Electron configuration of transition metal ions

Such matters can be represented in a different way in terms of the d-electron configuration of transition metal ions in a molecular orbital scheme (Fig. 7.113). 

Fig. 7.113. d-Electron configuration of transition-metal ions at the surface of perovskites, for the case of magnanites and of nickelates (below). (Reprinted from J. O M. Bockris and T. Ottagawa, J. Phys. Chem., 87 2966,1983.)... 

The electronic configurations of transition metal ions, like those of main group ions, are determined by removal of the electrons from the shell of highest n value first. Next, electrons may be lost from the d subshell next to the valence shell. The capability of removing a variable number of electrons makes it possible for most transition metals to have ions of different charges. 

The number of states for the nd n = 3, 4, 5) electronic configurations of transition metal ions is equal to the number of combinations. Interelectronic repulsions partially remove the degeneracy, leading to the spectroscopic terms with (25 4- 1)(2L-E 1) degeneracy. In a lattice, the degeneracy of the terms is partially removed by... 

Electron Configurations of Transition Metal Ions In contrast to most main-group ions, transition metal ions rarely attain a noble gas configuration, and the reason, once again, is that energy costs are too high. The exceptions in Period 4 are scandium, which forms Sc ", and titanium, which occasionally forms Ti in some compounds. The typical behavior of a transition element is io form more than one cation by losing all of its ns and some of its (n — l)d electrons. (We focus here on the Period 4 series, but these points hold for Periods 5 and 6 also.)... 

A further requirement for the existence of orbital angular momentum due to orbital rotation is that there must not be an electron in the second orbital with the same spin as that in the original orbital. With these rules, it is possible to deduce which electron configuration of transition metal ions will have its orbital angular momentum fully or partially quenched. This information is summarized in Table XIII. 

Luminescence centers of transition-metal ions The general outer electronic configuration of transition-metal ions (cl-block elements) is (n - ns. ... 

Electron Configurations of Transition Metal Ions In contrast to many main-... 

Unpaired electrons and magnetism - One of the consequences of the open (incompletely filled) d" configuration of transition-metal ions may be the presence of one or more unpaired electrons. Such compounds could be described as radicals, and they are detected by techniques such as electron spin resonance spectroscopy. 

Being able to write correct electron configurations for transition metal ions becomes very important in discussions of coordination compounds (Chemistry 2). 

The electron configuration for the Co3+ ion is ls22s22p63s23p63d6. If you missed this, review electron configurations of transitional metals. The Co3+ ion would have a total of 24 electrons 10 pairs of electrons and four unpaired electrons in the 3d orbitals. Atoms in which one or more electrons are unpaired are paramagnetic. 

The Cr+ and Mn+ ions have ground-state electronic configurations 3<754.v° and 3d54s1, respectively, and both react slowly (relative to other transition metal ions) with S8 but do not react with P4 (whereas other transition metal ions react readily). The Ca+ (3d°4s1) ion reacts rapidly with S8 (98) (more rapidly than most bare transition metal ions) but reacts very slowly with P4 producing the [CaP]+ ion. The Ba+ ion also reacts readily with S8 but is unreactive to P4 (99). These observations indicate that the electronic configuration of the metal ion and the properties of the reacting molecule are important in determining reactivity. The formation of stable product ions is also important. Whereas most transition metals react with S8 to produce [MS4]+ ions, the product ion for Ca+ and Ba+ is the [MS3]+ ion. 

Write electron configurations of transition metal atoms and ions compare periodic trends in atomic properties of transition elements with those of main-group elements explain why transition elements have multiple oxidation states, how their metallic behavior (type of bonding and oxide acidity) changes with oxidation state, and why many of their compounds are colored and paramagnetic ( 22.1) (SP 22.1) (EPS 22.1 -22.17)... 

In general, octahedral complexes of transition-metal ions possessing 0, 1, or 2 electrons beyond the electronic configuration of the preceding noble gas, ie, i/, (P configurations, are labile. The (P systems are usually inert the relative lability of vanadium(II) may be charge and/or redox related. 

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