Nitrogen ground state electronic configuration, 19

Use the aufbau principle to write the condensed ground state electron configurations for nitrogen, phosphorus, and arsenic. 

Bismuth, Bi, the 83rd element of the periodic table is the most metallic and the least abundant of the elements in the nitrogen family (group 15). It has an atomic mass of 208.980 and a ground state electronic configuration of [Xe] 4f 5d %s 6p. The bismuth atom usually utilizes the three 6p electrons in bond formation and retains the two 6s electrons as an inert pair, hence the oxidation state -1-3 exhibited by bismuth in the vast majority of its compounds. However, a variety of organobismuth compounds can contain the element in the -1-5 oxidation state. Coordination numbers are 2, 3,4, 5 and 6. Bismuth not only has metallic characteristics but also exhibits many properties similar to those of semiconductors and insulators. Consequently, it is often classified as a semi-metal or metalloid. Bismuth compounds are usually colorless unless the metal is bound to a chromophore. 

The element nitrogen has the symbol N and an atomic number (or Z number) of 7, i.e., the neutral atom has seven protons and seven neutrons in the nucleus and correspondingly seven electrons. The ground-state electronic configuration of these seven electrons is Is ls lp, that is, two electrons are in the K shell (1 ) and five in the L Shell two in the 2s orbital and three in the 2p orbital distributed among the p, Py, and p orbital (the five valence electrons). The three Ip electrons are unpaired with spins parallel as shown in Fig. 10.1. 

No information concerning the distribution of the unpaired electron on the chelate ligands of four-coordinated low-spin Co(II) Schiff base complexes is available from single crystal EPR spectra. In particular, no nitrogen hf interaction, which is sensitive to the ground state configurations, is observed. 

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