Periodicity

Created by: Sopha8
Created on: 22-05-14 09:04

Why do first ionisation energies increase as you go along a period?

proton no. increases, stronger attraction, but smiliar energy level/shielding=harder to take electron

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Where are the 2 decreases in first inonisation energies trend across a period?

1) between group 2-3, 1 electron of element in group 3 in p orbital-further from nuclues, additional sheilding=easier to take, 2) between 5-6, paired electron in p obrital of group 5-repulsion, similar shielding, easier to take

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What happens to the atomic radius across a period? why?

decrease-proton increase, higher charge, electrons pulled closer, extra electron in same shell so no similar shielding

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What does melting and boiling points depend on?

bond strength and structure

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Define first ionisation enegy

energy needed to remove 1 mole of electrons from each atom in 1 mole of gaseous atoms to form 1 mole gaseous 1+ ions

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What factors affect ionisation energy?

1) nulear charge-more protons, stronger attraction, high IE 2) distance-elecrton close to nulceus=stronger atttraction, higher IE 3) shielding-more shells so outer have shielding from nulcues=lower IE

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Why are second ionisation energies higher than the first?

electron being removed from positive ion

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Other cards in this set

Card 2

Front

Where are the 2 decreases in first inonisation energies trend across a period?

Back

Card 3

Front

What happens to the atomic radius across a period? why?

Back

Card 4

Front

What does melting and boiling points depend on?

Back

Card 5

Front

Define first ionisation enegy

Back

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Periodicity