Is fluorine metal or nonmetal?
There is a chemical element with the symbol F and atomic number 9.At standard conditions, it is a pale yellow diatomic gas.It is the most reactive element, as it reacts with all other elements except for argon, neon, and helium.
In terms of universal abundance, fluorine is 24th and 13th.As it was added to metal ores to lower their melting points, the Latin word fluo meaning "flow" gave the mineral its name.Several early experimenters died or were injured when trying to separate fluorine from its compounds.The process of low-temperature electrolysis is still used for modern production.During World War II, the Manhattan Project started the production of fluorine gas.
Half of the mined fluorite is used in steelmaking, due to the expense of refining pure fluorine.The rest of the fluorite is converted into hydrogen fluoride, which is corrosive and plays a key role in the refining of aluminum.Refrigerants, electrical insulation, and cookware are some of the uses of Molecules containing a carbon–fluorine bond that have high chemical and thermal stability.The drugs contain CF bonds.The ion from dissolved fluoride salts is used in toothpaste and water fluoridation.The global sales of fluorochemicals are more than US$15 billion a year.
SF6 has the highest global warming potential of any known substance and is generally greenhouse gases with global-warming potentials 100 to 23,500 times that of carbon dioxide.The strength of the carbon–fluorine bond is what keeps the compounds in the environment.Plants and sea sponges are known to synthesise organofluorine poisons that help deter predator activity.There are no comments at this time.
Two electrons in a filled inner shell and seven in an outer shell are required for the florine atoms to have nine electrons.The atom's physical properties are affected by the high effective nuclear charge that the outer electrons experience.[3]
The removal of electrons from neutral fluorine atoms is complicated by the third-highest ionization energy of all elements.It has the highest electronegativity of any element and has a high electron affinity, second only to chlorine.The florine atoms have a small covalent radius similar to those of oxygen and neon.note 1
The low bond energy of difluorine is similar to the easily cleaved peroxide bond and accounts for its high reactivity.The bonds to other atoms are very strong because of fluorine's high electronegativity.Wood and water spontaneously combust under a fluorine jet when unreactive substances react quickly.[22]
Different conditions are required for the reactions of fluorine with metals.To prevent passivation from the formation of metal fluoride layers, most other metals such as aluminum and iron must be powdered.Solid nonmetals react vigorously in liquid fluorine.Both hydrogen sulfide and sulfur dioxide can be combined with fluorine, the latter sometimes exploding.[26]
Like some of the alkali metals, hydrogen reacts with fluorine.Carbon reacts at room temperature to yield fluoromethane.A non-stoichiometric carbon monofluoride can be produced with fluorine above 400 C.Carbon dioxide and carbon monoxide react at or just above room temperature, whereas paraffins and other organic chemicals generate strong reactions.Although nitrogen trifluoride is stable, nitrogen requires an electric discharge at elevated temperatures for a reaction to occur, due to the strong triple bond in nitrogen.Oxygen does not combine with fluorine under ambient conditions, but can be made to react using electric discharge at low temperatures and pressures.The noble gases only react under special conditions and only with fluorine.40
When pure, fluorine is pale yellow and sometimes described as yellow-green.It has a biting odor that can be detected at 20 ppb.The transition temperature is similar to that of oxygen and nitrogen.[42]
There are two solid forms of fluorine.The latter is transparent and soft, unlike the orthorhombic systems of other solid halogens.A phase transition into opaque and hard -fluorine can be caused by further cooling to.The condensation of fluorine can be more violent than the transition from - to.There are 3 notes.
The stable isotope 19F is only found naturally in abundance.It has a high magnetogyric ratio and is the only stable isotope used in magnetic resonance.18F is the most stable with a half-life of more than 100 minutes.Most radioisotopes decay in less than a second.The heavier the isotopes 17F and 18F, the more decay they will undergo.Two metastable isomers of fluorine have a half-life of less than a second.[54]
Among the lighter elements, fluorine's abundance value of 400 ppb is 24th among elements in the universe, and other elements from carbon to magnesium are twenty or more times as common.Nuclear cross sections allow for further fusion with hydrogen or helium to create oxygen or neon.There are 56 and 57 words.
