Inorganic Chemistry

The reactivity series below shows the order of metals from most to least reactive. Potassium, Sodium, Lithium, Calcium, Magnesium, Zinc, Iron, Copper.

Arrange the following three metals in order of reactivity, from most reactive to least reactive: magnesium, copper, iron.

Iron(III) oxide reacts with aluminium powder when heated.

Write a word equation for this reaction.

Explain which substance is oxidised and which substance is reduced in this reaction, in terms of oxygen transfer.

In the reaction above, which metal is displaced from its oxide?

State what is meant by a displacement reaction involving a metal oxide.

When carbon is heated with iron(III) oxide, the following reaction occurs:

Identify which substance is reduced in this reaction and explain your answer in terms of oxygen transfer.

Name one use of carbon as a reducing agent in industry.

Explain why carbon cannot be used to extract magnesium from magnesium oxide.

Use the reactivity series to explain why this reaction occurs. Identify which metal is displaced and why.

In terms of electron transfer, describe what happens to aluminium and what happens to iron(III) oxide in the reaction above. Use your answer to part (a) to help you.

State the general equation for the reaction of a metal with cold water.

Iron does not react with cold water, but does react with copper(II) sulfate solution.

Potassium reacts vigorously with cold water. Complete the ionic equation for this reaction and identify the gas produced:

A student adds small pieces of magnesium, iron, and copper to separate test tubes containing dilute hydrochloric acid. State the trend in reactivity observed for these three metals with dilute acids.

Give one observation the student would make when magnesium reacts with dilute hydrochloric acid.

Using the data in the table, identify the most reactive and the least reactive metal.

A new, unfamiliar metal 9 is found to react with dilute hydrochloric acid and produces a temperature change greater than zinc but less than magnesium. Predict, using the reactivity series, where 9 would be placed relative to magnesium and zinc. Explain your answer.

Use the data to arrange the three metals from most reactive to least reactive with dilute sulfuric acid.

Write a balanced chemical equation (with state symbols) for the reaction between zinc and dilute sulfuric acid.

Explain why the student must use the same number of moles, rather than the same mass, of each metal to fairly compare their reactivity.

A metal called cobalt is placed between iron and copper in the reactivity series. Predict whether cobalt will react with dilute sulfuric acid under the same conditions. Give a reason for your answer.

Calculate the temperature rise for each metal. Complete the table below.

Based on your answers to part a, describe and explain the trend in reactivity of these metals with dilute hydrochloric acid.

Predict the temperature rise the student would expect if she repeated the experiment using 0.010 mol of chromium. Explain your answer.

State the two conditions necessary for iron to rust.

Describe how galvanising protects iron from rusting. Include what metal is used and how it provides two types of protection.

Ships are often fitted with blocks of magnesium on their steel hulls. Explain how these magnesium blocks protect the iron hull from rusting.

Explain why the iron hull will eventually begin to rust if the magnesium blocks are not replaced.

Describe the conditions required for iron to rust. (2 marks)

Explain how galvanising prevents rusting, even if the zinc coating is scratched. (2 marks)

Large steel ships are often protected from rust by attaching blocks of a different metal to their hulls.

Explain how galvanising protects iron from rusting, and why this method is more effective than simply painting the iron.

A buried iron pipeline is protected by attaching solid blocks of a more reactive metal. Using the result of part (a), explain why these 'sacrificial anode' blocks must be replaced regularly. In your answer, explain why the metal used for sacrificial protection must be more reactive than iron.