Metals and their ions

This competition for electrons is reminiscent of the competition for protons among acids and bases. The similarity suggests that we might develop a table in which metals and their ions are... 

Reactions with Heavy Metals and their Ions... 

Inorganic impurities buffers, inorganic reagents, catalysts, heavy metals and their ions (mostly originating from the apparatus), and reduction and oxidation factors... 

Similarly, zinc will be deposited and magnesium will be dissolved in a solution containing both metals and their ions, since... 

Metals and their ions or complexes often possess unpaired electrons but, by convention, they are not considered to be radicals, and radical dots are not used in their formulae. However, there may be occasions when a radical ligand is bound to a metal or metal ion where it is desirable to use a radical dot. 

Electron Configurations of the Transition Metals and Their Ions... 

Table SI. 2 The electronic configuration of the 3d transition metals and their ions...

Electron Configurations of the Transition Metals and Their Ions 738 Atomic and Physical Properties of the Transition Hements 739 Chemical Properties of the Transition Elements 741... 

A number of metals and their ions such as lead, mercury, bismuth and zinc [27, 147] were also reported to hinder not only the hydroformylation but also the homogeneous hydrogenation of the aldehydes formed to the alcohols. 

Predictions of cell potentials for spontaneous reactions of any combination of metals and their ions can be easily calculated. Tbe two balf-cells are botb written as reduction potentials. However, it is not possible for both reactions to accept electrons one half-cell must be reversed so it releases electrons. The half-cell that is always reversed is the one with more negative (or least positive) electrode potential. The cell potential is then the sum of the electrode potentials (including their signs). 

Electron configuration M 4s 3d 4s 3d 4s 3d 4s 3d 4s 3/ 4s 3d " The electron configurations of the first-row transition metals and their ions were discussed in Section 6.9 and Section 7.5, respectively. 

The energy separations between one set of orbitals and the next become smaller for As orbitals and beyond, and the relative energy ordering of these orbitals can actually vary among elements. These variations result in irregularities in the electron configurations of the transition metals and their ions (as we shall see later). 

In this chapter, we examine the properties of the transition metals and their ions more closely. We also examine the properties of coordination compounds in some detail. We first discussed this common type of transition metal compound in Chapter 16 (see Section 16.8). In a coordination compound, bonds to a central metal ion split the d orbitals much as they are split in the aystals of gemstones. The theory that explains these splittings and the corresponding colors is crystal field theory, which we also explore in this chapter. 

Recall from Section 8.7 that the transition metals form ions by losing electrons from the ns orbital before losing electrons from the (n - V)d orbitals. For example, Fe " has an electron configuration of [Ar] 3(f, because it has lost both of the 4i electrons to form the 2-1- charge. Examples 24.1 and 24.2 review the steps in writing electron configurations for transition metals and their ions. 

Writing Electronic Configurations forTransition Metals and Their Ions (24.2) Examples 24.1, 24.2 For Fhactice 24.1, 24.2 Exercises 19-20, 57,58... 

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