Corrosion Processes Quiz

<p>Corrosion that occurs evenly across the entire surface (B)</p> Signup and view all the answers

<p>Storing in a wet environment (D)</p> Signup and view all the answers

<p>The color of the metal surface (D)</p> Signup and view all the answers

<p>Removing oxygen from the environment (D)</p> Signup and view all the answers

<p>Loss of luster (C)</p> Signup and view all the answers

<p>Losing electrons by the metal (C)</p> Signup and view all the answers

<p>Tarnishing of silver (B)</p> Signup and view all the answers

<p>They are converted into more stable compounds (B)</p> Signup and view all the answers

<p>Corrosion increases rapidly with higher temperatures (A)</p> Signup and view all the answers

<p>Corrosion concentrated in specific areas of a material (A)</p> Signup and view all the answers

<p>High levels of humidity (C)</p> Signup and view all the answers

<p>Fatigue and cracking (C)</p> Signup and view all the answers

<p>Oxidation corrosion (A)</p> Signup and view all the answers

<p>It always takes place in a vacuum. (B)</p> Signup and view all the answers

<p>Magnesium (C), Zinc (D)</p> Signup and view all the answers

<p>CVD does not require a vacuum. (B), CVD can create coatings on complex geometries. (D)</p> Signup and view all the answers

<p>2–5 microns (D)</p> Signup and view all the answers

<p>Anode (A)</p> Signup and view all the answers

<p>Low temperature (B)</p> Signup and view all the answers

<p>It contains a reducible species. (B)</p> Signup and view all the answers

<p>Wear resistance (B)</p> Signup and view all the answers

<p>To absorb moisture from the air (B)</p> Signup and view all the answers

<p>Prevention of corrosion on carbon steel (D)</p> Signup and view all the answers

<p>In sacrificial anodes, a more active metal is used, while impressed current uses a DC power source (C)</p> Signup and view all the answers

<p>The metal surface is made the anode of an electrochemical cell (C)</p> Signup and view all the answers

<p>Metallic and non-metallic coatings (B)</p> Signup and view all the answers

<p>They protect products from humidity and water vapors (A)</p> Signup and view all the answers

<p>To provide temporary corrosion protection (D)</p> Signup and view all the answers

<p>By absorbing moisture, which is necessary for growth (D)</p> Signup and view all the answers

<p>Coating steel with zinc (D)</p> Signup and view all the answers

<p>If ∆G is negative, the reaction is thermodynamically possible (B)</p> Signup and view all the answers

<p>The heat treatment and stress state of the material (B)</p> Signup and view all the answers

<p>Thermodynamics can predict the direction or tendency of corrosion (C)</p> Signup and view all the answers

<p>A method that uses an external voltage source for protection (D)</p> Signup and view all the answers

<p>To minimize their energy and reach a more stable state (B)</p> Signup and view all the answers

<p>It can negatively affect corrosion resistance (B)</p> Signup and view all the answers

<p>Metal oxidation (B)</p> Signup and view all the answers

<p>Visible cracks (B)</p> Signup and view all the answers

<p>Maintaining low levels of oxygen (B)</p> Signup and view all the answers

<p>Iron reacts with oxygen and water (A)</p> Signup and view all the answers

<p>Increases the rate of corrosion (A)</p> Signup and view all the answers

<p>Nuclear power (C)</p> Signup and view all the answers

<p>Fe(s) + O2(g) + H2O(l) → Fe2O3.xH2O(s) (B)</p> Signup and view all the answers

<p>Chloride ions (D)</p> Signup and view all the answers

<p>Corrosion of components (B)</p> Signup and view all the answers

A natural process that converts a refined metal into a more chemically stable oxide. It's like a metal returning to its most natural state.

The gradual decay of metals or nonmetals caused by air, moisture, or chemical reactions.

Corrosion is a natural, spontaneous, and thermodynamically stable process. It's how materials tend to return to their most stable state.

A type of corrosion that affects metals. It's a chemical reaction where a metal breaks down due to its environment.

Metals are generally unstable, except for noble metals. They can be converted into more stable compounds like oxides, hydroxides, carbonates, and sulfides.

High humidity or water vapor condensation on metal surfaces can cause corrosion.

