Reactivity series, displacement, extraction methods: Practice Questions

Which of the following statements correctly matches a metal to its most likely occurrence in nature and its corresponding extraction method?

A student is given three metals, X, Y, and Z, and performs the following experiments:

(1) X reacts with dilute hydrochloric acid to produce hydrogen gas, while Y shows no observable reaction with the acid.
(2) A piece of metal X is placed in an aqueous solution of \( \text{Y(II) sulfate} \); a coating of metal Y forms on the surface of X.
(3) The oxide of Z cannot be reduced by heating with carbon powder, whereas the oxide of X is reduced when heated with carbon.

Which of the following identifies the correct order of reactivity (from most reactive to least reactive) and the most likely extraction method for metal Z?

Given the following information about metals D, E, and F:

Which statement about these metals is most accurate?

Which of the following metals is commonly extracted from its ore by heating its oxide with carbon?

Consider the following observations from three experiments:
(1) Metal X reacts with steam but not with cold water.
(2) Metal Y displaces X from an aqueous solution of X(II) sulfate.
(3) The oxide of Z decomposes upon heating alone.
Which of the following represents the increasing order of reactivity of the three metals?

Identify the gas produced when lead(II) oxide (\( \text{PbO} \)) is heated with carbon, and state the type of chemical change the \( \text{PbO} \) undergoes.

When iron powder is added to an aqueous solution of tin(II) chloride, a grey solid is deposited on the surface of the iron. Identify the oxidizing agent in this reaction and explain why the reaction occurs with reference to the reactivity series.

Metal X can displace lead from \(\text{Pb(NO}_3)_2(\text{aq})\) but its oxide cannot be reduced by heating with carbon, whereas metal Y is found naturally in its native state. Compare the stability of the compounds formed by X and Y, and explain how this determines the order of their discovery by humans.

The timeline of metal discovery is closely related to the reactivity of metals. Lead has been used since ancient times, while magnesium was not isolated until the early 19th century.

(a) Describe a laboratory method to extract lead from lead(II) oxide (\( \text{PbO} \)).

(b) Explain why the method described in (a) is unsuitable for extracting magnesium from magnesium oxide (\( \text{MgO} \)).

(c) Name the industrial method used today to extract magnesium from its molten ore.

(d) Suggest why magnesium was discovered much later than lead in human history.

A student investigates the chemical properties and extraction methods of three metals, L, M, and N. The observations from the experiments are summarized below:

(1) Metal L reacts vigorously with cold water to produce a colorless gas and a solution that turns red litmus paper blue.
(2) Metal M does not react with cold water but reacts with steam. Its oxide can be reduced to the metal by heating with carbon powder.
(3) Metal N does not react with steam or dilute hydrochloric acid. It is commonly found in nature as a native element.

(a) Arrange the metals L, M, and N in decreasing order of reactivity. (1 point)
(b) Suggest the industrial extraction method for metal L. Explain why the method used for metal M (reduction with carbon) is unsuitable for the extraction of L. (2 points)
(c) Predict the visible change when a strip of metal M is placed into an aqueous solution of N(II) nitrate. Write a balanced ionic equation for the reaction that occurs. (2 points)