Coupled Transport of Electrons and Protons in a Bacterial Cytochrome c Oxidase—DFT Calculated Properties Compared to Structures and Spectroscopies

Abstract

After a general introduction to the features and mechanisms of Cytochrome c Oxidases (CcOs) in mitochondria and aerobic bacteria, we present DFT calculated physical and spectroscopic properties for the catalytic reaction cycle compared with experimental observations in bacterial ba₃ type CcO, also with comparisons/contrasts to aa₃ type CcOs. The Dinuclear Complex (DNC) is the active catalytic reaction center, containing a heme a₃ Fe center and a near lying Cu center (called Cu_B) where by successive reduction and protonation, molecular O₂ is transformed to two H₂O, and protons are pumped from an inner region across the membrane to an outer region by transit through the CcO integral membrane protein. Structures, energies and vibrational frequencies for Fe-O and O-O modes are calculated by DFT over the catalytic cycle. The calculated DFT frequencies in ba₃ CcO are compared with measured frequencies from Resonance Raman spectroscopy to clarify the composition, geometry, and electronic structures of different intermediates through the reaction cycle, and to trace reaction pathways. X-ray structures of the resting oxidized state are analyzed with reference to the known experimental reaction chemistry and using DFT calculated structures in fitting observed electron density maps. Our calculations lead to a new proposed reaction pathway for coupling the P_R → F → O_H (ferryl-oxo → ferric-hydroxo) pathway to proton pumping by a water shift mechanism. Through this arc of the catalytic cycle, major shifts in pK_a’s of the special tyrosine and a histidine near the upper water pool activate proton transfer. Additional mechanisms for proton pumping are explored, and the role of the Cu_B⁺ (cuprous state) in controlling access to the dinuclear reaction site is proposed.

Graphical Abstract

DFT calculated structures, vibrational frequencies, and energiesprovide insights into the reaction/proton pumping cycle ofcytochromec oxidase.

1. Introduction-Overview

Cytochrome c oxidase (CcO) (Complex IV) is the terminal electron acceptor in the electron transport chain of mitochondria and of aerobic bacteria. It functions as an oxygen binding, redox driven proton pump across the mitochondrial or paraplasmic membrane, respectively. The functions, mechanisms, and kinetics of various types of CcO in various organisms ranging from aerobic bacteria to mitochondria in eukaryotic cells, including many types of mammalian cells are complex, and encompass both extensive similarities and important differences.^1–6 As discussed below, CcO is part of the electron transport chain, and operates as part of a biological network of integral membrane proteins.^7–12 Collectively, Complexes I-IV generate an electrochemical proton gradient which drives the synthesis of ATP.¹³ All cytochrome c oxidases of mitochondria (Type aa₃), or in aerobic bacteria (different types aa₃ or ba₃) have closely related core subunits, which are the energy generating core of the system, combining redox driven catalytic cycling coupled to proton pumping in the intact membrane embedded protein complex. There are typically three different core energy subunits. Mitochondria also have a number of additional regulatory subunits. To explore the outstanding problems of mechanism and kinetics in these proteins requires a multimodal attack, including X-ray structures, spectroscopies, kinetics, physical properties, and theory/calculations. Our goal is to use quantum chemistry as a unifying framework for exploring important features of geometric and electronic structure throughout the catalytic reaction cycle, encompassing structures, energetics, dynamics, and spectroscopy, relating these to proton pumping mechanisms as well. We will look at one particular bacterial cytochrome c oxidase in detail, cytochrome ba₃ from Thermus thermophilus (Tt).¹⁴

2. Mapping System Structures, Active Elements, and Pathways

2.1. Defining the Paths and Linkages of Electron and Proton Transport through the Electron Transport Chain in Mitochondria and Aerobic Bacteria

The transport of electrons through the electron transport chain common to mammalian mitochondria and aerobic bacteria occurs using mobile electron and proton carriers interacting with the integral membrane Complexes I,II,III,IV (see Figure 1) embedded in the mitochondrial inner membrane or the periplasmic membrane in aerobic bacteria.¹³ The linkage between these electron carriers and the integral membrane protein Complexes allows proton pumping to occur across the membrane, which lead to the build-up of a transmembrane electrochemical potential. This transmembrane potential difference is the source of most biological energy in the form of ATP. Protons entering the inside of the inner membrane from the outside pass through a rotor in the integral membrane protein Complex V (ATP Synthase) and ATP is synthesized from ADP and inorganic phosphate (Pi) driven by the transmembrane electrochemical potential.

Figure 1.

Schematic of the four integral membrane protein complexes I-IV in the electron transport chain in mitochondria. Reprint with permission from Figure 1 of Ref 13, copyright © 2008 Elsevier.

In the electron transport chain, there are two types of mobile carriers. Reduced ubiquinone (called QH₂) is a relatively small amphiphilic organic cofactor that carries two electrons and two protons (2e⁻,2H⁺). By contrast, cytochrome c is a mobile protein carrier of single electrons (1e⁻) only. Reduced ubiquinone is generated from the oxidized form by loss of (2e⁻,H⁺) from reduced NADH in the catalytic process NADH → NAD⁺ + 2e⁻ + H⁺ in Complex I. Complex I also pumps protons across the membrane by a complicated electron linked proton transfer process. Complex II also generates QH₂ from the oxidized form Q. Further along the electron transport chain, Complex III delivers electrons one at a time to the mobile metalloprotein cytochrome c, Cytc(ox) +1e⁻ → Cytc(red), for the oxidized (heme Fe³⁺) and reduced (heme Fe²⁺) forms respectively.

2.2. A Comparison of Two Integral Membrane Proteins—Complexes III and IV

While all of these complexes contribute to generating the membrane potential, and all but Complex II pump protons across the inner membrane, our focus here is on Complex IV, cytochrome c oxidase (CcO) in two relevant types, aa₃ (A-Type, found in mitochondria and in some aerobic bacteria), and ba₃ (B-Type, found in other aerobic bacteria, which will be our main focus).

In the presence of these complicated biological networks, it is very helpful to compare and contrast different systems. A conceptually and historically important comparison and contrast is between Complex III and Complex IV.

In Complex III (Cytochrome bc₁), the redox and proton transfer cycle is called Mitchell’s Proton Motive Q Cycle. It is a “Redox Loop Mechanism” with an internal mobile carrier ubiquinone, and large scale movements of membrane domains, in particular, the Rieske iron-sulfur cluster protein fragment, with the Fe₂S₂ cluster and nearby amino acid residues called the head group.¹⁵

The overall full cycle stoichiometry is

$$2{\text{QH}}_2\left(\text{outer}\right)+\text{Q}\left(\text{inner}\right)+{\left(2{\text{H}}^{+}\right)}_{\text{in}}\to 2\text{Q}\left(\text{outer}\right)+{\left(2{\text{e}}^{-}\right)}_{\text{out}}+{\left({\text{4H}}^{+}\right)}_{\text{out}}+{\text{QH}}_2\left(\text{inner}\right)$$ (1)

There are two cycles in series where two separate QH₂(outer) enter the protein, to pump (4H⁺+2e⁻) out, reduce two oxidized Cytochrome c (Cytc) by 1e⁻ each, and where Q(inner) picks up 2e⁻ total from two cycles of QH₂(outer), and 2H⁺_in from the inside (n side, negative (−)) of the membrane. Outer means near the Q_o binding site within the protein, toward the positive outer side of the membrane (p side), while inner means near the Q_i binding site within the protein, near the negative inner side of the membrane (n side).

