Basic Sites on Alumina with Preadsorbed Ethanol and Ammonia—An IR Study

The adsorption of ethanol and ammonia changes the basic properties of alumina, and new basic sites are created. Ethanol reacts with surface Al-OH groups, forming ethoxy group Al-O-C2H5. The substitution of Al-OH by Al-O-C2H5 increases the negative charge of neighbouring oxygen atoms, and they became sufficiently basic to react with adsorbed CO2 forming carbonate species CO32−. These carbonates were found to be monodentate and bidentate species. Preadsorption of ammonia also increases the basicity of alumina, but the mechanism is different than for ethanol adsorption. Adsorbed ammonia interacts with surface Lewis acid sites being three-coordinated aluminium atoms. This interaction is accompanied by an electron transfer from ammonia molecules to surface sites, and increases the basicity of the neighbouring oxygens, which can react with the absorbed CO2. The carbonate species formed are polydentate ones.

The oxygen atoms and hydroxyl groups on metal oxides have a negative charge.Generally, the less electronegative the metal is, the more negative both the oxygens and surface hydroxyls are.These sites are potential basic sites.However, the local environment of surface sites may cause bigger polarization of the M-O and M-OH bond; therefore, these sites are more basic than other ones, and these O 2− or OH − may react with adsorbed CO 2 molecules, forming carbonate species (CO 3  2− ) or bicarbonate species (HCO 3 − ).Our earlier IR [18] study evidenced that, for alumina, only ca.5-10% of surface hydroxyls was able to react with CO 2 , forming bicarbonate species, and surface oxygens practically did not react with CO 2 .On the other hand, ca.30% of hydroxyls situated on zirconia surface reacted with CO 2 , forming bicarbonate, and some surface oxygens also reacted with CO 2 , forming carbonates.Bigger reactivity of surface sites on zirconia with CO 2 , if comparing with alumina, may be related to lower electronegativity of Zr if comparing with Al (1.33 and 1.61, respectively).However, for both alumina and zirconia, only a relatively small fraction of surface sites is sufficiently basic to react with CO 2 forming bicarbonate and carbonate species.The surface hydroxyls reacting with CO 2 will be denoted as OH − , and surface oxygens reacting with CO 2 will be denoted as O 2− .
The adsorption studies and TPD experiments provide information on the total concentration of all the basic sites, O 2− plus OH − , without distinguishing between them.
On the other hand, IR spectroscopic studies of CO 2 adsorption can discriminate between O 2− and OH − .O 2− reacting with CO 2 produces carbonate species (CO 3 2− ), whereas OH − forms bicarbonates (HCO 3 − ).Carbonate and bicarbonate species show different IR spectra [10,13,[15][16][17].Both carbonates and bicarbonates may be bonded to surface sites in different ways.They may be monodentate, bidentate, or polydentate.Therefore, a careful analysis of the IR spectrum of adsorbed CO 2 informs not only which kind of basis sites (O 2− or OH − ) are present on the surface, it also provides additional information how the (bi)carbonate species are bonded to adsorption sites.However, the IR results concerning CO 2 adsorption obtained by the above-mentioned authors have only qualitative aspects.Recently, we elaborated [18] a new method of quantitative IR studies of concentrations of both O 2− and OH − .The extinction coefficients of diagnostic IR bands were determined and, finally, the concentrations of both O 2− and OH − on the surfaces of ZrO 2 , CeO 2 Al 2 O 3 , CuO, ZnO, Ga 2 O 3 and MgO were determined.We also elaborated a new method for determination of the total concentration of all the basic sites (O 2− plus OH − ) on oxides via the desorption of CO 2 monitored by IR.The sum of concentrations of O 2− and OH − , determined separately in our IR experiments, was very close to total basic sites concentration determined in desorption studies [18,19].
The present study concerns the problem of modification of basic properties of alumina by the adsorption of ethanol and ammonia prior to adsorption of CO 2 .Our previous studies [20] evidenced that the reaction of alcohols with surface Al-OH groups produced alcoxy groups.It was interesting to know how the substitution of Al-OH by Al-O-C 2 H 5 would modify the basicity of neighbouring surface sites.Another problem was the study of effect of adsorption of ammonia, which interacts with Lewis acid sites (being threecoordinated Al) on the basicity of neighbouring surface sites.In this study, the information on the basicity of surface sites was obtained by adsorption of CO 2 as probe molecule.The concentration of OH − was determined from the intensity of the δ OH band (1230 cm −1 ), and the extinction coefficient of this band determined in our previous study.[18].The total basicity (concentration of O 2− plus OH − ) was determined in desorption studies monitored by IR [19].The concentration of O 2− was the difference between the total basicity (O 2− plus OH − ) and the concentration of OH − .

