Salts are ionic compounds they are widely used to make everyday products. In this unit we will look at how we can make salts and look a littlemore deeply at what acids are and how they react with other substances. Before you start this unit is is vital that you understand the ionic bonding principles in the C3 Structure and Bonding topic .

Specification links

• Set 1 all of 4.4.1 and 4.4.2

• Set 2 all of 5.4.1 and 5.4.2

• Set 3 all of 5.4.1 up to 5.4.2.4

Task 1b: Listen to the podcast for an overview of this topic:

Task 3b: Make notes that:

• Define displacement reaction

• Write word and balanced symbol equations for the reactions between:

• Iron Sulphate (FeSO₄) and Magnesium

• Copper Sulphate (CuSO₄) and Magnesium

• Copy and complete the word equations on slide 19 and self mark using slide 20

• Define oxidation and reduction in terms of losing or gaining oxygen

Set 1 and 2 only:

• Define oxidation and reduction in terms of losing or gaining electrons.

• Identify the metal that is oxidised and reduced in the following reactions:

• Magnesium + Copper sulphate → Magnesium sulphate + Copper

• Potassium + Zinc chloride → Potassium chloride + Zinc

• Calcium + Aluminium nitrate → Calcium nitrate + Aluminium

• List the steps involved in writing an ionic equation.

• Write the word, symbol and ionic equations for the following reactions:

• Copper nitrate + Magnesium

• Iron chloride + Sodium

• Aluminium sulphate + Calcium

• Magnesium nitrate + Potassium

• Copper chloride + Aluminium

• Zinc sulphate + Sodium

Task 4b:

• Define native

• Define ore

• Describe how metals less reactive than carbon are extracted from their ores

• Write a word and balanced symbol equation to show the reduction of iron oxide with carbon.

• Write a word and symbol equation to show the reduction of tungsten with hydrogen

Set 1 and 2 only

• Describe what a half equation shows

• Write a half equation to show the reduction of lead from lead oxide (PbO)

• Write the ionic equation and 2 half equations for the following reaction:

Sodium + Copper sulphate → Sodium sulphate + Copper

Task 4c: Answer the exam questions and self mark

Task 5b: Make notes that:

• Give the general word equation for the reaction between a metal and acid

• Name the salts formed from hydrochloric acid, sulphuric acid and nitric acid

• Name the salts formed in the following reactions:

• Sodium + Sulphuric acid →

• Calcium + Nitric acid →

• Lithium + Hydrochloric acid →

• Write the word and balance symbol equations for the reaction between zinc and sulphuric acid

• Set 1 and 2 only: Write the ionic and half equations for the reaction between zinc and sulphuric acid

Task 6b: Make notes that:

• Describe how to work out the formulae of salts

• Give the formula of the following salts:

• Ammonium nitrate

• Lithium sulphate

• Aluminium chloride

• Copper(II) chloride

• Define a base

• Define an alkali

Task 4d: Answer the exam question (mark scheme on slide 23):

A student investigated the reactions of copper carbonate and copper oxide with dilute hydrochloric acid. In both reactions one of the products is copper chloride.

Describe how a sample of copper chloride crystals could be made from copper carbonate and dilute hydrochloric acid.

(4 marks)

Task 7b: Make notes that:

• Give the general word equation for the reaction between an acid and an alkali

• Write the word and balance symbol equations for the reaction between hydrochloric acid and sodium hydroxide

• Give the general word equation for the reaction between an acid and a carbonate

• Write the word and balance symbol equations for the reaction between hydrochloric acid and calcium carbonate

Set 1 and 2 only:

• Write the ionic equation for the reaction between hydrochloric acid and sodium hydroxide

• Write the ionic equation for the reaction between hydrochloric acid and calcium carbonate

• Complete the questions on slide 12 and self mark using slide 13

Task 7c: Answer the exam questions and self mark

Task 8b: Make notes that:

• State the ion all acids contain

• Describe the relationship between pH and the concentration of H⁺ ions

• State the ion all alkalis contain

• Describe how to measure the pH of a solution

Set 1 and 2 only:

• Describe the difference between a strong and weak acid

Task 8c : Answer the exam questions and self mark