(Cycle 1):

$${\text{QH}}_2\left(\text{outer}\right)+\text{Q}\left(\text{inner}\right)\to \text{Q}\left(\text{outer}\right)+{\left(2{\text{H}}^{+}\right)}_{\text{out}}+{\text{Q}}^{•-}\left(\text{inner}\right)+{\left({\text{1e}}^{-}\right)}_{\text{out}}$$ (2)

(Cycle 2):

$${\text{QH}}_2\left(\text{outer}\right)+{\text{Q}}^{•-}\left(\text{inner}\right)+2{{\text{H}}^{+}}_{\text{in}}\to \text{Q}\left(\text{outer}\right)+{\text{QH}}_2\left(\text{inner}\right)+{\left(2{\text{H}}^{+}\right)}_{\text{out}}+{\left({\text{1e}}^{-}\right)}_{\text{out}}$$ (3)

The one Full Cycle (Eq. 1) is the sum of the two asymmetric Cycles 1 and 2 depicted below it. The molecule Q^•−(inner) is the semiquinone radical anion that is a common intermediate linking these cycles. Although it is not in the cycles summarized above, Q^•−(outer) is an unstable intermediate which facilitates the bifurcation of electron flow via heme b_L. It is a product of the QH₂(outer) oxidation and deprotonation which occurs through the interaction with the Rieske Fe₂S₂ cluster protein.

Figure 2 depicts the electron transfers in more detail, but not the proton paths. The Figure is Schematic, and does not show the major conformational shift of the Fe₂S₂ head group moving to dock with the cytochrome c₁ binding site.^16–19

Figure 2.

Metal centers and electron transfers in Cyt bc₁ (Complex III). Reprint with permission from Figure 2 in https://quantbiolab.com/research/superoxide-production-in-the-bc1-complex, copyright © 2020 Ilia Solov’yov and Peter Husen, QuantBio.

Anticipating our later discussion of CcO, the mechanism of CcO differs from that of Cyt bc₁ in a number of important ways. In Cyt bc₁, there is an internal mobile carrier of electrons and protons, QH₂, which can move both within the membrane and within the protein forming two pools and having two binding sites labelled Q_o and Q_i, for electron and proton transfer. There is a bifurcation (splitting) of electron transfer pathways between an upper pathway, and a lower pathway, which occurs near Q_o. As mentioned before, there is extensive mobility of the iron-sulfur fragment subunit. By contrast, in CcO, there are no mobile carrier molecules for electrons or protons; all electron and proton transfers are through the protein and water network, and all mobility involves either water or protein sidechains and backbone movements. The conformational changes are smaller, where present. The electron transfer path starts with 1e⁻ transfer from cytochrome c, which was reduced by Cyt bc₁. The subsequent electron transfer pathway is unidirectional, forming an approximate L shaped pathway from the Cu_A site (a copper-dimer complex) to heme a (or heme b) Fe to the heme a₃ Fe, and then terminating in the Cu_B site. In CcO’s, there is a splitting in proton pathways, which is, in part, a consequence of the difference between the so-called chemical protons, which react with electrons and bound oxygen species to finally produce water, and the pathways of pumped protons. There are also significant differences between the two families of CcO, the A-Family versus the B-Family.

2.3. Cytochrome c Oxidases—Similarities in the Catalytic Cycle, Differences in the Proton Pumping and Reaction Pathways of ba₃ (B-Family) vs. aa₃ (A-Family)

In Figure 3, we present a structural map of the overall path of reactants and products for the ba₃ type (B-Family) of CcOs, specifically for the protein from Tt.^14,20–23 The heme b and its Fe_b is not seen in Figure 3, since it lies behind the dinuclear center Cu_B-Fe_a3-heme in this perspective. The positioning of heme a in aa₃ CcO is similar.

Figure 3.

Schematic of cytochrome ba₃ with noted functionalities. SU is subunit. Reprint with permission from Figure 1 of Ref 24, https://pubs.acs.org/doi/10.1021/ic500363h, copyright © 2014 American Chemical Society (further permissions for reusing this figure should be directed to the ACS).

The mechanism for the chemical reaction

$${\text{O}}_2+4{\text{e}}^{-}+4{{\text{H}}^{+}}_{\text{in}}\to 2{\text{H}}_2\text{O}$$ (4)

is similar for both families, but the proton pumping input and exit pathways, and the water exit pathways are different. One should note that the proton input pathway (from the bottom of the figure upward) is opposite to that of the electron (e⁻_in) entry, from the top, originating from reduced cytochrome c. (Figure 3). The molecular oxygen (O₂) is more hydrophobic and enters the protein from the membrane via a fairly hydrophobic channel. After the pumped protons are included, the overall equation becomes

$${\text{O}}_2+4{\text{e}}^{-}+\left(4+\text{n}\right){{\text{H}}^{+}}_{\text{in}}\to 2{\text{H}}_2\text{O}+{{\text{nH}}^{+}}_{\text{out}}$$ (5)

where n = 4 (approximately, in the aa₃ type), and n = 2 to 4 in the ba₃ type (as found for Tt).²⁵ Current experimental evidence is consistent with less efficient pumping pathways in Tt ba₃, but still with very significant pumping.²⁶

Differences in proton pathways between aa₃ Class^27–32 (in mitochondria and in aerobic bacteria) versus ba₃ Class^14,20–23 (in other aerobic bacteria) are depicted in Figure 4, showing these protein structures with the different proton paths superimposed, D and K Path in aa₃, versus K_B path, also called the K analogue path, in ba₃. The different subunits are shown in purple (Subunit I) and yellow (Subunit II). The K-input path in aa₃ (Rhodobacter sphaeroides)²⁸ is named for a lysine (K362) along that pathway. In Tt ba₃, there is no similar structural lysine present in the K_B pathway, although there are other similar features, like the glutamic acid at the entrance, and the proton pathway exit point at a special tyrosine (Y288 in aa₃ and Y237 in ba₃). A more dramatic difference is the presence of a hydrophilic pathway with a line of waters (green) and a number of hydrophilic or charged residue sidechains in aa₃ from R. sphaeroides, in contrast to the absence of this pathway in ba₃ from Tt. Also, the position of the important and often charged glutamic acid (E286) in aa₃ (R. sphaeroides) (Figure 4) is structurally fairly homologous to that of the nonpolar isoleucine (I-Ile235) in ba₃ (Tt) (Figure 3).

Figure 4.

Comparison of the proton delivery pathways for the A- and B-types CcO’s. Reprint with permission from Figure 3 of Ref 33, H. Y. Chang, et al. 2009.

There is value in performing some simple bookkeeping analysis of differences in proton transport pathways in the different forms of CcO, aa₃ Type vs. ba₃ Type. First, we show a simple schematic Figure 5 of the electrochemical potential difference (mainly a difference in the electrostatic potential) across the membrane. This is useful for clarity of language, and to show directionality of the potential across the membrane. The inside of the membrane is the n side (negative potential, −) while the outside is the p side (positive, +). Referring back to Figure 3 and Eqs. 4 and 5, both the chemical reaction, where the electrons and protons react and combine with O₂ (Eq. 4), and the proton pumping (Eq. 5) contribute proportionately (ratio 4:n charges) to the overall electrostatic potential (proportional to (4+n) charges translocated). The reacting protons are called the Chemical © protons while the protons that are pumped are the Vector (V) protons.

Figure 5.

the Electrochemical potential gradient across the membrane.

Table 1 shows the different sources of protons for chemical reaction (C) versus protons shuttled into the pumping pathways (V). This is a condensation of observations based on electrometry and kinetics with and without ionophores on lipid vesicles with embedded proteins, and also utilizing mutagenesis to sort out proton transfer pathways. Clearly, large differences exist here between aa₃ type and ba₃ type. The ba₃ type has only one type of pathway in (K Path), which must account for both the Chemical protons entry into the reaction area (called the “reaction chamber”), and for the Vector protons to be pumped. There must be a bifurcation point (or region), where these pathways split. By contrast, the aa₃ type has two different paths in, K and D. The K path analogue in ba₃ must do all the work of supplying both the 4 Chemical and 2 to 4 Vector protons. By contrast, the experimental evidence available indicates that the K path makes a smaller (2 proton) contribution to the overall chemical reaction, and none at all to the proton pumping in aa₃. In aa₃, the mechanism of the D pathway remains a matter of controversy. Further, in the mitochondrial protein, as found in eukaryotes, there is also a proposed H pathway, which may do some or all of the proton pumping in place of the D path in aa₃ type bacteria.

