Metals and Non-Metals Overview
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Questions and Answers

Which of the following properties is NOT typically associated with metals?

  • Malleable
  • Gains electrons easily (correct)
  • Good conductors of electricity
  • Ductile

    • Metalloids possess only properties of metals.

    False

    Name one exception to the general property of metals being hard.

    Sodium or Potassium

    Mercury is an exception to the general state of metals because it exists as a ______ at room temperature.

    <p>liquid</p> Signup and view all the answers

    Which of the following is a characteristic of non-metals?

    <p>Can be gases, liquids, or solids</p> Signup and view all the answers

    Match the types of metals with their properties:

    <p>Sodium = High reactivity with oxygen Iron = Low reactivity with oxygen Beryllium = Amphoteric metal Lead = Amphoteric metal</p> Signup and view all the answers

    Iodine is an example of a non-metal that is lustrous.

    <p>True</p> Signup and view all the answers

    What is the term for metals that can react both as acids and bases?

    <p>Amphoteric metals</p> Signup and view all the answers

    Which of the following metals reacts explosively with cold water?

    <p>Sodium</p> Signup and view all the answers

    Gold reacts with water.

    <p>False</p> Signup and view all the answers

    What is the main purpose of galvanization?

    <p>To protect iron or steel from corrosion by coating it with zinc.</p> Signup and view all the answers

    The process of removing impurities from metals after extraction is called __________.

    <p>refining</p> Signup and view all the answers

    Match the following metals with their extraction methods:

    <p>Sodium = Electrolysis Copper = Roasting and Reduction Zinc = Roasting and Calcination Aluminium = Electrolysis</p> Signup and view all the answers

    Which of the following statements about nitric acid is true?

    <p>It is a strong oxidizer.</p> Signup and view all the answers

    Metals like aluminium only react with hot water.

    <p>True</p> Signup and view all the answers

    What is the byproduct of roasting zinc sulfide?

    <p>Sulfur dioxide</p> Signup and view all the answers

    In metallurgical terms, __________ are the impurities found in ores.

    <p>gangue</p> Signup and view all the answers

    Match the following phenomena with their effects:

    <p>Corrosion of Iron = Rust formation Corrosion of Copper = Green patina Corrosion of Silver = Black tarnish Corrosion of Aluminum = Oxide layer</p> Signup and view all the answers

    What is the primary use of aqua regia?

    <p>Dissolving noble metals</p> Signup and view all the answers

    Electrolysis is primarily used for extracting low reactive metals.

    <p>False</p> Signup and view all the answers

    What is the reaction process that involves heating an ore in the absence of air called?

    <p>Calcination</p> Signup and view all the answers

    What does the process of enrichment in metallurgy involve?

    <p>Removing gangue particles from the ore</p> Signup and view all the answers

    Study Notes

    What are Metals and Non-Metals?

    • Metals are elements that can lose electrons from their outermost shell.
    • Non-metals are elements that can gain electrons from their outermost shell.
    • Metalloids have properties of both metals and non-metals.
    • Noble Gases have a completely filled outermost shell; they neither lose nor gain electrons.

    Physical Properties of Metals and Non-Metals

    • Malleability: Ability to be hammered into thin sheets; most metals are malleable, but exceptions exist.
      • Exceptions: Arsenic and Mercury
    • Ductility: Ability to be drawn into thin wires; most metals are ductile, but exceptions exist.
    • Hardness: Most metals are hard, but exceptions exist.
      • Exceptions: Sodium and Potassium (can be cut with a knife)
    • Sonority: Ability to produce a ringing sound when struck; most metals are sonorous, but Mercury is an exception.
    • Lustre: Ability to shine or reflect light; most metals are lustrous, but some non-metals are lustrous.
      • Exceptions: Iodine and Graphite
    • Melting and Boiling Point: Metals generally have high melting and boiling points, but some exceptions exist.
      • Exceptions: Gallium and Cesium (melt at room temperature)
    • Electrical Conductivity: Most metals are good conductors of electricity, but exceptions exist.
      • Exceptions: Mercury and Lead
    • Thermal Conductivity: Most metals are good conductors of heat, but exceptions exist.
      • Exception: Graphite
    • State: Most metals are solid at room temperature; Mercury is liquid. Non-metals exist in solid, liquid, or gaseous states at room temperature.
    • Density: Metals are denser than non-metals, with an exception for Mercury.
      • Exceptions: Mercury (a liquid at room temperature.)