Basic Sites on Al 2 O 3 -CO 2 Adsorption
The spectrum of CO 2 adsorbed on Al 2 O 3 activated at 720 K is presented in Figure 1A.The band interpretation was based on the earlier results of Collins et al. [16].The visualization of the vibration of carbonate species is given in [21].The spectra show intensive bands of bicarbonate species: ν sym C-O at 1435-1480 cm −1 , ν asym C-O at 1660-1680 cm −1 , and the bending of OH group δ OH at ca. 1230 cm −1 .The band of ν sym C-O is complex.It is composed of submaxima of monodentate and bidentate bicarbonates (1435 and 1455 cm −1 resp.).The high frequency component (at 1475 cm −1 ) cannot be clearly identified.It is not excluded that it can be assigned to ν sym C-O of polydentate carbonate species.The bands of carboxylate species, ν sym C-O at ca. 1200 cm −1 and ν asym C-O 1700-1800 cm −1 [6], are present too.The bands of carbonate species (1300-1400 cm −1 ) are relatively weak.These results evidence that the basic sites on alumina surface are mostly basic OH − , the contribution of O 2− is rather low.Similar results were also obtained by other authors [22,23].The spectrum of OH groups of Al 2 O 3 shows four distinct OH bands at 3770, 3755, 3730 and 3675 cm −1 .The assignment of these hydroxyl bands was proposed by Knözinger and Ratnasamy [24].The band at 3770 cm −1 was assigned to terminal Al-OH in which Al is four-coordinated, 3755 cm −1 , to bibridged hydroxyls in which both Al are hexacoordinated, 3730 cm −1 , to bibridged hydroxyls in which one Al is four-coordinated and the second one is hexacordinated.The 3675 cm −1 band was assigned to tribridged hydroxyls in which all three Al are hexacoordinated.The band at 3585 cm −1 may be due to oxohydroxy species.These free OH groups were denoted as: type I, IIB, IIA, and III.
three Al are hexacoordinated.The band at 3585 cm −1 may be due to oxohydroxy species.These free OH groups were denoted as: type I, IIB, IIA, and III.According to Knozinger et al. [24], they differ in the electrical charge: those of type I are the most negative, and those of type III are positive.The reaction of OH groups with CO2 causes appearance of new C-OH bands typical of bicarbonate species.The band at 3613 cm −1 may be assigned to bidentate, and the band at 3677 cm −1 to monodentate bicarbonates.

