ES Section 1 (b), (c), (d), (e), (b) the explanation (given the necessary information) of the chemical processes occurring during the extraction – – (f), (g), (h), (i), (j), (k) of the halogens from minerals in the sea The presence of halide in the (c) techniques and procedures in the electrolysis of aqueous solutions; half-equations for the processes sea provides the entry to the occurring at electrodes in electrolysis of molten salts and aqueous solutions: (i) formation of oxygen or a properties of the halogens and halogen or metal ions at the anode; (ii) formation of hydrogen or a metal at the cathode reactions between halide ions. The (d) reactions of s-, p- and d-block elements and their compounds in terms of electron transfer: (i) use of manufacture of bromine and half-equations to represent simple oxidation and reduction reactions; (ii) the definition of oxidation and chlorine then provide the context reduction as loss and gain of electrons; (iii) identification of oxidising and reducing agents for discussion of redox chemistry, (e) the oxidation states assigned to and calculated for specified atoms in formulae (including ions) and electrolysis and the nomenclature explanation of which species have been oxidised and which reduced in a redox reaction of inorganic compounds. (f) use of oxidation states to balance redox equations that do not also involve acid–base reactions; ….. (g) use of systematic nomenclature to name and interpret the of inorganic compounds (h) a description of the following physical properties of the halogens: appearance and physical state at room temperature, volatility, solubility in water and organic solvents (i) the relative reactivities of the halogens in terms of their ability to gain electrons (j) the details of the redox changes which take place when chlorine, bromine and iodine react with other halide ions, including observations, equations and half-equations (k) the reactions between halide ions (Cl–, Br– and I–) and silver ions (Ag+) and ionic equations to represent these precipitation reactions, the colours of the precipitates and the solubility of silver halides in ammonia
ES – Section 1 – (b), (c), (d), (e), (f), (g), (h), (i), (j), (k) The presence of halide in the sea provides the entry to the properties of the halogens and reactions between halide ions. The manufacture of bromine and chlorine then provide the context for discussion of redox chemistry, electrolysis and the nomenclature of inorganic compounds. (b) the explanation (given the necessary information) of the chemical processes occurring during the extraction of the halogens from minerals in the sea (c) techniques and procedures in the electrolysis of aqueous solutions; half-equations for the processes occurring at electrodes in electrolysis of molten salts and aqueous solutions: (i) formation of oxygen or a halogen or metal ions at the anode; (ii) formation of hydrogen or a metal at the cathode (d) reactions of s-, p- and d-block elements and their compounds in terms of electron transfer: (i) use of half-equations to represent simple oxidation and reduction reactions; (ii) the definition of oxidation and reduction as loss and gain of electrons; (iii) identification of oxidising and reducing agents (e) the oxidation states assigned to and calculated for specified atoms in formulae (including ions) and explanation of which species have been oxidised and which reduced in a redox reaction (f) use of oxidation states to balance redox equations that do not also involve acid–base reactions; ….. (g) use of systematic nomenclature to name and interpret the of inorganic compounds (h) a description of the following physical properties of the halogens: appearance and physical state at room temperature, volatility, solubility in water and organic solvents (i) the relative reactivities of the halogens in terms of their ability to gain electrons (j) the details of the redox changes which take place when chlorine, bromine and iodine react with other halide ions, including observations, equations and half-equations (k) the reactions between halide ions (Cl–, Br– and I–) and silver ions (Ag+) and ionic equations to represent these precipitation reactions, the colours of the precipitates and the solubility of silver halides in ammonia
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