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- Oxidation and reduction are chemical reactions that involve the transfer of electrons or oxygen/hydrogen atoms123.Some examples of oxidation and reduction are123:
- Combustion of methane: CH 4 (g) + 2 O 2 (g) → CO 2 (g) + 2 H 2 O (g). Methane loses four hydrogen atoms and oxygen gains four hydrogen atoms.
- Oxidation of copper: 2 Cu (s) + O 2 (g) → 2 CuO (s). Copper loses two electrons and oxygen gains two electrons.
- Photosynthesis: 6 CO 2 (g) + 6 H 2 O (l) → C 6 H 12 O 6 (s) + 6 O 2 (g). Carbon dioxide gains six hydrogen atoms and water loses six hydrogen atoms.
- Reduction of copper (II) oxide: CuO (s) + H 2 (g) → Cu (s) + H 2 O (g). Copper (II) oxide gains two electrons and hydrogen loses two electrons.
Learn more:✕This summary was generated using AI based on multiple online sources. To view the original source information, use the "Learn more" links.Some examples of common redox reactions are shown below. CH A 4 (g) + 2 O A 2 (g) → CO A 2 (g) + 2 H A 2 O (g) (combustion of methane) 2 Cu (s) + O A 2 (g) → 2 CuO (s) (oxidation of copper) 6 CO A 2 (g) + 6 H A 2 O (l) → C A 6 H A 12 O A 6 (s) + 6 O A 2 (g) (photosynthesis)www.khanacademy.org/science/ap-chemistry-beta/…For example, magnesium is oxidised when it reacts with oxygen to form magnesium oxide: magnesium + oxygen → magnesium oxide 2Mg + O 2 → 2MgO Reduction is the gain of electrons by a substance. It is also the loss of oxygen from a substance. For example, copper (II) oxide can be reduced to form copper when it reacts with hydrogen:www.bbc.co.uk/bitesize/guides/zv7f3k7/revision/1Oxidation is the loss of hydrogen. Reduction is the gain of hydrogen. Notice that these are exactly the opposite of the oxygen definitions (#1). For example, ethanol can be oxidized to ethanal: An oxidizing agent is required to remove the hydrogen from the ethanol.chem.libretexts.org/Bookshelves/Analytical_Chemi… - People also ask
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WEBLearn the history and definitions of oxidation and reduction, and how to assign oxidation numbers to atoms. See examples of oxidation-reduction reactions in nature, energy production, and biochemistry.
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