Five-coordinate aluminum bromides: Synthesis, structure, cation formation, and cleavage of phosphate ester bonds

Article abstract of DOI:10.1021/ja054684s

The alkane elimination reaction between Salen(^tBu)H₂ ligands and diethylaluminum bromide was used to prepare three Salen aluminum bromide compounds salen(^tBu)AlBr (1) (salen = N,N′-ethylenebis- (3,5-di-tert-butylsalicylideneimine)), salpen(^tBu)AlBr (2) (salpen = N,N′-propylenebis(3,5-di-tert-butylsalicylideneimine)), and salophen( ^tBu)AlBr (3) (salophen = N,N′-o-phenylenenebis(3,5-di-tert- butylsalicylideneimine)). The compounds contain five-coordinate aluminum either in a distorted square pyramidal or a trigonal bipyramidal environment. The bromide group in these compounds could be displaced by triphenylphosphine oxide or triphenyl phosphate to produce the six-coordinate cationic aluminum compounds [salen(^tBu)Al(Ph₃PO)₂]Br (4), [salpen( ^tBu)Al(Ph₃PO)₂]Br (5), [salophen( ^tBu)Al(Ph₃PO)₂]Br (6), and [salophen-( ^tBu)Al{(PhO)₃PO)}₂]Br (7). All the compounds were characterized by ¹H, ¹³C, ²⁷Al, and ³¹P NMR, IR, mass spectrometry, and melting point. Furthermore, compounds 1-3 and 5-7 were structurally characterized by single-crystal X-ray diffraction. Compounds 1-3 dealkylated a series of organophosphates in stoichiometric reactions by breaking the ester C-O bond. Also, they were catalytic in the dealkylation reaction between trimethyl phosphate and added boron tribromide.

Full text of DOI:10.1021/ja054684s

Published on Web 01/07/2006
Five-Coordinate Aluminum Bromides: Synthesis, Structure,
Cation Formation, and Cleavage of Phosphate Ester Bonds
Amitabha Mitra, Lauren J. DePue, Sean Parkin, and David A. Atwood*
Contribution from the Department of Chemistry, UniVersity of Kentucky,
Lexington, Kentucky 40506-0055
Received July 13, 2005; E-mail: datwood@uky.edu.
Abstract: The alkane elimination reaction between Salen(tBu)H2 ligands and diethylaluminum bromide was
used to prepare three Salen aluminum bromide compounds salen(tBu)AlBr (1) (salen ) N,N′-ethylenebis-
(3,5-di-tert-butylsalicylideneimine)), salpen(tBu)AlBr (2) (salpen ) N,N′-propylenebis(3,5-di-tert-butylsali-
cylideneimine)), and salophen(tBu)AlBr (3) (salophen ) N,N′-o-phenylenenebis(3,5-di-tert-butylsalicylide-
neimine)). The compounds contain five-coordinate aluminum either in a distorted square pyramidal or a
trigonal bipyramidal environment. The bromide group in these compounds could be displaced by
triphenylphosphine oxide or triphenyl phosphate to produce the six-coordinate cationic aluminum compounds
[salen(tBu)Al(Ph3PO)2]Br (4), [salpen(tBu)Al(Ph3PO)2]Br (5), [salophen(tBu)Al(Ph3PO)2]Br (6), and [salophen-
(tBu)Al{(PhO)3PO)}2]Br (7). All the compounds were characterized by 1H, 13C, 27Al, and 31P NMR, IR, mass
spectrometry, and melting point. Furthermore, compounds 1-3 and 5-7 were structurally characterized
by single-crystal X-ray diffraction. Compounds 1-3 dealkylated a series of organophosphates in
stoichiometric reactions by breaking the ester C-O bond. Also, they were catalytic in the dealkylation
reaction between trimethyl phosphate and added boron tribromide.
demand Diels-Alder reaction.8 The chloride group in Salen-
Introduction
(tBu)AlCl can be displaced by strong donors, such as, H2O,
Examples of five-coordinate group 13 bromide compounds
reported so far have been limited to indium.1 This is despite
the fact that the chloride compounds have been quite popular
for synthetic and catalytic applications.2-6 Specifically, Salen
aluminum chloride (Salen ) N,N′-alkylene(or arylene)bis-
(salicylideneimine)) compounds have been the subject of interest
recently for their ease of synthesis and cation formation and
subsequent catalysis. The compounds contain five-coordinate
aluminum with a single 27Al NMR peak in the range δ 43-57
ppm. The coordination environment around the central alumi-
num is either trigonal bipyramidal or square pyramidal depend-
ing on the “backbone” (the connection between the nitrogens)
of the ligand. With three or more methylene units in the
backbone (e.g., salpen) a tbp geometry is obtained whereas for
two methylene units (e.g., salen) or 1,2-arylene (e.g., salophen)
a sqp geometry is observed.7
MeOH, THF, or HMPA to give cationic aluminum compounds
(Scheme 1).9-11 Also, solvent-free cations can be achieved by
removing the chloride of SalenAlCl with GaCl3 (Scheme 1).12
In general, the utility of the SalenAlCl compounds has relied
on their ability to produce the cation [SalenAl(base)2]+. It is
likely that the bromide derivatives will have greater utility on
the basis of the weaker Al-Br bond strength (bond energy: 511
kJ mol-1 for Al-Cl vs 430 kJ mol-1 for Al-Br).13 Thus, it is
anticipated that cation formation may occur for the bromide
derivatives with less strong bases, thereby broadening the
potential applicability of the compounds.
This article will detail the synthesis of five-coordinate Salen
aluminum bromides and the formation of six-coordinate alu-
minum cations in combination with a Lewis base. Also, the
ability of these compounds to dealkylate organophosphate
compounds will be demonstrated.
SalenAlCl compounds have been used in oxirane polymer-
ization,2 phospho-transfer reactions,3 conjugate addition of
nucleophiles to unsaturated imides,4-6 and an inverse electron
Experimental Section
General Remarks. All air-sensitive manipulations were conducted
using standard benchtop Schlenk line technique in conjunction with
an inert-atmosphere glovebox. All solvents were rigorously dried prior
(1) Hill, M. S.; Atwood, D. A. Main Group Chem. 1998, 2, 191-202.
