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Boosting ionic conductivity in LixAlCl3-xOx solid electrolytes through anion-mixing-engineered ion diffusion channels
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Liming Zhanga, Chenjie Loub, Shuaika Liangc, Wei Xiac, Rui Wangd, Longfei Lia, Chengyu Fua, Mingxue Tangb, Rong Xiange, Wei Wangf, Yichun Xug, Hongfa Xianga, Xuyong Fenga
Chinese Chemical Letters | 2026, 37(10) : 111558
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Chinese Chemical Letters | 2026, 37(10): 111558
• Communication •
Boosting ionic conductivity in LixAlCl3-xOx solid electrolytes through anion-mixing-engineered ion diffusion channels
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Liming Zhanga, Chenjie Loub, Shuaika Liangc, Wei Xiac, Rui Wangd, Longfei Lia, Chengyu Fua, Mingxue Tangb, Rong Xiange, Wei Wangf, Yichun Xug, Hongfa Xianga, Xuyong Fenga
Affiliations
  • aSchool of Materials Science and Engineering, Anhui Provincial Key Laboratory of Advanced Functional Materials and Devices, Hefei University of Technology, Hefei 230009, China
  • bCenter for High Pressure Science and Technology Advanced Research, Beijing 100193, China
  • cNingbo Key Laboratory of All-Solid-State Battery, Eastern Institute for Advanced Study, Eastern Institute of Technology, Ningbo 315201, China
  • dFaculty of Materials Science and Chemistry, China University of Geosciences, Wuhan 430074, China
  • eState Key Laboratory of Fluid Power and Mechatronic Systems, Zhejiang Provincial Key Laboratory for Atomic-level Manufacturing, School of Mechanical Engineering, Zhejiang University, Hangzhou 310027, China
  • fCAS Key Laboratory of Design and Assembly of Functional Nanostructures, Fuzhou 360002, China
  • gInstitute of Solid State Physics, Hefei Institutes of Physical Science, Chinese Academy of Sciences, Hefei 230031, China
About Author:

1

These authors contributed equally to this work.

CRediT authorship contribution statement

Liming Zhang: Writing – original draft, Methodology, Formal analysis, Data curation.

Chenjie Lou: Formal analysis, Data curation.

Shuaika Liang: Formal analysis, Data curation.

Wei Xia: Investigation, Formal analysis.

Rui Wang: Writing – original draft, Resources, Funding acquisition.

Longfei Li: Data curation.

Chengyu Fu: Data curation.

Mingxue Tang: Resources, Investigation, Formal analysis, Data curation.

Rong Xiang: Writing – review & editing, Funding acquisition.

Wei Wang: Writing – review & editing, Formal analysis.

Yichun Xu: Writing – original draft, Formal analysis, Data curation.

Hongfa Xiang: Writing – review & editing, Supervision, Resources, Funding acquisition, Conceptualization.

Xuyong Feng: Writing – review & editing, Supervision, Investigation, Funding acquisition, Conceptualization.

Published: 2026-10-15 doi: 10.1016/j.cclet.2025.111558
Outline
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Solid-state electrolytes composed of earth-abundant elements offer significant cost advantages for large-scale energy storage applications. However, their widespread adoption is hindered by inherently low ionic conductivity. In this study, we report a low-cost solid-state electrolyte, LixAlCl3-xOx (0.6 ≤ x ≤ 1.1), with dramatically enhanced ionic conductivity achieved through the construction of fast ion-conducting channels via an innovative anion mixing strategy. First-principles calculations and experimental characterizations reveal that the Cl−/O2− anion mixing expands the distribution of Li+ ions within the lattice while reducing the distance between adjacent sites. This structural optimization results in a low Li+ migration activation energy of 0.3 eV and elevates the ionic conductivity from 10−3 mS/cm to 1.5 mS/cm. Furthermore, the Cl-/O2- mixing synergistically combines the advantages of both anions, endowing the LixAlCl3-xOx electrolyte with high-voltage stability (up to 3.96 V vs. Li+/Li), robust interfacial compatibility, and air stability. When integrated into all-solid-state batteries with a LiCoO2Li0.8AlCl2.2O0.8Li6PS5ClLi-Si configuration, it delivers an initial capacity of 127 mAh/g and retains 94.4% of its discharge capacity after 180 cycles at 0.3 C.

