The charge that would be present on an atom if the element or compound in which the atom is found were ionic.
A formally defined charge that an atom in a compound or ion would have if the compound or ion existed entirely of monatomic ions.
the charge an atom in a substance would have if the pairs of electrons in each bond belonged to the more electronegative atom
the degree of oxidation of an atom or ion or molecule; for simple atoms or ions the oxidation number is equal to the ionic charge; "the oxidation number of hydrogen is +1 and of oxygen is -2"
an artificial bookkeeping device that represents the charge on an atom in a compound
A number assigned to each atom to help keep track of the electrons during a redox-reaction.
For a given element, the number of electrons it can transfer to another element with which it combines. To Top
The charge which an atom of the element has, or appears to have, in a compound.
oxidation state; positive valence. A convention for representing a charge of an atom embedded within a compound, if the compound were purely ionic. For example, H2O is a covalent compound; if it were ionic, the hydrogens would be H+ (oxidation number +1) and the oxygen would be O2- (oxidation number -2). Oxidation number rises for at least one atom in a compound that is oxidized; oxidation number becomes smaller if the compound is reduced.
The oxidation number of an element in a molecule or complex is the charge that it would have if all the ligands were removed along with the electron pairs that were shared with the central atomhttp://www.iupac.org/goldbook/O04363.pdf "Oxidation number" from the IUPAC Gold Book (PDF file). It is used in the inorganic nomenclature of inorganic compounds. It is represented by a Roman numeral; the plus sign is omitted for positive oxidation numbers.