(2) Munoz-Hernandez, M.-A.; McKee, M. L.; Keizer, T. S.; Yearwood, B. C.;
Atwood, D. A. J. Chem. Soc., Dalton Trans. 2002, 3, 410-414.
(3) Duxbury, J. P.; Cawley, A.; Thornton-Pett, M.; Wantz, L.; Warne, J. N.
D.; Greatrex, R.; Brown, D.; Kee, T. P. Tetrahedron Lett. 1999, 40, 4403-
4406.
(4) Sammis, G. M.; Danjo, H. J.; Jacobsen, E. N. J. Am. Chem. Soc. 2004,
126, 9928-9929.
(5) Taylor, M. S.; Jacobsen, E. N. J. Am. Chem. Soc. 2003, 125, 11204-11205.
(6) Vanderwal, C. D.; Jacobsen, E. N. J. Am. Chem. Soc. 2004, 126, 14724-
14725.
(8) Magesh, C. J.; Makesh, S. V.; Perumal, P. T. Bioorg. Med. Chem. Lett.
2004, 14, 2035-2040.
(9) Atwood, D. A.; Jegier, J. A.; Rutherford, D. J. Am. Chem. Soc. 1995, 117,
6779-6780.
(10) Atwood, D. A.; Jegier, J. A.; Rutherford, D. Inorg. Chem. 1996, 35, 63-
70.
(11) Atwood, D. A. Coord. Chem. ReV. 1998, 176, 407-430.
(12) Munoz-Hernandez, M.-A.; Sannigrahi, B.; Atwood, D. A. J. Am. Chem.
Soc. 1999, 121, 6747-6748.
(7) Munoz-Hernandez, M.-A.; Keizer, T. S.; Wei, P.; Parkin, S.; Atwood, D.
A. Inorg. Chem. 2001, 40, 6782-6787.
(13) Kerr, J. A.; Stocker, D., W. In CRC Handbook of Chemsitry and Physics,
81st ed.; Lide, D. R., Ed.; CRC Press: Boca Raton, FL, 2000-2001.
9
10.1021/ja054684s CCC: $33.50 © 2006 American Chemical Society
J. AM. CHEM. SOC. 2006, 128, 1147-1153
1147

A R T I C L E S
Mitra et al.
of salpen(tBu)H2 (1.57 g, 3.10 mmol) in toluene by cannula. The
reaction mixture was refluxed for 17 h. The cloudy yellow solution
was concentrated under vacuum to about one-third of its volume. The
yellow precipitate was isolated by cannula filtration, washed with ∼15
mL of hexane, dried under vacuum, and recrystallized from toluene.
X-ray-quality crystals were grown from slow diffusion of hexane vapor
into a concentrated CH2Cl2 solution. Yield: 1.04 g (55%). Mp: 333-
Scheme 1. Formation of Cationic Aluminum Compounds with
Salen Ligands
1
334 °C (dec). H NMR (CDCl3): δ 1.30 (s, 18H, C(CH3)3), 1.50 (s,
18H, C(CH3)3), 2.23 (m, 2H, CH2CH2CH2), 3.85 (m, 4H, NCH2), 7.07
(d, 2H, Ph-H), 7.56 (d, 2H, Ph-H), 8.29 (s, 2H, NdCH). 13C NMR
(CDCl3): δ 27.2 (CH2), 29.7 (C(CH3)3), 31.3 (C(CH3)3), 33.9 (CCH3)3),
35.4 (CCH3)3), 55.1 (NCH2), 118.1 (Ph), 127.2 (Ph), 131.4 (Ph),138.9
(Ph), 141.0 (Ph), 162.5 (Ph), 172.0 (N)CH). 27Al NMR (CDCl3): δ
36 (W1/2 ) 3339 Hz). IR (KBr; ν in cm-1): 2956 m, 2906 w, 2866 w,
1642 s, 1624 s, 1548 m, 1463 s, 1418 m, 1390 w, 1361 m, 1312 m,
1259 m, 1180 m, 1097 w, 863 m, 847 m, 784 w, 755 w, 601 m. MS
(EI, positive): m/z 531 (M+ - Br, 100%).
to use. All glassware was cleaned with a base and an acid wash and
dried in an oven at 130 °C overnight. The ligands salen(tBu)H2,
salpen(tBu)H2, and salophen(tBu)H2 were synthesized according to the
literature procedure.14 NMR data were obtained on Varian Gemini-
200 and Varian VXR-400 instruments. Chemical shifts are reported
1
relative to SiMe4 for H and 13C and AlCl3 in D2O for 27Al and are
reported in ppm. Infrared transmission spectra were recorded at room
temperature in a potassium bromide pellet on a Fourier transform
Magna-IR ESP 560 spectrometer. The elemental analyses of the
compounds were within acceptable limits.
Synthesis of Salophen(tBu)AlBr (3). A rapidly stirred solution of
Et2AlBr in toluene, prepared in situ by the redistribution of triethyla-
luminum (0.21 g, 1.80 mmol) and aluminum(III) bromide (1 M solution
in dibromomethane 0.90 mL, 0.90 mmol), was combined with a solution
of salophen(tBu)H2 (1.46 g, 2.70 mmol) in toluene by cannula. The
golden yellow solution was refluxed for 15 h. Then it was concentrated
under vacuum to about one-third of its volume. Yellow crystals
precipitated after cooling at -30 °C for 24 h. The crystals were isolated
by cannula filtration, washed with hexane, and dried under vacuum.