    Chemical Properties of Metals and Non-Metals

    • Reaction with Oxygen: Metals react with oxygen to form metal oxides.
      • High Reactivity Metals: Sodium and Potassium react rapidly with oxygen.
      • Low Reactivity Metals: Iron reacts slowly with oxygen.
      • Amphoteric Metals: Form both acidic and basic oxides.
        • Amphoteric Example Metals: Beryllium, Zinc, Tin, Lead, Aluminium, and Antimony ("Sub-Jane Padho Likho Aur BanoJanab")
    • Reaction with Water: Most metals react with water to form metal hydroxides.
      • Highly Reactive Metals: Sodium reacts explosively with cold water.
      • Less Reactive Metals: Aluminium reacts with steam (hot water).
      • Least Reactive Metals: Gold does not react with water.
      • Non-Metals: Non-metal oxides react with water to form acids.
    • Reaction with Acids: Metals react with dilute acids to form salts and hydrogen gas.
      • Nitric Acid (HNO3): A strong oxidizer; does not release hydrogen in most reactions.
        • Exceptions with HNO3: Magnesium and Manganese.
    • Aqua Regia: A highly corrosive mixture (conc. nitric acid and hydrochloric acid, 1:3 molar ratio) used to dissolve noble metals (gold and platinum).

    Reactivity Series

    • Reactivity Series: A series of metals arranged by decreasing reactivity. Used to predict if one metal will displace another in a salt solution.
    • Memory Aid: "Katerina ne Car maangi Alto, Jan (Sangeet) Cold Water ko bhi Denge na to bhi ye bade Khatarnaak Tarike se React Karenge!"

    Metallurgy

    • Metallurgy: The science and technology of extracting metals from ores and processing them into desirable forms.
    • Minerals: Naturally occurring elements or compounds in the Earth's crust.
    • Ores: Minerals from which metals can be extracted economically.
    • Gangue: Impurities in the ore.

    Methods of Extraction of Metals

    • Enrichment of Ore: Removing gangue from ore.
    • Extraction of Metals:
      • Low Reactive Metals (e.g., Copper):
        • Roasting: Heating the ore with oxygen to convert sulfide to metal oxide.
        • Reduction: Reducing the metal oxide to get the pure metal.
        • Refining: Removing impurities from the extracted metal.
      • Mid Reactive Metals (e.g., Zinc):
        • Roasting (sulfide ores): Same as for low reactive metals.
        • Calcination (carbonate ores): Heating the ore in the absence of air.
        • Reduction: Similar to low reactive metals.
        • Refining: Removing impurities.
      • High Reactive Metals (e.g., Sodium):
        • Electrolysis: Using electric current to extract the metal from a molten salt.
        • Refining: Similar to other refining methods.

    Important Points to Remember

    • Reactivity series determines the extraction method.
    • Roasting, calcination, and reduction are key steps in extraction.
    • Electrolysis is a vital method for extracting highly reactive metals.
    • Refining is the final step for purity.

    Extraction of Metals

    • Zinc Oxide Extraction: Heating zinc sulfide in air to produce zinc oxide and sulfur dioxide.
    • Reduction: Removing oxygen from a compound.
    • Thermite Reaction: Aluminum reducing iron oxide to iron, generating a lot of heat; used in joining railway tracks.
    • Electrolytic Reduction: Extracting highly reactive elements from molten salts.
    • Electrolytic Refining of Copper: Impure copper (anode) and pure copper (cathode) in a copper sulfate solution resulting in pure copper on cathode, and anode mud.

    Important Concepts and Processes

    • Roasting: Heating ore (typically sulfides) in the presence of oxygen, producing sulfur dioxide.
    • Calcination: Heating ore (typically carbonates) in the absence of oxygen, producing carbon dioxide.

    Corrosion

    • Corrosion: Metal reactions with the environment forming new compounds, changing properties.
    • Examples:
      • Silver reacting with sulfur compounds to form black silver sulfide.
      • Copper reacting with carbon dioxide and water to form green copper carbonate.
      • Iron reacting with oxygen and water to form brown iron oxide (rust).

    Alloys

    • Alloys: Homogeneous mixtures of two or more metals, or a metal and a non-metal.
    • Alloy Purposes: To improve the properties of metals (strength, hardness, corrosion resistance).
    • Examples:
      • Steel (iron, chromium, nickel)
      • Brass (copper, zinc)
      • Solder (lead, tin)

    Galvanization

    • Galvanization: Coating iron or steel with zinc.
    • Zinc's higher reactivity protects iron from corrosion; zinc acts as a sacrificial anode.

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    Description

    This quiz explores the definitions and physical properties of metals and non-metals, including characteristics such as malleability, ductility, hardness, sonority, and lustre. It also touches upon exceptions and the role of metalloids and noble gases. Test your knowledge on fundamental concepts of chemistry!

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