oxidation number

(noun)

The net sum of the negative, less the positive, charges on an atom.

Related Terms

  • paramagnetic
  • Oxidation State
  • 18 electron rule
  • manganese
  • roman numeral
  • electronegativity

(noun)

The hypothetical charge that an atom in a molecule/compound would have if all bonds were purely ionic. It indicates of the degree of oxidation of an atom in a chemical compound.

Related Terms

  • paramagnetic
  • Oxidation State
  • 18 electron rule
  • manganese
  • roman numeral
  • electronegativity

Examples of oxidation number in the following topics:

  • Oxidation Numbers of Metals in Coordination Compounds

    • O2- and S2- have oxidation numbers of -2.
    • In a molecule or compound, the oxidation number is the sum of the oxidation numbers of its constituent atoms.
    • Solution: The oxidation number of C is -3.
    • The oxidation number of H is +1 (H+ has an oxidation number of +1).
    • What is the oxidation number of chromium?
  • Electronegativity and Oxidation Number

    • Six rules can be used when assigning oxidation numbers:
    • In compounds with nonmetals, the oxidation number of hydrogen is +1.
    • Oxygen is assigned an oxidation number of -2 in most compounds.
    • In oxygen difluoride (OF2), the oxidation number of oxygen is +2, while in dioxygen difluoride (O2F2), oxygen is assigned an oxidation number of +1 because fluorine is the more electronegative element in these compounds, so it is assigned an oxidation number of -1.
    • Apply the rules for assigning oxidation numbers to atoms in compounds
  • Naming Coordination Compounds

    • Transition-metal and coordination compounds are named using a set of rules that describe oxidation numbers and anion and cation composition.
    • The oxidation number appears as a Roman numeral in parenthesis after the cation.
    • For metals, the oxidation number is the same as the charge.
    • Therefore, the platinum oxidation number is +4.
    • However, the brackets as well as the different oxidation number of the platinum result in a very different name.
  • Manganese

    • The most common oxidation states of the metal manganese are +2, +3, +4, +6, and +7; the +2 oxidation state is the most stable.
    • Manganese compounds where manganese is in oxidation state of 7+ are powerful oxidizing agents.
    • Compounds with oxidation states 5+ (blue) and 6+ (green) are strong oxidizing agents.
    • The most stable oxidation state (oxidation number) for manganese is 2+, which has a pale pink color, and many manganese(II) compounds are common, such as manganese(II) sulfate (MnSO4) and manganese(II) chloride (MnCl2).
    • Predict the oxidation or reduction propensity of a manganese species given its formula or oxidation state.
  • Oxidations & Reductions

    • To determine whether a carbon atom has undergone a redox change during a reaction we simply note any changes in the number of bonds to hydrogen and the number of bonds to more electronegative atoms such as O, N, F, Cl, Br, I, & S that has occurred.
    • If the number of hydrogen atoms bonded to a carbon increases, and/or if the number of bonds to more electronegative atoms decreases, the carbon in question has been reduced (i.e. it is in a lower oxidation state).
    • If the number of hydrogen atoms bonded to a carbon decreases, and/or if the number of bonds to more electronegative atoms increases, the carbon in question has been oxidized (i.e. it is in a higher oxidation state).
    • If there has been no change in the number of such bonds, then the carbon in question has not changed its oxidation state.
    • Peracid epoxidation and addition of bromine oxidize both carbon atoms, so these are termed oxidation reactions.
  • Oxides

    • Metal oxides typically contain an anion of oxygen in the oxidation state of −2.
    • Most of the Earth's crust consists of solid oxides, the result of elements being oxidized by the oxygen in air or water.
    • In these oxides, the coordination number of the oxide ligand is 2 for most electronegative elements, and 3–6 for most metals.
    • Although most metal oxides are polymeric, some oxides are monomeric molecules.
    • Those attacked only by acids are basic oxides; those attacked only by bases are acidic oxides.
  • Oxidation States

    • For example, Cl- has an oxidation state of -1.
    • When present in most compounds, hydrogen has an oxidation state of +1 and oxygen an oxidation state of −2.
    • Generally, the oxidation state for most common elements can be determined from their group number on the periodic table.
    • As stated in rule number four above, the sum of the oxidation states for all atoms in a molecule or polyatomic ion is equal to the charge of the molecule or ion.
    • Predict the oxidation states of common elements by their group number.
  • Phosphorus Compounds as Reducing Agents

    • Trivalent phosphorus is easily oxidized.
    • The triphenylphosphine oxide produced in reactions 1 & 3 is a very stable polar compound, and in most cases it is easily removed from the other products.
    • Triphenylphosphine is also oxidized by halogens, and with bromine yields dibromotriphenylphosphorane, a crystalline salt-like compound, useful for converting alcohols to alkyl bromides.
    • As in a number of earlier examples, the formation of triphenylphosphine oxide in the irreversible SN2 step provides a thermodynamic driving force for the reaction.
  • Chromium

    • A large number of chromium(III) compounds are known.
    • It is dehydrated by heating to form the green chromium(III) oxide (Cr2O3), which is the stable oxide with a crystal structure identical to that of corundum.
    • Chromium(VI) compounds are powerful oxidants at low or neutral pH.
    • Both the chromate and dichromate anions are strong oxidizing reagents at low pH.
    • The oxidation state +5 is only realized in few compounds but are intermediates in many reactions involving oxidations by chromate.
  • Copper

    • Copper is a ductile metal with very high thermal and electrical conductivity; its symbol is Cu and its atomic number is 29.
    • In contrast to the oxidation of iron by wet air, this oxide layer stops further corrosion.
    • Both cuprous and cupric oxides are known.
    • In contrast to the oxidation of iron by wet air, this oxide layer stops the further, bulk corrosion.
    • Both cuprous and cupric oxides are known.
Subjects
  • Accounting
  • Algebra
  • Art History
  • Biology
  • Business
  • Calculus
  • Chemistry
  • Communications
  • Economics
  • Finance
  • Management
  • Marketing
  • Microbiology
  • Physics
  • Physiology
  • Political Science
  • Psychology
  • Sociology
  • Statistics
  • U.S. History
  • World History
  • Writing

Except where noted, content and user contributions on this site are licensed under CC BY-SA 4.0 with attribution required.