Mastering Redox Reactions: How to Write Oxidation and Reduction Equations

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Discussion Overview

The discussion focuses on how to write oxidation and reduction equations for redox reactions, specifically examining the reaction between IO3- and I- to form I2. Participants seek guidance on completing and balancing the reaction.

Discussion Character

  • Homework-related, Technical explanation

Main Points Raised

  • One participant expresses confusion about writing redox equations and seeks help with a specific reaction.
  • Another participant points out that the provided equation is incomplete and suggests determining the oxidation states of the elements involved.
  • Some participants mention the need to complete the equation and refer to examples in textbooks for guidance.
  • There is a suggestion to use different methods for balancing redox reactions, including half-reactions and oxidation numbers.

Areas of Agreement / Disagreement

Participants generally agree that the equation is incomplete and that determining oxidation states is essential. However, there is no consensus on the specific steps to take next, as different methods for balancing redox reactions are mentioned without resolution.

Contextual Notes

Limitations include the incomplete nature of the provided reaction and the lack of specific details on how to apply the suggested methods for balancing redox reactions.

jen24007
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hey guys! i am lost with my current unit...redox reactions. i was wondering if any chem whizzes could lead me in the right direction as how to write the oxidation and reduction equations for the following reaction:

IO-3 (aq) + I- (aq)--> I2 (aq)

Any help would be greatly appreciated! I still have no idea why i took AP chem...:confused:
 
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First of all the equation isn't complete. What happened to the oxygen atom? In general you should first determine the oxidation state of each element in the reaction, there are rules which can be applied to help you do this, can you remember them?

~H
 
Gokul43201 said:
Hoot : The problem requires you to complete the equation.

Oo right, makes sense now.

~H
 

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