Why are the d and f orbitals in transition metals considered localized?

Click For Summary
SUMMARY

The d and f orbitals in transition metals are considered localized due to their positioning in inner shells (n-1 and n-2) and their proximity to the nucleus. This localization is further influenced by the filling of the sub-shells, which affects the effective nuclear charge experienced by the electrons. As these sub-shells fill, the electrons in d- and f-orbitals experience less shielding from each other, resulting in a higher effective nuclear charge and a reduction in orbital size. Consequently, noble metals exhibit lower oxidation states and reduced reactivity compared to earlier d-block elements.

PREREQUISITES
  • Understanding of atomic orbitals and their configurations
  • Knowledge of effective nuclear charge and electron shielding
  • Familiarity with transition metals and their properties
  • Basic principles of quantum mechanics related to electron behavior
NEXT STEPS
  • Research the concept of effective nuclear charge in detail
  • Study the electron configurations of transition metals
  • Explore the reactivity trends of transition metals across the periodic table
  • Learn about the role of d and f orbitals in chemical bonding and catalysis
USEFUL FOR

Chemistry students, materials scientists, and professionals studying transition metal properties and their applications in catalysis and materials design.

Rzbs
Messages
52
Reaction score
11
TL;DR
Why are d and f orbitals localized?
Why d and f orbitals in transition metals considered localize?
Is it an experimetal result that d and f orbitals are more near to nuclea than s orbital in transition metals or there is another reason for considering them localized in a solid?
 
Physics news on Phys.org
d and f orbitals are orbital in inner shells (n-1 and n-2, respectively), hence they are more localized in the inner of the atoms. The precise size depends also on the filling of the sub-shells. electrons in d- and f- orbitals hardly shield each other from the nuclear charge. Hence, as the filling of the sub-shell increases, the electrons see an increasingly higher effective nuclear charge, which leads to a shrinking of the obitals. Therefore, e.g. the noble metals have relatively low oxidation states and are little reactive in comparison to the earlier elements in the d-block.
 
Thanks
 

Similar threads

Counting d-electrons in M(I) transition metals
  • · Replies 4 ·
Replies
4
Views
2K
Why do the d, f orbitals of transition metals have less reactivity?
  • · Replies 1 ·
Replies
1
Views
2K
Do all transition metals have the n2 and (n-1)d orbitals?
  • · Replies 2 ·
Replies
2
Views
2K
Undergrad Why Is Crystal-Field Splitting Different for f-Orbitals Compared to d-Orbitals?
  • · Replies 1 ·
Replies
1
Views
3K
Why Is the d-Orbital Considered in Sc Term Symbols?
  • · Replies 5 ·
Replies
5
Views
3K
Undergrad Free Electron Theory: Majority From d/f Orbitals?
  • · Replies 1 ·
Replies
1
Views
3K
Undergrad Orbitals and selection rules in a synchrotron
  • · Replies 18 ·
Replies
18
Views
2K
Why are some d-electron configurations more stable? (1st row)
  • · Replies 4 ·
Replies
4
Views
2K
Undergrad Why are there not more ferromagnetic Materials?
  • · Replies 1 ·
Replies
1
Views
3K
Why do transition metals have multiple oxidation states?
  • · Replies 10 ·
Replies
10
Views
5K