Gases like chlorine, hydrogen oxides, ammonia, and sulfur oxides can corrode parts of electronic equipment.

To prevent corrosion, you can apply a thin layer of zinc to iron, paint it, or grease it. These coatings act as barriers against the environment.

Corrosion that affects the entire surface of a material uniformly.

Corrosion that is concentrated in specific areas of a material, creating localized damage.

The process where metal atoms lose electrons and the surrounding environment gains them.

The rate of corrosion is directly influenced by the availability of oxygen, water, and other chemicals.

Selecting materials resistant to corrosion, removing oxygen, or using corrosion inhibitors.

The metal reverts to its natural oxidation state, usually through reactions with oxygen or other atmospheric gases.

Corrosion occurring in the presence of electrolytes, like water or moisture, where electrons are transferred.

Corrosion that occurs when metals react directly with gases like carbon dioxide and sulfur dioxide without water.

These substances absorb moisture from the air to keep the environment around metal products dry.

These bags are designed to prevent condensation and water vapors from collecting on products, protecting them from humidity, oxygen, and grease.

These temporary coatings are often used for corrosion protection on unfinished surfaces, pipes, steel products, and car underbodies, especially when removal is required.

These coverings adhere to the metal's surface, limiting its exposure to corrosive environments.

This method, more commonly used than anodic protection, prevents corrosion by converting active sites on a metal surface to passive sites using an external electrical current.

This method is used in environments with extreme corrosion in the chemical and mining industries. It prevents corrosion by making the metal surface the anode of an electrochemical cell and controlling the electrode potential.

These coatings include pure metals, solid solutions, and alloys.

These coatings can be organic or inorganic, and can be applied in solid, liquid, or gas forms.

Coating steel with zinc to prevent corrosion. It acts as a sacrificial layer, corroding instead of the steel.

A method using an external voltage source to protect underground structures from corrosion. It makes the metal negatively charged, preventing it from being oxidized.

A branch of science that deals with energy changes during reactions, like corrosion. It helps predict if corrosion is possible.

A measure of how much energy is released or absorbed during a reaction. If it's negative, corrosion is possible.

The more negative the value, the more likely a metal will corrode. Think of it as a stronger driving force for corrosion.

All reactions involved in corrosion must be reversible for thermodynamic calculations to be accurate.

The ability of a material to resist corrosion. Different metals have different levels of resistance.

A technique for creating thin films on a substrate using physical reactions to transform a solid or liquid source material into a gas, which then condenses into a solid film. The process always takes place in a vacuum.

A technique for creating thin films on a substrate using chemical reactions to transform a gaseous or vapor source material into a solid film. It can take place at different pressures, from vacuum to atmospheric.

Metallic coatings like aluminum, zinc, and chromium can improve a surface's hardness, wear resistance, and resistance to oxidation.

Non-metallic coatings like oxides, nitrides, or polymers can enhance a substrate's appearance, corrosion resistance, and wear resistance.

A device converting chemical energy into electrical energy through a process called electrochemical corrosion.

The corroding metal in an electrochemical corrosion cell, where it gets eaten away.

A metal, graphite, or semiconductor that acts as an electron conductor in an electrochemical corrosion cell, without being corroded.

A solution containing ions that participate in the electrochemical reactions of corrosion.

Stress corrosion can be dangerous because it occurs under stress, even in seemingly safe environments, making it hard to predict and prevent.

Cracks, color or texture changes, and unexpected failure are signs of stress corrosion. Cracks often start at weak points, making them hard to see before they grow big.

Controlling stress corrosion involves reducing oxygen and chloride ions, and using less reactive steels. This minimizes the conditions needed for corrosion.

Nuclear power, chemical and food processing, oil and gas extraction, and medical and pharmaceutical industries are all vulnerable to stress corrosion.

Acid rain accelerates metal corrosion by increasing its rate. For example, the Statue of Liberty's green patina is caused by acid rain and oxidation over time.

Acid rain reacts with limestone and marble to create gypsum, which flakes off and damages stone surfaces. This can make old inscriptions unreadable.

Iron reacts with oxygen and water to form hydrated iron(III) oxide, also known as rust, a brown powder.

Salt in water and acid rain accelerate rusting. These factors create a more reactive environment for iron.