Phosphorus electronic configuration

How many valence electrons has carbon Silicon Phosphorus Hydrogen Write the electron configurations for neutral atoms of each element. 

The electron configuration in the valence orbitals of the sulfur atom (3s 3p4) suggests that it will form two covalent bonds by making use of two half-filled 3p orbitals. This is, in fact, observed in the molecule S8, which is present in the common forms of solid sulfur. The S8 molecules assume the form of a puckered ring, as shown in Figure 20-3. As with the phosphorus, the stability of this crystalline form of sulfur is due to van der Waals forces between discrete molecules. 

This problem clearly did not worry Stoner, who just went ahead and assumed that three quantum numbers could be specified in many-electron atoms. In any case, Stoner s scheme solved certain problems present in Bohr s configurations. For example, Bohr had assigned phosphorus the configuration 2,4,4,41, but this failed to explain the fact that phosphorus shows valencies of three and five. Stoner s configuration for phosphorus was 2,2,2,4,2,2,1, which easily explains the valencies, since it becomes plausible that either the two or the three outermost subshells of electrons form bonds. 

Use the aufbau principle to write complete electron configurations and complete orbital diagrams for atoms of the following elements sodium, magnesium, aluminum, silicon, phosphorus, sulfur, chlorine, and argon (atomic numbers 11 through 18). 

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

As a result of this electron-filling scheme for jellium clusters, the magic numbers for closed shell configurations in a jellium cluster are very different from those in free atoms. The first magic number of chemical significance in a jellium sphere is the 20 valence electron configuration of white phosphorus P4 and other isoelectronic species of the type E4 (E = As, Sb, Bi) and E4" (E = Si, Ge, Sn, Pb), which are shown by the NICS method to be highly aromatic systems [39, 79]. 

Indicate the position of phosphorus in Mendeleev s periodic table of the elements, its electron configuration, the size of its atom, and its oxidation states. 

For vanadium and chromium the first ionization energies are much lower than the first ionization energies of phosphorus and sulphur, respectively. This explains the high heats of formation of VC13 and CrCl3. In uranium, the tetravalent state is more stable than that in tungsten because uranium as an actinide has a different electron configuration. 

Phosphorus is directly below nitrogen in the periodic table. (The relationship of the chemistry of phosphorus to that of nitrogen is somewhat like the sulfur-oxygen relationship discussed in the introduction to Chapter 17.) The phosphorus atom electron configuration is Ne 3.s,23/J3, and it has five outer-shell electrons, as shown by its Lewis symbol in Figure 18.1. Because of the availability of underlying 3d orbitals, the valence shell of phosphorus can be expanded to more than eight electrons. 

RhCl(PPh3) 3 The chlorine radical (Cl ) accepts an electron from rhodium metal (electronic configuration Ad1,5s2) to give Cl and Rh+. The chloride ion then donates two electrons to the rhodium ion to form a dative or a coordinate bond. Each PPh3 donates a lone pair of electrons on the phosphorus atom to the rhodium ion. The total number of electrons around rhodium is therefore 8 + 2 + 3X2=16, and the oxidation state of rhodium is obviously 1 +. The other way of counting is to take the nine electrons of rhodium and add one electron for the chlorine radical and six for the three neutral phosphine ligands. This also gives the same electron count of 16. 

Phosphorus and sulfur are neighboring elements in Period 3 of the periodic table and have the following valence electron configurations phosphorus is 3sz3p3, and sulfur is 3s23p4. 

The chemistrj of nitrogen and phosphorus is dominated by a tendency of the atoms to complete their octets, an end which may be achieved in a considerable number of ways. The electron configuration of the nitrogen molecule may be described in molecular orbital terms as... 

---