What about the 1st ionization energy of aluminium and magnesium? Why is it that aluminium has lesser 1st ionization energy than magnesium? Is it the same with sulfur and phosphorus?
Well this video has provided information about the first group elements only. With regards to your question , the answer lies in the electronic configuration. Al-1s2 2s2 2p6 3s2 3p1 and Mg - 1s2 2s2 2p6 3s2. Mg has a completely filled s orbital so it has acquired higher stability relative to Al. It is hard to remove an electron from a stable atom so Mg has a greater first IE. Phosphorous has a higher 1st IE in comparison to Sulphur. The reason again lies in the electronic configuration as well as the orientation of the p orbital. P- 1s2 2s2 2p6 3s2 3(px1 py1 pz1) S- 1s2 2s2 2p6 3s2 3p(px2 py1 pz1) The outermost electron in Sulphur already faces electron-electron repulsion (in 3px) so less energy is required to remove it. Hence IE1 Phosphorous > IE2 Sulphur
is there a periodic table *trend* for 2nd Ionization energy (such as the one we have for 1st IE) ??????????
This topic was explained very well. Thank you.
you are a savior
is the second ionization energy ALWAYS higher than the first??
Yes
Where are you getting these values from for IE1 and IE2?
+milly *Necroposting here* These are universally accepted values for the energy needed for Li. You can see this in any textbook.
HoKogan hi my history textbook doesn’t appear to have the ionization energies, any help?
I wish u were my teacher!❤
very well explained thank you
quite an useful explanation. thank u
at 1: 00 how did you calculated that ionization energy ?can anybody tell me?
Aspboss he looked it uo
So what if the outermost electron is more than one,can IE be possible
what is order of third ionization energy of Nitrogen and boron
THIS VIDEO IS LIFFFEEE
What about the 1st ionization energy of aluminium and magnesium? Why is it that aluminium has lesser 1st ionization energy than magnesium?
Is it the same with sulfur and phosphorus?
Well this video has provided information about the first group elements only. With regards to your question , the answer lies in the electronic configuration. Al-1s2 2s2 2p6 3s2 3p1 and Mg - 1s2 2s2 2p6 3s2. Mg has a completely filled s orbital so it has acquired higher stability relative to Al. It is hard to remove an electron from a stable atom so Mg has a greater first IE.
Phosphorous has a higher 1st IE in comparison to Sulphur. The reason again lies in the electronic configuration as well as the orientation of the p orbital.
P- 1s2 2s2 2p6 3s2 3(px1 py1 pz1)
S- 1s2 2s2 2p6 3s2 3p(px2 py1 pz1)
The outermost electron in Sulphur already faces electron-electron repulsion
(in 3px) so less energy is required to remove it. Hence IE1 Phosphorous > IE2 Sulphur
always best
That video is just 8 years old and his way of teaching is better than paid tutoring XD
12th comment!