# Oxidation Mechanism of Biomedical Titanium Alloy Surface and Experiment

Authors: Kai Ma; Rui Zhang; Junlong Sun; Changxia Liu
Journal: International Journal of Corrosion
 (2020)

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## Abstract

The biological activity, biocompatibility, and corrosion resistance of implants depend primarily on titanium dioxide (TiO2) film on biomedical titanium alloy (Ti6Al4V). This research is aimed at getting an ideal temperature range for forming a dense titanium dioxide (TiO2) film during titanium alloy cutting. This article is based on Gibbs free energy, entropy changes, and oxygen partial pressure equations to perform thermodynamic calculations on the oxidation reaction of titanium alloys, studies the oxidation reaction history of titanium alloys, and analyzes the formation conditions of titanium dioxide. The heat oxidation experiment was carried out. The chemical composition was analyzed with an energy dispersive spectrometer (EDS). The results revealed that titanium dioxide (TiO2) is the main reaction product on the surface below 900°C. Excellent porous oxidation films can be obtained between 670°C and 750°C, which is helpful to improve the bioactivity and osseointegration of implants.


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## Body

## 1. Introduction

Titanium alloy is widely used as a biomaterial due to its superior biocompatibility, mechanical properties close to human bones, and enhanced corrosion resistance. These properties have made the alloys suitable for use in a wide spectrum of biomedical applications including artificial bones, artificial joints, dental roots, and medical devices. The excellent performance of titanium alloy is mainly due to the oxide film as shown in Figure1 [1]. The functional composition of the oxide film is mainly titanium dioxide (TiO2). Titanium dioxide has good biocompatibility, stable chemical property, and low solubility in water, which prevents substrate metal ions from dissolution. Furthermore, it also improves the wear and fatigue resistance of implants in the human body.Figure 1
Cross-sectional view of the microarc oxidation sample.The conventional surface treatment methods of titanium alloy include glow discharge plasma deposition, oxygen ion implantation, hydrogen peroxide treatment, thermal oxidation, sol-gel method, anodic oxidation, microarc oxidation, laser alloying, and pulsed laser deposition. These methods have different characteristics and are applied in different fields. Glow discharge plasma deposition can get a clean surface, and the thickness of the oxide film obtained is 2 nm to 150 nm [2–8]. The oxide film obtained from oxygen ion implantation is thicker, about several microns [9–14]. Hydrogen peroxide treatment of titanium alloy surface is a process of chemical dissolution and oxidation [15, 16]. The dense part of the oxide film is less than 5 nm [17–21]. The oxide film generated from the thermal oxidation method has a porous structure, and its thickness is commonly about 10-20 μm [22–25]. The oxide film from the sol-gel method is rich in Ti-OH, a composition that could induce apatite nucleation and improve the combining of implants and bone. It has a thickness of less than 10 μm [26–28]. Applied with the anodic oxidation method, the surface can generate a porous oxide film of 10 μm to 20 μm thickness [29–31]. Similarly, the oxide film generated from the microarc oxidation method is also porous and has a thickness of 10 μm to 20 μm [32, 33].Unfortunately, we studied that all of the above methods are employed after machining or forming, and they require a long process chain and costly production types of equipment [21–24]. Therefore, we proposed a titanium alloy implant preparation process that integrated with cutting and surface modification. The oxygen-rich atmosphere increases the partial pressure of oxygen in the oxidizing environment, and the heat generated during the cutting process increases the temperature and the rate of the oxidation. It uses the cutting heat and oxygen-rich atmosphere generated during the cutting process to form the oxide film (TiO2) to improve the corrosion resistance of the titanium alloy. The experimental equipment is shown in Figure 2. Since the cutting temperature is the most important factor in the oxide film formation process, this paper carried out researches based on theoretical analysis and experimental investigation to acquire an ideal temperature range for the cutting process to achieve the oxide layer.Figure 2
Experimental device for turning and rolling in an oxygen-enriched atmosphere.