Table 1.

Proton Transport Pathways in CcO: Differences in Proton Channels.

aa3 Type (Bacterial and Mitochondrial)
Types	Chemical (C)	Vector (V)	Total Over Paths
K Path	2	0	2
D Path	2	4	6
All Paths	4	4	8
ba3 Type (Bacterial)
Types	Chemical (C)	Vector (V)	Total Over Paths
K Path	4	2-4	6-8
D Path	0	0	0
All Paths	4	2-4	6-8

2.4. Distinctive Features of ba₃ in Spectroscopy and Kinetics

For our purposes, it will be sufficient to explore some aspects of the chemical catalytic reaction cycle pathways, and potential mechanisms of proton pumping in the ba₃ type from Tt, and to draw some comparisons and contrasts with aa₃ type CcO’s. In addition to the greater simplicity inherent in having all protons come in through the K pathway, there is a practical experimental advantage in tracing the reaction kinetics. In both aa₃ and ba₃ types, the electron pathway proceeds by 1e⁻ transfer from cytochrome c (reduced, Fe²⁺, Cyt c), first to the Cu_A Complex (containing a 2Cu dimer), and then to an Fe heme b (in ba₃) or heme a (in aa₃) and on to the dinuclear (DNC) (also called binuclear BNC) Complex, containing an Fe_a3 heme closely associated with a Cu_B-(His)₃ unit. The Fe heme b versus Fe heme a₃ difference makes it easier to distinguish by optical difference spectroscopy between reduction of Fe_b versus Fe_a3, while these bands are overlapping in Fe_a versus Fe_a3.

2.5. Catalytic Reaction Cycle of CcO

The catalytic reaction cycle of the Dinuclear Complex (DNC) is depicted in Figure 6. We include important intermediate states that have been identified spectroscopically as well as others that have been proposed linking observed states.³⁴ To explore this cycle, we begin with State R, the reduced state, where Fe_a3 and Cu_B have respective oxidation states, Fe²⁺ and Cu⁺. For the entire CcO protein to be in the fully reduced state, the other metal centers also must be reduced. For Cu_A, the reduced copper dimer state is then Cu⁺-Cu⁺. The corresponding oxidized state is the unusual delocalized mixed valence dimer, Cu^1.5+-Cu^1.5+. The other mononuclear heme Fe center (either heme b or heme a depending on CcO type) has reduced state Fe²⁺ and is low spin S = 0. Both Cu_A and the mononuclear Fe are 1e⁻ donors to the DNC, so there is a net of 4 electrons available to carry out the catalytic 4e⁻ reduction of O₂ to 2H₂O in Eq. 4 (or Eq. 5). We will refer to the mononuclear heme Fe center and Cu_A pair as Fe/Cu_A. The reaction cycle commences by coordination of O₂ to Fe_a3 to form the adduct state A. The cycle then progresses quickly through the proposed Peroxo and Hydroperoxo states to the experimentally identified states P_M/P_R and further to state F. O₂ has already been reduced by four electrons in states P_M/P_R, with three electrons provided by Fe_a3 and Cu_B and one electron provided by the special tyrosine in state P_m, while one electron has been replenished from Fe/Cu_A in state P_R. One chemical proton has been taken up at this point and uptake of a second chemical proton leads to state F. The subsequent reduction of the heme a₃ ferryl-oxo complex via another electron from Fe/Cu_A and uptake of another proton is significantly slower and leads to active cycling oxidized state O_H via the postulated intermediate state F_H. In summary, at this point, consumption of the 4 available electrons to reduce O₂ results in the active cycling oxidized State O_H. To continue cycling, two electrons must be delivered from Cytc to the DNC to reduce Fe_a3 and Cu_B transiting via Cu_A/Fe, and soon after two more electrons total from Cytc are needed at Fe/Cu_A to regenerate the fully reduced State R. Up to 4 vectorial protons are pumped across the membrane during the reaction cycle. The reaction cycle intermediates observed spectroscopically were characterized by optical difference spectroscopy³⁵ and by Resonance Raman (RR) spectroscopy ,³⁶ but the detailed active site structures were only partly established this way. In the Figure, the kinetic rate constants were taken from Einarsdottir’s kinetics study using optical difference spectroscopy on the ba₃ form of CcO from Tt,³⁵ while the RR frequencies presented are for Fe-O stretch vibrations for aa₃ type from bovine mitochondria.^37–52 For ba₃, the corresponding RR spectra have not been done, but the catalytic mechanism and intermediates should be similar. The kinetics of ba₃ are known to be different in detail from that in aa₃ bacterial proteins and mitochondrial proteins by optical difference spectroscopy. One main difference is that the O₂ binding affinity and rate constant are higher in ba₃ than aa₃. For proton transfers, the redox, oxygen binding species, and protonation states of intermediates are clearer than the detailed sequence and timing of pumping events, which also differ between ba₃ and aa₃.³⁵ The mechanisms and reaction energetics (and kinetics) of proton transfer both within the catalytic cycle and for proton pumping have considerable uncertainties.

Figure 6.

Feasible intermediate states of the DNC in the catalytic cycle, in which A, P_M/P_R, F, and O_H were identified by resonance Raman experiments on A-type oxidases,^37–52 and their DNC’s are likely in the forms presented above. Although the Peroxo, Hydroperoxo, and F_H states (drawn in red frames) were not observed experimentally, they may exist for a short time. Tyr is the special Y288 in aa₃ and Y237 in ba₃.

In Table 2, we summarize known mechanisms for proton and electron transport in redox active proteins. Since both protons and electrons are quantum objects, both can exhibit tunneling through proteins by covalent pathways, by hydrogen bonded pathways, and also through space, the last with much more difficulty. The ranges quoted reflect the shorter tunneling range of protons, which are about 1800 times as massive as electrons. This tunneling is through barriers, but there are also adiabatic (bonded) pathways for electrons, and normal barrier transits for proton transfers. Both electrons and protons can be carried on mobile carriers like ubiquinone, and protons can be transferred by movement and protonation/deprotonation of amino acid side chains, or carried on water as H₃O⁺ or OH⁻. Further, chains of waters and amino acid sidechains can perform effective fast long range proton transfer by concerted or partly coordinated proton transfers along a hydrogen bonded chain, as first proposed by Grotthuss.⁵³ The more concerted form of this process requires a very ordered chain of H-bonded units, and a set of low barriers that can be only imperfectly attained in most biological systems. All of these different mechanisms need to be considered in redox driven proton pumps like CcO and Cytochrome bc₁.

Table 2.

Modes of Proton Mobility and Electron Mobility.