Basic Sites on Al2O3 with Preadsorbed Ethanol
The reaction of alcohols with surface hydroxyls on oxides produces alkoxyl groups according to the scheme: X-OH + HO-R = X-O-R + H2O.In order to study how the substitution of surface Al-OH by Al-O-C2H5 changes the basic properties of alumina, CO2 was adsorbed on alumina on which ethanol was preadsorbed at room temperature and, subsequently, non-reacting ethanol and water were removed by evacuation at 370 K.
The spectra recorded upon the adsorption of ethanol on activated alumina followed by evacuation are presented in Figure 2A.The spectra show intense bands at 1130 and 1170 cm −1 of monodentate ethoxyls, as well as at the 1390 and 1450 cm −1 bands of the CH3 and CH2 groups.
The spectra of hydroxyl groups are presented in Figure 2B.The formation of ethoxy groups is accompanied by the loss of some hydroxyls.The hydroxyls of highest stretching frequencies are the most reactive against ethanol.This agrees with the fact that, according to Knozinger et al. [24], high frequency hydroxyls are the most negative.
The spectra of (bi)carbonate species formed by the reaction of CO2 with basic sites on alumina with preadsorbed ethanol (i.e., containing surface ethoxy groups) are presented in Figure 2A, and may be compared with the spectra of (bi)carbonates formed on alumina surface without ethoxyls.At the presence of ethoxy groups, the band of bending of OH (δOH at 1230 cm −1 ) is lower than that without ethoxyls, indicating that the contribution of bicarbonates is lower too.This may be related to the fact that the reaction with ethanol consumed some of the most basic Al-OH, therefore the amount of basic OH − able to react with CO2 is smaller.The spectra of (bi)carbonate species formed on alumina with preadsorbed ethanol (Figure 2A) show some new bands that were absent without ethanol.A possible interpretation of these new bands will be now discussed.The new bands at 1340 and 1615 cm −1 may be attributed to νsym C-O and νasym C-O in bidendate carbonates, respectively.The band at 1385 cm −1 may be assigned to monodentate carbonates, and the bands at 1430 and 1480 cm −1 to polydentate carbonates.The presence of relatively strong bands of carbonate species formed at the presence of ethoxyl groups is evidence that some surface oxygens that were not enough basic to react with CO2 became basic if Al-OH were According to Knozinger et al. [24], they differ in the electrical charge: those of type I are the most negative, and those of type III are positive.The reaction of OH groups with CO 2 causes appearance of new C-OH bands typical of bicarbonate species.The band at 3613 cm −1 may be assigned to bidentate, and the band at 3677 cm −1 to monodentate bicarbonates.