## 2. Oxidation Mechanism of Titanium Alloy

### 2.1. Thermodynamic Analysis of Titanium Alloy Oxidation Reaction

Thermodynamics is mainly used in studying reaction balance and energy balance in chemistry. Data calculated by thermodynamics can reveal the moving direction of chemical equilibrium and energy balance. The oxidation of titanium alloy has several possible reactions under different conditions:(1)Reaction1:3Ti+52O2=Ti3O5(2)Reaction2:2Ti+32O2=Ti2O3(3)Reaction3:Ti+O2=TiO2rutilen(4)Reaction4:Ti+O2=TiO2anatase(5)Reaction5:Ti+12O2=TiO(6)Reaction6:TiO+12O2=TiO2(7)Reaction7:12Ti2O3+14O2=TiO2(8)Reaction8:13Ti3O5+16O2=TiO2For the different reaction equations, the condition of limits and temperature range of reaction are different. To determine the reaction temperature range, Gibbs free energy, entropy changes, and oxygen partial pressure equations are usually used in the calculations [34, 35] as follows:
(9)ΔGTΘ=ΔH298Θ−TΔφT′,(10)ΔSTΘ=ΣniSi,TΘproduct−ΣniSi,TΘreactant,(11)ΔGTΘ=RTlnPO2∗,where ΔGTΘ is standard Gibbs free energy; ΔH298Θ is the standard enthalpy of reaction; ΔφT′ is the reaction Gibbs free energy function; ΔSTΘ is the standard reaction entropy difference; Si,TΘ is standard molar entropy of pure substance i at temperature T; R is the gas constant; T is reaction temperature; and PO2∗ is standard equilibrium oxygen partial pressure of reaction.It can be observed from Figure3 that the Gibbs free energy values of these 8 reactions are negative. So, oxidation of titanium alloy is a spontaneous reaction. With the lower value of Gibbs free energy, an easier reaction could occur. The Gibbs free energy in reaction (1) is the minimum, where the Ti3O5 composition is generated. The values of Gibbs free energy increase from reaction (1) to reaction (5). The productions of these reactions, respectively, are Ti3O5, Ti2O3, TiO2, and TiO according to the reactivity of titanium. However, the final products are determined by two major factors, temperature and oxygen partial pressure. Although Ti3O5 and Ti2O3 are more stable than TiO2 based on thermodynamics theory, the oxidation products mainly are TiO2 on the surface of titanium alloy when the cutting temperature is less than 1000°C [36]. The titanium ions in Ti3O5 and Ti2O3 are at intermediate valence state and can be further oxidized to the highest valence state in the atmosphere [37].Figure 3
Variation of Gibbs free energy at different temperatures.Figure4 shows standard reaction entropy difference curves. It can be observed that the TiO2 is generated in reactions (3), (6), (7) and (8). But there are differences in standard entropy change among these reactions. It can be seen from Figure 4 that compared with Ti2O3 and TiO, the absolute value of the standard entropy difference of Ti2O5 oxidation to TiO2 is the smallest, which means that the required entropy change is the smallest. Low-valence oxides (Ti3O5, Ti2O3, and TiO) are easier to be oxidized to TiO2 than titanium. With the increase of temperature, the entropy change (absolute value) required for low-valence oxide becomes bigger. When the temperature is higher, the low-valence oxide becomes more stable. Equation (11) is the oxygen partial pressure calculation formula, where PO2∗ is the standard equilibrium oxygen partial pressure. It represents the trend of oxygen escaped from the oxide. When the oxygen partial pressure of the gaseous phase is lower than the equilibrium oxygen partial pressure, oxide could not keep stable and began to decompose. On the contrary, the oxide would keep stable. As the standard equilibrium oxygen partial pressure gets higher, the oxide becomes easier to decompose.Figure 4
Standard reaction entropy difference at different temperatures.As shown in Figure5, oxygen partial pressure increases with temperature, and the oxygen partial pressure of titanium oxidation is 0.0035 MPa which is lower than 0.02 MPa at the oxidizing temperature of 1227°C (1500 K); TiO2 would not decompose. Therefore, at the temperature below 1227°C, the main oxidation products of titanium alloy are TiO2.Figure 5
Standard equilibrium oxygen partial pressure at different temperatures.


