Hydrolysis Mechanism of Bismuth in Chlorine Salt System Calculated by Density Functional Method

Based on the density functional theory, this paper presents the calculated cellular electronic properties of BiCl3, BiOCl and Bi3O4Cl, including unit cell energy, band structure, total density of states, partial density of states, Mulliken population, overlapping population, etc. Combined with the thermodynamic analysis of Bi hydrolysis process in chlorine salt system, the conversion mechanism of oxychloride bond in BiCl3 to form BiOCl and Bi3O4Cl by hydrolysis, ethanololysis and ethylene glycol alcohololysis was obtained by infrared spectroscopy. The results indicate that the energy of Bi3O4Cl cell system was lower than that of BiOCl cell, indicating that the structure of Bi3O4Cl was more stable. From the analysis of bond fluctuation, the electron nonlocality in BiOCl belt was relatively large, and the orbital expansibility was strong; thus the structure of BiOCl was relatively active. The state density map of Bi3O4Cl had the widest energy gap, i.e., the covalent bond between Bi3O4Cl was stronger than BiOCl. Therefore, the hydrolysis of BiCl3 would preferentially generate Bi3O4Cl with a more stable structure. The number of charge arrangement, overlapping population and infrared spectrogram indicate that there were two basic ways in the hydrolysis and alcoholysis of BiCl3. Firstly, two chlorine atoms in BiCl3 were replaced by hydroxyl groups ionized by water and alcohol to form [Bi(OH)2Cl] monomer, and BiOCl and Bi3O4Cl were formed by intra-molecular dehydration or inter-molecular dehydration. The other way was that the Bi atom directly reacted with the OH ionized by water and alcohol to form the [Bi-OH] monomer, and the Cl atom replaced the H atom on the hydroxyl group in the [Bi-OH] monomer to further form BiOCl and Bi3O4Cl.

oxychloride to form the bismuth oxide [21][22] have been extensively reported. However, the mechanism of bismuth oxide hydrolysis preparation by bismuth chloride compound photo catalyst has not been reported. The present study was thus motivated.
To explore the element hydrolysis mechanisms for the preparation of bismuth oxychloride, in this paper, electronic structure of BiCl3, BiOCl, Bi3O4Cl was calculated using density functional method. The formation mechanisms was explored from the respects of cell structure, band structure, density of states, charge layout number and overlapping inhabit in BiCl3 basic reaction and process of hydrolysis, alcohol solution, and further confirmed by infrared spectrum from the perspective of valence change.

Structure design and calculation of bismuth compounds
Based on the first principle density functional theory (DFT), combined with the CASTEP [23][24] module of the planar pseudopotential method, the cell structure of bismuth compounds was optimized, and the energy band structure, total state density and separation density, charge arrangement number and overlap polymerization number were calculated. BiCl3, BiOCl and Bi3O4Cl cell models were established according to relevant parameters shown in Table 1. The exchange effect of electronelectron interaction between crystal cells was corrected by general gradient approximation (GGA). PBE in GGA was adopted to deal with the interaction correlation energy between electrons. The grid points of k-space were selected by the Monkhorst-Pack scheme, and the total energy and charge density of the system were integrated in the Brillouin zone. The k-vectors of the Brillouin zone was selected as 1×2×2, 5×5×2, and 5 × 5 × 4; plane wave truncation could be set to 258.5 eV, 489.8 eV and 489.8 eV, respectively. The self-consistent precision was set to be 2.0 × 10 -6 eV / atom, and the force acting on each atom did not not exceed 0.05 eV /nm.

