The discussion centers on the ionization energy of titanium compared to vanadium, specifically exploring the reasons behind the observed trend in the first row of d orbitals from scandium to zinc. Participants are examining the implications of electron configurations and shielding effects on ionization energy.
Participants express differing views on the reasons for the ionization energy trend, with some proposing shielding effects while others question the validity of this explanation. The discussion remains unresolved with multiple competing perspectives.
There are limitations in the assumptions made regarding electron configurations and the application of the Aufbau principle, which may not fully account for the observed trends in ionization energy.
crays said:Hi, may i know why is the first row of the d orbitals (starting from scandium to zinc) should such a weird graph of ionization energy against number of protons? Here the proton number 22 element (titanium) has a higher ionization energy than the proton number 23 element (Vanadium). It is not half filled or fully filled. What's the reason?
GCT said:Probably has something to do with the additional shielding of the valence electrons with the extra electron in the d shell thus causing the IE to become slightly more negative ... Not certain about this.
chemisttree said:Correct!