Limits to Poisson’s ratio in isotropic materials – general ...
Limits of phosphorus hypervalency explored
Transcript of Limits of phosphorus hypervalency explored
Science
IR instrument combination gives reflectance spectrum of spot area of acrylic polymer % Transmittance 100 I
90
80
70
60
50
40
30
20
10
Spectrum of a 4Q-;ftm spot of pojymethyl methacrylate on silicon wafer, coliected with 4 crrr1 resolution using an IBM instruments IR microscope on an IBM IB/ 38 FHft spectrophotometer
Ι ι ι J_ J I t L—L 4U00 3500 3000 2500 2000
Wave number, cm"1 1500 1000
Phοtomicrograph (magnification 300X, 1 cm = 33μπ\) of polymethyl methacrylate on silicon wafer corresponds to spectrum above
tungsten needle. IR microscopy showed the substance to be sodium carboxymethylcellulose. This finding helped to identify the coating as a cosmetic that the suspect used.
To identify specks of spray paint in a hit-and-run case, Paleneik used a pyrolysis technique that McCrone Associates developed. Using this technique, the IR spectrum of a paint speck pyrolyzed in a melting-point capillary tube, extracted, and dried
showed the presence of bisphenol A. This helped in tracing the paint to the car in the case.
Detective Kubic described several cases he had investigated with police officers. In one case, red fibers were found near the body of a man shot to death in his driveway. IR microscopy showed that the fibers came from a rug laid in the back seat of a car parked nearby. On taking up the rug and a plywood floor from the back seat, officers found more red fibers beneath. They proved to come not from the rug but from a red ski cap that a suspect wore. These findings linked the suspect to the car and the car to the scene of the slaying.
In a hit-and-run case, Kubic and his partners had to trace the make and model of the car from a speck of paint. Light microscopy showed that the car had been repainted. Using a tungsten needle, the investigators pried a layer of original black paint from between the white topcoat and a brown primer. IR microscopy of the black paint identified it and pointed to the kind of car involved.
In another case, a child riding a
bicycle was hit by a car, and the Mineola criminologists looked for evidence to implicate a particular car. IR microscopy showed that a smear of blue paint on one of the car's rubber bumper guards had come from the bicycle, and that a bit of resin on the front of the car hood had come from a cap on one of the bicycle handlebar grips.
The IR microscope attachments int roduced at the symposium by Analect and IBM have binocular, stereoscopic eyepieces to view samples in visible light. Moving an outside lever selects for viewing under visible light or for recording of transmission or reflectance IR spectra. A user may move metal plates with pinholes of different diameters over samples to mask areas whose IR spectra are to be determined. For such samples as fibers, rectangular slits are adjustable for widths and lengths.
The Analect attachment, not including an FTIR spectrometer, is priced at $23,000 and the IBM at $35,000. Also, for $17,000, Analect offers an attachment for transmission spectroscopy only. D
Limits of phosphorus hypervalency explored A quirky molecule first made about 10 years ago at Iowa State University is helping chemists there explore the limits of hypervalency in nonmetallic elements such as phosphorus. The molecule is an amine phosphate in which three of the phosphate oxygens each are connected to the same nitrogen via a two-carbon bridge. Nomenclature fans would call it 2,8,9-trioxa-5-aza-l-phosphabicyclo[3.3.3]undecane 1-oxide.
When graduate student Dean S. Milbrath prepared it as part of his doctoral thesis research for chemistry professor John G. Verkade, neither one realized what he had stumbled onto. But molecular orbital calculations done on this molecule in collaboration with professor Henk M. Buck and coworkers at Eindhoven University of Technology in the Netherlands revealed an intriguing possibility: The nitrogen atom might
16 December 9, 1985 C&EN
be able to donate some electron density to the four-coordinate phosphorus atom, forming an axial or transannular bond; in the process, the phosphorus would become hy-pervalent.
