Theoretical study of the adsorption characteristics and the environmental influence of ornidazole on the surface of photocatalyst TiO2.

In this paper, density functional theory (DFT) was performed to study the adsorption properties of ornidazole on anatase TiO2(101) and (001) crystal facets under vacuum, neutral and acid-base conditions. We calculated the adsorption structure of ornidaozle on the anatase TiO2 surface, optimal adsorption sites, adsorption energy, density of states, electronic density and Milliken atomic charge under different conditions. The results show that when the N(3) atom on the imidazole ring is adsorbed on the Ti(5) atom, the largest adsorption energy and the most stable adsorption configuration could be achieved. According to the analysis of the adsorption configuration, we found that the stability of C(2)-N(3) bond showed a weakening trend. The adsorption wavelengths of the electronic transition between the valence band and conduction band of ornidazole on the TiO2 surface were in the visible light wavelengths range, showing that the TiO2 crystal plane can effectively make use of visible light under different conditions. We speculate the possibility of ornidazole degradation on the surface of TiO2 and found that the reactive site is the C-N bond on the imidazole ring. These discoveries explain the photocatalytic degradation of ornidazole by TiO2 and reveal the microscopic nature of catalytic degradation.

Introduction

Ornidazole (n class="Chemical">1-(3chloro-2-hydroxypropyl)-2-methyl-5-nitroimidazole) is a third-generation nitroimidazole drug with anti-anaerobic activity that is commonly used to treat trichomoniasis and amoeba infections[1]. For pharmaceuticals taken by humans and animals, most of the dose is excreted in the form of urine and feces as the original drug or metabolites[2]. Due to the high water-solubility and low biodegradation rates of residual drugs, they are not easily degraded in the environment and are ultimately enriched in water body[3]. The remaining antibiotics in the water environment can be accumulated in human bodies through the food chain even at low concentrations[4]. Drug toxicology experiments have shown that these drugs have potential hazards (genotoxicity[5], neurotoxicity[6], mutagenic[7], etc.). The residues also produce resistant bacteria to interfere with ecosystem stability[8]. Therefore, how to remove antibiotic residues in the environment is of great importance. Although many methods for the degradation of targeted drugs are reported in the literature (absorption, biodegradation, and chemical oxidation), low concentrations of residual drugs are difficult to remove and may cause secondary pollution. Therefore, the use of these methods is subjected to restrictions.

TiO2 photocatalysis is an advanced oxidan class="Chemical">tion technology using strong oxidizing species such as hydroxyl radicals (·OH), superoxide anions (·O2) and perhydroxyl radicals (HOO·) to mineralize organic matter into carbon dioxide, water and inorganic ions[9,10]. At the same time, TiO2 photocatalysis has been applied in many ways, such as the degradation of industrial dyes, pesticide residues, drug residues, etc., due to its mild reaction conditions, no secondary pollution and no toxic byproduct properties. Mohammad et al.[11] adopted anatase TiO2 as a photocatalyst to degrade two types of reactive azo dyes. By continuously changing the test parameters, the two dyes could be completely degraded. Combining quantum chemical theory calculations with experiments, Liu[12] employed the yttrium-doped TiO2 (TiO2/Ce) hydrosol as a photocatalyst to analyze the degradation effect of the pesticide residue dimethoate, and conducted meritorious studies on the subsequent pesticide residues as well. Marothu[13] found that the heterogeneous photocatalytic degradation technology is very effective towards the anti-Parkinson–like entacapone with anatase TiO2, and they studied the effects of the parameters of degradation, such as the catalyst loading, acidity and alkalinity of the solution, and initial concentration. In the present study, anatase TiO2 was utilized as a catalyst to study the adsorption properties of ornidazole on the TiO2(101) and (001) facets under different conditions. We hope to supply some theoretical information for the research of ornidazole.

Results and Discussion

The molecular structure of ornidazole (seen in Fig. S1) and the stable crystal planes of n class="Chemical">TiO2(101) and (001) were optimized. The molecular dynamics of ornidazole on the TiO2(101) and (001) crystal facets was simulated by the LAMMPS program. Based on the relaxation results, we selected the relatively stable adsorption configurations to further optimize the molecular structures by the Materials Studio program. The adsorption energies for the adsorption configurations are shown in Table 1.

