Group 7

Front 1

Oxidising power of a halogen

Back 1

The oxidising power of a halogen is a measure of the strength with which a halogen atom is able to attract and capture an electron to form a halide ion

Front 2

Half equations of a halogen

Back 2

Front 3

Trends in reactivity of Group 7

Back 3

Reactivity DECREASES DOWN the group:

More shells, atomic radius increases

Greater shielding effect

Weaker nuclear attraction

Less able to attract and capture another electron

Fluorine is most reactive

Front 4

Displacement reactions

Back 4

A displacement reaction is a reaction in which a more reactive element displaces a less-reactive element from an aqueous solution of its halide ions

Front 5

Colours of displacement reactions for halogens

Back 5

Front 6

For each displacement reaction you must write :

Back 6

Overall redox reaction

Ionic equation

Observations

Front 7

Displacement reactions

Back 7

A more reactive halogen will displace a less reactive halogen.

Front 8

Disproportionation reaction definition

Back 8

A disproportionation reaction is a reaction in which the same element is both oxidised and reduced

Front 9

Disproportionation of chlorine in water

Back 9

Front 10

Disproportionation of chlorine in aqueous sodium hydroxide

Back 10

Front 11

Test for a halogen - chlorine

Back 11

Front 12

Halogen test - bromine

Back 12

Front 13

Halogen test - iodine ions

Back 13