About this Journal Submit a Manuscript Table of Contents
ISRN Physical Chemistry
Volume 2013 (2013), Article ID 164868, 7 pages
http://dx.doi.org/10.1155/2013/164868
Research Article

Acid-Free Nitration of Benzene and Toluene in Zeolite NaZSM-5

Department of Chemistry, East Tennessee State University, P.O. Box 70695, Johnson City, TN 37614, USA

Received 20 December 2012; Accepted 22 January 2013

Academic Editors: F. M. Cabrerizo, B.-T. Liu, X. Rozanska, and E. Yeow

Copyright © 2013 Scott J. Kirkby. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract

The syntheses of nitrobenzene and p-nitrotoluene directly from benzene, toluene, and NO2 within the pore network of the initially acid-free zeolite NaZSM-5 are reported for the first time. The active species , formed by the interaction of NO2 with the Na+ cations present on the internal surface, results in the acid-free electrophilic substitution of the aromatic ring. There are two distinct reservoirs for the reagents: one associated with close proximity to the cation sites and the other associated with the siliceous areas of the pore network. Up to 34% of the hydrocarbon and 70% of the available NO2 are reacted at 50°C. Only the cation associated sites are reactive at low temperature, and there appears to be little mobility between the sites under the reaction conditions. There is no evidence of a second nitration occurring. This represents a novel route to the single nitration of benzene and toluene and for toluene, the generation of the para isomer exclusively. The pore network of the NaZSM-5 restricts the available reaction volume and transition state geometry allowing only the para-substituted product.

1. Introduction

As part of an investigation into employing heterogeneous catalysis to selectively produce small industrial intermediates, nitrobenzene and para-nitrotoluene were synthesized directly from benzene and toluene and NO2 in the initially acid-free zeolite, NaZSM-5.

Approximately 95% of the >1.5 106 tonnes of nitrobenzene produced annually is used in the production of aniline [1]. Most of the remainder is used for precursors in rubber, pesticides, dyes, and pharmaceuticals such as Acetaminophen [1, 2]. Para-nitrotoluene is used in the synthesis of p-toluidine, which in turn is used to manufacture dyes and as accelerators for cyanoacrylate adhesives [3].

ZSM-5 is a medium pore pentasil zeolite [4, 5] with two perpendicular channel systems (see Figure 1). The first is a straight channel of elliptical cross section of 0.55 0.51 nm, and the second is sinusoidal with dimensions of 0.56 0.53 nm [6]. Its most valuable industrial process is the isomerization of xylenes to enhance the fraction of para-xylene in the product stream [79]. This is thought to result from the aluminosilicate channel wall restricting the available transition state volume and enhancing the diffusion of the para-isomer down the pores [10]. The void space of the channel system easily accommodates para-substituted benzene rings, but is too restricted to allow easy movement of ortho- and meta-substituted species. ZSM-5 would thus be ideal for the selective formation of para-nitrotoluene.

fig1
Figure 1: Molecular modeling representation of the two-dimensional pore network for Zeolite ZSM-5.

Economic considerations for industrial intermediates favor selection of the least expensive reagent, hence NO2 for nitration, even at the cost of selectivity. Traditional methods for the nitration of aromatic rings using NO2 involve strong acids to generate , which is the active entity in an electrophilic substitution of the ring [11, 12]. Use of solid-acid catalysts, such as alumina/silica/metal oxides achieves excellent conversions, but with limited ability to enhance the proportion of any isomer [13, 14]. Acid zeolites have been used successfully as solid-acid catalysts to achieve nitration of aromatics with varying levels of selectivity [1517]. These methods require a high-temperature acid activation step. In contrast, it has been shown that the electrostatic fields of the Na+ cations in NaZSM-5 are capable of enhancing the electrophilic character of small molecules adsorbed into the channel system at room temperature [18]. This would allow the use of NaZSM-5 as a heterogeneous nitration catalyst without conversion of the zeolite to an acid form and high-temperature activation of the acid sites.

2. Experimental

NaZSM-5 was prepared from commercial NH4ZSM-5 (Zeolyst, product no. CBV15014, lot no. 15014-1525-63, SiO2/Al2O3 = 150) by ion exchanged using sodium acetate. The exchange was repeated until could not be detected by FT-IR spectroscopy. Thus the Na/Al ratio was inferred to be 1. Also, it is important to note that there was no detectable Brønsted acid hydroxyl peak at 3611 cm−1 [19].

