Oxidation reactions are an incredibly important reaction type in chemistry. They involve the transfer of electrons between substances, leading to changes in oxidation states of atoms. Understanding oxidation-reduction reactions is key for chemistry students.
In an oxidation reaction, a molecule, atom or ion loses electrons. This is known as oxidation. The oxidizing agent causes oxidation by taking electrons from another substance. Some common oxidizing agents include oxygen, halogens, sulphuric acid and permanganate ions.
Let's look at the reaction between magnesium metal and oxygen gas as an example:
2Mg(s) + O2(g) → 2MgO(s)
In this reaction, magnesium metal is oxidized by oxygen gas. The magnesium atoms give up two electrons each to oxygen molecules. This causes the magnesium to increase in oxidation state from 0 to +2. Meanwhile, the oxygen gains electrons and is reduced.
Oxidation reactions result in a loss of electrons and an increase in oxidation state. Other signs of oxidation include:
- Gain of oxygen
- Loss of hydrogen
- Gain of electronegativity
- Loss of electrons in bond rearrangement
Being able to identify oxidized and reduced species in a reaction is critical. Some tips include:
- Metals tend to get oxidized and nonmetals reduced
- Atoms that gain oxygen are oxidized
- Atoms that lose oxygen are reduced
- Atoms that gain electrons are reduced
Common oxidizing agents to recognize include halogens, concentrated acids, oxygen, sulfur and permanganate compounds. Reducing agents provide electrons and include metals, hydrides and other electron-rich substances.
Oxidation reactions power many important chemical processes we rely on. From combustion engines to hand warmers, batteries and more, these reactions are at the heart of chemistry. Gaining a solid understanding of electron transfers in oxidation will serve any aspiring chemist well in grasping chemical reactivity.
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