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Slide 2

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They are highly reactive!
Fluorine pale yellow gas
Chlorine green gas
Bromine red brown liquid
Iodine grey solid
Electronegativity increases up the group (larger
atoms attract electrons less than smaller
ones.)
Boiling points increase down the group (due to
increasing strength of Van der Waals forces)…read more

Slide 3

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Halogens displace less reactive halide ions from
solution!
Halogens gain electrons in reactions.
Become less oxidising down the group.
Reactions :
Cl2 (aq) with KBr (aq) Br2
Cl (aq) with KI (aq) I2
Br (aq) with KI (aq) I2
Iodine doesn't displace any of the above.…read more

Slide 4

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Halogens displace less reactive halide ions from
solution!
Therefore:
Cl will displace bromide and iodine! Ionic
equation =
Cl2 (aq) + 2Br- (aq) 2Cl- (aq) + Br 2 (aq)
Cl2 (aq) + 2I- (aq) 2Cl- (aq) + I2 (aq)
Br will displace iodine! Ionic equation =
Br(aq) + 2I-(aq) 2Br-(aq) + I2 (aq)
Iodine has no reaction with F-, Cl- or Br- !!…read more

Slide 5

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Chlorine and sodium hydroxide
makes Bleach
2NaOH(aq) + Cl2 (aq) NaClO(aq) + NaCl(aq) + H2O
(l)
Oxi 0 +1 -1
Cl goes up and down in oxidation states =
disproportionation.…read more

Slide 6

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Uses: cleaning, water treatment, killing bacteria etc.
Mixing chlorine with water
disproportionation.
Cl2 (aq) + H2O(l) HCl (aq) + HClO
Oxi= 0 -1 +1
HClO + H2O(l) ClO- + H3O + (l)
The Chlorate (I) ions Kills bacteria.…read more

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