Extraction of Metals Quiz

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Questions and Answers

Which method is primarily used to extract highly reactive metals from their ores?

  • Thermal decomposition
  • Reduction with coke
  • Self-reduction
  • Electrolysis (correct)

What term describes the undesirable impurities found in ore?

  • Concentration
  • Ore
  • Matrix
  • Gangue (correct)

Which metals are typically extracted through the self-reduction method?

  • Iron and Lead
  • Copper and Mercury (correct)
  • Silver and Gold
  • Zinc and Calcium

What is the primary reason why extracting highly reactive metals cannot be achieved through heating with carbon?

<p>They react with carbon to form stable compounds. (D)</p> Signup and view all the answers

What does metallurgy refer to in the context of metal extraction?

<p>The extraction and refining of metals. (B)</p> Signup and view all the answers

Which of the following is not a method used for metal extraction based on reactivity?

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

Which of the following elements is considered very less reactive and found in a metallic state in nature?

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

What is the process called when gangue is removed from ore?

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

Which method involves igniting a mixture to obtain pure metals?

<p>Gold-Schmidt aluminothermic reduction (A)</p> Signup and view all the answers

What type of metals are typically reduced using electrolytic methods?

<p>Highly reactive metals (B)</p> Signup and view all the answers

During the electrolytic refining process, the impure metal serves as the _____?

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

What is the product formed at the cathode during the electrolysis of sodium chloride?

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

Which of the following is NOT a common impurity typically removed in the refining of metals?

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

What is the role of the ignition mixture in the thermite reaction?

<p>To initiate the reaction (D)</p> Signup and view all the answers

What by-product is typically formed from the reaction of iron(III) oxide and aluminum?

<p>Aluminum oxide (C)</p> Signup and view all the answers

What type of oxide is formed when non-metals react with oxygen?

<p>Acidic oxides (C)</p> Signup and view all the answers

What occurs to impurities during the electrolytic reduction process?

<p>They settle as anode mud (A)</p> Signup and view all the answers

What phenomenon explains why calcium floats when formed in the presence of water?

<p>Hydrogen gas bubbles adhere to calcium's surface (A)</p> Signup and view all the answers

Which of the following is a non-lustrous metal?

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

Which of the following metals will not displace copper from a solution of its salts?

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

What is the green substance formed on a copper plate exposed to air for a week?

<p>Basic copper carbonate (C)</p> Signup and view all the answers

What is the primary reason sodium chloride conducts electricity only in molten or aqueous states?

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

Which process involves depositing metal onto a surface using electric current?

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

What compound is formed by the reaction of iron with steam over prolonged exposure?

<p>Iron (II,III) oxide (C)</p> Signup and view all the answers

Which element reacts with oxygen to form a compound that has a high melting point and is soluble in water?

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

What is a common example of an alloy that consists of copper and zinc?

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

What happens to metal ions at the cathode during electrolysis?

<p>They are reduced to pure metal. (D)</p> Signup and view all the answers

Which method prevents corrosion by forming a protective layer of zinc?

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

Why do alloys generally exhibit increased resistance to corrosion?

<p>The mixture of metals alters their chemical properties. (A)</p> Signup and view all the answers

What is the primary function of sacrificial protection in preventing corrosion?

<p>To corrode instead of the protected metal. (B)</p> Signup and view all the answers

What is the outcome when calcium is added to water?

<p>It floats on the surface. (A)</p> Signup and view all the answers

What is the result of oxidation at the anode during electrolysis?

<p>The release of electrons. (C)</p> Signup and view all the answers

Which property is NOT true for sulphur as a non-metal?

<p>It can undergo malleability. (C)</p> Signup and view all the answers

What explains the acidic nature of magnesium oxide?

<p>It forms magnesium hydroxide with water. (C)</p> Signup and view all the answers

What characteristic of ionic compounds is highlighted by their ability to conduct electricity?

<p>They dissociate into ions in molten or aqueous forms. (A)</p> Signup and view all the answers

Why are sodium and potassium metals stored under kerosene?

<p>To prevent oxidation from air. (A)</p> Signup and view all the answers

Which statement correctly describes aluminium oxide?

<p>It is amphoteric due to reactions with acids and bases. (C)</p> Signup and view all the answers

What happens to a blue copper sulphate solution when an iron strip is introduced?

<p>It turns pale green due to formation of iron sulphate. (B)</p> Signup and view all the answers

What indicates that magnesium is a metal based on its properties?

