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Boosting the performance of reversible solid oxide electrochemical cells with a novel hybrid oxygen electrode, Pr 1.39 Ba 0.14 Sr 0.53 Co 1.48 Fe 0.76 O 6- δ -Ba 0.66 Sr 0.34 CoO 3- δ

Solid oxide electrochemical cells (SOECs) stand out as a highly promising clean energy technology that offers several benefits, showing significant potential to play a pivotal role in the transition towards a sustainable and low-carbon energy future. SOECs can efficiently convert the chemical energy stored in fuels to electricity in fuel cell mode, and produce various chemicals from abundant feedstocks (e.g., CO 2 , H 2 O) and intermittent solar/wind-based renewable electricity. Despite extensive efforts that have been devoted to designing novel materials and optimizing SOEC manufacturing processes, aiming to achieve enhanced energy efficiency, the current SOECs still suffer from poor performance, which is mainly due to the sluggish oxygen reduction reaction (ORR) and oxygen evolution reaction (OER) kinetics. To address this challenge, in this work, we have successfully designed an in situ formed hybrid oxygen electrode material (Pr 1.39 Ba 0.14 Sr 0.53 Co 1.48 Fe 0.76 O 6- δ -Ba 0.66 Sr 0.34 CoO 3- δ ), which significantly improves the surface oxygen exchange coefficient and bulk oxygen-ion diffusion coefficient, enhancing the OER and ORR electrocatalytic activities. Further, the SOECs equipped with this newly developed oxygen electrode achieved exceptional performance for power generation using both hydrogen and propane as the fuels. At 750 °C, a peak power density of 2.4 W cm -2 was obtained with H 2 as the fuel. Additionally, the SOECs attain unprecedented performance in steam electrolysis mode. A current density of 4.4 A cm -2 was achieved at 1.3 V and 750 °C, which represents the highest performance among all yttria-stabilized zirconia (YSZ) electrolyte-based SOECs. The SOECs also deliver remarkable stability during the accelerated stability testing, highlighting the great potential of Pr 1.39 Ba 0.14 Sr 0.53 Co 1.48 Fe 0.76 O 6- δ -Ba 0.66 Sr 0.34 CoO 3- δ as a high-performance oxygen electrode for next generation SOECs.

08 HYDROGEN↗

Reduction of CO 2 and CS 2 with Uranium(III) Metallocene Aryloxides

Herein, the reactivity of two metallocene aryloxide U(III) complexes, [(C 5 Me 5 ) 2 U(O-Ar)], Ar = 4- t BuC 6 H 4 , 1; Ar = 2,6- t Bu 2 -4-CH 3 C 6 H 2 (BHT), 3, with CO 2 and CS 2 has been investigated. The reaction of 1 with CO 2 produces a bridging oxo complex, [{(C 5 Me 5 ) 2 (4- t BuC 6 H 4 -O)U} 2 (μ 2 -O)], 4, while 3 with CO 2 results in reductive disproportionation to form the bridging carbonate species, [{(C 5 Me 5 ) 2 (BHT)U} 2 (μ 2 -κ 2 :η 1 -CO 3 )], 5. The difference in reactivity can be attributed to the steric properties of the ligand because the reaction of 3 with an oxo-delivering agent yields a U(V) terminal oxo complex, [(C 5 Me 5 ) 2 (BHT)U=O], 6. Reduction of CS 2 to form a bridging (CS 2 ) 2- ligand, [{(C 5 Me 5 ) 2 (tBuC 6 H 4 -O)U}2(μ 2 -CS 2 )], 7, is observed with 1, while the reaction of 3 with CS 2 also produces a bridging (CS 2 ) 2- reduced ligand complex, followed by C-H bond activation of a methyl group from one (C5Me 5 ) 1- ring, [(C5Me 5 ) 2 (BHT)U{μ 2 -C(H)S 2 }U(C 5 Me 4 CH 2 )(C 5 Me 5 )(BHT)], 8. All compounds are characterized by NMR and IR spectroscopy, and their solid-state structures are determined by X-ray crystallography.