### 2.2. The Kinetic Reaction Mechanism of Titanium Alloy Oxidation

The process of titanium oxidation is determined by the reactions between titanium and oxygen on the surface layer. The titanium oxidation process includes two aspects: oxygen vacancy diffusion through the anionic oxide layer and the instability and decomposition of TiO2 on the surface layer [38]. A large amount of oxygen can dissolve in titanium. However, the diffusion of oxygen to the titanium substrate is slower [39]. The oxygen content at the interface between the oxidized layer and the titanium substrate is lower. Oxidation rate can be improved by increasing oxygen concentration and temperature, for they are two major factors that influence the oxidation rate. Higher oxygen concentration makes titanium oxidation diffuse further in the depth direction. The activity of titanium atoms on the surface increased as the temperature gets higher. The higher temperature also improves the diffusion rate of oxygen atoms and titanium atoms in the oxide layer. At room temperature, the oxidation forms a thin oxide layer on titanium surface at first, and the oxide layer becomes porous when it is thick enough. Titanium obviously is oxidized when the temperature is above 600°C. The oxygen diffusion in titanium is quicker, and the oxidation is more fierce when the temperature is between 700°C and 800°C [39].The oxidation kinetics of titanium alloy is a theory about reaction rate and diffusion speed. The thermodynamic function can provide a profile of reaction possibilities, spontaneous tendencies, and reaction direction from the state stability variation in reaction. The thermodynamic function does not refer to the oxide reaction process of titanium, nor does the movement and chemical activity of titanium atoms and oxygen atoms. In thermodynamics theory, when the temperature is higher, the standard equilibrium oxygen partial pressure increases, and the decomposition of oxide becomes easier. The oxide starts to break down when the standard equilibrium oxygen partial pressure becomes larger in the oxidation environment. However, the oxidation rate (forward) and decomposition rate (backward) of oxidation products both increase with the temperature. The decomposition speed is equal to the oxidation rate when the Gibbs free energy gets to zero. The decomposition speed is larger than the oxidation rate when the Gibbs free energy is above zero, and the forward reaction would not occur spontaneously. Thermodynamics can be used in judging reaction tendencies when reaction approaches equilibrium at a certain temperature. However, it cannot describe the oxidation rate. In contrast, the kinetic reaction mechanism can describe the oxidation rate and cannot judge reaction tendency. So, these theories reveal the oxidation mechanism from different aspects. With the temperature increases, the decomposition of oxide is possible. Therefore, at the temperature below 1227°C, a higher temperature is helpful for titanium alloy oxidation, and the main oxidation products in this process are TiO2.


## 2.1. Thermodynamic Analysis of Titanium Alloy Oxidation Reaction

Thermodynamics is mainly used in studying reaction balance and energy balance in chemistry. Data calculated by thermodynamics can reveal the moving direction of chemical equilibrium and energy balance. The oxidation of titanium alloy has several possible reactions under different conditions:(1)Reaction1:3Ti+52O2=Ti3O5(2)Reaction2:2Ti+32O2=Ti2O3(3)Reaction3:Ti+O2=TiO2rutilen(4)Reaction4:Ti+O2=TiO2anatase(5)Reaction5:Ti+12O2=TiO(6)Reaction6:TiO+12O2=TiO2(7)Reaction7:12Ti2O3+14O2=TiO2(8)Reaction8:13Ti3O5+16O2=TiO2For the different reaction equations, the condition of limits and temperature range of reaction are different. To determine the reaction temperature range, Gibbs free energy, entropy changes, and oxygen partial pressure equations are usually used in the calculations [34, 35] as follows:
(9)ΔGTΘ=ΔH298Θ−TΔφT′,(10)ΔSTΘ=ΣniSi,TΘproduct−ΣniSi,TΘreactant,(11)ΔGTΘ=RTlnPO2∗,where ΔGTΘ is standard Gibbs free energy; ΔH298Θ is the standard enthalpy of reaction; ΔφT′ is the reaction Gibbs free energy function; ΔSTΘ is the standard reaction entropy difference; Si,TΘ is standard molar entropy of pure substance i at temperature T; R is the gas constant; T is reaction temperature; and PO2∗ is standard equilibrium oxygen partial pressure of reaction.It can be observed from Figure3 that the Gibbs free energy values of these 8 reactions are negative. So, oxidation of titanium alloy is a spontaneous reaction. With the lower value of Gibbs free energy, an easier reaction could occur. The Gibbs free energy in reaction (1) is the minimum, where the Ti3O5 composition is generated. The values of Gibbs free energy increase from reaction (1) to reaction (5). The productions of these reactions, respectively, are Ti3O5, Ti2O3, TiO2, and TiO according to the reactivity of titanium. However, the final products are determined by two major factors, temperature and oxygen partial pressure. Although Ti3O5 and Ti2O3 are more stable than TiO2 based on thermodynamics theory, the oxidation products mainly are TiO2 on the surface of titanium alloy when the cutting temperature is less than 1000°C [36]. The titanium ions in Ti3O5 and Ti2O3 are at intermediate valence state and can be further oxidized to the highest valence state in the atmosphere [37].Figure 3
Variation of Gibbs free energy at different temperatures.Figure4 shows standard reaction entropy difference curves. It can be observed that the TiO2 is generated in reactions (3), (6), (7) and (8). But there are differences in standard entropy change among these reactions. It can be seen from Figure 4 that compared with Ti2O3 and TiO, the absolute value of the standard entropy difference of Ti2O5 oxidation to TiO2 is the smallest, which means that the required entropy change is the smallest. Low-valence oxides (Ti3O5, Ti2O3, and TiO) are easier to be oxidized to TiO2 than titanium. With the increase of temperature, the entropy change (absolute value) required for low-valence oxide becomes bigger. When the temperature is higher, the low-valence oxide becomes more stable. Equation (11) is the oxygen partial pressure calculation formula, where PO2∗ is the standard equilibrium oxygen partial pressure. It represents the trend of oxygen escaped from the oxide. When the oxygen partial pressure of the gaseous phase is lower than the equilibrium oxygen partial pressure, oxide could not keep stable and began to decompose. On the contrary, the oxide would keep stable. As the standard equilibrium oxygen partial pressure gets higher, the oxide becomes easier to decompose.Figure 4
Standard reaction entropy difference at different temperatures.As shown in Figure5, oxygen partial pressure increases with temperature, and the oxygen partial pressure of titanium oxidation is 0.0035 MPa which is lower than 0.02 MPa at the oxidizing temperature of 1227°C (1500 K); TiO2 would not decompose. Therefore, at the temperature below 1227°C, the main oxidation products of titanium alloy are TiO2.Figure 5
Standard equilibrium oxygen partial pressure at different temperatures.