There are three explanations for the presence of fluorine.
At 700 parts per million, ferriine is the 13th most common element in the Earth's crust.Antozonite, a variant of fluorite, has been shown to have an occidental presence of elemental fluorine.The majority of fluorine is fluoride-based minerals.Cryolite is the most significant.The main source of fluorine is Fluorite, which is abundant worldwide.China and Mexico are major suppliers.The source of most of the world's fluoride is an accidental source.Cryolite is used in the production of aluminum.Natural sources of cryolite have been exhausted and are now synthesised commercially.61
There is an angle coming out of aggregate-like rock.
fluorine is found in minerals such as topaz.halides are insoluble and do not occur in commercially favorable concentrations.There are trace quantities of uncertain origin in volcanic eruptions.A 2012 study reported the presence of 0.04% F2 by weight in antozonite, attributing these inclusions to radiation.[68]
fluorite was described as an Additive used to lower the melting point of metals.He wrote the Latin word for flow for fluorite rocks.The name evolved into fluorspar and then fluorite.The composition of fluorite was later determined to be calcium difluoride.[75]
Glass etching was done with hydrofluoric acid.In 1764, Andreas Sigismund Marggraf characterized it when he heated fluorite with sulfuric acid and the resulting solution corroded its glass container.The Swedish chemist named the acidic product fluss-spats syran after the experiment he did.In 1810, the French physicist suggested that hydrogen and an element similar to chlorine constituted hydrofluoric acid.In a letter to Sir Humphry Davy dated August 26, 1812, he proposed that this then-unknown substance may be named fluorine.Greek, Russian, and some others use the name ftor or derivatives, from the Greek (phthorios, destructive), following Ampre's suggestion.The New Latin name fluorum gave the element its current symbol F.note 7
Several 19th-century experimenters were deemed "fluorine martyrs" after misfortunes with hydrofluoric acid because of initial studies that were so dangerous.The lack of a simple and suitable electrolyte, as well as the extreme corrosiveness of both hydrogen fluoride and elemental fluorine, hindered the isolation of the element.A method to produce anhydrous samples from acidified potassium bifluoride was devised by Edmond Frémy, but he discovered that the resulting (dry) hydrogen fluoride did not conduct electricity.Frémy's former student Henri Moissan persevered, and after much trial and error found that a mixture of potassium bifluoride and dry hydrogen fluoride was a conductor.He cooled the reaction to extremely low temperatures in a special bath and forged cells from a more resistant mixture of platinum and iridium.In 1886, after 74 years of effort by many chemists, Moissan isolated the element fluorine.[89]
In 1906, two months before his death, Moissan received the Nobel Prize in Chemistry.
He provided great services in his investigation and isolation of the element fluorine.The world admires the great experimental skill with which you have studied that savage beast.note 9
In the late 1920s, the Frigidaire division of GM was experimenting with chlorofluorocarbons and in 1930, a joint venture between GM and DuPont was formed to market a new type of refrigerant called freon-12 (CCl2F2).By 1949, it replaced earlier and more toxic compounds, increased demand for kitchen refrigerators, and became profitable.Polytetrafluoroethylene (Teflon) was discovered in 1938 by Roy J. Plunkett, who was working on refrigerants at Kinetic.[89]
During World War II, large-scale production of fluorine began.Germany and the Manhattan Project both used high-temperature electrolysis to make tons of chlorine trifluoride.Since UF6 is corrosive, gaseous diffusion plants need special materials: nickel for membranes, fluoropolymers for seals, and liquid fluorocarbons as coolants and lubricants.Post-war fluorochemical development was driven by this burgeoning nuclear industry.95
There is a rich chemistry of florine.It combines metals, nonmetals, metalloids and most noble gases and almost exclusively assumes an oxidation state of 1.When it forms covalent bonds, fluoroine's high electron affinity results in a preference for ionic bonding, which is polar and almost always single.99, 100, and 11 are notes.