Basic Sites on Al 2 O 3 with Preadsorbed Ethanol
The reaction of alcohols with surface hydroxyls on oxides produces alkoxyl groups according to the scheme: X-OH + HO-R = X-O-R + H 2 O.In order to study how the substitution of surface Al-OH by Al-O-C 2 H 5 changes the basic properties of alumina, CO 2 was adsorbed on alumina on which ethanol was preadsorbed at room temperature and, subsequently, non-reacting ethanol and water were removed by evacuation at 370 K.
The spectra recorded upon the adsorption of ethanol on activated alumina followed by evacuation are presented in Figure 2A.The spectra show intense bands at 1130 and 1170 cm −1 of monodentate ethoxyls, as well as at the 1390 and 1450 cm −1 bands of the CH 3 and CH 2 groups.The information on the concentration of OH − on Al2O3 without and with ethoxy groups was obtained from the intensity of the δOH band (at 1230 cm −1 ) and its extinction coefficient, as determined in our previous study [18].These values are presented in Table 1.The information on the total concentration of all the basic sites was obtained in studies of the desorption of CO2 monitored by IR spectroscopy by using a method described in our previous paper [19].These values are also presented in Table 1.Assuming that the The spectra of hydroxyl groups are presented in Figure 2B.The formation of ethoxy groups is accompanied by the loss of some hydroxyls.The hydroxyls of highest stretching frequencies are the most reactive against ethanol.This agrees with the fact that, according to Knozinger et al. [24], high frequency hydroxyls are the most negative.
The spectra of (bi)carbonate species formed by the reaction of CO 2 with basic sites on alumina with preadsorbed ethanol (i.e., containing surface ethoxy groups) are presented in Figure 2A, and may be compared with the spectra of (bi)carbonates formed on alumina surface without ethoxyls.At the presence of ethoxy groups, the band of bending of OH (δ OH at 1230 cm −1 ) is lower than that without ethoxyls, indicating that the contribution of bicarbonates is lower too.This may be related to the fact that the reaction with ethanol consumed some of the most basic Al-OH, therefore the amount of basic OH − able to react with CO 2 is smaller.The spectra of (bi)carbonate species formed on alumina with preadsorbed ethanol (Figure 2A) show some new bands that were absent without ethanol.A possible interpretation of these new bands will be now discussed.The new bands at 1340 and 1615 cm −1 may be attributed to ν sym C-O and ν asym C-O in bidendate carbonates, respectively.The band at 1385 cm −1 may be assigned to monodentate carbonates, and the bands at 1430 and 1480 cm −1 to polydentate carbonates.The presence of relatively strong bands of carbonate species formed at the presence of ethoxyl groups is evidence that some surface oxygens that were not enough basic to react with CO 2 became basic if Al-OH were substituted by Al-O-C 2 H 5 .The reaction of CO 2 with basic sites affects only a few of the hydroxyl groups on alumina with ethoxy groups (Figure 2B, bottom spectrum).It may be explained by taking into account that some hydroxyls were already consumed by the reaction with ethanol and, therefore, a relatively small amount of bicarbonates was formed by the reaction of OH − with CO 2 .
The information on the concentration of OH − on Al 2 O 3 without and with ethoxy groups was obtained from the intensity of the δ OH band (at 1230 cm −1 ) and its extinction coefficient, as determined in our previous study [18].These values are presented in Table 1.The information on the total concentration of all the basic sites was obtained in studies of the desorption of CO 2 monitored by IR spectroscopy by using a method described in our previous paper [19].These values are also presented in Table 1.Assuming that the total concentration of basic sites is the sum of concentrations of OH − and O 2− , the concentration of O 2− can be calculated by subtraction.The values of O 2− concentration are also given in Table 1.According to the data given in Table 1, Al 2 O 3 without ethoxy groups contains mostly OH − , the contribution of O 2− is significantly lower, and the formation of ethoxy groups by the reaction with ethanol produces important amounts of new O 2− able to react with CO 2 .This statement agrees with the conclusion obtained by comparing the spectra of CO 2 adsorbed on Al 2 O 3 without and with ethoxy groups (Figure 2A).The spectra suggest the appearance of new mono-, bi-, and polydentate carbonates on Al 2 O 3 treated with ethanol.The spectrum of ammonia adsorbed on alumina (Figure 3) shows several bands.The bands typical of ammonia interacting with Lewis acid sites are three-coordinated surface Al atoms as follows: 1620 cm −1 (antisymmetric deformation of NH 3 ), 3270, and 3360 cm −1 (symmetric and antisymmetric N-H stretching).The presence of such three-coordinated Al atoms was evidenced by Knozinger and Ratnasamy [24].These bands decrease as the ammonia is desorbed by evacuation at increasing temperatures (Figure 3).Ammonia adsorbed on alumina also interacts with Al-OH groups via hydrogen bonding.The minima on the difference spectra (Figure 3B) correspond to these Al-OH groups that are engaged in hydrogen bonding.There is no proton transfer from Al-OH to NH 3 , because the band of the ammonium ion (at ca.1430 cm −1 ) is absent.Evacuation at increasing temperatures (Figure 3B), which removes ammonia from Al sites (decrease of 1620 cm −1 ), also removes ammonia from OH groups.The minima in the difference spectra in Figure 3B become more "shallow".However, it should be noted that even the desorption at relatively high temperature (400 K) did not remove all the NH 3 from OH groups (Figure 3B, bottom difference spectrum).The interaction of CO 2 with Al 2 O 3 with preadsorbed ammonia from which ammonia was partially removed by desorption at various temperature was followed.

