Sodium methoxide is the simplest sodium alkoxide. With the formula , it is a white solid, which is formed by the deprotonation of methanol. It is a widely used reagent in industry and the laboratory. It is also a dangerously caustic base.
Preparation and structure
Sodium methoxide is prepared by treating methanol with sodium:
The reaction is so exothermic that ignition is possible. The resulting solution, which is colorless, is often used as a source of sodium methoxide, but the pure material can be isolated by evaporation followed by heating to remove residual methanol.
As a solid, sodium methoxide is , with sheet-like arrays of centers, each bonded to four oxygen centers.
The structure, and hence the basicity, of sodium methoxide in solution depends on the solvent. It is a significantly stronger base in DMSO where it is more fully ionized and free of hydrogen bonding.
Applications
Organic synthesis
Sodium methoxide is a routinely used base in organic chemistry, applicable to the synthesis of numerous compounds ranging from
to
.
[ As a base, it is employed in dehydrohalogenations and various .]
Industrial applications
Sodium methoxide is used as an initiator of anionic addition polymerization with ethylene oxide, forming a polyether with high molecular weight.
Stability
The solid hydrolyzes in water to give methanol and sodium hydroxide. Indeed, samples of sodium methoxide are often contaminated with sodium hydroxide, which is difficult to detect. The compound absorbs carbon dioxide from the air to form methanol and sodium carbonate, thus diminishing the alkalinity of the base.
Commercial batches of sodium methoxide show variable levels of degradation, and were a major source of irreproducibility when used in .
Safety
Sodium methoxide is highly Causticity and reacts with water to give methanol, which is toxic and volatile.
NFPA 704
The ratings for this substance vary widely.
See also
