Alkoxide

Short description: Conjugate base of an alcohol

Structure of the methoxide anion. Although alkali metal alkoxides are not salts and adopt complex structures, they behave chemically as sources of RO−

In chemistry, an alkoxide is the conjugate base of an alcohol and therefore consists of an organic group bonded to a negatively charged oxygen atom. They are written as RO−
, where R is the organic substituent. Alkoxides are strong bases and, when R is not bulky, good nucleophiles and good ligands. Alkoxides, although generally not stable in protic solvents such as water, occur widely as intermediates in various reactions, including the Williamson ether synthesis.[1][2] Transition metal alkoxides are widely used for coatings and as catalysts.[3][4]

Enolates are unsaturated alkoxides derived by deprotonation of a C–H bond adjacent to a ketone or aldehyde. The nucleophilic center for simple alkoxides is located on the oxygen, whereas the nucleophilic site on enolates is delocalized onto both carbon and oxygen sites. Ynolates are also unsaturated alkoxides derived from acetylenic alcohols.

Phenoxides are close relatives of the alkoxides, in which the alkyl group is replaced by a derivative of benzene. Phenol is more acidic than a typical alcohol; thus, phenoxides are correspondingly less basic and less nucleophilic than alkoxides. They are, however, often easier to handle, and yield derivatives that are more crystalline than those of the alkoxides.

## Contents

* 1 Structure
* 2 Preparation
* 2.1 From reducing metals
* 3 Properties
* 3.1 Reactions with alkyl halides
* 3.2 Hydrolysis and transesterification
* 3.3 Formation of oxo-alkoxides
* 3.4 Thermal stability
* 4 Illustrative alkoxides
* 5 Further reading
* 6 References

## Structure

Alkali metal alkoxides are often oligomeric or polymeric compounds, especially when the R group is small (Me, Et).[3] The alkoxide anion is a good bridging ligand, thus many alkoxides feature M
2O or M
3O linkages. In solution, the alkali metal derivatives exhibit strong ion-pairing, as expected for the alkali metal derivative of a strongly basic anion.

Structure of the Li
4(OBu-t)
4(thf)
3 cluster, highlighting the tendency of alkoxides to aggregate and bind ether ligands.[5]

Carbon (C)

Lithium (Li)

Oxygen (O)

Hydrogen (H)

## Preparation

### From reducing metals

Alkoxides can be produced by several routes starting from an alcohol. Highly reducing metals react directly with alcohols to give the corresponding metal alkoxide. The alcohol serves as an acid, and hydrogen is produced as a by-product. A classic case is sodium methoxide produced by the addition of sodium metal to methanol:

[math]\ce{ 2 CH3OH + 2Na -> 2CH3ONa + H2 }[/math]

Other alkali metals can be used in place of sodium, and most alcohols can be used in place of methanol. Another similar reaction occurs when an alcohol is reacted with a metal hydride such as NaH. The metal hydride removes the hydrogen atom from the hydroxyl group and forms a negatively charged alkoxide ion.

## Properties

### Reactions with alkyl halides

The alkoxide ion and its salts react with primary alkyl halides in an SN2 reaction to form an ether via the Williamson Ether Synthesis.

### Hydrolysis and transesterification

Aliphatic metal alkoxides decompose in water as summarized in this idealized equation:

Al(OR)
3 \+ 3 H
2O → Al

3 \+ 3 ROH

In the transesterification process, metal alkoxides react with esters to bring about an exchange of alkyl groups between metal alkoxide and ester. With the metal alkoxide complex in focus, the result is the same as for alcoholysis, namely the replacement of alkoxide ligands, but at the same time the alkyl groups of the ester are changed, which can also be the primary goal of the reaction. Sodium methoxide, for example, is commonly used for this purpose, a reaction that is used in the production of biodiesel.

### Formation of oxo-alkoxides

Many metal alkoxide compounds also feature oxo-ligands. Oxo-ligands typically arise via the hydrolysis, often accidentally, and via ether elimination:

RCO
2R' + CH
3O−
→ RCO
2CH
3 \+ R'OH

### Thermal stability

Many metal alkoxides thermally decompose in the range ~100–300 °C. Depending on process conditions, this thermolysis can afford nanosized powders of oxide or metallic phases. This approach is a basis of processes of fabrication of functional materials intended for aircraft, space, electronic fields, and chemical industry: individual oxides, their solid solutions, complex oxides, powders of metals and alloys active towards sintering. Decomposition of mixtures of mono- and heterometallic alkoxide derivatives has also been examined. This method represents a prospective approach possessing an advantage of capability of obtaining functional materials with increased phase and chemical homogeneity and controllable grain size (including the preparation of nanosized materials) at relatively low temperature (less than 500−900 °C) as compared with the conventional techniques.

## Illustrative alkoxides

name  | molecular formula  | comment

|
|

Tetraethyl orthosilicate | Si(OEt)4 | for sol-gel processing of Si oxides; Si(OMe)4 is avoided for safety reasons
Aluminium isopropoxide | Al4(OiPr)12 | reagent for Meerwein–Ponndorf–Verley reduction
Potassium tert-butoxide,  | K4(OtBu)4 | basic reagent for organic elimination reactions

## Further reading

* Turova, Nataliya Y. (2004). "Metal oxoalkoxides. Synthesis, properties and structures". Russian Chemical Reviews 73 (11): 1041–1064. doi:10.1070/RC2004v073n11ABEH000855. Bibcode: 2004RuCRv..73.1041T.

## References

1. ↑ Williamson, Alexander (1850). "Theory of Ætherification". Phil. Mag. 37 (251): 350–356. doi:10.1080/14786445008646627. https://zenodo.org/record/1431121. (Link to excerpt.)
2. ↑ Boyd, Robert Neilson; Morrison, Robert Thornton (1992). Organic Chemistry (6th ed.). Englewood Cliffs, N.J.: Prentice Hall. pp. 241–242. ISBN 9780136436690.
3. ↑ 3.0 3.1 Bradley, Don C.; Mehrotra, Ram C.; Rothwell, Ian P.; Singh, A. (2001). Alkoxo and Aryloxo Derivatives of Metals. San Diego: Academic Press. ISBN 978-0-08-048832-5.
4. ↑ Turova, Nataliya Y.; Turevskaya, Evgeniya P.; Kessler, Vadim G.; Yanovskaya, Maria I. (2002). The Chemistry of Metal Alkoxides. Dordrecht: Kluwer Academic Publishers. ISBN 9780792375210.
5. ↑ Unkelbach, Christian; O'Shea, Donal F.; Strohmann, Carsten (2014). "Insights into the Metalation of Benzene and Toluene by Schlosser's Base: A Superbasic Cluster Comprising PhK, PhLi, and tBuOLi". Angew. Chem. Int. Ed. 53 (2): 553–556. doi:10.1002/anie.201306884. PMID 24273149.

* v
* t
* e

Coordination complexes

Inorganic ligands

* H2O
* NH3
* N3-
* N2
* O2
* CN−
* CO
* CO2
* F−
* Cl−
* Br−
* I−

Organic ligands
* C5H5
* acac
* CH2＝CH-CH2−
* PR3
* (Me3Si)2N-
* S2C2R22-
* RCN
* =C
* ≡C

0.00

(0 votes)

Original source: https://en.wikipedia.org/wiki/Alkoxide. Read more

|

Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:Alkoxide&oldid=2597906"
*[v]: View this template
*[t]: Discuss this template
*[e]: Edit this template