Basic Sites on Al2O3 with Preadsorbed Ammonia
The spectrum of ammonia adsorbed on alumina (Figure 3) shows several bands.The bands typical of ammonia interacting with Lewis acid sites are three-coordinated surface Al atoms as follows: 1620 cm −1 (antisymmetric deformation of NH3), 3270, and 3360 cm −1 (symmetric and antisymmetric N-H stretching).The presence of such three-coordinated Al atoms was evidenced by Knozinger and Ratnasamy [24].These bands decrease as the ammonia is desorbed by evacuation at increasing temperatures (Figure 3).Ammonia adsorbed on alumina also interacts with Al-OH groups via hydrogen bonding.The minima on the difference spectra (Figure 3B) correspond to these Al-OH groups that are engaged in hydrogen bonding.There is no proton transfer from Al-OH to NH3, because the band of the ammonium ion (at ca.1430 cm −1 ) is absent.Evacuation at increasing temperatures (Figure 3B), which removes ammonia from Al sites (decrease of 1620 cm −1 ), also removes ammonia from OH groups.The minima in the difference spectra in Figure 3B become more "shallow".However, it should be noted that even the desorption at relatively high temperature (400 K) did not remove all the NH3 from OH groups (Figure 3B, bottom difference spectrum).The interaction of CO2 with Al2O3 with preadsorbed ammonia from which ammonia was partially removed by desorption at various temperature was followed.The spectra of CO2 adsorbed on alumina without and with preadsorbed ammonia are presented in Figure 4A.The excess ammonia (sufficient to saturate all the adsorption sites) was adsorbed at room temperature, and the physisorbed molecules were removed by evacuation at 340 K. CO2 was subsequently adsorbed on such a pretreated sample.The intensity of the δOH is comparable for alumina without and with ammonia; however, the intensity of carbonate bands is significantly higher in the presence of ammonia.It suggests that the neutralization of Lewis acid sites (three-coordinated Al) and engaging of some Al-OH in hydrogen bonding with ammonia increases the negative charge on neighbouring oxygens, which became sufficiently basic to react with CO2, forming CO3 2− .The amount of OH − reacting with CO2 does not change.
In order to get information on the assignment of IR bands of (bi)carbonate species formed on alumina at the presence of ammonia, the stability of these species was studied.Our previous study [18] evidenced that bicarbonates are less stable than carbonates, they decompose by evacuation at relatively low temperatures, and the IR bands that disappear via low temperature evacuation can, therefore, be assigned to bicarbonataes, and those  The spectra of CO 2 adsorbed on alumina without and with preadsorbed ammonia are presented in Figure 4A.The excess ammonia (sufficient to saturate all the adsorption sites) was adsorbed at room temperature, and the physisorbed molecules were removed by evacuation at 340 K. CO 2 was subsequently adsorbed on such a pretreated sample.The intensity of the δ OH is comparable for alumina without and with ammonia; however, the intensity of carbonate bands is significantly higher in the presence of ammonia.It suggests that the neutralization of Lewis acid sites (three-coordinated Al) and engaging of some Al-OH in hydrogen bonding with ammonia increases the negative charge on neighbouring oxygens, which became sufficiently basic to react with CO 2 , forming CO 3 2− .The amount of OH − reacting with CO 2 does not change.
the adsorption of CO2 and evacuation at 350 K.This spectrum represents weakly bonded bicarbonate species; therefore, the bands at 1230, 1410 and 1660 cm −1 can be assigned to bicarbonates.The bands remaining upon evacuation at a relatively high temperature (410 K-bottom spectra in Figure 4D) at 1460, 1590 and 1610 cm −1 are due to polydentate carbonates.This interpretation is supported by the data presented in previous papers [11,15,16].

