Synthesis and Study of Asymmetrically Layered Zirconium

Chapter 13

Synthesis and Study of Asymmetrically Layered Zirconium Phosphonates 1

David A. Burwell and Mark E. Thompson

Downloaded by UNIV OF GUELPH LIBRARY on August 6, 2012 | http://pubs.acs.org Publication Date: July 14, 1992 | doi: 10.1021/bk-1992-0499.ch013

Department of Chemistry, Princeton University, Princeton, NJ 08544

Zr(O PCH CH COOH) (O ΡOΗ) •0.5Η O, Zr-COOH-OH, and Zr(O PCH CH COOH) (O PH) •0.5H O, Zr-COOH-H, were prepared by the reaction of ZrOCl with a mixture of (EtO) P(O)CH CH COOH and either phosphoric or phosphorous acid in the presence of HF. Zr-COOH-OH forms as a single phase material with an interlayer spacing of 13.8 Å. This phase has not been reported previously. Both Zr-COOH-OH and Zr-COOH-H react with thionyl chloride to give partial conversion of the carboxylic add groups to acyl chlorides. These acyl chloride derivatives react readily with amines and alcohols to give amides and esters, respectively. 3

2

2

3

1.5

2

3

0.5

2

1.25

2

3

0.75

2

2

2

2

2

Intercalation of layered inorganic solids has been employed over the years to alter both the bulk physical properties and chemical reactivity of materials (7). Only recently, however, have investigators begun to take advantage of the 2-dimensionallyordered framework of intercalation hosts to construct new materials with imposed solid-state structures. Some unique applications of this concept include the use of layered solids to assemble molecular multilayers at solid-liquid interfaces (2), study quantum-sized semiconductor particles (5), modify electrode surfaces (4), and prepare low-dimensional conducting polymers (5). In addition to these applications, layered solids continue to be investigated for uses in ion exchange (6) and catalysis (7). In 1978, Alberti et at. reported the synthesis of a new class of layered metal phosphonates, M (O^PR) (#). These compounds crystallize with layered structures similar to that of a-Zr(O^FOH)2 H20 (a-ZrP). Each layer consists of a plane of metal atoms linked together by phosphonate groups. The metal atoms are octahedrally coordinated by oxygen atoms, with the three oxygens of each phosphonate tetrahedron IY

2

#

1

Corresponding author

0097-6156/92/0499-0166S06.00/0 © 1992 American Chemical Society

In Supramolecular Architecture; Bein, T.; ACS Symposium Series; American Chemical Society: Washington, DC, 1992.

13. BURWELL & THOMPSON

Asymmetrically Layered Zr Phosphonates

bound to three different metal atoms. This arrangement forces the organic groups to lie above and below the inorganic layer. The synthesis of these layered materials was extended by Dines and coworkers to include a wide range of organic functional groups such as ZitO^PC H ) and Zr(0 P(CH2) X)2 (where η = 1 - 5; X = H , Cl, SH, SEt, OH, COOH, SO3H, OC^L ) (9). Excellent reviews on the structure, properties, and applications of layered phosphonates have appeared recently (10). With few exceptions, intercalation of organic guest molecules into inorganic hosts has been promoted by only three types of reaction: acid-base, ion-exchange and redox. However, with the variety of reactive groups available in layered group 4 metal phosphonates, it should be possible to promote intercalation using organic reactions of those groups. To this end, we have very recently reported the syntheses of amides and esters from an acyl chloride zirconium phosphonate (77). These new materials are well ordered, thermally stable and easily characterized. Our first step in the preparation of new layered metal phosphonates from Zr(03PŒ CT2COOH) is the synthesis of an acyl chloride derivative, Ζφ Ρ€Η CHoCOa) (72). Z r ( < ^ F O T 2 ) 2 is layered with an interlayer spacing ca. 0.6 A larger than the starting acid. It reacts readily with amines and alcohols to give layered amides and esters, Eq. 1 (77). The structures of these new layered materials are similar to those obtained by amine intercalation of α-ZrP and Zr(0 PCH CH COOH^ except that the guest is held in the interlayer space by a covalent bond rather than an electrostatic one. 6