Yield: 1.54 g (88%). Mp: 320 °C (dec). 1H NMR (CDCl3): δ 1.37 (s,
18H, C(CH3)3), 1.63 (s, 18H, C(CH3)3), 7.24 (d, 2H, Ph-H), 7.35 (m,
2H, Ph-H), 7.66 (m, 2H, Ph-H), 7.71 (d, 2H, Ph-H), 8.94 (s, 2H, Nd
CH). 13C NMR (CDCl3): δ 29.8 (C(CH3)3), 31.2 (C(CH3)3), 34.1
(C(CH3)3), 35.6 (C(CH3)3), 115.4 (Ph), 115.7 (Ph), 118.5 (Ph), 126.7
(Ph), 127.5 (Ph), 128.2 (Ph), 129.1 (Ph), 133.2 (Ph), 137.5 (Ph), 139.8
(Ph), 141.6 (Ph), 161.2 (Ph), 162.4 (Ph), 164.1 (NdCH). 27Al NMR
(CDCl3): δ 32 (W1/2 ) 5183 Hz). IR (KBR; ν in cm-1): 2961 s, 2905
w, 2868 w, 1621 s, 1554 m, 1542 s, 1469 s, 1474 m, 1445 m, 1420 m,
1391 m, 1361 s, 1311 m, 1255 m, 1202 w, 1179 w, 865 w, 847 m, 786
X-ray data were collected on either a Nonius Kappa-CCD (com-
pounds 2, 5-7; Mo KR radiation) or a Bruker-Nonius X8 Proteum
(compounds 1 and 3; Cu KR radiation) diffractometer. All calculations
were performed using the software package SHELXTL-Plus.15-18 The
structures were solved by direct methods and successive interpretation
of difference Fourier maps followed by least-squares refinement. All
non-hydrogen atoms were refined anisotropically. The hydrogen atoms
were included using a riding model with isotropic parameters tied to
the parent atom. Crystallographic data were deposited with the
Cambridge Crystallographic Data Center (CCDC reference nos.:
276666 (1); 276668 (2); 276667 (3); 276669 (5); 276670 (6); 276671-
(7)), and copies of the data can be obtained free of charge on application
to CCDC, 12 Union Road, Cambridge CB2 1EZ, U.K. (fax +44-1223-
336033; E-mail deposit@ccdc.cam.ac.uk).
Synthesis of Salen(tBu)AlBr (1). A rapidly stirred solution of Et2-
AlBr in toluene, prepared in situ by the redistribution of triethylalu-
minum (0.42 g, 3.60 mmol) and aluminum(III) bromide (1 M solution
in dibromomethane, 1.8 mL, 1.80 mmol), was combined with a solution
of salen(tBu)H2 (2.69 g, 5.46 mmol) in toluene by cannula. The reaction
mixture was refluxed for 8 h and filtered. The volatiles were removed
under vacuum from the clear yellow filtrate to give a yellow
microcrystalline solid which was purified by recrystallization from
toluene. Single crystals suitable for X-ray analysis were grown from
slow diffusion of hexane vapor into a concentrated CH2Cl2 solution.
Yield: 2.69 g (73.8%). Mp: 330-332 °C (dec). 1H NMR (CDCl3): δ
1.33 (s, 18H, C(CH3)3), 1.57 (s, 18H, C(CH3)3), 3.97 (m, 4H, NCH2),
7.08 (d, 2H, PhH), 7.60 (d, 2H, PhH), 8.40 (s, 2H, NdCH). 13C NMR
(CDCl3): δ 29.7 (C(CH3)3), 31.3 (C(CH3)3), 34.0 (CCH3)3), 35.5
(CCH3)3), 54.5 (NCH2), 118.2 (Ph), 127.3 (Ph), 131.6 (Ph), 139.1 (Ph),
141.3 (Ph), 162.7 (Ph), 170.4 (NCH). 27Al NMR (CDCl3): δ 38 (W1/2
) 5183 Hz). IR (KBr; ν in cm-1): 2962 m, 2905 w, 2866 w, 1648 s,
1628 s, 1544 m, 1475 m, 1444 m, 1421 w, 1390 w, 1361 w, 1310 w,
1257 w, 1180 w, 867 w, 845 m, 816 w, 786 w, 756 w, 608 m, 586 w.
MS (EI, positive): m/z 597 (M+, 8%), 517 (M+ - Br, 100%), 501
(M+ - Br - O, 44%).
w, 757 w, 610 m. MS (EI, positive): m/z 646 (M+, 13%), 565 (M+
Br, 95%), 549 (M+ - Br - O, 100%).
-
Synthesis of [Salen(tBu)Al(Ph3PO)2]Br (4). A rapidly stirred
solution of salen(tBu)AlBr (0.41 g, 0.69 mmol) in toluene was combined
with triphenylphosphine oxide (0.38 g, 1.38 mmol). The cloudy yellow
slurry became clear greenish yellow with heating. The solution was
refluxed for 16 h. A pale yellow precipitate formed after cooling to
room temperature. The precipitate was isolated by cannula filtration
and dried under vacuum. Yield: 0.77 g (97%). Mp: 260 °C. 1H NMR
(CDCl3): δ 1.31 (s, 18H, C(CH3)3), 1.42 (s, 18H, C(CH3)3), 3.67 (s,
br, 4H, NCH2), 6.86 (d, 2H, Ph-H), 7.29-7.54 (m, 32H, Ph-H), 8.04
(s, 2H, NdCH). 13C NMR (CDCl3): δ 29.8 (C(CH3)3), 31.4 (C(CH3)3),
33.9 (C(CH3)3), 35.5 (C(CH3)3), 53.3 (NCH2), 118.6 (Ph), 127.3 (Ph),
128.1 (Ph), 128.6 (Ph), 128.9 (Ph), 128.1 (Ph), 129.5 (Ph), 128.1 (Ph),
130.4 (Ph), 132.0 (Ph), 132.3 (Ph), 132.8 (Ph), 132.9 (Ph), 137.5 (Ph),
139.9 (Ph), 162.7 (Ph), 168.7 (NCH). 27Al NMR (CDCl3): δ -6 (W1/2
) 7859 Hz). 31P{1H} NMR (CDCl3): δ 34 (s). IR (KBr; ν in cm-1):
2951 s, 2901 w, 2862 w, 1621 s, 1547 w, 1439 m, 1422 w, 1391 w,
1358 w, 1258 w, 1173 s (νPdO), 1121 m, 856 w, 787 w, 757 w, 724 s,
694 m, 610 m, 539 s. MS (MALDI-TOF): m/z 795 (M+ - Br - Ph3-
PO, 100%), 517 (M+ - Br - 2Ph3PO, 36%).