Infrared spectrum analysis -Bi 3+ hydrolysis experiment in chlorine salt system
BiCl3 in two solid and liquid states was hydrolyzed and alcoholylyzed in different systems. BiCl3 solid powder and its solution (0.17 mol/LBi 3+ , 1 mol/L Cl -) were mixed with the same amount of deionized water, ethanol and ethylene glycol at 25℃ (water bath) for 2 h. Then the solutions were adjusted to pH=4 and treated in the ultrasonic cleaner ultrasonic for 1 hour. The precipitation was achieved by centrifugal method and filtrated with repeated washing, and the product was obtained after drying at 60℃ for 6 h. All the experiments were performed by blank experiment, i.e., to determine the infrared spectrum of the same volume of deionized water, ethanol, ethylene glycol and hydrochloric acid.

First principle analysis of bismuth compounds 3.1.1 Energy analysis of bismuth compounds
The until cell structure of BiCl3, BiOCl and Bi3O4Cl from structure optimization and energy calculation are shown in Table 2. It has been reported that the lower the total cell energy, the more stable the cell structure [25][26][27]. The cell energy of Bi3O4Cl was lower than that of BiOCl. Therefore, Bi3O4Cl was preferential to form stable structure when BiCl3 was hydrolyzed. https://doi.org /10.37358/Rev. Chim.1949 Rev. Chim., 71 (6)

Band analysis of bismuth compounds
As shown in Figure 1, BiCl3 had a band width of 37.2 eV and a forbidden band width of 3.996 eV; BiOCl had a band width of 38.8 eV and a forbidden band width of 2.707 eV; while Bi3O4Cl had a band width of 40.5 eV and a forbidden band width of 2.704 eV.
The wider the width of the energy band was, the larger the undulation was, the smaller the effective mass of the electrons in the energy band was, and the larger the degree of non-locality was, the stronger the atomic orbital scalability of the energy band was ,and the more active nature was. On the contrary, the narrower band indicates that the eigenstate corresponding to this band was mainly composed of atomic orbitals of a certain grid point in the local area. The electron locality of this band was very strong, the orbital expansion was weak, and the nature was stable [28][29].
Therefore, it can be seen from Figure 1 that the energy bandwidth of BiOCl was smaller than the bandwidth of Bi3O4Cl, and the undulation of the BiOCl band was relatively larger than that of Bi3O4Cl. Therefore, in terms of band width, BiOCl was narrower, the electron locality of the band was stronger, the orbital expansion was weak, and the property was relatively stable. From the band undulation, Bi3O4Cl had a small degree of undulation and could carry electrons. The degree of nonlocality was small, the orbital expansion was weak, and the nature was relatively stable. The stabilities of BiOCl and Bi3O4Cl would be further analyzed.   Figure 2 shows that the valence band (-21.9-0 eV) of BiCl3 was mainly formed by the electron states of Bi 6s6p and Cl 2s2p; the conduction band (0-15.3 eV) was excited by the electron states of Cl 2p and Bi 6p, and the peak value at the Fermi energy level was mainly associated to the electron orbitals of Cl 2p and Bi 6p.

Analysis of bismuth compounds about density of state
Regarding the BiOCl, the valence band (-21.9-0 eV) was mainly formed by the electronic states of Bi 6s6p5d, O 2s2p and Cl 2s2p, while the conductance band (0-16.9 eV) was assigned to the electronic states of Bi 6s6p5d, O 2s2p and Cl 2s2p.
Regarding the Bi3O4Cl, the valence band (-22.4-0 eV) was mainly formed by the electron states of Bi 6s6p, O 2s2p and Cl 2s2p, and the conduction band (0-18.1 eV) was assigned to the electron states of O 2p and Bi 6s6p. The peak value at the Fermi level was mainly contributed by the electron orbitals of Cl 2p, O 2p and Bi 6s6p.
Because the size of the pseudo gap (the peak and valley of the low-energy bonding state and the high-energy anti-bonding state are defined as the pseudo gap) of the state density map can reflect the strength of covalent bonds. The wider the pseudoenergy gap is, the stronger the covalency is. The larger the horizontal coordinate of the peak state density is, the easier it is for the electrons outside the nucleus to be distributed in the high energy region, and the easier it is to lose electrons; otherwise, the easier it is to gain electrons [30][31].
Therefore, according to the state density diagram in Figure  Comparing the pseudoenergy gap width of BiCl3, BiOCl and Bi3O4Cl, viz. BiCl3<BiOCl<Bi3O4Cl, the covalent bond between Bi3O4Cl atoms was stronger than BiCl3 and BiOCl. This suggested that BiCl3 hydrolysis was more likely to produce relatively stable Bi3O4Cl.