5

2

3

11


5

2

2

3

2

2

O T

3

Zr(O^PCH CH COa)2 + 2HXR 2

2

c o c l

2

2

Zr(0 PCH CH COXR) + 2HC1

2

3

2

2

2

X = NH, O; R = w-alkyl group

Amide compounds with alkyl chains ranging in length from 1 to 18 carbons have been prepared. The interlayer spacing regularly increases, at increments consis tent with a 59° angle between the alkyl chain and the surface of the host (Figure 1) (77). This angle is close to that seen for amine intercalation into both α-Zr and Zr(05PCH CH COOH) (56° and 53°, respectively) (IS). IR data suggest that the amides engage in trans-typo hydrogen bonding, as shown in Figure 2. The covalent bonding in amide and ester compounds leads to added thermal and chemical stability, as compared to materials prepared by Bronsted acid-base reactions. For example, Zr(C^PCH CH CONHC6H 3) shows the onset of its major weight loss ca. 200°C higher than Zr(O^PŒ CH COO-) (Ç H 3NHb ) . The amide is also significantly less susceptible to hydrolysis. After five days at 60°C in 3 M HC1 only 10% of the amide groups are hydrolyzed, while the same conditions convert the ammonium carboxylate compounds completely to the acid in less than three hours. In the preparation of 2^C>3PCH CH CC)Q) we found it necessary to first intercalate Z r i O ^ F Œ 2 ) 2 with amine, giving the carboxylate salt, and then react the salt with SOCl . The directreactionof ZÔ^PO^CT^COOHfe with SOCI2 does not lead to measurable conversion of the acid groups to acyl chlorides. A possible explanation for this is that the interlayerregionis so tightly packed that SOCl 2

2

2

2

2

1

2

+

2

2

2

O T

C O O H

2

2

2

6

1

2

2

3 1 1

2

2


168

SUPRAMOLECULAR ARCHITECTURE


60

10 H 0

'

1

4

'

1

8

«

1

12

•

1

16

«

1 20

Number of Carbons Figure 1. Plot of amide interlayer spacing versus number of carbons in alkyl chain.

Figure 2. Schematic drawing of amide intralayer hydrogen bonding.

can not diffuse into the solid to react. If this is the case, making the material more porous should increase its rate of reaction with SOCI2. With this idea in mind we have examined the chemistry of mixed component phosphonate-phosphate and phosphonate-phosphite compounds. The structures exhibited by these materials should be more porous than the pure phosphonates. We report herein the synthesis and characterization of mixed component carboxylic acids, acyl chlorides, amides and esters.


13.

Asymmetrically Layered Zr Phosphonates 169

BURWELL & THOMPSON

Results and Discussion


An alternative to amine pre-intercalation for converting pendant carboxylic acids to acyl halides involves the use of mixed component zirconium phosphonatephosphate or phosphonate-phosphite compounds. While crystal structures have not been determined, it has been proposed that these materials are composed of asymmet rical α-type layers (14). That is, the inorganic portion of the layers, 7i{0^-)2, is structurally similar to that of α-ZrP, but bound to the phosphorus are two different pendant groups (Figure 3a). Asymmetrically-layered zirconium phosphonates have previously been reported by Dines et al. (15), Alberti and co-workers (16), and Clearfield (17).

H

H

H

ÔÔ

ÔÔ

On O'O

ο' ο ι 0^0

ô

0^0

p' ο H B o*ô

ο' ο oô

oô

o^Q

y

H

OOOH

H,

H

0

0^0

0

ι

H

H

0^0

\ \ \\

ι

ο ο I

H

Ο ο

0

ο' ο

0

H

(a)

(b)

Figure 3. Schematic drawings of (a) Zr(0 PCH CH CX)OH) (O POH) ·0.5Άρ ZrC0 PCH a^COOH) ^ ^ P H ^ - O ^ O . 3

3

2

2

2

15

3

05

and (b)

1

The use of mixed component systems to prepare acyl chloride derivatives offers two potential advantages over analogous single component materials. First, substitution of the relatively large phosphonate groups with relatively small phosphate or phosphite groups may produce somewhat porous materials. This would allow a chlorinating agent easier access to carboxylic acid sites in the interior of the crystal lites. Second, a marked decrease in total interlayer bonding is expected, as compared to the pure phosphonate phase, due to the lower concentration of hydrogen bonding carboxylic acid groups on the lamellar surfaces. Here we assume that the phosphate and phosphite groups in the mixed systems are similar to those found in α-ZrP and Zr((>3PH)2, respectively, where they do not participate in interlayer hydrogen bonding (18). The diminished interlayer bonding reduces the amount of energy required to spread the layers and, therefore, increases the likelihood of reaction. The combination of these effects could, in theory, alleviate the need for ammonia intercalation prior to




