Elements that can be oxidizing AND reducing agents?

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SUMMARY

Three chemical species that can act as both oxidizing and reducing agents are hypochlorites (Cl), hypobromites (Br), and hypoidoites (I). These compounds undergo disproportionation reactions, allowing them to exhibit dual behavior in redox processes. Additionally, hydrogen peroxide (H2O2) and sulfur dioxide (SO2) are also identified as candidates for this dual functionality. Understanding the definitions of oxidizing and reducing agents is crucial for grasping these concepts.

PREREQUISITES
  • Understanding of redox reactions and their mechanisms
  • Familiarity with the redox table and standard electrode potentials
  • Knowledge of disproportionation reactions
  • Basic chemistry concepts related to oxidizing and reducing agents
NEXT STEPS
  • Study the mechanisms of disproportionation reactions in detail
  • Learn about the standard electrode potentials of various oxidizing and reducing agents
  • Explore the properties and reactions of hydrogen peroxide (H2O2) in redox chemistry
  • Investigate the role of sulfur dioxide (SO2) in oxidation-reduction processes
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Chemistry students, educators, and anyone interested in understanding the complexities of redox reactions and the behavior of chemical agents in various reactions.

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Hello people, so there is a gr.11 chem question that I've been struggling with...

a) Identify three oxidizing agents (other than Fe2+) from the redox table that can also react as reducing agents.
b)try to explain this suprising behavior.

so, any ideas? i have a redox table in my textbook, but i am not sure how to determine the chemicals that behave as oxidizing and reducing agents...Any help is appreciated o:)
 
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Start from the definition of reducing and oxidizing agent, and if you understand why Fe2+ can be both a reducing and an oxidizing agent depending on the reaction, you can easily answer that question.
 
As several of the halogens compounds undergo REDOX reactions with themselves (so called disproportionation), one can include hypochlorites (or Chlorine), hypobromites (or Bromine) and hypoidoites (or Iodine).


Examples:

Cl2 + H2O <----> HCl + HOCl

I2 + H2O <---> HI + HIO

3 NaClO ---> 2 NaCl + NaClO3

3 HIO ---> 2 HI + HIO3

Other candidates, H2O2 and SO2.
 

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