I completely agree with Craig and Rob. My point was only to procure those reagents in a small qty. and use ASAP. Otherwise, they will be sitting on the shelves for many yrs. (then worry about quenching and disposal). Students/researchers will avoid using those reagents after sometime, because they are worried for their substrate, particularly for multi-step (30 steps?) syntheses.
Regarding peroxide formation in solvents, it all comes down to the details of the chemistry.
Etherial solutions of Grignard and Lithium reagents will react with trace amounts of oxygen to destroy the OO bond and lead to the alkoxide ( 2 RM + O2 -> 2 R-O-M ). The reactions of Grignard reagents with oxygen were studied in detail by Walling (JACS, 1955, 77, 6032-6038 http://pubs.acs.org/doi/pdf/10.1021/ja01627a069 ). The only way to stop at the peroxy anions was to slowly add the Grignard reagent to an excess of oxygen ( RM + O2 -> R-O-M ). That will not happen from merely storing a closed reagent bottle for a few months.
How long can solutions of Grignard and Lithium reagents be stored?
Alkyllithium reagents in hydrocarbon solvents are quite stable (Organolithiums: Selectivity for Synthesis, J. Clayden, Pergamon, 2002 and Organolithium Methods, B. J. Wakefield, Academic Press, 1988). N-Butyllithium in hexane can be stored a year at room temperature. Alkyllithium reagents in ethereal solvents are much less stable, so methyllithium in diethyl ether has a half life of 3 months at 25 C. Thus methyllithium in diethyl ether will have a half life closer to a year at 5 C in a refrigerator.
In contrast, t-Butyllithium is very reactive and has a half life of one hour in diethyl ether at 0 C and only 45 minutes in tetrahydrofuran (THF) at –20 C. Thus, a good method to quench t-Butyllithium is with THF.
Grignard reagents are all less reactive than lithium reagents just discussed.
So why do the Sigma Aldrich SDS for methyl lithium in diethyl ether and methyl magnesium bromide in diethyl ether state “May form explosive peroxides”? (I did not find the phrase “accumulates peroxides” in the SDS.)
Mainly as a precautionary statement. If the reagents are added to excess oxygen, peroxides could form as discussed above. And once all the active reagent is gone, the diethyl ether could undergo oxidation. Thus, a stored, sealed bottle of active reagent will not form peroxides.
Since lithium and sodium metals have even greater reducing potential than Grignard and Lithium reagents, hydrocarbon or ethereal solvents stored over lithium and sodium metals will not form peroxides.
In contrast with solutions of active metal reagents, stabilizers such as hydroquinones or phenols are sometimes added to solvents. And rather than say a 1 M solution, only 0.1% might be added. Hydroquinones will quench peroxides by reduction. Phenols can scavenge radicals thus stopping oxidative radical chain reactions. Thus, solvents distilled to remove the stabilizers will be capable of peroxide formation upon extended exposure to air.
UCLA Department of Chemistry & Biochemistry
University of California Center for Laboratory Safety
Grignards are interesting beasts, particularly with respect to precipitates. There is a Schlenk equilibrium between the alkylmagnesium halide on one side and the dialkylmagnesium plus magnesium dihalide on the other:
2 RMgX <----> R2Mg + MgX2 (that should be an equilibrium arrow)
The actual behavior can be far more complex as dimers and higher oligomers are likely to form in more concentrated solutions, some of which will also have limited solubility, particularly in less polar solvents. And, of course, some of these species will have solvent molecules coordinated as well.
Found a quick simple reference for this here: http://www.chtf.stuba.sk/~szolcsanyi/education/files/Organicka%20chemia%20II/Prednaska%204_Aldehydy%20a%20ketony_Reakcie%20I/Doplnkove%20studijne%20materialy/Grignard%20Reagents%20and%20Reactions/Grignard%20Reagents-Structure%20and%20Properties.pdf as well as a detailed discussion here: http://22.214.171.124/lectures/CHEM_462/7113_Literature/ashby%201967.pdf
The presence of precipitate in a Grignard does not mean it is "bad" per se. However, all Grignard solutions should be titrated to determine the actual molarity before use. There are routine literature methods for such titrations, and they are easily done on a very small scale. But yes, Tilak is right, if you see an unusually heavy amount of precipitate this suggests that the bottle has aged, and the precipitate may be from reaction with oxygen/water and/or loss of solvent, at which point starting fresh is probably better from a synthetic standpoint.
Safety Emporium - Lab & Safety Supplies featuring brand names
you know and trust. Visit us at http://www.SafetyEmporium.com
esales**At_Symbol_Here**safetyemporium.com or toll-free: (866) 326-5412
Fax: (856) 553-6154, PO Box 1003, Blackwood, NJ 08012
On Aug 18, 2016, at 10:38 AM, TILAK CHANDRA <tilak.chandra**At_Symbol_Here**WISC.EDU> wrote:
Generally, Grignard and pyrophoric reagents such as tert-BuLi should be used/consumed ASAP. These reagents are not good for long term storage purpose. If you see lot of solid sitting in the bottom of reagent bottle, definitively they are not useful for the reaction.
Procuring less volume of these sensitive reagents is always plus.
I strongly recommend the chapter on Peroxide-Forming Chemicals in the ACS Handbook of Chemical Health & Safety. I prepared a talk on peroxidizables for our chemistry department a couple years ago and found it invaluable (both the main text and the references).
I’m leery of accepting the argument that Grignard reagents and other reactive compounds contained in the peroxidizable will necessarily suppress the formation of peroxidizables without any actual evidence. If the compound in question is a free-radical scavenger, I get it, but while Grignards sometimes form via a free-radical mechanism, I’ve never heard of them being considered scavengers or stabilizers.
Another consideration is that the peroxides may form a different phase than the ether or THF, and sometimes the critical concentration for that phase behavior is quite low. This is the source of the crystals sometimes seen floating in bottles of isopropyl ether. So your other compounds may not be relevant because they can’t reach the peroxides to degrade them.
A Sigma-Aldrich SDS for methlymagnesium bromide in solution (diethyl ether) I just pulled specifically states that it accumulates peroxides.
Dr. Daniel R. Kuespert
Homewood Laboratory Safety Advocate
Krieger School of Arts & Sciences/Whiting School of Engineering
The Johns Hopkins University
103G Shaffer Hall
3400 North Charles St.
Baltimore, MD 21218
On Aug 16, 2016, at 17:15, Humphrey, Karalyn J. <Karalyn_Humphrey**At_Symbol_Here**BAYLOR.EDU> wrote:
We’re in discussion with a research group who uses quite a number of materials flagged by our inventory system as being peroxide formers. Their claim is that certain of their materials will be unlikely to form peroxides because there are other chemicals mixed in with things life THF and ether (for example, methylmagnesium bromide in THF). My thought is that their logic is sound, but I wanted to push the question to a broader group to see if there is a consensus out there.
Karalyn (Karen) Humphrey, Ph.D
Laboratory Safety Program Manager
& Radiation Safety Officer
Department of Environmental, Health & Safety
Office: Draper 244.10
"… our job in safety is to make the task happen, SAFELY; not to interfere with the work…” Neal Langerman
Previous post | Top of Page | Next post