Trends in Group 7 (halogens)

What is the trend in melting/boiling points down the group

Increases due to increase in london dispersion forces

How does fluorine appear at room temp

Pale yellow gas

How does chlorine appear at room temp

Pale green/yellow gas

How does bromine appear at room temp

orange-brown liquid

How does iodine appear at room temp

Grey-black solid

What colour is bromine as a gas

Orange

What colour is iodine as a gas

Purple

How does chlorine appear in aqueous solution

Colourless/pale green

How does chlorine appear in organic solvents

Colourless/pale green

How does bromine appear in aqueous solution

Orange

How does bromine appear in organic solvents

Orange

How does iodine appear in aqueous solution

Yellowy-Brown

How does iodine appear in organic solvents

Purple

Why is the electronegativity of halogens significant

Halogens have high electronegativity meaning they are good oxidising agents. Going down the group, atoms get larger so it is harder to gain electrons (reactivity decreases down the group)

what is the trend in volatility down group 7

Volatility decreases down the group as molecular size increases, leading to stronger van der Waals forces.

what is the structure of halogens

exist as diatomic molecules so are simple molecular structures with weak London dispersion dories between them caused by instantaneous dipole-induced dipole forces

explain the trend in boiling point, melting point and volatility down group 7

the more electrons, the Greater London forces, therefore the larger the molecule, the stronger these forces between molecules. therefore, down the group, it gets more difficult to separate the molecules so boiling and melting points increase. it gets more difficult to separate the molecules so volatility of halogens decreases down the group.

what is the trend of electronegativity down the group

decreases down the group, therefore their oxidising power decreases going down the group.

which element in group 7 is the strongest oxidant agent

fluorine due to its high electronegativity and small atomic radius, allowing it to attract electrons more effectively than other halogens.

what is the trend in reactivity down group 7

reactivity decreases down the group due to increasing atomic size and shielding effect, making it harder for the larger atoms to attract electrons.