Theoretical Basis of Electrocatalysis

Abstract

In this chapter, we introduce the density functional theory (DFT)-based computational approaches to the study of various electrochemical reactions (hydrogen evolution reaction (HER), oxygen evolution reaction (OER), oxygen reduction reaction (ORR)) occurring on heterogeneous catalysis surfaces. A detailed computational approach to the theoretical interpretation of electrochemical reactions and structure-catalytic activity relationships for graphene-based catalysts will be discussed. The electrocatalytic activity of catalysis can be theoretically evaluated by overpotential value determined from free energy diagram (FED) of electrochemical reactions. By comparing electrocatalytic activity of systematically designed graphene-based catalysts, we will discuss the structure-catalytic activity relationships, especially the electronic and geometrical effects of heteroatom dopants.

1. Introduction

With the climate change, fast consumption of fossil fuels, and environment situations due to carbon release, the research and development of clean energy is of vital importance in the coming decades. Promising applications of electrocatalysis for clean energy conversion, for example fuel cells, water electrolysis, metal-air batteries, and CO₂ to fuel conversion, are the subjects of both extensive fundamental and utilitarian studies. These technologies play a crucial role in the future of sustainable energy utilization infrastructure, and thus huge research efforts have been dedicated to improving the electrocatalytic activity of these reactions, which include electrocatalytic oxygen reduction reaction (ORR), and hydrogen oxidation reaction (HOR) that occur on the cathode and anode of a hydrogen-oxygen fuel cell, respectively, and hydrogen evolution reaction (HER) and oxygen evolution reaction (OER) at the cathode and the anode of an electrolytic cell producing gaseous molecular hydrogen and oxygen, respectively. These reactions play an important role in regenerative fuel cells and dominate their overall performance [1, 2, 3, 4, 5]. Understanding the HER/OER/ORR mechanisms of various catalysts could provide design guidelines for material and process development, as well as facilitating the discovery of new catalysts. Above all, the detailed OER/ORR mechanisms in acid/alkaline environment are still being studied. Generally, OER/ORR can proceed in Langmuir-Hinshelwood (LH) or Eley-Rideal (ER) mechanisms [6]. The LH mechanism comprises all reactive intermediates on the surface while the ER mechanism includes species from the electrolyte that reacts with the surface intermediate. Despite the controversy over the mechanism, ER mechanism is generally accepted with lower reaction energy barrier than that of LH mechanism [7], and many researchers have conducted theoretical studies on OER/ORR based on the ER mechanism. However, there are two feasible reaction pathways in ER mechanism, two-step pathway and four-step pathway depending on the relative stability of O* and OOH* intermediates generated after the adsorption of O₂ on the catalyst [8]. Thus, we sought to describe the detailed reaction pathway of the OER/ORR as well as proposing solutions for the determination of the preferred reaction pathway on the ER mechanism.

Precious metals such as platinum (Pt), iridium (Ir), and ruthenium (Ru)-based catalysts [9, 10, 11] are generally needed to promote the HER for the generation of hydrogen fuel from the electrochemical splitting of water, the ORR in fuel cells for energy conversion, and the OER in metal-air batteries for energy storage. Besides the requirement for high catalytic activity, other issues related to these catalysts are their limited reserves and comparatively high cost, which have precluded these renewable energy technologies from large-scale commercial applications. In this regard, huge amount of efforts has been devoted to develop novel electrocatalysts to completely or partially replace precious metal catalysts in energy technologies. Along with the intensive research efforts in developing nonprecious electrocatalysts to reduce or to replace precious metal catalysts, various carbon-based, metal-free catalysts have been extensively studied because they have unique advantages for designated catalysis due to their tunable molecular structures, abundance and strong tolerance to acid/alkaline environments when used as alternative HER/OER/ORR catalysts. A rapidly growing field of metal-free catalysis based on carbon-based materials has developed, and a substantial amount of literature in both on the theoretical and experimental fields has been generated. Recent studies have revealed that graphene, [12] graphite, [13] vertically aligned nitrogen-doped carbon nanotubes (VA-NCNTs), [14] heteroatom-doped CNTs, [15] and nitrogen-doped graphene sheets [16] have excellent catalytic performance. The presence of N in N-doped graphene leads to more chemically active sites, a high density of defects and high electrochemical activity. Due to these enhanced electronic properties, N-doped catalysts in the C network are attractive for a wide range of applications, including as metal-free catalysts for HER/OER/ORR in fuel cell systems. Recently, carbon nitride-based catalysts (C₃N₄ and C₂N) with N-rich including both graphitic and pyridinic N moieties is a promising catalyst due to its competitiveness over a wide range of electrocatalyst processes, despite pure C₃N₄ and C₂N itself being inert with regard to HER/OER/ORR activity. Here, we attempted to enhance the catalytic activity of graphene, C₃N₄ and C₂N by introducing heteroatoms, which is an effective way to manipulate its electronic structure and electrochemical properties.

In this chapter, we will introduce metal-free bifunctional electrocatalysts of the heteroatom-doped graphenes (GXs, where G and X represent graphene and the heteroatom dopant) for HER [17] and the heteroatom-doped C₃N₄ (X_Y-C₃N₄s, where X and Y indicate the dopant and doping site on C₃N₄, respectively) for OER/ORR [18, 19, 20]. From the doping effect which shows better performance for HER/OER/ORR, we first present evidence that structural deformation and periodic lattice defects play the fundamental role in the HER activity of GXs by adjusting the electronic properties of graphene. We found that graphene doped with third row elements has higher HER activity with out-of-plane structural deformation compared to graphene doped with second row elements, in which graphene tends to maintain its planar structure. We systematically describe a structure-activity relationship in GXs for HER based on a thorough understanding of the effects of dopants, respectively. In addition, the third row elements-doped graphenes (GSi, GP and GS) show an interesting regularity described by a simple 3 N rule: GXs give outstanding HER activity with sustained metallic property when its primitive cell size has 3 × 3 N (N is integral) supercell size of pure graphene. Secondly, we describe not only the detailed OER/ORR mechanisms but also improved OER/ORR activity of C₃N₄ by introducing dopants such as P or S into the C₃N₄ matrix. Especially, we explore the causes of variation in HER/OER/ORR performance with respect to the type of dopant by comparing geometric and electronic structures of GXs and X_Y-C₃N₄s.

From these geometric and electronic structures, we demonstrated that GXs [17] and X_Y-C₃N₄ [18, 19, 20] show outstanding HER/OER/ORR activity with synergistic geometric and electronic effects, which coordinatively increase unsaturated sp³-C via structural deformation and improve electrical conductance by modulating the electronic structure with extra electrons from dopants. Our theoretical investigations suggest that the synergistic effect between geometric and electronic factors plays an important role in HER/OER/ORR catalytic activities. It can be emphasized that there is a close correlation between the geometric/electronic structure and HER/OER/ORR catalytic activities. This understanding of the structure-activity relationship will give an insight into the development of new highly efficient electrocatalytic materials.

2. Theoretical background

2.1. Hydrogen evolution reaction

HER is a multistep process that takes place on the surface of catalyst, and there are two proposed mechanisms: Volmer-Heyrovsky and Volmer-Tafel. Both Volmer-Heyrovsky and Volmer-Tafel mechanisms describe the hydrogen atom adsorption and hydrogen molecule desorption reactions among (1) an initial state $\mathit{2}{\mathit{H}}^{+}+\mathit{2}{\mathit{e}}^{-}$, (2) an intermediate adsorbed state ${\mathit{H}}^{\ast }+{\mathit{H}}^{+}+{\mathit{e}}^{-}$or $\mathit{2}{\mathit{H}}^{\ast }$, and (3) a final product state $\mathit{2}{\mathit{H}}^{+}+\mathit{2}{\mathit{e}}^{-}$, where the $\ast$and ${\mathit{H}}^{\ast }$denote the active site and adsorbed hydrogen atom on the surface of the catalyst, respectively. Because the initial and final states are equivalent at equilibrium reduction potential, U = 0, the Gibbs free energy of the intermediate state, $\left|{\mathit{\Delta G}}_{{\mathit{H}}^{\ast }}\right|$, has been considered as a major descriptor of the HER activity for a wide variety of catalysts. Therefore, the optimum value of $\left|{\mathit{\Delta G}}_{{\mathit{H}}^{\ast }}\right|$should be zero for a spontaneous reaction without activation energy barrier. The Pt catalyst facilitates HER with a low activation energy, $\left|{\mathit{\Delta G}}_{{\mathit{H}}^{\ast }}\right|$∼0.09 eV [21]. In this work, we have considered the Volmer-Tafel mechanism to calculate the Gibbs free energy of the intermediate state, ${\mathit{\Delta G}}_{{\mathit{H}}^{\ast }}^{\text{Volmer}}\left({\mathit{\theta }}_{\mathit{H}{\mathit{1}}^{\ast }}\right)$, ${\mathit{\Delta G}}_{{\mathit{H}}^{\ast }}^{\text{Volmer}}\left({\mathit{\theta }}_{\mathit{H}{\mathit{2}}^{\ast }}\right)$, ${\mathit{\Delta G}}_{{\mathit{H}}^{\ast }}^{\text{Heyrovsky}}\left({\mathit{\theta }}_{\mathit{H}{\mathit{1}}^{\ast }}\right)$, and ${\mathit{\Delta G}}_{{\mathit{H}}^{\ast }}^{\text{Tafel}}\left({\mathit{\theta }}_{\mathit{H}{\mathit{2}}^{\ast }}\right)$with different hydrogen coverage at the active sites, ${\mathit{\theta }}_{\mathit{H}{\mathit{1}}^{\ast }}$, and ${\mathit{\theta }}_{\mathit{H}\mathit{2}\ast }$, as shown in Figure 1. The Gibbs free energy of the adsorbed hydrogen is calculated as:

$${\mathit{\Delta G}}_{{\mathit{H}}^{\ast }}={\mathit{\Delta E}}_{{\mathit{H}}^{\ast }}+{\mathit{\Delta E}}_{\mathit{ZPE}}-\mathit{T\Delta }{\mathit{S}}_{\mathit{H}}$$E1

Figure 1.

Schematic of Volmer-Heyrovsky and Volmer-Tafel mechanisms.${\mathit{\Delta G}}_{{\mathit{H}}^{\ast }}^{\text{Volmer}}\left({\mathit{\theta }}_{\mathit{H}{\mathit{1}}^{\ast }}\right)$,${\mathit{\Delta G}}_{{\mathit{H}}^{\ast }}^{\text{Volmer}}\left({\mathit{\theta }}_{\mathit{H}{\mathit{2}}^{\ast }}\right)$,${\mathit{\Delta G}}_{{\mathit{H}}^{\ast }}^{\text{Heyrovsky}}\left({\mathit{\theta }}_{\mathit{H}{\mathit{1}}^{\ast }}\right)$, and${\mathit{\Delta G}}_{{\mathit{H}}^{\ast }}^{\text{Tafel}}\left({\mathit{\theta }}_{\mathit{H}{\mathit{2}}^{\ast }}\right)$are free energies of the first-, and second-Volmer steps, Hyrovsky and Tafel step, where${\mathit{\theta }}_{\mathit{H}{\mathit{1}}^{\ast }}$, and${\mathit{\theta }}_{\mathit{H}{\mathit{2}}^{\ast }}$indicate different hydrogen coverage of active sites.

where

is hydrogen adsorption energy and

is the difference in zero point energy (ZPE) between the adsorbed state and the gas phase.

refers to the entropy of adsorption of

which is the

where ${\mathit{S}}_{{\mathit{H}}_{\mathit{2}}}^{\mathit{0}}$is the entropy of ${\mathit{H}}_{\mathit{2}}$in the gas phase at STP. ZPE and entropic corrections,

of the heteroatom-doped graphenes (GXs, where G and X represent graphene and the heteroatom dopant), are listed in Table 1. The hydrogen adsorption energy

can be defined in two ways: the integral and differential H adsorption energy as a function of the H coverage in Eqs. (2) and (3), respectively.

eV	ZPE	TS	△ZPE	T△S	△ZPE- T△S
G-H*	0.25	—	0.11	−0.21	0.32
GB-H*	0.25	—	0.12	−0.21	0.32
GN-H*	0.29	—	0.16	−0.21	0.36
GP-H*	0.30	—	0.17	−0.21	0.37
GS-H*	0.31	—	0.18	−0.21	0.38
GSi-H*	0.30	—	0.17	−0.21	0.37
H2	0.27	0.41	—	—	—

Table 1.

Zero point energy (ZPE) and entropic (TS) correction for heteroatom doped-graphenes (G, GB, GN, GP, and GSi) at 298 K.

The gas phase values were from reference 17, while the values for the adsorbed species were taken from DFT calculations. The same values for the adsorbed species for all the N X Nmodels were used, as vibrational frequencies have been found to depend much less on the surface than the bond strength.

$${\mathit{E}}_{{\mathit{H}}^{\ast }}^{\mathit{int}}\left(\mathit{n}\right)=\mathit{1}/\mathit{2}\left[\mathit{E}\left(\text{surf}+{\mathit{nH}}^{\ast }\right)-\mathit{E}\left(\mathit{\text{surf}}\right)\right]-\mathit{1}/\mathit{2}\mathit{E}\left({\mathit{H}}_{\mathit{2}}\right)$$E2

$${\mathit{E}}_{{\mathit{H}}^{\ast }}^{\text{diff}}\left({\mathit{\theta }}_{{\mathit{H}}^{\ast }}\right)={\mathit{\delta E}}_{{\mathit{H}}^{\ast }}^{\mathit{int}}\left(\mathit{n}\right)/\mathit{\delta n}=\left[{\mathit{E}}_{{\mathit{H}}^{\ast }}^{\mathit{int}}\left(\mathit{n}\right)-{\mathit{E}}_{{\mathit{H}}^{\ast }}^{\mathit{int}}\left(\mathit{n}-\mathit{1}\right)\right]/\mathit{\Delta n}$$E3

where $\mathit{n}$, ${\mathit{H}}^{\ast }$and ${\mathit{\theta }}_{\mathit{H}\ast }$refer to the number of hydrogen atoms, adsorbed hydrogen on the surface, and hydrogen coverage, respectively.

In contrast to the single hydrogen reaction of the Volmer step, two hydrogen atoms mediate the Tafel step. Therefore, we obtain the Gibbs free energy of the intermediate state during the Volmer and Tafel steps with the following equations to determine the different hydrogen coverages of active sites.

$${\mathit{\Delta G}}_{{\mathit{H}}^{\ast }}^{\text{Volmer}}={\mathit{\Delta E}}_{{\mathit{H}}^{\ast }}^{\text{Volmer}}+{\mathit{\Delta E}}_{\mathit{ZPE}}-\mathit{T\Delta S}$$E4

E5

$${\mathit{\Delta G}}_{{\mathit{H}}^{\ast }}^{\text{Tafel}}={\mathit{\Delta E}}_{{\mathit{H}}^{\ast }}^{\text{Tafel}}+{\mathit{\Delta E}}_{\mathit{ZPE}}-\mathit{T\Delta S}$$E6

E7

2.2. Oxygen evolution reaction and oxygen reduction reaction

2.2.1. Reaction pathways in alkaline media

The generally acceptable OER mechanism is the four-electron associative mechanism in alkaline media. The four elementary steps of OER mechanism are described as follows:

$${\mathit{OH}}^{-}+\ast \to {\mathit{OH}}^{\ast }+{\mathit{e}}^{-}$$E8

$${\mathit{OH}}^{\ast }+{\mathit{OH}}^{-}\to {\mathit{O}}^{\ast }+{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)+{\mathit{e}}^{-}$$E9

$${\mathit{O}}^{\ast }+{\mathit{OH}}^{-}\to {\mathit{OOH}}^{\ast }+{\mathit{e}}^{-}$$E10

$${\mathit{OOH}}^{\ast }+{\mathit{OH}}^{-}\to \ast +{\mathit{O}}_{\mathit{2}}\left(\mathit{g}\right)+{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)+{\mathit{e}}^{-}$$E11

where * represents the active site on the surface, (l)and (g)refer to liquid and gas phases, respectively, and O^*, OH^*and OOH^*are adsorbed intermediates.