Table 1

Adsorption energies for the adsorption configurations of ornidazole adsorbed on TiO2(101) and (001) facets.

Condition	(101) surface		(001) surface		Condition	(101) surface		(001) surface
	Compound	E ads	Compound	E ads		Compound	E ads	Compound	E ads
Vacuum conditions	A1	1.30	a1	2.68	Acid conditions	C1	3.04	c1	2.81
	A2	0.91	a2	2.18		C2	1.95	c2	2.88
	A3	0.89	a3	2.63		C3	2.10	c3	2.60
	A4	0.86	a4	1.91		C4	2.13	c4	2.41
	A5	1.16	a5	2.55		C5	2.21	c5	2.51
Neutral conditions	B1	2.45	b1	2.64	Basic conditions	D1	2.35	d1	2.42
	B2	2.00	b2	2.41		D2	2.03	d2	2.56
	B3	2.19	b3	2.39		D3	1.89	d3	1.72
	B4	2.45	b4	2.45		D4	2.45	d4	2.64
	B5	2.59	b5	2.52		D5	2.52	d5	2.89

Adsorption under vacuum conditions

As shown in Fig. 1, A1~A5 and a1~a5 are five stable configuran class="Chemical">tions of ornidazole adsorbed on TiO2(101) and (001) facets under vacuum conditions, respectively. The nitro moiety O atom and the hydroxyl group O atom on the imidazole ring can absorb on the Ti(5) atom. The H atoms of the C(2) methyl group, on the N(1) branch and on C(4) can form hydrogen bonds with the O(2) atom. Such bonds do not exist that for the N(3) atom adsorbed on the Ti(6) atom and the H atom adsorbed on the O(3) atom. Thus, it is shown that the Ti(5) and O(2) atoms are more active than the Ti(6) and O(3) atoms. Some bond lengths on the surface of TiO2 are slightly deformed owing to the interaction of the ornidazole molecule with the TiO2 surface. Zhang[14] founded that the hydrogen bond can enhance the stability of the multilayer dye aggregates on the TiO2 surface. The study by Chang showed that the hydrogen bond between HNO3 and TiO2 can enhance the adsorption energy and the stability of the adsorption configuration[15]. It is observed that the adsorption configuration can be stabilized by the formation of hydrogen bonds.

Figure 1

The adsorption structures of ornidazole on the TiO2(101) and (001) facets under vacuum conditions.

From Table 1, can be observed that under the vacuum condin class="Chemical">tions, A1 is the most stable adsorption configuration on the TiO2(101) surface. For A1 mode, the N(3) atom adsorbed on the Ti(5) atom, and the H atom of the methyl moiety and the C(2) atomic branch form hydrogen bonds with the O(2) atom on the TiO2(101) plane. The adsorption distances are 2.341, 2.073 and 2.422 Å, respectively. Due to the interaction of the ornidazole molecule with the surface of TiO2, some bond lengths are changed. C(2)-N(3) and N(3)-C(4) in the imidazole ring change from 1.335 and 1.354 Å to 1.352 and 1.361 Å, respectively, and the C(2)-N(3)-C(4) bond angle changes from 106.1°to 107.3°. The bond length of C(2)-N(3) increases even more than the N(3)-C(4), which means that the process of adsorption make C(2)-N(3) more unstable and favors the attack of the hydroxyl radicals.

Similarly, Table 1 shows that under vacuum condin class="Chemical">tions, a1 is the most favorable configuration with the highest adsorption energy about 2.83 eV. In a1 configuration (Fig. 1), the N(3) atom adsorbed on the Ti(5) atom and the H atom on the C(2) atomic branch of ornidazole adsorbed on the O(2) atom. The adsorption distances are 2.267 and 2.444 Å, respectively. The C(2)-N(3) bond length in the imidazole ring has been greatly changed due to the adsorption, increasing from 1.335 Å to 1.346 Å. This result indicates that the stability of C(2)-N(3) bond weakens, which favors the attack of the hydroxyl radicals and ring opening degradation.

