Treatment of fluoride salts

Element name: Fluorine Element symbol: F Atomic weight of the element: 19.00 Element type: Non-metal Concentration in seawater: (ppm) 0.0001 in the Pacific Ocean Surface; 950 in the Earth’s crust Proton count: 9 Neutron count: 10 Atomic number: 9 Period to which it belongs: 2 Group to which it belongs: VIIA Oxidation states: Mainly F-1; Others Electron shell arrangement: 2–7 Crystal structure: The unit cell is a simple cubic cell. Chemical bond energy: (kJ/mol) F-F 159, F-O 190, F-N 272, C-F 484. Ionization energy (kJ/mol): M – M+ 1681, M+ – M2+ 3374, M2+ – M3+ 6050, M3+ – M4+ 8408, M4+ – M5+ 11023, M5+ – M6+ 15164, M6+ – M7+ 17867, M7+ – M8+ 92036, M8+ – M9+ 106432. Unit cell parameters: a = 550 pm, b = 328 pm, c = 728 pm, α = 90°, β = 90°, γ = 90°. Discoverer: H. Moissan. Year of discovery: 1886. Discovery process: In 1886, H. Moissan in France produced fluorine by electrolyzing dried potassium hydrogen fluoride using a platinum-iridium alloy as electrodes in a platinum U-tube. Element description: A monovalent non-metal element belonging to the halogens. Under normal conditions, fluorine gas is a pale yellow-green, highly flammable, irritating toxic gas; it is one of the strongest oxidizing agents known, with the elemental symbol F. Fluorine is a pale yellow gas with a density of 1.69 grams per liter. Its melting point is -219.62°C, and its boiling point is -188.14°C. Its valence is -1. Fluorine has the highest electronegativity, with an ionization energy of 17.422 electron volts; it is the most reactive element among non-metals. It possesses strong oxidizing properties and can react with most hydrogen-containing compounds such as water and ammonia, as well as with all chemical substances in liquid, solid, or gaseous state except helium, neon, and argon. The reaction of fluorine with water is complex; it primarily produces hydrogen fluoride and oxygen, along with smaller amounts of hydrogen peroxide, dioxygen difluoride, and ozone. It can also replace other non-metal elements in compounds. It can react violently with all non-metallic and metallic elements to form fluorides and cause combustion. It is highly corrosive and toxic; extreme caution must be exercised when handling it, and its liquid or vapors must not come into contact with the skin or eyes. Element source: It can be obtained from an electrolytically melted mixture of potassium fluoride and anhydrous hydrogen fluoride. Uses of the element: Liquid fluorine can be used as an oxidizer for rocket fuel. Fluoroplastics and fluororubbers possess particularly excellent properties. Polymer materials such as fluoroplastics and fluororubbers possess excellent properties and are used in fluorine-oxygen torches and for the production of various fluorides. Elementary supplementary information: It was through repeated analyses by chemists in the early 19th century that the composition of hydrochloric acid was confirmed, and chlorine was identified as an element; due to its similarities to chlorine, fluorine was quickly recognized as an element as well, existing in hydrofluoric acid. Although its elemental form was not isolated until the 1880s. Like chlorine, fluorine is one of the elements widely distributed in nature; among the halogens, its abundance in the Earth’s crust is second only to that of chlorine. As early as the first half of the 16th century, the natural fluorine compound fluorite (CaF2) was described in the writings of European mineralogists; at that time this mineral was used as a flux, added to the ore being melted in order to lower its melting point. Therefore, the Latin name for fluorine, fluorum, comes from fluo (to flow). Its element symbol was thus designated as F. Lavoisier included the hydrofluoric acid group as an element in his table of chemical elements in 1789. By 1810, Davy had established that chlorine was an element; in the same year, the French scientist Ampère, based on the similar properties and composition of hydrofluoric acid and hydrochloric acid, boldly inferred the existence of a new element in hydrofluoric acid. He also suggested naming this element fluorine, following the naming convention for chlorine. However, elemental fluorine could not be produced for a long time; it was not until June 26, 1886, that it was synthesized by Moissan, a student of the French chemist Freytag. For this, Moissan was awarded the Nobel Prize in Chemistry in 1906; he became the second person to receive this prize for his contributions to the discovery of chemical elements. It is quite meaningful to compare the history of the discovery of chlorine and fluorine. Chlorine was identified as an element more than 30 years after its pure form was isolated ； Fluorine was identified as an element even before it was separated into its elemental form. This historical fact shows that in the process of understanding objective things, once one gradually grasps some of their laws, it becomes possible to understand them more quickly and clearly. Main properties and uses: Melting point is -219.6 °C, boiling point is -188.1 °C, and density is 1.696 g/L (at 0 °C). A pale yellow gas; it is the most reactive non-metallic element. Used to produce fluorinating reagents and as a flux in metal smelting, etc. PS: Fluorine, with an atomic number of 9 and an atomic weight of 18.9984032; its name derives from the English name of its main mineral, fluorite. In 1812, the French scientist Ampère suggested that there was a new element present in hydrofluoric acid, but free fluorine has never been produced. It was not until 1886 that French chemist Moissan produced elemental fluorine by electrolyzing potassium fluoride in anhydrous hydrofluoric acid. Because fluorine is highly reactive, free fluorine does not exist in nature. The abundance of fluorine in the Earth’s crust is 0.072%, with important minerals including fluorite and calcium fluorophosphate. The only natural isotope of fluorine is fluorine-19. Fluorine is the most reactive and strongest oxidizing substance; it can combine with all other elements ； Fluorine reacts violently with substances such as bromine, iodine, sulfur, phosphorus, carbon, and silicon at low temperatures ； Fluoride ions are small in size and can easily form stable coordination compounds with many cations ； Fluorine reacts rapidly with hydrocarbons in an uncontrolled manner. Fluorine is the first element in the halogens family, but it was discovered the latest. It took over 100 years, from the year 1771 when the Swedish chemist Scheele produced hydrofluoric acid, to the year 1886 when the French chemist Moissan isolated elemental fluorine. During this period, many people such as David, Gay-Lussac, and the Knox brothers were poisoned while trying to produce elemental fluorine, and Luyet and Nickel died due to severe poisoning. Mouvasan summarized the lessons learned from previous research; he believed that fluorine is so reactive that it cannot be electrolyzed, and the fluorine produced through electrolysis will combine with any substance it comes into contact with. If low-temperature electrolysis is used, it could be a way to solve the problem. After numerous experiments, on June 26, 1886, the Frenchman Moissan finally succeeded in producing free fluorine at low temperatures by electrolyzing a mixture of potassium fluohydride and anhydrous hydrogen fluoride, for which he was awarded the Nobel Prize in Chemistry.

It is highly toxic; it’s best to use activated carbon to absorb the gas! Emissions at high altitudes pollute the environment; are there anyone who knows something about this? If you’re involved in design, exhaust gases must be properly treated! Hehe, ask someone with experience

Are there any specific details on this topic, such as the adsorption efficiency of activated carbon and what to do after adsorption? I work in environmental impact assessment, and we’re supposed to design treatment plans – it’s so difficult! !

This solution should not be developed by those responsible for environmental impact assessments; it is not within your jurisdiction. It should be provided by the manufacturer or the design institute

Let’s negotiate with the manufacturer again; they’re quite anxious as well. If anyone has any experience in this area, please share it, thank you :)