The reactions were carried out in 6–9 mg (12.5 mm diameter) self-supporting pellets of neat NaZSM-5 contained in a stainless steel gas cell within a variable temperature vacuum cryostat (Oxford Instruments model DN1714). The wafers were dehydrated overnight at 200°C (maximum cryostat temperature, and below the normal NH4ZSM-5 to HZSM-5 conversion temperature of 400–600°C) under vacuum (Varian turbo molecular pump model V-60). The zeolite was exposed to 2.0 torr of either benzene or toluene (Aldrich 99.9%) for one half hour at room temperature after which the gas cell was evacuated to below 5 mtorr. The sample was then cooled or heated to the experimental temperature and allowed to stabilize for 1.5 hours. 10.0 torr of room temperature NO2 (Matheson 99.5%) gas was released into the gas cell, and then after thirty seconds the cell was closed. Time zero for the kinetics corresponds to the initial release of the NO2 into the sample cell.

The gas cell and the cryostat were fitted with KCl windows to allow the in situ collection of FT-IR spectra. Spectra were collected using an IBM-Bruker IR-44 spectrometer. 100 scans at 1 cm−1 resolution were coadded and ratioed against a background of the empty dehydrated pellet at 25°C. Time zero for the kinetics was the initial release of NO2 into the cell. 100 scans required approximately 100 s to collect on the IR-44, and thus each data point in the kinetics plot corresponds to a 100 s wide time slice.

The identity of the major reaction product was determined by comparison with spectra of authentic samples of nitrobenzene, and ortho-, meta-, and para-isomers of dinitrobenzene and nitrotoluene (all from Aldrich, 99%) obtained by the vapor-phase loading of a freshly dehydrated clean pellet.

3. Results and Discussion

The IR spectrum of the dehydrated NaZSM-5 pellet (see Figure 2) contains several peaks in the >1300 cm−1 IR window. They are a broad peak at 3588 cm−1 from residual water (OH stretch) in the lattice. This peak has two shoulders at 3739 and 3688 cm−1 corresponding to SiOH hydroxyls on the surface of the crystallites [19]. Another residual water peak (bend) occurs at 1636 cm−1. A small sharp peak occurs at 1485 cm−1 from trace impurities introduced during ion exchange of the zeolite. The peak at 1392 cm−1 is caused by silicone vacuum grease migrating onto the IR cell windows during the dehydration process.

164868.fig.002
Figure 2: FT-IR spectrum of a dehydrated NaZSM-5 pellet. Note: the effective window for monitoring adsorbed species extends from 4000 to approximately 1300 cm−1 because of the intense framework modes below that point.

There are two moderate intensity framework modes at 2006 and 1882 cm−1. Again, there is no IR evidence of Brønsted acid sites at 3611 cm−1 [19]. Adsorption of benzene or toluene into the pellet results in shifts of the framework modes to lower frequency as the lattice distorts to accommodate the hydrocarbon [19]. This may be observed by the slight drop in the baseline of the difference spectrum ((zeolite with hydrocarbon)—empty zeolite) near 1300 cm−1 and the distortion of the baseline near 2006 and 1882 cm−1 (see Figure 3). Similarly the residual water is disturbed leading to a dip in the difference spectrum at 1636 cm−1 and formation of a broad band at 3637 cm−1. The surface SiOH are also disturbed leading to minima at 3730 and 3688 cm−1.

164868.fig.003
Figure 3: FT-IR spectrum ((zeolite + hydrocarbon)—empty zeolite) for benzene adsorbed into the pore network of NaZSM-5 at room temperature.

Adsorption of benzene onto NaZSM-5 results in new bands at 3094, 3074, 3040, 1985, 1954, 1858, 1809, 1517, 1480, 696, and 672 cm−1 (see Figure 3). Frequency shifts relative to gas-phase C6H6 are small [20]. The weak absorption at 1517 cm−1 is assigned to the ( ) ring mode, which is infrared inactive in the gas phase [20]. The appearance of this mode indicates interaction with the zeolite environment that breaks the symmetry. The two pair of modes at 1985/1858 and 1954/1809 cm−1 (see inset of Figure 3) for C6H6 indicate two primary adsorption sites. The higher frequency pair is associated with the cation site, while the lower pair corresponds to benzene adsorbed on the “silica” framework. The “silica modes” are much more intense and narrower than for the “cation modes” suggesting that the majority of the benzene is not associated with a cation and that the cation environments are very inhomogeneous.

