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Batteries 101
Jordi Cabana Assistant Professor in Chemistry
[email protected] Office: 4146SES, Tel: 312-355-4309
LAS493, 11/11/14
What is a battery? The Daniell cell
All ba&eries are made of: -‐‑ Two electrodes: compounds or elements at different potentials (e.g., standard reduction potentials in solution). They must uptake/release ions and electrons. -‐‑ An electrolyte: can only conduct ions, electronic insulator. Electrons flow through the external circuit.
Rechargeable batteries are based on redox reactions
Palacin, Chem. Soc. Rev. 38 (2009), 2565.
1) Anode – Oxidation 2) Cathode – Reduction Semantic challenge: strictly speaking, in a rechargeable ba&ery, the anode/cathode change on discharge/charge. In reality, you will often see cathode being used for the “positive electrode”.
Batteries come in various flavors (I)
“Classical”: Two solid electrodes Liquid electrolyte
Br2/HBr
H2
HBr
Charge
Discharge
H2↔ 2H+ + 2eH2↔ 2H+ + 2eBr2 + 2H+ + 2e ↔ 2HBrBr2 + 2H+ + 2e ↔ 2HBr
Air-‐‑based: One solid electrode One solid/gas electrode Liquid electrolyte
Flow cell: Two solid electrodes: only provide electrons. Liquid electrolyte: also carries active compounds. ⇒ catholyte/anolyte.
Can also be made with solid electrolytes (polymers, ceramics): may require operating at high T, molten electrodes.
Combinations are possible (e.g. solid electrode vs. catholyte)
Girishkumar et al., J. Phys. Chem. Lett. 1 (2010), 2193.
Source: A. Weber
Q=nF
What metrics matter? 1) Rechargeable (secondary) vs. non-‐‑rechargeable (primary): defined by the extent of
undesired and irreversible electrochemical reactions occur during discharge (spontaneous process). E.g.: Zn/MnO2 (primary) vs. Li-‐‑ion (secondary).
2) Energy storage: Back to the Daniell cell… 1) Anode (oxidation): Zn(s) → Zn2+
(aq)+ 2e-‐‑ E0 = −0.76 V 2) Cathode (reduction): Cu2+
(aq) + 2e-‐‑ → Cu(s) E0 = +0.34 V ΔE= 1.1 V
• Power storage: ability of the cell to deliver its energy fast (days to… milliseconds?).
• Life can be defined many ways: • Calendar life: time before a ba&ery dies, whether it is used or not. • Shelf life: time before a ba&ery dies if it is being stored unused (related to self-‐‑
discharge). • Cycle life: number of times a ba&ery can be recharged before it dies.
ΔG=QE
P=IE
5) Anyone said Safety and Cost? Simple: no explosions, cheaper than gasoline!
Free Energy (Work)
How about those units?
E=QV= Wh/kg or Wh/l In SI: 1 Wh = 1 VAh 1 mAh = 3.6 C
P=IV= W/kg or W/l
You will hear a lot about a certain electrode material delivering x mAh/g (=Specific capacity)
Cash is king…
Costco was here on 11/10/14
Battery technology charges ahead, McKinsey&Co, July 2012 http://www.mckinsey.com/insights/energy_resources_materials/battery_technology_charges_ahead#
…and we still have ways to go! Battery technology charges ahead, McKinsey&Co, July 2012 http://www.mckinsey.com/insights/energy_resources_materials/battery_technology_charges_ahead#
“Developments in ba&ery manufacturing and component pricing will drive the majority of the savings from 2011 to 2015, while advances in capacity-‐‑boosting ba=ery technologies will drive the majority of reductions from 2016 to 2020 and beyond”
How do we bend that curve downwards?
Goodenough and Kim, Chem. Mater. 22 (2010), 593. Possibility 1: Engineer the device to minimize “packaging”. “Packaging” needed because: • Ba&eries need intensive management. • Ba&eries need safety features. • We cannot cycle electrodes that are more than 1 0 0 µ m t h i c k ⇒ l o w e r a c t i v e material/”packaging” ratio.
Possibility 2: Find electrodes and electrolytes that enable higher Q or E (higher ΔG): • We have a lot of possibilities… because none is good enough!
To maximize Q, you pick the lightest (and cheapest!) elements you can
Noble gases are out because they are essentially not redox active
To maximize E, pick elements that have redox activity a very different potentials
1) Anode (oxidation): Li(s) → Li+ + e-‐‑ E0 = −3.04 V 2) Cathode (reduction): F2(g) + 2e-‐‑ → 2F-‐‑ E0 = +2.87 V The Li/F2 ba&ery: at 5.91 V, highest energy density of all, but…
Li: F2:
Other less dangerous options… L i q u i d Electrodes
S o l i d Electrodes
Water Electrolytes
Solid Electrolytes
Organic Electrolytes
Note the progression in cell voltage from water to organic…
Palacin, Chem. Soc. Rev. 38 (2009), 2565.
