91Ó°ÊÓ

Oxidation is a key concept in redox reactions which stands for the loss of electrons by an atom. When an atom undergoes oxidation, it means that it loses some of its electrons.
This loss of electrons causes the atom to have a higher positive charge than before. For instance, let's consider a neutral atom. If it loses one electron, it becomes a positively charged ion with a charge of +1. This is because electrons carry a negative charge, so losing electrons makes the overall charge more positive.
It's important to remember that oxidation involves an increase in the oxidation state of an atom, signaling that electrons are leaving the atom. A practical way to keep this in mind is through the mnemonic "OIL RIG" which represents "Oxidation Is Loss" of electrons.

Reduction, in contrast to oxidation, involves the gain of electrons by an atom. This process is essential in redox reactions since it accompanies oxidation. When an atom undergoes reduction, it gains electrons and thus its oxidation state decreases.
Adding more electrons leads to a more negative overall charge of the atom. For example, if a neutral atom receives one electron, it will become a negatively charged ion with a charge of -1. This happens because electrons are negatively charged, so adding them increases the overall negativity of the atom.
Another useful mnemonic to recall reduction is the other half of "OIL RIG": "Reduction Is Gain" of electrons. This helps us remember that reduction is all about gaining electrons and thereby reducing the oxidation state.

Electron transfer is the fundamental process that ties oxidation and reduction together in redox reactions. This transfer involves the movement of electrons from one atom to another.
In a typical redox reaction, an electron donor (which is oxidized) transfers electrons to an electron acceptor (which is reduced). This synchronized movement of electrons explains why changes in the oxidation states of atoms occur during redox reactions.
Understanding electron transfer also involves recognizing that it is responsible for the energy transformations in many chemical reactions. These reactions drive biological processes like cellular respiration, and technological applications like batteries.
To wrap it up, the concept of electron transfer simplifies redox reactions, indicating the flow from electron-rich regions to electron-deficient locations.