24 ATOMIC ORBITAL THEORY Example.In hybridizing a 2s with a 2p orbital to form two hybrids,it is possible to put more p character and less s character into one hybrid and less p and more s into the other.Thus,in hybridizing an s and a p.orbital,it is possible to generate one hybrid that has 52.8%p (sp)character.The second hybrid must be 47.2%p and is therefore spo9(/+r)lx 100%=472%:r=089).Such noneauivalent car oxygen h s mo re p charac a lone pair of electrons.If dissimilar atoms are bonded to a carbon atom,the sp hybrid orbitals will always be nonequivalent. Figure 1.49.The three hybrid sp2 atomic orbitals (all in the same plane). Acknowledgment.The authors thank Prof.Thomas Beck and Prof.William Jensen for helpful comments. SUGGESTED READING See,for example The Educypedia (The Educational Encyclopedia)http://users.telenet.be Mar s Oxfond Unisniy Pr Lonon.19s Coulson,C.A.Valence.Oxford University Press:London,1952. Douglas,B.MeDaniel,D.H.;and Alexander,J.J.Concepts and Models of Inorganie Chemistry.3rd ed.John Wiley Sons:New York.1994. Gamow .G.and Cleveland,J.M.Physics.Prentice-Hall:Englewood Cliffs.NJ.1960. Jensen.W.B.Computers Maths.Appl..12B.487 (1986):J.Chem.Ed.59.634 (1982) Pauling,L.Nature of the Chemical Bond,3rd ed.Comell University Press:Ithaca,NY,1960. Example. In hybridizing a 2s with a 2p orbital to form two hybrids, it is possible to put more p character and less s character into one hybrid and less p and more s into the other. Thus, in hybridizing an s and a pz orbital, it is possible to generate one hybrid that has 52.8% p (sp1.11) character. The second hybrid must be 47.2% p and is therefore sp0.89 ([x/(l  x)] 100%
47.2%; x
0.89). Such nonequivalent car￾bon orbitals are found in CO, where the sp carbon hybrid orbital used in bonding to oxygen has more p character than the other carbon sp hybrid orbital, which contains a lone pair of electrons. If dissimilar atoms are bonded to a carbon atom, the sp hybrid orbitals will always be nonequivalent. Acknowledgment. The authors thank Prof. Thomas Beck and Prof. William Jensen for helpful comments. SUGGESTED READING See, for example, The chemistry section of Educypedia (The Educational Encyclopedia) http://users.telenet.be/ educypedia/education/chemistrymol.htm. Atkins, P. W. Molecular Quantum Mechanics, 2nd ed. Oxford University Press: London, 1983. Coulson, C. A. Valence. Oxford University Press: London, 1952. Douglas, B.; McDaniel, D. H.; and Alexander, J. J. Concepts and Models of Inorganic Chemistry, 3rd ed. John Wiley & Sons: New York, 1994. Gamow, G. and Cleveland, J. M. Physics. Prentice-Hall: Englewood Cliffs, NJ, 1960. Jensen, W. B. Computers Maths. Appl., 12B, 487 (1986); J. Chem. Ed. 59, 634 (1982). Pauling, L. Nature of the Chemical Bond, 3rd ed. Cornell University Press: Ithaca, NY, 1960. For a description of the f orbitals, see: Kikuchi, O. and Suzuki, K. J. Chem. Ed. 62, 206 (1985). 24 ATOMIC ORBITAL THEORY 120° Figure 1.49. The three hybrid sp2 atomic orbitals (all in the same plane). c01.qxd 5/17/2005 5:12 PM Page 24