PPT 9.1 Oxidation and reduction

Oxidation and Reduction Made Easy With These Simple Tips given in the PPT 9.1 Oxidation and reduction. Oxidation and reduction are key concepts in chemistry, but they can seem overwhelming at first. Learn how to simplify them with our simple strategies!
Oxidation and reduction are important chemical processes, but not everyone is born a chemistry whiz. Fear not – with our simple strategies, you’ll soon master the basics of oxidation and reduction and be able to tackle more complex topics.

Understand the Basics: Oxidation and Reduction.
Oxidation and reduction are basic concepts in chemistry. Oxidation is defined as the loss of electrons from an atom, molecule, or compound. Reduction is the opposite; it’s defined as the gain of electrons to an atom, molecule, or compound. In oxidation-reduction (or redox) reactions, one element gains electrons while another element loses electrons. This exchange of electrons causes a chemical reaction to occur.

Learn the Different Classes of Reactions Involved in Oxidation-Reduction Reactions.
Oxidation-reduction reactions can be divided into different classes. The most common are single-replacement reactions, double-replacement reactions, combination reactions, disproportionation reactions, and combustion reactions. Learning about the different types of redox reactions will help you understand them better and make it easier to identify which type of reaction is occurring in a given scenario.

Use Line Diagrams to Visualize Oxidation-Reduction Reactions.
Line diagrams can help you visualize redox reactions by showing the movement of electrons between elements. In a line diagram, an arrow is used to represent one electron. Whenever a reactant molecule donates electrons, the reacting atom’s arrows points away from it. When a product molecule gains electrons, the arrows point towards its direction. With this method, you can easily identify which species are oxidized (losing electron) and which ones are reduced (gaining electrons).

Learn the Rules for Writing Equations for Redox Reactions.
There are a few key rules for writing equations for redox reactions. The oxidation number of the atom must always be balanced on either side of the equation, meaning that the sum of the oxidation numbers on one side must equal the other side. You can also use oxidation numbers to identify which atoms are oxidized or reduced, since elements with higher oxidation numbers will have been oxidized while those with lower numbers have been reduced. It is also important to ensure that all species in both reactants and products follow their respective molecular formulae.

Understand How Oxidation States Are Used in Redox Reactions.
Oxidation states are assigned to atoms based on the number of electrons that it has gained or lost and how many valence electrons it already had. This can be done by taking the oxidation number of each element in the compound and comparing them against a common reference such as oxygen or hydrogen. When one element is oxidized, its oxidation state increases, while when it is reduced, the oxidation state decreases. This key concept allows you to quickly identify which atoms have been oxidized or reduced along with the overall identity of any given reaction.

PPT 9.1 Oxidation and reduction should be revised and you should practice the questions as well.

Read about IB DP chemistry IA here.