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Oxidation and Reduction Reactions (Redox Reactions)
This is an introduction to oxidation-reduction reactions, also known as redox reactions. Learn what redox reactions are, get examples of oxidation-reduction reactions, and find out why redox reactions are important.
What Is an Oxidation-Reduction or Redox Reaction?
Any chemical reaction in which the oxidation numbers (oxidation states) of the atoms are changed is an oxidation-reduction reaction. Such reactions are also known as redox reactions, which is shorthand for reduction-oxidation reactions.
Oxidation and Reduction
Oxidation involves an increase in oxidation number, while reduction involves a decrease in oxidation number. Usually, the change in oxidation number is associated with a gain or loss of electrons, but there are some redox reactions (e.g., covalent bonding) that do not involve electron transfer. Depending on the chemical reaction, oxidation and reduction may involve any of the following for a given atom, ion, or molecule:
Oxidation involves the loss of electrons or hydrogen OR gain of oxygen OR increase in oxidation state.
Reduction involves the gain of electrons or hydrogen OR loss of oxygen OR decrease in oxidation state.
Example of an Oxidation-Reduction Reaction
The reaction between hydrogen and fluorine is an example of an oxidation-reduction reaction:
H2 + F2 → 2 HF
The overall reaction may be written as two half-reactions:
H2 → 2 H+ + 2 e− (the oxidation reaction)
F2 + 2 e− → 2 F− (the reduction reaction)
There is no net change in charge in a redox reaction so the excess electrons in the oxidation reaction must equal the number of electrons consumed by the reduction reaction. The ions combine to form hydrogen fluoride:
H2 + F2 → 2 H+ + 2 F− → 2 HF
Importance of Redox Reactions
The electron transfer system in cells and oxidation of glucose in the human body are examples of redox reactions. Oxidation-reduction reactions are vital for biochemical reactions and industrial processes as well. Redox reactions are used to reduce ores to obtain metals, to produce electrochemical cells, to convert ammonia into nitric acid for fertilizers, and to coat compact discs.
Oxidation and reduction (video) | Khan Academy – the oxidation state or the oxidation states for the atoms in the water molecule let's write that down so h2 h2o we would say that oxygen has an ger ger and this is to remember that losing an electron means you are being oxidized or losing electrons is oxidation and gaining electrons is reduction so…providing the electrons necessary to reduce the oxidation number of hydrogen, the oxidation number of zinc increases from 0 to +2; zinc is oxidized. Oxygen doesn't change its oxidation state. The oxidizing agent is permanganate, and the reducing agent is oxalate.the hydrogen is oxidized and the oxygen is reduced. The combination of nitrogen and oxygen which occurs at high temperatures follows the same pattern. In some reactions, the oxidation is most prominent. For example in the burning of methane
PDF Microsoft Word – Chapter 12.doc – Oxidation is the taking away of electron from one atom Reduction is addition of an electron to one atom. The result is Sodium ends up with a loss of electron density and a positive charge.The electrons that are lost in the oxidation reaction are the same electrons that are gained in the reduction reaction. These two reactions are commonly When it loses the electron, chemists say that the sodium metal has been oxidized to the sodium cation. (A cation is an ion with a positive charge…Oxidation and Reduction-the Activity Series. Another important class of reactions are those reactions where electrons are transferred and single replacement When one element (oxidation number = 0) replaces another, that element (usually a metal) is oxidized (loses electrons) and the element that is…
Oxidation and Reduction – Oxidation-reduction potential (ORP) or redox is a measurement that indicates how oxidizing or reducing a liquid is. Both oxidation and reduction can happen in the same reaction, which is why reactions involving oxidation and reduction are often called redox reactions.This is an introduction to oxidation-reduction reactions, also known as redox reactions. Learn what redox reactions are and get examples. Oxidation-reduction reactions are vital for biochemical reactions and industrial processes as well. Redox reactions are used to reduce ores to obtain metals…Oxidation is the loss of electrons and reduction is the gain of electrons. It means that oxidation and reduction should occur at same time however may occur at different places and the electrons can travel through wires or may be through ions in liquid medium.