All solid-state batteries  /  Mix anion solid state electrolytes  /  Halide  /  Solid state NMR  /  Neutron pair distribution function
Liming Zhang, Chenjie Lou, Shuaika Liang, Wei Xia, Rui Wang, Longfei Li, Chengyu Fu, Mingxue Tang, Rong Xiang, Wei Wang, Yichun Xu, Hongfa Xiang, Xuyong Feng. Boosting ionic conductivity in LixAlCl3-xOx solid electrolytes through anion-mixing-engineered ion diffusion channels[J]. Chinese Chemical Letters, 2026 , 37 (10) : 111558 - . DOI: 10.1016/j.cclet.2025.111558
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The high cost of solid-state electrolytes (SSEs) poses a significant barrier to the industrial adoption of all-solid-state lithium-ion batteries (ASSLBs). This cost is primarily driven by two factors: the use of expensive raw materials and energy-intensive synthesis processes [1]. For instance, elements such as La in Li7La3Zr2O12 [2–6], Ge in Li10GeP2S12 [7–9], and Sc/In Li3ScCl6/Li3InCl6 [10–12] are scarce and significantly increase material costs. Although earth-abundant elements like P, S, and Cl are used in sulfide SSEs (e.g., Li6PS5Cl), the complex preparation process of Li2S still elevates the overall cost [13]. Similarly, oxide electrolytes with garnet and NASICON structures require sintering temperatures exceeding 1000 ℃, leading to high energy consumption [4,14–17]. Halide SSEs, such as Li2ZrCl6, often involve inefficient synthesis methods like long time high-energy ball milling (500 rpm for 45 h) [18–23]. These challenges underscore the urgent need to develop low-cost SSEs composed of earth-abundant elements and scalable synthesis methods.
Aluminum (Al), the most abundant metallic element in the Earth's crust (Figs. S1a and b in Supporting information), offers a promising solution. Aluminum chloride (AlCl3), a low-cost precursor with a melting point of 194 ℃, enables the synthesis of SSEs (e.g., LiAlCl4) at relatively low temperatures (< 200 ℃) [24–27]. However, the ionic conductivity of solid LiAlCl4 remains low (10-6 S/cm at 25 ℃), limiting its applicability in ASSBs [24,28].
The ionic conductivity of SSEs is closely tied to their structural properties. Short distances between adjacent charge carriers, particularly in face-sharing polyhedra, are critical for achieving rapid ion conduction. Notable examples include body-centered sulfides [29–33] and LaCl3-based Li+/Na+ conductors [34,35]. In LiAlCl4, however, all Li+ ions occupy octahedral sites (4e, O site), which are either corner-sharing or edge-sharing, with a Li-Li distance exceeding 4.22 Å (Fig. 1a). The migration of Li+ ions between adjacent octahedral sites involves passing through one or two tetrahedral sites (T site), following an O-T-O or O-T-T-O pathway. The higher site energy of tetrahedral sites increases the activation energy for ion diffusion, resulting in low ionic conductivity (Fig. 1b and Fig. S2 in Supporting information) [25]. Previous studies have shown that structural distortion induced by high-energy ball milling can reduce the energy of Li+ ions in tetrahedral sites, enabling partial relocation of Li+ ions to these sites [24]. This approach increases the ionic conductivity of LiAlCl4 by approximately 20 times, reaching 2.1 × 10−5 S/cm [24]. Nevertheless, this value remains insufficient for practical applications.
Anion mixing has emerged as an effective strategy for tuning the site energy and distribution of Li+ ions in SSEs. Since anions directly coordinate with Li+ ions, they exert a strong influence on Li+ site energy. Anion mixing (e.g., Cl−/O2−, S2−/Cl−, and S2−/O2−) enables Li+ ions to occupy a wider range of sites, shortening the migration distance between charge carriers and enhancing ionic conductivity [18,36–45]. In this study, we employ Cl−/O2− mixing to significantly improve the ionic conductivity of LixAlCl3-xOx. This strategy increases the number of Li+-occupied sites and reduces the distance between adjacent sites, leading to a lower ion migration activation energy (0.30 eV) and a remarkable enhancement in ionic conductivity (1.5 × 10−3 S/cm).