The Variety of Electron and Proton Transport in Proteins and Membranes
• Electron tunneling – max range about 11-14 Å	• Proton tunneling – max range about 1 Å
• Electron transport on mobile carrier	• Proton transport on mobile carrier
	• Proton transport on amino acid sidechain
	• Proton transport by diffusion on water (H2O as carrier)
	• Grotthuss Process53 – fast proton transfer along chains of water molecules, also in combination with amino acid sidechains (Bucket Brigade Mechanism)

3. DFT Methods, Directions, and Applications

3.1. DFT Electronic Structure and Geometry Optimization

The starting geometries for electronic and geometry optimization for the DNC intermediate states are based on the ba₃ CcO X-ray crystal structure 3S8G¹⁴ for the “resting oxidized as-isolated” state.^24,54–60 These atom arrangements and geometries are altered to those proposed for the various states of the catalytic cycle based on what is known from spectroscopies and kinetics, with subsequent geometry optimization and further exploration of alternative structures. The geometry optimizations are performed using the ADF^61–63 codes with the spin-polarized broken-symmetry method.^64–66 Different DFT functionals like PW91, B3LYP, B3LYP*, OPBE, and OLYP have been tested in our earlier work (see section 3.9).^24,34 While the OLYP-D3-BJ exchange-correlation potential with dispersion correction (D3-BJ force field)⁶⁷ has been used in our recent studies,^58–60 together with the triple-ξ-polarization (TZP) Slater type basis sets on the metals, and DZP (double-ξ-polarization) on all other atoms, and with the COSMO^68–71 solvation model for the outer environment with dielectric constant (ε = 18.5), reflecting considerable polarity as found in the remaining protein complex and solvent outside the quantum cluster region. For some states of the catalytic cycle in our vibrational frequency calculations,⁵⁹ we have added energy corrections for spin-projection effects using the Yamaguchi equation,^72–74 but we have not tried to incorporate these into our very recent resting as-isolated State O calculations;⁶⁰ we think that effects there will prove to be small, since the spin coupling between Fe^2+,3+ and Cu²⁺ in those geometries is small.

Figure 7 gives our geometry optimized quantum cluster model for State A,⁵⁹ the ferric-superoxide complex of the DNC, formed upon binding of molecular oxygen to the ferrous Fe²⁺ in State R which can be compared to the schematic form in Figure 6. Notice also that Cu is in the reduced cuprous redox state, Cu⁺, which affects the subsequent reaction path.

Figure 7.

Our quantum cluster model for state A of the DNC, built from the X-ray crystal structure 3S8G of ba₃ CcO from Tt.¹⁴ For more visibility, some apolar or link H atoms are not shown on the picture. Taken with permission from Figure 3 of Ref 59, copyright © 2019 American Chemical Society.

As already suggested in Figure 6, for a good representation of the catalytic cycle, different binding states of oxygen species, different Fe and Cu redox states in the DNC, different protonation states (also tautomeric states), and different water locations must be evaluated. The presence of water as both a medium useful for stabilization of states and transit, and also as a reaction product introduces further essential complexities. As depicted in Figure 7, Tyr237 in Tt ba₃ (and the structurally homologous Tyr288 in aa₃ enzymes) is special; the Tyr phenol is covalently linked to the His233 sidechain ring via a C-N covalent bond, and the His ring is a ligand to Cu_B. This linkage is universal in aa₃ and ba₃ CcO’s and unique from all other metalloenzymes. At this point, we reflect also on the combination of different redox states and protonation states accessible for amino acid sidechains in CcO. For the special tyrosine, there are three states Tyr-O^• (neutral radical), Tyr-O⁻ (anion), and Tyr-OH (neutral protonated). The Tyr-O is also the end of the K pathway for protons. For other residues, we will see later that there is a potentially redox active tryptophan with states Trp (neutral) and Trp^•+ (radical cation). Histidine is usually considered to have three states His(neutral, protonated at δ), His(neutral, protonated at ε), and His⁺(cation, protonated at both). However, when bonded to a high oxidation state metal Cu²⁺, the His⁻ (anion) state is also possible.

Turning now to the Fe_a3 sites, in addition to the relevant redox states Fe²⁺, Fe³⁺, Fe⁴⁺, there are different site spin states possible: high-spin (HS), intermediate-spin (IS), and low-spin (LS). For Cu_B, the redox states cycle between Cu⁺ and Cu²⁺ and connect to the linked redox and protonation states of the special His-Tyr pair.

3.2. Vibrational Frequencies

For vibrational frequency calculations,⁵⁹ we used two different complementary methods at the geometry optimized structures.⁶¹ From the original cluster model of about 200 atoms, we compute a partial Hessian (about 110 atoms) using analytic frequency calculations in the region surrounding the FeCu center, excluding atoms in the upper cluster region (Arg449, His376, Asp372, and four upper waters) plus two waters that are shifted up HOH604 and HOH608 in the intermediate states F, F_H, and O_H. We have also done comparative calculations with the numerical mobile block Hessian method,^75,76 where the residue sidechains in the upper region and nearby waters are treated as individual mobile blocks. Both methods yield very similar vibrational frequencies for Fe-O stretching modes, and also for O-O or O-Fe-Por bending modes.

3.3. Recent DFT Work on ba₃ in Comparison with Experimental Spectroscopy (Resonance Raman): Fe-O and O-O Geometries versus Stretch Frequencies

In Figure 8, we report a graph comparing calculated versus experimentally observed Resonance Raman frequencies for Fe_a3-O stretching frequencies over intermediate states of the catalytic cycle.⁵⁹ In Figure 9, we explore the accuracy of an old empirical correlation for bond lengths versus frequencies, called Badger’s rule⁷⁷ applied to examining Fe-O bond lengths versus stretch frequencies. We find that this correlation is very good and reliable based on our calculations. Also, Figure 10 shows that the calculated O-O stretch frequencies correlate very well, linearly, with the O-O bond length; Figure 11 shows that these same frequencies correlate similarly well with the calculated Mayer Bond Order.⁷⁸ There are only a few structures in the cycle which have intact O-O bonds, but the frequencies for superoxide O-O in State A, and O-O in our Peroxo structure match those in related synthetic systems^79–82 very well (see the discussion below).

Figure 8.

Calculated vs. available experimental Fe_a3-O vibrational stretching modes for the DNC intermediate states. Reprinted with permission from Ref 59, copyright © 2019 American Chemical Society.

Figure 9.

Correlation between the calculated Fe_a3-O bond lengths (r_Fe-O, Å) and the corresponding Fe_a3-O stretch frequencies (1/ν_Fe-O^2/3, based on Badger’s rule) for the eight DNC state structures studied.⁵⁹ Reprint with permission from Figure 7 of Ref 59, copyright © 2019 American Chemical Society.

Figure 10.

Correlation between the calculated O-O stretching frequencies (ν(O-O), cm⁻¹) and the O-O bond lengths (r_O-O, Å). Taken with permission from Figure 6 of Ref 59, copyright © 2019 American Chemical Society.

Figure 11.

Correlation between the calculated O-O stretching frequencies (cm⁻¹) and the Mayer O-O bond orders (MBO). Taken with permission from Figure 6 of Ref 59, copyright © 2019 American Chemical Society.

Starting from a map of the basic catalytic cycle (Figure 6), we consider the changes in Fe-O bonding, and O-O bonding where present over the cycle.⁵⁹ Beginning with the fully reduced State R (HS Fe²⁺ and Cu⁺), when molecular oxygen binds (O₂ triplet, S=1 spin state), the bound state is formally an iron-oxygen adduct (State A), but the electronic structure is closer to that of ferric LS Fe³⁺ bonded to superoxide radical anion O₂^•−. The bonding represents a balance between a partial bond broken in O₂, from loss of part of the O=O π bond, and the energy gained from one electron transfer from Fe²⁺ to O=O, plus the bonding energy from the forming σ-π hybrid to the Fe(3d) shell. The strong ligand field from O₂⁻ binding changes the Fe³⁺ spin state from HS → LS, and this also affects the Fe-O stretch frequency. The O₂ binds in a bent end-on structure, and this description is very much like the bonding in oxymyoglobin (oxy-Mb).^83,84 The calculated Fe-O frequencies in oxy-Mb are similar to those predicted in State A of CcO, and the experimental frequencies are also very similar between the two Fe metalloproteins (~570 cm⁻¹).^{37–44,85–87} The predicted Fe-O frequencies are in both cases less than the experimental frequencies by about 10% (50 cm⁻¹) out of about 570 cm⁻¹. This is the largest deviation in calculations from experiment for all Fe-O bonding species observed throughout the catalytic cycle. We also have excellent predictions for the O-O bond frequency in State A of CcO, but here the experimental data available are for synthetic porphyrin systems.^79,88–91

