10.2 Chemical reactions of halogens
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What is oxidation ability for the halogens What type of reaction are these
. How easily they can gain an electron to become 1- ions, so they reduce themselves but oxidise other elements Redox reactions
Pattern of oxidation ability down group 7 and explain
. Oxidation ability decreases going down the group Because the number of filled energy levels increases down the group so attraction between the positive nucleus and negative outer electron shell decreases so it becomes more difficult for the atom to gain electrons to become a 1- ion Eg fluorine has the best oxidising power
What is the oxidation power of chlorine half equation
Cl2 + 2e- —> 2Cl-
What is a displacement reaction with the halides
. Halogens react with metal halides in a solution so the halide in the compound is replaced by a more reactive halogen, but not by a less reactive one.
What is the reaction for chlorine displacing bromide ions with the oxidation/reduction numbers on top What is the ionic equation What are the spectator ions?
0 1- 0 1- Cl2(aq) + 2NaBr(aq) —> Br2(aq) + 2NaCl(aq) Cl2 + 2Br- —> Br2 + 2Cl- Sodium ions
What is the pattern of halogens when displacing and oxidising
They always displace the ion of the halogens below it Eg F2 displaces Cl- Br2 displaces I-
Which halogen has the strongest oxidising power
. Flourine
How is bromine extracted from sea water
. Sea water has bromine ions which can be oxidised by chlorine to produce bromine Cl2 + 2Br- —>Br2 +2Cl-
What can you see in the reaction between chlorine and sodium bromide
The two colourless starting materials react to make the red/brown colour of bromine