Manganese: electron configuration

Ground-state electronic configuration is ls 2s 2p 3s 3p 3i 4s. Manganese compounds are known to exist in oxidation states ranging from —3 to +7 (Table 2). Both the lower and higher oxidation states are stabilized by complex formation. In its lower valence, manganese resembles its first row neighbors chromium and especially iron ia the Periodic Table. Commercially the most important valances are Mn, Mn ", or Mn ". ... 

The most obvious features of Fig. 24.1 are the relative positions of the -t-2 oxidation states. For manganese this state, represented by the high-spin Mn cation, is much the most stable. This may be taken as an indication of the stability of the symmetrical d electron configuration. 

Perhaps the most obvious metallic property is reflectivity or luster. With few exceptions (gold, copper, bismuth, manganese) all metals have a silvery white color which results from reflecting all frequencies of light. We have said previously that the electron configuration of a substance determines the way in which it interacts with light. Apparently the characteristic reflectivity of metals indicates that all metals have a special type of electron configuration in common. 

Some of the atomic properties of manganese differ markedly from its neighbors. For example, at constant pressure it takes 400 kj (2 sf) to atomize 1.0 mol Cr(s) and 420 kj to atomize 1.0 mol Fe(s), but only 280 kj to atomize 1.0 mol Mn(s). Propose an explanation, using the electron configurations of the gaseous atoms, for the lower enthalpy of atomization of manganese. 

Except for the elements at the ends of the rows, each transition metal can exist in several different oxidation states. The oxidation states displayed by the 3d transition metals are shown in Table 20-1. The most important oxidation states are highlighted in the table. The most common oxidation state for the 3d transition metals is +2, known for all the elements except Sc. Chromium, iron, and cobalt are also stable in the +3 oxidation state, and for vanadium and manganese the -H4 oxidation state is stable. Elements from scandium to manganese have a particularly stable oxidation state corresponding to the loss of ah the valence electrons configuration). 

As expected there is a close resemblance in the chemical behaviour of technetium and rhenium whereas the properties of both elements differ considerably from those of manganese. The electronic configuration of technetium in the ground state is 4d 5s. Technetium is a silver-grey metal which tarnishes slowly in moist air. 

Combination of broad emission band and narrow line is typical for elements with d electronic configuration, such as Cr +, Mn and Manganese participation is supported by chemical analyses of benitoite, where chromium was never mentioned as micro-impurity, while Mn is known with concentrations changing from 0.03 to 0.11% (Laurs et al. 1997). Such concentrations are quite enough for luminescence generation. Substitution in Mn +form substituting... 

Write the electron configuration of the manganese atom. Give examples of compounds corresponding to the different oxidation states of manganese. Indicate the position of manganese in the electrochemical series of the metals. How does it react with water, and with solutions of acids in the cold and with heating Write the equations of the relevant reactions. 

Otherwise, unusual valency states are often observed in cyanide complexes. A Mn complex K5Mn(CN)6 has been reported here the stable 18-electron configuration causes the valency of manganese to take the very unusual value of one, and the compound is formed in spite of the extremely unfavourable cation anion ratio. Still more remarkable are the complex nickel cyanides. KGN and Ni(CN)2 form a complex K2Ni(CN)4, in which sixteen electrons are involved in the bond formation. The diamagnetism and the square structure of the Ni(CN)4 ion show that the bonding is due to dsp2 hybridization. 

Manganese has a 3c/ 4v- electron configuration, and compounds in all oxidation slates from 0 to 7+ are known, although those of 1+ and 5+... 

Explain in terms of electron configurations why the atomic radius of manganese is larger than that of chromium. 

Fig. 5.46. Electronic configurations for high spin manganese(III) (A) and H NMRD profiles of a water solution of the tetraphenylsulfanyl porphyrin (TPPS4) manganese(III) complex at 278 (A), 293 ( ) and 308 (T) K [200] (B).

---