I could be wrong, but at 12:51, wouldn't the ionization energy for F be higher than Cl because the nucleus has a stronger pull on the electrons, and therefore, we would need more energy to remove the electron.
this is correct. F is smaller, so nucleus exhibits stronger pull on e- (higher Zeff, though marginally), leading to more energy needed to pry an e- away.
The GOAT returns
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I could be wrong, but at 12:51, wouldn't the ionization energy for F be higher than Cl because the nucleus has a stronger pull on the electrons, and therefore, we would need more energy to remove the electron.
this is correct. F is smaller, so nucleus exhibits stronger pull on e- (higher Zeff, though marginally), leading to more energy needed to pry an e- away.
Ya he correctly said that F has a smaller radius, so that means it must have a higher IE.
I always just think of the BEAR trend in each corner.
great explanations!
27:54 Do you think the nucleus gives a fuck what happens to that...
made my day. Thank you for your thorough explanations.
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THANK YOU :)
I agreeeeeee
In periodic table:
------->
|
down arrow ^increased FE, EN, EA, IE
Atomic radius increases with the opposite arrows from above
Hope this helps
Thank you for your excellent explanations! Could you please tell me what the MCAT is?