COMMUNICATIONS TO THE EDITOR
Sept. 20, 1964
3885
Time, min. 200
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Gafolyst], mJles/liter
Fig. 2.--sOlvolysis of copolymer I (6.14 X lo-' M in ester groups) catalyzed by poly( N-vinylimidazole) ( - A - ), 2 5 X 10-6-2 X low2M in imidazole groups, and by N-methylimiM. X dazole(-e-), 5 X 10--2
3
30
T h e , rnin
Fig. l.-%lvolysis of copolymer I (6.14 M in ester groups): - 0 - , without catalyst; - 0 - , with 0.02 hf N-methylimidazole; -A-, with 2.5 X lo-' M (concentration expressed in imidazole units) poly(N-vinylimidazole); - V - , with 5 X 10 M poly(N-vinylimidazole); -A- , with 0.02 M poly( S-vinylimidazole). Solid lines, read bottom time scale; broken lines, read top time scale.
duced. The polymeric catalyst-substrate system is particularly favorable for demonstrating these phenomena since the individual substrate molecules possess numerous anionic sites that are attracted by the multiple cationic sites on the catalyst. In support of the concept that reversible association between catalyst and substrate is involved in these reactions it was found that poly(acry1ic acid), which competes with the copolymer for binding sites on poly(N-vinylimidazole), functioned as an inhibitor in the catalyzed solvolyses (Table I). TABLEI' 101k'. min. -1
65 2@ 14' a Copolymer I, 6.4 X 10-6 M in ester groups; poly(N-vinylM in imidazole units. * k' decreased someimidazole), 5 X what as the reaction progressed. These values correspond to the first 30y0 of the reaction. 0 5
x 10-4 io x 10-4
TABLEI1 Catalyst
Fig. 3.--sOlvolysis
groups],
moles/llter
of copolymer I , catalyzed by poly( N-vinylimidazole, 5 X IO-' M.
phenyl 9-isopropylbenzoate solvolyzed somewhat faster than copolymer I. On changing the catalyst to poly(N-vinylimidazole) it was found that copolymer I solvolyzed markedly faster than dinitrophenyl 9isopropylbenzoate. Selectivity results from acceleration in the rate of solvolysis of the substrate capable of binding to the catalyst. (9) Toni-Gillett Fellow, 1961; Lubrizol Foundation Fellow, 1962
Poly(acrylic acid) (moles/l. of ester groups)
10sk, min. - 1 (dinitrophenyl 10:k, min. -1 isopropylbenzoate) (copolymer I)
None N-Methylimidazole (2 X l o w zM ) Polyvinylimidazole ( 5 X lo-' M in imidaiole units)
IO4 [Ester
2.2 56,5 3.1
1.54 33. 65
Data demonstrating selective solvolysis of a pair of substituted dinitrophenyl benzoates are given in Table 11. With N-methylimidazole as catalyst 2,4-dinitro-
DEPARTMENT OF CHEMISTRY ROBERT L. LETSINGER NORTHWESTERN UNIVERSITY IRVIN KLAUS~ EVANSTON, ILLINOIS RECEIVED J U N E 25, 1964
The Effect of Electrolytes on Circular Dichroism Curves of [Co(en)r]C13 Sir :
It is well known that the observed optical rotation of optically active complexes depends upon the optically inactive ions present as charge compensators. Some previous studies of this effect have been carried out either a t a fixed concentration of inactive ion,' or a t only one wave length.* Tsuchida3 has reported that the maximum in the optical rotatory dispersion (ORD) (1) M . J. Albinak, D C . Bhatnagar, S Kirschner, and A J Sonnesea, Can. J . Ckem., 89, 2360 (19131). (2) R . Larsson, Acto Ckem. Scand., 16, 2267 (1962). (3) R . Tsuchida, J . Chem. SOC.Japan, Pure Chem S e c f . , 68, 621 (1937).
3886
Fig. 1.-Effects
COMMUNICATIONS TO THE EDITOR
of electrolytes on the circular dichroism curve of 1.6 X M [Co(en)3JClacontaining: electrolyte, ( 2 ) 0.5 Af NaCI, ( 3 ) 3.0 A1 NaOH, (4)0.5 M Sa2SO4, and ( 5 ) 0.5 M NaaPO,.
