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Transcript
CHEM 203 Topics Discussed on Nov. 25 Toxic and carcinogenic properties of Cr(VI) compounds – including CrO3 Electrophilic reactivity of metal-oxo linkages, Mt=O: Mt = any metal O O Nu: nucleophiles add Mt Mt easily to the metal O Mt Nu Pyridinium chlorochromate (PCC): electrophilic metal-oxo O linkage Cr Cl O VI O chromium trioxide: a common source of Cr (VI) N H O Cl Cr O O N H pyridinium chloride pyridinium chlorochromate PCC oxidation of primary alcohols to aldehydes & secondary alcohols to ketones R CH2 OH O generic Cl Cr O primary VI alcohol O substitution of chloride O Hα R C H R O H an aldehyde O VI Cr O O ± H+ Hα O VI Cr a special type OH O R C H a chromate ester H IV OH complex O Cr OH redox rxs. + O of elim. react. Cr(III) + Cr(VI) a Cr(IV) complex fine details of the mechanism of PCC oxidation remain unclear. The mechanism shown above is one of a number of plausible mechanism that differ for the precise sequence of events leading to the Cr(VI) complex that ultimately decomposes to give the carbonyl product. OH Likewise: R1 2 H R generic secondary alcohol PCC O R1 R2 a ketone The conversion of an alcohol into a carbonyl compound as an oxidation reaction Lecture of Nov. 25 p. 2 overall: oxid. st. = –1 if R2 = H oxid. st. = 0 if R2 = alkyl H O R1 C OH + Cl Cr O VI O R2 oxid. st. = +1 if R2 = H oxid. st. = +2 if R2 = alkyl R R1 C 2 O + O O IV OH Cl Cr the OH-bearing C atom advances from the oxidation state of –1 or 0 to that of +1 or +2: it undergoes a two-electron oxidation. the Cr atom recedes from the oxidation state of +6 to that of +4: it undergoes a two-electron reduction. Inability of tertiary alcohols to undergo oxidation, due to the absence of α-H's Conversion of chromium trioxide into chromic acid, H2CrO4 (the Cr analog of H2SO4) O electrophilic metal-oxo Cr O VI O linkage H2O O H O Cr O VI H O O HO Cr OH VI O ± H+ chromic acid: a Cr(VI) compound The Jones reagent: a solution of chromic acid, H2CrO4, in aqueous H2SO4: O electrophilic metal-oxo Cr O VI O linkage H2O O H O Cr O VI H O ± H+ O the Jones reagent is prepared by adding HO Cr OH VI CrO3 to aq. H2SO4 O chromic acid: a Cr(VI) compound IMPORTANT: PCC is used ONLY in anhydrous (=water-free) media, while Jones rgt. is an aqueous solution. This seemingly minor difference has a major influence on the course of the reaction of primary alcohols with the two reagents. The Jones reagent: oxidation of primary alcohols to carboxylic acids and secondary alcohols to ketones in aqueous medium Reaction of the Jones reagent with primary alcohols: initial formation of a chromate ester: R CH2 O HO Cr OH VI OH O Hα R C H O OH Cr OH O O H VI ± H+ Hα R C H O OH Cr OH OH O VI Reaction of the Jones reagent with primary alcohols: decomposition of the chromate ester to give an aldehyde: Lecture of Nov. 25 p. 3 O Hα R C H OH Cr OH OH O R VI O H an aldehyde but the aldehyde is not the final product of the reaction (the carboxylic acid is): evidently, something must happen to the aldehyde that causes it to become a carboxylic acid… Acid-promoted equilibration of the aldehyde with a geminal diol in aqueous acid: H R O H R H O H O H H O H H H O R very H electrophilic H OH H O OH H OH + H O H H a geminal ("gem") diol R H note: geminal diols (obtained by the reversible hydration of carbonyl functions) display a pair of OH groups connected to the same carbon atom. Vicinal diols (obtained by OsO4 oxidation of alkenes) have their OH groups connected to adjacent carbon atoms: R1 OH C OH HO OH C C R4 R1 R2 R2 R3 a geminal diol: both OH groups are attached to the same C atom a vicinal diol: the OH groups are attached to adjacent C atoms (iii) further oxidation of the gem-diol to an acid by Cr(VI) through a second round of the mechanism shown earlier: OH R CH OH gem-diol H2CrO4 "round II" of Jones mechanism O R C OH [ + Cr(III) ] carboxylic acid Oxidation of secondary alcohols to ketones with the Jones reagent; e.g.: R2 a generic secondary R1 C alcohol H O HO Cr OH OH O HO OH HO O + Cr OH Cr OH ± H O H O O O R1 C R1 C H H R2 R2 + R1 O R2 a ketone note: ketones can — and do — form geminal diols by reaction with H3O , but the geminal diol of a ketone cannot undergo further oxidation because it has no α-H's Lecture of Nov. 25 p. 4 Summary of the above oxidation reactions: R–CH2–OH to R–CHO possible only in a water-free medium: requires PCC R–CH2–OH to R–COOH possible only in an aqueous medium: requires Jones reagent 1 2 1 2 R R CH–OH to R R C=O may be achieved with either PCC or Jones reagent Principle: any carbonyl compound will equilibrate with the corresponding geminal (gem-) diol in an aqueous acidic medium. However, gem-diols are thermodynamically disfavored relative to carbonyls, and this primarily on entropic grounds. Therefore, any attempt to isolate gem-diols will actually return the corresponding carbonyl compounds (at least as far as the carbonyl compounds seen in CHEM 203 are concerned) H R1 O R2 H H O H O R1 H H O R2 H H R1 O H OH O R2 Overall ΔG slightly positive H R1 OH OH R2 a geminal ("gem") diol