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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. It can also be classified as a haloalkane or halomethane. Tetrafluoromethane is a useful refrigerant but also a potent greenhouse ...
The partial charges in the polarized carbon–fluorine bond The carbon–fluorine bond is a polar covalent bond between carbon and fluorine that is a component of all organofluorine compounds . It is one of the strongest single bonds in chemistry (after the B–F single bond, Si–F single bond, and H–F single bond), and relatively short, due ...
Carbon tetrafluoride (tetrafluoromethane) Cerium tetrafluoride, CeF 4; Cobalt tetrafluoride, CoF 4; Curium tetrafluoride, CmF 4; Diboron tetrafluoride, B 2 F 4, a colorless gas; Dinitrogen tetrafluoride, N 2 F 4 (Tetrafluorohydrazine) Einsteinium tetrafluoride, EsF 4; Germanium tetrafluoride, GeF 4; Hafnium tetrafluoride, HfF 4; Iridium ...
In terms of Lewis structures, formal charge is used in the description, comparison, and assessment of likely topological and resonance structures [7] by determining the apparent electronic charge of each atom within, based upon its electron dot structure, assuming exclusive covalency or non-polar bonding.
The structure of organofluorine compounds can be distinctive. As shown below, perfluorinated aliphatic compounds tend to segregate from hydrocarbons. This "like dissolves like effect" is related to the usefulness of fluorous phases and the use of PFOA in processing of fluoropolymers. In contrast to the aliphatic derivatives, perfluoroaromatic ...
Lewis structure is best used to calculate formal charges or how atoms bond to each other as both electrons and bonds are shown. Lewis structures give an idea of the molecular and electronic geometry which varies based on the presence of bonds and lone pairs and through this one could determine the bond angles and hybridization as well.
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 −
An optimal Lewis structure can be defined as that one with the maximum amount of electronic charge in Lewis orbitals (Lewis charge). A low amount of electronic charge in Lewis orbitals indicates strong effects of electron delocalization. In resonance structures, major and minor contributing structures may exist. For amides, for example, NBO ...