Naturally, the AP® Chemistry exam is almost guaranteed to ask you to calculate an empirical formula for at least one substance, if not more. You’ll learn how to make these calculations in this section of the AP® Chemistry Crash Course. Let’s get started!
Welcome to another of our Ultimate AP® Chemistry Guide series! This time, we’re going to teach you all about electrochemistry. We’ll start off with a quick overview of what electrochemical reactions are. Then we’ll go over the terms “oxidation” and “reduction”, what redox reactions are, and how to balance them.
Stoichiometry is one of the most important topics on the AP® Chemistry exam, so it’s vital that you understand it and all of its applications. Stoichiometry derives from the Greek, “stoicheionmetron,” meaning “element measure”. In other words, stoichiometry is the practice of using a chemical reaction equation to predict the results of the reaction. We’ll go into more detail about that later.
Le Chatelier’s Principle, despite its intimidating name, is actually a very simple idea and quite important to AP® Chemistry. It simply means that if a reaction at equilibrium is disturbed in a way that would shift the balance to one side, the reaction will move to restore the equilibrium.
The Ideal Gas Law summarizes all of the various experiments in the 17th and 18th century that strove to define the relationships between the different properties of a gas. These relationships can all be explained by the ideal gas law. The ideal gas law is based on three critical assumptions.
In this article, we’re going to teach you all about Solubility Rules. No discussion of solubility rules is complete without first understanding the notation associated with solubility analysis. Understanding solubility on a deep level requires us to view the topic from a particulate approach, which means we will have to discuss the Kinetic Molecular Theory in detail.
When you get to the thermodynamics section of AP® Chemistry, one of the hardest things to remember is the definition of enthalpy vs. entropy. This tutorial explains the theory behind enthalpy and entropy using the laws of thermodynamics. Then we will talk about the definition of enthalpy and how to calculate it, using enthalpy practice questions.
Rutherford proposed that an atom was made up of a dense, positive nucleus, surrounded by mostly empty space and negative electrons. Rutherford’s model of the atom prevailed for many years until scientists started noticing inconsistencies. Physics established that an electron moving in a curved path around a nucleus must give off energy.As it continuously loses energy, the electron should spiral into the nucleus. Since this does not happen, there needed to be a new model to describe atoms.
This AP® Chemistry crash course review will go over the fundamentals of acid-base chemistry and its applications to the AP® Chemistry exam. There are three definitions of what constitutes an acid and a base. Each of these definitions is useful for different purposes.