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Chapter 17: Problem 57

What process is represented by the corrosion of a metal? Why is corrosion undesirable?

Short Answer

Expert verified
Corrosion is a natural process that occurs as a result of chemical or electrochemical reactions between a metal and its environment, leading to the deterioration of the material and forming oxides or other compounds on the metal's surface. The process is undesirable due to several factors, including structural damage, economic loss, environmental impact, and aesthetic concerns. For example, rusting of iron is a common type of corrosion that weakens the metal and can lead to structural failure, maintenance costs, pollution, and an unsightly appearance.

Step by step solution

01

Define Corrosion

Corrosion is a natural process that typically results from a chemical or electrochemical reaction between a metal (or alloy) and its environment. This reaction leads to the deterioration or degradation of the material, often resulting in the formation of oxides, salts, or other compounds on the surface of the metal.
02

Explain How Corrosion Occurs

Corrosion generally occurs due to a metal's exposure to environmental factors such as moisture, oxygen, chemicals, and changes in temperature or pH. The electrochemical nature of most corrosion processes involves the flow of electrons between the metal surface and the environment, causing the metal to lose electrons and thus, oxidize. The rusting of iron is an example of corrosion. The process begins when iron (Fe) reacts with water (H2O) and oxygen (O2) in the atmosphere: \[\text{Fe (s)} \rightarrow \text{Fe}^{2+} \text{(aq)} + 2e^-\] \[\text{O}_2 \text{(g)} + 2H_2 \text{O (l)} + 4e^- \rightarrow 4OH^- \text{(aq)}\] These equations together lead to the formation of iron (III) hydroxide, which then reacts further with water and oxygen to form iron (III) oxide, or rust: \[\text{Fe}^{3+} \text{(aq)} + 3OH^- \text{(aq)} \rightarrow Fe(OH)_3 \text{(s)}\] \[\text{4Fe(OH)}_3 \text{(s)} + O_2 \text{(g)} \rightarrow 2Fe_2O_3鈥_2O \text{(s)}\]
03