Alkali metals have the same arrangement of sodium chloride and analogous chlorides.With the exception of beryllium difluoride, which exhibits some covalent character and has a quartz-like structure, alkaline earth difloride has strong ionic bonds but are insoluble in water.Most of the metals and rare earth elements are ionic trifluoride.There are 104 and 105 words.
Those of zirconium, hafnium, and several actinides are ionic with high melting points, while those of titanium are not.The trend continues with their linear polymers and oligomeric complexes.Most of the metal is volatile but for liquid MoF6 and ReF6, and gaseous WF6.The only metal that is characterized is Rhenium heptafluoride.The metal fluorides have more fluorine atoms.[118]
In this case, hydrogen and fluorine combine to yield hydrogen fluoride, which is similar to water.Compared to heavier hydrogen halides, it is miscible with water.Aqueous hydrogen fluoride, also known as hydrofluoric acid, is formed on contact with water.Unlike the other hydrohalic acids, which are strong, hydrofluoric acid is a weak acid.The other acids can't attack glass.[131]
Metalloids and p-block nonmetals have a variety of reactivities.Heavy nonmetals can form hypervalent fluorides.[133]
Boron trifluoride has an incomplete octet.It combines with Lewis bases like ammonia to form adducts.The group analogues, Silicon and germanium, behave as Lewis acids.The pnictogens form trifluoride that increases in reactivity and basicity with higher molecular weight.The strongest neutral Lewis acid known is found in antimony, which is the most reactive of the trifluorides.There are 118 and 140 words.
The only compound with oxygen in an oxidation state of +2 is sulfur, and there are different types of fluorides.The latter are stable by more fluorine atoms and lighter central atoms.It is possible for chlorine, bromine, and iodine to form mono-, tri- and pentafluoride.Industrial applications using chlorine trifluoride require precautions similar to those used for fluorine.149
Since 1962, no reaction with other elements has been possible with noble gases, which have complete electron shells.One of the noble gases that forms a difluoride is krypton.argon and hydrogen fluoride combine under extreme conditions to give argon fluorohydride.Helium and neon have no long-lived fluorides, and no neon fluoride has ever been observed.[151]
The strongest bond in organic chemistry is the carbon–fluorine bond.It is almost non-existent in nature, but is used in artificial compounds.The compounds involved in research in this area are diverse and reflect the complexity inherent in organic chemistry.[94]
The melting and boiling points of alkanes are lowered, density increases, and solubility in hydrocarbons decrease, as a result of the substitution of hydrogen atoms with more fluorine atoms.The insoluble nature of perfluorocarbons makes them react only with liquid ammonia.[158]
The term perfluorinated compound is used for a compound that would otherwise be a perfluorocarbon if not for the presence of a functional group.These compounds share many properties with perfluorocarbons such as stability and hydrophobicity, while the functional group enhances their reactivity, enabling them to adhere to surfaces or act as surfactants.The unfluorinated carbon atoms near the functional group are considered to be perfluoroinated.161
The melting points of polymers increase as well as the stability of the molecule.The high melting point of Polytetrafluoroethylene makes it difficult to mold.Various PTFE derivatives are less temperature tolerant but easier to mold.The fluoropolymers retain some hydrogen atoms, but they don't behave like perfluorinated ones.169
Most of the fluorine compounds are produced from hydrogen fluoride or hydrofluoric acid.The endothermic reaction of fluorite with sulfuric acid produces hydrogen fluoride.
About 20% of manufactured HF is a byproduct that can be degraded to release H2SiF6.
Moissan's method is used to produce industrial quantities of fluorine, via the electrolysis of a potassium fluoride/hydrogen fluoride mixture.The temperatures are elevated and the KF2HF is melting at 70 C.It's essential that KF acts as catalyst since pure HF can't be electrolyzed.If nickel is used, it can be stored in steel cylinders that have passivated interiors.Monel may be used instead of nickel for regulators valves and pipework.Frequent passivation and the exclusion of water and greases must be done.Under low pressure and anhydrous conditions, fluorine gas may be carried in glassware in the laboratory.175
While preparing for a 1986 conference to celebrate the 100th anniversary of Moissan's achievement, Karl O. Christe thought that chemical fluorine generation should be possible since some metal fluoride anions have no stable neutral counterparts.He came up with a way to evolve fluorine at high yield and atmospheric pressure.