## 2.2. The Kinetic Reaction Mechanism of Titanium Alloy Oxidation

The process of titanium oxidation is determined by the reactions between titanium and oxygen on the surface layer. The titanium oxidation process includes two aspects: oxygen vacancy diffusion through the anionic oxide layer and the instability and decomposition of TiO2 on the surface layer [38]. A large amount of oxygen can dissolve in titanium. However, the diffusion of oxygen to the titanium substrate is slower [39]. The oxygen content at the interface between the oxidized layer and the titanium substrate is lower. Oxidation rate can be improved by increasing oxygen concentration and temperature, for they are two major factors that influence the oxidation rate. Higher oxygen concentration makes titanium oxidation diffuse further in the depth direction. The activity of titanium atoms on the surface increased as the temperature gets higher. The higher temperature also improves the diffusion rate of oxygen atoms and titanium atoms in the oxide layer. At room temperature, the oxidation forms a thin oxide layer on titanium surface at first, and the oxide layer becomes porous when it is thick enough. Titanium obviously is oxidized when the temperature is above 600°C. The oxygen diffusion in titanium is quicker, and the oxidation is more fierce when the temperature is between 700°C and 800°C [39].The oxidation kinetics of titanium alloy is a theory about reaction rate and diffusion speed. The thermodynamic function can provide a profile of reaction possibilities, spontaneous tendencies, and reaction direction from the state stability variation in reaction. The thermodynamic function does not refer to the oxide reaction process of titanium, nor does the movement and chemical activity of titanium atoms and oxygen atoms. In thermodynamics theory, when the temperature is higher, the standard equilibrium oxygen partial pressure increases, and the decomposition of oxide becomes easier. The oxide starts to break down when the standard equilibrium oxygen partial pressure becomes larger in the oxidation environment. However, the oxidation rate (forward) and decomposition rate (backward) of oxidation products both increase with the temperature. The decomposition speed is equal to the oxidation rate when the Gibbs free energy gets to zero. The decomposition speed is larger than the oxidation rate when the Gibbs free energy is above zero, and the forward reaction would not occur spontaneously. Thermodynamics can be used in judging reaction tendencies when reaction approaches equilibrium at a certain temperature. However, it cannot describe the oxidation rate. In contrast, the kinetic reaction mechanism can describe the oxidation rate and cannot judge reaction tendency. So, these theories reveal the oxidation mechanism from different aspects. With the temperature increases, the decomposition of oxide is possible. Therefore, at the temperature below 1227°C, a higher temperature is helpful for titanium alloy oxidation, and the main oxidation products in this process are TiO2.