Infrared spectra obtained upon loading of C6D6 into NaZSM-5 mirror the effects observed for the parent molecule. Bands of the occluded benzene-d6 are at 2389, 2285, 2270, 1616, 1350, and 1328 cm−1. The existence of two major types of adsorption sites is supported by the 2285/2270 cm−1 splitting of the CD stretching mode [19]. Analysis of the spectra suggests that the 2270 cm−1 component is associated with benzene adsorbed on Na+ and the 2285 cm−1 peak with adsorption on siliceous parts of the zeolite wall [19]. Infrared bands of toluene adsorbed on the zeolite (3089, 3069, 3032, 2984, 2925, 2875, 1955, 1939, 1870, 1854, 1800, 1606, 1597, 1565, 1523, 1496, 1452, 1379, 1340, 747, 726, and 694 cm−1) are very close to those of the gas-phase molecule. As for benzene, two distinct loading sites are observed. One associated with the Na+ cation and one corresponding to adsorption on the silica pore wall.

Adsorption of NO2 into the zeolite favors formation of N2O4 especially at lower temperature. Three different forms of N2O4 may be observed in the lattice. Symmetric O2NNO2 with symmetry is the predominant specie (intense absorption at 1741 cm−1). Since NaZSM-5 is transparent in the region 770 to 630 cm−1, low frequency modes of this species at 742 and 685 cm−1 are observed as well. Asymmetric O2NONO with both D and D′ symmetries is also observed at 1807 and 1894 cm−1, respectively [21]. At 25°C and 50°C, symmetry N2O4 is converted to D′ O2NONO as observed by the loss of intensity of the form’s peaks and the concurrent increase in the peak at 1894 cm−1. This inter conversion is not observed after several hours at 0°C. D and D′ forms differ from each other by the torsion angle about the O2N–ONO bond [21]. There is no consumption of the D or D′ forms during the reaction with either benzene or toluene.

When the temperature of the zeolite is raised from 0 to 50°C, the N2O4 bands diminish. At the same time, there is an intensity increase for absorptions at 2127, 1980 1892, 1677, 1413, and 1371 cm−1, all of which are assigned to monomeric species formed at the expense of the dimer. Figure 4 shows the spectrum of NO2 loaded NaZSM-5 at 50°C after spectral subtraction of the residual gas-phase NO2. Both nitrogen and oxygen “contact” adsorbed forms of NO2 are observed at 1580 and 1420 cm−1, respectively, which are close to their values on silica. The strong band at 1892 cm−1 lies in a region where NO absorbs (gas phase, 1876 cm−1) [22]. The species is introduced as an impurity of the reactant gas. There is, however, no evidence of NO or N2O3 formation under the experimental conditions.

164868.fig.004
Figure 4: FT-IR difference spectrum for NO2 adsorbed into a clean dehydrated pellet of NaZSM-5 at 50°C.

In addition to rearrangement, charge-transfer products are also found. has an absorption in the range 2340 to 2380 cm−1 depending in its local environment [23]. No bands were observed in this region. Testova et al. [15] have reported bands at 2345 and 2140 cm−1 in HZSM-5 while Chao and Lundsford report peaks at 2000 and 2100 cm−1 in NaY [24]. Comparison with the acetyl radical [25, 26] suggests that it may be more appropriate to designate these species as zeolite (abbreviated from here on as for brevity) resulting from donation of electron density from the NO2 HOMO to the when the complex forms. As δ increases, the peak of the symmetric stretch will shift to a higher frequency (see Figure 5). The broad bands at 2048 and 1983 cm−1 most likely represent these and species.

164868.fig.005
Figure 5: Schematic molecular orbital diagram for NO2, , and . The grayed electron represents the diminished electron density in the HOMO because of donation to the zeolite Na+ cation. The result is a shift of the vibrational frequency to higher wave number. As δ increases, so does the frequency. The extent of the donation depends on the local environment of the cation in the zeolite.