In contrast to OER, ORR can proceed either by a two-step or four-step pathways depending on the relative stability of O^*and OOH^*intermediates generated after the adsorption of O₂on the catalyst. The two-step pathway of ORR in alkaline environment is summarized using the following elementary steps,

$${\mathit{O}}_{\mathit{2}}+{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)+\mathit{2}{\mathit{e}}^{-}\to {\mathit{O}}^{\ast }+\mathit{2}{\mathit{OH}}^{-}$$E12

$${\mathit{O}}^{\ast }+\mathit{2}{\mathit{OH}}^{-}+{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)+\mathit{2}{\mathit{e}}^{-}\to \mathit{4}{\mathit{OH}}^{-}$$E13

whereas the four-step pathway has following elementary steps:

$${\mathit{O}}_{\mathit{2}}+{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)+{\mathit{e}}^{-}\to {\mathit{OOH}}^{\ast }+{\mathit{OH}}^{-}$$E14

$${\mathit{OOH}}^{\ast }+{\mathit{e}}^{-}\to {\mathit{O}}^{\ast }+{\mathit{OH}}^{-}$$E15

$${\mathit{O}}^{\ast }+{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)+{\mathit{e}}^{-}\to {\mathit{OH}}^{\ast }+{\mathit{OH}}^{-}$$E16

$${\mathit{OH}}^{\ast }+{\mathit{e}}^{-}\to \ast +{\mathit{OH}}^{-}$$E17

Looking at the elementary reaction steps of ORR, both reaction pathways lead to the same final products as 4OH⁻and the different intermediate states after the adsorption of O₂on the catalyst, O^*in (Eq. (12)) and OOH^*in (Eq. (14)). Therefore, it is worth mentioning that the transformation step of

to

in (Eq. (12)) or

to

in (Eq. (14)) can be important index to determine the ORR pathway.

2.2.2. Derivation of the free energy relations

The free energy change of each elementary reaction of OER in alkaline media can be expressed as follows:

$${\mathit{\Delta G}}_{\mathit{1}}={\mathit{G}}_{{\mathit{OH}}^{\ast }}+{\mathit{\mu }}_{{\mathit{e}}^{-}}-\left({\mathit{\mu }}_{{\mathit{OH}}^{-}}+{\mathit{G}}_{\ast }\right)$$E18

$${\mathit{\Delta G}}_{\mathit{2}}={\mathit{G}}_{{\mathit{O}}^{\ast }}+{\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)}+{\mathit{\mu }}_{{\mathit{e}}^{-}}-\left({\mathit{G}}_{{\mathit{OH}}^{\ast }}+{\mathit{\mu }}_{{\mathit{OH}}^{-}}\right)$$E19

$${\mathit{\Delta G}}_{\mathit{3}}={\mathit{G}}_{{\mathit{OOH}}^{\ast }}+{\mathit{\mu }}_{{\mathit{e}}^{-}}-\left({\mathit{G}}_{{\mathit{O}}^{\ast }}+{\mathit{\mu }}_{{\mathit{OH}}^{-}}\right)$$E20

$${\mathit{\Delta G}}_{\mathit{4}}={\mathit{G}}_{\ast }+{\mathit{\mu }}_{{\mathit{O}}_{\mathit{2}}}+{\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)}+{\mathit{\mu }}_{{\mathit{e}}^{-}}-\left({\mathit{G}}_{{\mathit{OOH}}^{\ast }}+{\mathit{\mu }}_{{\mathit{OH}}^{-}}\right)$$E21

Therefore, the free energy change of each elementary reaction can be calculated using (1) the chemical potentials of hydroxide, electron, liquid water and oxygen molecule (${\mathit{\mu }}_{{\mathit{OH}}^{-}},{\mathit{\mu }}_{{\mathit{e}}^{-}},{\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)}\text{and} {\mathit{\mu }}_{{\mathit{O}}_{\mathit{2}}}$) and (2) the free energies of each intermediate (${\mathit{G}}_{{\mathit{OH}}^{\ast }}$, ${\mathit{G}}_{{\mathit{O}}^{\ast }}$, and ${\mathit{G}}_{{\mathit{OOH}}^{\ast }}$) on the surface of catalyst (*). In the following paragraph, we describe the theoretical method to calculate the free energy change of each elementary reaction of the proposed reaction path based on the relation between the standard electrode potential and the chemical potential of hydroxides and electrons in alkaline environment.

2.2.3. The chemical potentials of ${\mathit{OH}}^{-}$, ${\mathit{e}}^{-}$, ${\mathit{H}}_{\mathit{2}}\mathit{O}$, and ${\mathit{O}}_{\mathit{2}}$

In alkaline environment, the standard oxygen reduction reaction is described as follows:

$${\mathit{O}}_{\mathit{2}}\left(\mathit{g}\right)+\mathit{2}{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)+\mathit{4}{\mathit{e}}^{-}\to \mathit{4}{\mathit{OH}}^{-}{\mathit{E}}^{\mathit{0}}=\mathit{0.402}\mathit{V}$$E22

and the standard reduction potential (

) is 0.402 V at T = 298.15 K. In terms of chemical potentials, the equations are expressed as follows:

$${\mathit{\mu }}_{{\mathit{o}}_{\mathit{2}}\left(\mathit{g}\right)}+\mathit{2}{\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)}+\mathit{4}{\mathit{\mu }}_{{\mathit{e}}^{-}}=\mathit{4}{\mathit{\mu }}_{{\mathit{OH}}^{-}}$$E23

$${\mathit{\mu }}_{{\mathit{e}}^{-}}-{\mathit{\mu }}_{{\mathit{OH}}^{-}}=-\mathit{1}/\mathit{4}\left({\mathit{\mu }}_{{\mathit{O}}_{\mathit{2}}\left(\mathit{g}\right)}+\mathit{2}{\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)}\right)$$E24

The left side in (Eq. (24)), the chemical potentials of electron and hydroxide, could be derived further as follows:

$${\mathit{\mu }}_{{\mathit{e}}^{-}}={\mathit{\mu }}_{{\mathit{e}}^{‐}}^{\mathit{0}}-\mathit{eU}$$E25

$${\mathit{\mu }}_{{\mathit{OH}}^{-}}={\mathit{\mu }}_{{\mathit{OH}}^{‐}}^{\mathit{0}}+{\mathit{\kappa }}_{\mathit{B}}{\mathit{\text{Tlna}}}_{{\mathit{OH}}^{-}}$$E26

where

represents the shift in electron energy when a bias is applied and

,

represent the chemical potentials of electron and hydroxide at standard conditions

. Therefore,

$${\mathit{\mu }}_{{\mathit{e}}^{-}}-{\mathit{\mu }}_{{\mathit{OH}}^{-}}=\left({\mathit{\mu }}_{{\mathit{e}}^{‐}}^{\mathit{0}}-\mathit{eU}\right)‐\left({\mathit{\mu }}_{{\mathit{OH}}^{‐}}^{\mathit{0}}+{\mathit{\kappa }}_{\mathit{B}}{\mathit{\text{Tlna}}}_{{\mathit{OH}}^{-}}\right)$$E27

$${\mathit{\mu }}_{{\mathit{e}}^{-}}-{\mathit{\mu }}_{{\mathit{OH}}^{-}}={\mathit{\mu }}_{{\mathit{e}}^{‐}}^{\mathit{0}}-{\mathit{\mu }}_{{\mathit{OH}}^{‐}}^{\mathit{0}}‐\mathit{eU}=‐\mathit{1}/\mathit{4}\left({\mathit{\mu }}_{{\mathit{O}}_{\mathit{2}}\left(\mathit{g}\right)}+\mathit{2}{\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)}\right)$$E28

at standard and equilibrium conditions $\left({\mathit{a}}_{{\mathit{OH}}^{‐}}=\mathit{1},\mathit{T}=\mathit{298.15}\mathit{K},\text{and}\mathit{eU}={\mathit{E}}^{\mathit{0}}=\mathit{0.402}\mathit{V}\right)$. In the case of the right side in Eq. (24), the chemical potentials of liquid water and oxygen molecule (

and

) can be calculated from the approximations proposed by Norskov et al., where the chemical potential of liquid water (

) is equal to the chemical potential of water in the gas phase (

), at T = 298.15 K and 0.035 bars.

$${\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)}={\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{g}\right)}={\mathit{E}}_{\mathit{DFT}}^{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{g}\right)}+{\mathit{ZPE}}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{g}\right)}-{\mathit{TS}}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{g}\right)}^{\mathit{0}}$$E29

Moreover, the chemical potential of oxygen molecule (

) is derived from the standard free energy change of the reaction:

$$\mathit{1}/\mathit{2}{\mathit{O}}_{\mathit{2}}\left(\mathit{g}\right)+{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)\leftrightarrow {\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)$$E30

Because the experimental standard free energy change is −2.46 eV, the equation can be written as:

$${\mathit{G}}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)}^{\mathit{0}}-\mathit{1}/\mathit{2}{\mathit{G}}_{{\mathit{O}}_{\mathit{2}}\left(\mathit{g}\right)}^{\mathit{0}}-{\mathit{G}}_{{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)}^{\mathit{0}}=-\mathit{2.46}\mathit{eV}$$E31

