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Chlorine pentafluoride is an interhalogen compound with formula ClF5. This colourless gas is a strong oxidant that was once a candidate oxidizer for rockets. The molecule adopts a square pyramidal structure with C4v symmetry, as confirmed by its high-resolution 19F NMR spectrum. It was first synthesized in 1963.
Xenon hexafluoride is a noble gas compound with the formula XeF6. It is one of the three binary fluorides of xenon that have been studied experimentally, the other two being XeF2 and XeF4. All known are exergonic and stable at normal temperatures. XeF6 is the strongest fluorinating agent of the series. It is a colorless solid that readily sublimes into intensely yellow vapors.
Chromium(III) fluoride is an inorganic compound with the chemical formula CrF3. It forms several hydrates. The compound CrF3 is a green crystalline solid that is insoluble in common solvents, but the hydrates [Cr(H2O)6]F3 (violet) and [Cr(H2O)6]F3·3H2O (green) are soluble in water. The anhydrous form sublimes at 1100–1200 °C.
Silver(II) fluoride is a chemical compound with the formula AgF2. It is a rare example of a silver(II) compound - silver usually exists in its +1 oxidation state. It is used as a fluorinating agent.
Copper(II) fluoride is an inorganic compound with the chemical formula CuF2. The anhydrous form is a white, ionic, crystalline, hygroscopic salt with a distorted rutile-type crystal structure, similar to other fluorides of chemical formulae MF2 (where M is a metal). The dihydrate, CuF2·2H2O, is blue in colour.
Ammonium bifluoride is the inorganic compound with the formula [NH4][HF2] or [NH4]F·HF. It is produced from ammonia and hydrogen fluoride. This colourless salt is a glass-etchant and an intermediate in a once-contemplated route to hydrofluoric acid.
Xenon difluoride is a powerful fluorinating agent with the chemical formula XeF
2, and one of the most stable xenon compounds. Like most covalent inorganic fluorides it is moisture-sensitive. It decomposes on contact with water vapor, but is otherwise stable in storage. Xenon difluoride is a dense, colourless crystalline solid.
Xenon compounds are compounds containing the element xenon (Xe). After Neil Bartlett's discovery in 1962 that xenon can form chemical compounds, a large number of xenon compounds have been discovered and described. Almost all known xenon compounds contain the electronegative atoms fluorine or oxygen. The chemistry of xenon in each oxidation state is analogous to that of the neighboring element iodine in the immediately lower oxidation state.
Aluminium fluoride is an inorganic compound with the formula AlF3. It forms hydrates AlF3·xH2O. Anhydrous AlF3 and its hydrates are all colorless solids. Anhydrous AlF3 is used in the production of aluminium. Several occur as minerals.
Krypton difluoride, KrF2 is a chemical compound of krypton and fluorine. It was the first compound of krypton discovered. It is a volatile, colourless solid at room temperature. The structure of the KrF2 molecule is linear, with Kr−F distances of 188.9 pm. It reacts with strong Lewis acids to form salts of the KrF+ and Kr
2F+
3 cations.
Manganese tetrafluoride, MnF4, is the highest fluoride of manganese. It is a powerful oxidizing agent and is used as a means of purifying elemental fluorine.
The tetrafluoroammonium cation is a positively charged polyatomic ion with chemical formula NF+
4. It is equivalent to the ammonium ion where the hydrogen atoms surrounding the central nitrogen atom have been replaced by fluorine. Tetrafluoroammonium ion is isoelectronic with tetrafluoromethane CF
4, trifluoramine oxide ONF
3, tetrafluoroborate BF−
4 anion and the tetrafluoroberyllate BeF2−
4 anion.
Fluorine forms a great variety of chemical compounds, within which it always adopts an oxidation state of −1. With other atoms, fluorine forms either polar covalent bonds or ionic bonds. Most frequently, covalent bonds involving fluorine atoms are single bonds, although at least two examples of a higher order bond exist. Fluoride may act as a bridging ligand between two metals in some complex molecules. Molecules containing fluorine may also exhibit hydrogen bonding. Fluorine's chemistry includes inorganic compounds formed with hydrogen, metals, nonmetals, and even noble gases; as well as a diverse set of organic compounds. For many elements the highest known oxidation state can be achieved in a fluoride. For some elements this is achieved exclusively in a fluoride, for others exclusively in an oxide; and for still others the highest oxidation states of oxides and fluorides are always equal.
