about an equilibrium system.

Before you can solve equilibrium problems, you need to understand what happens to an equilibrium system when conditions are changed. Learn about a fundamental idea, Le Chatelier's Principle, which lays the groundwork for a broader understanding of equilibrium.