Christe said that the reactants had been known for more than 100 years.According to some references, fluorine was too reactive for chemical isolation.[178]
In 1989 there were 5.6 million metric tons of Fluorite mined.In 1994 chlorofluorocarbon restrictions lowered this to 3.6 million tons.Around 4.5 million tons of ore and revenue of US$550 million were generated in 2003 and later reports estimated global fluorochemical sales at 15 billion and predicted 2016–18 production figures of 3.5 to 5.9 million ton.70% of pure metspar is used in iron smelting whereas the other 70% is converted to the key industrial intermediate hydrogen fluoride.[63]
There are at least 17,000 metric tons of fluorine produced each year.It costs only $5 per kilogram, but many times more as an element because of its handling challenges.Under vertical integration, most processes use in situ generation.[184]
The preparation of UF6 for the nuclear fuel cycle is the largest application of fluorine gas.It's formed from uranium dioxide and hydrofluoric acid.The presence of 235U or 238U in the florine makes it possible for the enrichment of the U.S.'s nuclear material.The need for hazardous polychlorinated biphenyls is eliminated with the production of the inert SF6 for high-voltage transformers and circuitbreakers.There are several fluorine compounds used in electronics.In the synthesis of organic fluorides, florine is also used, but its reactivity often necessitates conversion first to the softer brF3 or IF5 in order to allow fluorination.Sulfur tetrafluoride is used instead of fluoroinated pharmaceuticals.[63]
3 kilo of metspar is added to each metric ton of steel to lower its melting point.Most acidspar is reacted with sulfuric acid to form hydrofluoric acid, which is used in steel pickling, glass etching and alkane cracking.The replenishment of cryolite and aluminum trifluoride is necessitated by their occasional reactions with the smelting apparatus.The metric ton of aluminum requires about 51 lbs of flux.The second largest portion of fluorosilicates is used in water fluoridation and laundry effluent treatment.Other important fluorides include those of nickel and cobalt.63, 102, and 192 are the numbers.
Refrigerant gases and fluoropolymers have increased their market share.Surfactants generate over $1 billion in revenue each year.Industrial fluorocarbon production is indirect, mostly through the use of chlorocarbon chlorines, because of the danger from direct hydrocarbon–fluorine reactions.The Fowler process is used to treat the hydrocarbons with solid fluorine carriers.91 and 195 were the days.
The amount of fluorine, chlorine, carbon, and hydrogen present is identified by R-numbers.The production of chlorofluorocarbons like R-11, R-12, and R-114 peaked in the 1980s.After widespread international prohibition, their production was less than a tenth of their peak.HCFCs and HFCs were designed to be replacements for fluorine in the organic industry.R-22, chlorodifluoromethane, and R-141b are important HCFCs.The main HFC is R-134a with a new type of molecule HFO-1234yf coming to prominence due to its global warming potential of less than 1%.[197]
In 2006 and 2007, 180,000 metric tons of fluoropolymers were produced.The global market was estimated at $6 billion in 2011.Free radicals can be used to form fluoropolymers.It was 163.
