Silicene oxides: formation, structures and electronic properties.

Understanding the oxidation of silicon has been critical to the success of all types of silicon materials, which are the cornerstones of modern silicon technologies. For the recent experimentally obtained two-dimensional silicene, oxidation should also be addressed to enable the development of silicene-based devices. Here we focus on silicene oxides (SOs) that result from the partial or full oxidation of silicene in the framework of density functional theory. It is found that the formation of SOs greatly depends on oxidation conditions, which concern the oxidizing agents of oxygen and hydroxyl. The honeycomb lattice of silicene may be preserved, distorted or destroyed after oxidation. The charge state of Si in partially oxidized silicene ranges from +1 to +3, while that in fully oxidized silicene is +4. Metals, semimetals, semiconductors and insulators can all be found among the SOs, which show a wide spectrum of electronic structures. Our work indicates that the oxidation of silicene should be exquisitely controlled to obtain specific SOs with desired electronic properties.

The progress of the experimental synthesis of silicene, the silicon counterpart of graphene, has been generating great interest12345678. It is conjectured that silicene is even more advantageous than graphene91011121314. For instance, the spin-orbit interaction of silicene is stronger than that of graphene, leading to detectable quantum spin-Hall effects in silicene1415. The salient structural feature of buckling for silicene facilitates the tuning of the electronic properties of silicene by external fields161718. In addition, silicene is clearly much more compatible with the existing well-established silicon technologies than graphene. Silicene-based devices may be readily incorporated into current silicon integrated circuits.

When silicene-based devices are fabricated, the oxidation of silicene is of the great question during the processing1920. This is due to the fact that silicon routinely reacts with oxygen to form silicon oxide, which has been playing a critical role in the success of all types of current silicon materials such as bulk silicon21, silicon nanowires2223 and silicon nanocrystals2425. It is rather reasonable that the oxidation of silicene should also be addressed to realize the full potential of silicene in all kinds of applications. De Padova et al.19 and Molle et al.20 have recently shown that the oxidation of silicene only starts at a high dose (1000 L) of pure molecular oxygen. The relatively low reactivity of silicene to molecular oxygen may be due to the added sp2 hybridization of silicon atoms19. When exposed to air, however, silicene is readily oxidized without identified reasons20. This indicates that the mechanism for the oxidation of silicene may seriously depend on oxidation conditions.

Up to now, very limited work has been carried out to investigate silicene oxides (SOs) that result from the oxidation of silicene, although it is imperative that the properties of SOs should be elucidated to guide the design of silicene-based device structures. By means of first-principles calculation, Wang et al.26 have recently studied the mechanical and electronic properties of a specific SO with the stoichiometry of Si:O = 1:1 (silicene monoxide). The silicene monoxide is obtained by analogizing its formation to that of a thermal-reduction-induced graphene monoxide27. In fact, the graphene monoxide can only be produced by the thermal reduction of a multilayer graphene oxide. Diffusion in the multilayer structure limits the reduction process, leading to the kinetics-controlled formation of graphene monoxide27. It is clear that the current non-existence of multilayer silicene oxides disables the formation of silicene monoxide in a fashion similar to graphene monoxide. In the present work, we begin with silicene, which is composed of a single layer of silicon atoms. Oxidizing agents such as atomic oxygen (O) and hydroxyl (OH) in a variety of bonding configurations are incorporated into the lattice of silicene to form SOs. The formation of all the SOs is evaluated in the point of view of thermodynamics. It turns out that the charge state of Si in partially oxidized silicene ranges from +1 to +3, while that of Si in fully oxidized silicene is +4. When silicene is oxidized by O, single-side over-bridging O () is the most likely incorporated O configuration during the oxidation. If OH is the oxidizing agent, boat-like OH (OH) and umbrella-like OH (OH) may be the most likely incorporated in the resulting SOs. When O and OH both exist, fully oxidized silicene may be readily produced. The structural characteristics of all the SOs have been identified in this work. We find that the electronic properties of SOs significantly depend on the bonding of O and OH. Metallic, semimetallic, semiconducting and insulating SOs can all be obtained.

