Oxidizing agent and reducing agent with example?

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C+o2=co2c is oxidised n o2 is reduced

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Oxidizing Agent:

An oxidizing agent, also known as an oxidant, is a substance that causes another substance to undergo oxidation. It is responsible for accepting electrons, gaining oxygen atoms, or losing hydrogen atoms in a chemical reaction. Oxidizing agents are typically substances that are electronegative and have a high affinity for electrons. They are often involved in reactions where they remove electrons from other substances.

Examples of Oxidizing Agents:

1. Oxygen (O2): Oxygen is a common oxidizing agent, especially in combustion reactions. It readily accepts electrons from other substances, resulting in oxidation. For example, when iron reacts with oxygen in the presence of moisture, it undergoes oxidation and forms iron oxide (rust).

2. Potassium Permanganate (KMnO4): Potassium permanganate is a strong oxidizing agent commonly used in laboratory settings. It is capable of oxidizing a wide range of substances. For instance, in the presence of an acidic medium, potassium permanganate can oxidize ethylene glycol to produce carbon dioxide, water, and manganese dioxide.

3. Hydrogen Peroxide (H2O2): Hydrogen peroxide is another example of an oxidizing agent. It is commonly used as a disinfectant and bleaching agent. Hydrogen peroxide can oxidize various substances, such as organic compounds, by accepting electrons. For instance, it can oxidize sulfides to sulfoxides or sulfones.

Reducing Agent:

A reducing agent, also known as a reductant, is a substance that causes another substance to undergo reduction. It is responsible for donating electrons, gaining hydrogen atoms, or losing oxygen atoms in a chemical reaction. Reducing agents are typically substances that are electropositive and have a low affinity for electrons. They are often involved in reactions where they give up electrons to other substances.

Examples of Reducing Agents:

1. Hydrogen (H2): Hydrogen gas is a common reducing agent. It readily donates electrons to other substances, resulting in reduction. For example, in the Haber process, hydrogen is used as a reducing agent to convert nitrogen gas into ammonia.

2. Sodium Bisulfite (NaHSO3): Sodium bisulfite is a reducing agent commonly used as a food preservative and in various chemical reactions. It can donate sulfur dioxide (SO2) or hydrogen sulfite (HSO3-) ions, which act as reducing agents. For instance, it can reduce iodine (I2) to iodide ions (I-) in the presence of water.

3. Carbon Monoxide (CO): Carbon monoxide is a reducing agent that is often produced as a byproduct of incomplete combustion. It can donate electrons to other substances, causing reduction. For example, in the iron smelting process, carbon monoxide reduces iron oxide (Fe2O3) to elemental iron (Fe).

In summary, oxidizing agents are substances that accept electrons, while reducing agents are substances that donate electrons. These agents play crucial roles in redox reactions, where one substance undergoes oxidation while another undergoes reduction.

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