37 INORGANIC, ORGANIC, PHYSICAL, AND ANALYTICAL CH↗

Decoupling first-cycle capacity loss mechanisms in sulfide solid-state batteries

Solid-state batteries (SSBs) promise more energy-dense storage than liquid electrolyte lithium-ion batteries (LIBs). However, first-cycle capacity loss is higher in SSBs than in LIBs due to interfacial reactions. The chemical evolution of key interfaces in SSBs has been extensively characterized. Electrochemically, however, we lack a versatile strategy for quantifying the reversibility of solid electrolyte (SE) redox for established and next-generation SSB electrolytes. In this work, we perform tailored electrochemical tests and operando X-ray diffraction to disentangle reversible and irreversible sources of capacity loss in positive electrodes composed of Li 6 PS 5 Cl SE, Li(Ni 0.5 Mn 0.3 Co 0.2 )O 2 (NMC), and carbon conductive additives. We leverage an atypically low voltage cutoff (2.0 V vs. Li/Li + ) to quantify the reversibility of SE redox. Using slow (5.5 mA g NMC −1 ) cycling paired with >100 h low-voltage holds, our cells achieve a surprising 96.2% first-cycle coulombic efficiency, which is higher than previously reported (mean: 72%, maximum: 91.6% across surveyed literature). We clarify that sluggish NMC relithiation kinetics have been historically mistaken for permanently irreversible capacity loss. In conclusion, through systematic decoupling of loss mechanisms, we uncover the unexpected reversibility of SE redox and isolate the major contributors to capacity loss, outlining a strategy for accurate assessment of next-generation SE materials and interface modifications.

54 ENVIRONMENTAL SCIENCES↗

IUE Observations of the Gaseous Component of the Local Interstellar Medium

Discovery of interstellar Ge, Ga, and Kr is reported. Several intercombination lines of Fe 2 are detected. The depletion is most pronounced in Ca, Ti, and V. The highly ionized gas C 4 and Si 4 is not co-extensive with the Si 2 and C 2 gas nor with the O 6 gas. The molecular gas (CO) shows very small velocity dispersion (b approximately 1 km/sec). HD 149404 has the richest interstellar spectrum (except molecules) of all the stars in this study. HD 147889, the heavily obscured star in the Rho Oph cloud, has the strongest interstellar CO spectrum. Noisy nature of the spectra precludes detection of other molecules.

Gilra, D. P.↗

Siderophile Element Constraints on the Conditions of Core Formation in Mars

Siderophile element concentrations in planetary basalts and mantle samples have been used to estimate conditions of core formation for many years and have included applications to Earth, Moon, Mars and asteroid 4 Vesta [1]. For Earth, we have samples of mantle and a diverse collection of mantle melts which have provided a mature understanding of the how to reconstruct the concentration of siderophile elements in mantle materials, from only concentrations in surficial basalt (e.g., [2]). This approach has led to the consensus views that Earth underwent an early magma ocean stage to pressures of 40-50 GPa (e.g., [3,4]), Moon melted extensively and formed a small (approx. 2 mass %) metallic core [5], and 4 Vesta contains a metallic core that is approximately 18 mass % [6,7]. Based on new data from newly found meteorites, robotic spacecraft, and experimental partitioning studies, [8] showed that eight siderophile elements (Ni, Co, Mo, W, Ga, P, V and Cr) are consistent with equilibration of a 20 mass% S-rich metallic core with the mantle at pressures of 14 +/- 3 GPa. We aim to test this rather simple scenario with additional analyses of meteorites for a wide range of siderophile elements, and application of new experimental data for the volatile siderophile and highly siderophile elements.

Righter, K.↗

Heterointercalation in Chevrel-Phase Sulfides: A Model Periodic Solid for the Investigation of Chain Electron Transfer

Modulation of electron density localization on periodic crystal solids through electron transfer from interstitial cations can directly influence the bonding configurations of small-molecule intermediates at the catalyst binding site. This study presents the microwave-assisted solid-state synthesis of four heterointercalant Chevrel-phase (CP) sulfides with varying metal cation intercalants with compositional and electronic structure investigations of the electron density redistribution as a result of intercalation. The heterointercalant CP sulfides, with the general formula Cu x M y Mo 6 S 8 (where M = Cr, Mn, Fe, Ni; x, y = 1.5−2.5), are presented here for the probe reaction of electrochemical CO 2 reduction. A change in product selectivity is observed toward the production of methanol at low overpotentials of −0.5 V vs reversible hydrogen electrode (RHE), as a result of the intercalant combination present within the CP interstitial cavity. Structural confirmation of all materials was examined through Rietveld refinement of the powder X-ray diffraction (PXRD) data, high-resolution transmission electron microscopy (HR-TEM), and selected-area electron diffraction (SAED). Electron transfer from the intercalated metal cations to the Mo 6 S 8 cluster was investigated via X-ray photoelectron spectroscopy (XPS) of the intercalated metal cations and the chalcogenide cluster. Electron transfer was further confirmed through X-ray absorption analysis (XAS) of the K-edges of Mo and intercalants. Intermediate studies of electrochemical reduction of formaldehyde to methanol resulted in a faradaic efficiency of ∼78% methanol production on Cu x Ni y Mo 6 S 8 . The results presented herein identify distinct principles for materials design that can be utilized in other compositional spaces within the broad families of periodic crystal solids.

