How many electrons in d orbital

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Understanding the Electron Configuration in d Orbitals

Introduction to d Orbitals

The d orbitals are a set of five orbitals found in the electron configuration of atoms. These orbitals are crucial in understanding the chemical bonding and properties of transition metals and other elements with partially filled d shells. Each d orbital can hold a maximum of two electrons, leading to a total of ten electrons across all five d orbitals in a given energy level .

Electron Distribution in d Orbitals

In a free atom, the five d orbitals are degenerate, meaning they have the same energy level. However, when these atoms form compounds, the energy levels of the d orbitals can split due to the influence of surrounding ligands. Despite this splitting, the angular parts of the orbital wave functions remain unchanged, which is significant for the overlap with other orbitals, such as 2s or 2p orbitals on ligands .

Role of d Orbitals in Chemical Bonding

The d orbitals play a critical role in the chemical bonding of transition metals and other elements. For instance, in heavy alkaline earth metals like calcium, strontium, and barium, the (n-1)d orbitals contribute to the bonding within endohedrally doped cage clusters. Although the contribution from these d orbitals is relatively small (ranging from 1% to 14%), it significantly affects the stability and properties of the clusters, such as shortening the distances between the metal and the cage and altering the HOMO-LUMO gaps .

Persistence of d Orbitals in Compounds

The presence of a definite number of electrons in d orbitals is evident in both gaseous molecules and condensed matter, including metallic lanthanides. This persistence is supported by atomic spectra analysis and photo-electron spectra, which highlight the importance of local kinetic energy and the total symmetry of closed shells . The d orbitals' contribution to the overall electron configuration and chemical behavior of these elements is thus well-documented and critical for understanding their properties.

Conclusion

In summary, the d orbitals can hold a total of ten electrons, distributed across five orbitals. These orbitals are essential in the chemical bonding and properties of transition metals and other elements with partially filled d shells. Their role is evident in various compounds and is supported by experimental evidence from atomic and photo-electron spectra. Understanding the behavior and contribution of d orbitals is crucial for insights into the chemical and physical properties of these elements.

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Most relevant research papers on this topic

Dyson-orbital concepts for description of electrons in molecules.

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The Persistence of p, d, f and g Orbitals in Compounds

The persistence of p, d, f, and g orbitals in compounds is supported by atomic spectra and photo-electron spectra, with local kinetic energy and total symmetry of closed shells playing crucial roles.

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Theoretical Basis for d-Orbitals

D-orbitals in the free atom have equal energy and electron distributions, and their overlap with 2s or 2p orbitals on ligands is crucial for understanding valence shell expansion.

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Small Amount Makes a Big Difference: Critical (n - 1)d Valence Orbitals of Heavy Alkaline Earth Metals inside Cage Clusters.

Heavy alkaline earth metals' valence orbitals in cage clusters include both ns and (n -1)d orbitals, affecting encapsulation stabilities, shortened Ae-cage distances, and lowered Ae valences.

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The configuration energies of d-block elements (groups 3-11) generally increase across a row, with the highest values occurring at nickel, silver, and gold, all lower than silicon's CE, except for gold, which has a CE equal to silicon's.

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