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Redox Reactions Explained

Redox reactions involve the transfer of electrons, with reduction being the gain and oxidation the loss of electrons. Key concepts include understanding oxidation states, identifying oxidation and reduction, and balancing redox reactions using specific methods. The document also includes assignments for practical understanding and suggests further reading on related topics.

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13 views3 pages

Redox Reactions Explained

Redox reactions involve the transfer of electrons, with reduction being the gain and oxidation the loss of electrons. Key concepts include understanding oxidation states, identifying oxidation and reduction, and balancing redox reactions using specific methods. The document also includes assignments for practical understanding and suggests further reading on related topics.

Uploaded by

olayinkaadeyinka25
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
Available Formats
Download as PDF, TXT or read online on Scribd
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Understanding Redox Reactions

Introduction to Redox Reactions


Redox reactions are chemical reactions that involve the transfer of electrons
between two species. The term Redox is derived from two key concepts:
1. Reduction: The gain of electrons by a molecule, atom, or ion.
2. Oxidation: The loss of electrons by a molecule, atom, or ion.
Redox reactions are essential in understanding chemical processes such
as combustion, corrosion, respiration, and photosynthesis.

Key Concepts to Learn Redox Reactions


To understand redox reactions, you need to be familiar with the following:

1. Oxidation States
The oxidation state (or oxidation number) of an atom in a compound is
a number that represents the total number of electrons lost or gained by it.
Rules for assigning oxidation states:
• The oxidation state of an element in its pure form is always 0. For ex-
ample: O2 , H2 , etc.F ormonoatomicions, theoxidationstateisequaltothechargeof theion.F or
Na+ = +1, Cl− = −1.
• Oxygen generally has an oxidation state of -2 (except in peroxides, where it
is -1).
• Hydrogen generally has an oxidation state of +1 (except in metal hydrides,
where it is -1).
• The sum of the oxidation states in a neutral compound is 0.
• The sum of the oxidation states in a polyatomic ion is equal to the charge of
the ion.

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2. Identifying Oxidation and Reduction
• Oxidation: Increase in oxidation state.

• Reduction: Decrease in oxidation state.

For example, in the reaction:

Zn + Cu2+ → Zn2+ + Cu

• Zn is oxidized from 0 to +2 (loss of electrons).

• Cu2+ isreducedf rom + 2to0(gainof electrons).

3. Balancing Redox Reactions


Balancing redox reactions involves two key methods:

1. Oxidation number method: Balancing changes in oxidation states.

2. Ion-electron method: Balancing the half-reactions separately for


oxidation and reduction.

Assignment
Answer the following questions to test your understanding of redox reactions:

1. Define oxidation and reduction in terms of:

• Electron transfer.
• Oxidation states.

2. Assign the oxidation states to all elements in the following compounds:

(a) H2 OKMnO4
(b) H2 SO4

3. Balance the following redox reaction in acidic medium:

Cr2 O2−
7 + Fe
2+
→ Cr3+ + Fe3+

4. Identify the oxidizing and reducing agents in the reaction:

Zn + HCl → ZnCl2 + H2

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Further Reading
Explore the following topics to deepen your understanding of redox reactions:

• Electrochemical cells.

• Applications of redox reactions in daily life.

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