With a little prodding, says Ver-kade, that's what the molecule seems to do. For example, when former graduate student Leslie E. Carpenter II treated the amine phosphate with boron trifluoride, he discovered that the electron-deficient boron binds to the phosphoryl oxygen—not, as one might expect, to the nitrogen. In addition, a dative bond from the nitrogen to the phosphorus forms, creating a neutral, tricyclic paddle-wheel structure called a phosphatrane [/. Am. Chem. Soc, 107, 7084 (1985)]. In the process, the geometry around the phosphorus shifts from four-coordinate tetrahedral to five-coordinate trigonal bipyramidal. The phosphorus, by strict definition, has become hypervalent because it is surrounded by 10 electrons, rather than its usual octet, and it coordinates to five groups, rather than the usual three or four.
Carpenter and Verkade have demonstrated that other Lewis acids, by virtue of their electron-withdrawing ability, also can trigger the collapse of the amine phosphate to a phosphatrane. This happens, for instance, when a triethylsilyl group is attached to the phosphoryl oxygen. Even more unexpected, Carpenter found that by using an excess of the silylating reagent, he could hitch a second triethylsilyl moiety to the oxygen, forming a dication (positive charges on oxygen and nitrogen).
Working with the Eindhoven group, the Iowa State researchers also generated cationic phosphatranes simply by protonating or di-protonating the phosphoryl oxygen.
More surprises were in store when Carpenter treated the amine phosphate with anhydrous phosphoric acid. A white solid immediately precipitated out of solution. A 31P nuclear magnetic resonance spectrum of the solid product, as well as other evidence, suggests a novel "double-cage" adduct in which an H2P04~ moiety is hydrogen-bonded to a hydroxy phosphatrane cation.
This solid-state NMR spectrum is the only concrete evidence Verkade has so far to support the proposed structure of the adduct. That's because the adduct is so insoluble that Carpenter, now a postdoctoral research associate at Rensselaer Polytechnic Institute, never was able to crystallize it and get an x-ray structure. The one solvent that does dissolve the adduct—dimethylsulfox-ide—also dissociates it into the re-actants used to make it, Verkade says.
The Iowa State professor readily admits that the pleasing symmetry of the proposed structure is speculation on his part, but, he adds, "it's not bad speculation because it explains why the stuff is so insoluble." In the proposed structure, the bond dipole moments all point in the same direct ion, and, w h e n summed, give a molecular dipole moment of about 10.7 debye units. Such an extraordinarily large dipole moment could explain the ad-
duct's extreme insolubility, Verkade notes.
Although the trigonal bipyramidal structure of other phosphatranes already has been established by x-ray methods, these new derivatives created by Carpenter cry out for crystal structures. But the prospects for some of them don't look very promising. The trifluorobo-ratooxy derivative, which hasn't been isolated, is "probably a lost cause," in Verkade's words, "because the BF3 group dissociates too easily." The phosphoric acid adduct appears to be too insoluble for crystallization. The silylated phosphatranes, on the other hand, offer some hope because they have been isolated as an apparently microcrystal-line mixture. Verkade thinks other silyl derivatives may be easier to crystallize in pure form. One of his new coworkers is now tackling the challenge, with continuing support from the National Science Foundation.
React to this... HOOCCH2 - CH - NH - (CH2COOH)2
COOH SUBSTITUTED ASPARTIC ACIDS
NaS-C-N(CH2COONa)2
SOLUBLE DITHIOCARBAMATES
HOOCCH2-N-CH2COOH IMINODIACETIC ACID (IDA)
CH,-C 1 COOCH2-CH CH2-N (CH2COOH)2
OH CHELATING POLYMERS
J n
Start your next new product with HAMPSHIRE® IDA. • Pharmaceuticals · Pesticides · Polymers
• Chemical Intermediates · Cosmetics Discover a world of Amino Acid Chemistry.
Write for our idea-packed, 28-page brochure.
GRACE Organic Chemicals Division, W. R. Grace & Co.