Results

Partially oxidized silicene

Figure 1 shows the optimized structures of silicene and SOs that result from the partial oxidation of silicene with both top and side views. The characteristics of all the optimized structures are tabulated in Table 1 (notations of all the O and OH configurations are introduced in Table S1 in the Supporting Information). In the single-atom-thick honeycomb lattice of silicene, the bond length of Si-Si (2.28 Å), the bond angle of Si-Si-Si (116°) and the buckling distance (0.45 Å) are all consistent with those reported in previous works15282930 (Figure 1 (a)). When each Si-Si bond is transformed to a Si-O-Si bond by an O atom during the oxidation of silicene, the buckling of Si atoms actually disappears in the resulting SO (Figure 1 (b)). All the O atoms are also in the same plane, which is only 0.02 Å away from that of Si atoms. Therefore, quasi-in-plane bridging O (O) can be used to denote the incorporated O. It is likely that each Si-Si bond at only one pair of opposite sides in a hexagonal ring is oxidized. But the oxidation results in two Si-O-Si bonds, which are symmetric with respect to the oxidation-flatted plane of Si atoms (Figure 1 (c)). This leads to the configuration of double bridging O (O) for the incorporated O. An O atom may also overbridge two neighboring Si atoms via their unpaired electrons. The overbridging O atoms can be located at either both sides () or single side () of the original silicene (Figure 1 (d) and Figure 1 (e)). When the oxidizing agent is OH, each Si atom may be simply bonded to an OH group via the unpaired electron of Si. For a single hexagonal ring in the honeycomb lattice of silicene, the number of OH groups located at one side of the hexagonal ring may be zero, one, two or three. We denote the OH groups in the resulting SOs as top-like OH (OH) (Figure 1 (f)), umbrella-like OH (OH) (Figure 1 (g)), boat-like OH (OH) (Figure 1 (h)) and armchair-like OH (OH) (Figure 1 (i)), respectively. Please note that OH and OH alternately passivate Si atoms with a step of one and two Si atoms at both sides of the original silicene, respectively. Among all the oxidizing agents only OH and OH do not change the original arrangement of Si atoms in silicene. The buckling distance, Si-Si bond length and Si-Si-Si bond angel of the SO with OH or OH are all the same as those of silicene (Table 1). In the lattices of the SOs with OH and OH all the Si-Si-Si bond angles decrease to be between 103 and 113°. The Si-Si bonds in the SO with OH are either stretched or compressed, while those in the SO with OH are all stretched. For the SO with O the bond length of Si-Si and bond angle of Si-Si-Si decrease to 2.19 Å and 106°, respectively. All the Si-Si bonds are stretched and some of Si-Si-Si bond angles increase up to 122° in the SO with or . All the above-mentioned structural changes lead to the distortion of the honeycomb lattice of silicene. The buckling distances of Si atoms in the distorted honeycomb lattices of the SOs with OH, OH, O, and are 1.14, 0.03, 0, 0.02 and 0.03 Å, respectively. It is clear that no Si-Si bonds exist in the SO with O (Figure 1 (b)). The length of ~83% Si-O bonds is 1.91 Å, while that of the remaining Si-O bonds is 1.42 Å. The Si-O-Si bond angles fall in the range from 104 to 112°. All the structural characteristics of the SO with O indicate that the honeycomb lattice of silicene is destroyed by the incorporation of O.

Figure 1

Optimized structures of (a) silicene and silicene oxides with (b) O, (c) O, (d) , (e) , (f) OH, (g) OH, (h) OH and (i) OH.

Both top and side views of the structures are shown. The unit cell of each structure is indicated by a rhombus or rectangle. Si, O and H atoms are denoted by green, red and grey balls, respectively.

Table 1

Formulas and structural properties such as the buckling distance (Δ) of Si, the bond length of Si-Si and the bond angle of Si-Si-Si for silicene and partially oxidized silicene (SOs with O, O, , OH, OH, OH and OH). Each bandgap (E) is obtained with the PBE correlation exchange functional. The more accurate values of E obtained with the B3LYP correlation exchange functional are shown in the brackets

	Formula	Δ (Å)	<Si-Si> (Å)	∠(Si-Si-Si) (°)	Eg (eV)
Silicene	Si2	0.45	2.28	116	0 (0)
Oqb	Si2O3	0	----	----	5.2 (6.6)
Odb	Si4O4	0	2.19	106	----
	Si6O3	0.03	2.34	110–122	0.5 (0.7)
	Si6O3	0.02	2.34	110–122	0.3 (0.6)
OHtl	Si2(OH)2	0.45	2.28	116	----
OHul	Si6(OH)6	0.03	2.34	104–113	0.2 (0.4)
OHbl	Si4(OH)4	1.14	2.06–2.34	103–112	0 (0)
OHal	Si2(OH)2	0.45	2.28	116	0.4 (0.4)

We have worked out the formula of each SO by examining its unit cell (Table 1). The formulas of the SOs with O, O, , , OH, OH, OH and OH are Si2O3, Si4O4, Si6O3, Si6O3, Si2(OH)2, Si6(OH)6, Si4(OH)4 and Si2(OH)2, respectively. Therefore, the charge states of Si are +3 and +2 for the SOs with O and O, respectively. The charge states of Si are all +1 for the SOs with , , OH, OH, OH and OH. It is clear that the highest charge state (+4) of Si has not been obtained in these SOs. Therefore, they only result from the partial oxidation of silicene.

