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Comprehensive Redox Reactions Study Guide: Detailed Notes on Oxidation-Reduction, Balancing Equations, Electrochemistry, and Applications"$7.99
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Comprehensive Redox Reactions Study Guide: Detailed Notes on Oxidation-Reduction, Balancing Equations, Electrochemistry, and Applications"
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Course
Chemistry and biology
Institution
This document is comprehensive guide on redox ct for students and chemistry enthusiasts.It covers all key topics like oxidation, reduction and many more ..It is useful for all NEET aspirant as well as for JEE aspirant and all cbse, state board college students. A valuable resource for exam preparat...
“Many Chemical reactions involve transfer of electrons from one chemical
substance to another. These electron-transfer reactions are termed as
Oxidation-Reduction or Redox reactions.
𝗢𝘅𝗶𝗱𝗮𝘁𝗶𝗼𝗻
(i) Loss of electron
- Example: Fe²⁺ → Fe³⁺ + e⁻
- Sub-points:
- Loss of hydrogen
- Gain of oxygen
- Gain of electronegative element OR loss of electropositive element
𝗥𝗲𝗱𝘂𝗰𝘁𝗶𝗼𝗻
i) Gain of electron
- Example: Cl₂ + 2e⁻ → 2Cl⁻
- Sub-points:
- Gain of hydrogen
- Loss of oxygen
- Loss of electronegative element OR gain of electropositive element
𝗥𝗲𝗱𝗼𝘅 𝗿𝗲𝗮𝗰𝘁𝗶𝗼𝗻
The reaction in which oxidation as well as reduction takes place together is
known as a redox reaction.
”REDOX REACTIONS IN TERMS OF ELECTRON TRANSFER (MODERN
IDEA)
Oxidation process is the process in which one or more electrons are lost by
an atom, ion, or molecule.
Example: Zn → Zn²⁺ + 2e⁻
, Reduction process is the process in which one or more electrons are gained
by an atom, ion, or molecule.
Example: Cu²⁺ + 2e⁻ → Cu
Oxidising agent or Oxidant: These reagents oxidize others and reduce
themselves. Compounds that consume electrons during a redox reaction are
termed oxidants.
Examples of powerful oxidizing agents: O₂, K₂Cr₂O₇, HNO₃, conc. H₂SO₄
Reducing agent or Reductant
Reducing agents are compounds that can reduce other substances while
oxidizing themselves during a chemical reaction. These reagents undergo
loss of electrons in a redox reaction, leading to an increase in oxidation
number for an element. Examples of powerful reducing agents include KI etc
Additionally, there are compounds that can function as both oxidizing agents
and reducing agents, such as H₂O₂ , NO₂-
Oxidation State :
Oxidation state of an atom in a molecule or ion is the hypothetical or real
charge present on an atom due to Electronegativity difference.
Or
Oxidation state of an element in a compound represents the number of
electrons lost or gained during its
Change from free state into that compound.
Some important points concerning oxidation number:
1) Electronegativity values of no two elements are same –
P> H
C>H
S>C
Cl> N
2) Oxidation number of an element may be positive or negative.
3) Oxidation number can be zero, whole number or a fractional value.
Ex.
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