What is the definition of first ionisation enthalpy
The energy needed to remove one electron from each atom in one mole of gaseous atoms forming one mole of gaseous 1+ ions
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What state does the atom need to be in?
Gaseous
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How does atomic radius affect ionisation enthalpy?
a larger molecule decreases atomic radius as there is less attraction between negative electrons and positive nucleus
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How does nuclear charge affect ionisation enthalpy?
The more protons there are in a nucleus, the more outer electrons will be attracted to it making it harder to remove one. Ionisation enthalpy increases.
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Why is it easier to remove an electron that is in a pair?
Repulsion, which offsets attraction
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Why do successive ionisation enthalpies increase?
Electrons are being removed from an increasingly positive ion and so the attraction between the nucleus and the remaining electrons increase. There is also less electron repulsion due to fewer electrons and this makes it harder to remove an electron.
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Does ionisation enthalpy increase or decrease down a group?
Decrease
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Does ionisation enthalpy increase or decrease across a period?
Increase
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Other cards in this set
Card 2
Front
What state does the atom need to be in?
Back
Gaseous
Card 3
Front
How does atomic radius affect ionisation enthalpy?
Back
Card 4
Front
How does nuclear charge affect ionisation enthalpy?
Back
Card 5
Front
Why is it easier to remove an electron that is in a pair?
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