Reactivity Series of Metals
Chemistry ⇒ Metals and Non-metals
Reactivity Series of Metals starts at 8 and continues till grade 12.
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See sample questions for grade 9
A strip of zinc is placed in copper sulfate solution. What will you observe?
A student adds a piece of magnesium to dilute hydrochloric acid. What gas is evolved?
Arrange the following in order of increasing reactivity: Silver, Iron, Sodium, Zinc.
Arrange the following metals in decreasing order of reactivity: Magnesium, Zinc, Iron, Copper.
Describe what happens when iron is placed in copper sulfate solution.
Explain why copper cannot displace zinc from zinc sulfate solution.
Explain why gold and platinum are used to make jewelry.
Explain why metals like potassium and sodium are not found free in nature.
Explain why potassium is stored under oil.
Explain why sodium cannot be extracted from its ore by reduction with carbon.
Which metal is more reactive: Aluminium or Iron?
Which metal is more reactive: Calcium or Magnesium?
Which metal is more reactive: Iron or Copper?
Which metal is more reactive: Lead or Tin?
Which metal is more reactive: Zinc or Lead?
A solution contains both copper(II) ions and silver(I) ions. If a strip of zinc is placed in the solution, which metal(s) will be deposited on the zinc strip? Explain your answer.
A student places a strip of metal X in a solution of iron(II) sulfate. After some time, a grey deposit forms on the strip and the solution turns pale green. What can you infer about the position of metal X relative to iron in the reactivity series? Explain your reasoning.
Arrange the following metals in order of decreasing ability to displace hydrogen from acids: Tin, Potassium, Lead, Calcium.
Describe how the reactivity series of metals is experimentally determined using displacement reactions.
Explain why aluminium, despite being high in the reactivity series, does not react with cold water or dilute acids as vigorously as expected.