After formation of State A, one electron transfer from Cu⁺ to Fe³⁺ bound superoxide leads to very fast steps that have not been directly seen either by optical difference spectroscopy or RR spectroscopy. We have calculated in sequence a Peroxo bridging state after 1e⁻ transfer, and then a Hydroperoxo state following protonation. The Hydroperoxo state is probable, and the proton is thought to originate from the protonated Tyr237. For the Peroxo state, it is not evident if the bridging structure is formed before the following proton transfer occurs. In a structurally analogous synthetic Fe³⁺-O₂²⁻-Cu²⁺ complex, the measured O-O stretch frequency (870 cm⁻¹) is close to the one we calculated (906 cm⁻¹, 4% deviation).⁸² However, in the CcO protein, the initial O atom coordination to Cu could be looser, and the 1e⁻ and 1H⁺ transfers may even occur concertedly. The proton position on the oxygen nearer the Cu²⁺ is needed for the next reaction steps. For the rapid cleavage of the O-O σ bond, one electron is transferred from Fe³⁺ to make the ferryl-oxo, Fe⁴⁺=O²⁻, while the other electron can come either from the Tyr237 by through-bond electron transfer to make State P_M, or directly from the mononuclear heme b Fe²⁺ (equivalently from heme a Fe in aa₃) to produce State P_R. (If P_M , the Tyr^• radical state, is generated first, the next electron transfer to make P_R again comes from Fe_b). In State P_R, the bridge has the form of Fe⁴⁺=O²⁻ coordinated by a hydrogen bond to OH⁻-Cu²⁺. After the OH⁻ is protonated, this changes to State F, and the Fe-O stretch frequency decreases by about 20 cm⁻¹ in the experimental RR data from 804 cm⁻¹ to 785 cm⁻¹.^{45,47–52,92} A similar frequency shift is found in the DFT calculations, from 844 cm⁻¹ to 823 cm⁻¹ (5% deviation from experiment for the frequencies).⁵⁹ There is a slight DFT calculated lengthening (+0.01 Å) of the Fe-O bond, but it is probably more important that the Fe⁴⁺=O²⁻⋯H₂O-Cu²⁺ hydrogen bond shortens (from 2.67 Å to 2.52 Å, calculated), and strengthens with H₂O-Cu²⁺ coordination compared to OH⁻-Cu²⁺, consistent with a stronger electrostatic interaction. This shows that the Fe-O stretch frequency can reflect moderate local interactions in addition to the direct Fe-O bond length correlation.

The Fe-O vibrational frequency undergoes a major downshift (to 450 cm⁻¹, experimental)⁵⁰ when a (1e⁻,1H+) addition to the active site (1e⁻ coming from the heme b Fe, and 1H⁺ from the K pathway) produces the State O_H, which is the active oxidized state ready for further cycling. This corresponds to a much longer Fe³⁺-O bond. We calculate a nearly symmetric Fe³⁺-OH⁻-Cu²⁺ geometry, with Fe-O, Cu-O distances of 1.98 Å and 1.99 Å found for HS-Fe³⁺. The bridging OH⁻ group is hydrogen bonded to a water molecule that lies outside the line between Fe-OH⁻-Cu, allowing the near symmetric bridge. With the OLYP-D3-BJ potential, the IS-Fe³⁺ state is calculated lower in energy than HS-Fe³⁺ by 7 kcal/mol, and has a very similar active site geometry. (See Supporting Information Table S1 in Han Du, IC 2020).⁶⁰

In this paper,⁶⁰ we used a larger basis set TZP on all atoms. The geometries are similar to those with the smaller basis set. We very recently recalculated the O_H(Fe-OH⁻-Cu) state vibrational frequencies. The Fe-O frequencies decrease by about 25 to 30 cm⁻¹. The Fe-O stretch frequency is clearer in the HS-Fe³⁺ than in the IS-Fe³⁺ state, where there is more extensive mixing of Fe-O stretching with Fe-O bend modes and Fe-porphyrin modes. In both cases, the calculated frequencies are similar, for HS, Fe-O frequency 423 cm⁻¹, and for IS, we identified a mode with some Fe-O stretch character at 413 cm⁻¹. In earlier experimental work, Rousseau ruled out the LS Fe³⁺-OH⁻ state because he expected a high Fe-O stretch frequency.⁵⁰ Our calculations further support this result, with calculated LS Fe-O distance of 1.88 Å, and a high calculated stretch frequency of 514 cm⁻¹ (14% deviation from exp) for LS, versus (6%) for HS, and (8%) for IS. The LS state is also higher in energy than both the HS and IS states. Also, we wanted to evaluate whether a state of composition Fe^HS,3+-OH⁻⋯H₂O-Cu²⁺ with a bridging hydroxyl-water hydrogen bond, and with the H₂O coordinated to Cu²⁺ is feasible for State O_H , since it has a similar Fe-O bond distance. Several Fe-O-H vibrational modes are obtained in the region 408-437 cm⁻¹, still in good agreement with exp. 450 cm⁻¹. However, the hydroxyl-water bridge state energetically lies well above the corresponding O_H(Fe-OH⁻-Cu) structure, in which the bridging OH⁻ has H-bonding interaction with an outer water molecule (see Ref 60 and Supporting Material). We have paid close attention to State O_H because it is an essential oxidized state for continued cycling, and also because of the contrast with the resting oxidized state, which is the oxidized state structurally characterized by synchrotron or X-ray Free Electron Laser (XFEL) structures.

3.4. The Pathway from P_R → F → O_H

While exploring the reaction pathway from P_R → F → O_H, we found a probable proton pumping pathway using a water shift mechanism.⁵⁸ Figure 12 displays relevant structures before a shift up of a water dimer (13abeled HOH604, HOH608) from a hydrogen bonding position to the OH⁻ (State P_R) or H₂O (State F) ligand on Cu_B²⁺ into the upper water pool adjacent to His376 (neutral or protonated cation). Figure 13 presents a schematic of the entire reaction pathway from P_R → F → O_H including the initiation of the pumping process by proton loss from His376-H⁺. The important features of this detailed mechanism are: (1) proton transfers by H⁺ uptake from the K path onto Tyr237 and from there to the OH⁻-Cu_B²⁺ are needed to allow the water dimer shift to occur; (2) there is then an energetically favorable proton uptake by Tyr237⁻, in the transition c → d; (3) both the H₂O-Cu_B²⁺ and neutral Tyr237 need to be present, and are energetically favored before the water dimer shift occurs with a small energy cost, calculated ΔG = +4.2 kcal mol⁻¹. The calculated pK_a shift of His376⁺ before and after the water dimer shift is large, from 12.2 to 6.5, ΔpK_a = 5.7 equivalent to a relative ΔG = 7.8 kcal mol⁻¹. Following the reaction pathway from d → e → f, after the proton loss from H376⁺, a subsequent proton transfer from Tyr376 (neutral) is favorable. It is important that the Tyr237 (neutral, protonated) does not lose its proton by back leakage into the K pathway after the water shift, because that water shift also lowers the pK_a of Tyr237 strongly, from pK_a = 11.0 to 5.5 when His376 is protonated. A general problem of this type has been considered by other groups. Knapp and coworkers have proposed, based on electrostatics and dynamics modeling, that when the Tyr237 is protonated (Y237-OH), the hydrogen bonded pathway (a Grotthuss type pathway) in the K path is broken so that backflow is inhibited.⁹³ This appears reasonable as it stands, but there is considerably more to learn about the K path proton transfer mechanism both in ba₃ and aa₃ types of CcO.

Figure 12.