37 INORGANIC, ORGANIC, PHYSICAL, AND ANALYTICAL CH↗

HCOOH Decomposition on Sub-Nanometer Pd 6 Cluster Catalysts: The Effect of Defective Boron Nitride Supports Through First Principles

The catalytic properties of a hexagonal boron nitride- (h-BN) supported Pd 6 sub-nanometer cluster in the context of formic acid (HCOOH) decomposition were studied by means of periodic Density Functional Theory (DFT) calculations. The effect of support defectivity – boron (h-B v N) and nitrogen (h-BN v ) monovacancies – on the competition between the formate (HCOO)- and carboxyl (COOH)-mediated decomposition pathways was analyzed. Defects are responsible for charge-transfer leading to a positively or negatively charged cluster, and open new reactive channels in which vacancy-mediated dehydrogenation pathways can occur. Pd 6 cluster reconstructions, induced by the adsorption of reaction intermediates and by the presence of monovacancies in the support, greatly stabilize the formation of CO from COOH, which could drastically decrease the selectivity towards hydrogen production. Here, a simplified descriptor-based analysis, based on selected thermochemical quantities calculated on charged cluster models, suggests that Pd 6 sub-nanometer clusters supported on pristine h-BN and h-BN v can be more selective than Pd 6 supported on defective h-B v N towards HCOOH dehydrogenation.

37 INORGANIC, ORGANIC, PHYSICAL, AND ANALYTICAL CH↗

High-throughput characterization of Ag–V–O nanostructured thin-film materials libraries for photoelectrochemical solar water splitting

Ag–V–O thin-film materials libraries, with both composition (Ag 22-77 V 23-78 O x ) and thickness (123–714 nm) gradients were fabricated using combinatorial reactive magnetron co-sputtering aiming on establishing relations between composition, structure, and functional properties. As-deposited libraries were annealed in air at 300 °C for 10 h. High-throughput characterization methods of composition, structure and functional properties were used to identify photoelectrochemically active regions. The phases AgV 6 O 15 , Ag 2 V 4 O 11 , AgVO 3 , and Ag 4 V 2 O 7 were observed throughout the composition gradient. The photoelectrochemical properties of Ag–V–O films are dependent on composition and morphology. An enhanced photocurrent density (~300–554 μA/cm 2 ) was obtained at 30 to 45 at.% Ag along the thickness gradient. Thin films of these compositions show a nanowire morphology, which is an important factor for the enhancement of photoelectrochemical performance. The photoelectrochemically active regions were further investigated by high-throughput synchrotron-X-ray diffraction and transmission electron microscopy (Ag 32 V 68 O x ) which confirmed the presence of Ag 2 V 4 O 11 as the dominating phase along with the minor phases AgV 6 O 15 and AgVO 3 . This enhanced photoactive region shows bandgap values of ~2.30 eV for the direct and ~1.87 eV for the indirect bandgap energies. Finally, the porous nanostructured films improve charge transport and are hence of interest for photoelectrochemical water splitting.

36 MATERIALS SCIENCE↗

One-electron redox kinetics of aqueous transition metal couples Zn 2+/+ , Co 2+/+ , and Ni 2+/+ using pulse radiolysis

The one-electron redox potentials for aqueous metal couples Co 2+/+ and Ni 2+/+ have been investigated by using pulse radiolysis using their reactions with a series of reference compounds to establish the most positive upper limits of E 0 . Experiments with Zn + were also carried out to confirm the characteristic shape of the expected reduction kinetics. Both formate ions and t-BuOH were employed to scavenge ˙OH radicals and ˙H atoms. Kinetics and fitted first and second order reaction rates have been reported for reactions with methyl viologen, fluorescein, Ru(NH 3 ) 6 3+ , Co(en) 3 2+ , Co(sepulcrate) 3+ , Ru(bpy) 3 2+ , Cr(bpy)33+, and Ni(Me 6 [14]4,11-dieneN4) 2+ . Previous work demonstrated that both Co 2+ and Ni 2+ can be reduced by CO 2 ˙- radicals, giving a negative E 0 limit of -1.9 V vs. SHE. A definite reaction of Ni + with fluorescein di-anions provides a new upper limit of the Ni 2+/+ couple as -0.906 V vs. SHE. The reaction of Co + with Ru(bpy) 3 2+ has been confirmed, giving E 0 = -1.3 V vs. SHE as a rigorous upper limit of the Co 2+/+ couple. In the case of Co 2+/+ , kinetics were complicated by a self-catalyzed metal clustering phenomenon. Initiation rate constants of this process have also been reported.

