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
61–70 of 359 · Easy
Question 61
1 mark · Easy
Answer and see the solution →State the colour you would expect for the vapour of bromine at room temperature based on group trends.
Question 62
3 marks · Easy
Answer and see the solution →This question is about why chlorine is more reactive than iodine.
(a)[1 mark]State the charge on the ion formed when a chlorine atom gains an electron.
(b)[2 marks]Describe, using electronic configuration, why a chlorine atom is better at gaining an electron than an iodine atom.
Question 63
2 marks · Easy
Answer and see the solution →Explain, in terms of electronic configuration, why bromine is less reactive than chlorine.
Question 64
3 marks · Easy
Answer and see the solution →Below is a table of some Group 7 elements and their melting points.
Melting points of some halogens Element Melting Point (°C) Fluorine -220 Chlorine -101 Bromine -7 Iodine 114 (a)[1 mark]Describe the trend in melting point as you go down Group 7.
(b)[2 marks]Predict whether astatine would have a higher or lower melting point than iodine. Give a reason for your answer.
Question 65
1 mark · Easy
Answer and see the solution →State how many electron shells are completely full in a chlorine atom.
Question 66
3 marks · Easy
Answer and see the solution →This question is about the properties of the halogens.
(a)[1 mark]What is the formula of the ion formed when iodine forms an ionic salt?
(b)[2 marks]Describe the colour and state of iodine at room temperature.
Question 67
2 marks · Easy
Answer and see the solution →The table below gives the melting points of chlorine and bromine (both Group 7 elements):
Element Melting point (°C) Chlorine -101 Bromine -7 Iodine is the next element down the group after bromine. Use the data to estimate a likely melting point for iodine and explain your reasoning based on group trends.
Question 68
2 marks · Easy
Answer and see the solution →A chlorine atom can react to form a chloride ion. Calculate the total number of electrons in this chloride ion. Explain your answer using the electronic configuration.
Question 69
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 70
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.