Adsorption under solvent conditions

To take into account the adsorpn class="Chemical">tion characteristics of the ornidazole molecule on the TiO2 crystal surface under solvent conditions, we used the same method to optimize the stable adsorption structures of ornidazole on the TiO2(101) and (001) crystal facets under solvent conditions.

Adsorption under neutral conditions

The modes of B1~B5 and n class="Gene">b1~b5 are shown in Fig. 2, under neutral solvent conditions. The adsorption of ornidazole on the TiO2 surface is still multisite adsorption. Due to the addition of the water solvent model, the H atoms of H2O molecules form hydrogen bonds with O atoms on the crystal surface, and the O atoms of H2O molecules and Ti atoms form Ti-O and Ti-OH bonds on TiO2(101) and (001) surfaces, respectively. The degree of deformation of the crystal facets is greater than that under vacuum conditions to maintain the stability of the adsorption configuration. In terms of the adsorption energies (Table 1), the B5 and b1 configurations are the most stable structures of ornidazole on the anatase TiO2(101) and (001) crystal facets, which are 2.45 and 2.64 eV, respectively. The adsorption characteristics of B5 and b1 are similar to those of the A1 and a1 configurations, and the stability of C(2)-N(3) bond tends to be weak and is susceptible to attack by hydroxyl radicals. After adsorption the N(3)-C(2) bond length become longer compare to vacuum conditions. In the solvent conditions, H2O molecules are revolved around ornidazole, there may be strong interactions between H2O molecules and the ornidazole molecule. Meanwhile, the adsorption energy increase relative to the vacuum conditions. Zhang[16] et al. studied the adsorption of CO atoms on the CuCl(111) surface in solvent condition. Mendive[17] studied the adsorption of oxalate on anatase(100) and rutile(110) in aqueous solution. The water solvent stabilized the adsorption structure and also illustrates the effect of water solvent on the adsorption energy of the surface.

Figure 2

The adsorption structures of ornidazole on the TiO2(101) and (001) facets in neutral conditions. The H2O molecules are represented by bond line notation.

Adsorption under acidic conditions

Figure 3 shows the adsorption distances and sites of n class="Disease">C1~C5 and c1~c5 configurations under acidic conditions. Due to the interactions of the ornidazole molecule, water molecules, proton and chloride ion with TiO2, a subtle deformation of the TiO2 crystal plane occurs. As shown in Table 1, in terms of the adsorption energy, C1 mode is the most stable configuration under acidic conditions. The adsorption properties of C1 are similar to those of A1 except that more hydrogen bonds have formed. The c2 configuration has the largest adsorption energy, 2.89 eV, and is the most stable adsorption configuration of ornidazole on the TiO2(001) surface under acidic conditions. In the c2 configuration, the N(3) atom of ornidazole is not adsorbed on the Ti(5) atom. However, by investigating the bond lengths of the c2 configuration, we found that the bond lengths of C(2)-N(3) and C(4)-C(5) increase after adsorption from 1.335 and 1.384 Å to 1.354 and 1.398 Å, respectively. The length of C(2)-N(3) is longer than that of C(4)-C(5). At the same time, we also analyzed the other four configurations and found that the bond lengths of the ornidazole molecule change differently and that the C(2)-N(3) bond length obviously increases, disclosing adsorption makes the stability of C(2)-N(3) weaker and more susceptible to attack by hydroxyl radicals.

Figure 3

The adsorption modes of ornidazole on the TiO2(101) and (001) facets in acid conditions. The H2O molecules are represented by bond line notation, and the Cl atom is represented by green circles.