170

reaction with SOCI2 in our effort to prepare acyl chloride derivatives. Moreover, an acyl chloride prepared from a mixed material similar to that shown in Figure 3a, may lead to new porous phosphate compounds in which amide or ester groups act as pillars. A mixed component material can take on several distinct architectures. In one structure type, each surface of the host lamellae contains a mixture of two different pendant groups, as shown for example in Figure 3a The observed interlayer spacing in this material is typically close to that for the pure phase of the largest pendant group (e.g., Zr(O^PCH2CH2COCe)2 in Figure 3a). In a second type of structure, one face of each lamella contains predominantly one pendant group, while the opposite face contains predominantly the other pendant group (Figure 3b). Here the repeat distance perpendicular to the layers is close to the sum of the interlayer spacings for the single-component phases (e.g., Ζ π ^ Ρ Ο Η ^ CH COOH) and ZriO^PH^ in Figure 3b) (10a). This structure type is commonly observed when the two pendant groups are chemically very different (e.g., hydro phobic and hydrophilic) (16). Lastly, a mixed material may be composed of large regions which contain only one of the pendant groups, i.e., the components are phase separated. In this instance, two phases will be observed, with interlayer spacings close to those for the single-component compounds. To further investigate the reactivity of layered carboxylic acids, we prepared the mixed component systems Zr(03PŒ2Œ COOH)2^ (03POH) *yH20 (ZrCOOH-OH) and Zr(03PCH2CH2C00H)2_ (C^PH) *yH20 (Zr-COOH-H). The interlayer spacings of these compounds, along with others prepared in this study, are given in the following table. 2

2

2

x

x

x

x

Table. Interlayer spacings of compounds prepared in this study. Compound

d (Â)

2Χ0 ΡΟΗ) ·Η 0 3

2

7.6

2

Zr(0 Pa^CH COOH) Zr(0 PCH CH COa) Zr(03ÏOâ^COOH) ^(0 POH) ^«05H 0

12.9 135 13.8

^ P O ^ a ^ C ^ J ^ ^ ^ K X ^ ^KÔ^œO^j^FH^^-OÔ Zr^FC^CH,^

25.0 19.6Î 31.8Î

3

3

2

2

2

2

2

1

^Knp^cioyoc^),

3

()

^Ο ΡΗ) 3

2

28.5T

0 7 5

t predominant phase 4 4

Zr-COOH-OH was prepared by precipitating Z r with an aqueous solution equimolarh2-carboxyethy^ The powder x-ray diffraction (XRD) pattern of Zr-COOH-OH exhibits three orders of sharp (001) reflections corresponding to an average interlayer spacing of 13.8 Â. The singlecomponent analogs of the individual components in Zr-COOH-OH, i.e., Zr(C^PCH2CH2COOH)2 and α-ZrP, have interlayer spacings of 12.9 Â and 7.6 Â, respectively (19). Since no other reflections are seen in the powder X R D pattern at




