8.3. Group VII properties
A subsection of Chemistry, 0620, through 8. The Periodic Table
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This question is about the halogens and compounds of the halogens. The properties of some halogens are shown in the table. element melting point in °C boiling point in °C density of liquid at its boiling point in g / cm3 atomic radius in nm chlorine –101 –35 0.099 bromine –7 3.12 0.114 iodine 4.93 0.133 astatine 6.35 Complete the table to estimate: ● ● the density of liquid chlorine ● ● the boiling point of iodine.  Describe the trend in the atomic radius of the halogens down the group. Predict the physical state of bromine at 50 °C. Give a reason for your answer. Bromine reacts with an aqueous potassium salt to form iodine and a different potassium salt. Complete the word equation for this reaction. bromine + iodine +  Fluorine is above chlorine in GroupVII of the Periodic Table. Explain, using ideas about the reactivity of the halogens, why chlorine does not react with aqueous sodium fluoride. Balance the chemical equation for the reaction of fluorine with ammonia. NH3 + F2 N2 + 6HF A compound of fluorine has the formula XeO3F2. Complete the table to calculate the relative molecular mass of XeO3F2. Use your Periodic Table to help you. type of atom number of atoms relative atomic mass xenon oxygen 3 × 16 = 48 fluorine  relative molecular mass =  The compound XeO3F2 readily undergoes reduction. What is meant by the term reduction? 
0620_w19_qp_31
THEORY
2019
Paper 3, Variant 1
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This question is about the halogens and compounds of the halogens. The properties of some halogens are shown in the table. element melting point in °C boiling point in °C density of liquid at boiling point in g / cm3 colour fluorine –220 –188 1.51 chlorine –101 1.56 light green bromine –7 3.12 red-brown iodine grey-black Complete the table to estimate: ● ● the boiling point of chlorine ● ● the density of iodine.  Describe the trend in the melting points of the halogens down the group. Predict the physical state of bromine at –20 °C. Which one of the following is most likely to be the colour of fluorine? Tick one box. dark green light grey-black light yellow purple  Chlorine reacts with an aqueous potassium salt to form iodine and a different potassium salt. Complete the word equation for this reaction. chlorine + iodine +  When aqueous sodium fluoride is added to chlorine, no reaction occurs. Explain, using ideas about the reactivity of the halogens, why no reaction occurs. State one use of chlorine. Aqueous silvernitrate is used to test for chloride ions and iodide ions. The solutions are first acidified with dilute nitric acid. Explain why dilute hydrochloricacid is not used to acidify the solutions. Complete the table to show the expected observations. ion observations on adding aqueous silver nitrate chloride (Cl –) iodide (I–)  A compound of chlorine has the formula C6H4Cl 2. Complete the table to calculate the relative molecular mass of C6H4Cl 2. Use your Periodic Table to help you. type of atom number of atoms relative atomic mass carbon 6 × 12 = 72 hydrogen chlorine  relative molecular mass =  
0620_w19_qp_32
THEORY
2019
Paper 3, Variant 2
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