Adsorption under alkaline conditions

As demonstrated in Fig. 4, D1~D5 and d1~d5 are five adsorption n class="Chemical">configurations of ornidazole on the TiO2(101) and (001) facets under alkaline conditions, respectively. From Table 1 we observe that D5 (adsorption energy of 2.52 eV) is the most stable adsorption configuration of ornidazole on the TiO2(101) surface. Similarly, in terms of the adsorption energy (shown in Table 1), d5 (2.89 eV) is the most stable adsorption configuration of ornidazole on the TiO2(001) surface. The adsorption properties of the D5 and d5 configurations are also similar to those of A1 and a1 under vacuum conditions, except that in the d5 structure, more hydrogen bonds form and the O atom in the hydroxyl moiety interacts with Ti(5). Adsorption also makes the stability of C(2)-(N3) weaker and thus susceptible to attack by hydroxyl radicals and ring-opening degradation.

Figure 4

The adsorption modes of ornidazole on the TiO2(101) and (001) facets in basic solution. The H2O molecules are represented by bond line notation, and the Na atom is represented by purple circles.

By analyzing the adsorption energy and adsorpn class="Chemical">tion configuration of the ornidazole molecule on the TiO2 crystal surface under vacuum and aqueous conditions, we found that the adsorption configuration is more stable under aqueous conditions. The adsorption of ornidazole on the TiO2 surface is affected by the intermolecular surface tension and hydrogen bonding. After adsorption, the crystal surface is slightly deformed due to the influence of the ornidazole molecule, water molecules, proton and ion on the crystal plane of TiO2. We also found that when the ornidazole molecule adsorbed on the TiO2(001) crystal plane, the degree of deformation of the crystal plane is much greater than that of the (101) plane under vacuum or aqueous solution conditions, which may be related to the fact that the anatase TiO2(001) crystal plane has more unsaturated titanium ions and a higher surface activity[18-20]. Therefore, the (001) surface may be more favorable for photocatalysis. Additionally, the overall adsorption energy of ornidazole is found to be the highest under acidic conditions. The isoelectric point of TiO2 is 6.3[21], which indicates that the positive charge on the surface of TiO2 is beneficial to the adsorption of the ornidazole molecule when the pH is less than 6.3. In contrast, the negative charge on the surface of TiO2 is not conducive to the adsorption of the ornidazole molecule. The results may provide a certain reference for the degradation conditions of ornidazole.

On the basis of the characteristics of the molecular adsorpn class="Chemical">tion structure, we found that the most stable adsorption configuration of ornidazole on two surfaces of TiO2 is the N(3) atom adsorbed on the Ti(5) atom. After the ornidazole adsorbed on TiO2 surface, the bond length of C-N much longer. Thus, according to the adsorption results, it is reasonable to speculate that the ring-opening reaction site of ornidazole is the C-N bond[22-24].

Electronic structure

To further investigate the interacn class="Chemical">tion and bond characteristics of the ornidazole molecule with the TiO2 crystal plane, we calculated the density of states (DOS), projected density of states (PDOS), electron density, and Milliken atomic charge of adsorption configurations under vacuum and aqueous conditions. The DOS and PDOS of the TiO2(101) and (001) facets consist of the 2p and 3d valence bands (VB) of O and Ti, while the conduction bands (CB) are primarily composed of the 3d orbital of Ti.

The DOS and PDOS of the ornidazole-adsorbed n class="Chemical">TiO2 surface under vacuum conditions are giving in Fig. S2 and Fig. S3. From these figures we found that the s-orbital composition of the TiO2(001) plane is even more than that of the TiO2(101) plane. For semiconductor photocatalytic materials, the electronic transition between the CB and VB is affected by the energy gap. If the energy gap is in the visible light range, visible light can be effectively utilized. Therefore, the energy gaps of different crystal plane adsorption configurations, which are the differences between the highest occupied molecular orbital (HOMO) and lowest unoccupied molecular orbital (LUMO) energies, can be used to judge the utilization of visible light. By calculating the energy gap, their values are the difference. The calculated energy gap of bulk TiO2 is 2.87 eV, which is close to the experimental value of 3.20 eV[25]. After adsorption, the energy gap became narrower. The energy gap values of A1~A5 are 2.03, 2.27, 1.94, 1.96, and 2.00 eV, respectively. In the structures of a1~a5, the energy gap values are 1.98, 1.61, 1.75, 1.56, and 2.03 eV, respectively. The electronic transition wavelength between the VB and the CB corresponds to visible light (the visible photon energy gap range is approximately 1.7~3.1 eV)[26,27], demonstrating that using visible light to drive the degradation of ornidazole on TiO2 surface is effective.

