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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.