Synthesis of Salpen(tBu)AlBr (2). A rapidly stirred solution of Et2-
AlBr in toluene, prepared in situ by the redistribution of triethylalu-
minum (0.24 g, 2.08 mmol) and aluminum(III) bromide (1 M solution
in dibromomethane, 1.0 mL, 1.00 mmol), was combined with a solution
Synthesis of [Salpen(tBu)Al(Ph3PO)2]Br (5). A rapidly stirred
solution of salpen(tBu)AlBr (0.32 g, 0.53 mmol) in toluene was
combined with triphenylphosphine oxide (0.29 g, 1.05 mmol). The
cloudy yellow slurry became clear yellow with heating. The solution
was refluxed for 10 h. A yellow precipitate formed after cooling to
room temperature and concentrating the solution. The precipitate was
isolated by cannula filtration and dried under vacuum. Yield: 0.42 g
(14) Rutherford, D.; Atwood, D. A. Organometallics 1996, 15, 4417-4422.
(15) Sheldrick, G. M., SHELXS97 and SHELXL97; University of Go¨ttingen:
Go¨ttingen, Germany, 1997.
(16) Sheldrick, G. M. SHELXTL-plus; Siemens Analytical X-ray Instruments,
Inc.: Madison, WI, 1997.
(17) Sheldrick, G. M. SHELXTL, version 5.0; Bruker AXS, Inc.: Madison, WI,
1998.
1
(69%). Mp: 246 °C. H NMR (CDCl3): δ 1.31 (s, 36H, C(CH3)3),
(18) Siemens R3m Software, version 4.0; Siemens Analytical X-ray Instruments,
Inc.: Madison, WI, 1990.
2.08 (m, 2H, CH2CH2CH2), 3.56 (m, 4H, NCH2), 7.05 (d, 2H, Ph-H),
9
1148 J. AM. CHEM. SOC. VOL. 128, NO. 4, 2006

Phosphate Dealkylation with Aluminum Bromides
A R T I C L E S
Scheme 2. Formation of Salen(tBu)AlBr Compounds
7.27-7.59 (m, 32H, Ph-H), 8.29 (s, 2H, NdCH). 13C NMR (CDCl3):
δ 27.2 (CH2), 29.9 (C(CH3)3), 31.6 (C(CH3)3), 34.2 (C(CH3)3), 35.5
(C(CH3)3), 56.6 (NCH2), 118.8 (Ph), 128.1 (Ph), 128.4 (Ph), 129.0 (Ph),
129.2 (Ph), 130.3 (Ph), 131.3 (Ph), 132.4 (Ph), 132.6 (Ph), 133.1 (Ph),
133.2 (Ph), 139.2 (Ph), 140.2 (Ph), 162.6 (Ph), 172.8 (NdCH). 27Al
NMR (CDCl3): δ 0 (W1/2 ) 4835 Hz). 31P{1H} NMR(CDCl3): δ 35
(s). IR (KBr; ν in cm-1): 2950 s, 2905 w, 2866 w, 1632 s, 1620 s,
1548 m, 1478 m 1461 m, 1439 s, 1426 s, 1391 w, 1358 m, 1316 m,
1279 w, 1255 m, 1200 w, 1162 s (νPdO), 1120 s, 1094 w, 999 w, 841
m, 786 w, 753 m, 726 s, 693 s, 537 s. MS (MALDI-TOF): m/z 809
(M+ - Br - Ph3PO, 11%), 531 (M+ - Br - 2Ph3PO, 100%).
Synthesis of [Salophen(tBu)Al(Ph3PO)2]Br (6). A rapidly stirred
solution of salophen(tBu)AlBr (0.51 g, 0.79 mmol) in toluene was
combined with triphenylphosphine oxide (0.44 g, 1.58 mmol). The
yellow slurry was refluxed for 14 h and then cooled to room temperature
and concentrated. Yellow crystals precipitated, which were isolated by
cannula filtration and dried under vacuum. Yield: 0.58 g (61%). Mp:
304-305 °C (dec). 1H NMR (CDCl3): δ 1.34 (s, 18H, C(CH3)3), 1.50
(s, 18H, C(CH3)3), 6.92 (d, 2H, Ph-H), 7.06-7.40 (m, 34H, Ph-H),
7.62 (d, 2H, Ph-H), 8.11 (s, 2H, NdCH). 13C NMR (CDCl3): δ 30.1
(C(CH3)3), 31.6 (C(CH3)3), 34.3 (C(CH3)3), 35.9 (C(CH3)3), 116.2 (Ph),
119.1 (Ph), 125.6 (Ph), 126.7 (Ph), 128.5 (Ph), 128.6 (Ph), 128.8 (Ph),
128.9 (Ph), 129.3 (Ph), 129.8 (Ph), 132.2 (Ph), 132.4 (Ph), 133.0 (Ph),
133.1 (Ph), 137.6 (Ph), 138.2 (Ph), 140.8 (Ph), 159.9 (Ph), 164.9
(N)CH); 27Al NMR (CDCl3): δ 42 (W1/2 ) 5078 Hz). 31P{1H} NMR-
(CDCl3): δ 33 (s). IR (KBr; ν in cm-1): 2954 s, 2901 w, 2862 w,
1614 s, 1586 s, 1547 m, 1536 s, 1469 m, 1440 m, 1413 w, 1391 m,
1357 w, 1266 w, 1199 m, 1172 s (νPdO), 1121 s, 847 w, 787 w, 757 w,
756 w, 726 s, 693 m, 602 w, 538 s. MS (MALDI-TOF): m/z 43 (M+
- Br - Ph3PO, 100%).
dealkylation was calculated from the peak integrations of methyl
bromide produced and unchanged phosphate.
Catalytic Dealkylation of Phosphate. In a typical experiment 15
mg (0.025 mmol) salen(tBu)AlBr was dissolved in 1 mL of CDCl3 in
a glass vial. The solution was transferred to an NMR tube in which
trimethyl phosphate (28.65 µL, 0.25 mmol, density 1.197 g/mL) and
boron tribromide (0.25 mL, 0.25 mmol, 1 M solution in hexane) were
1
added with a syringe. The mixture was shaken and monitored by H
NMR. The % dealkylation was calculated from the peak integrations
of methyl bromide produced and unchanged phosphate.