The DOS and PDOS of adsorption n class="Chemical">configuration under neutral aqueous conditions are plotted in Figs S4 and S5. The band structure of TiO2 changes due to the action of H2O molecules on TiO2 surface, in the water solvent conditions. After adsorption, the Ti 3d states still govern the CB edge, and the s-orbital component of the VB energy level is increased. Two peaks of s orbital form between −21 eV and −15 eV, and the energy range of the p orbital is broadened from −5~0 eV to −8~0 eV. From −8~0 eV, two sets of peaks appear, in which the peak height and peak area are increased compared to that of pure TiO2. The increase in the s-orbital and p-orbital components elucidates that the 1 s orbital of the H atom and the 2p orbital of the O atom in the H2O molecules participate in hybridization. The s orbital appears near the Fermi level, which corresponds to the HOMO orbital of the system. When the number of electrons in the HOMO or LUMO orbital increase, the electron donating ability of the system also increase, showing that the chemical activity of TiO2 is improved. As well, the TiO2(001) surface has more p-orbital components, indicating that there may be more 2p orbitals of O in the H2O molecules involving in the hybridization and that the chemical activity of the TiO2(001) surface is greater than that of the (001) plane. The TiO2 energy gap is narrowed after adsorption. The energy gaps of B1~B5 are reduced to 2.313, 2.153, 2.121, 2.331, and 2.251 eV. The b1~b5 energy gaps are reduced to 2.127, 1.704, 2.005, 2.029, and 2.077 eV, respectively. The above energy gaps all in the visible light range, showing that the TiO2 surface can effectively utilize visible light under water solvent conditions.

The DOS and PDOS for the adsorption of n class="Chemical">ornidazole on anatase TiO2(001) and (001) facets under acidic conditions are shown in Figs S6 and S7, respectively. Clearly, the TiO2 band structure is similar to that of the neutral solution. The energy gap is narrower after adsorption than that of pure anatase TiO2. The C1~C5 energy gaps are reduced to 2.301, 2.306, 1.900, 2.052, and 1.162 eV, respectively. The light absorption frequency is reduced, except for the C5 configuration, and they are all in the visible wavelength range. The energy gaps of c1~c5 are 1.789, 1.824, 1.722, 2.131, and 1.958 eV, respectively, which are in the visible light range. These results show that, under acidic conditions, the TiO2 crystal surface can effectively use visible light.

The DOS and PDOS of adsorbed-TiO2 under alkaline n class="Chemical">conditions are shown in Figs S8 and S9, respectively. The band structure is similar to that of the neutral conditions. Adsorption results in the narrowing of the TiO2 energy gap. Specifically, the D1~D5 energy gaps are reduced to 2.325, 1.978, 1.640, 2.327, and 2.336 eV, respectively, and the d1~d5 energy gaps are 1.990, 2.043, 1.700, 1.932 and 1.930 eV, respectively. All of the energy gaps are in the visible range, and thus, the TiO2 crystal plane can effectively use visible light, under basic conditions.

Figure 5 shows the electron density of ornidazole on the n class="Chemical">TiO2 crystal surface under vacuum conditions. We observed an overlap between the charge density of the imidazole ring and the TiO2 surface. From Table S1, we can see that under different conditions, the number of electrons on the imidazole ring increases after adsorption, which shows that the electrons of the crystal surface have shifted to the imidazole ring during the adsorption process. These results demonstrate that electron transfer occurs between the imidazole ring and TiO2 surface and that a new chemical bond is formed. During the process of adsorption, the ornidazole molecule interacts with the surface of TiO2 and undergoes chemical adsorption.

Figure 5

Electronic configurations of ornidazole on TiO2(101) and (001) facets.