Analysis of the charge layout of bismuth compounds
The number of charge layouts can reflect the gain and loss of atomic electrons. A positive charge indicates the loss of electrons, and a negative charge indicates the gain of electrons. The gain and loss of electrons can feedback the strength of the bond interaction between atoms. The more electrons are transferred, the stronger the bond interaction between atoms will be, and vice versa [32]. Table 3 shows that each BiCl3 crystal cell contained 12 Cl atoms, among which 8 Cl atoms got 0.42 electrons and 4 Cl atoms got 0.45 electrons respectively. Four Bi atoms, each of them lost 1.29 electrons. Each Bi atom lot an electron from two Cl atoms that gained an electron of 0.42 and one Cl atom that gained an electron of 0.45. The more electrons are transferred, the stronger the interaction between atomic bonds will be. Therefore, in BiCl3 structure, the interaction between the two groups of [Bi-Cl] bonds was weaker than that of the other group. Therefore, BiCl3 preferentially would break up two groups of [Bi-Cl] bonds with weak interaction during hydrolysis to form Bi(OH)2Cl.
BiOCl cell contained 2 groups [BiOCl], in which each Bi atom lost 1.48 electrons, each Cl atom gained 0.56 electrons, and each O atom gained 0.92 electrons. The electrons lost by each Bi atom were gained by one Cl atom and one O atom. The more electrons are transferred, the stronger the bond interaction between atoms will be; thus, the bond interaction between [Bi-O] was stronger than that between [Bi-Cl], which was easy to remove Cl ions in the later stage, and to refine Bi2O3 or Bi powder. According