Bragg angles corresponding to repeat distances larger than 4.4 Â, it appears that a single, regularly-spaced phase containing layers of a fixed percentage of each component is likely (Figure 3a). Spectroscopic data suggest that Zr-COOH-OH is very similar to Zi^C^PCH CH COOH)2. The O O stretch in the IR spectrum of Zr-COOH-OH appears at 1701 cm- , as compared to 1700 cm- for Zit03PCT CH COOH)2. The C crosspolarized (CP) magic angle spinning (MAS) NMR spectra of these two compounds are essentially identical. Both exhibit carbonyl isotropic chemical shifts at 180.0 ppm and broad resonances in the methylene region. The P MAS NMR spectrum of ZrCOOH-OH clearly shows the presence of two different phosphorus groups. The phosphonate resonance is a broad peak centered at 9.2 ppm, while that of the phosphate is much sharper and falls at -22.1 ppm. The broadening of the phosphonate peak is probably due to a dispersion of local electronic environments (Le., static disorder), while the sharp phosphate peak suggests that all the phosphate groups have similar environments. The thermogravimetric analysis (TGA) of Zr-COOH-OH closely resembles that of Zr(03PCH CH COOH) and supports a stoichiometry of Zr(0 PCH CH COOH) (H20 are 10.1% C and 2.3% H. We believe the carbon value is low due to the trapping of organic pyrolysis products in the inorganic matrix; these products are only slowly lost at high temperature. Our TGA experiment shows that ca. 50% of the weight loss observed for Zr-COOH-OH is lost between 600° and 1100°C. In the short burning time used for flash combustion C, Η, Ν analysis (i.e., < 30 sec), a significant amount of the carbonaceous material presumably remains trapped in the inorganic matrix. Other investigators have also encountered this problem with elemental analyses of layered metal phosphonates (16). For this reason, we regard our thermal analysis data as a more accurate measure of composition when the TGA is run under an oxygen atmosphere. Taken together, the above data suggest that Zr-COOH-OH is somewhat different than the mixed component systems reported by Alberti and co-workers. Albert! et al. reported a compound formulated as Zr(0^rKH Œ CœHXO^PΟΗ)·Η2θ with an average interlayer spacing of 129 Â (16) — identical to that of Z r ( ( ^ P Œ Œ C O O H ) . Subsequently, Alberti et al. reported a series of mixed compounds, Zr(O PCH2CH2COOH)2 _ (0^POH) , with χ ranging from 0.9 to 1.2 and interlayer spacings ranging from 9.8 Â to 10.2 Â (20). Zr-COOH-H was prepared by precipitating Z r with an aqueous solution of a 2:1 molar ratio of phosphorous acid and 2-cWboxyethylphosphonic acid The powder XRD pattern of this material contains reflections from three distinct phases. The interlayer spacings of these phases are: 19.6,12.7 and 6.5 Â. The 12.7 Â phase likely contains mostly phosphonate pendant groups, while the 6.5 Â phase probably 2

2

1

1

1 3

2

2


3 1

2

2

2

15

3

3

2

2

2

1

2

2

2

2

2

2

2

2

2

3

r

x

x

4 4


2


172

consists of mostly phosphite groups. The 19.6 Â phase may contain alternating mostly-phosphonate and mostly-phosphite layers since its interlayer spacing nearly equals the sum of the other two separations. This type of phase separation is expected since the carboxylic acid groups are hydrophilic, while the phosphite groups are relatively hydrophobic. For comparison, Alberti et al. reported a 12.2 Â interlayer spacing for Zr(0 PCH CTl2COOH) ^ ( Ο ^ Ρ Η ^ Η λ ^ Ο (16). The TGA of Zr-COOH-H is consistent with a stoichiometry of Z r ^ P Œ ^ CH COOH)i 25(Ο^ΡΗ)ο.75·0.5Η2θ. However, since three distinct phases are present it is impossible to determine the exact stoichiometry of each phase. Again, the C, Η, Ν analysis was of little help in determining the stoichiometry. Values of 7.04% C, 1.77% H, and 0% Ν were obtained. Theoretical values for Zr(03FCH CH CO) 125(Q3 H)o 75·0·5Η Ο are 12.8% C and 2.3% H ; while for Z r ^ P C r ^ O V COOH)(0^PH>H O, they are 10.6% C and 2.4% H. The IR spectrum of Zr-COOH-H looks like that of Z K O ^ P Œ Œ C O O H ) with a superimposed P-H stretch at 2473 cnr . The 1703 cm" C=0 stretch of ZrCOOH-H suggests a similarity between these carboxylic acid groups and those found both in Zr-COOH-OH and Zr(03PCH CH COOH)2. The C CP MAS NMR spectrum also closely resembles that of Zr(O^FCH Œ COOH) with the carbonyl isotropic chemical shift at 179.8 ppm and an incompletely averaged methylene region. The P M A S NMR spectrum of Zr-COOH-H shows three resonances: 11.8,8.0, and -14.7 ppm of relative intensities 30:100:80, respectively. Owing to the similarities of these chemical shifts to those of the single component analogs, these peaks have tentatively been assigned to the mostly-phosphonate phase (12.7 Â), the phosphonate-phosphite phase (19.6 Â), and the mostly-phosphite phase (6.5 Â), respectively. The relative intensities of the P peaks qualitatively match those observed in the powder XRD pattern. That is, the dominant phase, for which a sharp (000 reflection is observed, is the 19.6 Â phase. A small, broad reflection of ca. 10% the intensity of the 19.6 Â reflection is seen at 12.7 Â, while the 6.5 Â reflection is of about 30% the intensity of the 19.6 Â reflection and is also rather broad. The smaller percentage of phosphonate groups in Zr-COOH-H relative to Zr-COOH-OH, coupled with the smaller size of phosphite groups relative to phosphate groups, suggest that a guest molecule may have more access to the carboxylic acid sites of Zr-COOH-H than Zr-COOH-OH. In fact, we have found that under identical conditions Zr-COOH-H gave a significantly higher conversion to its acyl chloride derivative than did Zr-COOH-OH Contacting the solids with refluxing S O Q for two weeks did not fully convert either to the corresponding acyl chloride. However, while the IR spectrum of the product from Zr-COOH-H exhibits two C=0 stretches at 1801 (-COC1) and 1703 cm" (-COOH) (figure 4b), the IR spectrum of the product from Zr-COOH-OH shows a 1715 cnr absorption with only a high energy («1800 cm" ) shoulder. Absorotions at 1715 cnr have been observed during many reactions of Zr(03PCH CH COOH) , and have been attributed to a carboxylic acid phase in which the interlayer hydrogen bonding network has been disrupted (21). Heating Zr-COOH-OH and Zr-COOH-H to 170°C under vacuum to drive off interstitial water prior to treatment with refluxing SOCl increased the yield of both acyl chlorides, but still did not result in full conversion of either. The IR spectrum of the reaction product from dehydrated Zr-COOH-OH (Figure 4a) exhibited distinct 2

