Exchange stabilization and the variation of ionization energy in the pn and dn series

Blake, Antony B.

doi:10.1021/ed058p393

Cited by 10 publications

(8 citation statements)

References 3 publications

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“…A secondary effect, which is not brought out by Eq. (3), is the higher repulsion exercised between electrons in the same orbital as compared with different orbitals (Blake 1981). We discuss this elsewhere (see footnote 4).…”

Section: Principal Valencymentioning

confidence: 99%

Valencies of the lanthanides

Johnson

Nelson

2017

Found Chem

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The valencies of the lanthanides vary more than was once thought. In addition to valencies associated with a half-full shell, there are valencies associated with a quarter- and three-quarter-full shell. This can be explained on the basis of Slater’s theory of many-electron atoms. The same theory explains the variation in complexing constants in the trivalent state (the “tetrad effect”). Valency in metallic and organometallic compounds is also discussed.

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Section: Principal Valencymentioning

confidence: 99%

Valencies of the lanthanides

Johnson

Nelson

2017

Found Chem

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“…It has been shown [17,18] that exchange interactions need to be taken into account in evaluating ionisation energies of atoms and atomic ions. Repulsion between electrons at a constant distance from each other is the same whether they have parallel or anti-parallel spins.…”

Section: Methodsmentioning

confidence: 99%

Applying the soft sphere model to improve the understanding of bonding in transition metals

Lang

2020

Heliyon

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Development in the understanding of electronic structure and chemical bonding and the importance of metals is outlined. A summary of the main features of the soft sphere model of metallic bonding and structure is provided. The soft sphere model is used to show that there are four main components involved in the bonding of transition metal solids and the enthalpy of atomisation of gaseous transition metal atoms are calculated according to the model and results when compared to literature values give good agreement.

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“…4 These and some other authors clearly state that there is no extra stability for a filled or half-filled subshell compared with a subshell containing one electron less. [4][5][6][7] The s 1 and s 0 electron configurations of neutral isolated atoms of some transition elements can be explained by considering that each subshell energy level is split into two levels, a and b, related to the spin of the electrons, as can be seen in Figure 1. The Coulomb energy on account of the pairing of two electrons in the same orbital is assigned to the b level, because of which this level appears to be at a higher energy than the a level.…”

Section: -3mentioning

confidence: 99%

The use of Rich and Suter diagrams to explain the electron configurations of transition elements

2013

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Recebido em 25/9/12; aceito em 2/2/13; publicado na web em 24/5/13Rich and Suter diagrams are a very useful tool to explain the electron configurations of all transition elements, and in particular, the s 1 and s 0 configurations of the elements Cr, Cu, Nb, Mo, Ru, Rh, Pd, Ag, and Pt. The application of these diagrams to the inner transition elements also explains the electron configurations of lanthanoids and actinoids, except for Ce, Pa, U, Np, and Cm, whose electron configurations are indeed very special because they are a mixture of several configurations.Keywords: periodic table; electronic configuration; Rich and Suter diagrams.The electronic configuration of chemical elements is a very important and initial topic in all introductory chemistry courses. To obtain them, the Aufbau principle is used in connection with the orbitals energies. However, the explanation of the s 1 ground-state electron configurations of Cr and Cu is generally based on the special stability attributed to a half-filled and filled subshell, respectively. 1-3Otherwise, these configurations can be explained by the very elegant Rich and Suter diagrams. 4 These and some other authors clearly state that there is no extra stability for a filled or half-filled subshell compared with a subshell containing one electron less. [4][5][6][7] The s 1 and s 0 electron configurations of neutral isolated atoms of some transition elements can be explained by considering that each subshell energy level is split into two levels, a and b, related to the spin of the electrons, as can be seen in Figure 1. The Coulomb energy on account of the pairing of two electrons in the same orbital is assigned to the b level, because of which this level appears to be at a higher energy than the a level. In Figure 1a, the number 6 at the crossing point between the 3da and 4sa lines has the meaning 3da 5 and 4sa 1 , and the same meaning applies to Figure 1c.This type of diagram is very easily grasped by students and makes the explanation of the "anomalous" s 1 and s 0 electron configurations of transition elements much more reasonable. As can be seen in Figure 1a, the 4s 2 3d 3 vanadium electron configuration comes from the fact that both levels, 4sa and 4sb, have a lower energy than 3da. As we move to the right on the periodic table, the atomic number increases and all the levels go down. Because the 3d levels are closer to the core, they decrease faster than the 4s level, and the 3da level crosses the 4sb level when passing from V to Cr. It causes that for Cr, the 3da level must be completely filled with five electrons before we can put any electrons in the 4sb level. Because Cr only has six electrons in the valence shell, there is no electron to occupy the 4sb level, which results in the 4s 1 3d 5 electron configuration of Cr. The same situation occurs upon going from Ni to Cu. For Ni, the 4sb level is below 3db, whereas for Cu these levels cross and 3db becomes lower than 4sb. This means that the levels must be filled in the sequence: 3da 5 4sa 1 3db 5 , and because ...

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Exchange stabilization and the variation of ionization energy in the pn and dn series

Abstract: This article is concerned with two types of ionizations that are of special importance to chemists. The author's main purpose is to clarify current textbook interpretations of the peculiar decrease in ionization energy following completion of a half-filled p or d shell.

Cited by 10 publications

References 3 publications

Valencies of the lanthanides

Valencies of the lanthanides

Applying the soft sphere model to improve the understanding of bonding in transition metals

The use of Rich and Suter diagrams to explain the electron configurations of transition elements

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