Analysis of overlapping concentration number of bismuth compounds
The overlapping population can be used to express the interaction between atoms, analyze the bonding properties between atoms, and identify the bonding strength between atoms. When the number of overlapping population is positive, the bonding between atoms is covalent bond. The larger the value is, the stronger the covalent bond is and the more stable the structure is. When the overlapping population is negative, the bonding between atoms is antibonding. The smaller the value is, the stronger the repulsion between atoms is, and the worse the stability of crystal cells is. When the overlap concentration number is 0, there are ionic bonds between atoms [33][34][35]. The overlapping population of BiCl3, BiOCl and Bi3O4Cl are shown in Table 4.
The positive overlapping population of BiCl3 indicates that the chemical bond between the Cl atom and the Bi atom was covalently bonded. The population of the four groups of Bi-Cl bonds was 0.30, and the population of the eight groups of Bi-Cl bonds was 0.28. The larger the population, the stronger the stability of the covalent bond. Each [BiCl3] unit contained a Bi-Cl bond with a population of 0.30 and two Bi-Cl bonds with a population of 0.28; thus, hydrolysis occurred when BiCl3 was dissolved in water, followed by that the hydroxide generated by water ionization was replaced. Two of the Cl atoms in the Bi-Cl bond with a population of 0.28 formed Bi(OH)2Cl, which further formed BiOCl, which was consistent with the above-mentioned charge distribution number analysis.
The positive overlapping population of BiOCl meant that the chemical bonds between O and Bi atoms were covalently bonded, i.e., the total overlap population was 1.12. The overlapping population of O-O was -0.23 (<0), which meant that the O-O bond formed an anti-bond, i.e., the two O atoms were mutually exclusive. The smaller the negative value, the stronger the inter-atomic repulsive force. The stability of the unit cell was therefore lower.
It is known from the overlap of Bi3O4Cl that the O-Bi bond can form a covalent bond or an antibond. The 24 groups of O-Bi bonds were covalently linked, and the total overlap population were 4.2. The anti-bonds were formed between the 4 groups of O-Bi bonds, and the total overlap population was -0.04. The negative overlap of 10 groups of O-O bonds was less than 0, indicating that the 10 groups of O-O bonds were formed with anti-bonds, i.e., the total overlap population was -0.66. The smaller the overlapping population of the anti-bonds, the atoms representing the anti-bonds were received in the unit cell would suffer greater the repulsive force, the more unstable the unit cell.
Comparing the size and number of overlapping populations of BiOCl and Bi3O4Cl, we can see that the total number of overlapping populations of BiOCl covalent bonds was 1.12, the total number of overlapping populations of anti-bonds was -0.28, the total number of overlapping populations of covalent bonds, and the overlap of anti-bond. The sum of the total number of settlements was 0.84, and the effect of covalent bonds was 4 times that of reverse bonds [36][37]. The greater the role of covalent bonds, the more stable the structure; the total number of overlapping settlements of Bi3O4Cl covalent bonds was 4.20. The sum of the numbers was -0.70, the sum of the number of overlapping settlements of covalent bonds, the number of overlapping settlements of anti-bonds was 3.50, and thus, the effect of covalent bonds was 6 times that of reverse bonds. It can be seen that Bi3O4Cl had a stronger covalent bond between atoms than BiOCl, and the interaction force between atoms was large, i.e., the stability of the unit cell Bi3O4Cl was higher BiOCl, and a series of Bi (OH) 2Cl would be generated during the hydrolysis of BiCl3. It was easier to continue to remove water to generate Bi3O4Cl. In summary, the energy of Bi3O4Cl was lower than that of BiOCl, the width of constraint energy gap was: BiOCl<Bi3O4Cl, which suggested the covalent bond between Bi3O4Cl atoms was stronger than that of BiOCl, and BiCl3 was more likely to form more stable Bi3O4Cl. The number of charge distribution shows that BiCl3 was hydrolyzed. In the process, the two bonds with weak bond interaction [Bi-Cl] were preferential to be broken to form Bi(OH)2Cl; the bond between [Bi-O] in BiOCl and Bi3O4Cl iwas stronger than [Bi-Cl], and the Cl atoms were thus easier to be removed in the later stage, and the Bi2O3 or Bi powder was easier to be refined. The overlapping populations of the overlapping groups / unit covalent bonds of the two unit counter bonds were further compared: Bi3O4Cl>BiOCl. This indicated that a series of Bi(OH)2Cl produced in the hydrolysis process of BiCl3 could easily continue to remove a molecule of water to generate Bi3O4Cl.
In order to understand whether the fracture and formation process of valence bond during BiCl3 hydrolysis was consistent with the calculated results, the thermodynamic analysis of Bi 3+ hydrolysis process under chlorine salt system was conducted in the designed experiment, and the hydrolysis path of BiCl3 and the formation mechanism of chloro-oxygen valence bond were further analyzed by infrared spectroscopy to verify the calculated results.

