Manganese ionization energy

Identify the element with the higher first ionization energy in each of the following pairs (a) manganese and cobalt ... 

Lichtenberger et al. (209) have reported the He(I) photoelectron spectrum of the manganese compound (ju.-CH2)[(i75-C5H4CH3)Mn(CO)2]2 (3b) in the ionization energy range below 11 eV and have compared the results... 

The second ionization energies of the elements calcium through manganese increase from left to right in the periodic table with the exception that 72(Cr) > /2(Mn). The electron configurations of the elements are ... 

How are metallic character and first ionization energy related [7.58] It is possible to define metallic character as we do in this book and base it on the reactivity of the element and the ease with which it loses electrons. Alternatively, one could measure how well electricity is conducted by each of the elements to determine how metallic the elements are. On the basis of conductivity, there is not much of a trend in the periodic table Silver is the most conductive metal, and manganese the least. Look up the first ionization energies of silver and manganese which of these two elements would you call more metaUic based on the way we define it in this book ... 

Suppress ionization by adding high concentrations of salts of easily ionized metals, notably the alkali metals. Analytes having low ionization energies may be partially ionized in hotter flames. Manganese, with a fairly typical ionization potential of 7.4 eV, is 10% ionized in the NOA flame. Alkali metal salts are added at a few hundred times greater concentration than analytes so as to overwhelm sample-to-sample variation. The same amounts are added to standards. Errors due to ionization may easily be reduced to 1 or 2%. 

The values of third ionization energies gradually increase from scandium to zinc, but drop from manganese to iron. The formation of the iron(iii) ion, Fe, involves the removal of an electron from a doubly occupied 3d orbital this electron is more easily removed because it is repelled by the other electron in the orbital (Figure 13.8). 

---