Vol. 86
(1) no additional
curve of (+)- [ C ~ ( e n ) ~ ] is B rshifted ~ toward shorter The data presented were chosen i o show the comwave length on addition of KBr until a 1 : 1 mole ratio parison of anions a t constant molarity (except for is reached. The peak shifts back toward the original NaOH). The effects of different electrolytes reach concentration for higher proportions of KBr. This saturation levels at different concentrations. For conimunication reports results of a study of the effects CI- the effect increases to a maximum at 2 M NaCl. of electrolytes on the circular dichroism (CD) of ( +)546The maximum effect of OH- is that shown (3 M Na[Co(en)a]Cl,.HzO (en = ethylenediamine). The inOH). The effect of the OH- ion is about the same as dividual components of C D spectra are more easily that of other univalent anions of the same concentraseparated than those of O R D or absorption ~ p e c t r a . ~ tion, and hence there are no large pH effects which might This makes the interpretation of C D spectra much confuse the effect of Pod3-. The curve for Podseasier and it permits the effect of electrolytes on inrepresents the limiting effect with this ion. The effect dividual components to be examined. These effects with 0.05 M Na3P04 was almost as great. cannot be seen from O R D or absorption spectra. For the negative peak, the S042- ion has an effect The C D measurements were made as follows. The which is intermediate between that of univalent ions desired electrolyte was dissolved in water, added to a (of the same concentration) and the Pod3-ion. The measured volume of a stock solution of (+)64,3- [ C ~ ( e n ) ~ ] - same order is not observed for the low.,energy ‘E, C13, and diluted to a volume so that the solution was peak, although the serious overlap of these two peaks 1.G X 10V3 -11with respect to the complex and concould cause irregularities. tained the desired molarity of the electrolyte. The Work is in progress to determine to what extent the CD curves were obtained ‘ o n a Jouan dichrograph different factors play a role in the over-all changes in using 5-cm. Beckman cells. Typical results are shown C D data with complexes of different charge types. in Fig. 1. I t is apparent that the effects of electrolytes can be Several gross changes are observed in the C D spectra greatly confused from ORD or absorption spectra where on addition of a large excess of electrolyte. With the the individual components are not separated. The exception of Na3P04,the electrolytes increase the ininvestigation of “outer sphere” complexes from such tensity of all C D peaks, but not to the same extent for data can give false impressions of even the order of all electrolytes or for all peaks. The low energy posistabilities of the complexes. The interpretation of the relative intensities of the ’A2and ‘E, components of tive peak (‘A -., IEa) shows a small increase for sodium salts of C1-, OH -, and s04’- ions, while this peak de[ C ~ ( e n ) ~ ]in C l solution ~ and in solid 2 [( + ) - C ~ ( e n ) ~ creases in intensity in the presence of S a s P 0 4 . The C13].NaC1~6H20 by McCaffery and Mason6 is also negative C D peak (‘A ---t ‘Az) increases in intensity for questionable in light of the expected great effect of the C1- ions in the crystal lattice. all of the electrolytes, with the Po43-ion having a much greater effect than the other anions. It is posThis technique has been demonstrated as an aid in sible that the very large effect of P043- on the ‘A2 interpreting C D spectra by the enhancement of weak bands by the addition of an electrolyte to the solution peak may pull down the ‘Ea peak, masking the real effect of P o d 3 -on the latter peak. The effects on the of optically active [C0(en)~gly]I2.~ second positive C D peak are very small for all elecThe relative effectsof the anions are not the same as expected from the association constants determined for trolytes except Na3P04. (4) R E. l h u g l a s , R . A. Haines, and J. G. Brushmiller, Inorg. 11!14 (1Y63).
Chem., 9,
( 5 ) A . J. McCaffery and S. F. Mason, M o l . P h y s . , 6, 359 (1963). ( 6 ) C.T.Liu a n d B. E. Douglas, Inor#. Chem., S, 1368 (1964).
Sept. 20, 1964
[C0(en)~]3+ with OH-, C1-, and Sod2by an independe n t method.' However, it should be noted that spectrochemical effects need not necessarily be in the same order as thermodynamic association constants, and, of course, the effects of the different electrolytes are not the same for the two C D bands.
I
(7) D. R. Stranks, "Advances in the Chemistry of the Coordination Compounds," S. Kirschaer, Ed., Macmillan Co., New York, N . Y . , 1961, p 574.
t,
HERBERT L. SMITH DEPARTMENT OF CHEMISTRY BODIEE. DOUGLAS THE UNIVERSITY OF PITTSBURGH PITTSBURGH, PENNSYLVANIA 15213 RECEIVED JULY 6,1964
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Radiolysis in the Adsorbed State' Sir : Studies of the decomposition by y-rays of molecules adsorbed on chemically inert mineral supports2-6 have shown that excitation energy delivered to the solid from the radiation can migrate to the surface and become available for decomposition of the adsorbate. For a further study !of this process, we have selected azoethane, ( C ~ H ~ ) ~ as N Xadsorbate, , since the chief decomposition product, nitrogen, is readily separated and measured. Minor gaseous products, hydrogen and methane, which separate with the nitrogen and are measured simultaneously, serve as indicators of the occurrence of other modes of decomposition which presumably require more energy than needed for the production of nitrogen. Radiolysis of pure liquid azoethane gave G(N2) = 3.69, G(H2)= 0.46, and G (CHI) = 0.076.