Thermodynamic analysis of Bi 3+ hydrolysis process in chloride system
In the Bi 3+ -Cl-H2O system, Bi 3+ was hydrolyzed at a lower pH, resulting in multiple solid phase intermediates including BiOCl, Bi3O4Cl, Bi2O3, and Bi(OH)3. Controlling the appropriate reaction conditions could enhance Bi 3+ to form a series of stable hydrolysates.
The stability constants of bismuth, chlorine and hydroxide ions and the standard formation molar free energy of related substances by software HSC and FactSage are listed in Table 5  The reaction of Bi 3+ and Clto form complex ions in Bi 3+ -C-H2O system is expressed by formula (1). The reaction of Bi 3+ with OHforming complex ions is represented by formula (2); Bi 3+ and Clformation and OHforming the complexing constants of the complex ions are shown in Table 6.   (11) where [Cl -] T 0 and [Bi 3+ ] T 0 were the total concentration of bismuth and chlorine, respectively. 1)equilibrium of BiOCl solution: From the reaction (3), it was known that 1 mol of bismuth ion and 1 mol of chloride ion were required to form 1 mol of BiOCl; thus we could obtain the following equation: -[Cl -] T (12) By substituting equations (10) and (11) into equation (12), we could obtain: , which was a constant; Substituting the reaction formula (3) into the formula (9), we could obtain: 2)equilibrium of Bi2O3 solution: Similarly, when pH≥2, [Cl -] was approximately equal to [Cl -] T 0 , which was also a constant; Substituting the reaction formula (6) into the formula (9), equation (15) can be obtained: 3)equilibrium of Bi3O4Cl solution: The formation of 1 mol of Bi3O4Cl required 3 mol of bismuth ions and 1 mol of chloride ions, shown as follows, , which was a constant. Substituting the reaction formula (7) into the formula (9), then:
Substituting the reaction formula (8) into the formula (9), then: When the total concentration of bismuth and the total concentration of chlorine were given, the relationship between pH and lg(Bi 3+ ) was made by the above formulas (14), (15), (17) and (18), as shown in Figure 3. The figure shows the equilibrium line between the solid phase and the liquid phase. The area above the curve was the solid phase stability zone. The area below the curve was the liquid phase stability zone. It can be divided into four solid phase stability zones, namely BiOCl, Bi2O3, Bi(OH)3 and Bi3O4Cl. In the Bi 3+ -Cl-H2O system, when the control 3<pH<5, stable BiOCl and Bi3O4Cl could be formed, so that the Bi 3+ hydrolysis verification experiment in the chloride salt system was chosen to adjust the pH to 4. of hydrazine hydrolysis in chloride system

Analysis of bismuth hydrolysis mechanism under chlorine salt system by infrared spectroscopy
The filtrates of BiCl3 hydrolytic action, alcoholysis reaction and alcoholysis reaction with ethylene glycol were characterized by infrared spectrum, and blank experiment was performed for comparative analysis to verify the reaction path of BiCl3 in the hydrolysis process and the conversion mechanism of chlorine oxygen [38][39]. The results are shown in Figure 4 to Figure 7, and the characteristic infrared peaks are shown in Table 8.

Infrared spectroscopy analysis of BiCl3 solid hydrolysis in Bi 3+ -Cl-H2O system
It can be seen from curves A and B in Figure 4 that, a peak occurred at 3313.21 cm -1 assigned to O-H stretching vibration, and a peak occurred at 1643.38 cm -1 assigned to bending vibration of O-H molecules. On the one hand, due to the addition of BiCl3 and its hydrolysis, the degree of hydroxyl ionization in water was strengthened, the number of free hydroxyl groups in water was increased, and the concentration of hydroxyl groups was relatively large. On the other hand, due to the ionization of BiCl3 after BiCl3 was added, Bi atom replaced H atom of water ([H-OH]) to form a [Bi-OH] monomer. In the [Bi-OH] monomer, there was a hydrogen bond between the oxygen atom in the OH and another water molecule, which was not easy to be broken; the electronegativity of chlorine was 3.16, the electronegativity of hydrogen in water was 2.1, and free Cl ions were generated in water. It was easy to replace the hydrogen atom in the water hydroxyl group to form [Cl-O-Bi], which was BiOCl, and the Bi atomic nucleus was larger than the H nucleus. It was easy to form Bi[OH]3 with the hydroxyl group generated by water ionization. Since Bi[OH]3 was unstable, it would continue to hydrolyze to form BiOCl or Bi3O4Cl. Cl atom was replaced by the H atom in the water hydroxyl group, and therefore, the electron cloud density increased, the force constant k increased, and the induction effect occurred. The group frequency shift to a high wave number, and correspondingly, the infrared spectrum of the water had a red shift. The stronger the electronegativity of the element, the stronger the induction effect, and the more obvious the shift of the position of the absorption peak to the high wave number [40][41].
Comparing curves A and B in Figure 4, the absorption peak at 1643.38 cm -1 only shift to the peak by https://doi.org /10.37358/Rev. Chim.1949 Rev. Chim., 71 (6)  0.25 cm -1 , and the absorption peak at 3313.21 cm -1 shift by 9.22 cm -1 , which demonstrates that the red shift of the absorption peak at 3313.21 cm -1 was not only due to the increase of the hydroxyl group concentration in the solution, but also due to that the chlorine replaced the hydrogen in the water hydroxyl group to induce an effect.

