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The Pauling 3-Electron Bond

In 1931, Pauling introduced the 3-electron bond structure A--B as a way to summarize resonance between the Lewis valence-bond structures A -B and A- B, i.e., Pauling wrote A---B= A -B - A- B. [Pg.42]

Strength of a 3-electron bond should be approximately equal to that of a 1-electron bond. If we indicate the spins of the electrons, as in [Pg.43]

For the three electrons of the Pauling 3-electron bond , a molecular orbital description of them can also be constructed using the bonding and antibonding molecular orbitals v / b =a-pAb and = a-b. The Pairli exclusion principle [Pg.43]

Chapter 3 Wave-Functions and Valence-Bond Structures for 1-Electron Bonds,.  [Pg.44]

The above considerations show that the Green and Linnett structure A B, with one bonding and two non-bonding electrons, provides a better and clearer diagramatic representation of the electron distribution than does the Pauling stmcture A---B. Therefore we shall use the A-B representation in the remainder of this book. However, (perhaps misleadingly), we shall continue to refer to this valence-bond stmcture as a Pauling 3-electron bond stmcture. [Pg.44]


The remainder of this chapter provides a discussion of the need for an increased-valence theory. A reading of it is not required in order to follow the Pauling 3-electron bond and Lewis theory of Chapters 3-9. [Pg.12]

For 6-electron 4-centre (and longer JV-centre) bonding units, similar types of properties exist for most of the increased-valence structures. For example, by spin-pairing the odd-electrons of the Pauling 3-electron bond stmctures A B and C i), increased-valence structure A - B—C - D for 6-electron 4-centre bonding units is obtained. This structure summarizes resonance between the Lewis... [Pg.32]

When electrostatic interactions between the electrons are neglected, the total electronic energies for the Pauling 3-electron bond and the no-bond configurations ) nd Y are given by Eqs. (38) and (39). [Pg.50]

When the Heitler-London wavefimction a(l)b(2) + b(l)a(2) is used as the wavefimction for the A-B electron-pair bond, and an electron is added to the antibonding molecular orbital ( ) ab = a - Ab, the Pauling 3-electron bond identity. [Pg.53]

The Pauling 3-electron bond valence bond structure ( H is also... [Pg.54]

The results of calculations by Baird and Taylor" show that as the difference in electronegativity between A and B in the Pauling 3-electron bond stmcture... [Pg.60]

The Pauling 3-electron bond theory of hypoligation has wide applicability. All d - d transition-metal complexes of the type will involve one or more Pauling 3-electron bonds in their valence-bond stmctures, if the metal-ion has insufficient vacant inner d and valence-shell s and p orbitals available to form N electron-pair M-L o-bonds with the N ligands. [Pg.72]

By utilizing Pauling 3-electron bonds , we can reduce the number of valence-bond structures that we need from four to two. Thus the resonance between Lewis structures (1) and (2) generates the Pauling 3-electron bond structure (5). [Pg.76]

Resonance between the Pauling 3-electron bond structures (7) and (8) (or (9) and (10)) do not account for one NOj bond-property. The N-O bond-lengths of 1.19 A are similar to Pauling s estimate of 1.20 A for an N-O double bond (cf 1.214 A for CHjN = O f. However, resonance between stractures (7) and (8), each of which has seven bonding electrons, would imply that the N-O bonds for NO2 should be longer than double bonds. To obtain an additional bonding electron in each structure, it is necessary to utilize the increased-valence procedures that we shall describe in Chapters 11 and 12. [Pg.78]

Valence-bond structures with Pauling 3-electron bonds are also appropriate for a number of radicals with 19 valence-shell electrons. As our first example, we shall examine the bonding for the anion O3. The Pauling 3-electron bond structures (22) and (23) for this radical summarize resonance between Lewis structures (24) and (26), and (24) and (25), respectively. [Pg.79]

For CIO2, the Pauling 3-electron bond structures are (30) and (31), if only the chlorine 3 s and 3p orbitals are utilized for bonding. [Pg.80]

A B. This is because resonance between the Pauling 3-electron bond and Y A B is equivalent to resonance... [Pg.81]

However, as we shall discuss in Section 8-l(c), the concomitant bonding interaction between two 0-Cu(ll)-0 moieties arises primarily from covalent-ionic resonance of the Pauling 3-electron bond type (cf. Section 7-3) rather than from the spin-pairing of the unpaired-electrons in the covalent structures. [Pg.107]

Alternatively, because the n-orbital configuration (hjj) (njjQ) (7to) for the Pauling 3-electron bond is equivalent to (n o) (nJjo) in which... [Pg.127]

The 5 = 1 spin excited state is predicted to have an N-O bond-length whieh is similar to that of the ground-state, and a linear arrangement for the C, N and O atoms. The linearity will improve the overlap that exists between the h and % orbitals (h grows into ) and thereby increases the strength of the Pauling 3-electron bond for the three n electrons (provided that the overlap integral does not exceed 1/3 cf Section 3-10). [Pg.127]

Valence-bond stmcture (5) is equivalent to (the lower-energy) resonance between the electron spin stmctures (3) and (4). It is also equivalent to (the lower-energy) resonance between the Lewis stmctures (6) and (7), each of which has an electron-pair bond and a lone-pair of electrons. The latter equivalence arises because the Pauling 3-electron bond configuration (a) (Vab) (by with =2L + lda is equivalent to (a) (b) +A(a) (b) i.e. the Panling 3-electron... [Pg.140]


See other pages where The Pauling 3-Electron Bond is mentioned: [Pg.11]    [Pg.11]    [Pg.27]    [Pg.31]    [Pg.31]    [Pg.42]    [Pg.43]    [Pg.44]    [Pg.44]    [Pg.44]    [Pg.45]    [Pg.45]    [Pg.47]    [Pg.48]    [Pg.50]    [Pg.52]    [Pg.53]    [Pg.60]    [Pg.61]    [Pg.77]    [Pg.79]    [Pg.80]    [Pg.81]    [Pg.83]    [Pg.105]    [Pg.109]    [Pg.111]    [Pg.126]    [Pg.128]    [Pg.131]    [Pg.131]    [Pg.132]    [Pg.134]    [Pg.138]   


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