## 3. Experimental Work

### 3.1. Materials and Methods

Ti6Al4V rods were used in the experiments. The diameter of these Ti6Al4V rods is 14 mm, and the length of rods is 5 mm. The Ti6Al4V samples should be polished to the same surface roughness and then ultrasonically cleaned in acetone and absolute ethanol for ten minutes. The rods were heated in the furnace (Figure6) to an initial temperature of 400°C. Above 400°C, different specimens were heated at intervals of 50°C. The rods were oxidized in static air with three oxidation times of 5 min, 10 min, and 15 min. The oxidized samples were observed using an energy dispersive spectrometer (EDS). The results obtained are discussed in the next section.Figure 6
Heating furnace and temperature control system.


### 3.2. Results and Analysis

#### 3.2.1. EDS Analysis of Oxide Layers

The EDS analysis of oxide layers at different temperatures and time is shown in Figure7. The substrate elements (Ti, Al, and V) and oxygen element were detected by EDS when the temperature was lower than 800°C. The oxygen mainly appeared in the spectrum above 800°C; those oxygen content in the oxide layer significantly increased. It showed a significant increase in diffusion of oxygen in the oxide layer. The reaction of titanium and oxygen gets obvious. As illustrated in Figure 8, as the oxidation temperature gets higher, the content of oxygen in the oxide layer becomes higher. Within the range of temperatures used here, it can be observed that as the temperature increases, the curve of oxygen content follows a parabolic curve. Furthermore, at the same oxidation temperature of 650°C, the oxygen element content of the oxide film layer is different at different oxidation times. It indicated that the longer oxidation time results in higher oxygen content.Figure 7
EDS analysis of oxide layers at different temperatures and time.Figure 8
Curve of oxygen content at different temperature.


## 3.1. Materials and Methods

Ti6Al4V rods were used in the experiments. The diameter of these Ti6Al4V rods is 14 mm, and the length of rods is 5 mm. The Ti6Al4V samples should be polished to the same surface roughness and then ultrasonically cleaned in acetone and absolute ethanol for ten minutes. The rods were heated in the furnace (Figure6) to an initial temperature of 400°C. Above 400°C, different specimens were heated at intervals of 50°C. The rods were oxidized in static air with three oxidation times of 5 min, 10 min, and 15 min. The oxidized samples were observed using an energy dispersive spectrometer (EDS). The results obtained are discussed in the next section.Figure 6
Heating furnace and temperature control system.


## 3.2. Results and Analysis

### 3.2.1. EDS Analysis of Oxide Layers

The EDS analysis of oxide layers at different temperatures and time is shown in Figure7. The substrate elements (Ti, Al, and V) and oxygen element were detected by EDS when the temperature was lower than 800°C. The oxygen mainly appeared in the spectrum above 800°C; those oxygen content in the oxide layer significantly increased. It showed a significant increase in diffusion of oxygen in the oxide layer. The reaction of titanium and oxygen gets obvious. As illustrated in Figure 8, as the oxidation temperature gets higher, the content of oxygen in the oxide layer becomes higher. Within the range of temperatures used here, it can be observed that as the temperature increases, the curve of oxygen content follows a parabolic curve. Furthermore, at the same oxidation temperature of 650°C, the oxygen element content of the oxide film layer is different at different oxidation times. It indicated that the longer oxidation time results in higher oxygen content.Figure 7
EDS analysis of oxide layers at different temperatures and time.Figure 8
Curve of oxygen content at different temperature.


## 3.2.1. EDS Analysis of Oxide Layers

The EDS analysis of oxide layers at different temperatures and time is shown in Figure7. The substrate elements (Ti, Al, and V) and oxygen element were detected by EDS when the temperature was lower than 800°C. The oxygen mainly appeared in the spectrum above 800°C; those oxygen content in the oxide layer significantly increased. It showed a significant increase in diffusion of oxygen in the oxide layer. The reaction of titanium and oxygen gets obvious. As illustrated in Figure 8, as the oxidation temperature gets higher, the content of oxygen in the oxide layer becomes higher. Within the range of temperatures used here, it can be observed that as the temperature increases, the curve of oxygen content follows a parabolic curve. Furthermore, at the same oxidation temperature of 650°C, the oxygen element content of the oxide film layer is different at different oxidation times. It indicated that the longer oxidation time results in higher oxygen content.Figure 7
EDS analysis of oxide layers at different temperatures and time.Figure 8
Curve of oxygen content at different temperature.


