Metal Reactivity and Extraction Quiz
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Questions and Answers

What observation would you expect when a freshly cut piece of sodium is exposed to the air?

  • It turns a reddish-brown colour.
  • It remains shiny and grey.
  • It starts to bubble and produces gas.
  • It quickly becomes dull and white. (correct)

    • Why are gold and platinum considered unreactive metals?

  • They react explosively with water.
  • They react readily with oxygen at room temperature.
  • They form strong acidic solutions.
  • They do not easily participate in chemical reactions. (correct)

    • What is the term used to describe the arrangement of metals based on their reactivity?

  • The metallic bond sequence
  • The reactivity series (correct)
  • The oxidation table
  • The atomic number chart

    • What process is utilized to extract metals from their oxides, based on the reactivity series?

    <p>Displacing a less reactive metal by a more reactive one.</p> Signup and view all the answers

    In the extraction from ores, what is the role of carbon or carbon monoxide in the process?

    <p>As a reducing agent to gain oxygen from the metal oxide</p> Signup and view all the answers

    What is the general word equation for extracting metals using carbon?

    <p>metal oxide + carbon → metal + carbon dioxide</p> Signup and view all the answers

    What is the purpose of the lid on the crucible during the extraction of copper from copper oxide using carbon?

    <p>To prevent carbon from reacting with oxygen in the air</p> Signup and view all the answers

    A metal's position in the reactivity series indicates its tendency to:

    <p>Undergo chemical reactions and form new substances</p> Signup and view all the answers

    Which of the following best describes the behavior of a highly reactive metal when exposed to oxygen?

    <p>It will quickly form a visible oxide layer.</p> Signup and view all the answers

    What is a key general characteristic of metals that are placed lower in the reactivity series?

    <p>They are less likely to take part in chemical reactions</p> Signup and view all the answers

    Considering their reactivity, why are some metals extracted from their oxides by displacement?

    <p>Because they are less reactive than other metals.</p> Signup and view all the answers

    Based on the reactivity series, what determines whether a metal will react with water, acid, or oxygen?

    <p>Its level of reactivity</p> Signup and view all the answers

    Study Notes

    Metal Reactivity and Extraction

    • Metals vary in their reactivity, some reacting easily, others not.
    • Reactivity series: A list ordering metals from most to least reactive. A more reactive metal can displace a less reactive one from its compounds. Reactivity is a substance's tendency to undergo a chemical reaction.
    • Reactive metals readily form new substances. E.g., Sodium reacts rapidly with air, losing its shine. This is due to the high reactivity of sodium.
    • Unreactive metals, like gold and platinum, resist reacting with air even at high temperatures. These metals are unreactive, meaning they do not easily take part in chemical reactions.
    • Metal reactivity affects extraction methods. Reactivity affects what reactions the metal participates in. Metals can react with water, acid, and oxygen.

    Extracting Metals

    • Metal ores: Natural rocks containing usable amounts of metals or metal compounds.
    • Extraction method depends on metal's reactivity and ore stability.
    • In all cases, metal ions gain electrons to form metallic atoms.

    Extracting Unreactive Metals

    • Heating the ore is enough to extract the metal.
    • Example: Heating silver oxide produces silver metal and oxygen.
      • Word equation: silver oxide → silver + oxygen
      • Chemical equation: 2 Ag₂O(s) → 4 Ag(s) + 2 O₂(g)

    Extracting Reactive Metals

    • Ores of reactive metals need carbon or carbon monoxide.
    • Carbon is more reactive than some metals, so can extract them from their oxides.
    • Example metals: zinc, iron, tin, lead, and copper(least reactive of these).
    • General word equation: metal oxide + carbon → metal + carbon dioxide
    • Practical example: extracting copper from copper oxide.
    • Mix copper oxide powder with carbon powder.
    • Heat strongly in a crucible (covered to prevent oxygen reaction with carbon).
    • Filter out the copper pieces via water.
    • Word equation: copper oxide + carbon → copper + carbon dioxide
    • Chemical equation: 2 CuO(s) + C(s) → 2 Cu(s) + CO₂(g)

    Extracting Very Reactive Metals

    • Melting and electrolysis (using direct current) are crucial for very reactive metals, including those used in solutions or solutions themselves.
    • Ions get electrons at the negative electrode, forming metal atoms.
    • Electrolysis can also extract less reactive metals like copper.
    • Example: Magnesium is a very reactive metal. It ignites when heated and burns with a brilliant white flame.

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    Description

    Test your knowledge on the reactivity of metals and their extraction methods. This quiz covers the reactivity series, how different metals react, and the extraction processes for both reactive and unreactive metals. Challenge yourself with questions that explore the science behind metal ores and chemical equations involved in metal extraction.

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