The formation energy (E) per atom of oxygen in a SO can be calculated by using where E is the total energy of the SO. E is the total energy of silicene. N and N are the numbers of O and OH, respectively. and are the chemical potentials of O2 and OH, respectively. Figure 2 shows the change of E with respect to for each SO by fixing at the total energy of oxygen gas (−7.5 eV). is the difference between in the oxidation system of silicene and that in water (−10.8 eV). For the SOs induced by the partial oxidation with O (e. g., in the atmosphere of oxygen gas), E increases in the order of , , O and O. For those induced by the partial oxidation with OH (e. g., in water), E increases in the order of OH/OH, OH and OH. Therefore, we should expect that the oxidation of silicene in the atmosphere of oxygen gas the most likely leads to the formation of the SO with . When silicene is only oxidized by OH, the SOs with OH and OH are the most likely produced.

Figure 2

Formation energy of a silicene oxide with O, O, , , OH, OH, OH, OH, O + O, O + , O + , O + OH, O + OH, O + OH or O + OH with respect to the difference between the chemical potential of OH in the oxidation system of silicene and that in water.

We now move to the electronic properties of all the partially oxidized silicene. Figure 3 shows the band structure and density of states (DOS) of each partially oxidized silicene. For comparison, the band structure and DOS of silicene have also been included in Figure 3. Consistent with previous results, silicene is semimetallic with a zero bandgap111426 (Figure 3 (a)). The top of the valence band and the bottom of the conduction band linearly cross at the Fermi level, where the DOS is negligible. O opens the bandgap of silicene by 5.2 eV (Figure 3 (b)). Such a large bandgap means that the SO with O is actually an insulator. We notice that there are two deep energy levels in the bandgap of the SO with O. By examining the partial DOS of the SO with O (Figure S1 in the Supporting Information), we find that the two deep energy levels mainly originate from the p orbital of O. Both the p-orbital of Si and the p-orbital of O significantly contribute to the conduction band of the SO with O. The valence band of the SO with O mainly originates from the p-orbital of O. It is known that a bandgap is usually underestimated in the density functional theory (DFT) based on the Perdew-Burke-Ernzerhof (PBE) correlation exchange functional. Thus, we have also performed DFT calculations based on the Becke, three-parameter, Lee-Yang-Parr (B3LYP) exchange-correlation functional to get the more accurate bandgap. For the SO with O, the B3LYP bandgap is 6.6 eV (Table 1).

Figure 3

Band structures and density of states (DOS) of (a) silicene and a silicene oxide with (b) O, (c) O, (d) , (e) , (f) OH, (g) OH, (h) OHor (i) OH.

Γ, K, M are special points in the first Brillouin zone of a cubic crystal. Γ, X, S are special points in the first Brillouin zone of a hexagonal crystal. Energy is shifted so that the Fermi level is 0 eV (the horizontal dashed line). Conduction bands, valance bands, deep energy levels and DOS are indicated by red, blue, green and pink lines, respectively.

The Fermi level is located in the conduction band for the SO with O (Figure 3 (c)), indicating that the SO with O is a metal. Figure 3 (d) shows that the SO with is an indirect-bandgap semiconductor. The valence-band maximum appears at Γ point, while the conduction-band minimum appears at M point. The bandgap is as large as 0.5 eV (the B3LYP bandgap is 0.7 eV). The SO with is also an indirect-bandgap semiconductor (Figure 3 (e)). The valence-band maximum and conduction-band minimum are located at Γ point and K point, respectively. The bandgap is 0.3 eV (the B3LYP bandgap is 0.6 eV). There are no energy levels in the bandgap of the SO with or . The origins of the conduction band and valence band for the SO with O, or are basically similar to those for the SO with O (Figure S1 in the Supporting Information).

