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6 Cards in this Set
- Front
- Back
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What 3 factors effect ionisation energy |
Atomic radius Nuclear charge Electron shielding |
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Explain the trend in ionisation energy across a period |
.nuclear charge increases .atomic radius decreases .shielding stays same .nuclear attraction increases .ionisation energy increases |
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Explain the trend in ionisation energy down a group |
Atomic radius increases More shielding Nuclear attraction decreases Ionisation decreases |
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Define ionisation energy |
Energy required to remove outer electron from 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions |
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Explain the difference in ionisation energy between beryllium and boron |
The valence electron removed in boron is from a P subshell which is of higher energy than an S subshell |
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Explain change in ionisation energy between oxygen and nitrogen |
.In nitrogen, all 3 orbitals in P subshell are occupied by only 1 electron each. .In oxygen, 1 of these orbitals (2Px) has 3 electrons with opposite spins .Therefore this is easier to remove as it is all ready being repelled .and oxygen has a lower ionisation energy |