Therefore, the chemical potential of oxygen molecule (

) can be approximately calculated as follows:

$$\begin{array}{l}{\mathit{\mu }}_{{\mathit{O}}_{\mathit{2}}\left(\mathit{g}\right)}=\mathit{4.92}+\mathit{2}\left({\mathit{E}}_{\mathit{DFT}}^{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{g}\right)}+{\mathit{ZPE}}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{g}\right)}-{\mathit{TS}}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{g}\right)}^{\mathit{0}}\right)\\ -\mathit{2}\left({\mathit{E}}_{\mathit{DFT}}^{{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)}+{\mathit{ZPE}}_{{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)}-{\mathit{TS}}_{{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)}^{\mathit{0}}\right)\end{array}$$E32

Therefore, Eq. (24) can be written as:

$${\mathit{\mu }}_{{\mathit{e}}^{-}}-{\mathit{\mu }}_{{\mathit{OH}}^{-}}-\mathit{eU}=-\mathit{1}/\mathit{4}\left({\mathit{\mu }}_{{\mathit{O}}_{\mathit{2}}\left(\mathit{g}\right)}+\mathit{2}{\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{g}\right)}\right)$$E33

Finally, we can obtain

value as 9.952 eV using the (Eq. (29)), (Eq. (32)) and (Eq. (33)) [20]. The enthalpy change (E_DFT), the zero-point energy correction (Δ_ZPE) calculated by the DFT calculations of vibrational frequencies, and entropy corrections (TS) are listed in Table 2.

Species	E (eV)	ZPE (eV)	TS (eV)
H2O (0.035 bar)	−14.22	0.56	0.67
H2	−6.76	0.27	0.41
O*	—	0.09	0.05
OH*	—	0.41	0.07
OOH*	—	0.46	0.16

Table 2.

Total energies (E) of H₂O and H₂ and zero point energy (ZPE) corrections and entropic contributions (TS) to the free energies.

Gas phase H₂O at 0.035 bar was used as the reference state because at this pressure gas phase H₂O is in equilibrium with liquid water at 300 K. The same values for the adsorbed species for all the models were used, as vibrational frequencies have been found to depend much less on the surface than the bond strength. We took the standard entropies from thermodynamic tables for gas phase molecules.

2.2.4. The free energies of each intermediate (${\mathit{G}}_{{\mathit{OH}}^{\ast }}$, ${\mathit{G}}_{{\mathit{O}}^{\ast }}$, and ${\mathit{G}}_{{\mathit{OOH}}^{\ast }}$) on the surface of catalyst (*)

Step 1.${\mathit{OH}}^{-}+\ast \to {\mathit{OH}}^{\ast }+{\mathit{e}}^{-}$

The first step is the adsorption step of active site with a release of an electron:

$$\begin{array}{l}{\mathit{\Delta G}}_{\mathit{1}}={\mathit{G}}_{{\mathit{OH}}^{\ast }}+{\mathit{\mu }}_{{\mathit{e}}^{-}}-\left({\mathit{\mu }}_{{\mathit{OH}}^{-}}+{\mathit{G}}_{\ast }\right)\\ =\left({\mathit{G}}_{{\mathit{OH}}^{\ast }}-{\mathit{G}}_{\ast }\right)+\left({\mathit{\mu }}_{{\mathit{e}}^{-}}^{\mathit{0}}-{\mathit{\mu }}_{{\mathit{OH}}^{-}}^{\mathit{0}}-\mathit{eU}\right)\end{array}$$E34

where respectively and could be expressed by DFT energies:

$${\mathit{G}}_{{\mathit{OH}}^{\ast }}={\mathit{E}}_{\mathit{DFT}}^{{\mathit{OH}}^{\ast }}+{\mathit{ZPE}}_{{\mathit{OH}}^{\ast }}-{\mathit{TS}}_{{\mathit{OH}}^{\ast }}^{\mathit{0}}$$E35

$${\mathit{G}}_{\ast }={\mathit{G}}_{{\mathit{OH}}^{\ast }}$$E36

Replacing (Eq. (33)), (Eq. (35)) and (Eq. (36)) in (Eq. (34)) we get:

$$\begin{array}{l}{\mathit{\Delta G}}_{\mathit{1}}=\left[\left({\mathit{E}}_{\mathit{DFT}}^{{\mathit{OH}}^{\ast }}+\mathit{ZPE}-{\mathit{TS}}^{\mathit{0}}\right)-{\mathit{E}}_{\mathit{DFT}}^{\ast }\right]+\left({\mathit{\mu }}_{{\mathit{e}}^{‐}}^{\mathit{0}}-{\mathit{\mu }}_{{\mathit{OH}}^{‐}}^{\mathit{0}}-\mathit{eU}\right)\\ =\left[\left({\mathit{E}}_{\mathit{DFT}}^{{\mathit{OH}}^{\ast }}+\mathit{ZPE}-{\mathit{TS}}^{\mathit{0}}\right)-{\mathit{E}}_{\mathit{DFT}}^{\ast }\right]+\mathit{9.952}\mathit{eV}\end{array}$$E37

Step 2:${\mathit{OH}}^{\ast }+{\mathit{OH}}^{-}\to {\mathit{O}}^{\ast }+{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)+{\mathit{e}}^{-}$

The second step is oxidation of the OH^*species to O^*with release of water and an electron:

$$\begin{array}{l}{\mathit{\Delta G}}_{\mathit{2}}={\mathit{G}}_{{\mathit{O}}^{\ast }}+{\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)}+{\mathit{\mu }}_{{\mathit{e}}^{-}}-\left({\mathit{G}}_{{\mathit{OH}}^{\ast }}+{\mathit{\mu }}_{{\mathit{OH}}^{-}}\right)\\ =\left({\mathit{G}}_{{\mathit{O}}^{\ast }}+{\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)}-{\mathit{G}}_{{\mathit{OH}}^{\ast }}\right)+\left({\mathit{\mu }}_{{\mathit{e}}^{‐}}^{\mathit{0}}-{\mathit{\mu }}_{{\mathit{OH}}^{‐}}^{\mathit{0}}-\mathit{eU}\right)\end{array}$$E38

The relation for

in terms of DFT energies is similar to the relation for (Eq. (35)). Replacing again the same equations as in the case for the first step in (Eq. (38)) we get:

$${\mathit{\Delta G}}_{\mathit{2}}=\left[\left({\mathit{E}}_{\mathit{DFT}}^{{\mathit{O}}^{\ast }}+{\mathit{E}}_{\mathit{DFT}}^{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{g}\right)}\right)-{\mathit{E}}_{\mathit{DFT}}^{{\mathit{OH}}^{\ast }}+\left(\mathit{\Delta ZPE}‐\mathit{T\Delta }{\mathit{S}}^{\mathit{0}}\right)\right]+\mathit{9.952}\mathit{eV}$$E39

Step 3:${\mathit{O}}^{\ast }+{\mathit{OH}}^{-}\to {\mathit{OOH}}^{\ast }+{\mathit{e}}^{-}$

The third step is represented by formation of the OOH^*on top of oxygen with a release of an electron:

$$\begin{array}{l}{\mathit{\Delta G}}_{\mathit{3}}={\mathit{G}}_{{\mathit{OOH}}^{\ast }}+{\mathit{\mu }}_{{\mathit{e}}^{-}}-\left({\mathit{G}}_{{\mathit{O}}^{\ast }}+{\mathit{\mu }}_{{\mathit{OH}}^{-}}\right)\\ =\left({\mathit{G}}_{{\mathit{OOH}}^{\ast }}-{\mathit{G}}_{{\mathit{O}}^{\ast }}\right)+\left({\mathit{\mu }}_{{\mathit{e}}^{-}}^{\mathit{0}}-{\mathit{\mu }}_{{\mathit{OH}}^{-}}^{\mathit{0}}-\mathit{eU}\right)\end{array}$$E40

The relation for ${\mathit{G}}_{{\mathit{OOH}}^{\ast }}$and ${\mathit{G}}_{{\mathit{O}}^{\ast }}$in terms of DFT energies is similar to the relation for (Eq. (35)). The same equations are replaced gradually in the (Eq. (40)) as follows:

$${\mathit{\Delta G}}_{\mathit{3}}=\left[{\mathit{E}}_{\mathit{DFT}}^{{\mathit{OOH}}^{\ast }}-{\mathit{E}}_{\mathit{DFT}}^{{\mathit{O}}^{\ast }}+\left(\mathit{\Delta ZPE}‐\mathit{T\Delta }{\mathit{S}}^{\mathit{0}}\right)\right]+\mathit{9.952}\mathit{eV}$$E41