## 4. The Influence of N, H, Al, V, and Ti on the Composition of Oxide Layers

The main compositions of Ti6Al4V are Ti, Al, and V. Therefore, when titanium alloy is heated in the air, titanium is also prone to react with the N2, H2, and O2. Aluminum and vanadium will also react with the oxygen. The Gibbs free energy curves are shown in Figure 9. The reaction equations are as follows:
(12)Reaction9:Ti+12N2=TiN(13)Reaction10:Ti+H2=TiH2(14)Reaction11:2Al+32O2=AlO23(15)Reaction12:2V+52O2=V2O5Figure 9
Gibbs free energy curves.


### 4.1. The Reaction between Titanium and Hydrogen

As shown in Figure9, the Gibbs free energy of titanium reaction with hydrogen is the highest value, so it is not easy for titanium to react with hydrogen. Because the Gibbs free energy is negative below 650°C, the reaction of titanium and hydrogen can be spontaneous only in this condition. Besides, the existence of the oxide layer will decrease the hydrogen absorption rate of titanium alloy. For example, the oxide layer with the thickness that is less than 0.45 μm can reduce the hydrogen absorption rate to one-fourth of its original value [38]. However, the existence of titanium hydride will lead to the expansion of the oxide layer due to hydrogen dissolving. Therefore, it can be concluded that to get the compact oxide layer and avoid the generation of titanium hydride, the heating temperature of titanium should be higher than 650°C.


### 4.2. The Reaction between Titanium and Nitrogen

From the values of Gibbs free energy, it can be deduced that the oxidizing reaction of titanium is much easier than nitriding reaction. The reaction rate of titanium and nitrogen depends on the diffusion rate of nitrogen through the titanium nitride layer. Furthermore, all of the oxides of titanium are more stable than titanium nitride [38]. Although the content of nitrogen in the atmosphere is about 80%, due to the low diffusion rate of nitrogen in titanium and titanium nitride, the reaction between titanium and nitrogen plays a minor role in the process of thermal oxidation of titanium alloy. The higher the temperature, the faster the diffusion rate of the nitrogen is. The titanium nitride is detected on the titanium alloy surface when the temperature is above 800°C. These results indicate that the reaction between titanium and nitrogen is drastic with the increase of the diffusion rate when the temperature is above 800°C.


### 4.3. The Reaction between Oxygen and Aluminum

As illustrated in Figure9, the absolute value of Gibbs free energy of the reaction between aluminum and oxygen is the largest. The affinity of aluminum and oxygen is greater than the affinity of titanium and oxygen, so Al2O3 is easier to generate. In the early stage of oxidation, the nucleation of Al2O3 and TiO2 exists on the surface. The growth of TiO2 is faster than Al2O3 [40, 41]. Furthermore, TiO2 quickly formed a compact oxidation protective film on the surface of titanium alloy, which prevented the continuous oxidation of aluminum. So, the content of the aluminum element in Ti6Al4V alloy is very low, and Al2O3 does not affect the oxidation rate of titanium alloys.


### 4.4. The Reaction between Oxygen and Vanadium

The Gibbs free energy of vanadium reaction with oxygen is smaller than aluminum with oxygen. Similar to the oxygenation of aluminum, the content of vanadium is very small. Other researches have shown that the oxides of vanadium are VO2 and V2O5 on the surface oxide layer with thermal treatment, and the V2O5 is the main oxide product [42]. V2O5 has a low melting point (675°C) and high saturation vapor pressure. The volatility of V2O5 is easy to occur under higher temperatures. Because of the volatilization of V2O5, the porous oxide layer can be generated on the titanium alloy surface when the temperature is above 700°C [43, 44]. The porous oxide layer has two advantages: on the one hand, it is good for the diffusion of oxygen to the oxide layer, and the oxidation rate increase drastically. Also, it can improve the adhesion, differentiation, and growth of the osteoblast and the biological activity of implants [45, 46].