For the SO with OH the Fermi level is located at the bottom of the conduction band (Figure 3 (f)). The DOS near the Fermi level is relatively large. Therefore, the SO with OH is actually a metal. For the SO with OH, the valence-band maximum and conduction-band minimum are located at K′ point (between K point and Γ point) and M point, respectively (Figure 3 (g)). The bandgap is 0.2 eV (the B3LYP bandgap is 0.3 eV). As shown in Figure 3 (h), the Fermi level crosses both the valence-band maximum and conduction–band minimum for the SO with OH. The DOS at the Fermi level is negligible. Clearly, the SO with OH is also a semimetal. The valence-band maximum and the conduction-band minimum of the SO with OH are located at M′ point (between Γ point and M point) and Γ′ point (between Γ point and M point), respectively (Figure 3 (i)). The indirect bandgap of the SO with OH is 0.4 eV (the B3LYP bandgap is also 0.4 eV). The valence band of the SO with one type of all the OH configurations also mainly originates from the p-orbital of O. The s-orbital of H now significantly contributes to the conduction band together with the p-orbital of O and the p-orbital of Si (Figure S1 in the Supporting Information).

For all the semiconducting partially oxidized silicene (SOs with , , OH and OH), we have calculated the effective masses (m*) of electrons and holes by using the method adopted by Ni et al.17 and Li et al.31 (Table S2 in the Supporting Information). It is found that m* is between 0.36 and 4.78 m0 (m0 is the electron rest mass). According to μ = eτ/m* (μ is the carrier mobility, e is the charge of an electron, τ is the scattering time that is assumed to approximate to that in graphene), we obtain that the carrier mobilities of the semiconducting partially oxidized silicene are in the order of magnitude of 10–102 cm2 V−1 s−1 (Table S2 in the Supporting Information).

Fully oxidized silicene

We find that O should be incorporated together with other types of O or OH configurations to achieve the charge state of +4 for Si in fully oxidized silicene. Figure 4 shows the SOs based on the combination of O and one of the configurations of O, , , OH, OH, OH and OH. Please note that the number of O atoms is reduced by one third for the SO with O + O because the existence of O only allows four O atoms to be incorporated in a hexagonal ring. The buckling distances of Si atoms in the SO with O + O and O + are 0.04 and 0.06 Å, respectively. Si atoms in all the other SOs are located in the same plane. This is the same as what happens to the SO only with O. By examining the unit cells (Figure 4), we obtain that the formulas of the SOs with O + O, O + , O + , O + OH, O + OH, O + OH and O + OHare Si2O4, Si6O12, Si6O12, Si4O6(OH)4, Si6O9(OH)6, Si2O3(OH)2 and Si2O3(OH)2, respectively (Table S3 in the Supporting Information).

Figure 4

Optimized structures of silicene oxides with (a) O+O, (b) O + , (c) O + , (d) O + OH, (e) O + OH, (f) O + OH and (g) O+OH.

Both top and side views are shown. The unit cell of each structure is indicated by a rhombus or rectangle. Si, O and H atoms are denoted by green, red and grey balls, respectively.

The formation energy of each fully oxidized silicene is also shown in Figure 2. When silicene is only oxidized in the atmosphere of oxygen gas, the most likely formed fully oxidized silicene is the SO with O + . If silicene is oxidized in an environment in which both O and OH exist, a high chemical potential of OH may most likely lead to the formation of the SO with O + OH.

Figure 5 shows the band structure and DOS of each fully oxidized silicene. For the SO with O + OH, the energy levels introduced by OH can basically fill up the bandgap that is opened by O. Therefore, the full oxidation of silicene with O + OH gives rise to a metallic product. The PBE (B3LYP) bandgaps of the SOs with O + O, O + OHand O + OH are 5.1 (6.4), 5.0 (5.4) and 5.1 (7.2) eV, respectively. This indicates that the SOs with O + O, O + OHand O + OHare insulators. Nevertheless, we should notice that there are deep energy levels in the rather wide bandgaps of these three insulators (Figure 5 (a), (f) and (g)). The SOs with O + , O + and O + OH are all indirect-bandgap semiconductors. Their PBE (B3LYP) bandgaps are 2.8 (3.9), 3.2 (4.3) and 2.1 (3.6) eV, respectively. Again, we see deep energy levels in the bandgaps of these three semiconductors. It should be pointed out that both the valance bands and conduction bands of all the fully oxidized silicene mainly originate from the p-orbital of O (Figure S1 in the Supporting Information). This signifies that O plays the dominant role for the electronic properties of all the fully oxidized silicene. The effective masses of electrons and holes for the semiconducting fully oxidized silicene are between 0.73 and 87.81 m0, leading to carrier mobilities in the order of magnitude of a few to 102 cm2 V−1 s−1 (Table S2 in the Supporting Information).