3

1

2


2

0 H

2

p

2

2

2

1

2

1

1 3

2

2

2

2

2

3 1

3 1

2

1

1

1

1

2

2

2

2


2

Asymmetrically Layered Zr Phosphonates 173


1

C=0 stretches at 1794 and 1715 cm" in roughly the same ratio as those in the product obtained from non-dehydrated Z r - C O O H - H (Figure 4b). Although neither mixed component system affords conversion of all carboxylic acid groups to acyl chlorides without pre-intercalation, both do yield partial conversion. We believe these results support the notion that strong interlayer hydrogen bonding is responsible for the lack of reactivity between Zr(03PCH CH COOH)2 and S O C l .


2

2

2

Figure 4. IR spectra of productsfromreaction of SOCl with dehydrated Zr-COOH-OH (top) and non-dehydrated Zr-COOH-H (bottom). 2

When the partially converted acyl chloride derivative of Z r - C O O H - O H was contacted with hexylamine, a material with a 25.0 Â interlayer spacing was formed. This represents an 11.2 Â increase in interlayer spacing over Z r - C O O H - O H . For comparison, the analogous hexylamide derivative, Zr(03PCH CH CONHC6Hi3) , has an interlayer spacing 14.1 A greater than Z r ( 0 P C H C H C O O H ) . Both IR and C N M R spectroscopy showed the presence of amide and ammonium carboxylate salt, as expected. When Z r - C O O H - O H was treated with hexylamine directly, the product showed four orders of (00/) reflections in the powder X R D pattern from a 26.2 Â phase. This compares to a interlayer spacing of 28.7 Â for the hexylammonium intercalate of Z r ( 0 P C H C H C O O H ) . Curiously, both the IR and C N M R spectra of this product suggest that a small amount amide was formed in addition to the expected hexylammonium product. When the partially converted acyl chloride derivative of Z r - C O O H - H was contacted with hexyl alcohol, a phase of interlayer spacing 28.5 Â was formed— an increase of 8.9 Â over the 19.6 Â separation of the host. This can be compared to a 12.7 Â increase in interlayer spacing upon conversion of Zr(03PCH CH COOH) to Z r ( 0 P C H C H C O O C H ) . The 12.7 À phase of Z r - C O O H - H appears to have 2

3

2

2

2

2

2

1 3

1 3

3

2

2

2

2

3

2

2

6

1 3

2

2


2

174


intercalated some alcohol, as a broad reflection of ca. 5% the intensity of the 28.5 Â reflection is seen at 13.8 Â. A 13.8 Â phase has been noticed in alcohol intercalation compounds of Z r ( C ^ P Œ Œ C œ H ) (27). A broad reflection at ca. 6.5 Â is also observed, indicating that the mostly-phosphite phase is unchanged. The IR spectrum shows two C=0 absorptions at 1741 and 1702 cm , corresponding to ester and acid, respectively. It should be noted that Zr-COOH-H as formed did not intercalate hexyl alcohol. Contacting Zr-COOH-H with hexylamine resulted in intercalation of the amine to give the hexylammonium carboxylate compound. The 19.6 Â phase increased in interlayer spacingto31.8 Â, while the 12.7 Â phase disappeared. The 6.5 Â phase also appears to have increased slightly to 6.7 A. 2

