Reactions of MetalsAQA GCSE Chemistry: Flashcards

Card 1 of 150 of 15 known

Question

What are the three main types of reactions that metals undergo according to the AQA GCSE specification?

Tap or press Space to reveal

Tap card or press Space to flip

See all 15 cards

What are the three main types of reactions that metals undergo according to the AQA GCSE specification?: Reactions with oxygen (forming metal oxides), reactions with water (forming metal hydroxide and hydrogen), and reactions with dilute acids (forming a salt and hydrogen).
Write the general equation for a metal reacting with oxygen.: metal + oxygen → metal oxide Example: 2Mg + O₂ → 2MgO
Write the general equation for a metal reacting with water.: metal + water → metal hydroxide + hydrogen Example: 2Na + 2H₂O → 2NaOH + H₂↑
Write the general equation for a metal reacting with a dilute acid.: metal + dilute acid → salt + hydrogen Example: Zn + 2HCl → ZnCl₂ + H₂↑
Describe the trend in reactivity of metals with water.: Reactivity increases down Group 1. Alkali metals (Na, K) react vigorously with water, whilst less reactive metals (Fe, Cu) do not react with water at room temperature.
Describe the trend in reactivity of metals with dilute acids.: More reactive metals (at the top of the reactivity series) react faster and more vigorously with dilute acids. Metals below hydrogen in the reactivity series do not react with dilute acids.
Define a displacement reaction in terms of metal reactivity.: A displacement reaction occurs when a more reactive metal displaces a less reactive metal from a compound. The more reactive metal loses electrons more readily and takes the place of the less reactive metal.
Write the equation for iron displacing copper from copper sulphate solution.: Fe + CuSO₄ → FeSO₄ + Cu Iron is more reactive than copper, so it displaces the copper.
Write the ionic equation for the displacement of copper by iron from copper sulphate solution (Higher Tier).: Fe(s) + Cu²⁺(aq) → Fe²⁺(aq) + Cu(s) Spectator ions (SO₄²⁻) are omitted.
What observation would you see when iron is added to copper sulphate solution?: The blue colour of the copper sulphate solution fades and disappears. A red/brown precipitate of copper forms on the surface of the iron.
Explain why magnesium is more reactive than copper in terms of electron loss.: Magnesium loses electrons more readily than copper because it has a weaker hold on its outer electrons. Mg loses 2 electrons easily to form Mg²⁺, whilst Cu holds its electrons more strongly.
What is the reactivity series and name three metals in order of decreasing reactivity.: The reactivity series is an ordered list of metals arranged by their ability to lose electrons and form positive ions. Example order: Potassium > Sodium > Magnesium > Iron > Copper
Why do metals below hydrogen in the reactivity series not react with dilute acids?: These metals (such as copper and silver) cannot lose electrons as easily as hydrogen ions can gain electrons. They are less reactive than hydrogen, so hydrogen ions cannot be displaced.
Write the ionic equation for magnesium reacting with hydrochloric acid (Higher Tier).: Mg(s) + 2H⁺(aq) → Mg²⁺(aq) + H₂(g) The Cl⁻ ions are spectator ions and are omitted.
Describe the difference between the reaction of sodium and magnesium with water.: Sodium reacts vigorously with water, moving across the surface and producing hydrogen gas that ignites. Magnesium reacts slowly with cold water but reacts more readily with steam, producing magnesium oxide and hydrogen gas.