2024-04-09T13:34:22+03:00[Europe/Moscow] en true <p>Metal + oxygen = ?</p>, <p>Oxidation reaction</p>, <p>Reduction reaction</p>, <p>What happens when group 1 reacts with water</p>, <p>Displacement reaction</p>, <p>Oxidation is the gain/loss of electrons</p><p>Reduction is the gain/loss of electrons</p>, <p>2e+ has this lost or gain electrons</p>, <p>Acid produce hydrogen ions (??) in aqueous solutions </p>, <p>Bases</p>, <p>Bases soluble in water also called ???</p>, <p>Alkalis produce hydroxide ions (???) in aqueous solutions </p>, <p>Is 0 on the pH scale acid or alkali </p>, <p>Acid + Metal = ???</p>, <p><strong>Neutralisation</strong></p>, <p>3 common salts</p>, <p>Acid + Carbonate =</p>, <p>Making soluble salts</p>, <p>Strong acids partially/fully ionise in aqueous solutions</p><p>Weak acids partially/fully ionise in aqueous solutions</p>, <p>Positive Electrode</p>, <p>Negative Electrode</p>, <p>Positive ions attracted to Anode or Cathode</p>, <p>Anode is oxidation (loss) / reductions (gain)</p>, <p>Metals more reactive than carbon extracted with ?</p><p>Metals less reactive than carbon extracted with ?</p>, <p>Hydrogen produced at cathode if metal more reactive then ??</p>, <p>Oxygen is always produced at anode unless what?</p>, <p>Electrolysis practical</p> flashcards
Chemistry Paper 1 - Chemical Reactions

Chemistry Paper 1 - Chemical Reactions

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  • Metal + oxygen = ?

    Metal oxide

  • Oxidation reaction

    gaining oxygen loss electron

  • Reduction reaction

    losing oxygen gain electron

  • What happens when group 1 reacts with water

    Reacts vigorously and produces alkaline solution

  • Displacement reaction

    A more reactive element can displace a less reactive element from its compound

  • Oxidation is the gain/loss of electrons

    Reduction is the gain/loss of electrons

    LOSS

    GAIN

  • 2e+ has this lost or gain electrons

    lost

  • Acid produce hydrogen ions (??) in aqueous solutions

    H+

  • Bases

    chemicals which can neutralise acid and produce salt n water

  • Bases soluble in water also called ???

    alkalis

  • Alkalis produce hydroxide ions (???) in aqueous solutions

    OH-

  • Is 0 on the pH scale acid or alkali

    Acid

  • Acid + Metal = ???

    Salt + Hydrogen

  • Neutralisation

    acid and a base react to form water and a salt

  • 3 common salts

    Chloride

    Sulfate

    Nitrate

  • Acid + Carbonate =

    Salt + Water + Carbon Dioxide

  • Making soluble salts

    Start with a fixed amount of hydlochoric acid

    Gently heat until almost boiling

    Add copper oxide and stir - keep repeating until it doesn't the oxide doesn't disappear after stirring anymore

    Use filtration to remove unreacted copper oxide

    Place Copper sulfate in evaporating dish and heat until half remains

    Leave it for 24h for crystals to form

    Scrape onto paper towel and pat it dry

  • Strong acids partially/fully ionise in aqueous solutions

    Weak acids partially/fully ionise in aqueous solutions

    Fully

    partially

  • Positive Electrode

    Anode - lack of electrons

  • Negative Electrode

    Cathode - covered with electrons

  • Positive ions attracted to Anode or Cathode

    Cathode

  • Anode is oxidation (loss) / reductions (gain)

    Oxidation

  • Metals more reactive than carbon extracted with ?

    Metals less reactive than carbon extracted with ?

    Electrolysis

    Displacement with carbon

  • Hydrogen produced at cathode if metal more reactive then ??

    Hydrogen (only copper silver less reactive than hydrogen btw)

  • Oxygen is always produced at anode unless what?

    Unless there a halogen ion and in that case that halogen is produced

  • Electrolysis practical

    use a measuring cylinder to add 40 ml of copper chloride solution into a beaker

    place two graphite rods into the copper sulfate solution - attaching one electrode to the negative terminal of a dc supply, and the other electrode to the positive terminal

    place two small test tubes over each electrode to collect any gases produced

    turn on the power supply and observe what happens at each electrode

    test any gas produced by holding a piece of blue litmus next to the electrode, or by holding a lit splint next to it

    record your observations and the results of your tests

    repeat steps 1‒6 using sodium chloride solution