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Published byStephan Bracknell Modified over 10 years ago
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M2 Halogens F 2 > Cl 2 > Br 2 > I 2 Oxidising agent forces another substance to lose electrons, so it must gain electrons itself. This means that F 2 will become F - more readily than Cl 2 etc. See Module book for why Oxidising power of the Halogens
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M2 Halogens Displacement reactions SpeciesColour Cl -, Br -, I - colourless Cl 2 pale yellow/green Br 2 yellow/brown I2I2 brown/black solid
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M2 Halogens Br 2 + 2Cl - no reaction Cl 2 + 2Br - 2Cl - + Br 2 pale green/yellow yellow/brown Cl 2 + 2I - 2Cl - + I 2 pale green/yellow brown/black solid Br 2 + 2I - 2Br - + I 2 yellow/brown brown/black solid Displacement reactions
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M2 Halogens I - > Br - > Cl - > F - This makes sense as it is the opposite to the oxidising ability of the halogens A reducing agent will force another substance to gain electrons, so it must lose electrons itself. Chlorine is unlikely to lose electrons, so it is a poor reducing agent. Reducing ability of the halide ions
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