Phosphorus valence electron configuration

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]. 

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. 

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. 

Phosphorus has a valence electron configuration of 3s 3p, similar to that of nitrogen. Phosphorus also forms many compounds with oxidation states ranging from —3 through -I-5. The most stable compounds have the -1-5 oxidation state. 

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. 

Phosphorus has 5 valence electrons, and chlorine has 7, so their isolated atoms have Lewis configurations, as shown in Figure 5-4. 

This configuration shows that a phosphorus atom has five valence electrons. Two valence electrons are in the 3s orbital, and three others are in the 3p orbitals. 

Phosphorus is in group 5A, so its atoms also have five valence electrons, in this case, in the configuration. Arsenic, also in group 5A, has atoms with a As Ap ... 

Solution The exceptionally large jump occurs after IE5, indicating that the element has five valence electrons and, thus, is in Group 5A(15). This Period 3 element is phosphorus (P Z = 15). Its electron configuration is s 2s 2p is ip ... 

Solution The outer-sheU electron configurations for P and F are 3s 3p and Is lp, respectively, and so the total number of valence electrons is 5 + (5 X 7), or 40. Phosphorus, like sulfur, is a third-period element, and therefore it can have an expanded octet. The Lewis structure of PF5 is... 

The n-type semiconductors are doped intrinsic semiconductors in which the dopant is a pentavalent element, for instance chemical elements of group VA(15) of the periodic chart such as arsenic (As), antimony (Sb), or phosphorus (P). The substitutional impurities will give a supplementary electron owing to their ns np electronic configuration containing five rather than four outer-shell electrons. Therefore, the density of holes in the valence band is exceeded by the density of electrons in the conduction band. A hole is a mobile electron vacancy in a semiconductor that acts like a positive electron charge with a positive mass. Then, the n-type behavior is induced by doping with the addition of pentavalent element... 

The octet rule stems from the fact that the main-group elements in most cases employ only an ns and three np valence-shell orbitals in bonding, and these orbitals hold eight electrons. Elements of the second period are restricted to these orbitals, but from the third period on, the elements also have unfilled nd orbitals, which may be used in bonding. For example, the valence-sheU configuration of phosphorus is... 

Atomic Structure The Nucleus Atomic Structure Orbitals 4 Atomic Structure Electron Configurations 6 Development of Chemical Bonding Theory 7 The Nature of Chemical Bonds Valence Bond Theory sp Hybrid Orbitals and the Structure of Methane 12 sp Hybrid Orbitals and the Structure of Ethane 13 sp2 Hybrid Orbitals and the Structure of Ethylene 14 sp Hybrid Orbitals and the Structure of Acetylene 17 Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur 18 The Nature of Chemical Bonds Molecular Orbital Theory 20 Drawing Chemical Structures 21 Summary 24... 

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