2

2


-1

Conclusion The direct reactions of thionyl chloride with porous phosphonate-phosphate and phosphonate-phosphite compounds lead to partial conversion of the phosphonate carboxylic adds to acyl chlorides. This reaction does not occur in the single component phosphonate analog, Zr(O^PCH CH COOH) . To form Zr(0 PCH CH COCl)2, Z r ( 0 3 F Œ Œ C O O H ) must be intercalated with an amine prior to treatment with thionyl chloride. While the porous materials did not give high yields of the desired acyl chloride, it is interesting to note that the partially-converted acyl chlorides behave in a similar fashion to Z r ( 0 P C H C H C O a ) toward alcohols and amines. Thus, it may be possible to prepare pillared materials with amide or ester groups supporting the zirconium phosphate layers. 2

2

2

2

2

3

2

2

2

3

2

2

2

Experimental Section 1 3

3 1

General Methods. Room temperature C and P solid-state N M R spectra were recorded on a JEOL 270 MHz spectrometer (67.9 and 109 MHz for C and P , respectively) equipped with a 7-mm probe from Doty Scientific. Highpower *H decoupling, cross polarization and magic angle spinning were employed for all 1 C spectra. A 50 kHz field strength was used for both H decoupling and cross polarization; spinning speeds were 3.5-4.0 kHz. C signals were referencedtoTMS (downfield shifts positive) by using adamantane as a secondary external reference. High-power H decoupling and MAS were employed for P spectra P signals were externally referenced to 85 wt% H3PO4 (downfield shifts positive). FTIR spectra were obtained on a Nicolet 730 FT-IR Spectrometer at a resolution of 4 cm . A DuPbnt Instruments Thermogravimetric Analyzer 951 and Thermal Analyst 2000 workstation were usedtoobtain TGA thermograms. Thermograms were run in an air atmosphere from room temperatureto1150°C at a scan rate of 10°C/min Powder x-ray diffraction patterns were obtained using either a Scintag PAD-V diffractometer or a Philips Electronics Instruments diffractometer (both Cu Κα radia tion). X R D analyses were typically conducted with powders which were preferentially aligned on a quartz single crystal or microscope slide. The calculated standard deviations for the interlayer spacings were no greater than 0.7 Â. Materials. Except where noted, all starting materials were purchased from Aldrich Chemical Company and were used as received. 1 3