Results and Discussion
Salen Aluminum Bromides. Compounds 1-3 were prepared
by alkane elimination between diethyl aluminum bromide and
Salen(tBu)H2 under reflux (Scheme 2). The compounds were
isolated by removing the solvent under vacuum or by precipita-
tion after concentration and cooling to -30 °C. All three
compounds were soluble in chloroform. The 1H NMR data were
very close to the corresponding chloride analogues reported in
1
the literature.14 For example, the H NMR data for all three
t
compounds show two singlets for the Bu-Ph groups in the
range δ 1.30-1.63 ppm. For 1 and 2 there are multiple CH2
peaks corresponding to the alkylene backbone protons from the
ligand ranging from δ 2.23 to 3.97 ppm. There is only one imine
singlet for each compound at δ 8.40, 8.29, and 8.94 ppm,
respectively. Like their chloride analogues, these values decrease
slightly with increasing backbone length from 1 to 2 and increase
in 3 because of the greater electronegativity and deshielding
effect of the aryl backbone compared to an alkyl backbone. The
Synthesis of [Salophen(tBu)Al{(PhO)3PO)}2]Br (7). To a rapidly
stirred solution of salophen(tBu)AlBr (0.68 g, 1.05 mmol) in toluene
was added triphenyl phosphate (0.69 g, 2.11 mmol). The clear golden
yellow solution was stirred at room temperature for 17 h. Concentration
followed by slow evaporation at room temperature gave yellow crystals
which were cannula filtered, washed with hexane, and dried under
vacuum. Yield: 1.08 g (79%). Mp: 120-122 °C (dec). 1H NMR
(CDCl3): δ 140 (s, 18H, C(CH3)3), 6.81-7.60 (m, 38H, Ph-H), 7.62
(d, 2H, Ph-H), 8.43 (s, 2H, NdCH). 13C NMR (CDCl3): δ 30.0
(C(CH3)3), 31.6 (C(CH3)3), 34.4 (C(CH3)3), 35.9 (C(CH3)3), 116.0 (Ph),
118.6 (Ph), 119.7 (Ph), 119.8 (Ph), 125.5 (Ph), 126.2 (Ph), 128.4 (Ph),
128.6 (Ph), 129.2 (Ph), 130.1 (Ph), 132.8 (Ph), 137.5 (Ph), 139.0 (Ph),
141.3 (Ph), 149.9 (Ph), 150.0 (Ph), 161.5 (Ph), 164.3 (N)CH). 27Al
NMR (CDCl3): δ 12 (W1/2 ) 15053 Hz). 31P{1H} NMR(CDCl3): δ
-21 (s). IR (KBR; ν in cm-1): 2953 m, 2901 w, 2866 w, 1614 s,
1587 s, 1547 m, 1536 m, 1487 s, 1392 w, 1359 w, 1278 s (νPdO), 1266
m, 1220 w, 1184 vs, 1163 s, 1029 s ((νP-O), 1078 m, 983 s, 848 w,
783 w, 753 m, 726 s, 686 w, 610 w, 523 w. MS (MALDI-TOF): m/z
843 (M+ - Br - 2(PhO)3PO, 100%).
t
presence of only one set of Bu peaks and one imine peak for
each compound suggests a symmetric solution state structure.
The 27Al NMR showed broad single peaks centered at δ 38,
36, and 32 ppm, respectively, for 1-3 which indicate the
presence of five-coordinate aluminum. However, these are
shifted upfield from the related chloride analogues (δ 57, 43,
52 ppm, respectively).14 This is in accordance with the lower
electronegativity of Br compared to Cl and hence more shielding
of the Al center.
The mass spectra (EI) of 1 and 3 contained molecular ion
peaks in low abundance. All three compounds had a peak
corresponding to the molecular ion minus bromide, and for 1
and 2 this was the most abundant peak. Compounds 1 and 3
also had peaks corresponding to molecular ion minus bromide
and one oxygen, and for 3 this was the most abundant peak. It
was interesting to note that the loss of bromide occurred and
t
not the loss of Bu from the ligand. This might provide some
Dealkylation of Phosphates. In a typical experiment salen(tBu)-
AlBr (30 mg, 0.05 mmol) was dissolved in 1 mL of CDCl3 in a glass
vial. The solution was transferred to an NMR tube in which trimethyl
phosphate (1.96 µL, 0.017 mmol, density 1.197 g/mL) was added with
a syringe. The mixture was shaken and monitored by 1H NMR. The %
indication of the relative weakness of the Al-Br bond in the
compounds.
The X-ray crystal structures of 1-3 confirmed the presence
of five-coordinate aluminum atoms (Figures 1-3). The crystal
9
J. AM. CHEM. SOC. VOL. 128, NO. 4, 2006 1149

A R T I C L E S
Mitra et al.
Figure 4. τ diagram. τ ) (R - â)/60. R (c-e) and â (b-d) are the angles
opposite to each other in the xy plane, where a is along the z-axis. By
convention â is the most obtuse angle.
Table 1. τ Values of Salen Aluminum Halide Compounds
Figure 1. Crystal structure of salen(tBu)AlBr (1).
compd
τ
value
ref
salpen(tBu)AlCl
0.77
0.18
0.20
0.77
0.32
7
7
salomphen(tBu)AlCl
salen(tBu)AlBr (1)
salpen(tBu)AlBr (2)
salophen(tBu)AlBr (3)
this work
this work
this work
Scheme 3. Formation of Six-Coordinate Aluminum Cations from
Salen(tBu)AlBr Compounds
Figure 2. Crystal structure of salpen(tBu)AlBr (2). There are two molecules
in the asymmetric unit; only one is shown.