The electrolyte developed in this study uses AlCl3 and LiOH as raw materials and can be prepared with heating at 200 ℃ for only 0.5 h (Fig. S1c in Supporting information). In contrast to crystalline LiAlCl4, the synthesized LixAlCl3-xOx exhibits a pure amorphous structure (Fig. S3 in Supporting information). The incorporation of O2− into LixAlCl3-xOx likely facilitates the formation of highly stable Al−O−Al fragments. During cooling from the molten state, the presence of these Al−O−Al fragments restricts atomic rearrangement (crystallization), resulting in the retention of an amorphous structure at room temperature [43]. However, when x exceeds 0.8, a LiCl phase emerges in the product, and its content increases with higher O2− concentrations (Fig. S3). This is because the enthalpy (H) and entropy (S) of LixAlCl3-xOx increases upon the incorporation of O2− (Li+) and formation of defects (O2− substituted Cl−, interstitial Li+). When ∆G = ∆H -T∆S < 0, the structure of LixAlCl3-xOx would be thermal-dynamically stable (x ≤ 0.8). Otherwise, the structure would be unstable and ultimately decompose to impurities such as LiCl (x > 0.8). In the main glass phase, more anion vacancies and fewer Li+ interstitial defects would be formed (Lix-yAlCl3-x-yOx). This indicates that the high energy of interstitial Li+ ions is the main defect leading to instability of LixAlCl3-xOx.
The Cl−/O2− mixing in the amorphous phase is further confirmed by X-ray photoelectron spectroscopy (XPS) (Fig. S4 in Supporting information). The Li 1s and Al 2p spectral peaks for Li0.8AlCl2.2O0.8 are situated between those of LiAlCl4 and LiAlO2, providing clear evidence of Cl−/O2− anion mixing in Li0.8AlCl2.2O0.8.
Solid-state nuclear magnetic resonance (ssNMR) spectroscopy is a powerful tool for probing the local structure and distribution of Li+ ions [46–48], providing critical insights into ion conduction mechanisms in LiAlCl4 and LixAlCl3-xOx (Figs. 1c-f). In LiAlCl4, a single 7Li resonance signal is observed, confirming that Li+ ions exclusively occupy octahedral sites (4e sites) coordinated by six Cl− ions (Fig. 1a and Fig. S5 in Supporting information) [43]. The introduction of O2− significantly alters the local Li+ environment in the halide SSE. The 6Li NMR spectra of LixAlCl3-xOx reveal three distinct resonance signals: one corresponding to the LiCl impurity (~−1.2 ppm) and two others (~−0.88 and −0.65 ppm) arising from different Li+ sites within the LixAlCl3-xOx structure (Fig. 1c). The presence of cross-peaks in the 2D exchange spectroscopy (EXSY) NMR spectra further confirms the rapid exchange of Li+ ions between these two distinct sites (Figs. 1d-f). In the 1D spectra, all signals representing different Li+ environments are clearly resolved. At a short mixing time (0.05 ms), the exchange of Li+ ions between the two sites is negligible (Fig. 1d). However, as the mixing time is extended to 1 ms and 100 ms, distinct cross-peaks emerge between the two Li+ chemical environments (−0.88 and −0.65 ppm), as highlighted in the dotted boxes in Figs. 1e and f. This observation demonstrates that Li+ ions dynamically migrate between neighboring sites, creating efficient conduction pathways.
The incorporation of O2− into LixAlCl3-xOx significantly enhances its ionic conductivity, reaching values on the order of 10−3 S/cm at 25 ℃. The composition is optimal at x = 0.8, when it is phase-pure amorphous without significant impurities (based on XRD), and the ionic conductivity reaches an optimum of 1.5 × 10−3 S/cm (Figs. 2a and c). For x < 0.8, the improvement in ionic conduction with increasing O2− content is attributed to the rising defect density resulting from O2−/Cl− mixing. Conversely, for x > 0.8, the decline in ionic conductivity is due to the formation of impurities (Fig. S3). Additionally, the amorphous structure induced by O2- doping should also facilitates the distribution of Li+ ions across multiple sites, further contributing to the enhanced ionic conductivity [24].
Conductivity measurements also reveal a significant reduction in activation energy to 0.30 eV for Li0.8AlCl2.2O0.8 (Figs. 2b and c, Fig. S6 in Supporting information). Furthermore, the electronic conductivity of Li0.8AlCl2.2O0.8, determined from DC polarization curves (Fig. 2d and Fig. S7 in Supporting information), is calculated to be 6.98 × 10−10 S/cm. This value is substantially lower than that of many widely studied solid-state electrolytes, highlighting the material's potential for minimizing electronic leakage in solid-state battery applications [49–51].