In our Model 1 (M1),⁵⁸ the two water molecules HOH604 and HOH608 are within the DNC as observed in the X-ray crystal structure 3S8G.¹⁴ The size of our DNC model clusters are the same as state A shown in Figure 7. A clearer view of the top portion of the cluster (top M1) and the central portions of states P_R and F are given here. In Model 2 (M2), the two water molecules HOH604 and HOH608 are shifted to the upper part of the DNC to the positions as shown on the upper-right (top M2) for protonated His376-H⁺ and lower-right (top M2) for neutral His376 cases.⁵⁸

Figure 13.

Feasible proton uptake/pumping processes connecting with the movement of water molecules in the DNC during the P_R → F transition based on our current Models (M) 1-3 calculations. The 2H₂O represents HOH604 and HOH608. In M1, the two water molecules are within the DNC H-bonded to the OH⁻ or H₂O Cu_B²⁺ ligands close to the positions observed in the X-ray crystal structure 3S8G.¹⁴ In M2, the 2H₂O are shifted to the upper water pool of the DNC. In M3, the water molecule that is a ligand of Cu_B²⁺ in M2, now dissociates from Cu_B²⁺ but still has H-bonding interaction with the ligand O²⁻. Figure is adapted with permission from Figure 4 of Ref 58, copyright © 2018 American Chemical Society.

We have analyzed this water dimer shift mechanism further with additional modeling. We find that if in the state just before the water dimer shift (pre-shift states are called M1 states), we add 2(H₂O) to the upper water pool in our quantum cluster model and calculate the His376⁺ pK_a for that (M1+2H₂O) state, the value is pK_a = 10.7, about 1.5 pH units below the corresponding M1 state discussed earlier, but still 4.2 pH units higher than the corresponding M2 state (after the 2H₂O shift, but with no net added waters). Our conclusion is that the descreening of the H₂O-Cu_B²⁺-(His)₃ ligand group when the water dimer moves to the upper water pool is the primary effect causing a strong change in the His376⁺ pK_a. The Tyr237 (neutral protonated) and the Fe_a3⁴⁺=O²⁻ are also descreened. Primarily, the descreening calculated at His376⁺ is a through space effect, while the effect on the Tyr237 pK_a is a mixture of through bond and through space effects. We have focused on a water dimer shift for two reasons. First, given the initial structures (M1 states), moving a dimer into the upper water pool looked to be less disruptive of the hydrogen bond network. Further, we were intrigued by the possible connection to the expected net H₂O molecule transport, since in each cycle 2(H₂O) is produced, and an effective mechanism for removal of the water product would be to move two waters into the water pool region above the DNC in each cycle. Water exit pathways from the water pool above the DNC, in the region of the shifted water molecules, to the p side of the membrane have been identified by molecular dynamics simulations.⁵⁷ Comparing the (M1+2H₂O) state with the M2 state, one can imagine that the water dimer shifted up only replaces the (2H₂O) already present in (M1+2H₂O), which then is transferred to the bulk water pool above, and produces a net transit of 2(H₂O). We have done a rough calculation of the extra free energy cost for moving 2H₂O from (M1+2H₂O) into bulk water and find that it is small.

3.5. The Resting State O versus the Cycling State O_H.⁶⁰

As depicted in Figure 6, the active cycling State O_H can decay to the relaxed lower lying State O in a few milliseconds (in solution studies with RR) when the next one electron transfer (1e⁻) to the DNC is delayed (or absent entirely). In the associated Resonance Raman spectra, the State O_H signal (whose observation is enhanced by comparing the normal ¹⁶O signal with the isotopic substitution ¹⁸O signal starting from reactant O₂ binding to State R, following through the reaction cycle) is lost on formation of State O. The resting State O is expected to be the same as that found in the resting “as isolated” system as formed in oxidizing conditions. By comparison, State O_H is a metastable catalytically active state. The different characters of State O_H versus State O were initially observed in kinetics studies using a combination of optical difference spectroscopy and electrometry with laser photoactivation over the cycle to follow the 1e⁻ redox transitions O_H + 1e⁻ → E_H compared to O + 1e⁻ → E.^94,95 In the following redox step which regenerates State R, one additional electron is added to the active site, and if needed, a proton may move into the active site vicinity to protonate an OH⁻. The kinetics seen for O_H → E_H is different from that observed for O → E. The first gives more efficient electron transfer, with the electron terminating at Cu_B, and proton transfer is more effective as well for both ba₃ and aa₃ type enzymes. In aa₃ type enzymes, proton pumping occurs just after State O_H, but not after State O.^96–98 Based on these differences in kinetics, some substantial structural differences are expected between O_H and O, but these specific differences are not evident.

There are various X-ray crystal structures of State O (as isolated oxidized species) early on and analyses of the solvent or oxygen species in the DNC based on the observed electron density between Fe_a3 and Cu_B, originally interpreted as a H₂O and an OH⁻ ligand between the metals. These include structures of bacterial aa₃ type CcO’s from Rhodobacter sphaeroides (Rs) and Paracoccus denitrificans (Pd).^27,28 Later, based on higher-resolution X-ray crystal structures using synchrotron radiation of oxidized CcO’s from Pd (PDB code 3HB3, 2.25 Å resolution),²⁹ and from bovine heart mitochondria (PDB code 2ZXW, 1.95 Å resolution),³⁰ two research groups identified an elongated electron density bridging Fe_a3 and Cu_B in the DNC, and proposed that this is a peroxide dianion (O₂²⁻). All of these systems were crystallized from a buffer solution. Following on earlier structures of ba₃ CcO crystallized from cryogenically stabilized solvent,²¹ higher resolution (1.8-1.9 Å) synchrotron X-ray crystal structures (PDB entries 3S8G and 3S8F)¹⁴ of ba₃ CcO from Tt were obtained in lipidic cubic phase (LCP), which is more membrane-like compared to buffered detergent solutions. These also showed a similar elongated electron density. The O1-O2 distances obtained by modeling the structure into the observed electron density maps range from 1.52 Å at the shortest for ba₃ Tt to a range of 1.6 Å − 1.9 Å for other structures in aa₃ CcO enzymes.

A recent low-dose X-ray structure on oxidized resting state CcO from bovine heart mitochondria also showed an apparent peroxide type ligand in the DNC,³¹ and a similar species was seen in an X-ray free-electron laser (XFEL) experiment (1.9 Å resolution).³² While the absorbed power in this XFEL experiment is very high, the diffraction data is collected over the period of the XFEL pulse, which is extremely short, typically between 10 fs and 50 fs, well before the crystal explodes from the longer term radiation damage. The delivered radiation dose is much less than in synchrotron experiments, where the dose is delivered over a much longer time, and the diffraction pattern data is also collected over an extended period. There are ways of mitigating the radiation damage in synchrotron experiments, including using multiple crystals, or irradiating different locations on a crystal. In contrast to synchrotron X-ray diffraction experiments, which are strongly reducing at the metals, because of electron recombination preferentially at those sites, XFELs experiments are strongly oxidizing at the metal sites because after metal ionization, there is little time for the electrons to recombine over the pulse duration.

