Reactivity of Metals Practice Questions

A piece of copper foil is heated strongly in air. A black solid forms on the surface of the foil.

Name the black solid.

Complete and balance the symbol equation for this reaction.

$\mathrm{Cu} + \mathrm{O_2} \rightarrow$ ________

Explain why the reaction in part (b) is an oxidation reaction.

Use the results to place the four metals in order of reactivity.

Start with the most reactive metal.

One of the metals is copper.

Give the letter of this metal and a reason for your choice.

Give the meaning of reduction in terms of oxygen.

Name the substance that is reduced in this reaction.

Name the substance that is oxidised in this reaction.

Name the two products of the reaction between calcium and water.

Give one observation the student could make during this reaction.

Complete and balance the symbol equation for the reaction.

$\mathrm{Ca} + \mathrm{H_2O} \rightarrow$ ________ $+$ ________

Copper does not react with cold water or with dilute hydrochloric acid.

What does this tell you about the position of copper in the reactivity series?

Give two observations the student could make.

Write the balanced symbol equation for the reaction, including the formula of each product.

The formula of zinc sulfate is $\mathrm{ZnSO_4}$.

The student then places a clean strip of zinc in magnesium sulfate solution. No reaction takes place.

Explain why.

Write the half equation for the change of iron atoms into iron(II) ions.

Write the half equation for the change of copper ions into copper atoms.

Identify the species that is reduced in this reaction and explain your answer in terms of electrons.

Zinc can be extracted from zinc oxide by heating with carbon, but magnesium cannot be extracted from magnesium oxide in this way.

Explain why.

Iron is extracted from iron(III) oxide, $\mathrm{Fe_2O_3}$, by heating with carbon. Carbon dioxide is also produced.

Balance the equation for this reaction.

____ $\mathrm{Fe_2O_3} +$ ____ $\mathrm{C} \rightarrow$ ____ $\mathrm{Fe} +$ ____ $\mathrm{CO_2}$

Name the substance that is oxidised in the reaction in part (b) and give a reason for your answer.

Lithium reacts rapidly with dilute hydrochloric acid. Copper does not react with dilute hydrochloric acid.

Explain, in terms of electrons and ions, why lithium is more reactive than copper.

Use the results to place the four metals in order of reactivity, starting with the most reactive.

What do the results for metal C show about the position of metal C in the reactivity series?

Give two variables, other than the mass of metal and the volume of acid, that the student must control so that her results are valid.

Suggest one improvement the student could make to increase the repeatability of her results.

Write the balanced symbol equation for the reaction of zinc oxide with carbon.

Name the substance that is reduced in this reaction. Explain your answer.

Use the information in the table to explain how the zinc can be separated from the other substances in the furnace.

Use the results to deduce the order of reactivity of the four metals. Start with the most reactive metal.

Metal Y forms ions with a $2+$ charge. Metal X forms ions with a $1+$ charge.

Write the ionic equation, including state symbols, for the reaction of metal Y with X nitrate solution.

Metal X is silver. Silver is found in the Earth as the metal itself, rather than as a compound.

Explain why.