Phosphorus atom A basic animation of the Phosphorus atom including element properties, it's date of discovery, and location on the Periodic Table. Image showing periodicity of valence s-orbital radius for the chemical elements as size-coded balls on a periodic table grid. The R max values for neutral gaseous element valence orbitals are abstracted from reference 1. Mann, Atomic Structure Calculations II.Hartree-Fock wave functions and radial expectation values: hydrogen to lawrencium, LA-3691, Los Alamos Scientific. The phosphorus atom has a total of 15 electrons so, we have to put 15 electrons in orbitals. The electrons will be placed in different orbitals according to the energy level: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f. Now, Phosphorus electron configuration P (15) = 1 s 2 2 s 2 2 p 6 3 s 2 3 p 3 (complete configuration).
Phosphorus is a component of bones, teeth, DNA, and RNA 1. In the form of phospholipids, phosphorus is also a component of cell membrane structure and of the body’s key energy source, ATP. Many proteins and sugars in the body are phosphorylated.
About Phosphorus
Like its close chemical relative, nitrogen, phosphorus is a nonmetallic element with a seemingly contradictory nature. Found in fundamental organic compounds such as DNA, ATP, and phospholipids, phosphorus is essential to life, yet it is also a component of dangerous explosives and some of the most potent poisons known, organophosphate nerve agents. However, upon closer consideration, these two sides of phosphorus are in fact inextricably connected: phosphorus would be incapable of playing its myriad biochemical roles without the very chemical properties that make it so reactive in isolation, while the lethal effects of nerve agents requires their structural similarity to the natural target of an enzyme which they irreversibly inhibit. The complex chemistry of phosphorus lends it to these roles and many others, making it an element that defies simple characterizations.
Despite its ubiquity, phosphorus was not known as an element for most of human history, as it is too reactive to be found naturally outside of compounds. Elemental phosphorus was first isolated by Hennig Brand in 1669. Brand was an alchemist who was experimenting with urine in an attempt to produce the philosopher’s stone, and instead produced a mysterious waxy white substance that glowed in the dark--a phenomenon now known to result from a slow light-producing reaction with oxygen. Brand showed his discovery to a number of others, and eventually sold his methods to D Krafft, who proceeded to exhibit the substance around Europe. The secret that the substance was produced from urine was soon leaked, leading to the production of the element by many other chemists.
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Matches were the first commercial use for phosphorus, but the early match industry was fraught with problems. White phosphorus, the form isolated by Brand, was both extremely unstable and toxic, and early matches caused accidental fires and poisonings of the workers who produced them. However, in 1850, Anton Schrotter von Kristelli showed that through controlled heating, white phosphorus could be transformed into a red substance that was more stable and that did not produce toxic phosphorus fumes. Today it is known that elemental phosphorus can additionally be induced to form even more stable violet and black crystalline forms through the application of temperature or pressure, though the red and white forms remain the most used. The use of red phosphorus, as well as various safety-enhancing design elements, such as the separation of reactive elements on match heads and a special striking surface in “safety matches”, allowed for the widespread use and production of considerably safer phosphorus matches.
In 1769, Johan Gottlieb Gahn and Carl Wilhelm Scheele showed that bones contained calcium phosphate, and that the pure element could be extracted from bone ash. Bone remained the major source of the element for the next seventy years. In the 1840s, it was recognized that bat and bird guano was another important source of phosphates, particularly for use in fertilizer. As early as 1850, phosphate rock was also used for a phosphorus source, but this method of production was very significant until after the development of electric arc furnace in 1890, which made the process significantly more feasible.
Industrial extraction of phosphorus from phosphate rock did not begin to approach the scale of today’s phosphorus industry until the World Wars, during which white phosphorus was used widely in weapons. Phosphorus is used in many incendiary devices, such as incendiary bombs and molotov cocktails, as well as in smoke screens. Phosphorus burns vigorously, producing fires that are difficult to extinguish and horrific wounds when it contacts human skin. Interestingly, its use is still allowed for bombs and smoke-producing munitions, but it is classified as a chemical agent when used in direct bombardment, and therefore this use is prohibited. The organophosphates developed for warfare are also considered illegal chemical weapons, though many countries still retain stockpiles of these compounds, which include VX and sarin gas. However, organophosphate pesticides, which operate through the exact same mechanism as these chemical weapons--the inhibition of acetylcholinesterase, which is necessary for normal nerve function-- and can be lethal in small doses when inhaled, ingested, or even absorbed through the skin, remain common tools in commercial agriculture. The potency of these compounds, as well as their extremely quick action in the body and their wide availability make them one of the most common causes of poisonings worldwide, and they are often implicated in suicides in rural areas.
