Chemical Forums

Chemistry Forums for Students => High School Chemistry Forum => Topic started by: XxslbabesxX on November 08, 2005, 09:28:08 PM

Title: ionization energy.
Post by: XxslbabesxX on November 08, 2005, 09:28:08 PM
Can someone explain to me why Sulfur has a lower first ionization energy than Phosphorus?

Also do group differences make more of a difference than does period differences when it comes to things like electron affinity and ionization energy.

Thanks!
Title: Re: ionization energy.
Post by: Blueshawk on November 08, 2005, 10:41:18 PM
It could be due the their electron affinity.

Electron Affinity of P is 71.7 kJ/mol

Electron Affinity of S is 200.4 kJ/mol

Therefore P has less ability or want to hold onto electrons, therefore the electrons are more easily removed and the energy potential is therefore greater.

Title: Re: ionization energy.
Post by: Mitch on November 08, 2005, 11:06:57 PM
Your numbers seem to indicate the opposite. One should note that electron affinity = -(delta h)