Discuss the role of oxidising and reducing agen... - SS1 Chemistry Redox Reactions Question

In redox reactions, oxidising agents and reducing agents are involved in the transfer of electrons.

 

Oxidising Agents:

Oxidising agents are substances that cause oxidation by accepting electrons from other species. They are reducing themselves in the process. Oxidising agents are electron acceptors and are often characterised by their high electronegativity or ability to gain electrons.

 

 

 

Examples of common oxidising agents:

-       Oxygen (O2): Oxygen is a strong oxidising agent and is involved in many combustion reactions.

-       Hydrogen peroxide (H2O2): Hydrogen peroxide is a powerful oxidising agent commonly used as a bleach or disinfectant.

-       Potassium permanganate (KMnO4): Potassium permanganate is a strong oxidising agent used in analytical chemistry and organic synthesis.

 

Reducing Agents:

Reducing agents are substances that cause reduction by donating electrons to other species. They oxidise themselves in the process. Reducing agents are electron donors and are often characterised by their low electronegativity or ability to lose electrons.

 

Examples of common reducing agents:

-       Hydrogen gas (H2): Hydrogen gas is a common reducing agent used in various industrial processes, such as the production of ammonia.

-       Carbon monoxide (CO): Carbon monoxide is a reducing agent involved in metallurgical processes for the extraction of metals from their ores.

-       Sodium borohydride (NaBH4): Sodium borohydride is a mild reducing agent used in organic synthesis and as a reducing agent in some chemical reactions.