The use of phosphates in fertilizer, while less immediately toxic, is another aspect of modern agriculture with sometimes troubling side-effects. Phosphorus is often a limiting nutrient in marine ecosystems, and phosphate-rich runoff from over-fertilized fields is therefore often the cause of overgrowth, which manifests as algal blooms. At minimum, a sudden growth of algae, followed by its die-off and decay, consumes dissolved oxygen in the water, producing hypoxic conditions that kill off animals and plants in large numbers. In particularly concerning cases, the species of algae in the bloom are themselves dangerous, producing neurotoxins that kill marine life directly and also accumulate in seafood, leading to poisonings. Despite these problems, fertilizer remains the largest use of industrially produced phosphorus. The use of phosphates as chelating water softening agents, often to increase the effectiveness of detergents, is also known to contribute to harmful effects of phosphate on the environment.
Beyond fertilizers, poisons, and water-softening agents, there are a number of other phosphate compounds with important applications. Various inorganic phosphates are used as food additives, often as leavening agents. Trisodium phosphate is widely used in cleaning agents and disinfectants, and sometimes as a flux in ceramic glazes or solder. Zinc dithiophoshate is a common anti-wear additive used in automotive lubricants such as motor oil. Tricresyl and tributyl phosphates are important plasticizers, used to produce nitrocellulose, acyrlates, and PVC, and also serve as solvents in inks, resins, and adhesives. Glyophosphate, known commercially as Roundup, is an widely-used systemic herbicides. Other important organophosphorus compounds include organic derivatives of phosphine, the phosphorus analogue of ammonia, which itself is used to produce many specialty phosphate chemicals and as pesticides and fumigants.
Phosphorus has a number of other commercial uses. In addition to being used to produce fertilizers and various industrial phosphates, phosphoric acid may be used for rust removal as an etching agent in dentistry, or for the production of phosphoric acid fuel cells. Phosphazenes are nitrogen-phosphorus compounds used to produce hybrid organic-inorganic polymers that can be engineered to have highly desirable properties. These polymers have been used to produce drug-delivering gels that degrade in the body, polymer electrolytes with potential for use in fuel cells and batteries, and elastomers that can withstand a variety of chemical and thermal environments, which frequently find use in aerospace components. Pure phosphorus is also used directly in metallurgy to make phosphor bronze, and sometimes finds use as a dopant to manipulate the electrical properties of semiconductors.
By Prof. L. Kaliambos (Natural philosopher in New Energy)
October 30, 2015
A phosphorus atom is an atomof the chemical element phosphorus with symbol P and atomic number 15. However unlike for hydrogen, aclosed-form solution to the Schrödinger equation for the many-electron atomslike the phosphorus atom has not been found. So, various approximations, suchas the Hartree–Fock method, could be used to estimate the ground state energies.Under these difficulties I published my paper “ Spin-spininteractions of electrons and also of nucleons create atomic molecular andnuclear structures” (2008) by analyzing carefully the electromagnetic interactionsof two spinning electrons of opposite spin. Under this condition we may use this correct image of phosphorus with the following electron configuration:
Phosphorus Atomic Weight
1s2.2s2.2px2.2py2.2pz2.3s2.3px1.3py1.3pz1
According to the “Ionization energies of the elements-WIKIPEDIA”the ionization energies (in eV) of the element phosphorus are the following: E1 =10.48669 , E2 = 19.7694 , E3 =30.2027 , E4 = 51.4439 , E5 = 65.0251, E6 = 220.421, E7 = 263.57 , E8 =309.60, E9 = 372.13 , E10 = 424.4, E11 = 479.46 . E12= 560.8. E13 =611.74, E14 = 2816.91, and E15 = 3069.842 .
Here the -( E1 +E2 + E3 ) is equal to the ground state energyE( 3px1 + 3py1 + 3pz1)of the three outer electrons. Then the - ( E4 + E5)is equal to the ground state energy E(3s2). Also, the -(E6 + E7 + E8 +E9 + E10 + E11 ) isequal to the ground state energy E( 2px2 + 2py2 +2pz2) . On the other hand the -( E12 + E13 )is equal to the ground state energy E(2s2) , while the -( E14 +E15) equals the ground state energy E(1s2). See also my papers about the explanation ofionization energies of elements in my FUNDAMENTAL PHYSICS CONCEPTS based on my paper of 2008.
