Simple Molecules And Intermolecular Forces
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Define London forces?
This is the movement of electrons causes temporary dipoles which induce dipoles in neighbouring molecules
Where are there no london forces ?
• giant covalent • metals
How do london forces increase and effect boiling point?
• more electrons will mean stronger london forces so more energy is required to break these intermolecular/london forces so higher melting and boiling point
Describe and explain what happens as you go down group 7 (hint - london forces )?
• as you go down group 7 both and melting points increases because there are more electrons • so london forces are stronger • so more energy is required to break theses intermolecular force
What does stronger london forces imply?
More electrons and higher boiling points
Why does carbon have a higher melting point compared to boron ?
• carbon has 4 covalent bonds whilst boron has 3
Explain why the halogens show this trend in boiling points ?
*the halpgen show an increase in boiling point as you go down the group *as their are strong london forces between the molecules as you go down the group *so more energy is required to break the intermolecular force as you go down
What happens to the reactivity as you go down group 2?
*as you go down reactivity increases *nuclear charge increases *electron shell increases *atomic radii increases *electron sheilding increases *decreases nuclear attraction between outer electron and nucleus so it’s easier to lose electrons _ exact same as group 7 but different outcome has it results in it being harder to gain electrons
Properties of water ?
*high melting and boiling point - strong hydrogen bonds *high surface tension *ice is less dense than water - open lattice structure *in water oxygen has double the number of lone pairs so water has double the number of hydrogen bonds so it will take twice the energy to break them