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
141–150 of 869
Question 141
5 marks · Hard
Answer and see the solution →Iodine solution is added to potassium chloride solution. No reaction is observed. Consider the redox processes involved in displacement reactions between halogens and halide ions.
(a)[2 marks]Explain, in terms of electron transfer, why iodine does not displace chloride ions from potassium chloride solution.
(b)[2 marks]A reaction does occur when bromine water is added to potassium iodide solution. State which species is oxidised and which is reduced in this reaction.
(c)[1 mark]Write the balanced ionic equation, including state symbols, for the reaction between bromine solution and iodide ions.
Question 142
2 marks · Hard
Answer and see the solution →Complete the ionic equation, including state symbols, for the reaction of fluorine gas with potassium bromide solution.
Question 143
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 144
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 145
2 marks · Easy
Answer and see the solution →Explain, in terms of electronic configuration, why bromine is less reactive than chlorine.
Question 146
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 147
1 mark · Easy
Answer and see the solution →State how many electron shells are completely full in a chlorine atom.
Question 148
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 149
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 150
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.