Fluorine how much does it cost

Is fluorine a toothpaste? Hydrofluoric acid HF is used to etch glass, including most of the glass used in light bulbs. What makes fluorine so reactive? Reactivity is an elements ability to gain an electron. So the better it is at "stealing" electrons, the more reactive it will be. The thing that makes fluorine so reactive is its electronegativity.

Therefore, since fluorine has a higher electronegatvity than chlorine, fluorine is more reactive. How do you get the number of neutrons? This means to find the number of neutrons you subtract the number of protons from the mass number. On the periodic table, the atomic number is the number of protons, and the atomic mass is the mass number.

Which element is the most reactive? The most reactive metal on the periodic table is francium. Francium, however, is a laboratory-produced element and only minute quantities have been made, so for all practical purposes, the most reactive metal is cesium. What is fluorine found in? Is fluorine toxic to humans? Fluorine gas is very irritating and very dangerous to the eyes, skin, and lungs.

Fluorine gas at low concentrations makes your eyes and nose hurt. At higher concentrations, it becomes hard to breathe. Exposure to high concentrations of fluorine can cause death due to lung damage. What doesn't fluorine react with? Fast Facts: Fluorine. Fluorine is the most reactive and most electronegative of all the chemical elements. Although we worked hard to reduce costs by improving production efficiency and other means, we have concluded that we have no alternative but to ask our customers to bear a part of the cost increase in order to ensure the stable supply of C 2 F 6 and CF 4 gases.

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Periodic Table. Glossary Allotropes Some elements exist in several different structural forms, called allotropes. Glossary Group A vertical column in the periodic table. Fact box. Glossary Image explanation Murray Robertson is the artist behind the images which make up Visual Elements. Appearance The description of the element in its natural form.

Biological role The role of the element in humans, animals and plants. Natural abundance Where the element is most commonly found in nature, and how it is sourced commercially. Uses and properties. Image explanation. The image reflects the highly reactive nature of the element. A very pale yellow-green, dangerously reactive gas. It is the most reactive of all the elements and quickly attacks all metals.

Steel wool bursts into flames when exposed to fluorine. There was no commercial production of fluorine until the Second World War, when the development of the atom bomb, and other nuclear energy projects, made it necessary to produce large quantities. Before this, fluorine salts, known as fluorides, were for a long time used in welding and for frosting glass. The element is used to make uranium hexafluoride, needed by the nuclear power industry to separate uranium isotopes. It is also used to make sulfur hexafluoride, the insulating gas for high-power electricity transformers.

In fact, fluorine is used in many fluorochemicals, including solvents and high-temperature plastics, such as Teflon poly tetrafluoroethene , PTFE. Teflon is well known for its non-stick properties and is used in frying pans. They are now banned.

Biological role. Fluoride is an essential ion for animals, strengthening teeth and bones. It is added to drinking water in some areas. The presence of fluorides below 2 parts per million in drinking water is believed to prevent dental cavities. Fluoride is also added to toothpaste. The average human body contains about 3 milligrams of fluoride. Too much fluoride is toxic.

Elemental fluorine is highly toxic. Natural abundance. The most common fluorine minerals are fluorite, fluorspar and cryolite, but it is also rather widely distributed in other minerals. Fluorine is made by the electrolysis of a solution of potassium hydrogendifluoride KHF2 in anhydrous hydrofluoric acid. Help text not available for this section currently. Elements and Periodic Table History.

The early chemists were aware that metal fluorides contained an unidentified element similar to chlorine, but they could not isolate it. Even the great Humphry Davy was unable to produce the element, and he became ill by trying to isolate it from hydrofluoric acid.

The British chemist George Gore in passed an electric current through liquid HF but found that the gas which was liberated reacted violently with his apparatus. He thought it was fluorine but was unable to collect it and prove it. 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. Relative supply risk 6. 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 Fluorine Podcast Transcript :. You're listening to Chemistry in its element brought to you by Chemistry World , the magazine of the Royal Society of Chemistry.

The year old technician spilled only a few hundred milliliters or so in his lap during a routine palaeontology experiment. He took the normal precaution in such situations, quickly dowsing himself with water from a laboratory hose, and even plunged into a nearby swimming pool while the paramedics were en route.

But a week later, doctors removed a leg, and a week after that, he was dead. The culprit: hydrofluoric acid colloquially known as HF , and the unfortunate man was not its first victim. Unlike its close relatives, hydrochloric and hydrobromic acid, HF is a weak acid.

This, coupled with its small molecular size, allows it to penetrate the skin and migrate rapidly towards the deeper tissue layers. Once past the epidermis, HF starts to dissociate, unleashing the highly-reactive fluoride ion.

Free fluoride binds tightly to both calcium and magnesium, forming insoluble salts which precipitate into the surrounding tissues. Robbed of their co-factors, critical metabolic enzymes can no longer function, cells begin to die, tissues to liquefy and bone to corrode away. And if calcium loss is rapid enough, muscles such as the heart stop working.

Burns with concentrated HF involving as little as 2. These brave scientists were battling to be the first to isolate elemental fluorine F 2 from its various compounds, using electrolysis.

To achieve this feat, Moissan not only had to contend with HF - the preferred electrolyte in such experiments - but fluorine itself, a violently reactive gas. Moissan's feat earned him the Nobel Prize in chemistry, but the celebration was short-lived. Another victim of fluorine's toxic effects, he died only two months later.

Yet Moissan's method lived on, and is used today to produce multi-ton quantities of fluorine from its ore fluorspar. The top-selling anti-depressant Prozac, the cholesterol-lowering drug Lipitor, and the antibacterial Cipro, all have fluorine to thank for their success.