Ratvi
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#1
Report Thread starter 6 years ago
#1
When ionisation energy decreases down a group, this is because the electron shielding outweighs thenuclear charge so it gets easier to remove electrons because the atomic radius increases. Or would it be when ionisation energy decreases down a group, this is because the increase in electron shielding and atomic radius outweighs the nuclear charge? Thanks
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EierVonSatan
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These are quite similar. But the second one is better plus you should write ''...outweighs the increasing nuclear charge down the group.''
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Ratvi
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Im just asking whether the atomic radius is a factor towards the ionisation energy or is it the overall factor which decides the ionisation energy
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EierVonSatan
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They're all interconnected factors. The atomic radius is necessarily larger (less electrostatic attraction to the nucleus) for atoms with greater numbers of shells (greater shielding).
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Kallisto
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If I'm not mistaken the ionisation energy is depend on the numbers in protons and the distance of the electrons to the nucleus (= radius). The greater the distance, the lesser the ionisation energy to remove an electron in an atom, but the more protons in a nucleus are the greater the ionisation energy is. That's why there are groups in PSE in which the ionisation energy both increases and decreases (measured by the first ionisation energy).
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