List of oxidation states of the elements

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This is a list of all the known oxidation states of the chemical elements, excluding nonintegral values. The most common oxidation states are in bold. This table is based on Greenwood's,[1] with all additions noted. Oxidation state 0, which is found for all elements, is implied by the column with the element's symbol. The format of the table, based on one devised by Mendeleev in 1869, highlights some of the periodic trends.

−1 H +1
He
Li +1
Be +1 +2 [2]
B +1 +2 +3
−4 −3 −2 −1 C +1 +2 +3 +4
−3 −2 −1 N +1 +2 +3 +4 +5
−2 −1 O +1 +2
−1 F
Ne
−1 Na +1
Mg +1 +2 [3]
Al +1 +3
−4 −3 −2 −1 Si +1 +2 +3 +4
−3 −2 −1 P +1 +2 +3 +4 +5
−2 −1 S +1 +2 +3 +4 +5 +6
−1 Cl +1 +2 +3 +4 +5 +6 +7
Ar
-1 K +1
Ca +1 +2 [4]
Sc +1 +2 +3
−1 Ti +2 +3 +4
−1 V +1 +2 +3 +4 +5
−2 −1 Cr +1 +2 +3 +4 +5 +6
−3 −2 −1 Mn +1 +2 +3 +4 +5 +6 +7
−2 −1 Fe +1 +2 +3 +4 +5 +6 +7 +8 [5][6]
−1 Co +1 +2 +3 +4 +5
−1 Ni +1 +2 +3 +4
Cu +1 +2 +3 +4
Zn +2
Ga +1 +2 +3
−4 Ge +1 +2 +3 +4
−3 As +2 +3 +5
−2 Se +2 +4 +6
−1 Br +1 +3 +4 +5 +7
Kr +2
-1 Rb +1
Sr +1 +2 [7]
Y +1 +2 +3 [8][9]
Zr +1 +2 +3 +4
−1 Nb +2 +3 +4 +5
−2 −1 Mo +1 +2 +3 +4 +5 +6
−3 −1 Tc +1 +2 +3 +4 +5 +6 +7
−2 Ru +1 +2 +3 +4 +5 +6 +7 +8
−1 Rh +1 +2 +3 +4 +5 +6
Pd +2 +4
Ag +1 +2 +3
Cd +2
In +1 +2 +3
−4 Sn +2 +4
−3 Sb +3 +5
−2 Te +2 +4 +5 +6
−1 I +1 +3 +5 +7
Xe +2 +4 +6 +8
-1 Cs +1
Ba +2
La +2 +3
Ce +2 +3 +4
Pr +2 +3 +4
Nd +2 +3
Pm +3
Sm +2 +3
Eu +2 +3
Gd +1 +2 +3
Tb +1 +3 +4
Dy +2 +3
Ho +3
Er +3
Tm +2 +3
Yb +2 +3
Lu +3
Hf +2 +3 +4
−1 Ta +2 +3 +4 +5
−2 −1 W +1 +2 +3 +4 +5 +6
−3 −1 Re +1 +2 +3 +4 +5 +6 +7
−2 Os +1 +2 +3 +4 +5 +6 +7 +8
−3 −1 Ir +1 +2 +3 +4 +5 +6 [10]
Pt +2 +4 +5 +6
−1 Au +1 +2 +3 +5
Hg +1 +2 +4 [11]
Tl +1 +3
−4 Pb +2 +4
−3 Bi +3 +5
−2 Po +2 +4 +6
−1 At +1 +3 +5 [12]
Rn +2 [13]
Fr +1
Ra +2
Ac +3
Th +2 +3 +4
Pa +3 +4 +5
U +3 +4 +5 +6
Np +3 +4 +5 +6 +7
Pu +3 +4 +5 +6 +7 +8 [14]
Am +2 +3 +4 +5 +6
Cm +3 +4
Bk +3 +4
Cf +2 +3 +4
Es +2 +3
Fm +2 +3
Md +2 +3
No +2 +3
Lr +3
Rf +4
Db +5 [15]
Sg +6 [16]
Bh +7 [17]
Hs +8 [18]

A figure with a similar format (shown below) was used by Irving Langmuir in 1919 in one of the early papers about the octet rule.[19] The periodicity of the oxidation states was one of the pieces of evidence that led Langmuir to adopt the rule.

