Pauling's principle of electroneutrality states that each atom in a stable substance has a charge close to zero. It was formulated by Linus Pauling in 1948 and later revised.[1] The principle has been used to predict which of a set of molecular resonance structures would be the most significant, to explain the stability of inorganic complexes and to explain the existence of π-bonding in compounds and polyatomic anions containing silicon, phosphorus or sulfur bonded to oxygen; it is still invoked in the context of coordination complexes.[2][3] However, modern computational techniques indicate many stable compounds have a greater charge distribution than the principle predicts (they contain bonds with greater ionic character).[4]
- ^ The Nature of the Chemical bond, L. Pauling, 1960, 3d edition, pp. 172-173, 270, 273, 547 Cornell University Press, ISBN 0-8014-0333-2
- ^ Housecroft, C. E.; Sharpe, A. G. (2004). Inorganic Chemistry (2nd ed.). Prentice Hall. ISBN 978-0-13-039913-7.
- ^ R.H. Crabtree, The Organometallic Chemistry of the Transition Metals, 6th edition, John Wiley & Sons, (e-book), ISBN 9781118788240
- ^ Kaupp, Martin (January 1, 2001). "Chapter 1: Chemical bonding of main group elements". In Frenking, Gernot; Shaik, Sason (eds.). The Chemical Bond: Chemical Bonding Across the Periodic Table. Wiley -VCH. pp. 15–16. ISBN 978-3-527-33315-8.
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