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Tetrafluoromethane is the product when any carbon compound, including carbon itself, is burned in an atmosphere of fluorine. With hydrocarbons, hydrogen fluoride is a coproduct. It was first reported in 1926. [7] It can also be prepared by the fluorination of carbon dioxide, carbon monoxide or phosgene with sulfur tetrafluoride.
If there is more than one carbon atom but no multiple bonds, there are three digits, and the number of carbon atoms minus one is the first digit. If there is only one carbon atom, then there are only two digits. The last two digits are always the number of hydrogen atoms plus one (H+1), followed by the number of fluorine atoms.
PFC-14 (Carbon tetrafluoride - CF 4) has grown to become the most abundant PFC in earth's atmosphere as of year 2015. [2] Sulphur hexafluoride (SF 6) is used primarily as an arc suppression and insulation gas. It can be found in high-voltage switchgear and is used in the production of magnesium.
R14 (New York City Subway car) R14 (Rodalies de Catalunya), a regional rail line in Catalonia, Spain; Carbon tetrafluoride, a refrigerant; Nkumbi language; R14: Reacts violently with water, a risk phrase; R14 battery, a dry cell; Renault 14, a French compact car
A tetrafluoride is a chemical compound with four fluorines in its formula. ... Californium tetrafluoride, CfF 4; Carbon tetrafluoride (tetrafluoromethane) Cerium ...
Carbon tetrafluoride (R-14) CF 4: 1.01 [1] 88.0: 3.72 – 6500 Poor insulator when used alone. In mixture with SF 6 somewhat decreases sulfur hexafluoride's dielectric properties, but significantly lowers the mixture's boiling point and prevents condensation at extremely low temperatures. Lowers the cost, toxicity and corrosiveness of pure SF 6 ...
Perfluoroalkanes are very stable because of the strength of the carbon–fluorine bond, one of the strongest in organic chemistry. [4] Its strength is a result of the electronegativity of fluorine imparting partial ionic character through partial charges on the carbon and fluorine atoms, which shorten and strengthen the bond (compared to carbon-hydrogen bonds) through favorable covalent ...
Carbon–fluorine bonds can have a bond dissociation energy (BDE) of up to 130 kcal/mol. [2] The BDE (strength of the bond) of C–F is higher than other carbon–halogen and carbon–hydrogen bonds. For example, the BDEs of the C–X bond within a CH 3 –X molecule is 115, 104.9, 83.7, 72.1, and 57.6 kcal/mol for X = fluorine, hydrogen ...