Presentation of Redox

1. Presentation of Redox By: Seth Princinsky, Joe bale, Brianna scott

2. Redox Reactions include all chemical reactions in which atoms have reached their oxidation stage.

3. Oxidation • Involves the loss of electrons • Reduction reactions are vital for bio chemical reactions and industrial processes. Redox reactions are used to obtain metals, to produce electrochemical cells. • Reduction- Involves the gain of electrons. • Ex-. 2ca tO2-> 2Ca O

4. Examples of oxidation • Oxidation is found in fires. • It causes the browning of fruit. • Oxidation and reduction process together they react and the oxidation is called the oxidizing agent.

5. The earths surface and the earth • The earths surface is a red boundary between the planets reduced the metalliccore. • The redox is important both the formation of minerals and the mobilization of minerals. • Redox can be seen in the color of rocks red is associated with oxidization conditions formation, Green is typically associated with reducing conditions. • Famous examples of redox conditions affecting geological include uranium deposits and more moqui marbles.

6. Reduction • Reduction- originally referred to the loss in weight upon heating a metallic ore such as a metal oxide to extract the metal. In other words, ore was reduced to metal. • Antoine Lavoisier showed that this loss of weight was due to the loss of oxygen as a gas.

7. Oxidizers • Substances that have the ability to oxidize other substances are said to be oxidative or oxidizing and are known as oxidizing agents, oxidants, or oxidizers. • Oxidants are usually chemical substances with elements in high oxidation states or else highly electronegative elements that can gain extra electrons by oxidizing another substance.

8. Ways to remember redox • Oil rig oxidation is lose of electrons reduction is a gain of electrons. • Leo the loin says ger lose of the electrons is oxidation gain of electrons is reduction. • Leoar says geroa lose of electrons is oxidation (reducing agent) And gain of the electrons is reduced (oxidizing agent).

9. Redox in biology • Photosynthesis involves the reduction of carbon dioxide into sugars and the oxidation of water into molecular oxygen. The reverse reaction respiration oxidizes sugars to produce carbon dioxide and water. • Cellular respiration is the oxidation of glucose to carbon dioxide in the reduction of oxygen to water. • This is the formula for cellular respiration when they are oxidized and reducted. • C6H12O8+ 6 O2 -> 6CO2 + 6 H2O

10. Reducers • Substances that have the ability to reduce are known as reducing agents or reductions. The reductant transfers electrons to another substance. • Examples of reducing agents are lithium, sodium magnesium, zinc and aluminum. • A method of reduction involves the use of hydrogen gas with palladium, platinum or nickel.

11. Redox industry • The primary process of reducing or at a high temperature to produce metals is known as smelting. • The production of compact discs depends on redox reaction, redox coats compact discs with a thin layer of metal.

12. Oxidizing agents • Oxidizing agents can be chemically hazardous. • Oxidizing agent is a substance that is not necessarily combustible.

13. Redox cycling • It is a wide variety of aromatic compounds are enzymatically reduced to form free radicals that contain one more electron then their parent compounds. • Examples of redox cycling: herbicide paraquat, and menadione.