Langmuir valence.png

[edit] References and notes

  1. ^ Greenwood, N. N.; Earnshaw, A. (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0080379419. , p. 28.
  2. ^ Be(I) has been observed in beryllium(I) hydride (BeH); see "Beryllium: Beryllium(I) Hydride compound data". bernath.uwaterloo.ca. http://bernath.uwaterloo.ca/media/252.pdf. Retrieved 2007-12-10. 
  3. ^ Low-valent magnesium compounds with Mg(I) have been obtained using bulky ligands; see Green, S. P.; Jones C.; Stasch A. (December 2007). "Stable Magnesium(I) Compounds with Mg-Mg Bonds". Science 318 (5857): 1754–1757. Bibcode 2007Sci...318.1754G. doi:10.1126/science.1150856. PMID 17991827. 
  4. ^ Ca(I) has been observed; see Krieck, Sven; Görls, Helmar; Westerhausen, Matthias (2010). "Mechanistic Elucidation of the Formation of the Inverse Ca(I) Sandwich Complex [(thf)3Ca(μ-C6H3-1,3,5-Ph3)Ca(thf)3] and Stability of Aryl-Substituted Phenylcalcium Complexes". Journal of the American Chemical Society 132 (35): 100818110534020. doi:10.1021/ja105534w. PMID 20718434. 
  5. ^ Fe(VII) and Fe(VIII) have been observed; see Yurii D. Perfiliev; Virender K. Sharma (2008). "Higher Oxidation States of Iron in Solid State: Synthesis and Their Mössbauer Characterization - Ferrates - ACS Symposium Series (ACS Publications)". http://pubs.acs.org/doi/abs/10.1021/bk-2008-0985.ch007. doi:10.1595/147106704X10801. 
  6. ^ Fe(VIII) has been observed in iron tetroxide (FeO4); see Kiselev, Yu. M.; Nikonov, M. V.; Tananaev, I. G.; Myasoedov, B. F. (2009). "On the Existence of Plutonium Tetroxide". Doklady Akademii Nauk (Pleiades Publishing, Ltd.) 425 (5): 634–637. doi:10.1134/S0012501609040022. ISSN 0012-5016. http://www.springerlink.com/content/cm95611m66t41505/. Retrieved February 25, 2012. 
  7. ^ Sr(I) has been observed in strontium monofluoride (SrF); see P. Colarusso et al. (1996). "High-Resolution Infrared Emission Spectrum of Strontium Monofluoride". J. Molecular Spectroscopy 175: 158. http://bernath.uwaterloo.ca/media/149.pdf. 
  8. ^ Y(I) has been observed in yttrium(I) bromide (YBr); see "Yttrium: yttrium(I) bromide compound data". OpenMOPAC.net. http://www.openmopac.net/data_normal/yttrium(i)%20bromide_jmol.html. Retrieved 2007-12-10. 
  9. ^ Y(II) has been observed in yttrium(II) hydride (YH2); see "Yttrium: yttrium(II) hydride compound data". WebElements.com. http://www.webelements.com/webelements/compounds/text/Y/H2Y1-13598351.html. Retrieved 2007-12-10. 
  10. ^ Ir(−3) has been observed in Ir(CO)33−; see Greenwood, N. N.; Earnshaw, A. (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 1117. ISBN 0080379419. 
  11. ^ Hg(IV) has been observed in mercury tetrafluoride (HgF4); see Xuefang Wang; Lester Andrews; Sebastian Riedel; and Martin Kaupp (2007). "Mercury Is a Transition Metal: The First Experimental Evidence for HgF4.". Angew. Chem. Int. Ed. 46 (44): 8371–8375. doi:10.1002/anie.200703710. PMID 17899620. .
  12. ^ At(VII) has never been confirmed; see Maria, Barysz (2010). Relativistic Methods for Chemists. Springer. p. 79. ISBN 9781402099755. 
  13. ^ Rn(II) has been observed in radon difluoride; see Stein, L. (1970). "Ionic Radon Solution". Science 168 (3929): 362–4. Bibcode 1970Sci...168..362S. doi:10.1126/science.168.3929.362. PMID 17809133.  and Kenneth S. Pitzer (1975). "Fluorides of radon and element 118". J. Chem. Soc., Chem. Commun.,: 760b - 761. doi:10.1039/C3975000760b. 
  14. ^ Unstable Pu(VIII) complexes can form in alkaline solutions; see Kiselev, Yu. M.; Nikonov, M. V.; Tananaev, I. G.; Myasoedov, B. F. (2009). "On the Existence of Plutonium Tetroxide". Doklady Akademii Nauk (Pleiades Publishing, Ltd.) 425 (5): 634–637. doi:10.1134/S0012501609040022. ISSN 0012-5016. http://www.springerlink.com/content/cm95611m66t41505/. Retrieved February 25, 2012. 
  15. ^ Db(V) has been observed in dubnium pentachloride (DbCl5); see H. W. Gäggeler (2007). "Gas Phase Chemistry of Superheavy Elements". Paul Scherrer Institute. pp. 26–28. http://lch.web.psi.ch/files/lectures/TexasA&M/TexasA&M.pdf. 
  16. ^ Sg(VI) has been observed in seaborgium oxide hydroxide (SgO2(OH)2); see Huebener et al.; Taut, S.; Vahle, A.; Dressler, R.; Eichler, B.; Gäggeler, H. W.; Jost, D.T.; Piguet, D. et al (2001). "Physico-chemical characterization of seaborgium as oxide hydroxide". Radiochim. Acta 89 (11–12_2001): 737–741. doi:10.1524/ract.2001.89.11-12.737. http://www-w2k.gsi.de/kernchemie/images/pdf_Artikel/Radiochim_Acta_89_737_2001.pdf. 
  17. ^ Bh(VII) has been observed in bohrium oxychloride (BhO3Cl); see "Gas chemical investigation of bohrium (Bh, element 107)", Eichler et al., GSI Annual Report 2000. Retrieved on 2008-02-29
  18. ^ Hs(VIII) has been observed in hassium tetroxide (HsO4); see "Chemistry of Hassium" (PDF). Gesellschaft für Schwerionenforschung mbH. 2002. http://www.gsi.de/documents/DOC-2003-Jun-29-2.pdf. Retrieved 2007-01-31. 
  19. ^ Langmuir Irving (1919). "The arrangement of electrons in atoms and molecules". J. Am. Chem. Soc. 41: 868–934. doi:10.1021/ja02227a002. 
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