Define redox reaction give one example?

A redox reaction, short for reduction-oxidation reaction, is a type of chemical process where the oxidation state of one or more substances changes. This occurs through the transfer of electrons between reactants. In simpler terms, during a redox reaction, one substance gets oxidized (loses electrons) while another gets reduced (gains electrons). These reactions are fundamental in various chemical processes, including combustion, respiration, and corrosion.

Breaking Down Redox Reactions

To understand redox reactions better, let’s look at the two key components involved:

• Oxidation: This is the process where a substance loses electrons. When a substance is oxidized, its oxidation state increases. For example, when iron (Fe) reacts with oxygen (O₂), iron loses electrons and is oxidized to form iron oxide (rust).
• Reduction: This is the opposite process, where a substance gains electrons, leading to a decrease in its oxidation state. In the same reaction, oxygen is reduced as it gains electrons from iron.

Example of a Redox Reaction

A classic example of a redox reaction is the reaction between hydrogen and oxygen to form water:

2H₂ + O₂ → 2H₂O

In this reaction:

• Hydrogen (H₂) is oxidized because it loses electrons, changing its oxidation state from 0 to +1.
• Oxygen (O₂) is reduced as it gains electrons, changing its oxidation state from 0 to -2.

Importance of Redox Reactions

Redox reactions are crucial in many areas of science and technology. For instance:

• In biological systems, cellular respiration is a redox process where glucose is oxidized to produce energy.
• In batteries, redox reactions occur to generate electrical energy.
• In environmental chemistry, redox reactions play a role in the degradation of pollutants.

Understanding redox reactions not only helps in grasping fundamental chemical principles but also in applying this knowledge to real-world scenarios, from energy production to biological functions.