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Oxidation and reduction in terms of oxygen transfer

This page looks at the various definitions of oxidation and reduction (redox) in terms of the transfer of oxygen, hydrogen and electrons. It also explains the terms oxidising agent and reducing agent.

Oxidation and reduction in terms of hydrogen transfer

Within our bodies, a sequence of oxidation-reduction reactions are used to burn sugars,such as glucose (C6H12O6) and the fatty acids in the fatswe eat.

Oxidation and reduction in terms of electron transfer

By taking one of the above redox reactions oxidation reduction reaction can be explained in terms of changing oxidation number.

STEP 5: Combine these half-reactions so that electrons areneither created nor destroyed. Two electrons are given off in the oxidationhalf-reaction and two electrons are picked up in the reduction half-reaction. We cantherefore obtain a balanced chemical equation by simply combining these half-reactions.

This is potentially very confusing if you try to learn both what oxidation and reduction mean in terms of electron transfer, and also learn definitions of oxidising and reducing agents in the same terms.

Oxidation and reduction in terms of electron transfer ..

We could balance the oxidation half-reaction in terms of the molecular formulas of thestarting material and the product of this half-reaction.

The tarnishing of silver is just one example of a broad class of oxidation-reductionreactions that fall under the general heading of corrosion. Anotherexample is the series of reactions that occur when iron or steel rusts. When heated, ironreacts with oxygen to form a mixture of iron(II) and iron(III) oxides.

It doesn't matter which half-reaction we balance first, so let's start with thereduction half-reaction. Our goal is to balance this half-reaction in terms of both chargeand mass. It seems reasonable to start by balancing the number of iodine atoms on bothsides of the equation.

DEFINITIONS OF OXIDATION AND REDUCTION (REDOX)
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Oxidation-reduction reaction | chemical ..

The key to identifying oxidation-reduction reactions is recognizing when a chemicalreaction leads to a change in the oxidation number of one or more atoms. It is therefore agood idea to take another look at the rules for assigning oxidation numbers. Bydefinition, the oxidation number of an atom is equal to the charge that would be presenton the atom if the compound was composed of ions. If we assume that CH4contains C4- and H+ ions, for example, the oxidation numbers of thecarbon and hydrogen atoms would be -4 and +1.

Oxidation and Reduction - WWW Project Top Page

Chemists therefore developed the concept of oxidation number to extendthe idea of oxidation and reduction to reactions in which electrons are not really gainedor lost. The most powerful model of oxidation-reduction reactions is based on thefollowing definitions.

Difference Between Oxidation and Reduction | …

Any set of rules, no matter how good, will only get you so far. You then have to relyon a combination of common sense and prior knowledge. Questions to keep in mind whileassigning oxidation numbers include the following: Are there any recognizable hidden in the molecule? Does the oxidation number make sense interms of the known electron configuration of the atom?

Oxidation-Reduction Reactions - Real-life applications

A classic demonstration of oxidation-reduction reactions involves placing a piece ofcopper wire into an aqueous solution of the Ag+ ion. The reaction involves thenet transfer of electrons from copper metal to Ag+ ions to produce whiskers ofsilver metal that grow out from the copper wire and Cu2+ ions.

Plants make their own food thru the process of photosynthesis

Lewis structures can play a vital role in understanding oxidation-reduction reactionswith complex molecules. Consider the following reaction, for example, which is used in theBreathalyzer to determine the amount of ethyl alcohol or ethanol on the breath ofindividuals who are suspected of driving while under the influence.

The Process of Photosynthesis in Plants: An Overview

An oxidation-reduction (redox) is a chemical reaction involving transfer of electrons between two species. An oxidation-reduction reaction is any chemical reaction where the oxidation number of a molecule, atom, or ion changes – by gaining or losing an electron. The redox reactions are very common and vital to the basic functions life, using in processes such as photosynthesis, respiration, combustion, and corrosion or rusting.

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