For understanding theionization energies E1, E2, E3 , E4 ,E5 , E6 , E7 , E8 , E9 ,E10 , E11 , E12, and E13,which givethe ground state energies of (2s2.2px2.2py2.2pz2.3s2.3px1.3py1.3pz1)you can see my “EXPLANATION OF PHOSPHORUS IONIZATIONS”.
Phosphorus Atomic Number
In the same way for theexplanationof the E14 and E15 which give the ground stateof the 1s2 electrons one must apply the basic formula of mypaper of 2008.
EXPLANATION OF -( Ε14 + E15 ) = - 5886.752 = E( 1s2), WHICH GIVES THE GROUND STATE ENERGY OF THE TWO 1s2 ELECTRONS
Asin the case of helium the binding energy E(1s2) is due to thetwo remaining electrons of 1s2 with n = 1. Thus we maycalculate the binding energy by applying my formula of 2008 for Z =15 as
E(1s2) = [(-27.21))152 (+ 16.95)15 - 4.1 ] /12 =- 5872.1
Howeverthe experiments of ionizations give - (E14 + E15 )= - 5886.752 . In other words one sees here that after the ionizations myformula of 2008 gives the value of 5872.1 eV which is smaller than theexperimental value of 5886.752 eV. Under this condition of ionizations Isuggest that n = 1 becomes n < 1 due to the fact that theionizations reduce the electron charges and now the nuclear charge is muchgreater than the electron charge of the two remaining electrons. So for Z =15 wedetermine the n by writing
(E14 +E15) = 5886.752 eV = - E(1s2) = -[(-27.21) )152 + ( 16.95)15 - 4.1 ] /n2
Thensolving for n we get n = 0.9988.
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However in the absence of adetailed knowledge about the electromagnetic force between the two spinningelectrons of opposite spin physicist today using wrong theories cannot explainthe ground state energy of the electrons 1s2. For example underwrong theories based on qualitative approaches many physicists believeincorrectly that the second electron of the 1s2 shell is less tightlybound because it could be interpreted as a shielding effect; the other electronpartly shields the second electron from the full charge of the nucleus. Anotherwrong way to view the energy is to say that the repulsion of the electronscontributes a positive potential energy which partially offsets the negativepotential energy contributed by the attractive electric force of the nuclearcharge.
Under such false ideas Ipublished my paper of 2008 . You can see the paper in “User Kaliambos”.
Historically, despite theenormous success of the Bohr model and the quantum mechanics of the Schrodingerequation based on the well-established laws of electromagnetism in explainingthe principal features of the hydrogen spectrum and of other one-electronatomic systems, so far, under the abandonment of natural laws neither was ableto provide a satisfactory explanation of the two-electron atoms. In atomicphysics a two-electron atom is a quantum mechanical system consisting of onenucleus with a charge Ze and just two electrons. This is the first case ofmany-electron systems. The first few two-electron atoms are:
Z =1 : H- hydrogenanion. Z = 2 : He helium atom. Z = 3 : Li+ lithiumatom anion. Z = 4 : Be2+ beryllium ion.
Prior to the development ofquantum mechanics, an atom with many electrons was portrayed like the solarsystem, with the electrons representing the planets circulating about thenuclear “sun”. In the solar system, the gravitational interaction betweenplanets is quite small compared with that between any planet and the verymassive sun; interplanetary interactions can, therefore, be treated as smallperturbations.
However, In the helium atomwith two electrons, the interaction energy between the two spinning electronsand between an electron and the nucleus are almost of the same magnitude, and aperturbation approach is inapplicable.
In 1925 the two young Dutchphysicists Uhlenbeck and Goudsmit discovered the electron spin according towhich the peripheral velocity of a spinning electron is greater than the speedof light. Since this discovery invalidates Einstein’s relativity it met muchopposition by physicists including Pauli. Under the influence of Einstein’sinvalid relativity physicists believed that in nature cannot existvelocities faster than the speed of light.(See my FASTER THAN LIGHT).