Figure 4. (A)
The spectra of the adsorbed CO2 on activated Al2O3 and Al2O3, on which NH3 was adsorbed and, subsequently, desorbed at 340 K. (B) The spectrum of OH groups on Al2O3 activated, spectra recorded upon adsorption of NH3, followed by desorption at 340 K, adsorption of CO2 on Al2O3 with preadsorbed NH3, as well as difference spectra.(C) The spectra of (bi)carbonate species on Al2O3 with preadsorbed ammonia recorded upon the desorption at 300, 320, 350, 390 and 410 K. (D) (Bi)carbonates on Al2O3 with preadsorbed NH3.Spectrum of the less stale species (spectrum upon adsorption of CO2 minus spectrum upon desorption at 350 K).Spectrum of the most stable species (remaining upon the desorption at 410 K).Spectra are normalized to the same band intensity.
Summing up, it can be said that, in the presence of preadsorbed ammonia, new basic sites O 2− are formed, and they react with CO2, forming mostly polydentate carbonyls.
The information on the concentration of basic sites OH − and O 2− was obtained by taking into account the intensity of the δOH band (at 1230 cm −1 ) and its extinction (D) (Bi)carbonates on Al 2 O 3 with preadsorbed NH 3 .Spectrum of the less stale species (spectrum upon adsorption of CO 2 minus spectrum upon desorption at 350 K).Spectrum of the most stable species (remaining upon the desorption at 410 K).Spectra are normalized to the same band intensity.
In order to get information on the assignment of IR bands of (bi)carbonate species formed on alumina at the presence of ammonia, the stability of these species was studied.Our previous study [18] evidenced that bicarbonates are less stable than carbonates, they decompose by evacuation at relatively low temperatures, and the IR bands that disappear via low temperature evacuation can, therefore, be assigned to bicarbonataes, and those that remain upon evacuation at higher temperatures can be assigned to carbonates.CO 2 was adsorbed on alumina with preadsorbed ammonia and, subsequently, (bi)carbonates were decomposed by evacuation at 300, 320, 350, 390 and 410 K.The spectra recorded upon each desorption step are presented in Figure 4C, and the difference spectra in Figure 4D.The top spectrum in Figure 4D is the difference between the spectra recorded upon the adsorption of CO 2 and evacuation at 350 K.This spectrum represents weakly bonded bicarbonate species; therefore, the bands at 1230, 1410 and 1660 cm −1 can be assigned to bicarbonates.The bands remaining upon evacuation at a relatively high temperature (410 K-bottom spectra in Figure 4D) at 1460, 1590 and 1610 cm −1 are due to polydentate carbonates.This interpretation is supported by the data presented in previous papers [11,15,16].
Summing up, it can be said that, in the presence of preadsorbed ammonia, new basic sites O 2− are formed, and they react with CO 2 , forming mostly polydentate carbonyls.
The information on the concentration of basic sites OH − and O 2− was obtained by taking into account the intensity of the δ OH band (at 1230 cm −1 ) and its extinction coefficient, as well as the total concentration of basic sites, which was determined in desorption experiments.
More details are given in the previous chapter, and the concentration values are presented in Table 1.Similarly, as for ethanol, the preadsorption of ammonia produces a significant amount of new basic O 2− .We suppose that this is the result of the transfer of electrons from basic ammonia molecule to Lewis acid sites (three-coordinated Al) next to neighbouring surface sites, which makes these neighbouring oxygen atoms sufficiently basic to react with CO 2 , forming CO 3  2− .In order to study how the basicity of the alumina surface depends on the amount of ammonia adsorbed, all the acid sites were saturated by ammonia at room temperature, and ammonia was subsequently desorbed by evacuation at temperatures 300, 340, 350, 370 and 400 K.The spectra of adsorbed ammonia recorded upon each desorption step are presented in Figure 3, and the fraction of the Lewis acid sites still bonding ammonia upon such desorption calculated from the intensity of the 1620 cm −1 band is given in Table 2. CO 2 was next adsorbed on such a pretreated sample, and the IR spectra are presented in Figure 5.The intensity of the carbonate bands decrease with the desorption temperature.The same conclusion was obtained by considering the results of desorption studies monitored by IR spectroscopy (Table 2).The total basicity (i.e., the amount of CO 2 desorbed) decreases with the ammonia desorption temperature.Summing up, it can be stated that the more ammonia remains on the alumina surface, the higher the basicity of surface oxygens measured by CO 2 adsorption is.In another words, the more Lewis acid sites neutralized by ammonia, the bigger the extend of electron transfer to surface sites is, and the more surface oxygen is sufficiently basic to react with CO 2 .