Step 4:${\mathit{OOH}}^{\ast }+{\mathit{OH}}^{-}\to \ast +{\mathit{O}}_{\mathit{2}}\left(\mathit{g}\right)+{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)+{\mathit{e}}^{-}$

The last step is the evolution of oxygen molecule:

$$\begin{array}{l}{\mathit{\Delta G}}_{\mathit{4}}={\mathit{G}}_{\ast }+{\mathit{\mu }}_{{\mathit{O}}_{\mathit{2}}\left(\mathit{g}\right)}+{\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)}+{\mathit{\mu }}_{{\mathit{e}}^{-}}-\left({\mathit{G}}_{{\mathit{OOH}}^{\ast }}+{\mathit{\mu }}_{{\mathit{OH}}^{-}}\right)\\ =\left({\mathit{G}}_{\ast }+{\mathit{\mu }}_{{\mathit{O}}_{\mathit{2}}\left(\mathit{g}\right)}+{\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)}-{\mathit{G}}_{{\mathit{OOH}}^{\ast }}\right)+\left({\mathit{\mu }}_{{\mathit{e}}^{-}}^{\mathit{0}}-{\mathit{\mu }}_{{\mathit{OH}}^{-}}^{\mathit{0}}-\mathit{eU}\right)\end{array}$$E42

Therefore, we leave from the following equation:

$$\begin{array}{l}{\mathit{\Delta G}}_{\mathit{4}}=\left[{\mathit{E}}_{\mathit{DFT}}^{\ast }+\left(\mathit{4.92}+\mathit{2}\left({\mathit{E}}_{\mathit{DFT}}^{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{g}\right)}-{\mathit{E}}_{\mathit{DFT}}^{{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)}\right)\right)+{\mathit{E}}_{\mathit{DFT}}^{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{g}\right)}\right]-{\mathit{E}}_{\mathit{DFT}}^{{\mathit{OOH}}^{\ast }}+\left(\mathit{\Delta ZPE}‐\mathit{T\Delta }{\mathit{S}}^{\mathit{0}}\right)]+\mathit{9.952}\mathit{eV}\end{array}$$E43

Finally, the summation of $\mathit{\Delta }{\mathit{G}}_{\mathit{1}}$, $\mathit{\Delta }{\mathit{G}}_{\mathit{2}}$, $\mathit{\Delta }{\mathit{G}}_{\mathit{3}}$, and $\mathit{\Delta }{\mathit{G}}_{\mathit{4}}$should be 1.608 eV.

The reaction free energies of O*, OH*and OOH*species on the surface of catalyst are corrected by ZPE and TS. Moreover, the free energy relations of the ORR in alkaline media can also be explained in the same vein as the OER above mentioned [20].

2.2.5. Reaction pathways in acidic media

The generally acceptable OER mechanism is the four-electron associative mechanism in acidic media. The four elementary steps of OER mechanism are described as follows:

$${\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)+\ast \to {\mathit{OH}}^{\ast }+{\mathit{H}}^{+}+{\mathit{e}}^{-}$$E44

$${\mathit{OH}}^{\ast }\to {\mathit{O}}^{\ast }+{\mathit{H}}^{+}+{\mathit{e}}^{-}$$E45

$${\mathit{O}}^{\ast }+{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)\to {\mathit{OOH}}^{\ast }+{\mathit{H}}^{+}+{\mathit{e}}^{-}$$E46

$${\mathit{OOH}}^{\ast }\to \ast +{\mathit{O}}_{\mathit{2}}\left(\mathit{g}\right)+{\mathit{H}}^{+}+{\mathit{e}}^{-}$$E47

where * represents the active site on the surface, (l) and $\left(\mathit{g}\right)$refer to liquid and gas phases, respectively, and O^*, OH^*and OOH^*are adsorbed intermediates. The ORR can proceed completely via a direct four-electron process in which O₂(g)is reduced directly to water H₂O(g), without involvement of hydrogen peroxide. The ORR mechanism is summarized using the following elementary steps,

$${\mathit{O}}_{\mathit{2}}\left(\mathit{g}\right)+{\mathit{H}}^{+}+{\mathit{e}}^{-}\to {\mathit{OOH}}^{\ast }$$E48

$${\mathit{OOH}}^{\ast }+{\mathit{H}}^{+}+{\mathit{e}}^{-}\to {\mathit{O}}^{\ast }+{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)$$E49

$${\mathit{O}}^{\ast }+{\mathit{H}}^{+}+{\mathit{e}}^{-}\to {\mathit{OH}}^{\ast }$$E50

$${\mathit{OH}}^{\ast }+{\mathit{H}}^{+}+{\mathit{e}}^{-}\to \ast +{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)$$E51

Here, we took the OER reactions ((44)–(47)) to derive the thermochemistry of both OER/ORR, because the ORR reactions (Eqs. ((48)–(51)) are inversed from the OER reactions (Eqs. ((44)–(47)). The catalytic activity of the OER/ORR processes can be determined by examining the reaction free energies of the different elementary steps.

2.2.6. Derivation of the free energy relations

The free energy change of each elementary reaction of OER can be expressed as follows:

$${\mathit{\Delta G}}_{\mathit{1}}={\mathit{G}}_{{\mathit{OH}}^{\ast }}+{\mathit{\mu }}_{{\mathit{H}}^{+}}+{\mathit{\mu }}_{{\mathit{e}}^{-}}-\left({\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)}+{\mathit{G}}_{\ast }\right)$$E52

$${\mathit{\Delta G}}_{\mathit{2}}={\mathit{G}}_{{\mathit{O}}^{\ast }}+{\mathit{\mu }}_{{\mathit{H}}^{+}}+{\mathit{\mu }}_{{\mathit{e}}^{-}}-\left({\mathit{G}}_{{\mathit{OH}}^{\ast }}\right)$$E53

$${\mathit{\Delta G}}_{\mathit{3}}={\mathit{G}}_{{\mathit{OOH}}^{\ast }}+{\mathit{\mu }}_{{\mathit{H}}^{+}}+{\mathit{\mu }}_{{\mathit{e}}^{-}}-\left({\mathit{G}}_{{\mathit{O}}^{\ast }}+{\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)}\right)$$E54

$${\mathit{\Delta G}}_{\mathit{3}}={\mathit{G}}_{\ast }+{\mathit{\mu }}_{{\mathit{O}}_{\mathit{2}}\left(\mathit{g}\right)}+{\mathit{\mu }}_{{\mathit{H}}^{+}}+{\mathit{\mu }}_{{\mathit{e}}^{-}}-\left({\mathit{G}}_{{\mathit{OOH}}^{\ast }}\right)$$E55

Therefore, the free energy change of each elementary reaction can be calculated using (1) the chemical potentials of proton, electron, liquid water and oxygen molecule (

), and ii) the free energies of each intermediate (${\mathit{G}}_{{\mathit{OH}}^{\ast }}$, ${\mathit{G}}_{{\mathit{O}}^{\ast }}$, and ${\mathit{G}}_{{\mathit{OOH}}^{\ast }}$) on the surface of catalyst (*). In the following paragraph, we describe the theoretical method to calculate the free energy change of each elementary reaction of the proposed reaction path based on the relation between the standard electrode potential and the chemical potential of protons and electrons in acidic environment.

2.2.7. The chemical potentials of H⁺, and ${\mathit{e}}^{-}$

In acidic environment, the standard hydrogen electrode is based on the redox half-cell,

$${\mathit{H}}^{+}\left(\mathit{aq}\right)+{\mathit{e}}^{-}\to \mathit{1}/\mathit{2}{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right){\mathit{E}}^{\mathit{0}}=\mathit{0.00}\mathit{V}$$E56

and the standard reduction potential (${\mathit{E}}^{\mathit{0}}$) is 0.00 V at T = 298.15 K. In terms of chemical potentials, the equation is expressed as follows:

$${\mathit{\mu }}_{{\mathit{H}}^{+}}+{\mathit{\mu }}_{{\mathit{e}}^{-}}=\mathit{1}/\mathit{2}{\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)}$$E57

In (Eq. (57)), the chemical potentials of proton, electron and hydrogen could be derived further as follows:

$${\mathit{\mu }}_{{\mathit{H}}^{+}}={\mathit{\mu }}_{{\mathit{H}}^{+}}^{\mathit{0}}-{\mathit{\kappa }}_{\mathit{B}}{\mathit{\text{Tlna}}}_{{\mathit{H}}^{+}}$$E58

$${\mathit{\mu }}_{{\mathit{e}}^{-}}={\mathit{\mu }}_{{\mathit{e}}^{-}}^{\mathit{0}}-\mathit{eU}$$E59

$${\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)}={\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}}^{\mathit{0}}-{\mathit{\kappa }}_{\mathit{B}}{\mathit{\text{Tlnp}}}_{{\mathit{H}}_{\mathit{2}}}$$E60

where

represents the shift in electron energy when a bias is applied and

,

represent the chemical potentials of electron and proton at standard conditions

. Therefore,

$${\mathit{\mu }}_{{\mathit{H}}^{+}}^{\mathit{0}}+{\mathit{\mu }}_{{\mathit{e}}^{‐}}^{\mathit{0}}=\mathit{1}/\mathit{2}{\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)}^{\mathit{0}}$$E61

at standard and equilibrium conditions (

and

). In the case of the right side in (Eq. (61)), we can define the standard chemical potential of hydrogen on the DFT scale from computational point of view:

$${\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}}^{\mathit{0}}={\mathit{E}}_{\mathit{DFT}}^{{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)}+{\mathit{ZPE}}_{{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)}-{\mathit{TS}}_{{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)}^{\mathit{0}}$$E62

Another approximation is that for liquid water and oxygen molecule,

and

can also be explained in the same vein as the OER in the alkaline media above mentioned.

