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To understand oxidation, let's start with a simple idea: electrons. Electrons are tiny particles that zoom around the nucleus of an atom. Oxidation is a process where a molecule, atom, or ion loses these electrons.
When a substance undergoes oxidation, it loses one or more electrons. So, the substance becomes more positively charged.
Here's a small tip: you can remember this with the mnemonic 'OIL RIG', where Oxidation Is Loss (of electrons).
In any chemical reaction that involves oxidation, there must be another process happening simultaneously: reduction. This means that while one substance is losing electrons (oxidation), another must be gaining them (reduction).

Now, let's turn to reduction, the other half of the 'OIL RIG' mnemonic, where Reduction Is Gain (of electrons).
Reduction is all about gaining electrons. When a molecule, atom, or ion gains electrons, it becomes more negatively charged.
Imagine you have a neutral atom. When it gains an electron, it becomes negatively charged because electrons carry a negative charge.
In every chemical reaction involving reduction, oxidation is also taking place. This means while one substance is gaining electrons (being reduced), another is losing electrons (being oxidized).
In a reaction, the substance that gets reduced is known as the oxidizing agent. This might sound confusing, but it makes sense: the oxidizing agent is the one that causes the oxidation by gaining electrons itself.

Chemical reactions often involve the transfer of electrons from one substance to another. This is key to understanding how oxidation and reduction work hand in hand.
Electrons can move from one substance to another, and this movement is essential to many chemical processes in everyday life.
Here's an example: when you light a match, the chemical reaction involves electron transfer. The substance on the match head loses electrons (oxidation) while oxygen in the air gains those electrons (reduction).
For oxidation and reduction to occur, there must be an exchange of electrons. The substance that gives away electrons (the one that gets oxidized) gives them to the substance that accepts them (the one that gets reduced).
The oxidizing agent is the one that accepts electrons, causing another substance to lose them. Therefore, the oxidizing agent is reduced in the process.
This interaction is fundamental in understanding many chemical reactions around us, from rusting metal to cellular respiration in our bodies.