Matrix isolated absorbs at 1244 cm−1 [27] and is thus not directly observable in ZSM-5 zeolite because of obstruction by the framework modes. Partially negative charged species most likely give rise to the doublet at 1413 and 1371 cm−1 [28]. The small bands at 1607 and 1677 cm−1 originate from NO2 that interacts only weakly with the zeolite’s environment because they are close to the gas-phase frequency [29].

In addition to intensity changes in the benzene peaks because of “sweep in” and displacement effects, adsorption of NO2 into benzene-loaded NaZSM-5 results in the spontaneous loss of reactant peaks and the concurrent growth of new infrared bands at 3083, 2873, 1533, 1520, 1456, 1378, 1352, 1319, 706, 682, and 682 cm−1 (see Figure 6(a)). These correspond to those for authentic nitrobenzene directly adsorbed into empty NaZSM-5. The reaction of benzene with NO2 is highly temperature dependent. At 0°C only 2-3 percent of the initial benzene peak intensity is lost after 240 minutes. This increases to 7 percent at 25°C and 34% at 50°C along with a corresponding consumption of approximately 70% of N2O4 originally present in the lattice (see Figures 7 and 8). For the 50°C experiments, there is also a loss of peak intensity between 2050 and 1980 cm−1 which corresponds to the various positive charge-transfer species of NO2. There is no spectroscopic evidence for a second nitration occurring. Using authentic nitrobenzene adsorbed into the lattice gives no detectable reaction with NO2 at 50°C after four hours. Above 50°C, the amount of adsorbed NO2/N2O4 is reduced, thus limiting the amount of product formed.

fig6
Figure 6: FT-IR spectra for the reaction of (a) benzene and (b) toluene with NO2 at 50°C. The traces are time , the initial exposure of the zeolite plus hydrocarbon to NO2 (dash); after four hours of reaction (dash-dot); difference (solid).
164868.fig.007
Figure 7: Representative normalized peak intensity versus time plots for the consumption of benzene at 0°C (●), 25°C (■), and 50°C ( ) for the benzene. Note: the intensity rise above one is the result of “sweep in” effects from the loading of NO2 into the zeolite lattice.
fig8
Figure 8: Normalized peak integral versus time plots for (a) the consumption of N2O4 (1741 cm−1) and (b) the growth of the asymmetric –NO2 stretch for benzene (●), benzene-d6 (▲), toluene (■), and toluene-d8 (♦) at 50°C.

Infrared product absorptions followed the expected first-order growth behavior, except for one of the two components of the intense asymmetric NO2 stretch of nitrobenzene (see Figures 8 and 9). Of the two bands at 1533 and 1520 cm−1, the higher frequency component exhibited a clear induction period. This is attributed to a second site of nitrobenzene inside the zeolite pores since it is also observed when loading an authentic sample of nitrobenzene into NaZSM-5. Experiments with benzene-d6 under the same conditions furnished some insight into the origin of this site splitting. The product spectrum of the C6D6 + NO2 reaction, which agreed well with the infrared spectrum of perdeuteronitrobenzene reported in the literature [30] showed a (NO2) doublet at 1526 and 1511 cm−1. As in the case of the parent isotope, the growth of the higher frequency peak exhibited an induction period. Comparison with the depletion profile of the (CD) absorption of C6D6 at 2285 and 2270 cm−1 suggests a connection between the benzene and nitrobenzene adsorption sites as shown in Figure 9. While the growth of (NO2) of C6D5NO2 upon C6D6 + NO2 reaction at 50°C shows both a 1526 and a 1511 cm−1 peak, the reaction at 0°C results only in growth at 1511 cm−1. The corresponding infrared difference spectrum in the (CD) region of C6D6 reveals that at 0°C depletion occurs exclusively at 2270 cm−1. By contrast, at 50°C, decrease of both the 2285 and 2270 cm−1 peaks is observed (see Figure 9). The 2270 cm−1 site is faster and has a much greater extent of reaction at a given temperature. This suggests that reaction of benzene adsorbed on Na+ cation sites (2270 cm−1) leads to nitrobenzene absorbing at 1526 cm−1, while benzene absorbed on siliceous areas of the zeolite pores is responsible for product growth at 1511 cm−1. This suggests that there are two independent reservoirs of reagents, and under the experimental conditions, there is little interconversion between the two below 50°C. The reason for this may be that in the “full” zeolite, diffusion slows appreciably. This would also explain that the much-reduced extent of reaction as only those regents directly adsorbed onto reactive sites are able to react at temperatures below 50°C.

fig9
Figure 9: Normalized peak integral versus time plots for (a) the consumption of the two CD modes of benzene-d6 and (b) for the growth of the asymmetric –NO2 stretch separated into <1520 (●) and >1520 cm−1  (▲) components and the sum (■).