Discuss the Undesirability of Corrosion

Corrosion is undesirable for several reasons: 1. Structural damage: Corroded metals lose their mechanical strength and integrity, which can result in catastrophic failure of structures, such as buildings, bridges, and pipelines. 2. Economic loss: The maintenance, repair, and replacement of corroded components and infrastructure can be time-consuming, costly, and disruptive, leading to significant financial burdens for individuals and organizations. 3. Environmental impact: The release of metal ions and chemical by-products of corrosion can harm the aquatic and terrestrial environments, contributing to soil and water pollution. 4. Aesthetic concerns: Corroded surfaces can be unsightly and may lead to the degradation of the appearance of buildings, vehicles, or other objects made of metal. In conclusion, corrosion represents the deterioration of metals due to chemical or electrochemical reactions with their environment. This process is undesirable because it can cause structural damage, economic loss, environmental impact, and aesthetic concerns.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Electrochemical reaction
Corrosion often involves an electrochemical reaction, where there is an exchange of electrons between the metal surface and the surrounding environment. This process starts with the metal losing electrons and becoming oxidized. For instance, when iron rusts, it undergoes oxidation by losing electrons:
\[\text{Fe (s)} \rightarrow \text{Fe}^{2+} \text{(aq)} + 2e^- \]These lost electrons are gained by other elements, such as oxygen in the presence of water:
\[\text{O}_2 \text{(g)} + 2H_2 \text{O (l)} + 4e^- \rightarrow 4OH^- \text{(aq)}\]
Through these reactions, compounds like oxides and hydroxides form, marking the essence of corrosion.
  • Electrons flow between the anode (where metal oxidizes) and the cathode (where reduction occurs).
  • Different environments can speed up or slow down these reactions.
Understanding this electrochemical basis is key to developing strategies to prevent or control corrosion effectively.
Metal deterioration
Metal deterioration is the result of ongoing electrochemical reactions like corrosion. These reactions alter the metal's structure and properties, leading to weakened or completely compromised materials.
The rust that you see on iron is a perfect example of how a solid, reliable material can slowly erode into a powdery substance that offers little to no support.
  • As metallic bonds break down, strength and durability decrease.
  • The visible effects might include pitting, embrittlement, or cracking.
Understanding this process helps in identifying signs of deterioration early. Early detection can ensure timely interventions that save structures and many other vital components.
Environmental impact
Corrosion doesn't just affect physical structures; it also poses a threat to the environment. When metals corrode, ions and other compounds can leach into the soil and water, potentially causing pollution.
  • Marine ecosystems are especially vulnerable as corroded metals may release toxic elements into the water.
  • Pollutants from corroded infrastructure can contaminate sources of drinking water.
Limiting the impact involves using materials resistant to corrosion and improving waste management practices to handle corroded debris adequately.
Structural damage
Structural damage is one of the most dangerous effects of corrosion. When the metal parts of a bridge, building, or pipeline corrode, it can lead to catastrophic failures.
Corroded metal loses its strength and becomes more prone to cracks or collapse, posing serious safety risks.
  • Regular inspections can detect corrosion before it leads to significant damage.
  • Employing protective measures like coatings or cathodic protection can extend the life of metal structures.
Ultimately, maintaining structural integrity requires a proactive approach to managing and mitigating the effects of corrosion.
Economic loss
The financial implications of corrosion are vast. Corrosion can lead to expensive repairs and replacements of damaged structures and machines.
Every year, billions of dollars are spent worldwide dealing with problems linked to corrosion.
  • Labor costs for repair and maintenance rise as parts deteriorate quicker than expected.
  • Extended downtime in industries, caused by corroded equipment, can lead to losses in productivity.
Effective corrosion management, such as designing with less corrosive materials and performing regular inspections, can mitigate these economic impacts and lead to cost savings in the long run.

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Most popular questions from this chapter

In each of the following reactions, identify which element is oxidized and which is reduced by assigning oxidation states. a. \(2 \mathrm{B}_{2} \mathrm{O}_{3}(s)+6 \mathrm{Cl}_{2}(g) \rightarrow 4 \mathrm{BCl}_{3}(l)+3 \mathrm{O}_{2}(g)\) b. \(\operatorname{GeH}_{4}(g)+\mathrm{O}_{2}(g) \rightarrow \operatorname{Ge}(s)+2 \mathrm{H}_{2} \mathrm{O}(g)\) c. \(\mathrm{C_{2} H_{4}(g)+C l_{2}(g) \rightarrow C_{2} H_{4} C l_{2}(l)}\) d. \(\mathrm{O}_{2}(g)+2 \mathrm{F}_{2}(g) \rightarrow 2 \mathrm{OF}_{2}(g)\)

Give some examples of how we make good use of oxidation-reduction reactions in everyday life.

Does an oxidizing agent donate or accept electrons? Does a reducing agent donate or accept electrons?

For each of the following oxidation-reduction reactions, identify which element is being oxidized and which is being reduced. a. \(2 \mathrm{Fe}(s)+3 \mathrm{F}_{2}(g) \rightarrow 2 \mathrm{FeF}_{3}(s)\) b. \(\mathrm{O}_{2}(g)+2 \mathrm{Cu}(s) \rightarrow 2 \mathrm{CuO}(s)\) c. \(\mathrm{F}_{2}(g)+2 \mathrm{KI}(a q) \rightarrow 2 \mathrm{KF}(a q)+\mathrm{I}_{2}(s)\) d. \(2 \mathrm{Al}(s)+3 \mathrm{H}_{2}(g) \rightarrow 2 \mathrm{AlH}_{3}(s)\)

Give an example of a simple oxidation-reduction equation. Identify the species being oxidized and the species being reduced. Identify the oxidizing agent and the reducing agent in your example.
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