Electrolyte determines achievable cell voltage
Compare the potential window of these organic solvents
• We need the electrolyte to be stable to reduction at the anode and oxidation at the cathode, i.e., inert in the potential window defined by electrode reactions.
• To maximize E, H2O is really not the best choice. • Note that we do not have an electrolyte that will be stable on both sides of the Li/F2
ba&ery, even if we were so crazy as to try…
Etacheri et al., Energy Environ. Sci. 4 (2011), 3243.
But, ultimately, electrodes define
both Q and E Let’s focus on them, using Li-ion batteries as
example
Raising Q is the most popular way to increase electrical energy
Q depends on the ability of a compound to accept-release ions (crystal chemistry) and electrons (redox chemistry). Do you know the stable oxidation states for transition metals? • LiCoIIIO2 → CoIVO2 280 mAh/g (but we can only go halfway because CoO2 is very unstable)
• Li + 6C → LiC6 372 mAh/g (these two are in your cellphones)
• 4Li + Si → Li4Si 3200 mAh/g
But putting a lot of Li comes at a price
+xLi Before After
4Li + Sn → Li4Sn 980 mAh/g (Compare with commercial graphite, at 370 mAh/g)
Xu et al., Nano Lett. 13 (2013), 1800.
This is how a battery looks like
Liu et al., Energy Environ. Sci. 4 (2011), 885.
Source: Q. Horn (Exponent)
Source: K. A. Persson
The atomic scale
Ni
Li O
Mn
0 5 10 15 20 2520
30
40
50
60
70
80
90
100
900C (air/1hr) 900C (air/1hr) + 500C (air/12hr) 900C (air/1hr) + 500C (O2/12hr) 900C (air/1hr) + 900C (air/12hr) 900C (O2/1hr) 900C (O2/1hr) + 500C (O2/12hr) 900C (O2/1hr) + 670C (O2/12hr)
900C (air/1hr) + 700C (O2/12hr) 900C (O2/1hr) + 700C (O2/12hr) 900C (air/1hr) + 700C (air/12hr) 900C (O2/1hr) + 730C (O2/12hr)
Nor
mal
ized
Dis
char
ge C
apac
ity (%
)
Cycle (#)
C/10
C/5
C/2
C
2C
5C
C/10
Disordered
Ordered
LiNi0.5Mn1.5O4
Atomic scale arrangement of ions in a la&ice can affect performance in an electrode.
We have gazillions of tiny grains in a real electrode!
Contact with current collector (Ti3+-rich)
Cross section (Ti4+-rich)
Pristine 10% DOD
25% DOD
50% DOD
Mechanism: Surface
+ Bottom-up
Kim et al., Adv. Funct. Mater. 23 (2013), 1214.
Li4Ti5O12
Electrode construction makes a huge difference
An electrode is a complex structure of: 1) active material, 2) conductive additive, 3) polymer binder, 4) SPACE. Process of assembly of the same components leads to dramatic performance differences.
Source: G. Liu (LBNL)
Electrode-electrolyte interfaces
The electrode surface may become to oxidizing or reducing for the electrolyte ⇒ side reactions that passivate electrode and/or consume electrolyte.
LNMO=LiNi0.5Mn1.5O4
Norberg et al., Electrochem. Commun. 34 (2013), 29.
Changing one electrode dramatically affects performance
LNMO=LiNi0.5Mn1.5O4
Pairing a given positive electrode with two different negative electrodes can lead to cells with completely different behavior.
Source: V. S. Ba=aglia (LBNL)
So we work hard at visualizing how chemical reactions happen at multiple scales
Picture
Picture
C1
C/20
Ni-Metal Oxide NiOScalebar 0.2mmPicture
Halfway reduced:
Oxidized to 2V:
operando XAS/XRD
3D Chemical tomography
TXM-‐‑XANES
µ-‐‑XAS
Atomic Particle Electrode Meirer et al., J. Synch. Rad. 18 (2011), 773.
Boesenberg et al., Sci. Rep. In press.
Conclusions • Conceptually, batteries are simple. • In reality, batteries are extremely complicated. Processes
that happen at very length scales can act as limiting. Need a large team to look at all of them! JCESR!
• Bending the cost curve is challenging in both vehicle and grid applications.
• In grid applications, the figure of merit requirements are not clear because specific applications vary (UPS-like to GW scale).
• There are solutions from engineering, chemistry, physics… but it all boils down to two electrodes and an electrolyte!