Relative reactivities iodide

In fee absence of fee solvation typical of protic solvents, fee relative nucleophilicity of anions changes. Hard nucleophiles increase in reactivity more than do soft nucleophiles. As a result, fee relative reactivity order changes. In methanol, for example, fee relative reactivity order is N3 > 1 > CN > Br > CP, whereas in DMSO fee order becomes CN > N3 > CP > Br > P. In mefeanol, fee reactivity order is dominated by solvent effects, and fee more weakly solvated N3 and P ions are fee most reactive nucleophiles. The iodide ion is large and very polarizable. The anionic charge on fee azide ion is dispersed by delocalization. When fee effect of solvation is diminished in DMSO, other factors become more important. These include fee strength of fee bond being formed, which would account for fee reversed order of fee halides in fee two series. There is also evidence fiiat S( 2 transition states are better solvated in protic dipolar solvents than in protic solvents. 

These observations reported in the mid-30 s on the relative reactivities of the C-4 and C-6 tosylates toward a nucleophile such as sodium iodide, lay dormant until 1963, when it was found (60) that treatment of methyl 2,3-di-0-benzoyl-4,6-di-0-methylsulfonyl-a-D-glucopyranoside (14) with potassium thiocyanate at 130°C. for 48 hours afforded a 40% yield of the corresponding 4,6-dithiocyanato derivative 15. 

Alkylation of enamines requires relatively reactive alkylating agents for good results. Methyl iodide, allyl and benzyl halides, a-halo esters, a-halo ethers, and a-halo ketones are the most successful alkylating agents. The use of enamines for selective alkylation has largely been supplanted by the methods for kinetic enolate formation described in Section 1.2. 

The [Rh(CO)2I2] ion is clearly an important species in systems derived from several different catalyst precursors fortuitously, it is a relatively nucleophilic rhodium species. Thus it reacts with methyl iodide at room temperature, whereas the related uncharged species, [Rh(CO)2Cl]2, is unreactive toward methyl iodide at low temperatures. This difference between neutral and charged species is also evidenced markedly in the relative reactivities of [RhL2(CO)X] and [RhL(CO)X2] toward methyl iodide, where a difference of five orders of magnitude has been observed (19). 

Table 5.4 Relative reactivities (normalized to iodide) for a series of nucleophiles under phase transfer, homogeneous dipolar aprotic, and homogeneous protic conditions, and the hydration number of the quaternary onium-anion ion pair [43]...

In this connection, it is helpful to look first at the reactivity of the anions. There is no generally acceptable measure of nucleophilic reactivity since both the scale and order of relative reactivities depend on the electrophilic centre being attacked (Ritchie, 1972). However, in the present reaction, the similarity in the reactivity of the different anions is remarkable. Thus, the Swain and Scott n-values (cf. Hine, 1962) indicate that the iodide ion should be 100 times more reactive than the chloride ion in nucleophilic attack on methyl bromide in aqueous acetone. In the present reaction, the ratio of the rate coefficients for iodide ions and chloride ions is 1.4. This similarity led to the suggestion that these reactions are near the diffusion-controlled limit (Ridd, 1961). If, from the results in Table 5, we take this limit to correspond to a rate coefficient (eqn 19) of 2500 mol-2 s 1 dm6 then, from the value of ken for aqueous solutions at 0° (3.4 x 109 mol-1 s 1 dm3 Table 1), it follows that the equilibrium constant for the formation of the electrophile must be ca. 7.3 x 10 7 mol-1 dm3. This is very similar to the equilibrium constant reported for the formation of the nitrosonium ion (p. 19). The agreement is improved if allowance is made for the electrostatic enhancement of the diffusion-controlled reaction by a factor of ca. 3 (p. 8) the equilibrium constant for the electrophile then comes to be ca. 2.4 x 10-7. 

The free energies of activation for the Sn2 reactions between acetate ion and ethyl chloride, bromide, and iodide in DMSO and in water have been calculated at the MP4/CEP-31+G(d)/MP2 level of theory.87 The solvent was accounted for using the PCM method. There was good agreement (<2.6 kcalmol-1) between the calculated and experimental values for the reactions in DMSO and water and the relative reactivities of the halides were predicted correctly in both solvents. However, the rate increases found experimentally when the solvent was changed from water to DMSO were underestimated by up to 4.5 kcalmol-1. 

The reactivity of the halide ions could not be evaluated directly since they have not been studied with the same substrate. However, -toluene-thiolate ion is nine orders of magnitude more reactive than chloride ion towards 2-chloro-l,l-diarylethylenes in dimethylformamide. Although comparison may not be justified (see below), a similar reactivity ratio exists for the reactions of j8-bromo-j -nitrostyrene with iodide ion in butyl cellosolve and thiophenoxide ion in methanol. Bromide ion is 0-6 times as reactive as chloride ion towards l-anisyl-l-phenyl-2-chloroethylene. These relative reactivities of the halide ions should be regarded only as rough estimates. Their very low reactivity is also shown by the chloride exchange in ethyl /3-chlorocrotonate, which is at least 106 times slower than the substitution by thioethoxide ion (Jones et al., 1960) while trichloroethylene does not exchange at all even at 245° (Bantysh et al., 1962). 

CH3. OH. CH2HgI, might serve as that intermediate but that would be difficult to reconcile with relative reactivities. The rate-determining step for allylmercuric iodide cleavage could be written as shown in equation (58) if the carbonium ion were the intermediate. This is analogous to the rate-determining step for propene hydration (equation... 

The difference in relative reactivity of aromatic iodides and triflates was exploited in this sequential synthesis of substituted terphenyls by repeated coupling with organozinc reagents. The more reactive iodide coupled at room temperature with palladium(O) and trio-fury]phosphine but warming to 65 °C was required for the triflate to participate in the second coupling. 

Ni catalysts are more reactive towards aryl halides, and aryl bromides and even chlorides can be successfully employed. On the other hand, Pd catalysts generally require aryl iodides and relatively reactive aryl bromides. 

Solvent effects were studied in the fate 1950s for reactions of alkylmagnesium compounds with 1-hexyne in diethyl ether. These reactions have already been discussed several times in this and in Chapter 11 (see Scheme 10) [22a], When 1.0 molEq triethylamine was added to the reaction mixture, the relative reactivity of methylmagnesium iodide toward 1-hexyne, which is 7 (the reactivity of ethylmagnesium bromide was arbitrarily set... 

Ammonium salts with two different alkyl chains were prepared directly via subsequent alkylations of dimethylamine with primary bromides and crystallization. Commercial hexadecyl-methylamine can be conveniently applied in the same way in order to convey functionality to cationic synkinons. A recent example describes subsequent alkylations with a small functional and a long-chain primary bromide (Scheme 2.4). A-acylated / -phenylenediamine was also alkylated at the second nitrogen atom which had two different alkyl chains, with or without extra functionality . After deacylation, this head group can be diazotized or coupled oxidatively with various heterocycles in water (Scheme 2.4). Photoactive and coloured membrane surfaces are thus obtained. Phenylene-diamine, pyridine and in particular A-methyl-4,4-bipyridinium chloride are relatively weak nucleophiles. Substitution of bromides is slow and the more reactive iodides can rarely be obtained commercially, but the selection of nitromethanes as solvent for bromide substitution is of great help as well as the addition of sodium iodide to enforce a Finkelstein reaction or a combination of both. 

Relative reactivity RCOCl > RCHO > tosylates, iodides > epoxides > bromides ketones > esters > nitriles. 

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