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Nitrogen trifluoride is the inorganic compound with the formula (NF 3).It is a colorless, non-flammable, toxic gas with a slightly musty odor.In contrast with ammonia, it is nonbasic.
Formal charges in ozone and the nitrate anion. In chemistry, a formal charge (F.C. or q*), in the covalent view of chemical bonding, is the hypothetical charge assigned to an atom in a molecule, assuming that electrons in all chemical bonds are shared equally between atoms, regardless of relative electronegativity.
Bond lengths and charge densities are shown as functions of how many hydride ligands are on the central atoms. For every new hydride, there is one less fluoride. [36] For silicon and phosphorus bond lengths, charge densities, and Mulliken bond overlap, populations were calculated for tetra and pentacoordinated species by this ab initio approach ...
NF3 may refer to: Nitrogen trifluoride (NF 3), a colorless gas used as an etchant; Zukertort Opening, an opening move in chess (1. Nf3) This page was last edited on 3 ...
As an example, summing bond orders in the ammonium cation yields −4 at the nitrogen of formal charge +1, with the two numbers adding to the oxidation state of −3: The sum of oxidation states in the ion equals its charge (as it equals zero for a neutral molecule). Also in anions, the formal (ionic) charges have to be considered when nonzero.
As a result of its small size and high negative charge density, the fluoride anion is the "hardest" base (i.e., of low polarizability). Because of this, fluorides in real salt crystals often have higher effective charges than oxides of the same metal, even though oxygen's formal charge is twice as great as fluorine's. [citation needed]
A demonstration that how some well known 1,3-dipoles like ozone, nitro compounds and azides can be shown to have a resonance structure having 1,3 relationship between positive and negative formal charges. Known 1,3-dipoles are: Azides (RN 3) Ozone (O 3) Nitro compounds (RNO 2) Diazo compounds (R 2 CN 2) Some oxides. Azoxide compounds (RN(O)NR)
An alternative definition of valence, developed in the 1920's and having modern proponents, differs in cases where an atom's formal charge is not zero. It defines the valence of a given atom in a covalent molecule as the number of electrons that an atom has used in bonding: [8] [9] [10] [11]