The Halogens (OCR A Level Chemistry)

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Sonny

Last updated

3 June 2022

Physical Properties of the Halogens

Trend in boiling points

Boiling point increases down the group
We can explain this trend by looking at the forces between the molecules
Halogens are non-metals and are diatomic molecules at room temperature
This means that they exist as molecules that are made up of two similar atoms, such as F₂
The halogens are simple molecular structures with weak London forces between the diatomic molecules caused by instantaneous dipole-induced dipole forces

The diagram shows that a sudden imbalance of electrons in a nonpolar molecule can cause an instantaneous dipole. When this molecule gets close to another non-polar molecule it can induce a dipole as the cloud of electrons repel the electrons in the neighbouring molecule to the other side

The more electrons there are in a molecule, the greater the instantaneous dipole-induced dipole forces
Therefore, the larger the molecule the stronger the London forces between molecules
This is why as you go down the group, it gets more difficult to separate the molecules and the boiling point increases

Reactivity of the Halogens

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 7 non-metals increases as you move up the group
Out of the 3 halogens, chlorine, bromine and iodine, chlorine is the most reactive and iodine is the least reactive

Observations in aqueous solution

The colour of the solution in the test tube shows which free halogen is present in solution.
- Chlorine = very pale green solution (often colourless),
- Bromine = yellow solution
- Iodine = brown solution(sometimes black solid present)
The colour of the organic solvent layer in the test tube shows which free halogen is present in solution
- Chlorine = colourless
- Bromine = yellow
- Iodine = purple

Observations with an organic solvent

Reaction of bromide ions and chlorine

Chlorine is above bromine in Group 7 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)

We can again see this is a redox reaction by taking a look at changes in the oxidation number of each element in the reaction
- Br = -1 → 0 so the bromine has been oxidised
- Cl = 0 → -1 so the chlorine has been reduced
- No change in oxidation number for the potassium
Rather than writing the full equation we can also write the ionic equation by removing the potassium spectator ion

2Br^- (aq) + Cl₂ (aq) → 2Cl^- (aq) + Br₂(aq)

Trend in Reactivity

The oxidising power of the halogens decreases going down the group (the halogens get less reactive)
This can be explained as follows:
- Atomic radius increases
- There are more inner shells so shielding increases
- There is less nuclear attraction to attract an electron from another species

Redox Reactions of the Halogens

Each halogen has 7 electrons in their outer shell with two electrons in the outer s sub-shell and 5 in the outer p sub-shell
- __s²__p⁵

Halogens react with metals by accepting an electron from the metal atom to become an ion with 1- charge
- For example:

Ca (s) + Cl₂(g) → CaCl₂(s)

consisting of Ca²⁺and 2Cl^-ions

Halogens are therefore oxidising agents:
- Halogens oxidise the metal by removing an electron from the metal (the oxidation number of the metal increases)
- Halogens become reduced as they gain an extra electron from the metal atom (the oxidation number of the halogen decreases)