Reduction

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.

In this video I look at the use of the two main reducing agents employed in organic chemistry. These are lithium aluminium hydride (lithal) and sodium borohydride. I outline the mechanism (nucleophilic addition) in which hydride ions react with C=O groups to form alcohols via alkoxide intermediates. I compare the reactivities of the two reducing agents and discuss the explosive risks associated with using lithium aluminium hydride with protic solvents such as water or methanol. A practical setup, that could be used to reduce aldehydes and ketone with lithal, is presented at the end. It is one in a series of short videos looking at the main organic practical techniques: heat & distill; reflux distillation; washing and drying in solvent extraction; recrystallisation and melting point determination; and others

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.

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.

Thanks for visiting. This animated video takes an in-depth look at the mechanism for the reaction between ethene and bromine.

In this video lesson, Mr. Scullion demonstrates a reacting mass problem involving ammonium dichromate. Try the problem out on your own prior to finding out the solution.

Aqueous sodium hydroxide is added to a solution of manganese (II) nitrate to precipitate manganese (II) hydroxide. This is then oxidised to manganese (IV) oxide using hydrogen peroxide. The structures of the complexes and the redox chemistry are discussed briefly.