described five-coordinate Salen aluminum chloride compounds,
are listed. Compounds 1 and 3 have τ values close to 0 indicative
of a distorted sqp geometry, whereas 2 has a τ value close to 1
indicating a distorted tbp geometry. This value may be important
in determining the accessibility of a sixth coordination site.22
Six-Coordinate Aluminum Cations. Four cationic com-
pounds, [salen(tBu)Al(Ph3PO)2]Br (4), [salpen(tBu)Al(Ph3PO)2]-
Br (5), [salophen(tBu)Al(Ph3PO)2]Br (6), and [salophen(tBu)-
Al{(PhO)3PO)}2]Br (7), were formed by displacement of the
bromide from compounds 1-3 with either triphenylphosphine
oxide or triphenyl phosphate (Scheme 3). Similar cationic
compounds were formed previously from Salen(tBu)AlCl with
H2O, THF, or MeOH.2,23 Salen aluminum chlorides do not form
cations with triphenylphosphine oxide, which confirms the value
of the SalenAlBr compounds in making new cations. Tri-
phenylphosphine oxide was also found to form [Me2Al-
(OPPh3)2]Br from Me2AlBr.24 However, it was not a strong
enough base to displace chloride from Me2AlCl even under
reflux. Instead, the adduct Me2AlCl‚OPPh3 formed.
Figure 3. Crystal structure of salophen(tBu)AlBr (3).
data collection parameters are listed in Supporting Information
Table S1, and selected bond lengths and angles in Table S2.
The Al-Br bond lengths fall in the range 2.35-2.36 Å, which
are longer than the Al-Cl bond length (∼2.18 Å) in Salen-
(tBu)AlCl compounds.7 The Al-N bond lengths (∼1.96-2.02
Å) are marginally longer than the Al-O bond lengths (∼1.76-
1.81 Å). The geometries of these compounds are close to either
square pyramidal or trigonal bipyramidal depending on the
ligand backbone. Salen and salophen have rigid backbones and
favor a square pyramidal geometry, while salpen with a longer,
flexible, propylene backbone favors a tbp geometry around the
aluminum. A similar trend was observed previously in the case
of Salen aluminum alkyl, chloride, and siloxide compounds.7,19,20
A quantitative measure, expressed as the “τ value”, can be
used to describe the distortion from perfectly sqp or tbp
geometry in these compounds (Figure 4).21 A perfectly sqp
geometry has a τ value equal to zero whereas a perfectly tbp
geometry has a τ value equal to 1. In Table 1 the calculated τ
values for compounds 1-3, along with some previously
1
The H NMR spectra of 4, 6, and 7 show two peaks for the
tBu groups of the ligand with each peak corresponding to 18
protons. Interestingly, for 5, there is only one tBu peak with 36
protons. This could be attributed to the shielding of the ortho-
(19) Atwood, D. A.; Hill, M. S.; Jegier, J. A.; Rutherford, D. Organometallics
1997, 16, 2659-2664.
(20) Dzugan, S. J.; Goedken, V. L. Inorg. Chem. 1986, 15, 2858-2864.
(21) Addison, A. W.; Rao, T. N.; Reedijk, J.; Van Rijn, J.; Verschoor, G. C. J.
Chem. Soc., Dalton Trans. 1984, 1349-1356.
(22) El-Bahraoui, J.; Wiest, O.; Feichtinger, D.; Plattner, D. A. Angew. Chem.,
Int. Ed. 2001, 40, 2073-2076.
(23) Jegier, J. A.; Munoz-Hernandez, M.-A.; Atwood, D. A. J. Chem. Soc.,
Dalton Trans. 1999, 15, 2583-2587.
(24) Jegier, J. A.; Atwood, D. A. Inorg. Chem. 1997, 36, 2034-2039.
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1150 J. AM. CHEM. SOC. VOL. 128, NO. 4, 2006

Phosphate Dealkylation with Aluminum Bromides
A R T I C L E S
tBu group of the ligand due to the ring current of the phenyl
groups of triphenylphosphine oxide. This shielding causes an
upfield shift of the tBu group thus superimposing it on the peak
of the other.25 In the aromatic regions there are overlapping
peaks due to the phenyl groups from both the ligands and
triphenylphosphine oxide or triphenyl phosphate. The 27Al NMR
shows very broad peaks at δ -6, 0, and 12 ppm for 4, 5, and
7, respectively. These correspond to the presence of six-
coordinate aluminum.26 However, for 6 this value is δ 42 ppm,
which is more likely to be the shift of a five-coordinate
aluminum atom.14 Thus, the solution product for 6 appears to
be different from the solid-state structure found in the X-ray
crystal studies where the aluminum atom is six-coordinate (see
next paragraph). One possible explanation could be that one of
the two loosely bound triphenylphosphine oxide ligands dis-
sociates in the polar NMR solvent (CDCl3) making the
aluminum five-coordinate. The 31P NMR spectra of 4-6 show
peaks at δ 34, 35, and 33 ppm, respectively. These are downfield
from the NMR shift of δ 29 ppm of free triphenylphosphine
oxide27 because of deshielding of the phosphorus due to
coordination of the phosphoryl group with aluminum. However,
for 7 this shift is δ -21 ppm which is slightly upfield from the
shift of -18 ppm of free triphenyl phosphate.27 The IR spectrum
shows strong PdO absorption at 1173, 1162, 1172, and 1278
cm-1 for 4-7, respectively. For 7, the stretching of the P-O
bond of the P-O-C linkage of the phosphate gives rise to a
strong band at 1029 cm-1. In the mass spectra (EI) of the six-
coordinate aluminum compounds no parent ion or parent ion
minus bromide ion was observed. However, all the compounds
show peaks corresponding to parent ion minus the bromide and
two triphenylphosphine oxide or triphenyl phosphate moieties
in high abundance. This indicates the weak coordination between
the Lewis base and the aluminum.
Figure 5. Crystal structure of [salpen(tBu)Al(Ph3P(O)2]Br (5).