37 INORGANIC, ORGANIC, PHYSICAL, AND ANALYTICAL CH↗

13 C ENDOR Characterization of the Central Carbon within the Nitrogenase Catalytic Cofactor Indicates That the CFe 6 Core Is a Stabilizing “Heart of Steel”

Substrates and inhibitors of Mo-dependent nitrogenase bind and react at Fe ions of the active-site FeMo-cofactor [7Fe–9S–C–Mo–homocitrate] contained within the MoFe protein α-subunit. The cofactor contains a CFe 6 core, a carbon centered within a trigonal prism of six Fe, whose role in catalysis is unknown. Targeted 13 C labeling of the carbon enables electron-nuclear double resonance (ENDOR) spectroscopy to sensitively monitor the electronic properties of the Fe–C bonds and the spin-coupling scheme adopted by the FeMo-cofactor metal ions. Here this report compares 13 CFe 6 ENDOR measurements for (i) the wild-type protein resting state (E 0 ; α-Val 70 ) to those of (ii) α-Ile 70 , (iii) α-Ala 70 -substituted proteins; (iv) crystallographically characterized CO-inhibited “hi-CO” state; (v) E 4 (4H) Janus intermediate, activated for N 2 binding/reduction by accumulation of 4[ e– /H + ]; (vi) E 4 (2H)* state containing a doubly reduced FeMo-cofactor without Fe-bound substrates; and (vii) propargyl alcohol reduction intermediate having allyl alcohol bound as a ferracycle to FeMo-cofactor Fe6. All states examined, both S = 1/2 and 3/2 exhibited near-zero 13 C isotropic hyperfine coupling constants, $^Ca$ = [-1.3 ↔ +2.7] MHz. Density functional theory computations and natural bond orbital analysis of the Fe-C bonds show that this occurs because a (3 spin-up/3 spin-down) spin-exchange configuration of CFe 6 Fe-ion spins produces cancellation of large spin-transfers to carbon in each Fe–C bond. Previous X-ray diffraction and DFT both indicate that trigonal-prismatic geometry around carbon is maintained with high precision in all these states. The persistent structure and Fe–C bonding of the CFe 6 core indicate that it does not provide a functionally dynamic (hemilabile) “beating heart”-instead it acts as “a heart of steel”, stabilizing the structure of the FeMo-cofactor-active site during nitrogenase catalysis.

37 INORGANIC, ORGANIC, PHYSICAL, AND ANALYTICAL CH↗

Synthesis,and structural characterization of [(CH3(C5H4N))Ga(SCH2(CO)O)]-[(4-MepyH)]+, a novel Ga(III) five coordinate complex.

The synthesis and structural characterization of a novel ionic Ga(III) five coordinate complex [{CH3(C5H4N)}Ga(SCH2(CO)O)2]-[(4-MepyH)]+, (4-Mepy = CH3(C5H5N)) from the reaction between Ga2Cl4 with sodium mercapto-acetic acid in 4-methylpyridine is described. Under basic reaction conditions the mercapto ligand is found to behave as a 2e- bidentate ligand. Single crystal X-ray diffraction studies show the complex to have a distorted square pyramidal geometry with the [(-SCH2(CO)CO-)] ligands in a trans conformation. The compound crystallizes in the P2(sub 1)/c (No. 14) space group with a = 7.7413(6) A, b = 16.744(2) A, c = 14.459(2) A, V = 1987.1(6) A(sup 3), R(F) = 0.032 and R(sub w) = 0.038.