2.2.8. The free energies of each intermediate (${\mathit{G}}_{{\mathit{OH}}^{\ast }}$, ${\mathit{G}}_{{\mathit{O}}^{\ast }}$, and ${\mathit{G}}_{{\mathit{OOH}}^{\ast }}$) on the surface of catalyst (*)

Step 1:

The first step is the adsorption step of OH^*on active site with a release of a proton and an electron:

$$\begin{array}{l}{\mathit{\Delta G}}_{\mathit{1}}={\mathit{G}}_{{\mathit{OH}}^{\ast }}+{\mathit{\mu }}_{{\mathit{H}}^{+}}+{\mathit{\mu }}_{{\mathit{e}}^{-}}-\left({\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)}+{\mathit{G}}_{\ast }\right)\\ =\left({\mathit{G}}_{{\mathit{OH}}^{\ast }}-{\mathit{\mu }}_{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{l}\right)}+{\mathit{G}}_{\ast }\right)+\left({\mathit{\mu }}_{{\mathit{H}}^{+}}^{\mathit{0}}+{\mathit{\mu }}_{{\mathit{e}}^{-}}^{\mathit{0}}-\mathit{eU}\right)\end{array}$$E63

where ${\mathit{G}}_{{\mathit{OH}}^{\ast }}$and ${\mathit{G}}_{\ast }$are expressed by DFT energies:

$${\mathit{G}}_{{\mathit{OH}}^{\ast }}={\mathit{E}}_{\mathit{DFT}}^{{\mathit{OH}}^{\ast }}+{\mathit{ZPE}}_{{\mathit{OH}}^{\ast }}-{\mathit{TS}}_{\mathit{OH}}^{\mathit{0}}$$E64

$${\mathit{G}}_{\ast }={\mathit{E}}_{\mathit{DFT}}^{\ast }$$E65

Replacing (Eq. (29)), (Eq. (62)), (Eq. (64)) and (Eq. (65)) in (Eq. (63)) we get:

$$\begin{array}{l}{\mathit{\Delta G}}_{\mathit{1}}=\left[\left({\mathit{E}}_{\mathit{DFT}}^{{\mathit{OH}}^{\ast }}-{\mathit{E}}_{\mathit{DFT}}^{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{g}\right)}-{\mathit{E}}_{\mathit{DFT}}^{\ast }\right)+\left(\mathit{\Delta ZPE}-\mathit{T\Delta }{\mathit{S}}^{\mathit{0}}\right)\right]\\ +\left({\mathit{\mu }}_{{\mathit{H}}^{+}}^{\mathit{0}}+{\mathit{\mu }}_{{\mathit{e}}^{-}}^{\mathit{0}}-\mathit{eU}\right)\\ =\left[\left({\mathit{E}}_{\mathit{DFT}}^{{\mathit{OH}}^{\ast }}-{\mathit{E}}_{\mathit{DFT}}^{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{g}\right)}-{\mathit{E}}_{\mathit{DFT}}^{\ast }\right)+\left(\mathit{\Delta ZPE}-\mathit{T\Delta }{\mathit{S}}^{\mathit{0}}\right)\right]\\ +\left(\mathit{1}/\mathit{2}{\mathit{E}}_{\mathit{DFT}}^{{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)}-\mathit{eU}\right)\end{array}$$E66

Step 2:

The second step is oxidation of the OH^*species to O^*with release of a proton and an electron:

$$\begin{array}{l}{\mathit{\Delta G}}_{\mathit{2}}={\mathit{G}}_{{\mathit{O}}^{\ast }}+{\mathit{\mu }}_{{\mathit{H}}^{+}}+{\mathit{\mu }}_{{\mathit{e}}^{-}}-{\mathit{G}}_{{\mathit{OH}}^{\ast }}\\ =\left({\mathit{G}}_{{\mathit{O}}^{\ast }}-{\mathit{G}}_{{\mathit{OH}}^{\ast }}\right)+\left({\mathit{\mu }}_{{\mathit{H}}^{+}}^{\mathit{0}}+{\mathit{\mu }}_{{\mathit{e}}^{-}}^{\mathit{0}}-\mathit{eU}\right)\end{array}$$E67

The relation for

in terms of DFT energies is similar to the relation for (Eq. (64)). Replacing again the same equations as in the case for the first step in (Eq. (66)), we get:

$${\mathit{\Delta G}}_{\mathit{2}}=\left[\left({\mathit{E}}_{\mathit{DFT}}^{{\mathit{O}}^{\ast }}-{\mathit{E}}_{\mathit{DFT}}^{{\mathit{OH}}^{\ast }}\right)+\left(\mathit{\Delta ZPE}-\mathit{T\Delta }{\mathit{S}}^{\mathit{0}}\right)\right]+\left(\mathit{1}/\mathit{2}{\mathit{E}}_{\mathit{DFT}}^{{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)}-\mathit{eU}\right)$$E68

Step 3:${\mathit{O}}^{\ast }\to {\mathit{OOH}}^{\ast }+{\mathit{H}}^{+}+{\mathit{e}}^{-}$

The third step is represented by formation of the O^* on top of oxygen with a release of a proton and an electron:

$$\begin{array}{l}{\mathit{\Delta G}}_{\mathit{3}}={\mathit{G}}_{{\mathit{OOH}}^{\ast }}+{\mathit{\mu }}_{{\mathit{H}}^{+}}+{\mathit{\mu }}_{{\mathit{e}}^{-}}-{\mathit{G}}_{{\mathit{O}}^{\ast }}\\ =\left({\mathit{G}}_{{\mathit{OOH}}^{\ast }}-{\mathit{G}}_{{\mathit{O}}^{\ast }}\right)+\left({\mathit{\mu }}_{{\mathit{H}}^{+}}^{\mathit{0}}+{\mathit{\mu }}_{{\mathit{e}}^{-}}^{\mathit{0}}-\mathit{eU}\right)\end{array}$$E69

The relation for

and ${\mathit{G}}_{{\mathit{O}}^{\ast }}$in terms of DFT energies is similar to the relation for (Eq. (64)). The same equations are replaced gradually in the (Eq. (69)) as follows:

$${\mathit{\Delta G}}_{\mathit{3}}=\left[\left({\mathit{E}}_{\mathit{DFT}}^{{\mathit{OOH}}^{\ast }}-{\mathit{E}}_{\mathit{DFT}}^{{\mathit{O}}^{\ast }}\right)+\left(\mathit{\Delta ZPE}‐\mathit{T\Delta }{\mathit{S}}^{\mathit{0}}\right)\right]+\left(\mathit{1}/\mathit{2}{\mathit{E}}_{\mathit{DFT}}^{{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)}-\mathit{eU}\right)$$E70

Step 4:

The last step is the evolution of oxygen molecule:

$$\begin{array}{l}{\mathit{\Delta G}}_{\mathit{4}}={\mathit{G}}_{\ast }+{\mathit{\mu }}_{{\mathit{O}}_{\mathit{2}}\left(\mathit{g}\right)}+{\mathit{\mu }}_{{\mathit{H}}^{+}}+{\mathit{\mu }}_{{\mathit{e}}^{-}}-{\mathit{G}}_{{\mathit{OOH}}^{\ast }}\\ =\left({\mathit{G}}_{\ast }+{\mathit{\mu }}_{{\mathit{O}}_{\mathit{2}}\left(\mathit{g}\right)}-{\mathit{G}}_{{\mathit{OOH}}^{\ast }}\right)+\left({\mathit{\mu }}_{{\mathit{H}}^{+}}^{\mathit{0}}+{\mathit{\mu }}_{{\mathit{e}}^{-}}^{\mathit{0}}-\mathit{eU}\right)\end{array}$$E71