Compounds 5-7 were structurally characterized by single-
crystal X-ray diffraction. The data collection parameters are
contained in Supporting Information Table S3, while Table S4
lists selected bond lengths and angles. Their structures consist
of a central six-coordinate aluminum atom in a distorted
octahedral geometry (Figures 5-7). The ligand occupies four
equatorial positions, and two phosphine oxide or phosphate
molecules occupy the two axial positions. The equatorial bond
angle is larger for O-Al-O (∼89.38-96.1°) compared to
N-Al-N (∼80.7-90.85°). This is a reflection of the steric
restrictions of the ligand creating a more “open” front for the
compound. The axial O-Al-O bond angles are distorted
(∼169.1-174.6°) from ideal linearity. The amount of distortion
is more for the phosphine oxide compounds 5 and 6 compared
to the phosphate compound 7. This is probably due to the fact
that the P-O-Ar linkage in 7 allows the bulky phenyl group
to move away from the equatorial ligand atoms and thus avoid
steric congestion. The axial Al-O distances (∼1.92-1.97 Å)
are longer than the equatorial Al-O distances (∼1.79-1.84)
due to the greater steric requirements of the axial groups.
Dealkylation of Organophosphates. Organophosphate esters
are found in both nerve gas agents and pesticides. The breaking
of the P-O-C linkages may be a means of deactivating these
toxic agents.28,29 Although extensive research is being carried
Figure 6. Crystal structure of [salophen(tBu)Al(Ph3PO)2]Br (6).
out on phosphate ester cleavage using various metal compounds
in models of biological phosphate hydrolysis,30-32 the use
of group 13 compounds in this field is limited. For example,
some phosphate cleavage has been achieved with organo-
aluminum reagents33 and aluminum or gallium amides.34-36
However, these reagents have not been considered as potential
nerve agent or pesticide decontamination reagents, probably due
to their limited scope or the high temperature and the long
reaction time required. Recently the use of boron-Schiff base
halides has shown promise for the catalytic cleavage of various
organophosphates at room temperature, opening the possibility
(28) Yang, Y.-C. Acc. Chem. Res. 1999, 32, 109-115.
(29) Yang, Y. C.; Baker, J. A.; Ward, J. R. Chem. ReV. 1992, 92, 1729-1743.
(30) Chin, J. Curr. Opin. Chem. Biol. 1997, 1, 514-521.
(31) Bashkin, J. K. Curr. Opin. Chem. Biol. 1999, 3, 752-758.
(32) Blasko, A.; Bruice, T. C. Acc. Chem. Res. 1999, 32, 475-484.
(33) Kitagawa, Y.; Hashimoto, S.; Iemura, S.; Yamamoto, H.; Nozaki, H. J.
Am. Chem. Soc. 1976, 98, 5030-5031.
(34) Pinkas, J.; Wessel, H.; Yang, Y.; Montero, M. L.; Noltemeyer, M.; Froeba,
M.; Roesky, H. W. Inorg. Chem. 1998, 37, 2450-2457.
(25) Atwood, D. A.; Rutherford, D. Organometallics 1995, 14, 3988-3995.
(26) Wang, Y.; Parkin, S.; Atwood, D. Inorg. Chem. 2002, 41, 558-565.
(27) Corbridge, D. E. C. Phosphorus: An Outline of its Chemistry, Biochemistry
and Technology, 5th ed.; Elsevier: Amsterdam, 1995; Vol. 6.
(35) Pinkas, J.; Chakraborty, D.; Yang, Y.; Murugavel, R.; Noltemeyer, M.;
Roesky, H. W. Organometallics 1999, 18, 523-528.
(36) Pinkas, J.; Loebl, J.; Dastych, D.; Necas, M.; Roesky, H. W. Inorg. Chem.
2002, 41, 6914-6918.
9
J. AM. CHEM. SOC. VOL. 128, NO. 4, 2006 1151

A R T I C L E S
Mitra et al.
Table 2. Dealkylation (%)a of Organophosphates with Compounds
1-3
1
2
3
time
TMP
TEP
14
TBP
TMP
TEP
75
TBP
TMP
TEP
TBP
30 min
2 h
4 h
6 h
8 h
10 h
12 h
24 h
64
79
89
91
93
95
96
96
12
35
44
44
56
58
62
67
69
7
18
30
40
46
58
64
69
85
7
100
100
100 100
100 100
a Calculated from the integration of 1H NMR spectra of methyl bromide
produced and unchanged trimethyl phosphate at room temperature in CDCl3.
In CD3OD after 24 h 1 showed no dealkylation while 2 and 3 had 4% and
3% dealkylation, respectively. Salen(tBu)AlCl showed 55% dealkylation
of TMP in CDCl3 after 24 h. TMP ) trimethyl phosphate, TEP ) triethyl
phosphate, and TBP ) tributyl phosphate.
Table 3. Catalytic Dealkylation (%) of Trimethyl Phosphate (TMP)
with Salen(tBu)AlBr Compoundsa
1
+
TMP
+
2
+
TMP
+
3
+
TMP
+
TMP +
time
BBr3 (1:10:10)
BBr3 (1:10:10)
BBr3 (1:10:10)
BBr3 (1:1)
Figure 7. Crystal structure of [salophen(tBu)Al{(PhO)3PO2}]Br (7).
30 min
2 h
6 h
88
100
100
100
78
92
100
100
82
84
95
95
58
67
67
81
Scheme 4 Plausible Dealkylation Pathway of Organophosphates
with Salen((tBu)AlBr Compounds
24 h
a Calculated from the integration of 1H NMR spectra of methyl bromide
produced and unchanged trimethyl phosphate at room temperature in CDCl3.
30 min for tributyl phosphate, as opposed to only 30%
conversion for trimethyl phosphate after 2 h.