Despite the conclusions discussed above, there are good reasons to be doubtful about the proposed peroxide ligand between Fe_a3 and Cu_B. In our view, this concern is particularly strong if the peroxide is proposed to be pre-existing prior to X-ray irradiation. A pre-existing peroxide bonded to Fe and Cu does not fit well with the known chemistry of either aa₃ type or ba₃ type CcO. When oxidized CcO is exposed to HOOH in aa₃ CcO proteins, it reaches the DNC, and reacts with the Fe-Cu center, generating the ferryl-oxo, Cu²⁺ tyrosine radical State P_M. By contrast, in ba₃ type CcO, HOOH does not have access to the Fe-Cu site at all. X-ray structures of the as isolated resting oxidized state (State O) showing a non-reactive peroxide or hydroperoxide then are contrary to this reaction chemistry. The active site positioning of the peroxide or hydroperoxide is also surprising. In the lipidic cubic phase structure solved for ba₃ CcO, the apparent Fe-O1 distance is about 2.4 Å and the Cu-O2 distance is about 2.25 Å, both fairly weak. Further, the apparent O-O distance in the LCP ba₃ is 1.5 Å or more; in other structures from aa₃ type enzymes, the observed range is very long 1.6 Å − 1.9 Å; these last distances are not consistent with any known peroxo or hydroperoxo type species, and yet these are much too short for hydrogen bonding between waters or OH⁻⋯H₂O bonds. In our earlier work on this problem,⁵⁴ our group proposed that the peroxide or hydroperoxide (preferably the latter) could be formed by X-ray radiation induced radical reactions near the metals, and further stabilized by the cryogenic temperatures near that of liquid nitrogen. We learned later that X-ray absorption and ionization is enhanced for photon energies near and above the metal K-edge energy, and the X-ray irradiation photon energy typically used is above both the Fe and Cu K edge ionization threshold. Fe and Cu K edge ionization can lead to Auger ionization at the metals, and to various transferred Auger effects producing radicals in bonded or nearby atoms. These effects can be very fast, even on the 10 fs – 50 fs XFEL time scale,⁹⁹ and may be observable, depending on the total radiation flux absorbed. However, the total X-ray radiation absorbed in the recent XFEL experiments is comparatively low, so that only about 10% or less of the Fe and Cu atoms will undergo core M(1s) ionization. While some effects due to X-ray irradiation in the XFEL experiments may be observable with careful attention to the time course, these effects are not likely to be the dominant effects in the observed diffraction pattern, since this pattern represents an average over many billions of DNC Fe-Cu sites in the crystal. Instead, we have explored the possibility that a single water molecule is weakly bonded alternatively to Fe_a3³⁺ and Cu_B²⁺ in the resting oxidized state.⁶⁰ The apparent peroxide molecule is then predicted to be a consequence of a superposition of H₂O positions between Fe and Cu from static and dynamic disorder. We have found that the potential energy surface between the Fe_a3 and Cu_B is very flat and the H₂O to metal bonding is weak. This holds true whether or not this H₂O is hydrogen bonded to another water molecule outside of the direct path between Fe and Cu. Figure 14 presents a superposition of our DFT calculated structures along this path with the observed electron density map derived from the published LCP high resolution (1.8 Å) synchrotron X-ray structure of ba₃ CcO.¹⁴

Figure 14.

The overlap of the electron density map that was reconstructed from the oxidized Tt ba₃ X-ray crystal structure 3S8G¹⁴ data file with our calculated resting O state DNC structures, in which a water molecule resides in different locations between the Fe_a3³⁺ and Cu_B²⁺ sites with very similar energies. Reprinted from Figure 7 of Ref 60, https://pubs.acs.org/doi/10.1021/acs.inorgchem.0c00724, copyright © 2020 American Chemical Society (further permissions for reusing this figure should be directed to the ACS).

Our conclusion here is that the State O_H → State O transition is probably a slow protonation of the bridging OH⁻ in State O_H, resulting in a water (H₂O) weakly coordinated alternatively to Fe_a3 or Cu_B. This apparently disrupts the electron transfer path to Cu_B.

3.6. Features of State O and State R Synchrotron X-ray Structures in Tt ba₃ CcO

Very recently, our group, in collaboration with a group at SSRL completed new high resolution synchrotron X-ray structures of State O and State R in ba₃ CcO from Tt. This work is undergoing final analysis now. We do want to emphasize some features that we have observed in common with earlier structures of ba₃ and found also in aa₃ structures. Confirming previous lower resolution work,²² we find that Fe sites both in heme b and heme a₃ are rapidly X-ray reduced from the original Fe³⁺ to Fe²⁺ based on microspectrophotometer absorption spectra, and these are the heme Fe states in the final X-ray structure. The State O structure is then referred to as State O_(PR), since it is at least partially reduced in the dinuclear complex region. The optical absorption observed at heme a₃ is consistent with having a 6-coordinate Fe²⁺, and we expect that this reflects Fe²⁺-H₂O binding. The Cu_B site does not have an observable optical spectroscopic signal at present, and so we cannot determine its redox state in this X-ray structure. After chemical reduction of the crystal at room temperature over an extended time, and freezing in liquid nitrogen, the fully reduced State R (also called R_(CR) to indicate Chemical Reduction)) exhibits different optical spectra at Fe_a3, consistent with a 5-coordinate Fe²⁺, and the solved X-ray structure shows no waters directly between Fe_a3 and Cu_{B ,} again consistent with the structure determined at lower resolution. This structure of State R has features in common with the chemically reduced forms of bovine mitochondrial aa₃ and of Rhodobacter sphaeroides aa₃ CcO.^100,101

A new water (W1) is observed in State R within close hydrogen bonding distance to Tyr237 compared to State O_(PR). W1 is located about 4 Å from Cu_B and Fe_a3, and similarly about 4.3 Å from the oxygen position in the next states of the reaction cycle. It is also about 4 Å from the Thr302(O) which is H-bonded to His282, a Cu_B ligand. This hydrogen bond positioning indicates two possible input pathways for protons binding to oxygen species or hydroxyl groups in the DNC reaction chamber area between Fe_a3 and Cu_B.

3.7. The Path from State R → State A → Peroxo → Hydroperoxo.

From State R, molecular O₂ binding produces State A. How then are the next States Peroxo and Hydroperoxo formed, and what is the proton pathway in? In recent work by Schaefer et al.¹⁰² and earlier work by Adam et al,⁸² this group proposed that after formation of the Peroxo state, a proton enters via an H-bonded chain from the special tyrosine to a water essentially like W1 discussed above, and this pathway leads to proton transfer to the O1 bonded to Fe_a3³⁺ and then shifting to O2 bonded to Cu_B²⁺ prior to O-O cleavage with the latter proton transfer being rate limiting. Although this pathway looks reasonable, we would like to propose an alternative, which does not require a pre-existing Peroxo bridge state, and uses some distinctive features of Cu_B⁺ coordination chemistry. The Cu⁺ redox state often exhibits lability in ligand binding, and we propose, starting from the State A (Superoxide bound) that His283 (see Figure 15) dissociates from Cu_B⁺ and protonates to His⁺, taking this proton from His282 via a ring flip, leaving His282⁻ as an unstable anion; flipping back, there will be a proton transfer from Thr302, generating Thr302⁻, whose proton is restored by H-bonded waters or amino acid sidechains, going back to Tyr237 at the end of the proton uptake K-pathway. The His283⁺ state, once formed may be further stabilized by a cation-π interaction with the nearby Trp229 ring. Meanwhile, electron transfer from Cu_B⁺ to the superoxide ligand bonded to Fe_a3³⁺ will be quickly followed by proton transfer from His283⁺, and then the Cu_B²⁺ bond to His283 will reform. This mechanism is fairly analogous to one that we found for the reaction center in CuZn superoxide dismutase, which also involves a Cu⁺-His protonation and bond breakage, and then subsequent Cu²⁺-His bond formation after proton loss.^103–107

Figure 15.

Major residues and water molecules in the DNC of the Tt ba₃ X-ray crystal structure 3S8G.¹⁴ For clarity, only prop-A and prop-D of the heme ring are presented here, the whole heme ring is not shown.

