Group 17 Elements with Halide Ions (DP IB Chemistry)

Group 17 Elements with Halide Ions

The Halogens

• These are the Group 17 non-metals that are poisonous and include fluorine, chlorine, bromine, iodine and astatine

• Halogens are diatomic, meaning they form molecules of two atoms

• All halogens have seven electrons in their outer shell

• They form halide ions by gaining one more electron to complete their outer shells

Colours and States at Room Temperature

Trends in physical properties of the halogens

Melting point

• The density and melting and boiling points of the halogens increase as you go down the group

Trend in the melting and boiling points of the halogens

The melting and boiling points increase down the group

Explaining the trend in reactivity in Group 17

• The reactivity of Group 17 non-metals decreases as you go down the group

• The halogens electron configurations all end in ns²np⁵

• Each outer shell contains seven electrons and when they react, they will need to gain one outer electron to get a full outer shell of electrons

• Going down the group, the electron affinity decreases and the atomic radius increases

• As you go down Group 17, the number of shells of electrons increases so shielding also increases

• This means that the outer electrons are further from the nucleus so there are weaker electrostatic forces of attraction that attract the extra electron needed

• The electron is attracted less readily, so the lower down the element is in Group 17 the less reactive it is

Reaction of the halogens with halide ions in displacement reactions

• A halogen displacement occurs when a more reactive halogen displaces a less reactive halogen from an aqueous solution of its halide

• The reactivity of Group 17 non-metals increases as you move up the group

• Out of chlorine, bromine and iodine, chlorine is the most reactive and iodine is the least reactive

Aqueous Solution Colour of Halogens

Halogen displacement reactions

Chlorine and bromine

• If you add chlorine solution to colourless potassium bromide solution, the solution becomes orange as bromine is formed

• Chlorine is above bromine in Group 17 so it is more reactive

• Chlorine will therefore displace bromine from an aqueous solution of a metal bromide

2KBr (aq)       +    Cl₂ (aq)  →     2KCl (aq)     +       Br₂(aq)

potassium bromide + chlorine → potassium chloride + bromine

Bromine and iodine

• Bromine is above iodine in Group 17 so it is more reactive

• Bromine will therefore displace iodine from an aqueous solution of a metal iodide

Br₂ (l) +      2NaI (aq)    →    2NaBr (aq)     +    I₂ (aq)

bromine +  sodium Iodide → sodium bromide + iodine