Banger, Kulbinder K.↗

Performance of a Novel In-Situ Converted Additive for High Voltage Li-ion Pouch Cells

In search for new classes of additives for high voltage NMC/graphite lithium-ion cells, the precursor additive bis(trimethylsilyl) malonate (bTMSM) is shown to be activated via a spontaneous reaction with LiPF 6 and LiBF 4 salts in carbonate-based electrolyte to form lithium tetrafluoro(malonato)phosphate (LiTFMP), and lithium difluoro(malonato)borate (LiDFMB), respectively. The reaction schemes and rates were studied via NMR spectroscopy and GCMS. The effects of LiTFMP and LiDFMB on high voltage electrochemical performance were then examined up to 4.5 V in Li[Ni 0.4 Mn 0.4 Co 0.16 ]O 2 (NMC442)/graphite and Li[Ni 0.6 Mn 0.4 Co 0.0 ]O 2 (NMC/640)/graphite pouch cells using aggressive voltage-hold cycling, long-term charge/discharge cycling, storage experiments, electrochemical impedance spectroscopy, and gas evolution measurements. While in situ converted additives suffer from gassing issues due to the presence of trimethylfluorosilane (TMSF) gas, a side product of the in situ reaction of bTMSM with LiPF 6 , the cycling and storage capability for the activated additives under study shows competitive performance and controlled impedance when compared to other well-known high voltage additives. Micro X-ray fluorescence spectroscopy (μXRF) confirmed that LiTFMP successfully minimizes the rate of transition metal deposition on the surface of graphite apparently by forming a protective agent at the cathode surface, hence allowing for improved cycling performance at high voltages.

25 ENERGY STORAGE↗

Understanding of A-site deficiency in layered perovskites: promotion of dual reaction kinetics for water oxidation and oxygen reduction in protonic ceramic electrochemical cells

Protonic ceramic electrochemical cells (PCECs) are promising solid-state energy conversion devices which enable the conversion of energy between electricity and hydrogen at intermediate temperatures. Rapid conversion between chemical and electrical energy via PCEC technology will assist in overcoming grand challenges in energy storage. To achieve highly efficient reversible operation between hydrogen production and electricity generation, boosting water-oxidation and oxygen reduction activities of the oxygen electrode while maintaining the durable operation is one of the early-stage technical opportunities. In this study, an A-site deficient layered perovskite (PrBa 0.8 Ca 0.2 ) 0.95 Co 2 O 6–δ has been developed as an oxygen electrode for a PCEC which presents superior electrochemical performances. The electrolysis current density reached as high as –0.72 A cm –2 at 1.3 V, and a peak power density of 0.540 W cm –2 was obtained at 600 °C in electrolysis and fuel cell mode, respectively. The PCEC with the new electrode shows good durability under practical operating conditions for 160 hours in both operating modes with no observable degradation. Here, the reversibility between the electrolysis and fuel cell mode is also successfully demonstrated.