The induction period may also result from dependence on the side product H+ from the more reactive sites. Only when sufficient H+ is present in the siliceous areas is the sufficiently active for nitration to occur. There is, however, no spectroscopic evidence to for the formation of HNO2 or during the course of the reaction.

Loading of toluene and NO2 into zeolite NaZSM-5 led to nitration of the arene at about 1.5 times the rate observed for benzene. Studies were again conducted at 0, 25, and 50°C. Decrease of the toluene bands was accompanied by loss of around 2000 cm−1 and symmetric D2h N2O4 (1741, 742, 685 cm−1) under concurrent product growth at 1564, 1522, 1508 (shoulder), 1345, and 737 cm−1. The spectral changes in the >1300 cm−1 region are shown in Figure 6(b). Comparison with spectra of authentic samples of o-nitro, m-nitro, and p-nitrotoluene in NaZSM-5 revel that only p-nitrotoluene is formed. The pore network of the NaZSM-5 restricts the available reaction volume and transition state geometry allowing only the para-substituted product [18]. As for benzene, there is no evidence for a significant isotope effect.

4. Conclusions

Nitrobenzene and p-nitrotoluene were synthesized directly from benzene, toluene and NO2 within the pore network of the initially acid-free zeolite NaZSM-5. The active species is formed by the interaction of NO2 with the cations present on the internal surface. There are two distinct reservoirs for the reagents: one associated with close proximity to the cation sites and the other associated with the siliceous areas of the pore network. The extent of reaction is highly temperature dependent with only 2-3% of the hydrocarbon reacting at 0°C and increasing to 34% (>70% of the available NO2) at 50°C. Only the cation-associated sites are reactive at low temperature, and there appears to be little mobility between the sites under the reaction conditions. There is no evidence of a second nitration occurring. This represents a novel route to the single nitration of benzene and toluene and for toluene, the generation of exclusively the para-isomer.

Acknowledgment

The author wishes to thank Dr. Heinz Frei, Lawrence Berkeley National Laboratory, for the assistance with the initial effort of this work.

