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OCR Chemistry A (H034) Approximately 4 lessons UNIT F321: Atoms, Bonds and Groups – Group 7 By the end of this topic you should be able to: Explain, in terms of Van der Waals’ forces, the trend in the boiling points of Cl2, Br2 and I2. Describe the redox reactions, including ionic equations, of the Group 7 elements Cl2, Br2 and I2 with other halide ions, in the presence of an organic solvent, to illustrate the relative reactivity of the Group 7 elements. Explain the trend in reactivity of Group 7 elements down the group from the decreasing ease of forming negative ions, in terms of atomic size, shielding and nuclear attraction. Describe the term disproportionation as a reaction in which an element is simultaneously oxidised and reduced, illustrated by: - The reaction of chlorine with water as used in water purification; The reaction of chlorine with cold, dilute sodium hydroxide, as used to form bleach; Reactions similar to those specified above Interpret and make predictions from the chemical and physical properties of the Group 7 elements and compounds. Contrast the benefits of chlorine use in water treatment (killing bacteria) with associated risks (hazards of toxic chlorine gas and possible risks from formation of chlorinated hydrocarbons). HOW SCIENCE WORKS (6a, 6b) Describe the precipitation reactions, including ionic equations, of the aqueous anions Cl-, Br- and I- with aqueous silver ions, followed by aqueous ammonia. Describe the use of these precipitation reactions as a test for different halide ions. Cedars Upper School – Mrs Sudbery