30 DIRECT ENERGY CONVERSION↗

Materials Data on Li3V6O13 by Materials Project

Li3V6O13 crystallizes in the triclinic P1 space group. The structure is three-dimensional. there are three inequivalent Li1+ sites. In the first Li1+ site, Li1+ is bonded to five O2- atoms to form LiO5 square pyramids that share a cornercorner with one VO6 octahedra, corners with two equivalent LiO5 square pyramids, edges with four VO6 octahedra, and an edgeedge with one LiO5 square pyramid. The corner-sharing octahedral tilt angles are 8°. There are a spread of Li–O bond distances ranging from 1.99–2.14 Å. In the second Li1+ site, Li1+ is bonded to five O2- atoms to form LiO5 square pyramids that share a cornercorner with one VO6 octahedra, corners with two equivalent LiO5 square pyramids, edges with four VO6 octahedra, and an edgeedge with one LiO5 square pyramid. The corner-sharing octahedral tilt angles are 8°. There are a spread of Li–O bond distances ranging from 1.99–2.15 Å. In the third Li1+ site, Li1+ is bonded in a square co-planar geometry to four O2- atoms. There are a spread of Li–O bond distances ranging from 2.01–2.21 Å. There are six inequivalent V+3.83+ sites. In the first V+3.83+ site, V+3.83+ is bonded to six O2- atoms to form a mixture of corner and edge-sharing VO6 octahedra. The corner-sharing octahedra tilt angles range from 0–15°. There are a spread of V–O bond distances ranging from 1.97–2.03 Å. In the second V+3.83+ site, V+3.83+ is bonded to six O2- atoms to form a mixture of corner and edge-sharing VO6 octahedra. The corner-sharing octahedra tilt angles range from 0–11°. There are a spread of V–O bond distances ranging from 1.84–2.04 Å. In the third V+3.83+ site, V+3.83+ is bonded to six O2- atoms to form distorted VO6 octahedra that share corners with three VO6 octahedra, a cornercorner with one LiO5 square pyramid, an edgeedge with one VO6 octahedra, and edges with four LiO5 square pyramids. The corner-sharing octahedra tilt angles range from 8–18°. There are a spread of V–O bond distances ranging from 1.71–2.18 Å. In the fourth V+3.83+ site, V+3.83+ is bonded to six O2- atoms to form distorted VO6 octahedra that share corners with three VO6 octahedra, a cornercorner with one LiO5 square pyramid, an edgeedge with one VO6 octahedra, and edges with four LiO5 square pyramids. The corner-sharing octahedra tilt angles range from 4–18°. There are a spread of V–O bond distances ranging from 1.70–2.17 Å. In the fifth V+3.83+ site, V+3.83+ is bonded in a 6-coordinate geometry to six O2- atoms. There are a spread of V–O bond distances ranging from 1.68–2.35 Å. In the sixth V+3.83+ site, V+3.83+ is bonded in a 6-coordinate geometry to six O2- atoms. There are a spread of V–O bond distances ranging from 1.69–2.36 Å. There are thirteen inequivalent O2- sites. In the first O2- site, O2- is bonded in a square co-planar geometry to one Li1+ and three V+3.83+ atoms. In the second O2- site, O2- is bonded in a square co-planar geometry to one Li1+ and three V+3.83+ atoms. In the third O2- site, O2- is bonded to two Li1+ and three V+3.83+ atoms to form OLi2V3 square pyramids that share corners with two equivalent OLi2V3 square pyramids, corners with two OLiV4 trigonal bipyramids, an edgeedge with one OLi2V3 square pyramid, and edges with seven OLiV4 trigonal bipyramids. In the fourth O2- site, O2- is bonded to two Li1+ and three V+3.83+ atoms to form OLi2V3 square pyramids that share corners with two equivalent OLi2V3 square pyramids, corners with two OLiV4 trigonal bipyramids, an edgeedge with one OLi2V3 square pyramid, and edges with seven OLiV4 trigonal bipyramids. In the fifth O2- site, O2- is bonded to one Li1+ and four V+3.83+ atoms to form distorted OLiV4 trigonal bipyramids that share a cornercorner with one OLi2V3 square pyramid, corners with three OLiV4 trigonal bipyramids, edges with three OLi2V3 square pyramids, and edges with five OLiV4 trigonal bipyramids. In the sixth O2- site, O2- is bonded to one Li1+ and four V+3.83+ atoms to form distorted OLiV4 trigonal bipyramids that share a cornercorner with one OLi2V3 square pyramid, corners with three OLiV4 trigonal bipyramids, edges with three OLi2V3 square pyramids, and edges with five OLiV4 trigonal bipyramids. In the seventh O2- site, O2- is bonded in a square co-planar geometry to two equivalent Li1+ and two V+3.83+ atoms. In the eighth O2- site, O2- is bonded in a linear geometry to two V+3.83+ atoms. In the ninth O2- site, O2- is bonded in a linear geometry to two V+3.83+ atoms. In the tenth O2- site, O2- is bonded in a linear geometry to two V+3.83+ atoms. In the eleventh O2- site, O2- is bonded in a linear geometry to two V+3.83+ atoms. In the twelfth O2- site, O2- is bonded to two equivalent Li1+ and three V+3.83+ atoms to form OLi2V3 trigonal bipyramids that share a cornercorner with one OLi2V3 square pyramid, corners with three OLiV4 trigonal bipyramids, edges with four OLi2V3 square pyramids, and edges with four OLiV4 trigonal bipyramids. In the thirteenth O2- site, O2- is bonded to two equivalent Li1+ and three V+3.83+ atoms to form OLi2V3 trigonal bipyramids that share a cornercorner with one OLi2V3 square pyramid, corners with three OLiV4 trigonal bipyramids, edges with four OLi2V3 square pyramids, and edges with four OLiV4 trigonal bipyramids.

