Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Unit
Inorganic Chemistry
869 practice questions
Topics covered
- The Alkali Metals85 practice questions
- The Halogens86 practice questions
- Gases in the Atmosphere86 practice questions
- Reactivity Series163 practice questions
- Extraction and Uses of Metals128 practice questions
- Acids, Alkalis and Titrations83 practice questions
- Acids, Bases and Salt Preparations156 practice questions
- Chemical Tests68 practice questions
Practice questions
161–170 of 869
Question 161
2 marks · Hard
Answer and see the solution →Astatine is the element below iodine in Group 7 of the Periodic Table.
Predict the colour and state of astatine at room temperature. Justify your predictions using group trends.
Question 162
5 marks · Easy
Answer and see the solution →Chlorine, bromine and iodine are Group 7 elements. In the laboratory, a student mixes chlorine water with potassium iodide solution.
(a)[1 mark]Write the ionic equation for the reaction that occurs between chlorine water and potassium iodide solution.
(b)[1 mark]State what you would observe during this reaction.
(c)[2 marks]Explain why chlorine is able to displace iodine from potassium iodide solution, but bromine cannot.
(d)[1 mark]Predict what you would see if bromine water was added to potassium chloride solution. Explain your answer.
Question 163
5 marks · Easy
Answer and see the solution →A laboratory investigation compares the ability of Group 7 elements to act as oxidising agents. The electronic structures of chlorine and bromine are shown below.
(a)[2 marks]Explain, in terms of electron transfer, why the reaction between chlorine and iodide ions is classed as a redox reaction.
(b)[2 marks]Chlorine is a stronger oxidising agent than bromine. Explain why, using ideas about the electronic configuration of halogen atoms.
(c)[1 mark]State how the reactivity of the halogens changes as you go down the group.
Question 164
5 marks · Easy
Answer and see the solution →Iodine is unable to displace bromine from potassium bromide solution. Use knowledge of redox and electronic structure to answer the following:
(a)Explain, in terms of electron transfer, what occurs to the bromide ions in a displacement reaction with chlorine.
(b)[2 marks]State whether iodine acts as an oxidising agent or reducing agent in displacement reactions, and explain your answer.
(c)[3 marks]Using information about electronic configuration, explain why chlorine is more reactive than bromine.
Question 165
5 marks · Easy
Answer and see the solution →A student adds bromine water to a solution of potassium iodide.
(a)[1 mark]Write the ionic equation for the reaction that takes place.
(b)[2 marks]State and explain what you would observe when bromine water is added to potassium iodide solution.
(c)[2 marks]Predict whether a similar reaction would occur if the student added iodine solution to potassium bromide solution. Explain your answer in terms of halogen reactivity.
Question 166
6 marks · Normal
Answer and see the solution →(a)[1 mark]State the physical state and color of chlorine at room temperature.
(b)[2 marks]Describe what you would observe when chlorine gas is bubbled through a solution of potassium iodide.
(c)[2 marks]Write a balanced chemical equation for the reaction in part b.
(d)[1 mark]Explain why this reaction happens in terms of the reactivity of the halogens.
Question 167
6 marks · Normal
Answer and see the solution →(a)[2 marks]Explain, with the aid of a balanced equation, what happens when sodium reacts with bromine.
(b)A student adds bromine water to a solution of potassium iodide in a test tube.
(i)[1 mark]State what you would observe.
(ii)[2 marks]Write a balanced equation for the reaction.
(iii)[1 mark]Explain why bromine can displace iodine in this reaction but not chlorine.
Question 168
6 marks · Normal
Answer and see the solution →A teacher wants to compare the reactivity of chlorine, bromine and iodine using displacement reactions with metal halide solutions.
(a)[2 marks]Chlorine is bubbled into a solution of potassium bromide. The solution turns orange. Explain why this colour change occurs. Include what is formed.
(b)[2 marks]A student adds bromine water to a solution of potassium chloride. No visible change is seen. Explain this observation, referring to relative reactivity.
(c)[2 marks]State and explain which halogen is the least reactive out of chlorine, bromine and iodine.
Question 169
7 marks · Hard
Answer and see the solution →This question is about the properties and reactions of halogens.
(a)[2 marks]State the physical state and colour of bromine and iodine at room temperature (20 °C).
(b)Aqueous chlorine is added to a solution containing potassium iodide. The solution changes colour.
(i)[2 marks]Write the ionic equation, including state symbols, for the reaction that takes place.
(ii)[2 marks]Explain why chlorine can displace iodine from potassium iodide solution but not the other way around.
(iii)[1 mark]Identify the oxidising agent and the substance that is reduced in this reaction.
Question 170
7 marks · Hard
Answer and see the solution →This question is about halogens and redox processes in their reactions.
(a)[2 marks]Describe the appearance and physical state of chlorine and iodine at room temperature.
(b)Bromine water is added to a solution of potassium iodide. The following reaction occurs:
(i)[2 marks]In terms of oxidation and reduction, explain which species is reduced and which is oxidised in the reaction.
(ii)[3 marks]State the colour change that is observed during this reaction. Explain the reason for this change.