References

  1. G. Booth, “Nitro compounds, aromatic,” in Ullmann's Encyclopedia of Industrial Chemistry, John Wiley & Sons, New York, NY, USA, 2007.
  2. A. Bhattacharya, V. C. Purohit, V. Suarez, R. Tichkule, G. Parmer, and F. Rinaldi, “One-step reductive amidation of nitro arenes: application in the synthesis of Acetaminophen,” Tetrahedron Letters, vol. 47, no. 11, pp. 1861–1864, 2006. View at Publisher · View at Google Scholar · View at Scopus
  3. K. Konstantinov, M. Pavlova, M. Glushkov, and L. Dicheva, “Synthesis of methyl 2-cyanoacrylate,” Khimiya i Industriya, vol. 5, pp. 218–219, 1982.
  4. R. J. Argauer and G. R. Landolt, U.S. Patent 3 702 886, 1972.
  5. F. G. Dwyer and E. E. Jenkins, U.S. Patent 3 941 871, 1976.
  6. D. H. Olson, G. T. Kokotallo, S. L. Lawton, and W. M. Meier, “Crystal structure and structure-related properties of ZSM-5,” The Journal of Physical Chemistry, vol. 85, no. 15, pp. 2238–2243, 1981. View at Publisher · View at Google Scholar
  7. R. W. Neuzil, U.S. Patent 3 558 730, 1973.
  8. R. W. Neuzil, U.S. Patent 3 558 732, 1973.
  9. J. J. Ward, “Molecular sieve catalysis,” in Applied Industrial Catalysis, B. B. Leach, Ed., vol. 3, p. 271, Academic Press, New York, NY, USA, 1984.
  10. J. Kårger and D. M. Ruthven, Diffusion in Zeolites and Other Microporous Solids, John Wiley & Sons, New York, NY, USA, 1992.
  11. J. March, Advanced Organic Chemistry, John Wiley & Sons, New York, NY, USA, 3rd edition, 1985.
  12. S. Takenaka, T. Nishida, and J. Kanemoto, U.S. Patent 4 476 335, 1984.
  13. I. Schumaker and K. B. Wang, U.S. Patent 4 415 744, 1983.
  14. I. Schumaker, U.S. Patent 4 618 733, 1986.
  15. N. V. Testova, L. V. Malysheva, K. G. Ione, E. A. Paukshtis, and N. F. Salakutdinov, “Zeolite catalysis for the solution of environmental problens,” in Proceedings of the International Meeting, Yaroslavl, Russia, 1992.
  16. N. F. Salkhutdinov, K. G. Ione, E. A. Kobzar, and L. V. Malysheva, “Gas-phase nitration of aromatic compounds by nitrogen dioxide on zeolites,” Zhurnal Organicheskoi Khimii, vol. 29, pp. 546–558, 1993.
  17. L. V. Malysheva, V. Ludmila, E. A. Paukshtis, and K. G. Ione, “Nitration of aromatics by nitrogen oxides on zeolite catalysts: comparison of reaction in the gas phase and solutions,” Catalysis Reviews, vol. 37, pp. 179–226, 1995.
  18. S. J. Kirkby and H. Frei, “Highly selective photochemical and thermal chlorination of benzene by Cl2 in NaZSM-5,” Journal of Physical Chemistry B, vol. 102, no. 37, pp. 7106–7111, 1998. View at Scopus
  19. H. P. Wang, T. Yu, B. A. Garland, and E. M. Eyring, “Benzene in zeolite ZSM-5 studied by diffuse reflectance infrared spectroscopy,” Applied Spectroscopy, vol. 44, no. 6, pp. 1070–1073, 1990. View at Scopus
  20. G. Herzberg, Infrared and Raman Spectra of Polyatomic Molecules, D. Van Nostrand, New York, NY, USA, 1945.
  21. R. V. St. Louis and B. Crawford Jr., “Infrared spectrum of matrix-isolated NO2,” Journal of Chemical Physics, vol. 42, no. 3, p. 857, 1965. View at Publisher · View at Google Scholar
  22. G. Herzberg, Spectra of Diatomic Molecules, D. Van Nostrand, New York, NY, USA, 1950.
  23. J. W. Nebgen, A. D. McElroy, and H. F. Klodowski, “Raman and infrared spectra of nitronium perchlorate,” Inorganic Chemistry, vol. 4, no. 12, pp. 1796–1799, 1965. View at Scopus
  24. C. C. Chao and J. H. Lundsford, “Infrared studies of the disproportionation reaction of nitric oxide on Y-type zeolites,” Journal of the American Chemical Society, vol. 93, no. 1, pp. 71–77, 1971. View at Publisher · View at Google Scholar
  25. S. Vasenkov and H. Frei, “Observation of acetyl radical in a zeolite by time. Resolved FT-IR spectroscopy,” Journal of the American Chemical Society, vol. 120, no. 16, pp. 4031–4032, 1998. View at Publisher · View at Google Scholar · View at Scopus
  26. S. Vasenkov and H. Frei, “Time-resolved study of acetyl radical in zeolite NaY by step-scan FT-IR spectroscopy,” The Journal of Physical Chemistry A, vol. 104, no. 18, pp. 4327–4332, 2000. View at Publisher · View at Google Scholar
  27. D. E. Milligan and M. E. Jacox, “Matrix-isolation study of the interaction of electrons and alkali metal atoms with various nitrogen oxides. Infrared spectra of the species NO-, NO2-, and N2O2-,” The Journal of Chemical Physics, vol. 55, no. 7, p. 3404, 1971. View at Publisher · View at Google Scholar
  28. P. H. Kasai and R. Bishop Jr., “Electron spin resonance study of nitric oxide adsorption on Linde type Y zeolites,” Journal of the American Chemical Society, vol. 94, no. 16, pp. 5560–5566, 1972. View at Publisher · View at Google Scholar
  29. G. Herzberg, Infrared and Raman Spectra of Polyatomic Molecules, D. Van Nostrand, New York, NY, USA, 1945.
  30. J. D. Laposa, “Vibrational spectra of nitrobenzene-d5,” Spectrochimica Acta A, vol. 35, no. 1, pp. 65–71, 1979. View at Publisher · View at Google Scholar