Why bending iron nails causes it to corrode faster?

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Discussion Overview

The discussion revolves around the phenomenon of increased corrosion rates in bent iron nails, exploring potential reasons for this observation. The scope includes theoretical explanations and personal experiences related to corrosion in different environments.

Discussion Character

  • Exploratory, Technical explanation, Homework-related

Main Points Raised

  • One participant notes personal experience with bent nails in a saltwater environment, stating they have not observed an increased corrosion rate unless the zinc coating was damaged.
  • Another participant proposes that oxidation occurs more readily at points of stress in metals, suggesting that these points act as anodes in the corrosion process, referencing specific half-reactions involved in oxidation and reduction.
  • This participant also mentions resources for further reading on the topic, including a textbook and a website on corrosion types.

Areas of Agreement / Disagreement

Participants do not appear to reach a consensus, as one individual shares a personal observation contradicting the claim of increased corrosion, while another provides a theoretical explanation for why bending may lead to increased corrosion at stress points.

Contextual Notes

The discussion includes varying personal experiences and theoretical insights, but does not resolve the underlying assumptions about the conditions affecting corrosion rates, such as environmental factors and material properties.

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Homework Statement


When bending iron nails, the corrosion rate increases. Does anyone knows, why is that?


Homework Equations





The Attempt at a Solution

 
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I've bent over many nails in a salt water environment, some of them I've been able to observe for as long as 40 years. I've never noticed an increased corrosion rate, except when I damaged the zinc coating.
 
Oxidation occurs most easily at points of stress in a metal. This point becomes an anode for the reaction of Iron with Oxygen, yielding the half-reaction of Fe→Fe2++2e-. The reduction half-reaction, therefore, is O2+2H2O+4e-→4OH-.

There are some nice illustrations of this on pages 816-817 of Chemistry, 9th Edition by Whitten, Davis, Peck, & Stanley.

The reason for this increased oxidation at the points of stress is that the atomic structure allows the process to occur more readily. The section on Cold Worked Corrosion at http://www.efunda.com/materials/corrosion/corrosion_types.cfm has some minimal information on this, and you can always look it up in more depth if you're interested/this is the information that you need.
 
Thanks for your help, guys :D
 

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