Molecules 2024, 29, x FOR PEER REVIEW 7 of 10 coefficient, as well as the total concentration of basic sites, which was determined in desorption experiments.More details are given in the previous chapter, and the concentration values are presented in Table 1.Similarly, as for ethanol, the preadsorption of ammonia produces a significant amount of new basic O 2− .We suppose that this is the result of the transfer of electrons from basic ammonia molecule to Lewis acid sites (three-coordinated Al) next to neighbouring surface sites, which makes these neighbouring oxygen atoms sufficiently basic to react with CO2, forming CO3 2− .
In order to study how the basicity of the alumina surface depends on the amount of ammonia adsorbed, all the acid sites were saturated by ammonia at room temperature, and ammonia was subsequently desorbed by evacuation at temperatures 300, 340, 350, 370 and 400 K.The spectra of adsorbed ammonia recorded upon each desorption step are presented in Figure 3, and the fraction of the Lewis acid sites still bonding ammonia upon such desorption calculated from the intensity of the 1620 cm −1 band is given in Table 2. CO2 was next adsorbed on such a pretreated sample, and the IR spectra are presented in Figure 5.The intensity of the carbonate bands decrease with the desorption temperature.The same conclusion was obtained by considering the results of desorption studies monitored by IR spectroscopy (Table 2).The total basicity (i.e., the amount of CO2 desorbed) decreases with the ammonia desorption temperature.Summing up, it can be stated that the more ammonia remains on the alumina surface, the higher the basicity of surface oxygens measured by CO2 adsorption is.In another words, the more Lewis acid sites neutralized by ammonia, the bigger the extend of electron transfer to surface sites is, and the more surface oxygen is sufficiently basic to react with CO2.
For IR studies, all oxides were pressed into thin wafers of ca.100-250 mg.Prior to IR experiments, wafers were evacuated in situ in an IR cell at 720 K for 30 min.CO 2 , ethanol and ammonia were adsorbed at room temperature.For CO 2 adsorption, the gas pressure in the IR cell was ca. 5 Torr.The band of molecular CO 2 was present in the IR spectra, evidencing that all basic sites reacting with CO 2 were saturated.For ethanol adsorption, the pressure in IR cell was ca. 3 Torr.Ethanol was contacted with alumina wafer for 3 min, and was subsequently desorbed via a 30 min evacuation at 370 K.In the experiments of ammonia adsorption, the pressure in the IR cell was 1-2 Torr.Ammonia was contacted with the alumina wafer for 3 min and, subsequently, it was desorbed by evacuation at various temperatures: 300, 340, 450, 370 and 400 K.The fraction of Lewis acid sites still covered by ammonia upon desorption was defined as the ratio of intensity of NH 3 band at 1620 cm −1 in the spectrum recorded upon the desorption and the intensity of this band upon the desorption at 300 K.In all experiments, the CO 2 was adsorbed at room temperature on the wafer of alumina with preadsorbed ethanol and ammonia.
The method of determination of total basicity (the concentration of O 2− plus OH − ) was described in detail in our previous paper [19]; some information on this method will be presented below.All the basic sites on alumina without and with preadsorbed molecules were first saturated with CO 2 at room temperature.Next, the gaseous CO 2 was removed from the cell, and physisorbed molecules were removed by 1 min evacuation at room temperature.CO 2 bonded to basic sites was subsequently desorbed at 470 K from the sample and trapped in a cold trap.The molecules trapped in the cold trap were next adsorbed on the wafer of zeolite NaY (which is a very efficient adsorbent).The amount of CO 2 adsorbed on NaY was calculated from the intensity of the CO 2 band at ca 2300 cm −1 and the extinction coefficient of this band.The total amount of CO 2 adsorbed on basic sites was calculated by taking into account the amount of CO 2 adsorbed on NaY, as well as the integrated intensities of all IR bands of the adsorbed (bi)carbonate species before and after evacuation at room temperature, and after the desorption at 470 K.More details are given in [19].
The spectra were recorded with a NICOLET 6700 spectrometer (Thermo Scientific, Cambridge, MA, USA) with a spectral resolution of 1 cm −1 .The spectra were recorded at the transmission mode.