The mass of the world's fluoropolymer production is represented by Polytetrafluoroethylene.The largest application is in electrical insulation.In the chemical industry, it is used to coat pipes, tubing, and gaskets.The fiberglass cloth is used for stadium roofs.Non-stick cookware is the major consumer application.The brand name Gore-Tex refers to the expanded PTFE as a fine-pored membrane and may be used for rainwear, protective apparel, and filters.They are more moldable, but also more costly, and have lower thermal stability than other fluoropolymers.Films are used in solar cells.200
The first and most prominent example is Nafion, which is a fluorinated ionomer.It was initially used as fuel cell material in spaceships and then replaced mercury-based chloralkali process cells.Efforts have been made to install fuel cells into automobiles.Perfluorobutane (C4F10) is a fire-extinguishing agent and is used as a crosslinked fluoropolymer mixture.205
Water and stains can be repelled with fluorosurfactants.Scotchgard alone generated over $300 million in 2000.Most of the cheaper products in the market are taken up by fluorosurfactants.The use of paints was only worth $100 million in 2006 because of compounding costs.[194]
Most of the agrichemicals have a few crop regulators.Increased biological stay time is one of the effects of fluorine substitution, which is usually a single atom or at most a trifluoromethyl group.Many European countries have banned the use of Trifluralin as a weedkiller because it is suspected of being a carcinogen.In mammals, acetic acid hydrogens are replaced with fluorine and sodium in order to disrupt cell metabolism.In the early 20th century, it was recognized as an insecticidal agent, and was later deployed in its current use.New Zealand uses it to protect its citizens from the Australian brushtail possum.Europe and the U.S. have banned it.There are 19 notes in this article.
Population studies from the 20th century show a reduction in dental caries.This was first thought to have been caused by the conversion of tooth hydroxyapatite into the more durable fluorappatite, but studies on pre-fluoridated teeth show that this is not the case.The control of public water supply fluoridation to fight tooth decay began in the 1940s and is now applied to water supplying 6 percent of the global population, including two-thirds of Americans.Water fluoridation has been associated with a reduction of tooth decay in children.Despite endorsements and evidence of no adverse effects, opposition still exists on ethical and safety grounds.The benefits of fluoridation are still measurable in low-income groups.fluoride toothpastes were first introduced in the U.S. in 1955 and are now ubiquitous in developed countries.
fluorine is found in twenty percent of modern pharmaceuticals.Lipitor made more revenue than any other drug until it became generic.Seretide, a top-ten revenue drug in the mid-2000s, contains fluticasone, which is fluorinated.The carbon–fluorine bond is very stable and many drugs are fluorinated to delay inactivation.The lipophilicity increases because the bond is more hydrophobic than the carbon–hydrogen bond.[224]
The fluorinated fluoxetine was one of the first to avoid the side effects of tricyclics and other antidepressants that interfered with neurotransmitters other than the serotonin target.The same treatment is given to many current antidepressants, including citalopram, its isomer escitalopram, and fluvoxamine and paroxetine.Quinolones are artificial broad-spectrum antibiotics that are often fluorinated to enhance their effects.Both ciprofloxacin and levofloxacin are included.In steroids, fludrocortisone is a blood pressure-raising mineralocorticoid, and triamcinolone and dexamethasone are strong glucocorticoids.The prototype halothane is more potent and less fluorinated than the majority of inhaled anesthetics.Faster waking times can be achieved with later compounds such as sevoflurane, which is almost insoluble in blood.[239]
The half-life of florine-18 is long enough to allow for its transport from production facilities to image centers.Computer-assisted tomography can be used for detailed images of the brain and most malignant tumors.[224]
Liquid fluorocarbons can hold large volumes of oxygen or carbon dioxide, more so than blood, and have attracted attention for their possible uses in artificial blood and in liquid breathing.Because fluorocarbons don't mix with water, they must be mixed into small droplets of perfluorocarbon to be used as blood.Initial clinical trials have been done for one of the products.One cyclist's near death in 1998 prompted an investigation into their abuse of these substances.Applications of pure perfluorocarbon liquid breathing include assisting burn victims and premature babies with deficient lungs.Only partial and complete lung filling have been tested in humans.The Alliance Pharmaceuticals effort reached clinical trials but was abandoned because the results were not better than normal therapies.[248]
It's not essential for humans or mammals, but small amounts of fluoroine can be beneficial for the strength of dental enamel.The benefits of small amounts of fluorine for bone strength have not been proven.Both the WHO and the Institute of Medicine of the US National Academies recommend a daily allowance and upper tolerated intake of fluorine.
