Initial Reaction of Hexachlorodisilane on Amorphous Silica Surface for Atomic Layer Deposition Using Density Functional Theory

Article information

J. Korean Ceram. Soc.. 2017;54(5):443-447

Publication date (electronic) : 2017 September 29

doi : https://doi.org/10.4191/kcers.2017.54.5.11

Ki-Young Kim, Jin-Hoon Yang, Dong-Gung Shin, Yeong-Cheol Kim

School of Energy Materials and Chemical Engineering, Korea University of Technology and Education, Cheonan 330-708, Korea

^†Corresponding author: Yeong-Cheol Kim, E-mail: yckim@koreatech.ac.kr, Tel: +82-41-560-1326, Fax: +82-41-560-1360

Received 2017 August 1; Revised 2017 September 8; Accepted 2017 September 8.

Abstract

The initial reaction of hexachlorodisilane (Si₂Cl₆, HCDS) on amorphous silica (SiO₂) surface for atomic layer deposition was investigated using density functional theory. Two representative reaction sites on the amorphous SiO₂ surface for HCDS reaction, a surface hydroxyl and a two-membered ring, were considered. The reaction energy barrier for HCDS on both sites was higher than its adsorption energy, indicating that it would desorb from the surface rather than react with the surface. At high temperature range, some HCDSs can have kinetic energy high enough to overcome the reaction energy barrier. The HCDS reaction on top of the reacted HCDS was investigated to confirm its self-limiting characteristics.

Keywords: Chemical properties; Simulation; Surface reaction; Density function theory

1. Introduction

As the silicon (Si)-based semiconductor device technology node decreases from 20 nm to below 10 nm, atomic layer deposition (ALD) has replaced chemical vapor deposition (CVD) for several crucial deposition processes that require tighter film thickness controllability and uniformity than ever before.1) The characteristic self-limiting surface reaction of ALD increases the temperature margin (called the temperature window) and the margin for gas flux variability. 2) Plasma enhanced ALD (PEALD) has been developed to deposit films at lower temperature.3) Thermal ALD, however, has still been a preferred choice because PEALD may degrade the device quality and suffer from non-conformality of high aspect ratio features.4,5)

To improve the versatility of ALD precursors, organic ligand-terminated Si precursors have been studied to replace the conventional chlorine (Cl)- or hydrogen (H)-terminated Si precursors.6–11) The conventional Cl- or H-terminated Si precursors, however, have remained the choice for ALD and CVD in the semiconductor industry mainly because of their cost benefits. Of the two precursors, Cl-terminated Si precursors are preferred because they exhibit a self-limiting surface reaction better than that of the H-terminated precursors, and therefore produce better film quality. 12,13) These beneficial effects of Cl-terminated Si precursors are mainly due to the stronger bonds of Cl with Si than with H; the strong bonds suppress the reaction between the molecules. They also suppress the homogeneous reaction in the gas phase, resulting in less containment of particles in films. The stronger bonds, however, reduce the deposition rate and therefore precursors with more than one Si atom have been used to circumvent the low deposition rate. Chung et al. reported higher deposition rates with molecules containing more Si atoms per molecule.14) Due to the abrupt cost hike for precursors with more than two Si atoms per molecule, hexachlorodisilane (Si₂Cl₆, HCDS), which contains two Si atoms, has come to be accepted in the semiconductor industry as the best choice for Si source. HCDS shows a growth rate in ALD higher than that of tetrachlorosilane (SiCl₄), mainly due to there being two Si atoms per molecule.15,16)

In this study, to understand thermal ALD, the initial reaction mechanism of HCDS on an amorphous silica (SiO₂) surface was investigated at atomic scale using density functional theory with consideration of van der Waals interaction. The HCDS reaction on top of the reacted HCDS was also considered in order to confirm its self-limiting characteristics.

2. Calculation Method

All DFT calculations were performed using the Vienna ab-initio simulation package (VASP) code.17–20) The electron wave functions were described using the projector augmented wave (PAW) method of Blöchl,21) which was implemented in the VASP code by Kresse and Joubert.22) The exchange correlation energy was described via the generalized gradient approximation (GGA) of Perdew, Burke, and Ernzerhof (PBE).23) All calculations considered van der Waals interactions based on Grimme’s D2 approach in PAW; the van der Waals interactions were described via a simple pair-wise force field that was optimized for several popular DFT functionals, such as PBE and B3LYP.24) The surface reaction energy barrier was calculated using the climbing nudged elastic bond tool.25)

Bulk amorphous SiO₂ was constructed based on crystalline β-cristobalite SiO₂, which shows local structure, density, and refractive index similar to those of amorphous SiO₂.26) A 2 × 2 × 1 crystalline β-cristobalite SiO₂ super cell, shown in Fig. 1(a), was melted at 7000 K and quenched from 3000 K to 0 K at a cooling speed of 100 K/fs using ab-initio molecular dynamics (MD). The super cell is 14.3 × 14.3 × 7.54 Å³ and contains 32 Si and 64 O atoms. The obtained bulk amorphous SiO₂, shown in Fig. 1(b), was converted to a surface structure by adding a 2 nm vacuum slab and removing all dangling bonds by attaching H atoms. The surface structure was annealed at 1000 K for 0.5 fs. There were three –OHs, two 2-membered (2 M) rings, three 3 M rings, and five 4 M rings on the resulting surface, shown in Fig. 1(c). In this study, the –OH and 2 M ring were considered as representative reaction sites for the HCDS reaction. HCDS was optimized within a 2 nm × 2 nm × 2 nm vacuum box using the PBE-D2 method to obtain the most favorable structure and bond dissociation energy. Its structure is shown in the vacuum region of Fig. 1(c).