3 1

3

l

1 3

l

3 1

3 1

-1



BURWELL & THOMPSON

Synthesis of Z r ( O P C H C H C O O H ) ( O P O H ) . 5 * 0 . 5 H O . ZrOCl *8H 0 (9.1 g) was dissolved in 50 ml distilled water and 4 ml HF solution (48 wt% in water) in a 250 ml plastic bottle. H3FO4 (3.1 g) and 2-carboxyethylphosphonic acid (4.8 g) were dissolved in 75 ml distilled water and added to the Z1OCI2HF solution. Some precipitate formed on contact The plastic bottle was filled with distilled water and sealed. The sealed bottle was placed in a 70°C oil bath for 4 days. The cooled mixture was centrifuged and the liquid decanted. The remaining white gel was dried at 100°C overnight The resulting transparent, glass-like solid was ground with mortar and pestle to a coarse white powder. IR (KBr): 3600-2500 (m, ν br), 1701 (s), 1293 (m), 1266 (m), 1203 (m), 1040 (vs, ν br), 815 (w), 551 (w), 519 (m), 470 (w) cm-1. Powder XRD: d = 13.8 Â. C CP MAS N M R Ô(COOH) = 180.0 ppm; ô(CH ) = 27.8 ppm (v br). P CP MAS NMR: ô(P-C) = 9.2 ppm, δ(Ρ-ΟΗ) = -22.1 ppm. TGA: room temperature-200°C, -2.5%; 200-600°C, -14.2%; 600-1150°C, -12.7%. Synthesis of Z r t O j P C H i C H ^ O C l h . s i O ^ O H J o . s . Z r - C O O H O H (0.5 g) was placed in a flask and dehydrated by heating to 170°C under vacuum for 3 hours. Theflaskwas then cooled to 0°C under nitrogen and 15 ml SOCI2 (previously cooled to 0°Q was addedtotheflask.The temperature of the mixture was raisedto9O°C and held there for 16 days under an nitrogen atmosphere. The SOCI2 was removed and the product dried under vacuum. IR (KBr): 3600-2500 (m, br), 1794 (m), 1715 (m), 1434 (m), 1413 (m), 1263 (s), 1040 (vs, ν br), 803 (s) 522 (s) cm-1. Synthesis of Z r ( 0 P C H C H C O O H ) ( 0 P H ) o . 7 5 * 0 . 5 H 0 . Ζτθα ·8Η 0 (6.5 g) was dissolved in 20 ml distilled water and 3.3 g HF solution (48 wt% in water) in a round bottom flask. To thisflaskwas added a solution of 4.6 g (H0) P(0)Œ CH2C00H and 5.0 g H3PO3 in 50 ml distilled water. Some precipitate formed on contact, and an additional 25 ml distilled water was added to fluidize the slurry. The mixture was refluxed for 24 hours under an argon atmosphere. The product was collected on a medium frit, washed with water, and driedtoa constant weight at 100°C. IR (KBr): 3600-2500 (m, br), 2473 (m), 1703 (s), 1266 (s), 1201 (s), 1075 (vs, br), 1035 (vs, br), 574 (m), 558 (m) cm" . Powder XRD: d = 19.6,12.7 and 6.5 Â. C CP MAS NMR: Ô(COOH) = 179.8 ppm; ô(CH ) = 28.4 ppm (v br). P CP MAS NMR: ô(mixed Ρ) = 8.0 ppm, δ(Ρ-Η) = -14.7 ppm, ô(P-Q = 11.8 ppm. T G A room temperature-200°C, -2.8%; 200-600°C, -11.5%; 600-1150°C, -9.9%. Synthesis of Z r ( O 3 P C H C H C O C I ) ( O 3 P H ) . 7 5 . Z r - C O O H - H ( 1.2 g) was addedto25 ml SOCl previously cooledto0°C under a nitrogen atmosphere. The mixture was stirred 2 weeks at 90°C under a nitrogen atmosphere. The SOCI2 was removed and the product dried under vacuum. IR (KBr): 3600-2800 (s, ν br), 2474 (m), 1801(m), 1703 (s), 1433 (m), 1413 (m), 1050 (vs, ν br) cm" . Synthesis of Z r ( 0 P C H C H C ( 0 ) O C H ) ι . ( Ο Ρ Η ) . 7 5 · Zr(0 PŒ2Œ2COa) 25(O^PH)o.75 (1 g) was addedtoaflaskalong with 25 ml hexyl alcohol. The mixture was stirred for 2 weeks at 60°C under a nitrogen purge. The product was collected on a fritted glass filter, washed with acetone and water, and dried at 100°Ctoa constant weight IR (KBr): 2959 (s), 2931 (s), 2872 (s), 2860 (s), 2474 (s), 1741 (s), 1702 (m), 1468 (m), 1428 (m), 1365 (m), 1247 (s), 1176 (s), 1050 (vs, ν br) cm" . Powder X R D : rf = 28.5Â. 3

2

2

L 5

0

3

2

2

2


1 3

3 1

2

3

2

2

l e 2 5

3

2

2

2

2

2

1

1 3

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Acknowledgement Acknowledgement is also made to the Donors of the Petroleum Research Foundation, administered by the American Chemical Society (ACS-PRF#22051-G3), and to the Air Force Office of Scientific Research (AFOSR90-0122) for the support of this project The purchase of the JEOL 270 NMR spectrometer was made possible by NSF Grant CHE-89-09857.


