Electron Configurations and Oxidation States

In which transition-metal ion of this group are the 3d orbitals completely filled  

Why does the maximum oxidation state increase linearly from Sc through Mn  

When transition metals are oxidized, they lose their outer s electrons before they lose electrons from the d subshell. --- (Section 7.4) The electron configuration of Fe is [Ar]3d 4s, for example, whereas that of Fe is [Ar]3d . Formation of Fe requires loss of one 3d electron, giving [Arj3d. Most transition-metal ions contain partially occupied d subshells, which are responsible in large part for three characteristics  

Transition metals often have more than one stable oxidation state. 

Many transition-metal compounds are colored, as shown in A FIGURE 23.3. 

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ELECTRONIC CONFIGURATIONS AND OXIDATION STATES OF TRANSITION METALS... 

Inorganic and physical chemistry Electronic configurations and oxidation states of transition metals... 

We first survey the general properties of transition metals, focusing on their electron configurations and oxidation states. (22.1)... 

SOMC is purely a surface phenomenon where an organometallic complex binds selectively with the surface by covalent (or sometimes ionic or both) bonds. One can then access to its electronic configuration and oxidation state, and this leads to a better understanding of the reaction mechanism. In SOMC, the surface acts as a ligand, which means one can tune the catalytic activity of the organometallic with the surface... 

Table 1. Electronic configuration and oxidation states of lanthanides...

Why are lanthanides called inner transition elements Discuss the electronic configuration and oxidation states of lanthanides. (C.C.S. Univ. 2007)... 

Symbol La atomic number 57 atomic weight 138.91 a rare-earth transition metal, precursor to a series of 14 inner-transition elements known as the lanthanide series electron configuration [XejSdiGs oxidation state -i-3 atomic radius 1.879A ionic radius (LaS+) 1.061A electronegativity 1.17 two natural isotopes are La-139 (99.911%) and La-138 (0.089%). 

Table 2. Electronic configurations, stable oxidation states and single ionization potentials (IP) for elements 104... 

Relativistic calculations allow more detailed predictions of the chemical properties of transactinides compared with those of their lighter homologues. Electi onic configurations and oxidation states predicted for the transactinide elements 104 to 120 on the basis of relativistic Hartree-Fock calculations are listed in Table 14.6. An important result of these calculations is the splitting of the p levels into a pi/2 sub-level for 2 electrons and a P3/2 sublevel for 4 electrons. 

A hundred years ago results from physics and physical chemistry had already influenced the conceptual status of inorganic chemistry. In the present context, it may be noted, in particular, how the experimental study of electrolysis processes had led to the concepts of cations, anions, and electrochemical equivalents. An important conclusion from these studies was, for example, that the monovalency of silver and the divalency of copper in their normal salts were more than just stoichiometric attributes. This conclusion, based upon integers, gives rise to the most important class of statements in chemistry, which we would like to call qualitative in a strong sense. We shall see further examples of this kind of statement below in connection with oxidation states, atomic electron configurations, and ground state specitications. 

The elemental nature of the central metal (its atomic number) is its key characteristic, but several of its properties depend also on its oxidation state and on the ensuing electron configuration and spin state. Hence, we see that the two most common oxidation states for copper, Cu(l) and Cu(ll), present complexes with very different properties in terms of their coordination numbers, stereochemical preferences, as well as spectroscopic and magnetic behavior. 

The most common oxidation states, corresponding electronic configurations, and coordination geometries of iridium are +1 (t5 ) usually square plane although some five-coordinate complexes are known, and +3 (t7 ) and +4 (t5 ), both octahedral. Compounds ia every oxidation state between —1 and +6 (<5 ) are known. Iridium compounds are used primarily to model more active rhodium catalysts. 

Chemical appHcations of Mn ssbauer spectroscopy are broad (291—293) determination of electron configurations and assignment of oxidation states in stmctural chemistry polymer properties studies of surface chemistry, corrosion, and catalysis and metal-atom bonding in biochemical systems. There are also important appHcations to materials science and metallurgy (294,295) (see Surface and interface analysis). 

Uranium is the fourth element of the actinide (SJ series. In the actinide series the electrons are more effectively shielded by the Is and 7p electrons relative to the 4f electrons (shielded by 6s, 6p) in the lanthanide (4p series. Thus, there is a greater spatial extension of 5f orbitals for actinides than 4f orbitals for lanthanides. This results in a small energy difference between and 5/ 6d7s electronic configurations, and a wider range of oxidation states is... 

Valence and oxidation state are directly related to the valence-shell electron configuration of a group. Binary hydrides are classified as saline, metallic, or molecular. Oxides of metals tend to be ionic and to form basic solutions in water. Oxides of nonmetals are molecular and many are the anhydrides of acids. 

In contrast to chloride compounds, niobium oxides have a VEC of 14 electrons, due to an overall anti-bonding character of the a2u state, caused by a stronger Nb-O anti-bonding contribution. In some cases, the VEC cannot be determined unambiguously due to the uncertainty in the electron distribution between the clusters and additional niobium atoms present in the majority of the structures. The 14-electron compounds exhibit semiconducting properties and weak temperature-independent paramagnetism. Unlike niobium chlorides, the oxides do not exhibit a correlation between the electronic configuration and intra-cluster bond distances. 

Table 1—Oxidation states, electronic configurations, and radii of the (III) ion of the lanthanide elements and yttrium...

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