What is phosphorus charge

Connelly, Neil G. Hartshorn, and Alan T. Cambridge: RSC Publishing, Cox, P. Oxford: Oxford University Press, Understanding the Properties of Matter, 2nd edition. Donohue, Jerry. The Structures Of The Elements, 2nd edition. Malabar, Florida: Robert E. Krieger Publishing Company, Dronskowski, Richard. Computational Chemistry of Solid State Materials. KGaA, Ebbing, Darrell D. General Chemistry, 8th edition. Emsley, John. The Elements, 3rd edition.

Firestone, Richard B. Table of Isotopes, 8th edition, volume 2. Edited by Virginia S. Shirley, with assistant editors Coral M. Baglin, S. Frank Chu, and Jean Zipkin. Galasso, Francis S. Structure and Properties of Inorganic Solids. Oxford: Pergamon Press, Ghosh, Dulal C. Green, Don W. Perry's Chemical Engineers' Handbook, 8th edition. Greenwood, N. Chemistry of the Elements, 2nd edition. Burlington, MA: Butterworth-Heinemann, Oxford: Butterworth-Heinemann, Gwyn Williams. Electron Binding Energies.

Accessed on April 30, Ho, C. Powell, and P. I—1 to I— Horvath, A. Huheey, James E. Keiter, and Richard L Keiter. Inorganic Chemistry: Principles of Structure and Reactivity, 4th edition. Ihde, Aaron J. The Development of Modern Chemistry. New York: Dover Publications, Inc. Accessed on May 5, Accessed on May 4, Karuzawa, M. Kittel, Charles. Introduction to Solid State Physics, 8th edition. Krause, M. Advanced Structural Inorganic Chemistry. Li, Y. Edited by Fred T.

Oxford: Elsevier Ltd. Share Flipboard Email. Anne Marie Helmenstine, Ph. Chemistry Expert. Helmenstine holds a Ph. She has taught science courses at the high school, college, and graduate levels.

Facebook Facebook Twitter Twitter. Updated December 24, Featured Video. Cite this Article Format. Helmenstine, Anne Marie, Ph. Element Charges Chart. Properties of Ionic and Covalent Compounds. What Does Reactivity Mean in Chemistry?

He discovered how it was produced and investigated it systematically. His assistant Ambrose Godfrey set up his own business making and selling phosphorus and became rich.

When it was realised that bone was calcium phosphate, and could be used to make phosphorus, and it became more widely available. Demand from match manufacturers in the s ensured a ready market. Atomic data. Bond enthalpies. Glossary Common oxidation states The oxidation state of an atom is a measure of the degree of oxidation of an atom. Oxidation states and isotopes. Glossary Data for this section been provided by the British Geological Survey. Relative supply risk An integrated supply risk index from 1 very low risk to 10 very high risk.

Recycling rate The percentage of a commodity which is recycled. Substitutability The availability of suitable substitutes for a given commodity.

Reserve distribution The percentage of the world reserves located in the country with the largest reserves. Political stability of top producer A percentile rank for the political stability of the top producing country, derived from World Bank governance indicators. Political stability of top reserve holder A percentile rank for the political stability of the country with the largest reserves, derived from World Bank governance indicators. Supply risk. Young's modulus A measure of the stiffness of a substance.

Shear modulus A measure of how difficult it is to deform a material. Bulk modulus A measure of how difficult it is to compress a substance. Vapour pressure A measure of the propensity of a substance to evaporate. Pressure and temperature data — advanced. Listen to Phosphorus Podcast Transcript :. You're listening to Chemistry in its element brought to you by Chemistry World , the magazine of the Royal Society of Chemistry.

Hello - this week fertilisers, fire bombs, phossy jaw and food additives. What's the connection? Here's Nina Notman. Phosphorus is a non-metal that sits just below nitrogen in group 15 of the periodic table. This element exists in several forms, of which white and red are the best known. White phosphorus is definitely the more exciting of the two. As it glows in the dark, is dangerously flammable in the air above 30 degrees, and is a deadly poison.

Red phosphorus however has none of these fascinating properties. So where did it all begin? Phosphorus was first made by Hennig Brandt in Hamburg in Germany in When he evaporated urine and heated the residue until it was red hot.

Glowing phosphorus vapour came off and he condensed it under water. And for more than years most phosphorus was made this way. This was until people realised that bone was a great source of phosphorus. Bone can be dissolved in sulfuric acid to form phosphoric acid, which is then heated with charcoal to form white phosphorus.

