Thermodynamics-based scheme

KELLER ETAL. A Unifying Thermodynamics-Based Scheme... 

Evans Jr. and coworkers reported a similar olefination reaction employing spirooxyphosphoranes of type 66. Upon treatment with a strong base (LiHMDS) and subsequent addition of benzaldehyde, the reaction proceeded to form anionic P(VI) intermediates (67,6 -106 to -116 ppm) that decomposed at room temperature to form the corresponding olefins and spiropentaoxyphosphoranes [ 105]. The stereoselectivity (E Z ratio) of the double bond-forming reaction depended upon the conditions evidence indicated the possibility of kinetic or thermodynamic control (Scheme 21). 

An unsymmetrical ketone can form two different enolates. In some situations it is possible to distinguish between them by trapping the separate enolates as their silyl enol ethers. The anions may then be regenerated from the silyl enol ether in an aprotic solvent under non-equilibrating conditions using fluoride ion. The rapidly formed kinetic enol of 2-methylcyclohexanone may be trapped using lithium di-isopropylamide as the base (Scheme 3.77a). On the other hand, the thermodynamically more stable enol is trapped with a milder base such as triethylamine (Scheme 3.77b). ... 

Caldwell et al. have also reported a stereoselective [2 + 2] photocycloaddition where the major product was the most thermodynamically stable. Scheme 54 shows that the cyclobutane product with the two aryl groups trans to each other predominates, but it is not the exclusive product. The proposed intermediates include a 1,2-biradical, where the p-orbitals are perpendicular to each other, and a 1,4-biradical intermediate which has time to assiune the most stable conformation before closing. The 1,2-biradical intermediate is supported by rate studies and quenching data, but these studies are not conclusive [41a]. In addition, the possibility of involvement of an exciplex prior to cycloaddition cannot be ruled out based on the studies Caldwell et al. have reported. 

It should also be mentioned that the measure-preserving thermostatting methods discussed in [373] refer rather to the underlying measure of the phase space and not the thermodynamic equilibrium distribution those methods are deterministic and, like Nose-Hoover based schemes, will exhibit thermodynamic errors due to both lack of ergodicity and discretization error, in addition to sampling errors. 

A different thermodynamic cycle (Scheme 3.8 and Equation 3.129) can give the free energy of H dissociation from a hydride complex. In some cases the results (Table 3.5) - have been confirmed by measuring the equilibrium constant for heterolytic cleavage of Hj by and a base B. 

The thermodynamic integration scheme can be appUed to different models including coarse-grained, partide-based models of amphiphihc systems and membranes [133, 134] (e.g., soft DPD-models [135-137], Lennard-Jones models [138,139], or solvent-free models [140-142] of membranes) as well as field-theoretic representations [28]. It can be implemented in Monte Carlo or molecular dynamic simulations, as well as SCMF simulations [40-42, 86], field-theoretic simulations [28], and external potential dynamics [27, 63, 64] or dynamic density functional theory [143, 144]. 

Scales for bases that are too weak to study in aqueous solution employ other solvents but are related to the equilibrium in aqueous solution. These equilibrium constants provide a measure of thermodynamic basicity, but we also need to have some concept of kinetic basicity. For the reactions in Scheme 5.4, for example, it is important to be able to make generalizations about the rates of competing reactions. 

The general features of the monensin synthesis conducted by Kishi et al. are outlined, in retrosynthetic format, in Scheme 1. It was decided to delay the construction of monensin s spiroketal substructure, the l,6-dioxaspiro[4.5]decane framework, to a very late stage in the synthesis (see Scheme 1). It seemed reasonable to expect that exposure of the keto triol resulting from the hydrogen-olysis of the C-5 benzyl ether in 2 to an acidic medium could, under equilibrating conditions, result in the formation of the spiroketal in 1. This proposition was based on the reasonable assumption that the configuration of the spiroketal carbon (C-9) in monensin corresponds to the thermodynamically most stable form, as is the case for most spiroketal-containing natural products.19 Spiro-ketals found in nature usually adopt conformations in which steric effects are minimized and anomeric effects are maximized. 

The intramolecular Michael addition11 of a nucleophilic oxygen to an a,/ -unsaturated ester constitutes an attractive alternative strategy for the synthesis of the pyran nucleus, a strategy that could conceivably be applied to the brevetoxin problem (see Scheme 2). For example, treatment of hydroxy a,/ -unsaturated ester 9 with sodium hydride furnishes an alkoxide ion that induces ring formation by attacking the electrophilic //-carbon of the unsaturated ester moiety. This base-induced intramolecular Michael addition reaction is a reversible process, and it ultimately affords the thermodynamically most stable product 10 (92% yield). 

This highly active epoxidation system, based on the controlled hydrolysis of BTSP with a catalytic amount of water, maximizes the formation of the Re monoperoxide complex at the expense of the more thermodynamically stable bis (peroxide) (Scheme 12.8). BTSP is very stable and can be prepared in molar amounts... 

More detailed and theoretical explanations of the role of the catalyst, based on this scheme, have appeared (72, 74, 77-82). In order to obtain experimental evidence for this scheme, some investigators did experiments in which 1,2-dimethylcyclobutane or cyclobutane were brought into contact with an active metathesis catalyst. However, 1,2-dimethylcyclobutane was stable under conditions where propene gave a high conversion to ethene and 2-butene (63). The experiments with cyclobutane led to the same conclusion (83). From this, and from the fact that cyclobutanes are not reaction products, although this can be expected thermodynamically, it follows that cyclobutanes are not free intermediates. This prompted Lewandos and Pettit (83) to propose a tetramethylene complex as the key intermediate ... 

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