3.8. Radical Transfer and Proton Pumping in State P_M

Based on EPR spectra for two different tyrosine radicals that they observed in State P_M, Yu et al.¹⁰⁸ proposed that a radical transfer mechanism in State P_M could be essential to a proton pumping step in the transition P_M → P_R. A similar mechanism could be operating in ba₃ CcO from Tt. (See Figure 15) In Tt ba₃, the relevant tyrosines are Tyr237 and Tyr136, the latter lying in the upper water pool with closely associated polar or charged amino acids capable of proton transfer. The tryptophan (Trp229) lies along a covalently bonded path from Tyr237 and His233 and further on, while the His233 main chain amide is also hydrogen bonded to the Trp229 carbonyl. One electron transfer from Trp229 to the Tyr237 radical will produce a Trp229^•+ cation radical and a Tyr237⁻ anion. There is again an electronic stabilization of His283-Trp229, but now His is the π system and Trp is the cation. The Trp229^•+ radical will exert a strong electrostatic interaction with the Tyr136, causing the loss of its proton, becoming Tyr136⁻, and the proton can then enter the upper pool of waters and polar amino acids. Whether or not there is a radical transfer between Tyr136⁻ and the Trp229^•+ cation radical, there will later be an electron transfer from the heme b Fe²⁺.

To reset the system, there must be a proton resupplied from an effective proton pathway to Tyr136⁻. Here the pathways differ between aa₃ type, involving the D pathway (or perhaps the H pathway in mammalian mitochondria), while we have found a different proton pathway in ba₃ from Tt (see Figures 15, 16 and 17). The resupply pathway includes Asp372, Proprionate A (Prop A), His376 based on prior work.⁵⁷ There are always at least two protons in this network, and sometimes three as we saw in the peroxide cleavage calculations⁵⁶ and our MD simulations.⁵⁷ The proton pumping pathway from His376 to Tyr136 and out along water transport pathways is displayed in Yang et al, BBA, 2016 (see Figures 16 and 17).⁵⁷ Notably, the conformation of Tyr136 is sensitive to the protonation state of His376, either opening or blocking a water exit pathway, potentially acting as conformational gate against proton backflow. The proton exit path(s) are probably similar in the water shift proton pumping mechanism, but these may differ in detail. We see that the description of the proton pumping process requires attention to the entire proton loading network (PLN) and associated pumping network, and not only a proton loading site (PLS).

Figure 16.

Water exit pathways in Tt ba₃ CcO identified from MD simulations.⁵⁷ Tyr136 acts as a conformational gate.

Figure 17.

Water exit pathway P2 obtained from MD simulations.⁵⁷ Left: Detailed water pathway highlighting relevant residues. The pathway connects the water pool above the DNC to the outer side of the membrane via a water pocket (yellow) and two regions (pink, Gap1 and Gap2) that open towards the bulk solvent. Gap 1 is surrounded by residues Arg52^II, Pro129^II, Pro221, Asp220 and Leu553; Gap 2 is surrounded by residues Leu553, Asp220, Ala224, Glu203 and Phe207. Right: Water occupancy averaged over the entire trajectory (isosurface plot at 25% occupancy), showing the path that connects the water pool to the protein exterior. Figure is taken with permission from Figure 8 of Ref 57. https://doi.org/10.1016/j.bbabio.2016.06.005, copyright © 2016 Elsevier.

3.9. Limitations in Current DFT Calculations

Our work and that from other groups have used a variety of standard DFT methods and exchange-correlation potentials. For our work, recent studies have used OLYP plus dispersion corrections,^58–60 while in earlier papers,^24,34 we tested PW91, B3LYP, B3LYP*, OPBE, OLYP for oxygen thermochemistry, and PW91 and B3LYP* for redox potentials for Fe^3+,2+ and Cu^2+,1+ of Fe_a3 and Cu_B.

For the O₂ thermochemistry, we evaluated the overall gas phase reaction

$${\text{O}}_2+2{\text{H}}_2\to 2{\text{H}}_2\text{O}$$ (6)

This Equation is the gas phase analogue of Eq.4. In our early work (see Table 3 of Ref 34), we found that there is a substantial deviation from experiment for the calculated ΔG for all these different DFT potentials, including OLYP in our 2014 paper.²⁴ Effectively the O₂ binding is too strong so that the deviation in ΔG (Calc.-Exp) ranges from 11.0 to 18.2 kcal mol⁻¹, compared to the experimental ΔG of reaction equal to −109.3 kcal mol⁻¹. The potentials in order of increasing deviation are (PW91, B3LYP, B3LYP*, OPBE, OLYP). Meanwhile, breaking down the equation above into two steps, we have

$${\text{O}}_2+{\text{H}}_2\to {\text{H}}_2{\text{O}}_2$$ (7)

$${\text{H}}_2{\text{O}}_2+{\text{H}}_2\to 2{\text{H}}_2\text{O}$$ (8)

We find that the OPBE error lies mainly in the π bond breaking, and OLYP should be similar, while the corresponding errors for PW91, B3LYP, B3LYP* are mainly in the following σ bond breaking. Clearly, these errors will affect the relative energies of different intermediates over the reaction cycle. In some steps, these errors are partly compensated by errors in the Fe_a3^3+,2+ and Cu_B^2+,1+ redox potentials. In our 2014 paper,²⁴ we made a rough estimate of the average redox potential error for Fe_a3 and Cu_B compared to what is known from experiment, finding the calculated redox potentials for B3LYP* to be too negative by about −0.3 V, which is equivalent to a ΔG (1e⁻ reduction) error of +7 kcal mol⁻¹. The errors in OPBE and OLYP for these redox steps are evidently of similar magnitude and direction.²⁴ In forming State A from State R by binding O₂ , the error in oxidizing Fe_a3²⁺ and reducing O₂ to superoxide O₂^•− radical ion may partially cancel, but the reaction cycle has several states with large changes in electronic structure. For the corresponding reaction cycle for aa₃ type CcO using B3LYP* as the exchange-correlation potential, Blomberg¹⁰⁹ has used a similar redox correction of 9 kcal mol⁻¹ for HS heme-Fe^3+,2+ redox and other empirical corrections for O₂ binding and other reaction steps. What is really needed are more accurate DFT potentials for use on the entire family of heme-copper oxidases and even more broadly throughout metallobiochemistry.

4. Concluding Remarks

In this work, we have followed the catalytic reaction cycle of the dinuclear complex in CcO with particular focus on the ba₃ enzyme in Thermus thermophilus. Comparisons of proposed reaction pathways, including DFT calculated geometries, redox and protonation states, energies, and spectroscopic properties can be closely related to experimental X-ray structural and spectroscopic observations, clarifying the physical properties of various intermediates. Calculations of specific vibrational modes over the catalytic cycle in comparison with resonance Raman spectra have proven particularly valuable.⁵⁹ We have developed some insights on proton transfers both into the reaction center Fe_a3-Cu_B active site and into the potential pathways for proton pumping. In ba₃ CcO, protons are delivered from the K pathway to the special Tyr237, and potentially on to Thr302, as we have proposed.^24,34 At that point, the proton may move through an outer pathway to Asp372 and then to His376 or farther. Alternatively, it may reprotonate His282 which earlier transferred a proton to His283 in some states, in preparation for protonating intermediates within the reaction chamber. We have presented this proposal in some detail for the State A → Hydroperoxo transition, where the Cu_B starts in the Cu⁺ cuprous state, emphasizing the lability of Cu⁺ -histidine bonding.⁵⁵ While this is perhaps the clearest and most likely example of a labile Cu_B coordination, there are a number of other states of the catalytic cycle that are formally Cu²⁺-Tyr⁻.

When we look at these states with spin density population analysis, we see that all of these states have significant spin density on both Cu_B and Tyr237.^59,60 This spin distribution is indicative of a quantum admixed state involving a resonance between Cu²⁺-Tyr⁻ (anion) and Cu⁺-Tyr^• (radical). If the lower electronic ground state is mainly Cu²⁺-Tyr⁻ (anion), then the activated intermediate state is mainly Cu⁺-Tyr^• (radical), and the main question becomes how high in energy this latter state lies for specific intermediates and transitions in the reaction pathway, and to what extent each promotes proton transfer into the reaction chamber. There remains a great deal more work to be done involving reaction energetics, pathways and dynamics in ba₃ CcO and the connections and contrasts with pathways in aa₃ from mitochondria and aerobic bacteria.