White phosphorus has found a range of rather nasty applications in warfare. It was used in the 20 th century in tracer bullets, fire bombs, and smoke grenades. The scattering of phosphorus fire bombs over cities in World War II caused widespread death and destruction. In July , Hamburg was subject to several air raids in which 25, phosphorus bombs were dropped over vast areas of the city.

This is rather ironically considering where phosphorus was first made. Another group of warfare agents based on phosphorus are nerve gases such as sarin. Sarin is a fluorinated phosphonate that was used by Iraq against Iran in the early to mids.

And was also released in a Tokyo subway in , killing 12 people and harming nearly a thousand others. White phosphorus has also found a wide range of other uses. One of these was in phosphorus matches that were first sold in Stockton-on-Tees in the UK in This created a whole new industry of cheap lights - but at a terrible cost.

Breathing in phosphorus vapour led to the industrial disease phossy jaw, which slowly ate away the jaw bone. This condition particularly afflicted the girls who made phosphorus matches. So these were eventually banned in the early s and were replaced by modern matches which use either phosphorus sulfide or red phosphorus. As well as in matches, today phosphorus has found other uses in lighting. Magnesium phosphide is the basis of self-igniting warning flares used at sea. When it reacts with water it forms the spontaneously flammable gas, diphosphine which triggers the lighting of the flare.

Super pure phosphorus is also used to make light emitting diodes. These LEDs contain metal phosphides such as those of gallium and indium.

In the natural world the elemental form of phosphorus is never encountered. It is only seen as phosphate, and phosphate is essential to life for numerous reasons. It is part of DNA, and also constitutes a huge proportion of teeth enamel and bones in the form of calcium phosphate.

Organophosphates are also important, such as the energy molecule ATP and the phospholipids of cell membranes. A normal diet provides our bodies with the phosphate it needs.

With tuna, chicken, eggs and cheese having lots. And even cola provide us with some, in the form of phosphoric acid. Today most of our phosphorus comes from phosphate rock that is mined around the world, and then converted to phosphoric acid. Fifty million tonnes are made every year and it has multiple uses.

It is used to make fertilisers, animal feeds, rust removers, corrosion preventers, and even dishwasher tablets. Some phosphate rock is also heated with coke and sand in an electric furnace to form white phosphorus which is then converted to phosphorus trichloride and phosphorous acid.

And it is from these that flame retardants, insecticides, and weed-killers are made. A little is also turned into phosphorus sulfides which are used as oil additives to reduce engine wear. Phosphate is also environmentally important. It naturally moves from soil, to rivers, to oceans, to bottom sediment. Here it accumulates until it is moved by geological uplift to dry land so the circle can start again. During its journey, phosphate passes through many plants, microbes, and animals of various eco-systems.

Too much phosphate however can be damaging to natural waters because it encourages unwanted species like algae to flourish.

These then crowd out other forms of desired life. There is now a legal requirement to remove phosphate from wastewaters in many parts of the world, and in the future this could be recycled as a sustainable resource so that one day the phosphate we flush down sinks and toilets might reappear in our homes in other guises such as in dishwasher tablets and maybe even in our food and colas.

Nina Notman with the tale of Phosphorus, the element extracted from the golden stream, otherwise known as urine. Next time Andrea Sella will be joining us with the explosive story of element number In a young French chemist, Bernard Courtois, working in Paris stumbled across a new element. His family's firm produced the saltpetre needed to make gunpowder for Napoleon's wars. They used wood ash in their process and wartime shortages of wood forced them instead to burn seaweed.

Adding concentrated sulphuric acid to the ash, Courtois, obtained an astonishing purple vapour that crystallized onto the sides of the container. Astonished by this discovery he bottled up the greyish crystals and sent them to one of the foremost chemists of his day Joseph Guy-Lussac who confirmed that this was a new element and named it iode - iodine - after the Greek word for purple.

And you can hear more about how Iodine exploded onto the world's stage on next week's Chemistry in its Element, I hope you can join us. I'm Chris Smith, thank you for listening and goodbye. Chemistry in its element is brought to you by the Royal Society of Chemistry and produced by thenakedscientists.

There's more information and other episodes of Chemistry in its element on our website at chemistryworld. Click here to view videos about Phosphorus. View videos about.