Natural organofluorines have not been found in animals.At least 40 plants in Africa, Australia and Brazil use fluoroacetate as a defense against herbivores.Other examples include fluoroacetone and 2-fluorocitrate.The adenosyl-fluoride synthase was discovered in 2002.[252]
It's highly toxic to living organisms.Its effects in humans start at concentrations lower than hydrogen cyanide's 50 parts per million and are similar to those of chlorine, which can cause serious irritation of the eyes and respiratory system.The damage to the eyes and noses can be done at 100 ppm, compared to 270 ppm for hydrogen cyanide, which will cause death in minutes.[259]
The weakest of the hydrohalic acids is hydrofluoric acid, which has a pKa of 3.2 at 25 C.While the other hydrohalic acids are gases, it is a volatile liquid due to the presence of hydrogen bonding.It can attack glass, concrete, metals and organic matter.[263]
At least nine U.S. workers died from contact poisoning caused by hydrofluoric acid, even though it is weak and neutral in the solution.Hypocalcemia and death can be caused by calcium and magnesium in the blood.There can be serious systemic toxicity caused by insoluble calcium fluoride formation.[265]
Exposure may not be apparent for eight hours, rising to 24 hours for lower concentrations, and a burn may initially be painless.If skin has been exposed to HF, it is possible to reduce damage by rinsing it under a jet of water.2.5% calcium gluconate gel or special rinsing solutions can be used to treat skin burns.The absorption of hydrofluoric acid requires further treatment.It is not advisable to use calcium chloride in lieu of calcium gluconate.There may be need for an amputation of the affected parts.[265]
A lethal dose of 5–10 g sodium fluoride, or 32–64 g fluoride ion per kilogram of body mass, represents a moderately toxic dose for adults.One-fifth of the lethal dose can cause adverse health effects, and chronic excess consumption can lead to skeletal fluorosis, which affects millions in Asia and Africa.hydrofluoric acid forms in the stomach and can be easily absorbed by the intestines, where it crosses cell membranes, binding with calcium and interfering with various enzymes.Exposure limits are determined by urine testing.[272]
Most cases of fluoride poisoning have been caused by accidental ingestion.Most calls to poison control centers come from the ingestion of toothpaste.There was an incident in Alaska that affected almost 300 people and killed one person.The Centers for Disease Control and Prevention recommends that children under the age of six brush their teeth only if they don't swallow toothpaste.One regional study looked at a year of pre-teen fluoride poisoning reports and found 87 cases, including one death.Most had no symptoms, but a few had stomach pains.There were few serious cases and 80% of the cases involved children under six.[279]
The Montreal Protocol set strict regulations on chlorofluorocarbons due to their ozone damaging potential.When liberated chlorine and bromine atoms attacked ozone, they were not decomposing until they reached higher altitudes.Predicts warned that several generations would pass before full recovery, even with the ban and early indications of its efficacy.The current replacements, hydrochlorofluorocarbons (HCFCs), are scheduled for substitution by the year 2040 with no chlorine and zero.The Environmental Protection Agency had already banned one HCFC's production and capped two others in 2003 when this date was brought forward to 2020.Global-warming potentials (GWPs) of Fluorocarbon gases are between 100 and 10,000, while sulfur hexafluoride has a value of 20,000.HFO-1234yf is a new type of refrigerant that has attracted global demand due to its GWP of less than 1 compared to the current standard HFC-134a.[197]
The strength of the carbon–fluorine bond leads to biopersistence.Perfluoroalkyl acids (PFAAs), which are sparingly water-soluble owing to their acidic functional groups, are noted persistent organic pollutants.PFOS and PFOA are known to reside in breast milk and the blood of newborn babies, with trace quantities found in polar bears to humans.There was no clear pattern of one chemical dominating, and higher amounts of PFOS were correlated to higher PFOA, as shown in a 2013 review.PFAAs can be found in the body, but they tend to concentrate in humans and the blood.Half-lives of days in rodents and years in humans vary greatly.Humans have not been able to establish an effect on current exposure levels of PFOS and PFOA.[289]
The florine F atomic number is 9 and the melting point is 53.63 K.
The chlorine atomic number is 17 and the boiling point is 172.31 K.