Titanium (atomic number 22) exhibits a higher ionization energy than Vanadium (atomic number 23) due to the effects of electron shielding and the configuration of d orbitals. The additional electron in Vanadium's d shell contributes to increased shielding, which lowers its ionization energy compared to Titanium. This phenomenon highlights the complexities of transition metal ionization energies, particularly in the first row of d block elements from Scandium to Zinc.
PREREQUISITESChemistry students, educators, and professionals interested in understanding the ionization energies of transition metals and the underlying principles of atomic structure.
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!