Fluorine azide or triazadienyl fluoride is a yellow green gas composed of nitrogen and fluorine with formula FN3. Its properties resemble those of ClN3, BrN3, and IN3. The bond between the fluorine atom and the nitrogen is very weak, leading to this substance being very unstable and prone to explosion. Calculations show the F–N–N angle to be around 102° with a straight line of 3 nitrogen atoms.
Platinum tetrafluoride is the inorganic compound with the chemical formula PtF
4. In the solid state, the compound features platinum(IV) in octahedral coordination geometry.
Difluorophosphate or difluorodioxophosphate or phosphorodifluoridate is an anion with formula PO2F−2. It has a single negative charge and resembles perchlorate and monofluorosulfonate in shape and compounds. These ions are isoelectronic, along with tetrafluoroaluminate, phosphate, orthosilicate, and sulfate. It forms a series of compounds. The ion is toxic to mammals as it causes blockage to iodine uptake in the thyroid. However it is degraded in the body over several hours.
Xenon octafluoride is a chemical compound of xenon and fluorine with the chemical formula XeF8. This is still a hypothetical compound. XeF8 is reported to be unstable even under pressures reaching 200 GPa.
Nickel tetrafluoride is an inorganic compound with a chemical formula NiF4.
Ammonium hexafluorovanadate is an inorganic chemical compound with the chemical formula (NH4)3VF6.
Ammonium hexafluorochromate is an inorganic chemical compound with the chemical formula (NH4)3CrF6.
References
- ↑ Shinn, Dennis B.; Crocket, David S.; Haendler, Helmut M. (November 1966). "The Thermal Decomposition of Ammonium Hexafluoroferrate(III) and Ammonium Hexafluoroaluminate. A New Crystalline Form of Aluminum Fluoride". Inorganic Chemistry . 5 (11): 1927–1933. doi:10.1021/ic50045a020. ISSN 0020-1669 . Retrieved 22 August 2024.
- ↑ Moriya, Keiichi; Matsuo, Takasuke; Suga, Hiroshi; Seki, Syûzô (1 August 1977). "On the Phase Transition of Ammonium Hexafluoroferrate(III)". Bulletin of the Chemical Society of Japan . 50 (8): 1920–1926. doi:10.1246/bcsj.50.1920 . Retrieved 22 August 2024.
- ↑ Pebler, Jurgen (January 1985). "Iron(57) Mo¨ssbauer effect and spin correlation time in ammonium hexafluoroferrate(III)". Journal of Solid State Chemistry . 56 (1): 58–65. Bibcode:1985JSSCh..56...58P. doi:10.1016/0022-4596(85)90252-X . Retrieved 22 August 2024.
- ↑ Slivnik, Jože; Družina, Branko; Žemva, Boris (1 November 1981). "Reactions of Some Ammonium Fluorometalates with XeF 2". Zeitschrift für Naturforschung B . 36 (11): 1457–1460. doi:10.1515/znb-1981-1119 . Retrieved 29 August 2024.
- ↑ Simons, J. H. (2 December 2012). Fluorine Chemistry V2. Elsevier. p. 20. ISBN 978-0-323-14543-5 . Retrieved 22 August 2024.
- ↑ Ryss, Iosif Grigorʹevich (1960). The Chemistry of Fluorine and Its Inorganic Compounds. State Publishing House for Scientific, Technical and Chemical Literature. p. 681. Retrieved 22 August 2024.
- ↑ Wang, Hong; Zhou, Yuebo; Mo, Chenggang; Zhang, Lina; Cui, Junjun (1 December 2021). "Fluorination of α-Fe2O3 by NH4HF2 to Produce FeF3". Russian Journal of Inorganic Chemistry. 66 (14): 2017–2026. doi:10.1134/S0036023621140060. ISSN 1531-8613 . Retrieved 25 August 2024.
- ↑ Slivnik, Jože; Družina, Branko; Žemva, Boris (1 November 1981). "Reactions of Some Ammonium Fluorometalates with XeF 2". Zeitschrift für Naturforschung B . 36 (11): 1457–1460. doi:10.1515/znb-1981-1119 . Retrieved 25 August 2024.
- ↑ Official Gazette of the United States Patent Office: Patents. The United States Patent Office. 4 January 1972. p. 781. Retrieved 22 August 2024.