3.2.5 Group VII. Trends in Physical Processes. 70 minutes. 70 marks. Page 1 of 7
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1 3.2.5 Group VII Trends in Physical Processes 70 minutes 70 marks Page 1 of 7
2 Q1. (a) State and explain the trend in electronegativity down Group VII from fluorine to iodine. Trend... Explanation... (i) Describe what you would observe when an aqueous solution of bromine is added to an aqueous solution containing iodide ions. Write an equation for the reaction occurring. Observation... Equation... Explain why bromine does not react with aqueous chloride ions. Describe what you would observe when aqueous silver nitrate is added to separate aqueous solutions of potassium fluoride and potassium bromide. Observation with KF(aq)... Observation with KBr(aq)... (d) Write an equation to show how solid potassium fluoride reacts with concentrated sulphuric acid. (e) Write an equation for the redox reaction of sodium bromide with concentrated sulphuric acid. (Total 11 marks) Q2. (a) Describe and explain the trend in the boiling points of the elements down Group VII from fluorine to iodine. Describe what you would observe when aqueous silver nitrate, followed by dilute aqueous ammonia, is added to separate aqueous solutions of sodium chloride and sodium bromide. Page 2 of 7
3 State the trend in the oxidising abilities of the elements down Group VII from chlorine to iodine. Explain how this trend can be shown by displacement reactions between halogens and halide ions in aqueous solutions. Illustrate your answer with appropriate observations and equations. (7) (Total 15 marks) Q3. (a) State the trend in the boiling points of the halogens from fluorine to iodine and explain this trend. Trend... Explanation... Each of the following reactions may be used to identify bromide ions. For each reaction, state what you would observe and, where indicated, write an appropriate equation. (i) The reaction of aqueous bromide ions with chlorine gas Observation... Equation... The reaction of aqueous bromide ions with aqueous silver nitrate followed by the addition of concentrated aqueous ammonia Observation with aqueous silver nitrate... Equation... Observation with concentrated aqueous ammonia... (iii) The reaction of solid potassium bromide with concentrated sulphuric acid Observation 1... Observation 2... (7) Page 3 of 7
4 Write an equation for the redox reaction that occurs when potassium bromide reacts with concentrated sulphuric acid. (Total 13 marks) Q4. (a) State and explain the trend in electronegativity down Group VII from fluorine to iodine. Trend... Explanation... State what you would observe when chlorine gas is bubbled into an aqueous solution of potassium iodide. Write an equation for the reaction that occurs. Observation... Equation... Identify two sulphur-containing reduction products formed when concentrated sulphuric acid oxidises iodide ions. For each reduction product, write a half-equation to illustrate its formation from sulphuric acid. Reduction product 1... Half-equation... Reduction product 2... Half-equation... Page 4 of 7
5 (d) Write an equation for the reaction between chlorine gas and dilute aqueous sodium hydroxide. Name the two chlorine-containing products of this reaction and give the oxidation state of chlorine in each of these products. Equation... Name of product 1... Oxidation state of chlorine in product 1... Name of product 2... Oxidation state of chlorine in product 2... (5) (Total 14 marks) Q5. (a) State the trend in electronegativity of the elements down Group VII. Explain this trend. Trend... Explanation... (i) State the trend in reducing ability of the halide ions down Group VII. Give an example of a reagent which could be used to show that the reducing ability of bromide ions is different from that of chloride ions. The addition of silver nitrate solution followed by dilute aqueous ammonia can be used as a test to distinguish between chloride and bromide ions. For each ion, state what you would observe if an aqueous solution containing the ion was tested in this way. Observations with chloride ions... Observations with bromide ions... Page 5 of 7
6 (d) Write an equation for the reaction between chlorine and cold, dilute aqueous sodium hydroxide. Give two uses of the resulting solution. Equation... Use 1... Use 2... (Total 12 marks) Q6. (a) Chlorine displaces iodine from aqueous potassium iodide. (i) Write the simplest ionic equation for this reaction... Give one observation that you would make when this reaction occurs..... In bright sunlight, chlorine reacts with water to form oxygen as one of the products. Write an equation for this reaction... Explain why chlorine has a lower boiling point than bromine (Extra space) (Total 5 marks) Page 6 of 7
7 Page 7 of 7
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