Infrared spectroscopy analysis of BiCl3 solid hydrolysis in Bi 3+ -Cl-C2H5OH system
Comparing curves C and D in Figure 5, the absorption peak at 3316.10 cm -1 shift to 3.76 cm -1 at the peak region, and the absorption peak at 636.44 cm -1 shift to the low peak region by 3.29 cm -1 , this was resulted from that the H on the -OH in ethanol was replaced by Cl, which increased the electron cloud density and the force constant k, and induced an effect. Therefore, the group frequency at 3316.10 cm -1 shift to a high wave number, and thus, the infrared spectrum of ethanol red-shift. The electronegativity of chlorine was relatively larger than that of hydrogen. The electronegativity of carbon was 2.55, the electronegativity of oxygen was 3.44, the electronegativity of hydrogen was 2.1, and the electronegativity of chlorine was 3.16; so it would replace -OH. After the upper H, a monomer such as [C-O-Cl] was formed. The greater the difference in the electronegativity between the two ends of the bond (the greater the polarity), the stronger the absorption peak, the stronger the polarity, the red shift of the absorption peak. The weaker the polarity, the blue shift of the absorption peak. O-Cl was weaker than -OH, and therefore, the absorption peak at 636.44 cm -1 shift to the low peak region, and blue shift occurred, which proves that H atom on -OH was replaced by Cl atom. Since the alcoholysis of BiCl3 was slow in ethanol, ammonia water was added to BiCl3+C2H5OH system to promote alcoholysis [42][43][44]. Comparing curves E and F in Figure 5, the peak at 1642.82 cm -1 was excited by stretching vibration of NH-NH3, wherein the absorption peak at 3358.72 cm -1 and the absorption peak at 562.79 cm -1 were red at the peak. The shift of 5.98 cm -1 and the blue shift of 18.99 cm -1 at the low peak further confirmed the substitution of BiCl3 in ethanol. https://doi.org /10.37358/Rev. Chim.1949 Rev. Chim., 71 (6)

Infrared spectroscopy analysis of BiCl3 solid hydrolysis in Bi 3+ -Cl-(CH2OH)2 system
In order to more clearly understand the mechanism of chlorine and oxygen regulation in the hydrolysis process of BiCl3, it was added to prove whether BiCl3 could undergo alcoholysis in ethylene glycol. Comparing curves G and H in Figure 6, it can be seen that 3297.97 cm -1 blue-shift by 4.93 cm -1 to the low peak. This was because the electronegativity of chlorine was relatively larger than that of hydrogen, and the electronegativity of carbon was 2.55. The electronegativity was 3.44, the electronegativity of hydrogen was 2.1, and the electronegativity of chlorine was 3.16. Therefore, after hydrogen was replaced by -OH, a monomer such as [C-O-Cl] was formed. The greater the difference in the electronegativity between the two ends of the bond (the greater the polarity), the stronger the absorption peak, the stronger the polarity, the red shift of the absorption peak; the weaker the polarity, the blue shift of the absorption peak. Therefore, the O-Cl was weaker than the -OH polarity, and the absorption peak at 3297.97 cm -1 shift to the low peak region, causing a blue shift, which proves that the hydrogen on the -OH was replaced by chlorine. On the other hand, the absorption peak of 881.27 cm -1 red-shift by 0.02 cm -1 and the absorption peak at 860.18 cm -1 blue-shift by 0.4 cm -1 , which was due to the unsubstituted -OH in ethylene glycol adjacent. The other -OH hydrogen was replaced by chlorine, resulting in the substitution of -OH; the electron cloud density increased, the force constant k increased, and the induced effect occurred, causing the absorption peak at 881.27 cm -1 to shift to a high wave number. The infrared spectrum of the diol slightly red-shift while the other was not replaced, so a blue shift occurred. Since the alcoholysis of BiCl3 in ethylene glycol was extremely slow and almost no alcoholysis occurred, ammonia water was added to BiCl3+(CH2OH)2 system to promote alcoholysis [45] .Comparing I and J in Figure 6, the peak at 1643.32 cm -1 was generated by the stretching vibration of NH-NH3; comparing curves E and F, the absorption peak at 3284.52 cm -1 had a blue shift of 3.47 cm -1 , the absorption peak at 882.33 cm -1 had a blue shift of 0.4 cm -1 , and the absorption peak at 860.99 cm -1 had a red shift of 0.49 cm -1 , which further confirmed the substitution of BiCl3 in ethylene glycol. The above proof was verified, and an absorption peak was added at 1643.27 cm -1 , which was generated by the -NH stretching vibration.