36 MATERIALS SCIENCE↗

Materials Data on V5CoO23 by Materials Project

(V5O14)2(CoO6)2(O2)3 crystallizes in the triclinic P-1 space group. The structure is zero-dimensional and consists of two cobalt;hexahydrate molecules, two trioxidane molecules, and one V5O14 cluster. In the V5O14 cluster, there are five inequivalent V sites. In the first V site, V is bonded in a 5-coordinate geometry to six O atoms. There are a spread of V–O bond distances ranging from 1.61–2.52 Å. In the second V site, V is bonded in a 5-coordinate geometry to six O atoms. There are a spread of V–O bond distances ranging from 1.61–2.52 Å. In the third V site, V is bonded in a 6-coordinate geometry to six O atoms. There are a spread of V–O bond distances ranging from 1.68–2.27 Å. In the fourth V site, V is bonded in a 6-coordinate geometry to six O atoms. There are a spread of V–O bond distances ranging from 1.72–2.09 Å. In the fifth V site, V is bonded in a 5-coordinate geometry to six O atoms. There are a spread of V–O bond distances ranging from 1.63–2.49 Å. There are fourteen inequivalent O sites. In the first O site, O is bonded in a trigonal non-coplanar geometry to three V atoms. In the second O site, O is bonded in a single-bond geometry to one V atom. In the third O site, O is bonded in a bent 120 degrees geometry to two V atoms. In the fourth O site, O is bonded in a trigonal non-coplanar geometry to three V atoms. In the fifth O site, O is bonded in a single-bond geometry to one V atom. In the sixth O site, O is bonded in a bent 120 degrees geometry to two V atoms. In the seventh O site, O is bonded in a bent 120 degrees geometry to two V atoms. In the eighth O site, O is bonded in a single-bond geometry to one V atom. In the ninth O site, O is bonded in a bent 120 degrees geometry to two V atoms. In the tenth O site, O is bonded in a bent 120 degrees geometry to two V atoms. In the eleventh O site, O is bonded in a single-bond geometry to one V atom. In the twelfth O site, O is bonded in a bent 120 degrees geometry to two V atoms. In the thirteenth O site, O is bonded in a 6-coordinate geometry to six V atoms. In the fourteenth O site, O is bonded in a bent 120 degrees geometry to two V atoms.

36 MATERIALS SCIENCE↗

Materials Data on V2ZnCoO7 by Materials Project

ZnCoV2O7 crystallizes in the monoclinic P2_1/c space group. The structure is three-dimensional. there are four inequivalent V5+ sites. In the first V5+ site, V5+ is bonded to four O2- atoms to form VO4 tetrahedra that share a cornercorner with one CoO5 trigonal bipyramid and corners with two equivalent ZnO5 trigonal bipyramids. There are a spread of V–O bond distances ranging from 1.68–1.79 Å. In the second V5+ site, V5+ is bonded to five O2- atoms to form distorted VO5 trigonal bipyramids that share a cornercorner with one VO4 tetrahedra, corners with two equivalent ZnO5 trigonal bipyramids, and an edgeedge with one VO4 tetrahedra. There are a spread of V–O bond distances ranging from 1.71–2.01 Å. In the third V5+ site, V5+ is bonded to four O2- atoms to form distorted VO4 tetrahedra that share corners with two equivalent CoO5 trigonal bipyramids and an edgeedge with one VO5 trigonal bipyramid. There are a spread of V–O bond distances ranging from 1.71–1.81 Å. In the fourth V5+ site, V5+ is bonded to four O2- atoms to form VO4 tetrahedra that share a cornercorner with one VO5 trigonal bipyramid, a cornercorner with one ZnO5 trigonal bipyramid, and corners with two equivalent CoO5 trigonal bipyramids. There are a spread of V–O bond distances ranging from 1.72–1.77 Å. There are two inequivalent Co2+ sites. In the first Co2+ site, Co2+ is bonded in a 6-coordinate geometry to six O2- atoms. There are a spread of Co–O bond distances ranging from 2.00–2.72 Å. In the second Co2+ site, Co2+ is bonded to five O2- atoms to form distorted CoO5 trigonal bipyramids that share corners with five VO4 tetrahedra and an edgeedge with one ZnO5 trigonal bipyramid. There are a spread of Co–O bond distances ranging from 1.98–2.11 Å. There are two inequivalent Zn2+ sites. In the first Zn2+ site, Zn2+ is bonded to five O2- atoms to form distorted ZnO5 trigonal bipyramids that share corners with three VO4 tetrahedra, corners with two equivalent VO5 trigonal bipyramids, and an edgeedge with one CoO5 trigonal bipyramid. There are a spread of Zn–O bond distances ranging from 2.04–2.47 Å. In the second Zn2+ site, Zn2+ is bonded in a 6-coordinate geometry to six O2- atoms. There are a spread of Zn–O bond distances ranging from 2.06–2.46 Å. There are fourteen inequivalent O2- sites. In the first O2- site, O2- is bonded in a bent 150 degrees geometry to one V5+ and one Zn2+ atom. In the second O2- site, O2- is bonded in a distorted trigonal non-coplanar geometry to one V5+ and two Zn2+ atoms. In the third O2- site, O2- is bonded in a distorted trigonal planar geometry to one V5+, one Co2+, and one Zn2+ atom. In the fourth O2- site, O2- is bonded in a distorted trigonal planar geometry to one V5+, one Co2+, and one Zn2+ atom. In the fifth O2- site, O2- is bonded in a 3-coordinate geometry to one V5+, one Co2+, and one Zn2+ atom. In the sixth O2- site, O2- is bonded in a 3-coordinate geometry to one V5+ and two Co2+ atoms. In the seventh O2- site, O2- is bonded in a 2-coordinate geometry to one V5+, one Co2+, and one Zn2+ atom. In the eighth O2- site, O2- is bonded in a 2-coordinate geometry to one V5+ and two Zn2+ atoms. In the ninth O2- site, O2- is bonded in a bent 150 degrees geometry to two V5+ atoms. In the tenth O2- site, O2- is bonded in a distorted water-like geometry to two V5+ atoms. In the eleventh O2- site, O2- is bonded in a distorted trigonal planar geometry to one V5+ and two Co2+ atoms. In the twelfth O2- site, O2- is bonded in a 3-coordinate geometry to one V5+, one Co2+, and one Zn2+ atom. In the thirteenth O2- site, O2- is bonded in a distorted trigonal non-coplanar geometry to one V5+, one Co2+, and one Zn2+ atom. In the fourteenth O2- site, O2- is bonded in a 3-coordinate geometry to two V5+ and one Co2+ atom.