il
O/
MICROMOLES OF AZOETHANE /WPM
3887
COMMUNICATIONS TO THE EDITOR
OF SOLID
Fig. 1.-Radiolysis products of azoethane adsorbed on silica gel, Corny-rays, dose 5.9 Mrads: open symbols, Fisher Scientific Co. gel, surface 775 m.*/g. determined by the B.E.T. method using N I ; solid symbols, gel heated to 800" in air for 16 hr., surface 500 m.I/g.; circles, Np; triangles, H1; squares, CH,; dotted line is "expected" nitrogen yield (see text).
When adsorbed on silica gel and radiolyzed (Fig. l ) , azoethane behaved much like p e n t a t ~ e . ~As , ~ the amount of azoethane on the gel was increased, the amount of product formed increased, very rapidly a t first, more slowly at higher coverages. The dotted (1) Research performed under the auspices of the U. S. Atomic Energy Commission. (2) J. M . Caffrey, J r . , and A. 0. Allen, J . P h y s . C h c m . , 61,33 (1958). (3) J. W. Sutherland and A . 0. Allen, ibid., 64, 1040 (1860). (4) R . Coekelbergs, A. Crucq, A. Frennet, J. Decot, and L. Timmerman. J .chim. p h y s . , 60, 51 (1963). (5) R . R . Hentz, J . P h y s . Chcm., 66, 1625 (1962). (6) W . H. Clingman, Jr., Ind. Eng.Chcm., 69, 72 (1960).
$ If
3 0
8
1.8 1.6 1.4 1.2
1.0 0.8 0.6 0.4
5 0.2 0
40
80 120 0 r 40 00 120 MICROMOLES' OF AZOETHANE/GF@M OF SOLID
Fig. 2.-Radiolysis products of azoethane adsorbed on magnesium oxide, Co@?-rays, dose 5 . 9 Mrads: left, oxide prepared by heating basic carbonate in air for 16 hr. to 600"; center, to 800"; right, t o 1140' (meaning of symbols as in Fig. 1 ) .
"liquid line" shown in the figures represents the amount of nitrogen that would be formed if only the energy absorbed by the azoethane were effective in decomposing it and the yield of nitrogen werk the same as for the liquid. T h a t the actual yield of nitrogen is many times greater than that shown by the liquid, line indicates transfer of energy from the solid. An interesting observation was made during the blank runs. Silica gel irradiated to 6 Mrads under vacuum turns blue. Simply on exposure to azoethane vapor, the blue color immediately disappeared, while nitrogen was evolved t o the extent of about 10% of what would have formed if the azoethane had been present during the irradiation. Similar observations are reported by Kohn and by Hentz.7 T h a t practically all the aolor centers interact with the added material seems less surprising if we remember that, in silica gel, practically all the solid lies within two atomic diameters of the surface. With magnesium oxide the results were more unexpected (Fig. 2). Three preparations were heated to different temperatures. Surface determination of the two higher temperature preparations, by the B. E.T. method using nitrogen, gave 29 m.'/g. for both. I t is known, however,8 that the higher calcination temperature yields an oxide of less imperfect crystalline structure and lower energy. Figure 2 shows that, a t low coverages, extensive energy transfer to azoethane occurs, the efficiency being greater the more perfect the crystal lattice. Most striking, however, is the decline a t higher coverages of the total amount of decomposition. Thus additional azoethane not only fails t o decompose b u t protects the first molecules adsorbed against decomposition. The amount of azoethane required for maximum yield is quite different for the different gaseous products, being higher for nitrogen than for methane. Hydrogen exhibited a maximum a t a still lower amount of azoethane for the sample of magnesium oxide prepared a t 800'. The decline sets in well below complete monolayer coverage, which should occur a t around 120 pmoles/g. if the area per adsorbed azoethane molecule is assumed (7) (a) H. W . Kohn, Nature, 184, 630 (1959); (b) R . R . Hentz. J P h y s . C h c m , 66, 2714 (1962). ( 8 ) R . Fricke and J. Lueke, 2. Elcklrochcm., 41, 174 (1935); R . M Dell and S. W . Weller, T r a n s . Faraday S o t , 6 6 , 2203 (1959).