Hydrolysis mechanism of BiCl3 liquid in Bi 3+ -HCl system
In order to verify whether the hydrolysis, alcoholysis, and glycolysis of solid BiCl3 were hydrolyzed, a simulated liquid test was performed. The above experiment was carried out by formulating a certain concentration of BiCl3 solution, and the same conditions were applied for infrared analysis. The final results are shown in Figure 7 (1), Figure 7 (2), and Figure 7 (3). The results were consistent with the results of Figure 4, Figure 5, and Figure 6, respectively, because the analysis results were basically the same, no more tautology here.

4.Conclusions
The electronic properties of BiCl3, BiOCl and Bi3O4Cl cells were calculated by density functional method here. The valence bond properties of the cell structure of BiCl3, BiOCl and Bi3O4Cl were analyzed from the respects of unit cell structure, unit cell energy, band structure, total density of states, partial density of states, Mulliken population and overlapping population. The atomic transfer pathway of BiOCl and Bi3O4Cl formed during the hydrolysis of BiCl3 was further analyzed by infrared spectroscopy. There were two main ways to prove that BiCl3 was hydrolyzed into oxychloride. One was that the [Bi-Cl] ionic bond between BiCl3 was broken, and the hydroxide replaced the chlorine atom to form Bi(OH)2Cl. Bi(OH)2Cl was extremely unstable in aqueous solution, and it was easy to continue hydrolysis. It contained two hydroxyl groups that were easy to combine with each other and lose a part of water. The other one was that the hydroxyl groups contained in Bi(OH)2Cl tended to react with H + in aqueous solution and lose a molecule of water. The number of Bi(OH)2Cl reactions involved determined the degree and complexity of the formation of a series of chlorinated compounds (BixOyClz). The ruthenium atom easily formed a [Bi-OH] monomer with a hydroxyl group, and the chlorine atom directly formed a BiOCl instead of a hydrogen atom on the hydroxyl group of the [Bi-OH] monomer. https://doi.org/10.37358/RC.20.6.8182 Infrared spectroscopy shows that under water, ethanol and ethylene glycol systems, water hydroxyl and alcohol hydroxyl groups had red-shift and blue-shift, respectively; the hydroxyl vibration in the high-wave region was caused by the substitution of chlorine atoms for hydrogen atoms, which increased the density of electron clouds, increased the force constant k, and induced effects. The group frequency shift to high wavenumbers, and the infrared spectrum shift red. -OCl was relatively weaker than -OH, so the hydroxyl vibration at the low peak region shift to the low peak region, causing a blue shift, which proved that the hydrogen atom on the -OH was replaced by a chlorine atom. It was consistent with the strength of the covalent bond between the calculated chlorine and oxygen, and the results of the density functional method were further verified using experimental results.