To elucidate the local structure of amorphous LixAlCl3-xOx and gain deeper insights into Li+ ion conduction pathways, density functional theory (DFT) calculations were performed (Figs. 3a-d). The initial structure of Li0.75AlCl2.25O0.75 was constructed by replacing 0.75 Cl− with O2− in AlCl3 and adding 0.75 Li+ ions to maintain charge neutrality. The hypothesized structure was heated to 800 K for 10 ps with a time step of 1 fs to obtain a fully melted configuration. Subsequently, the amorphous structure was annealed at lower temperatures by adjusting the model size to achieve the appropriate pressure. The final structure of Li0.75AlCl2.25O0.75 was energy-minimized (Fig. 3a and Table S1 in Supporting information). The simulated structure reveals that Al3+ ions remain in tetrahedral sites, with partial replacement of Cl− by O2− leading to the formation of Al-O-Al fragments (Fig. 3a and Fig. S8 in Supporting information). The framework of Li0.75AlCl2.25O0.75 consists of AlClnO4-n units, while Li+ ions occupy various interstitial sites, coordinated by different combinations of Cl− and O2− ions (e.g., 3Cl, 1O2Cl, 4Cl, 2O3Cl). Compared to LiAlCl4, the coordination environments of Li+ ions in Li0.75AlCl2.25O0.75 are more complex, resulting in two broad peaks in the NMR spectra (Fig. 2b). The substitution of Cl− with the more electronegative O2− reduces the electron cloud density around the Li+ nucleus, leading to a larger chemical shift (toward the left) [36,52]. Consequently, the left-shifted 6Li peak (−0.65 ppm) likely corresponds to Li+ ions coordinated with a higher number of O2− anions.
Compared to LiAlCl4, where Li+ ions predominantly occupy octahedral sites, the increased distribution of Li+ sites in LixAlCl3-xOx suggests a reduction in the distance between adjacent Li+ sites. A segment of the simulated Li0.75AlCl2.25O0.75 structure (Fig. 3b) confirms that the Li–Li distance (3.03–3.80 Å) is significantly shorter than that in LiAlCl4 (4.22–4.88 Å). This observation is further supported by the radial distribution function (RDF) of Li–Li (Fig. 3c), which reveals shorter Li-Li distances in Li0.75AlCl2.25O0.75. Additionally, the peaks corresponding to short Li-Li distances gradually diminish with increasing temperature, indicating structural collapse at elevated temperatures. At 600 K, the loss of short-range order confirms that Li0.75AlCl2.25O0.75 transitions to a molten state.
In solid-state electrolytes (SSEs), the distribution of Li+ ions is governed by their site energy at different interstitial positions, which is primarily determined by the bond energy between Li+ ions and surrounding anions. This bond energy can be described by the equation E(r) =−ZiZj4πɛ0r+Brn, where ε0 is the dielectric constant, B and n are constant, Zi and Zj are ion charge number, r is the distance between Li+ ions and surrounding anions [44]. When the anion type changes, the site energy and Li+ distribution in SSEs undergo significant modifications. In chloride-based SSEs, Li+ ions predominantly occupy octahedral interstices, where the distance between adjacent sites is relatively large. However, upon the introduction of O2− ions, the site energy of Li+ in tetrahedral and interstitial sites decreases, increasing the number of favorable distribution sites. Consequently, the distance between adjacent Li+ sites is substantially reduced.
The Li+ ion conduction in Li0.75AlCl2.25O0.75 was also simulated (Fig. 3d). The Li+ diffusion coefficients range from 10−6 cm2/s to 10−5 cm2/s between 300 K and 800 K, demonstrating rapid ion migration across this temperature range [38]. The calculated activation energy (0.16 eV) and ionic conductivity (26.6 mS/cm at 300 K) further confirm the presence of fast ion-diffusion channels and efficient ion conduction in Li0.75AlCl2.25O0.75. Notably, the Li+ ion probability densities reveal potential diffusion pathways (Fig. S9 in Supporting information). At 300 K, Li+ ions exhibit partial long-range diffusion through low-energy pathways. As the temperature increases to 600 K and 800 K, the more uniform probability densities suggest a flatter energy landscape in Li0.75AlCl2.25O0.75.
