Oxidation

We'll go step by step through how to balance an oxidation reduction (redox) reaction in acidic solution. Most importantly, both charges and atoms must balance. Here are the steps: first, calculate oxidations numbers for all the elements in the equation. Next, figure out what is being oxidized and what is being reduced. Then, write half reactions for the oxidation and reduction. After that, balance each half reaction: first, for the atoms other than O and H, then for O and H, and finally for charge by adding electrons. After being balanced, the oxidation and reduction half reactions are ready to be added back to together. Make sure that the number of electrons is the same in the oxidation and reduction half reactions. If they are not, multiply one or both of the half reactions to make the number of electrons the same. Then, combine the oxidation and reduction half reaction, canceling out stuff that appears on both sides of the equation. Lastly, do a final check to make sure that everything balances: both atoms and charge.

Don't make the most common mistake in Oxidation Reduction! This question confuses so many students. Watch this video to learn how to do this right. In chemistry, reduction is the gain of electrons, and oxidation is the loss. Oxidation reduction reactions are often called redox reactions for short.

We'll learn how to determine the oxidation numbers or oxidation states for a the elements in a chemical compound. The oxidation numbers tell us how electrons are divided up or shared between atoms in a chemical compound. The oxidation numbers also tell us how electrons move in an oxidation reduction (redox) reaction. There are a set a rules that we use to determine oxidation number. Group 1A elements (alkalai metals) always have an oxidation of +1. Group 2A elements (alkaline earth metals) always have an oxidation number of +2. Elements on their own have an oxidation number of 0, and monatomic ions have an oxidation number that is equal to the ionic charge.

Electrolysis of copper sulfate and its use to refine blister copper by electrolytic refining.

Electrochemistry_ Galvanic Cell with Cr (III) _ Cr (II) and Hydrogen Half Cells

This animated video takes an in-depth look at the mechanism for the reaction between propene and hydrogen bromide. This is an addition reaction to an asymmetric alkene, so there are two possible alkyl halide products. Markovnikov's rule and the stability of the primary and secondary carbocation intermediates are discussed.

In this video I look at the preparation of carboxylic acids from four other organic functional groups. First, from primary alcohols and aldehydes by the process of oxidation, and second, from esters and nitriles by the process of either acid-catalysed hydrolysis or alkaline catalysed hydrolysis.

This video is a follow-up to the use of the iodoform test in the identification of CH3CH(OH)R alcohols. With alcohols, the first stage in the test forms sodium iodate from iodine and sodium hydroxide. This has iodine in its +1 oxidation state and it oxidises the alcohol to the corresponding aldehyde or ketone. For this reason, the use of the test to identify CH3COR carbonyls, overlaps with the CH3CH(OH)R alcohol test. The structures are drawn out and discussed and the iodoform test is demonstrated.

This video looks at the laboratory oxidation of alcohols using acidified sodium dichromate. It outlines the procedure and explains the underlying redox chemistry. It is one in a series on alcohol chemistry.