Figure 5

Band structure and density of states (DOS) of a silicene oxide with (a) O+O, (b) O + , (c) O + , (d) O + OH, (e) O + OH, (f) O + OH or (g) O + OH.

Γ, K, K′, M are special points in the first Brillouin zone of a cubic crystal. Γ, X, S are special points in the first Brillouin zone of a hexagonal crystal. Energy is shifted so that the Fermi level is 0 eV (horizontal dashed line). Conduction bands, valance bands, deep energy levels and DOS are indicated by red, blue, green and pink lines, respectively.

Discussion

De Padova et al.19 and Molle et al.20 have recently carried out experiments on the oxidation of silicene in the atmosphere of oxygen gas. The low charge state (+1 and +2) of Si observed after the high oxygen exposure (1000 L) of silicene may be attributed to the formation of the SOs with , and O, which have lower E. The E of the SO with O is even higher than those of the SOs with O + and O + , and comparable to that of the SO with O + O. This means that +3 cannot be the dominant charge state for Si in only O-oxidized silicene. The charge state of Si may directly change from +1/+2 to +4 with the advancement of silicene oxidation in the atmosphere of oxygen gas19. Please note that silicene cannot be fully oxidized if it is only oxidized by OH (Figure 2 and Table 1). The charge state of Si in the final OH-induced SO is always +1 unless H is detached from OH to give rise to restructuring.

When silicene is oxidized in air, O from oxygen molecules and OH from water may both account for the oxidation. It appears that in Molle et al.'s work20 the air was an OH-rich environment, which lowered the E of each OH-incorporated SO. The oxidation of silicene was easily initiated to produce the SOs with all types of OH configurations, in which the charge state of Si was all +1. O then joined in the oxidation, leading to fully oxidized silicene by means of the combination of O and one type of OH configuration. Therefore, the charge state of Si changed from +1 to +4 during the oxidation of silicene in air20.

We have shown that a variety of SOs may be produced by the oxidation of silicene. The spectrum of electronic properties associated with these SOs is even wider than that obtained by the oxidation of graphene32. On one hand, we have been provided with an opportunity of making vastly different materials such as metals, semimetals, semiconductors and insulators from the single material of silicene only by means of oxidation. On the other hand, excellent control on the oxidation conditions of silicene needs to be exerted to obtain specific SOs with desired electronic properties. For example, one can control the oxidation of silicene in the atmosphere of oxygen gas to produce partially oxidized silicene with or . This effectively opens the bandgap of silicene without introducing any deep energy levels in the bandgap (Figure 3). The resulting semiconductor (the SO with or ) with a bandgap of 0.6 or 0.7 eV can very well remedy the zero-bandgap disadvantage of silicene. We should note that this bandgap opening is much more significant than those induced by vertical electric fields1617. By exquisitely tuning the oxidation of silicene with both O and OH, one may also produce insulators such as the SOs with O + OH and O + OH. These insulating SOs can be readily used in silicene-based devices such as field-effect transistors as gate oxides1733.

Methods

Density functional theory (DFT) as implemented in the Vienna ab initio simulation package (VASP) with the projector-augmented wave (PAW) method3435 has been employed in this work. The Perdew-Burke-Ernzerhof (PBE) correlation exchange functional at the generalized gradient approximation (GGA) level is adopted. The structures of silicene and SOs are initially optimized at 0 K. During the optimization the total energy and atomic forces for each structure are minimized. The sampling of reciprocal space is performed with the Monkhorst-Pack scheme36. The meshes of (5 × 5 × 1) and (9 × 9 × 1) special k points are used for the structural relaxation and density-of-states (DOS) calculation, respectively. Depending on the symmetry of the unit cell for a specific structure, an appropriate path in the first Brillouin zone is adopted to calculate the band structure37. All the calculations proceed until the changes in energy and the force on each atom are less than 1 × 10−6 eV per cell and 1 × 10−5 eV/Å, respectively. The Becke, three-parameter, Lee-Yang-Parr (B3LYP) exchange-correlation functional has also been used to calculate the bandgaps of SOs after their structures are optimized.

Author Contributions

X.D.P. and R.W. conceived the idea. R.W. performed the DFT calculations and analyzed the data. X.D.P., R.W. and Z.Y.N. discussed the calculation details and results together. Y.L. provided the Vienna ab initio simulation package (VASP) and guided the DFT calculations. S.S.L. and M.S.X. contributed to the data analysis. R.W., X.D.P. and D.R.Y. wrote the manuscript.