The simulated structure was further validated by neutron pair distribution function (nPDF) analysis. The PDF profile features a peak at 2.165 Å, corresponding to Al-Cl pairs, while strong peaks at 3.595 Å and 6.425 Å are attributed to Al-Al pairs. Below 6 Å, Li0.8AlCl2.2O0.8 exhibits multiple strong peaks, indicative of its characteristic short-range order. Beyond 10 Å, the peak intensity diminishes, reflecting the material's long-range disorder and amorphous nature, consistent with XRD results. To improve refinement accuracy, the structural unit of Li0.75AlCl2.25O0.75 was expanded to a 3 × 3 × 3 supercell. The refined nPDF spectrum yields an good fit (χ2 = 4.8), validating the simulated 3 × 3 × 3 structure (Fig. 3e) [53]. The refined structure is shown in Fig. 3f, which closely matches the initial simulation.
Like other chloride solid electrolytes, Li0.8AlCl2.2O0.8 is susceptible to deliquescence in natural air [54], but the electrolyte is well stabilized in dry air. After exposing Li0.8AlCl2.2O0.8 to a dry room atmosphere (dew point: −40 ℃) for 24 h, the ionic conductivity decreased slightly from 1.5 mS/cm to 1.1 mS/cm, while the amorphous structure remained intact (Fig. S10 in Supporting information). A minor mass increase from 0.3346 g to 0.3449 g further confirms its stability in dry air, attributed to the strong Al-O and Li-O bonds. Linear sweep voltammetry (LSV) of Li0.8AlCl2.2O0.8-Super P||Li0.8AlCl2.2O0.8||Li reveals an electrochemical stability window ranging from 1.12 V to 3.96 V vs. Li+/Li (Fig. S11 in Supporting information), comparable to other halide solid-state electrolytes [34,55].
To assess the practical applicability of Li0.8AlCl2.2O0.8 as a solid-state electrolyte (SSE), an all-solid-state battery (ASSB) was assembled using a commercial LiCoO2 composite cathode and a homemade Li-Si anode. A transition layer of homemade Li6PS5Cl was incorporated to isolate the Li0.8AlCl2.2O0.8 SSE from the Li-Si anode (Fig. 4a). Given the electrochemical stability window of Li0.8AlCl2.2O0.8, it was employed as a catholyte in the composite cathode. To enhance stability, Li-Si (with a higher potential than Li metal) was selected as the anode [56], while Li6PS5Cl (Fig. S12 in Supporting information), known for its compatibility with anodes, was used as the anolyte to separate Li0.8AlCl2.2O0.8 from the Li-Si anode. To minimize oxidation and decomposition of Li0.8AlCl2.2O0.8 above its oxidation potential (3.96 V vs. Li+/Li), conductive carbon was excluded from the composite cathode, enabling LiCoO2 to be charged to 4.2 V vs. Li-Si [57].
Cross-sectional SEM images of the ASSB (Figs. 4b and c) reveal layer thicknesses of ~24 µm (LiCoO2 composite cathode), 300 µm (Li0.8AlCl2.2O0.8 SSE), 110 µm (Li6PS5Cl SSE), and 130 µm (Li-Si anode). High-magnification SEM images (Fig. S13 in Supporting information) confirm the dense morphology of the Li0.8AlCl2.2O0.8 layer. Under a pressure of 150 MPa, Li0.8AlCl2.2O0.8 appears compact and pinhole-free (Fig. S13b), while Li6PS5Cl exhibits a porous structure (Fig. S13c). The total resistance of the ASSB before cycling exceeds 400 Ω (Fig. S14 in Supporting information), primarily attributed to the composite cathode (Fig. S15 in Supporting information). This high resistance stems from the high content (75 wt%) of poorly conductive LiCoO2 in the cathode layer.
The LiCoO2||Li0.8AlCl2.2O0.8||Li6PS5Cl||Li-Si ASSB was cycled at various current densities between 2.5 V and 4.2 V under an operating pressure of 120 MPa at 25 ℃ (Figs. 4d-g). At 0.1 C (25 ℃), the battery delivers a discharge capacity of 150 mAh/g with a high initial Coulombic efficiency (CE) of 97%, indicating highly reversible reactions (Fig. 4d). This performance underscores the effectiveness of the battery configuration and the excellent oxidation stability of Li0.8AlCl2.2O0.8, which minimizes side reactions during cycling. As the current density increases, the discharge capacities decrease to 138 mAh/g (0.2 C), 128 mAh/g (0.3 C), 108 mAh/g (0.5 C), and 73 mAh/g (1 C). The rate capability is currently limited by the high cathode resistance, necessitating further optimization of the cathode composition [67]. Remarkably, the ASSB retains 94.4% of its discharge capacity after 180 cycles at 0.3 C (Fig. 4g). Even after 1000 cycles at 1 C, the capacity retention reaches 70.6% (Fig. S16 in Supporting information), demonstrating exceptional cycling stability. Post-cycling resistance measurements (Fig. S14) reveal a slight reduction in total resistance after 180 cycles at 0.3 C or 1000 cycles at 1 C, further confirming the outstanding oxidation stability of Li0.8AlCl2.2O0.8 SSE.