Fig. 1

SiO₂ structures of (a) a crystalline β-cristobalite bulk, (b) an amorphous bulk, and (c) an amorphous surface with HCDS in vacuum. Si, O, Cl, and H atoms were colored by grey, red, green, and white, respectively.

3. Results and Discussion

Table 1 shows the bond length and angle of HCDS and the amorphous SiO₂ surface. The surface is represented by the –OH and 2 M ring. The bond lengths of HCDS and –OH of the amorphous SiO₂ surface are in good agreement with the literature.27,29) Fig. 2 shows the initial reaction of HCDS with the (a) –OH and (b) O of the 2 M ring of the amorphous SiO₂ surface. HCDS reacts with the –OH and produces an HCl as a by-product, while HCDS on the 2 M ring does not produce any by-product. Adsorption energy (ΔE_ad), energy barrier (ΔE_ba), and reaction energy (ΔE_re) are presented for the two representative reactions. ΔE_ad, ΔE_ba, and ΔE_re were calculated using the equations given below:

Table 1

Bond Length and Angle of HCDS and an Amorphous SiO₂ Surface

Fig. 2

Initial reaction of HCDS with the (a) –OH and (b) O of the 2M ring of the amorphous SiO₂ surface. Adsorption energy, energy barrier, and reaction energy are presented for the two representative reactions.

ΔEad=Er-EadΔEba=Etr-EadΔEre=Ead-Ere

where E_r, E_ad, and E_re represent the energy of the reference, adsorbed, and reacted states of HCDS, respectively, with the –OH or 2 M ring, and E_tr represents the energy of the transition state during the surface reaction. The positive values of ΔE_ad and ΔE_re indicate that the reactions are exothermic. ΔE_ad is obtained at 0 K (i.e. no entropy-temperature effect (−ΔS·T) was considered). Because ΔE_ad of HCDS near both sites was lower than its ΔE_ba, HCDS rather desorbs from the surface than reacts with the surface. Since HCDS, because its ΔE_ad value is lower than its ΔE_ba value, does not follow the typical adsorption and reaction route for the reaction with the amorphous SiO₂ surface, we need to consider another route.

Figure 3 shows the Maxwell-Boltzmann probability density function,30) which represents the speed for ideal gas molecules at low (blue solid line) and high (red solid line) temperatures, where E_K represents the kinetic energy of the ideal gas molecules. The gas molecules in the blue shadowed region at low temperature will adsorb on the surface and react with the surface if ΔE_ad is greater than the ΔE_ba; we do not have to consider the entropy-temperature effect in ΔE_ad because the entropy change is small for the molecules in the blue shadowed region (the size of the shadowed region is exaggerated for viewing purposes). Since ΔE_ad of HCDS is smaller than ΔE_ba even without considering the entropy-temperature effect, HCDS will not react with the surface after its adsorption. If E_K of the molecule is high enough to overcome ΔE_ba during its collision with the surface in an appropriate direction, the molecule will react with the surface. We can increase the number of molecules having high E_K by increasing the temperature, as shown in the red shadowed region in Fig. 3 (the size of the region is again exaggerated for viewing purposes). The number of HCDS molecules that show higher E_K than ΔE_ba was estimated to be about ten per 10⁶ at 700°C. This amount can be considered to be high enough for the reaction route, because trimethylaluminium (Al(CH₃)₃, TMA), which reacts with a surface after its adsorption because its ΔE_ad value is higher than its ΔE_ba value, typically consumes four per 10⁶ TMA molecules.29)

Fig. 3

Maxwell-Boltzmann probability density function representing speed for ideal gas molecules at low (blue solid line) and high (red solid line) temperatures, where E_K represents kinetic energy of the ideal gas molecules. The blue and red shadowed regions are exaggerated for viewing purposes and represent the parts of the ideal gas molecules involved in surface reaction at low and high temperatures, respectively.

The HCDS reaction on top of a –Si₂Cl₅ group that was formed by the reaction of the initial HCDS with the surface was evaluated to confirm its self-limiting characteristics as an ALD Si precursor. The Si-Cl and Si-Si bond breakings of HCDS were considered; the reactions produce Cl₂ and SiCl₄ as by-products, respectively. Fig. 4 shows the values of ΔE_ad, ΔE_ba, and ΔE_re for the HCDS reaction when there is a –Si₂₋ Cl₅ group in the two reaction routes. Near the –OH or 2 M ring, the value of ΔE_ba for both routes increased significantly compared with that of the initial HCDS reaction. The number of HCDS molecules that have higher values of E_K than of ΔE_ba was estimated to be about four per 10¹⁷ at 700°C. The reaction rate will be 10¹² times lower than that of the initial HCDS reaction, indicating that the molecule shows self-limiting characteristics.

Fig. 4

HCDS reaction with (a) Si-Cl bond breaking and (b) Si-Si bond breaking when HCDS is located on top of a –Si₂Cl₅ group. Adsorption energy, energy barrier, and reaction energy are presented for the two representative reactions.

4. Conclusions

The initial reaction of HCDS on an amorphous SiO₂ surface was investigated using density functional theory. HCDS could not react with the surface through its adsorption, because its adsorption energy was lower than the reaction energy barrier. HCDS was able to react with the surface when the temperature was raised to increase the number of HCDS molecules having high enough kinetic energy to overcome the reaction energy barrier. The HCDS reaction with the already reacted HCDS required much higher reaction energy, indicating that HCDS shows a self-limiting characteristic for ALD.

Acknowledgments

This paper was supported by the Education and Research Promotion Program of KOREATECH.

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