55 Hayden Avenue, Lexington, MA 02173 (617) 861-6600
CIRCLE 37 ON READER SERVICE CARD
December 9, 1985 C&EN 17
THE CHOICE IS EASY Borg-Warner Chemicals, the only single source for all these high-quality additives:
IILTRANOX.™ 246 Antioxidant 2,2 '-methylene-bis-( 4-meth\1-6-t-but\1phcnol )
OH OH
( C H ^ C n : Ô C H < ° V C H 3 > 3
CH 3 CH 3
ULTRANOX 236 Antioxidant 4,4'-thio-bis(2-t-buryl-S-mcthylphcnol)
CH3 CH3
H0Λ ° A s \ ° /"0H
C(CH3)3 QCHj ) ,
ULTRANOX 256 Antioxidant Polymeric sterically hindered phenol
OH r OH η
CH3 L OH, J n
IILTRANOX 254 Antioxidant Polymeric 2,2,4-trimethyl-l, 2-dihydroquinoline
C H ,
C H 3
N " C H 3
Η
ULTRANOX 226 Antioxidant 2,6 di-t-butyl-4-methylphenol
OH
( C H 3 ) 3 C Y ^ N - C ( C H 3 ) 3
CH 3
WESTON® TNPP TrisNonylphenyl Phosphite
EBS WAX Ν ,Ν'-ethylenebisstearamide
Call us also for SPINUVEX™ Hindered Amine Light Stabilizers, WESTON® Specialty Phosphite Stabilizers, BLENDEX® Modifier Resins, Surfactants, Emulsifiers, Phosphate Plasticizers, Polymer Lubricants and Alkylphenols. TM SPINUVEX is a trademark of Montefluos ™ULTRANOX is a trademark of Bore-Warner Chemicals. Inc. •κ. BLFNDHX and WKSTON are registered trademarksof
Borg-Warner Chemicals. Inc.
(304)424-5411 BorgWarner Chemicals
Science
Bicyclic molecule collapses to hypervalent tricyclics
Amine phosphate
BF3-(CH3CH2)20 (CH3CH2)3SiCI04 (1 equivalent)
.Si(CH2CH3)3
ΪΗ,ΡΟ,
P-p'Qr
f"* H^J
p-K
Trifluoroboratooxy phosphatrane
(CH3CH2)3SiCl04
(CH3CH2)3Si + Si(CH2CH3)3
Ο
Verkade's explorations in this area are aimed at finding out to what extent phosphorus "wants to be hypervalent/ ' he tells C&EN. The collapse of the amine phosphate to the phosphatrane cage seems to be driven by two stabilizing forces, he says. One is the effect of chelating the phosphorus as part of a tricyclic skeleton. The other is the formation of the axial four-electron three-center (N-P-O) bond. In this bond, the two pairs of electrons occupy two sigma molecular orbitals—one bonding, the other nonbonding. The electron density in the nonbonding orbital is concentrated mainly on the apical atoms (ni trogen and phosphoryl oxygen), which also carry lone pairs. When the oxygen's lone pair is donated to a Lewis acid such as the triethylsilyl cation, the buildup of positive charge on the oxygen is believed to cause the nonbond ing orbital to contract, Verkade explains. This lowers the orbital's energy and stabilizes the phosphatrane.
In an effort to find out how general these stabilizing factors are, Verkade and his coworkers also are
Hydroxy phosphatrane cation/dihydrogen phosphate adduct
studying other hypervalent systems. They find, for example, that alkoxy silatranes (the silicon analogs of phosphatranes) appear to behave much like their phosphorus cousins in that their alkoxy oxygens can be protonated and silylated. Other researchers in Verkade's labs have used tetra-alcohols to chelate a hypervalent phosphorus atom. In these compounds, the oxygen tips of the molecule's four "arms" form a rectangular array in whose midst sits the chelated atom, which carries a fifth group perpendicular to the plane. The Iowa State workers have shown that such rigid molecular frameworks can stabilize phosphorus and perhaps other hypervalent atoms in a rectangular pyramidal environment.
"Whether these particular compounds end up being dinosaurs that sit on a shelf remains to be seen," Verkade comments. At the very least, they make fascinating, and research-provoking, signposts on the road to a clearer understanding of hypervalency and chemical bonding in general.
Ron Dagani, Washington CIRCLE 34 ON READER SERVICE CARD
18 December 9, 1985 C&EN