Literature Cited (1) (a) Intercalation Chemistry, Whittingham, M. S.; Jacobson, A. J.; Eds.; Academic Press Inc.: New York, 1982. (b) Schöllhorn, R. in Inclusion Compounds; Academic Press: London, 1984. (c) Dresselhaus, M. S. Mater. Sci. Eng., B l 1988, 259. (d) Formstone, C. Α.; Fitzgerald, E. T.; O'Hare, D.; Cox, P. Α.; Kurmoo, M.; Hodby, J. W.; Lillicrap, D.; Goss-Custard, M. J. Chem. Soc., Chem. Commun. 1990, 501. (2) (a) Lee, H.; Kepley, L. J.; Hong, H.; Mallouk, T. E. J. Am. Chem. Soc. 1988, 110, 618. (b) Lee, H.;Kepley, L. J.; Hong, H.; Akhter, S.; Mallouk, T. E. J. Phys. Chem. 1988, 92, 2597. (c) Putvinski, T. M.; Schilling, M. L.; Katz, H. E.; Chidsey, C. E. D.; Mujsce, A. M.; Emerson, A. B. Langmuir, 1990, 6, 1567. (3) Cao, G.; Rabenberg, L. Κ.; Nunn, C. M.; Mallouk, Τ. Ε. Chem. Mater., 1991, 3, 149. (4) (a) Li, Z.; Lai, C.; Mallouk, T. E. Inorg. Chem. 1989, 28, 178. (b) Rong, D.; Kim, Y. I.; Mallouk, T. E. Inorg. Chem. 1990, 29, 1531. (5) (a) Kanatzidis, M. G.; Wu, C.; Marcy, H. O.; DeGroot, D. C.; Kannewurf, C. R. Chem. Mater. 1990, 2, 222. (b) Kanatzidis, M. G.; Hubbard, M.; Tonge, L. M.; Marks, T. J.; Marcy, H. O.; Kannewurf, C. R. Synth. Metals 1989, 28, C89. (c) Mehrotra, V.; Giannelis, E. P. Solid State Comm., 1991, 77, 155. (6) (a) Alberti, G.; Costantino, U. in ch. 5 of ref. 1a (b) Alberti, G.; Costantino, U.; Marmottini, F. in Recent Developments in Ion Exchange, Williams, P. Α.; Hudson, M. J.; Eds.; Elsevier Applied Science: New York, 1987. (c) Clearfield, A. Chem. Rev. 1988, 88, 125. (7) (a) Alberti, G.; Costantino, U. J. Mol. Catalysis 1984, 27, 235. (b) Clearfield, A. J. Mol. Catalysis 1984, 27, 251. (c) Hattori, T.; Ishiguro, Α.; Murakami, Y. J. Inorg. Nucl. Chem. 1978, 49, 1107. (d) Clearfield, Α.; Thakur, D. Appl. Catal. 1986, 26, 1. (8) Alberti, G.; Costantino, U.; Allulli, S.;Tomassini, N. J. Inorg. Nucl. Chem. 1978, 40, 1113. (9) (a) Dines, M. B.; DiGiacomo, P. M. Inorg. Chem. 1981, 20, 92. (b) Dines, M. B.; Griffith, P. C. Polyhedron 1983, 2, 607. (c) Dines, M. B.; Griffith, P. C. Inorg. Chem. 1983, 22, 567. (10) (a) Clearfield, A. Comments Inorg. Chem. 1990, 10, 89. (b) Alberti, G. in Recent Developments in Ion Exchange, Williams, P. A.; Hudson, M. J.; Eds.; Elsevier Applied Science: New York, 1987, 233. (11) Burwell, D. Α.;Thompson, M. E. Chem. Mater. 1991, 3, 730. (12) Burwell, D. Α.;Thompson, M. Ε. Chem. Mater. 1991, 3, 14.


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(13) Alberti, G.; Costantino, U. in ch. 5 of ref. 1a. (14) Alberti, G.; Costantino, U. J.Mol.Catalysis 1984, 27, 235. (15) Dines, M. B.; Cooksey, R. E.; Griffith, P.C.;Lane, R. H. Inorg. Chem. 1983, 22, 1003. (16) Alberti, G.; Costantino, U.; Környei, J.; Giovagnotti, L. Reactive Polymers 1985, 4, 1. (17) Clearfield, A. J. Mol. Catalysis 1984, 27, 251. (18) Troup, J. M.; Clearfield, A. Inorg. Chem. 1977, 16, 3311. (19) Dines, M. B.; DiGiacomo, P. M. Inorg. Chem. 1981, 20, 92. (20) Alberti, G.; Costantino, U.; Marmottini, F. in Recent Developments in Ion Exchange, Williams, P. Α.; Hudson, M. J.; Eds.; Elsevier Applied Science: New

York, 1987, 249. (21) Burwell, D. Α.; Thompson, M. E. unpublished results. RECEIVED January 16, 1992


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