S3.1.3/7 Trends in 1st Ionisation Energy [SL IB Chemistry discontinuities NOT needed in SL only HL]

[@nnataliered]

THANK YOUUU!

[@rorykyle418]

life saver

[@todayiglowup4286]

i dont get the aluminium part :/

[@JohnyLoveForYou]

Oh, man. That dial-up sound...

[@zeegg8]

you said (about silicon) that "a full, a half-full, or an empty p orbital is stable, and by removing that electron you leave a half-full 3p orbital and that's more stable". What do you mean by that? Are half-full p orbitals more stable than full p orbitals? If so, then why does Chlorine follow the trend -- it has 2 full p orbitals while silicon only has 1?

[@ibchemvids]

+MrNoodlegirl I think the IB fudges this issue a bit. Electrons would rather not pair up - there is a slight repulsion that makes the first electron in a pair "easier" to remove than expected. I do not know why this does not apply to chlorine - I am but a humble IB teacher - this is beyond the scope of the curriculum and my brain!

[@Alice-bob]

@@ibchemvids In an exam which explanation is deemed correct by the IB?

[@chloekeith4034]

amazinggg mann