<p>It is a good conductor of heat and electricity. (C)</p> Signup and view all the answers

Which of the following accurately reflects the behavior of compounds formed by metals and non-metals?

<p>They typically form ionic compounds. (A)</p> Signup and view all the answers

Flashcards

Metal Extraction

The process of separating metals from their ores.

Metallurgy

The science of extracting and refining metals from ores.

Ore

A mineral from which a metal can be extracted profitably.

Mineral

Naturally occurring element or compound.

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Gangue

Undesirable impurities in an ore.

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Electrolysis

Using electricity to drive chemical reactions.

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Reduction Process

Gain of electrons; metal oxide to metal.

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Self-Reduction

Reduction without external reducing agent.

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Highly Reactive Metals

Metals extracted with electrolysis.

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Moderately Reactive Metals

Metals extracted using reduction.

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Less Reactive Metals

Metals extracted by heating.

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Very Less Reactive Metals

Metals found in free metallic state.

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Thermite Reaction

Using Aluminum to reduce metal oxides.

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Electrolytic Refining

Using electricity to purify metals.

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Corrosion

Deterioration of metals due to environment.

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Coating

Protecting metal by surface layers.

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Alloying

Mixing metals to create new properties.

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Alloy

A homogeneous mixture of metals.

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Galvanization

Protecting iron with zinc.

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Electroplating

Using electricity to coat a metal with another.

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Sacrificial Protection

Protecting one metal by sacrificing another.

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Ionic Compounds

Compounds formed by electron transfer.

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High Melting Point

Ionic compounds require lots of energy to melt.

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Solubility in Water

Ionic compounds often dissolve in water.

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Conductivity (Molten/Aqueous)

Ionic compounds conduct electricity in solution.

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Study Notes

Occurrence of Metals

  • Earth's crust is the primary source of metals; seawater contains soluble salts.
  • Minerals are naturally occurring elements or compounds, while ores are minerals from which metals can be profitably extracted.

Extraction of Metals from Ores

  • Metallurgy refers to the extraction and refinement of metals from ores.
  • Extraction techniques depend on metals' reactivity:
    • Highly Reactive Metals: Extracted via electrolysis due to strong bonds with ore components (e.g., Potassium, Sodium, Calcium, Magnesium).
    • Moderately Reactive Metals: Extracted using the reduction process with agents like coke (e.g., Zinc, Iron, Lead).
    • Less Reactive Metals: Extracted through self-reduction by heating (e.g., Copper, Mercury).
    • Very Less Reactive Metals: Found in free metallic state (e.g., Silver, Gold, Platinum).

Concentration of Ores

  • Gangue (undesirable impurities) must be removed to enrich ores.
  • Low reactivity metals undergo self-reduction with heat, allowing the conversion of sulfide ores to oxides.

Methods of Metal Extraction

  • Thermite Reaction: A mix of concentrated oxide ore and aluminum reduces metal oxide to metal (e.g., Chromium and Iron).

  • Electrolytic Reduction: Reactive metals (e.g., Na, K, Mg) are reduced from molten oxides or hydroxides using electric current.

Refining/Purification of Metal

  • Impurities removed during refining include unreacted ore, byproducts, and non-metals.
  • Electrolytic Refining of Copper:
    • Uses impure copper as anode and pure copper as cathode; metal ions reduce on cathode.

Corrosion

  • Gradual deterioration of metals due to moisture, air, or chemicals (e.g., rusting of iron).

Prevention of Corrosion

  • Coating: Paint, oil, or grease prevents moisture and air contact.
  • Alloying: Alloys exhibit enhanced resistance; e.g., stainless steel.
  • Galvanization: Coating iron with zinc for protection from corrosion.
  • Electroplating: Coating one metal with another using electric current.
  • Sacrificial Protection: Mg prevents iron corrosion by undergoing oxidation instead.

Alloys

  • Homogeneous mixtures of metals or non-metals enhance properties like hardness and strength (e.g., Brass = Copper + Zinc, Bronze = Copper + Tin).

Previous Year Questions

  • Questions include arrangements of metals by reactivity, valency details, reactions with water, and features of ionic compounds.
  • Responses involve reasoning about properties of metals vs. non-metals, stimulus for alloy formation, and behaviors within chemical reactions.

Key Points on Ionic Compounds

  • Formed by the transfer of electrons from metals to non-metals.
  • General properties include high melting points, solubility in water, and conductivity in molten and aqueous forms.

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