Conclusions
The experiments of CO 2 adsorption evidenced that basic sites of OH − were present on the alumina surface, and the concentration of basic O 2− sites was relatively low.The reaction of surface hydroxyls Al-OH with ethanol produced ethoxy groups Al-O-C 2 H 5 .At the presence of ethoxy groups, some surface oxygen become sufficiently basic to react with CO 2 , forming CO 3 2− .These new carbonates were mainly monodentate and bidentate.A similar situation was observed if NH 3 was preadsorbed on alumina.Ammonia reacted with surface Lewis acid sites, i.e., three-coordinated Al atoms; the transfer of electrons from

Figure 1 .
Figure 1.(A) The spectrum of CO2 adsorbed on Al2O3.(B) The spectra of OH groups on Al2O3 activated, upon CO2 adsorption and difference spectrum.

Figure 1 .
Figure 1.(A) The spectrum of CO 2 adsorbed on Al 2 O 3. (B) The spectra of OH groups on Al 2 O 3 activated, upon CO 2 adsorption and difference spectrum.

Molecules 2024 ,
29, x FOR PEER REVIEW 4 of 10 substituted by Al-O-C2H5.The reaction of CO2 with basic sites affects only a few of the hydroxyl groups on alumina with ethoxy groups (Figure2B, bottom spectrum).It may be explained by taking into account that some hydroxyls were already consumed by the reaction with ethanol and, therefore, a relatively small amount of bicarbonates was formed by the reaction of OH − with CO2.

Figure 2 .
Figure 2. (A)The spectra of ethoxy groups recorded upon adsorption of ethanol and removal physisorbed molecules, the spectrum of CO2 adsorbed on activated Al2O3, and the spectrum recorded upon adsorption of CO2 on Al2O3 containing ethoxy groups.The spectrum of ethoxy groups has been subtracted.(B) The spectra of OH groups on Al2O3 activated upon the reaction with ethanol and upon adsorption of CO2 on Al2O3 containing ethoxy groups, as well as the difference spectra.

Figure 2 .
Figure 2. (A) The spectra of ethoxy groups recorded upon adsorption of ethanol and removal physisorbed molecules, the spectrum of CO 2 adsorbed on activated Al 2 O 3 , and the spectrum recorded upon adsorption of CO 2 on Al 2 O 3 containing ethoxy groups.The spectrum of ethoxy groups has been subtracted.(B) The spectra of OH groups on Al 2 O 3 activated upon the reaction with ethanol and upon adsorption of CO 2 on Al 2 O 3 containing ethoxy groups, as well as the difference spectra.

Figure 3 .
Figure 3. (A)The spectra of ammonia adsorbed on Al2O3 recorded upon the desorption at 300, 340, 350, 370 and 400 K. (B) The spectrum of OH groups on Al2O3 activated and difference spectra (spectra recorded upon the adsorption of ammonia and desorption at 300, 340, 350, 370 and 400 K minus spectrum of activated Al2O3).

Figure 3 .
Figure 3. (A) The spectra of ammonia adsorbed on Al 2 O 3 recorded upon the desorption at 300, 340, 350, 370 and 400 K. (B) The spectrum of OH groups on Al 2 O 3 activated and difference spectra (spectra recorded upon the adsorption of ammonia and desorption at 300, 340, 350, 370 and 400 K minus spectrum of activated Al 2 O 3 ).

Figure 4 .
Figure 4. (A) The spectra of the adsorbed CO 2 on activated Al 2 O 3 and Al 2 O 3 , on which NH 3 was adsorbed and, subsequently, desorbed at 340 K. (B)The spectrum of OH groups on Al 2 O 3 activated, spectra recorded upon adsorption of NH 3 , followed by desorption at 340 K, adsorption of CO 2 on Al 2 O 3 with preadsorbed NH 3 , as well as difference spectra.(C) The spectra of (bi)carbonate species on Al 2 O 3 with preadsorbed ammonia recorded upon the desorption at 300, 320, 350, 390 and 410 K. (D) (Bi)carbonates on Al 2 O 3 with preadsorbed NH 3 .Spectrum of the less stale species (spectrum upon adsorption of CO 2 minus spectrum upon desorption at 350 K).Spectrum of the most stable species (remaining upon the desorption at 410 K).Spectra are normalized to the same band intensity.

3 Figure 5 .
Figure5.The spectra of (bi)carbonate species formed on Al 2 O 3 with preadsorbed ammonia.The CO 2 was adsorbed upon adsorption of NH 3 , followed by desorption at 340, 350, 370 and 400 K.

Table 1 .
The concentration of all the basic sites (total basicity OH − + O 2− ), OH − , and of O 2− on Al 3 O 3 without and with ethoxy groups, as well as with ammonia preadsorbed (physisorbed ammonia was removed by evacuation at 340 K).

Table 2 .
The concentration of all the basic sites on Al 2 O 3 with preadsorbed ammonia as a function of ammonia desorption temperature.