11. Group 17
A section of Chemistry, 9701
Listing 10 of 617 questions
Iodine is used in many inorganic and organic reactions. State and explain the trend in volatility of the halogens, from chlorine to iodine. Explain why HI is the least thermally stable of HCl, HBr and HI. The table shows the electronegativity values for hydrogen, fluorine and iodine. element electronegativity value H 2.1 F 4.0 I 2.5 Explain, in terms of intermolecular forces, why HI has a lower boiling point than HF. Iodine reacts with hot concentrated aqueous sodium hydroxide in the same way as chlorine. Write an equation for the reaction of iodine and hot aqueous sodiumhydroxide. Iodoalkanes contain carbon-iodine bonds. The simplest iodoalkane is CH3I. CH3I can be made from methanol, CH3OH. Identify a reagent that can convert CH3OH to CH3I. 1,2‑diiodoethane, CH2ICH2I, can be made by bubbling ethene into liquid iodine. Fully name the type of mechanism shown in this reaction. J reacts with NaOH, forming different products dependent on the conditions used. I J Name J. J reacts with NaOHto form K. OH K Fully name the mechanism of the reaction of J with NaOHto form K. J reacts with NaOH dissolved in ethanol to form a mixture of two alkenes, L and M. AlkeneL is shown. I NaOH in ethanol and L J M In the box provided, draw the structure of M. Explain why L does not show geometrical (cis-trans) isomerism. L reacts with hot concentrated acidified KMnO4to form propanone and one other organic product. Identify the other organic product. Propanone reacts with excess alkaline aqueous iodine. Complete and balance the equation for this reaction. CH3COCH3 + I2 + OH– CH3COO– + H2O + I– +  State one observation that can be made in the reaction in . 
9701_w20_qp_21
THEORY
2020
Paper 2, Variant 1
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Iodine is used in many inorganic and organic reactions. State and explain the trend in volatility of the halogens, from chlorine to iodine. Explain why HI is the least thermally stable of HCl, HBr and HI. The table shows the electronegativity values for hydrogen, fluorine and iodine. element electronegativity value H 2.1 F 4.0 I 2.5 Explain, in terms of intermolecular forces, why HI has a lower boiling point than HF. Iodine reacts with hot concentrated aqueous sodium hydroxide in the same way as chlorine. Write an equation for the reaction of iodine and hot aqueous sodiumhydroxide. Iodoalkanes contain carbon-iodine bonds. The simplest iodoalkane is CH3I. CH3I can be made from methanol, CH3OH. Identify a reagent that can convert CH3OH to CH3I. 1,2‑diiodoethane, CH2ICH2I, can be made by bubbling ethene into liquid iodine. Fully name the type of mechanism shown in this reaction. J reacts with NaOH, forming different products dependent on the conditions used. I J Name J. J reacts with NaOHto form K. OH K Fully name the mechanism of the reaction of J with NaOHto form K. J reacts with NaOH dissolved in ethanol to form a mixture of two alkenes, L and M. AlkeneL is shown. I NaOH in ethanol and L J M In the box provided, draw the structure of M. Explain why L does not show geometrical (cis-trans) isomerism. L reacts with hot concentrated acidified KMnO4to form propanone and one other organic product. Identify the other organic product. Propanone reacts with excess alkaline aqueous iodine. Complete and balance the equation for this reaction. CH3COCH3 + I2 + OH– CH3COO– + H2O + I– +  State one observation that can be made in the reaction in . 
9701_w20_qp_23
THEORY
2020
Paper 2, Variant 3
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Identify the substances liberated at the anode and at the cathode during the electrolysis of saturated KCl . at the anode at the cathode  When dilute sulfuricacid is electrolysed, oxygen is liberated at the anode. Dilute sulfuricacid is electrolysed for 15.0minutes using a current of 0.750 A. Calculate the volume of oxygen that is liberated under room conditions.  volume of oxygen = cm3 The halogens chlorine, bromine and iodine differ in their strengths as oxidising agents. These strengths are indicated by the E o values for these halogens. Give the E o values for chlorine, bromine and iodine acting as oxidising agents. Deduce which of chlorine, bromine and iodine will react with a solution of Sn2+under standard conditions. Explain your answer. Include a relevant equation in your explanation. An excess of chlorine is added to a solution of acidified Mn2+under standard conditions. Give the formula of the product of this reaction that contains manganese. An electrochemical cell can be made by connecting an Fe3+ / Fe2+ half-cell to an S2O8 2– / SO4 2– half-cell under standard conditions. Calculate the standard cell potential of this electrochemical cell.  = V State the material that should be used as the electrode in each half-cell. in the Fe3+ / Fe2+ half-cell in the S2O8 2– / SO4 2– half-cell  Describe one change to each half‑cell that would increase the value of the cell potential. The temperature should remain at 298 K. Fe3+ / Fe2+ half-cell S2O8 2– / SO4 2– half-cell  
9701_w20_qp_42
THEORY
2020
Paper 4, Variant 2
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Questions Discovered
617