In conclusion, we have developed a low-cost LixAlCl3-xOx solid-state electrolyte (SSE) through an innovative anion mixing strategy, which offers a compelling combination of low cost, high oxidation stability, excellent interfacial compatibility, and superior ionic conductivity (Fig. 4h). The use of earth-abundant elements significantly reduces material costs, while the short sintering time (30 min) at a low temperature (200 ℃) further minimizes production expenses. The O2−/Cl− dual-anion design enables Li+ ions to occupy multiple sites within the LixAlCl3-xOx lattice, reducing Li+ migration distances and enhancing ionic conductivity. The optimized LixAlCl3-xOx SSE achieves a room-temperature ionic conductivity of 1.5 mS/cm, representing a three-order-of-magnitude improvement over LiAlCl4. The incorporation of O2− into the AlCl3-based halide not only improves oxidation stability but also enhances air stability, owing to the stronger bonding between O2− and Li+/Al3+. The dense morphology of LixAlCl3-xOx SSE ensures excellent interfacial contact with the cathode, further supporting its practical application. The exceptional oxidation stability and compactability of LixAlCl3-xOx make it a promising catholyte candidate for all-solid-state batteries (ASSBs). In a proof-of-concept demonstration, a LiCoO2/Li-Si ASSB incorporating Li0.8AlCl2.2O0.8 as the catholyte delivered outstanding electrochemical performance, achieving a high initial Coulombic efficiency of 97% and retaining 94.4% of its discharge capacity after 180 cycles at 0.3 C. These results highlight the significant potential of LixAlCl3-xOx SSEs for practical applications in next-generation solid-state batteries. However, the absence of conductive carbon and the high weight ratio of low conductive LiCoO2 (75%) at the cathode make the ASSB have high resistance which affects the rate performance. Further research could be enhancement of oxidation stability of SSE, adding conductive carbon if stability allows, or surface modify the LiCoO2 cathode to improve the battery performance.
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doi: 10.1016/j.cclet.2025.111558
  • Receive Date：2025-05-28
  • Online Date：2026-10-27
  • Published：2026-10-15
Article Data
Affiliations
History
  • Received：2025-05-28
  • Revised：2025-07-04
  • Accepted：2025-07-08
Affiliations
    aSchool of Materials Science and Engineering, Anhui Provincial Key Laboratory of Advanced Functional Materials and Devices, Hefei University of Technology, Hefei 230009, China
    bCenter for High Pressure Science and Technology Advanced Research, Beijing 100193, China
    cNingbo Key Laboratory of All-Solid-State Battery, Eastern Institute for Advanced Study, Eastern Institute of Technology, Ningbo 315201, China
    dFaculty of Materials Science and Chemistry, China University of Geosciences, Wuhan 430074, China
    eState Key Laboratory of Fluid Power and Mechatronic Systems, Zhejiang Provincial Key Laboratory for Atomic-level Manufacturing, School of Mechanical Engineering, Zhejiang University, Hangzhou 310027, China
    fCAS Key Laboratory of Design and Assembly of Functional Nanostructures, Fuzhou 360002, China
    gInstitute of Solid State Physics, Hefei Institutes of Physical Science, Chinese Academy of Sciences, Hefei 230031, China

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(H. Xiang)
(X. Feng)
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表12种不同金属材料的力学参数
科
Family		 属数
Number of
genus		 种数
Number of
species		 占总种数比例
Percentage of
total species (%)		 属
Genus		 种数
Number of
species		 占总种数比例
Percentage of total
species (%)
鹅膏菌科Amanitaceae 2 11 5.26 鹅膏菌属 Amanita 10 4.78
小菇科 Mycenaceae 2 12 5.74 丝盖伞属 Inocybe 5 2.39
多孔菌科 Polyporaceae 8 14 6.70 蜡蘑属 Laccaria 5 2.39
红菇科 Russulaceae 3 23 11.00 小皮伞属 Marasmius 6 2.87
小菇属 Mycena 11 5.26
光柄菇属 Pluteus 5 2.39
红菇属 Russula 17 8.13
栓菌属 Trametes 5 2.39
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