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Tetrafluoromethane, also known as carbon tetrafluoride or R-14, is the simplest perfluorocarbon (C F 4). As its IUPAC name indicates, tetrafluoromethane is the perfluorinated counterpart to the hydrocarbon methane .
Lewis structure of a water molecule. Lewis structures – also called Lewis dot formulas, Lewis dot structures, electron dot structures, or Lewis electron dot structures (LEDs) – are diagrams that show the bonding between atoms of a molecule, as well as the lone pairs of electrons that may exist in the molecule.
Lewis dot diagram structures show three formal alternatives for describing bonding in boron monofluoride. Silicon tetrafluoride , similar to carbon tetrafluoride and germanium tetrafluoride , adopts a molecular tetrahedral structure. [ 81 ]
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 ...
Carbonyl fluoride can also be prepared by reaction of phosgene with hydrogen fluoride and the fluorination of carbon monoxide, although the latter tends to result in over-fluorination to carbon tetrafluoride. The fluorination of carbon monoxide with silver difluoride is convenient: CO + 2 AgF 2 → COF 2 + 2 AgF. Carbonyl fluoride is unstable ...
A convenient, safe method for generating TFE is the pyrolysis of the sodium salt of pentafluoropropionic acid: [6]. C 2 F 5 CO 2 Na → C 2 F 4 + CO 2 + NaF. The depolymerization reaction – vacuum pyrolysis of PTFE at 650–700 °C (1,200–1,290 °F) in a quartz vessel – is a traditional laboratory synthesis of TFE.
The structure of the tetrafluoroborate anion, BF − 4. Tetrafluoroborate is the anion BF − 4. This tetrahedral species is isoelectronic with tetrafluoroberyllate (BeF 2− 4), tetrafluoromethane (CF 4), and tetrafluoroammonium (NF + 4) and is valence isoelectronic with many stable and important species including the perchlorate anion, ClO −
Phosphorus trifluoride (formula P F 3), is a colorless and odorless gas.It is highly toxic and reacts slowly with water. Its main use is as a ligand in metal complexes.As a ligand, it parallels carbon monoxide in metal carbonyls, [1] and indeed its toxicity is due to its binding with the iron in blood hemoglobin in a similar way to carbon monoxide.