The mass ratio of sodium to fluorine in sodium fluoride is 1. A sample of sodium fluoride produced What scientific concept do you need to know in order to solve this problem? Our tutors have indicated that to solve this problem you will need to apply the Law of Definite Proportions concept.
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Join thousands of students and gain free access to 46 hours of Chemistry videos that follow the topics your textbook covers. Analytical Chemistry Video Lessons.
Cell Biology Video Lessons. Genetics Video Lessons. 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. How is this possible? Because the flip side of fluorine's extreme reactivity is the strength of the bonds it forms with other atoms, notably including carbon.
This property makes organofluorine compounds some of the most stable and inert substances known to man. Fluorine's special status also stems from the 'fluorine factor', the ability of this little atom to fine-tune the chemical properties of an entire molecule.
For example, replacing hydrogen with fluorine can protect drugs from degradation by metabolic enzymes, extending their active lifetimes inside the body. Or the introduced fluorine can alter a molecule's shape so that it binds better to its target protein. Such precise chemical tinkering can now be carried out in pharmaceutical labs using an array of safe, commercially-available fluorinating agents, or the tricky transformations can simply be out-sourced to someone else.
Most of us also have fluorine to thank for our beaming smiles. The cavity-fighting agents in toothpaste are inorganic fluorides such as sodium fluoride and sodium monofluorophosphate. Fluoride not only decreases the amount of enamel-dissolving acid produced by plaque bacteria, but aids in the tooth rebuilding process, insinuating itself into the enamel to form an even harder surface which resists future attack.
And the list of medical applications doesn't stop there. Being put to sleep is a little bit less worrisome thanks to fluorinated anaesthetics such as isoflurane and desflurane, which replaced flammable and explosive alternatives such as diethyl ether and chloroform. Fluorocarbons are also one of the leading candidates in development as artificial blood, as oxygen is more soluble in these materials than most other solvents. And radioactive fluorine 18 F rather than the naturally-occurring 19 F is a key ingredient in positron emission tomography or PET , a whole-body imaging technique that allows cancerous tumours to be discovered before they spread.
Fluorochemicals are also a mainstay of industry. One of the most famous is the polymer polytetrafluoroethylene, better known as Teflon, which holds the title of world's most slippery solid.
Highly thermostable and water proof, it's used as a coating for pots and pans, in baking sprays, and to repel stains on furniture and carpets. Heating and stretching transforms Teflon into Gore-tex, the porous membrane of sportswear fame.
To do that, use the molar amsses of the two elements. Let's say that you have a sample of sodium fluoride that contains x grams of sodium and y grams of fluoride. The mole ratio will thus be. This tells you that you get one mole of fluorine for every one mole of sodium.
Automatically, you know that it also produced 1. The mass of fluorine will thus be. The mass ratio of sodium to fluorine in sodium fluoride is 1. A sample of sodium fluoride produces How much fluorine in grams forms? Stefan V.
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