CM-UY 1004 Lecture Notes - Lecture 7: Reagent, Reducing Agent, Stoichiometry

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2 Oct 2017

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Smallest amount of what"s needed = limiting reagent. Convert grams to moles (of what"s given) Which gives the least amount of product. For there to be oxidation, there has to be reduction. For there to be reduction, there has to be oxidation. Reducing agent= what"s being oxidized, oxidation number increases, what loses. Oxidation agent= what"s being reduced, oxidation decreases, what gains electrons. Loss of electrons oxidation, gain of electrons reduction. Oxidation involves loss of electrons, reduction involves gain of electrons electrons. Oxidation number: charge atom would have in molecule or ionic compound if electrons were completely transferred. Free elements have oxidation number of 0. Monatomic ions, oxidation number is charge of ion. Hydrogen is always +1 unless combining with a metal where its -1. Group 1 has +1, group 2 has +2 and fluorine is always -1. Sum of oxidation numbers of atoms in molecule or ion equals charge on molecule or ion. Combination reactions: 2 things combine into 1.

Related Questions

Oxidation-reduction reactions (often called "redox" for short) are reactions that involve the transfer of electrons from one species to another. Oxidation states, or oxidation numbers, allow chemists to keep track of these electron transfers. In general, one element will lose electrons (oxidation), with the result that it will increase in oxidation number, and another element will gain electrons (reduction), thereby decreasing in oxidation number.

An oxidizing agent is an element or compound in a redox reaction that oxidizes another species and itself gets reduced and is therefore the electron acceptor in the reaction.

A reducing agent is an element or compound in a redox reaction that reduces another species and itself gets oxidized and is therefore the electron donor in the reaction.

As a summary, keep in mind the following:

CM-UY 1004 Lecture Notes - Lecture 7: Reagent, Reducing Agent, Stoichiometry

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