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Accessing the full potential of aluminum alloy electrodes for Li-batteries: phase formation in the lithium-aluminum system
Ghavidel, Mohammadreza Zamanzad; Feygin, Eliana M.; Kupsta, Martin; Le, Jon; Fleischauer, Mike
ELECTROCHEMICAL RESULTS
Up to four distinct plateaus were present in voltage-capacity data. Plateaus are characteristic of co-existing phases.
Voltage plateaus were often preceded by a nucleation overpotential. The nucleation overpotential decreased as the temperature increased.
Some plateaus sagged significantly, indicating slow diffusion.
Lithium electrochemically inserted in to aluminum foil at 60 °C
forms three plateaus on insertion and removal. Subsequently
cooling the system to 30 °C cuts the capacity in half. The second
and third plateaus do not appear when testing at 30 °C.
MOTIVATION
Metal alloys have the potential to increase the capacity of lithium-ion batteries up to 50% over batteries made with standard graphite electrodes. Graphite stores lithium by intercalating lithium atoms between layers of graphine, and can store one Li per six carbon
atoms (~360 mAh g-1 or 0.17 Li/C). Metals store lithium via alloying
reactions. Equilibrium phase diagrams suggest Al4Li9 should form
(2250 mAh g-1 or 2.25 Li/Al). However, β-AlLi (1000 mAh g-1, 1 Li/Al)
is the only Al-Li phase typically observed at standard temperatures. Here, we explore the factors influencing this discrepancy.
METHODS
SUMMARY
Aluminum is an abundant, promising electrode material for lithium-ion batteries. We can access three new Al-Li phases and double the storage capacity for lithium by increasing the operating temperature.
Different phases of Li-Al were observed in the fully lithiated samples, depending on the insertion temperature.
STRUCTURAL+ELECTROCHEMICAL RESULTS
Plateaus observed during (de)lithiation correspond to the growth
of the next Al-Li phase. Al ↔ β-AlLi ↔ Al2Li3 ↔ AlLi2-x ↔ Al4Li9.
Electrochemical results follow the thermal phase diagram.
β-AlLi initially forms at temperatures above 50 ºC; measured and
expected capacities are in line (~1000 mAh g-1, 1 Li/Al). Large
nucleation overpotentials are evident at most temperatures.
Al2Li3 forms completely at temperatures above 60 ºC, measured
and expected capacities are in line (~1500 mAh g-1, 1.5 Li/Al).
Nucleation barriers are not prominent above 50 ºC.
AlLi2-x forms partially at 60 ºC, and more fully above 90 ºC.
Measured capacities are ~300 mAh g-1 higher than expected,
likely due to electrolyte breakdown at low potentials (~20 mV). Nucleation barriers are present.
Al4Li9 partially forms at temperatures above 100 ºC. Nucleation
barriers and slow diffusion are prominent even at 150 ºC.
Measured capacities on Li removal align with expected values.
CONCLUSION
Lithium can be electrochemically inserted in to and removed from thick aluminum foil at moderate temperatures.
Nucleation barriers and slow diffusion have large effects on the observed phases.
Nucleation of β-AlLi was particularly challenging. This may be due
to the native surface oxide present on aluminum foil.
Four different phases of Al-Li (β-AlLi, Al2Li3, AlLi2-x, and Al4Li9) can
be electrochemically formed at temperatures above 100 ºC.
Slow diffusion prevents the full capacity of Al4Li9 from being
realized, even at low current densities and high temperatures.
Liquid electrolyte breakdown adds to the measured capacity at
potentials below 0.02 V vs. Li/Li+.
Phase transitions on lithium removal can be used to quantify the amount of electrolyte consumed.
FUTURE WORK
Determining the limiting current density as a function of temperature on the nucleation of different Al-Li phases.
Quantifying the diffusion coefficient of Li in different Al-Li phases. Combining nucleation and diffusion insight to predict the
performance of all morphologies of aluminum alloy electrodes.
Develop in-situ x-ray diffraction techniques to verify phases and
phase transitions without cooling the sample to room
temperature. Additional phases (-AlLi, Al4Li5) may be present.
Figure 1: Potential vs. capacity curves for Li-Al cells cycled at three different temperatures.
Mohammadreza Zamanzad Ghavidel,
1,*Eliana M. Feygin,
2,3Martin Kupsta,
1Jon Le,
2and Mike Fleischauer
1,21Department of Physics, University of Alberta, Edmonton, Alberta
2National Research Council – Nanotechnology Research Centre, Edmonton, Alberta
3Department of Physics, University of Waterloo, Waterloo, Ontario
*zamanzad@ualberta.ca
Accessing the full potential of aluminum alloy electrodes for Li-batteries:
phase formation in the lithium-aluminum system
dHex dHexN dHex
Variable oligosaccharide chain (n=2-7) composed of Pen, dhex, Hex, HexA
T189 , S260 dHexNF
173Da
Figure 2: Potential vs. Capacity curves for Al foil cycled at 60 °C then
lithiated at 30 °C to 0.001 V vs. Li/Li+.
Electro-chemistry
X-ray diffraction
Teflon tape Al-Li alloy Gl ass PP Figure 3: XRD patterns collected from aluminum samples lithiated to0.001 V vs. Li/Li+ at different temperatures.
Figure 4: (A) Potential vs. capacity curves for Al-Li cells cycled at 100 °C
to specific potentials (as indicated). The data sets are self-consistent.
(B) XRD patterns from samples collected at potential specified in (A). Each insertion / removal data set was collected using a fresh Al foil.
Figure 5: Phase diagram of Al-Li (grey) and potential versus Li/Al ratio data (blue) collected at 100 ºC.
Figure 6: (top) Potential vs. capacity curves for Al foil lithiated at 120 °C
with different current densities. (bottom) Measured potential for the
β-AlLi ↔ Al2Li3 plateau at different temperatures and current densities.
Potential changes should be linear with 1/T for a given phase transition.
STRUCTURAL RESULTS
ELECTROCHEMICAL PHASE DIAGRAM
variable temperature test chamber
This is the first ever demonstration of the electrochemical