Hey there! Sign in to join this conversationNew here? Join for free
x Turn on thread page Beta
    • Thread Starter
    Offline

    0
    ReputationRep:
    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
    Offline

    18
    These are quite similar. But the second one is better plus you should write ''...outweighs the increasing nuclear charge down the group.''
    • Thread Starter
    Offline

    0
    ReputationRep:
    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
    Offline

    18
    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).
    • Community Assistant
    Online

    21
    ReputationRep:
    Community Assistant
    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).
 
 
 
Reply
Submit reply
Turn on thread page Beta
Updated: January 22, 2014
Poll
Do you like carrot cake?

The Student Room, Get Revising and Marked by Teachers are trading names of The Student Room Group Ltd.

Register Number: 04666380 (England and Wales), VAT No. 806 8067 22 Registered Office: International House, Queens Road, Brighton, BN1 3XE

Write a reply...
Reply
Hide
Reputation gems: You get these gems as you gain rep from other members for making good contributions and giving helpful advice.