Therefore, we leave from the following equation:

$$\begin{array}{l}{\mathit{\Delta G}}_{\mathit{4}}=\left[{\mathit{E}}_{\mathit{DFT}}^{\ast }+\left(\mathit{4.92}+\mathit{2}\left({\mathit{E}}_{\mathit{DFT}}^{{\mathit{H}}_{\mathit{2}}\mathit{O}\left(\mathit{g}\right)}-{\mathit{E}}_{\mathit{DFT}}^{{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)}\right)\right)+{\mathit{E}}_{\mathit{DFT}}^{{\mathit{OOH}}^{\ast }}\right]\\ +\left(\mathit{\Delta ZPE}-\mathit{T\Delta }{\mathit{S}}^{\mathit{0}}\right)+\left(\mathit{1}/\mathit{2}{\mathit{E}}_{\mathit{DFT}}^{{\mathit{H}}_{\mathit{2}}\left(\mathit{g}\right)}-\mathit{eU}\right)\end{array}$$E72

Finally, the summation of $\mathit{\Delta }{\mathit{G}}_{\mathit{1}}$, $\mathit{\Delta }{\mathit{G}}_{\mathit{2}}$, $\mathit{\Delta }{\mathit{G}}_{\mathit{3}}$, and $\mathit{\Delta }{\mathit{G}}_{\mathit{4}}$should be 4.92 eV.

The reaction free energies of OH^*, O^*and OOH^*species on the surface of catalyst considered by ZPE and TS. Moreover, the free energy relations of the ORR in acidic media can also be explained in the same vein as the OER above mentioned.

2.3. Free energy diagram (FED) and Overpotential($\mathit{\eta }$)

We can deduce an important parameter of electrocatalytic activity from the calculated $\mathit{\Delta G}$, the magnitude of the potential-determining step (G^HERand G^OER/ORR) in consecutive reaction steps. This is the specific reaction step with the largest $\mathit{\Delta G}$in the HER and OER/ORR elementary reaction steps, that is, the concluding step to achieve a downhill reaction in the free energy diagram (FED) with increasing potential N, as shown in Figure 2 for HER and Figure 3 for OER/ORR:

$${\mathit{G}}^{\mathit{HER}}=\text{max}\left[\mathit{\Delta }{\mathit{G}}_{\mathit{1}}^{\mathit{0}},\mathit{\Delta }{\mathit{G}}_{\mathit{2}}^{\mathit{0}}\right]$$E73

$${\mathit{G}}^{\mathit{OER}/\mathit{ORR}}=\text{max}\left[\mathit{\Delta }{\mathit{G}}_{\mathit{1}}^{\mathit{0}},\mathit{\Delta }{\mathit{G}}_{\mathit{2}}^{\mathit{0}},\mathit{\Delta }{\mathit{G}}_{\mathit{3}}^{\mathit{0}},\mathit{\Delta }{\mathit{G}}_{\mathit{4}}^{\mathit{0}}\right]$$E74

$${\mathit{G}}^{\mathit{ORR}}=\text{max}\left[\mathit{\Delta }{\mathit{G}}_{\mathit{1}}^{\mathit{0}},\mathit{\Delta }{\mathit{G}}_{\mathit{2}}^{\mathit{0}}\right]$$E75

Figure 2.

Free energy diagrams (FEDs) of (a) Volmer-Heyrovsky pathway and (b) Volmer-Tafel pathway for HER, and (c) four-step associative OER pathway, and (d) four-step ORR pathway in alkaline/acidic media, and (e) two-step ORR pathway in alkaline media at zero potential$\left(\mathit{U}=\mathit{0}\mathit{V}\right)$, at equilibrium reduction potential$\left(\mathit{U}=\mathit{x}\mathit{V}\right)$and at overpotential. The$\mathit{x}$values indicate 0.402 V (alkaline) or 1.230 V (acidic).

Figure 3.

(a) Primitive cells of single heteroatom doped-graphene (GX, where G means graphene and X is B, N, Si, P, and S dopant) and (b) HER activitiesΔG^Volmerof GX as a function of primitive cell size. Red mark indicates dopant. There are two different types of structures depending on dopant, (c) in-plane and (d) out-of-plane.

The theoretical overpotential at standard conditions is then given by (Eq. (76)) in acidic and alkaline conditions, respectively:

$${\mathit{\eta }}^{\mathit{HER}}=\left({\mathit{G}}^{\mathit{HER}}/\mathit{e}\right)-\mathit{x}\mathit{V},\mathit{x}=\mathit{0.000}\mathit{V}$$E76

$$\begin{array}{l}{\mathit{\eta }}^{\mathit{OER}/\mathit{ORR}}=\left({\mathit{G}}^{\mathit{OER}/\mathit{ORR}}/\mathit{e}\right)-\mathit{x}\mathit{V},\\ \mathit{x}=\mathit{1.230}\mathit{V}\left(\mathit{\text{acidic}}\right),\text{and}\mathit{0.402}\mathit{V}\left(\mathit{\text{alkaline}}\right)\end{array}$$E77

In the case of HER pathways, the Volmer-Heyrovsky reaction is an electrochemical reaction involving electrons at all steps, as shown in Figure 2(a). Therefore, when the external potential ($\mathit{U}=\mathit{0.50}\mathit{V}$) is applied, the chemical potential of steps involving electrons shifts by the external potential ($\mathit{U}=\mathit{0.50}\mathit{V}$), and the Volmer-Heyrovsky reaction changes from uphill to downhill reaction. In contrast to the Volmer-Heyrovsky reaction, the Volmer-Tafel reaction is an electrochemical reaction involving electrons only in the Volmer step, as shown in Figure 2(b). Therefore, when the adsorption of hydrogen is unstable, the downhill reaction is possible by applying the external potential ($\mathit{U}=\mathit{0.25}\mathit{V}$), but when the adsorption of hydrogen is stable, the reduction of H⁺is spontaneous reaction, and the desorption of H₂in the Tafel step is the rate determining step. However, the desorption of H₂is a thermodynamic reaction, which is not involved in electrons, not an electrochemical reaction. In the case of OER/ORR pathways, the theoretical overpotential (η^{ΟΕΡ/ΟΡΡ}) represents the relative stability of the intermediates between (4OH⁻ + *)^alkaline, (2H₂O(l) + *)^acidicand (O₂(g) + *),and vice versa, as shown in Figure 2(c)-(e). In addition, it can be calculated by applying standard density functional theory (DFT) in combination with the computational standard hydrogen electrode (SHE) model. Because the equilibrium reduction potential is $\mathit{U}=\mathit{1.230}\mathit{V}\left(\mathit{\text{acidic}}\right)$and $\mathit{0.402}\mathit{V}\left(\mathit{\text{alkaline}}\right)$, the chemical potential difference between (4OH⁻)^alkaline, (2H₂O(l))^acidicand O₂(g)should be 1.608 and 4.920 V, respectively. However, the actual catalytic behaviors deviate from the ideal case due to correlation with binding energies of the intermediates. Therefore, most catalysts require overpotential (η^HERand η^OER/ORR) in order to achieve an overall downhill reaction. Consequently, the η^HERand η^OER/ORRthe important indicators of catalytic activities of a catalyst, and the lower η^HERand η^OER/ORRindicate a thermodynamically superior catalyst.

3. Structure-catalytic activity relationships

3.1. Heteroatom doped graphene (GX) for HER catalyst

Figure 3 shows a schematic of the heteroatom doped-graphene (GX, where G means graphene and X is B, N, Si, P, and S dopant) structures. We have used the second row elements (B and N) and the third row elements (Si, P, and S) in the periodic table in order to investigate the structural and electronic doping effects on HER activity because the third row elements are relatively larger than the second row elements and p- and n-type doping effects can be expected from the electron deficient B, and electron rich N, P, and S elements give in-plane and out-of-plane structures, respectively, due to the size of the dopants.

