2014
DOI: 10.1063/1.4861177
|View full text |Cite
|
Sign up to set email alerts
|

Electronic properties of InP (001)/HfO2 (001) interface: Band offsets and oxygen dependence

Abstract: Using ab-initio methods, atomic structures and electronic properties of InP (001)/HfO2 (001) interface are studied within the framework of density functional theory. We examine the InP/HfO2 model interface electronic structures under varying oxidation conditions. The effects of indium and phosphorous concentrations on interfacial bonding, defect states, band offsets, and the thermodynamic stability at the interface are also investigated. The origin of interfacial gap states in InP (001)/HfO2 (001) interface ar… Show more

Help me understand this report

Search citation statements

Order By: Relevance

Paper Sections

Select...
4

Citation Types

2
13
0

Year Published

2015
2015
2024
2024

Publication Types

Select...
8
1

Relationship

4
5

Authors

Journals

citations
Cited by 16 publications
(15 citation statements)
references
References 42 publications
2
13
0
Order By: Relevance
“…The band offsets reported by Santosh et al . for a different O10 model (In terminated interfaces were not considered) seem to follow roughly this trend 22 . The band offsets are reflected also in the CLSs of the substitutional/impurity In and P atoms within deeper layers of the HfO 2 .…”
Section: Resultsmentioning
confidence: 70%
“…The band offsets reported by Santosh et al . for a different O10 model (In terminated interfaces were not considered) seem to follow roughly this trend 22 . The band offsets are reflected also in the CLSs of the substitutional/impurity In and P atoms within deeper layers of the HfO 2 .…”
Section: Resultsmentioning
confidence: 70%
“… 66 Density functional theory studies have been interpreted in a similar light. 67 Our results suggest that, on the contrary, P-rich oxides may be beneficial for InP surface passivation.…”
mentioning
confidence: 65%
“…The total DFT energies are used instead of the Gibbs free energies for the calculations of the formation energies because the entropy contributions and enthalpy changes due to finite temperatures (300-600 K) are negligible for all of the structures considered, resulting in no significant changes in the relative formation energies. The following equation to correlate the chemical potential with oxygen partial pressure has been used: 42,43 where p and p O are the partial pressures at temperature T and at one atmosphere, respectively. The whole range of thermodynamically allowed O chemical potential is labeled in the lower x-axis (see Fig.…”
Section: Resultsmentioning
confidence: 99%
“…We used the gas phase O 2 molecule and SO 2 as reference states, similarly to the formulation explained in previous works. 42,43 The standard molar enthalpies (heat) of formation (D f H ) at 298.15 K for MoS 2 , MoO 2 , and MoO 3 are À235.1, À588.9, and À745.1 kJ/mol (À2.436, À6.1035, and À7.7224 eV), respectively. 44 Their relative stability can be predicted by comparing the heat of formation of these materials from their constituents.…”
Section: Resultsmentioning
confidence: 99%