Previously, it was shown that Salen(tBu)AlCl compounds
readily formed cations through the replacement of chloride by
a donor ligand like THF, MeOH, or H2O.2,9,11,23,40,41 Cation
formation should be more favorable for the Salen bromide
compounds because bromide is a better leaving group due to
the weaker Al-Br bond (bond energy: 430 kJ mol-1 for Al-
Br vs 511 kJ mol-1 for Al-Cl). As noted previously in this
work, cations are readily formed when SalenAlBr compounds
are combined with triphenylphosphine oxide and triphenyl
phosphate. Cation formation was also observed for Salen boron
bromide compounds with THF.39 Thus, it is likely that
compounds 1-3 form cations through coordination of the Lewis
basic phosphate to the aluminum with displacement of the
bromide anion. This activates the R-carbon of the phosphate
for nucleophilic attack of the bromide (Scheme 4). A similar
activation of an ester carbon due to coordination of the
phosphoryl oxygen to a cationic center was reported before.42
The cation formation is followed by attack of the bromide on
the methyl group and elimination of methyl bromide. Ultimately,
all three ester bonds are cleaved to produce an unidentified
phosphate material “[(SalenAlO)3PO]”. This mechanism is
supported by the following observations:
of finding a soft, chemical, catalytic means of destroying nerve
gas agents and pesticides.37-39
Compounds salen(tBu)AlBr (1), salpen(tBu)AlBr (2), and
salophen(tBu)AlBr (3) dealkylated a series of organophosphate
compounds at room temperature to produce methyl bromide and
an unidentified aluminum phosphate compound that remained
in solution (Scheme 4). The dealkylation reaction was carried
out in an NMR tube in CDCl3. The percent conversion was
calculated from the integration of the remaining phosphate and
the methyl bromide produced (Table 2). The percent dealkyl-
ation was comparable to the binuclear boron Salen bromide
compounds Salen(tBu)[BBr2]2 reported before.37-39 For trimethyl
phosphate, compound 1, having an ethylene backbone, showed
greater dealkylation compared to 2 which has a propylene
backbone and 3 which has an aromatic backbone. For example,
with 1 the dealkylation was 89% complete in just 4 h and 96%
complete after 12 h. However, the difference in Salen ligand
backbone does not seem to affect the dealkylation of longer
chain phosphates. Another interesting observation is that the
percent dealkylation was greater for longer chain phosphates
compared to those with shorter chains. For example, with 2,
dealkylation was complete in 2 h for triethyl phosphate and in
(i) There is little dealkylation in CD3OD (Table 2). Methanol
is a stronger Lewis base than trimethyl phosphate, and although
a cation is formed,23 the phosphate cannot replace the CD3OD
to become activated. (ii) The dealkylation with salen(tBu)AlCl
(55% after 24 h, Table 2) is much less compared to the bromide
(37) Keizer, T. S.; De Pue, L. J.; Parkin, S.; Atwood, D. A. J. Organomet. Chem.
2003, 666, 103-109.
(40) Munoz-Hernandez, M.-A.; Parkin, S.; Yearwood, B.; Wei, P.; Atwood, D.
A. J. Chem. Crystallogr. 2000, 30, 215-218.
(38) Keizer, T. S.; De Pue, L. J.; Parkin, S.; Atwood, D. A. Can. J. Chem.
2002, 80, 1463-1468.
(41) Liu, S.; Munoz-Hernandez, M.-A.; Atwood, D. A. J. Organomet. Chem.
2000, 596, 109-114.
(39) Keizer, T. S.; De Pue, L. J.; Parkin, S.; Atwood, D. A. J. Am. Chem. Soc.
2002, 124, 1864-1865.
(42) Albanese, D.; Landini, D.; Maia, A. J. Org. Chem. 2001, 66, 3249-3252.
(43) Lum, R. C.; Grabowski, J. J. J. Am. Chem. Soc. 1992, 114, 8619-8627.
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1152 J. AM. CHEM. SOC. VOL. 128, NO. 4, 2006

Phosphate Dealkylation with Aluminum Bromides
A R T I C L E S
analogue. The Al-Cl bond is stronger than Al-Br bond, which
impedes the replacement of chloride with the phosphate and
hence the required cation formation. (iii) The triphenyl phos-
phate coordinated cationic compound 7 was structurally char-
acterized. Salen aluminum halide compounds do not dealkylate
triphenyl phosphate. No dealkylation was also found with Salen
boron bromide compounds.39 The reaction stops at the formation
of the phosphate coordinated cation. (iv) The postulate that the
bromide attacks the ester carbon instead of the phosphorus is
in agreement with the previous findings that, for cleavage of
phosphate esters in solution, nucleophiles with a high charge
density, such as, hydroxides and alkoxides, preferentially attack
the phosphorus whereas more polarizable nucleophiles such as
bromide or iodides attack the carbon.42,43
The dealkylation reaction with the Salen(tBu)AlBr compounds
was found to be catalytic in the presence of excess BBr3 (Table
3). With BBr3 only, the dealkylation of trimethyl phosphate is
low. However, compounds 1-3 in only 10 mol % with BBr3
dramatically increased the dealkylation. For example, with 1
the reaction was 100% complete within only 2 h. Although
detailed mechanistic studies are still under progress, it is likely
that BBr3 regenerates the Salen aluminum bromide compound
from the dealkylated phosphate material allowing the repetition
of the catalytic cycle.
readily formed six-coordinate aluminum cations when combined
with triphenylphosphine oxide or triphenyl phosphate. The
Salen(tBu)AlBr compounds dealkylated a series of trialkyl
phosphates in high percent conversion, and the reaction was
catalytic in the presence of excess boron tribromide. The
phosphates used in this study could be envisioned as model
compounds for organophosphate chemical warfare agents and
pesticides. Thus, the compounds could be developed into
potential nerve gas and pesticide decontamination agents.
Attempts to experimentally prove the proposed mechanistic
pathway and isolation and full characterization of the dealkylated
products are in progress and will be published in due course.
Acknowledgment. This work was supported by the Kentucky
Science and Engineering Foundation (KSEF Grant 148-502-
04-100). Instruments used in this research were obtained from
the CRIF (NMR, Grant CHE 997841) and MRI (X-ray, Grant
CHE 0319176) programs of the National Science Foundation
and from the Research Challenge Trust Fund of the University
of Kentucky. Partial support from the University of Kentucky
Tracy Farmer Center for the Environment is acknowledged.
Supporting Information Available: Crystal data collection
parameters (Tables S1 and S3), selected bond lengths and angles
(Tables S2 and S4), and CIF files for compounds 1-7. This
material is available free of charge via the Internet at
http://pubs.acs.org.
Conclusion
Three new five-coordinate aluminum bromides salen(tBu)-
AlBr (1), salpen(tBu)AlBr (2), and salophen(tBu)AlBr (3) have
been synthesized and fully characterized. These compounds
JA054684S
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J. AM. CHEM. SOC. VOL. 128, NO. 4, 2006 1153