So, great physicists likePauli, Heisenberg, and Dirac abandoned the natural laws of electromagnetism infavor of wrong theories including qualitative approaches under an idea ofsymmetry properties between the two electrons of opposite spin which lead tomany complications. Thus, in the “Helium atom-Wikipedia” one reads: “Unlike for hydrogen aclosed form solution to the Schrodinger equation for the helium atom has notbeen found. However various approximations such as the Hartree-Fock method ,canbe used to estimate the ground state energy and wave function of atoms”.
It is of interest to notethat in 1993 in Olympia of Greece I presented at the international conference“Frontiers of fundamental physics” my paper “Impact of Maxwell’s equation of displacement current on electromagnetic laws and comparison of the Maxwellian waves with our model of dipolic particles '. In that paper I showed that LAWS AND EXPERIMENTS INVALIDATE FIELDS AND RELATIVITY .At the same time I tried to find not only the nuclear force and structurebut also the coupling of two electrons under the application of the abandonedelectromagnetic laws. For example in the photoelectric effect the absorption oflight contributed not only to the increase of the electron energy but also tothe increase of the electron mass, because the particles of light have mass m =hν/c2. (See my paper 'DISCOVERY OF PHOTON MASS' ).
However the electron spinwhich gives a peripheral velocity greater than the speed of light cannot beaffected by the photon absorption. Thus after 10 years I published my paper 'Nuclear structure..electromagnetism' (2003), in which I showed not onlymy DISCOVERY OF NUCLEAR FORCE AND STRUCTURE but also that theperipheral velocity (u >> c) of two spinning electrons with opposite spingives an attractive magnetic force (Fm) stronger than the electricrepulsion (Fe) when the two electrons of mass m and charge (-e) areat a very short separation (r < 578.8 /1015 m). Because ofthe antiparallel spin along the radial direction the interaction of theelectron charges gives an electromagnetic force
Fem = Fe - Fm .
Therefore in my researchthe integration for calculating the mutual Fem led to thefollowing relation:
Fem = Fe - Fm = Ke2/r2 - (Ke2/r4)(9h2/16π2m2c2)
Of course for Fe =Fm one gets the equilibrium separation ro =3h/4πmc = 578.8/1015 m.
That is, for aninterelectron separation r < 578.8/1015 m the two electronsof opposite spin exert an attractive electromagnetic force, because theattractive Fm is stronger than the repulsive Fe . Here Fm is a spin-dependent force of short range. As aconsequence this situation provides the physical basis for understanding thepairing of two electrons described qualitatively by the Pauli principle, whichcannot be applied in the simplest case of the deuteron in nuclear physics,because the binding energy between the two spinning nucleons occurs when thespin is not opposite (S=0) but parallel (S=1). According to the experiments inthe case of two electrons with antiparallel spin the presence of a very strongexternal magnetic field gives parallel spin (S=1) with electric andmagnetic repulsions given by
Fem = Fe + Fm
So, according to thewell-established laws of electromagnetism after a detailed analysis of paired electrons in two-electron atoms I concluded that at r < 578.8/1015 m a motional EMF produces vibrationsof paired electrons.
Unfortunately today manyphysicists in the absence of a detailed knowledge believe that the twoelectrons of two-electron atoms under the Coulomb repulsion between theelectrons move not together as one particle but as separated particlespossessing the two opposite points of the diameter of the orbit around thenucleus. In fact, the two electrons of opposite spin behave like oneparticle circulating about the nucleus under the rules of quantum mechanicsforming two-electron orbitals in helium, beryllium etc. In my paper of 2008, I showed that the positive vibration energy (Ev) described in eV dependson the Ze charge of nucleus as
Ev = 16.95Z -4.1
Of course in the absence ofsuch a vibration energy Ev it is well-known that the ground state energyE described in eV for two orbiting electrons could be given by the Bohr modelas
E = (-27.21) Z2.
So the combination of theenergies of the Bohr model and the vibration energies due to the opposite spinof two electrons led to my discovery of the ground state energy of two-electronatoms given by
-E = (-27.21) Z2 +(16.95 )Z - 4.1
For example the laboratorymeasurement of the ionization energy of H- yields an energy ofthe ground state -E = - 14.35 eV. In this case since Z = 1 weget
-E = -27.21 +16.95 - 4.1 = -14.35 eV. In the same way writing for the helium Z =2 we get
-E = - 108.8 + 32.9 - 4.1 =-79.0 eV
The discovery of thissimple formula based on the well-established laws of electromagnetism was thefirst fundamental equation for understanding the energies of many-electronatoms, while various theories based on qualitative symmetry properties lead tocomplications.
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