Corrosion and Electroplating Quiz

<p>To prevent against corrosive conditions (B)</p> Signup and view all the answers

<p>Applying a layer of zinc (A)</p> Signup and view all the answers

<p>Silver rod dissolves to produce Ag+ ions. (D)</p> Signup and view all the answers

<p>Cr3+ ions (A)</p> Signup and view all the answers

<p>Antimonial-lead (D)</p> Signup and view all the answers

<p>Moist air (B)</p> Signup and view all the answers

<p>For better adhesion and corrosion resistance. (D)</p> Signup and view all the answers

<p>Electrical wires (D)</p> Signup and view all the answers

<p>The area with stains and dents (A)</p> Signup and view all the answers

<p>Oxidation of iron (D)</p> Signup and view all the answers

<p>Fe2O3·nH2O (B)</p> Signup and view all the answers

<p>It provides H+ ions that accelerate rusting (B)</p> Signup and view all the answers

<p>It is porous (A)</p> Signup and view all the answers

<p>Electrons facilitate the oxidation of iron (C)</p> Signup and view all the answers

<p>Iron is submerged in pure water (A)</p> Signup and view all the answers

<p>Alkaline detergent solutions and acid (D)</p> Signup and view all the answers

<p>Tin metal electrode (D)</p> Signup and view all the answers

<p>They dissolve into solution as copper ions ($Cu^{2+}$) (C)</p> Signup and view all the answers

<p>Copper sulphate solution in water (B)</p> Signup and view all the answers

<p>To deposit the metal onto the substrate (A)</p> Signup and view all the answers

<p>To provide a protective layer against rust (C)</p> Signup and view all the answers

<p>Depositing one metal over another using electrolysis (D)</p> Signup and view all the answers

<p>It is the source of metal ions for deposition (D)</p> Signup and view all the answers

<p>It rusts rapidly due to exposure to air and water (D)</p> Signup and view all the answers

<p>Cleaning the object to be plated (C)</p> Signup and view all the answers

<p>A saline solution of the metal's salt (A)</p> Signup and view all the answers

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

<p>To prevent exposure to oxidation (B)</p> Signup and view all the answers

Prevents the iron from reacting with oxygen and water, which causes rust.

Modern paints often contain chemicals that act as a barrier, preventing moisture and oxygen from reaching the iron surface.

Adding chromium and nickel to iron creates a more corrosion-resistant alloy, like stainless steel.

A metallic coating, like zinc, acts as a barrier, preventing corrosive substances from directly contacting the iron.

Galvanizing is the process of applying a protective zinc coating to iron, preventing it from rusting.

Removing stains on iron reduces the sites where corrosion can start, leading to rust prevention.

The gradual degradation of a metal caused by chemical reactions with its surroundings, often involving oxidation.

Painting or greasing metal surfaces creates a barrier that prevents oxygen and water from reaching the metal, slowing down rusting.

Alloying is mixing metals to create a new material with improved properties. In the case of rust prevention, adding metals like chromium and nickel to iron makes it more resistant to corrosion.

A specific type of corrosion affecting iron, resulting in the formation of a reddish-brown oxide called rust.

The region on a corroding metal where oxidation occurs, releasing electrons and forming metal ions.

Metallic coating involves covering a metal with another metal to protect it from corrosive conditions. Examples include zinc, tin, and chromium coating, common in food preservation.

Galvanizing, the process of coating iron with a thin layer of zinc, prevents rust even if the coating is damaged. The zinc layer acts as a sacrificial anode, corroding instead of the iron.

The region on a corroding metal where reduction occurs, accepting electrons and using them to reduce substances like oxygen.

The chemical reaction that results in the loss of electrons, often occurring at the anodic region during corrosion.

The chemical reaction that involves the gain of electrons, commonly happening at the cathodic region during corrosion.

The reddish-brown oxide, typically hydrated iron oxide (Fe2O3·nH2O), formed during rusting.

The requirement of both moisture (water) and oxygen for rusting to occur.

The process of depositing a thin layer of metal onto a surface using an electric current.

A method for purifying copper using electric current. Impure copper dissolves at the anode, and pure copper deposits at the cathode.

The electrode where oxidation takes place during electrolysis. In refining copper, impure copper acts as the anode.

The electrode where reduction takes place during electrolysis. In refining copper, pure copper acts as the cathode.

The process of applying a layer of zinc to iron to prevent rusting.

Electroplating of silver involves dissolving a silver rod (anode) to create silver ions (Ag+) which then deposit onto an object (cathode) as a thin coating.

Similar to silver plating, chromium plating uses a chromium solution and an electric current to deposit chromium onto a metal object, creating a hard and corrosion-resistant coating.

In electroplating, the anode is the metal that gets dissolved, providing the ions for the coating. The cathode is the object being coated.

Electroplating is often used to enhance the appearance, corrosion resistance and other properties of metal objects.

A method of protecting iron from rusting by coating it with a thin layer of tin.

The electrode where metal ions are produced and move into the solution during electroplating.

The electrode where metal ions are deposited, forming a coating during electroplating.

The solution containing metal ions that carries the electric current during electroplating.