36 MATERIALS SCIENCE↗

Design of a Scavenging Pyrrole Additive for High Voltage Lithium-Ion Batteries

We report 1-(dimethylamino) pyrrole (PyDMA) as an electrolyte additive for high voltage lithium-ion batteries based on LiNi 0.6 Mn 0.2 Co 0.2 O 2 (NMC622)//Graphite with an upper cutoff voltage of 4.4 V. Density Functional Theory (DFT) modeling indicates that the unique structure of PyDMA could be effective in preventing the hydrolysis of LiPF 6 in a carbonate electrolyte, mitigating issues related to HF formation. The calculations also indicated that the additive would oxidize at lower potentials than typical electrolyte solvents, which could lead to protective films at the cathode surface. These expectations were tested using Nuclear Magnetic Resonance (NMR) and extensive electrochemical characterization. NMR studies confirmed the superb dehydrating capability of PyDMA, which successfully prevents HF formation even at high water content. Addition of 0.5 wt% PyDMA resulted in improved capacity retention in full-cells, and also in lower levels of transition metal dissolution from the cathode. Incremental capacity (dQ/dV) analysis indicates that benefits of PyDMA at low concentration (0.5–1 wt%) are associated with decreased rates of Li + -trapping reactions, and that higher concentrations of the additive can lead to isolation of cathode domains. Furthermore, our study indicates that PyDMA could be a promising electrolyte additive for high voltage lithium-ion batteries at a low concentration.

25 ENERGY STORAGE↗

Stabilizing LiCoO 2 at 4.6 V by regulating anti-oxidative solvents

For LiCoO 2 (LCO) operating at high voltages (>4.5 V vs. Li/Li + ), the intensive side reactions between LCO and traditional ethylene carbonate (EC)-based electrolytes with LiPF 6 salts can produce plenty of corrosive species (such as HF and HPO 2 F 2 ), causing severe surface degradation. Herein, anti-oxidative fluoroethylene carbonate (FEC) and difluoroethylene carbonate (DFEC) were selected as co-solvents to reduce the generation of corrosive species. Besides, PF 6 − anions enrich the Helmholtz plane of the LCO/electrolyte interface and promote the formation of a robust cathode/electrolyte interphase (CEI) featuring LiF/Li x PO y F z /Li 3 PO 4 inorganics and P-containing organics under the synergy of fluorinated solvents, which significantly inhibits the catalysis of highly oxidative Co 4+ /O n− (0 < n < 2). Benefiting from the reduced corrosive species and reinforced CEI, the layered structure of the LCO surface is well preserved during long-term cycling, with a highly reversible O3/H1-3 phase transition. Consequently, a LCO||graphite pouch cell exhibits a remarkable capacity retention of 85.7% after 500 cycles in 3.0–4.55 V. Furthermore, this work provides a new insight into developing advanced functional electrolytes for high-voltage lithium-ion batteries.

Co/O loss↗