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Tetrafluoromethane is a potent greenhouse gas that contributes to the greenhouse effect. It is very stable, has an atmospheric lifetime of 50,000 years, and a high greenhouse warming potential 6,500 times that of CO 2. [10] Tetrafluoromethane is the most abundant perfluorocarbon in the atmosphere, where it is designated as PFC-14.
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 ...
Kinetic diameter is a measure applied to atoms and molecules that expresses the likelihood that a molecule in a gas will collide with another molecule. It is an indication of the size of the molecule as a target.
Carbonyl fluoride is a chemical compound with the formula C O F 2. It is a carbon oxohalide. This gas, like its analog phosgene, is colourless and highly toxic. The molecule is planar with C 2v symmetry, bond lengths of 1.174 Å (C=O) and 1.312 Å (C–F), and an F–C–F bond angle of 108.0°. [3]
C 4 F 10 O 2 S: nonafluorobutanesulfonyl fluoride: 375-72-4 C 4 FeI 2 O 4: iron tetracarbonyl diiodide: 14911-55-8 C 4 FeO 4: iron tetracarbonyl: 15281-98-8 C 4 H 2 Br 2 O 3: mucobromic acid: 488-11-9 C 4 H 2 Br 2 O 3: mucobromic acid lactone: 766-38-1 C 4 H 2 Cl 2 O 2: fumaryl chloride: 627-63-4 C 4 H 2 Cl 2 O 3: mucochloric acid: 87-56-9 C 4 ...
In the gas phase, a single water molecule has an oxygen atom surrounded by two hydrogens and two lone pairs, and the H 2 O geometry is simply described as bent without considering the nonbonding lone pairs. [citation needed] However, in liquid water or in ice, the lone pairs form hydrogen bonds with neighboring water molecules. The most common ...
It is a colorless corrosive gas that releases dangerous hydrogen fluoride gas upon exposure to water or moisture. Sulfur tetrafluoride is a useful reagent for the preparation of organofluorine compounds , [ 3 ] some of which are important in the pharmaceutical and specialty chemical industries.
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 ...