## 4.1. The Reaction between Titanium and Hydrogen

As shown in Figure9, the Gibbs free energy of titanium reaction with hydrogen is the highest value, so it is not easy for titanium to react with hydrogen. Because the Gibbs free energy is negative below 650°C, the reaction of titanium and hydrogen can be spontaneous only in this condition. Besides, the existence of the oxide layer will decrease the hydrogen absorption rate of titanium alloy. For example, the oxide layer with the thickness that is less than 0.45 μm can reduce the hydrogen absorption rate to one-fourth of its original value [38]. However, the existence of titanium hydride will lead to the expansion of the oxide layer due to hydrogen dissolving. Therefore, it can be concluded that to get the compact oxide layer and avoid the generation of titanium hydride, the heating temperature of titanium should be higher than 650°C.


## 4.2. The Reaction between Titanium and Nitrogen

From the values of Gibbs free energy, it can be deduced that the oxidizing reaction of titanium is much easier than nitriding reaction. The reaction rate of titanium and nitrogen depends on the diffusion rate of nitrogen through the titanium nitride layer. Furthermore, all of the oxides of titanium are more stable than titanium nitride [38]. Although the content of nitrogen in the atmosphere is about 80%, due to the low diffusion rate of nitrogen in titanium and titanium nitride, the reaction between titanium and nitrogen plays a minor role in the process of thermal oxidation of titanium alloy. The higher the temperature, the faster the diffusion rate of the nitrogen is. The titanium nitride is detected on the titanium alloy surface when the temperature is above 800°C. These results indicate that the reaction between titanium and nitrogen is drastic with the increase of the diffusion rate when the temperature is above 800°C.


## 4.3. The Reaction between Oxygen and Aluminum

As illustrated in Figure9, the absolute value of Gibbs free energy of the reaction between aluminum and oxygen is the largest. The affinity of aluminum and oxygen is greater than the affinity of titanium and oxygen, so Al2O3 is easier to generate. In the early stage of oxidation, the nucleation of Al2O3 and TiO2 exists on the surface. The growth of TiO2 is faster than Al2O3 [40, 41]. Furthermore, TiO2 quickly formed a compact oxidation protective film on the surface of titanium alloy, which prevented the continuous oxidation of aluminum. So, the content of the aluminum element in Ti6Al4V alloy is very low, and Al2O3 does not affect the oxidation rate of titanium alloys.


## 4.4. The Reaction between Oxygen and Vanadium

The Gibbs free energy of vanadium reaction with oxygen is smaller than aluminum with oxygen. Similar to the oxygenation of aluminum, the content of vanadium is very small. Other researches have shown that the oxides of vanadium are VO2 and V2O5 on the surface oxide layer with thermal treatment, and the V2O5 is the main oxide product [42]. V2O5 has a low melting point (675°C) and high saturation vapor pressure. The volatility of V2O5 is easy to occur under higher temperatures. Because of the volatilization of V2O5, the porous oxide layer can be generated on the titanium alloy surface when the temperature is above 700°C [43, 44]. The porous oxide layer has two advantages: on the one hand, it is good for the diffusion of oxygen to the oxide layer, and the oxidation rate increase drastically. Also, it can improve the adhesion, differentiation, and growth of the osteoblast and the biological activity of implants [45, 46].


## 5. Conclusions

Based on the analysis of the oxidation mechanism of biomedical titanium alloy and experimental investigation, the following major conclusions can be drawn:(1)
The main oxidation products of titanium alloy Ti6Al4V are TiO2 and a little Ti3O5, Ti2O3, and TiO when the heating temperature is below 900°C. At higher temperatures, especially in the condition of lower oxygen partial pressure, titanium alloy is more prone to be oxidized to low-valence oxide(2)
The affinity of titanium with oxygen is greater than titanium with hydrogen and nitrogen. Titanium is more prone to react with oxygen. The Gibbs free energy of titanium reaction with hydrogen is a positive value, and the reaction cannot be spontaneous when the temperature is above 650°C. The reaction between titanium and nitrogen is more prevalent when the temperature is above 800°C(3)
Although it is much easier for aluminum and vanadium to react with oxygen than titanium, due to the low content and short heating time, the oxide products of aluminum and vanadium make up a small proportion in the resulting oxide layer. Al2O3 will suppress the oxidation rate of titanium. While the volatilization of V2O5 will leave porous areas in the oxidation film, it is helpful for titanium oxidation and cell adhesion(4)
Temperature is the main factor that affects the oxidation rate of titanium alloy; the higher the temperature, the greater the oxidation rate and the thickness of oxide film. When the temperature is between 675°C and 750°C, a rapid oxidation rate and the porous TiO2 oxide layer can be obtained. A porous layer can improve the biological activity of implants and enable proper osseointegration



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