3.1.1. Structural and electronic doping effects on HER activity

On the atomic orbital hybridization characters of adjacent carbon atoms of dopant, the natural bond orbital (NBO) analysis show an increased p orbital contribution from sp² to sp³ hybridization of carbons adjacent to the dopant due to structural deformation from in-plane to out-of-plane. Compared to sp²-hybridized carbon, sp³-hybridized carbons more readily form an extra a hydrogen atom without additional structural change. Therefore, in out-of-plane structures, the subsequent two hydrogen atoms prefer to bind to only sp³ hybridized carbons adjacent to the dopant. However, in the case of in-plane structures having only sp²-hybridized carbons, the first hydrogen atom should result in structural deformation to form sp³-hybridized carbons. Therefore, the first hydrogen adsorption on the in-plane structure is less favorable than the reaction on out-of-plane structures. The second hydrogen atom can favorably bind to sp³-hybridized second neighboring carbons of dopant. Consequently, structural deformation with dopants that are third row elements is associated with improved HER activity due to atomic orbital hybridization, as shown in Figure 3(b). Looking at the electronic structures of GXs, p- and n-type doping effects are also expected from electron deficient and rich elements. In the case of in-plane GXs, electron deficient boron shifts its band structure up by withdrawing an electron from graphene, and electron rich nitrogen shifts its band structure down by donating an electron to graphene. Interestingly, in the case of out-of-plane GXs, electron rich phosphorous and sulfur dopant have no associated band shift. The origin of the flat band can be understood based on the localization of an extra electron onto the dopant site. In order to verify the relationship between geometric and electronic structures of GXs, we have systematically changed the structures of GXs from in-plane to out-of-plane structures and vice versa. These calculations clearly show that dopant can produce n- and p-type doping states as well as a localized state depending on the structure of GXs induced by the type of dopants. When the out-of-plane (in-plane) deformation is applied in the in-plane (out-of-plane) GXs, band structures change from the p-type doping state (localized state) to the localized state (p-type doping state). Therefore, it is worth mentioning that the localized electronic states can be associated with physical regularity of HER activities on the out-of-plane GXs.

3.2. Heteroatom doped C₃N₄ (X_Y-C₃N₄) for OER/ORR bi-functional catalyst

In this work, we have systematically investigated a metal-free bifunctional electrocatalyst of heteroatom-doped carbon nitride (X_Y-C₃N₄, where X and Y indicate the dopant and doping site on C₃N₄, respectively) for oxygen evolution and oxygen reduction reactions (OER and ORR) in alkaline media, considering the possible reaction pathways based on the Eley-Rideal (ER) mechanism as well as the doping effects on electrocatalytic activity. Moreover, we determined that the relative stability of O^*and OOH^*intermediates was a key factor determining the ORR pathway; accordingly, ORR follows a two-step reaction pathway governed by O^*rather than a four-step reaction pathway governed by OOH^*. Firstly, we calculated relative E_fand the most stable structures of heteroatom-doped C₃N₄ structures, X_Y-C₃N₄, where X = P, S, or PS and Y = C or N [18, 20]. By considering the E_f(formation energy) results as well as the various doping sites, we determined the most stable X_Y-C₃N₄ structures, P_CA-C₃N₄, P_NB-C₃N₄, S_CB-C₃N₄, S_NB-C₃N₄, P_CAS_CB-C₃N₄, P_NAS_NB-C₃N₄, and P_CAS_NB-C₃N₄, for the investigation of OER/ORR bifunctional electrocatalytic activities and their reaction mechanisms in alkaline media.

3.2.1. OER and ORR catalytic activity on X_Y-C₃N₄

Figure 4 (a) and (c) show the volcano plot of OER and ORR in alkaline media at all possible active sites on X_Y-C₃N₄, which represents the apparent catalytic activity, respectively. This theoretical analysis reveals that the P_CS_C-C₃N₄ structure has minimum η^OER(0.42 V) and η^ORR(0.27 V). The η^OER/ORRvalue of P_CS_C-C₃N₄ is comparable to those of the best conventional catalysts (∼0.42 V for OER on RuO₂ and ∼0.45 V for ORR on Pt). Most elementary steps in OER have an uphill reaction at 0.00 V and at equilibrium potential of 0.402 V. Analyzing the FED at the equilibrium potential of 0.402 V, we can define the rate determination step as the formation of OOH^*from O^*on P_CS_C-C₃N₄, as shown in Figure 4 (b). Therefore, the $\mathit{\Delta G}$at the rate determination step, 0.42 V, become the η^OERfor facilitating the OER as a spontaneously downhill reaction. By applying the increased electrode potential of 0.82 V, all elementary reactions can be downhill reactions for spontaneous OER. In the case of the ORR, we considered the O₂adsorption free energy (ΔG_O2*) and η^ORRare highly correlated to determine ORR activity. If the O₂adsorption reaction is very difficult to achieve as an initiation step in ORR, that material cannot have ORR activity, even though it can have a possibility to have a very small η^ORR. Therefore, we defined a new indicator of ORR activity as figure of merit (FOM), which is defined by FOM = −(η^ORR + ΔG_O2*). Using FOM, we constructed a volcano plot of ORR at all possible active sites on X_Y-C₃N₄ in order to compare the ORR catalytic activity, as shown in Figure 4 (c), where the P_CS_C-C₃N₄ structure have minimum η^ORRof 0.27 V.

Figure 4.

The volcano plots of (a) OER and (c) ORR at all possible active sites on X_Y-C₃N₄ and the free energy diagrams (FEDs) of P_CS_C-C₃N₄ structure having the best catalytic activity.

3.2.2. Structural and electronic doping effects on OER/ORR activity

The synergistic effect of P, S co-doping can be explained based on the geometric and electronic effects of heteroatoms [17, 18, 19, 20]. Considering the atomic size of heteroatoms, the relatively larger S and P dopants can cause structural deformation of X_Y-C₃N₄, which improves the OER and ORR activity by enhancing the stability of intermediates with increasing p orbital character of active sites adjacent to the dopant from sp² to sp³ hybridization. Compared to sp² hybridized orbitals on pure C₃N₄, sp³ character of active sites on X_Y-C₃N₄ is more suitable for forming chemical bonds with intermediate species. Therefore, in out-of-plane structures, the intermediates prefer to bind to sp³-hybridized active sites. Moreover, to verify the relationship between geometric and electronic structures of X_Y-C₃N₄, we intentionally changed the structures of X_Y-C₃N₄ from in-plane to out-of-plane to increase the activity for binding intermediate species by increasing the sp³ character of active sites on X_Y-C₃N₄. We investigated density of state (DOS) of pure C₃N₄ and X_Y-C₃N₄ (X = P, S, or PS and Y = N) to determine at what condition the OER/ORR exhibit outstanding performance [18, 20]. It can be expected that electron-rich heteroatom doping will induce electronic structure changes from a non-metallic doping effect to a metallic doping effect due to a downward band shift. As a result, P_CS_C-C₃N₄ shows the best OER/ORR activity by maintaining a metallic property despite the presence of out-of-plane deformation. Consequently, it can be emphasized that there is a close correlation between the electronic/geometric structure and OER/ORR catalytic activities, and the best bifunctional OER/ORR catalytic activity of P,S co-doped P_CS_C-C₃N₄ is attributed to a synergistic effect between the electronic and geometric effects.

4. Conclusion

We have systematically investigated the detailed mechanisms of HER/OER/ORR and the synergistic effect between geometric and electronic factors plays an important role in HER/OER/ORR catalytic activities of GXs and X_Y-C₃N₄. In this work, we demonstrated that the HER/OER/ORR activity of GXs and X_Y-C₃N₄ can be modulated by structural and electronic factors, including structural deformation with dopants. These structural and electronic factors enhance adsorbent binding strength during the reactions in HER/OER/ORR by generating sp³-hybridized atoms and facilitating charge transfer between adsorbents and GXs/X_Y-C₃N₄ as metallic properties. Additionally, we re-evaluated the generally accepted ER mechanism of OER/ORR by comparing the stability of intermediates governing the reactions, where we found that the OER/ORR respectively follows four-step and two-step reaction pathway. We also elucidated the importance of the ${\mathit{O}}_{\mathit{2}}$adsorption free energy (ΔG_O2*)in ORR activity. Considering the ΔG_O2*with a FOM, FOM = −(η^ORR + ΔG_O2*), we successfully represented the ORR activity of X_Y-C₃N₄. We believe that the understanding of the detailed mechanism as well as the relationship of structure-electrocatalytic activity of the HER/OER/ORR can facilitate development of new electrocatalytic materials.

Acknowledgments

This research was supported by grants from the Basic Science Research Program through the National Research Foundation of Korea (NRF) funded by the Ministry of Science, ICT, and Future Planning (NRF-2018R1A2B6006320). This work was also supported by the Supercomputing Center/Korea Institute of Science and Technology Information with supercomputing resources including technical support (KSC-2017-C3-0032).