Acetate bond length

Likewise the experimentally measured pattern of carbon-oxygen bond lengths m acetic acid is different from that of acetate ion Acetic acid has a short C=0 and a long C—O distance In ammonium acetate though both carbon-oxygen distances are equal... 

One after the other, examine methanol dimer and acetic acid dimer. Do the hydrogen-bond lengths in these systems differ significantly from the optimum distance in water dimer Are the hydrogen-bond angles in these compounds significantly different from those in water dimer Rationalize your results. 

Acetanilide, electrophilic aromatic substitution of, 939-940 Acetate ion, bond lengths in, 43 electrostatic potential map of, 43, 53, 56, 757 resonance in, 43 Acetk acid, bond angles in, 755 bond lengths in, 755 dimer of, 755 dipole moment of, 39 electrostatic potential map of, 53, 55... 

Earlandite structure, 6,849 Edge-coalesced icosahedra eleven-coordinate compounds, 1, 99 repulsion energy coefficients, 1,33,34 Edta — see Acetic acid, ethylenediaminetetra-Effective atomic number concept, 1,16 Effective bond length ratios non-bonding electron pairs, 1,37 Effective d-orbital set, 1,222 Egta — see Acetic acid,... 

In the acetate anion, the two oxygen atoms are equivalent, so we expect that the orbital descriptions about each O atom should be identical. You can verily that they are, and experiments further verily this the two carbon-oxygen bond lengths in acetate are identical. 

Me2CH, were obtained by iodine oxidation of dimeric platinum(II) complexes.419,420 The Pt—Pt bond lengths in the latter two compounds are 2.598(1) A and 2.578(1) A respectively,420 substantially longer than that in the acetate analogue. 

Fig. 17 Relationship between the lengths of the endo and exocyclic C-O bonds at the acetal centres of axial tetrahydropyran acetals [96] and the pKa of the conjugate acid ROH of the leaving group. Bond-length data, including standard deviations (represented as error bars) are from Briggs et al. (1984).

The further development of this approach is discussed below, in Section 4. Here we consider the evidence that the relationship between bond length and reactivity observed in the series of acetals based on structure [96] is general, rather than specific to acetals, or even specific to this particular system. 

Fig. 18 Dependence on pA nox of C-OX bond lengths for primary and secondary (cyclohexyl) sulphonate and acetate esters, and aryl and alkyl ethers. Data are best values averaged over varying numbers of compounds, and are taken from Amos el...

Thus the simplest rule that the longer the bond the faster it breaks is not general not only are bond lengths in different systems not necessarily a guide to relative reactivity, but exceptions are to be expected also in systems where the conformation about the centres of interest varies. In fact this latter restriction is probably itself limited to situations, as in the benzylic system, or in acetals, in which strong rr-type orbital overlap directly affects the C-OX bond there appears to be little dependence on torsion angle in the [Pg.166]

Carbon and oxygen atom positions were refined with anisotropic thermal parameters. Hydrogen atoms were not located. Figure 3 shows the molecular structure and the atom numbering scheme utilized for the x-ray data presented in the supplementary material for heritiana acetate. Coordinates, bond length, and bond angles for compound III acetate are available as supplementary material. 

Fig. 3.5. Typical experimental bond valences in (a) the trifluoroacetate anion and (b) the acetate ion (Brown 1980b). Bond valences are shown in the lower part of each figure and bond lengths (in pm) in the upper part.

Fig. 9.1. Structures of the acetate ion showing bond valences (above the bond) and bond lengths (in pm below the bond) (a) the ideal structure of the isolated ion (b) the structure normally observed in the solid state (c) the structure observed when bonded to a strong cation (Si) (d) the structure observed for the diprotonated acetate ion (e) the structure of the trifluoroacetate ion normally observed in the solid state.

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