Conclusion

In this work, DFT was used to study the adsorption characterisn class="Chemical">tics of ornidazole on the anatase TiO2(101) and the (001) facets under different conditions. The result showed that ornidazole can absorb on the TiO2 surface in vacuum or aqueous solution conditions, especially acidic conditions. After adsorption the bond length of C-N in the imidazole ring becomes longer, which is conducive to the attack and ring-opening degradation of the hydroxyl radicals. Through the molecular adsorption structure change characteristics, we found that the reaction site of degradation is the ring-opening of the C-N bond on the imidazole ring. At the same time, the hydrogen bonding played a role in the process of ornidazole adsorbed on the surface of TiO2. Compared with vacuum conditions, the hydrogen bonding effect in the adsorption process under aqueous conditions is more significant for the change in the adsorption characteristics. For different conditions, we found that the adsorption wavelengths of the electronic transition between the VB and CB of each adsorption configuration on the TiO2(101) and (001) crystal facets correspond to visible light. Our results reveal that the TiO2 can effectively use visible light and can be used as a photodegradation catalyst for ornidazole.

Methods

The anatase TiO2(101) and (001) crystal facets were invesn class="Chemical">tigated in this paper. From Fig. 6, it is can be observed that the surface of TiO2 show 5-fold and 6-fold coordinated Ti atoms (Ti(5) and Ti(6)), as well as 2-fold and 3-fold coordinated oxygen atoms (O(2) and O(3)). Notably, Ti(6) site does not exist in TiO2(001) surface layer. Based on a preliminary study of the effect of the plate thickness on the surface energy, when the (101) surface adopts a three-layer model[28] and the (001) surface adopts a layer model[29,30], the calculation time and accuracy can be balanced. To avoid the interaction between the molecule and the plate, a 15 Å vacuum layer in the Z direction was added. The (1 × 3) supecell and (3 × 3) supecell were used for antase TiO2(101) and (001) surfaces with a (TiO2)36 composition. The corresponding surface areas are 10.886 Å × 11.328 Å and 11.328 Å × 11.328 Å on the (101) and (001) surfaces of TiO2, respectively. In neutral aqueous solution, under the Universal force field and according to the density of 1 g/cm3, 48 and 69 H2O molecules are approximately added on the surfaces of TiO2(101) and (001), respectively. In acidic (basic) conditions, one H2O molecule was replaced by with a molecule of HCl (NaOH)[31].

Figure 6

The model of anatase TiO2(101) and (001) crystal facets.

Placing the ornidazole molecule on the n class="Chemical">TiO2(101) and (001) crystal facets, the distance between them was set to approximately 3.8 Å to avoid a strong interaction, and then we introduced the reactive force field (ReaxFF) and NVE ensemble under the LAMMPS program to perform a molecular dynamic calculation[32,33]. Based on the LAMMPS relaxation results, the local minimum structure was selected for further optimization by DFT.

The DFT calculation was performed using the n class="Chemical">DMol3 code of the MS package[34]. DMol3 applied the dual digital base group and polarization function to extend the electronic wave function and all structural optimization was performed on the basis of spin-polarized plane waves. The Kohn-Sham one-electron equations were solved in the generalized gradient approximation (GGA) by using the Perdew-Burke-Ernzerhof (PBE) functional[35], and the effective core potentials (ECP) was used to describe the core electrons. The polarized DNP[36] basis set was used to describe the atomic orbitals and the cutoff radius was set to 4.5 Å. For the calculation of the adsorption results, the convergence criterion is set to the following criteria: the energy was smaller than 2 × 10−5 Ha, the force was below 4 × 10−3 Ha/Å, and the max displacement was 5 × 10−3 Å. In addition, the self-consistent field (SCF) iterative energy tolerance was set to 1 × 10−5 Ha, and the multipole expansion was performed by the octupole moment.

The adsorption energy (E) is defined aswhere E is the free energy for the ornidazole molecule absorbed on TiO2 surface, E is the energy of the TiO2 surface, and E is the energy for the ornidazole molecule.

The lattice parameters of bulk anatase TiO2 optimized by the above method are a = b = 3.776 Å, and c = 9.486 Å, which are consistent with the experimental values of a = b = 3.785 Å and c = 9.514 Å[37,38]. The agreement shows that our calculation method and results are reliable.

Supplementary Dataset 1