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Sources

  • Energizer. (2012). Retrieved from http://www.energizer.com/learning-center/pages/how-batteries-work.aspx
  • BASF. (2013). Retrieved from http://www.basf.com/group/corporate/en/innovations/global-r-d-network/research-areas/video-lithium-ion-battery
  • Bui, M. (2010). Electrochemistry basics. Retrieved from http://chemwiki.ucdavis.edu/Analytical_Chemistry/Electrochemistry/Basics_of_Electrochemistry
  • Boundless. (n.d.). The lithium-ion battery. Retrieved from https://www.boundless.com/chemistry/electrochemistry/batteries/the-lithium-ion-battery/
  • Tro, N. J. (2011). Introductory chemistry. (4 ed., pp. 593-600). Boston: Pearson.

A crash course on

Lithium-ion batteries

Li-ion battery

Single cell

The graphic below illustrates how Li-ions are transferred through a battery cell, creating power for the device it serves

Single cell

Single lithium-ion cell

Single cell

Aluminum conductor (Al)

Once the lithium ions have been transferred from the carbon anode to the lithium-oxide cathode, the aluminum conductor transfers the energy of that reaction to the device it powers.

ENERGY

(Al conductor)

ENERGY

Single cell

Li atoms lose their +1

charge during the reaction

Li

Lithium Oxide cathode (LiCoO2)

Li

The transfer of the Li-ions to the cathode generates power, until the Li-ions run out.

ENERGY

Li

(cathode)

Li+

Once most of the Li ions have developed

a neutral charge (picked up one electron), the battery's on-board computer will turn the battery off and require the user to recharge.

Non-aqueous electrolyte (lithium salts)

A Li-ion battery is composed

of 6 layers. These layers work

together to charge and

discharge the battery.

Single lithium-ion cell

Single cell

ENERGY

Li+

During discharge, the lithium-ions utilize the electrolyte layer to transfer toward the separator. The separator prevents a flood of Li+ ion transfer, which could cause excessive heat or fire.

(separator)

Li+

During a recharge, the entire process is reversed, beginning at the cathode and ending at the anode, with the lithium atoms losing one electron, developing a positive charge.

Micro-perforated separator layer

Li+

(non-aqueous electrolyte solution)

Li+

Single cell

Li+

Carbon anode (C)

Li+

(anode)

Copper conductor (Cu)

A charged Li-ion battery has most of it's Li-ions stored in the anode (the negatively charged end of the battery). When a circuit is created between the aluminum and copper ends of the battery, Li-ions begin to make their way to the positively charged lithium oxide cathode.

Single cell

(Cu conductor)

Single lithium-ion cell

Single cell

Lithium-ion (Li-ion) batteries are the most commonly used power source for portable devices today; most new cell phones and laptops come equipped with a Li-ion battery. Previously, the nickel-cadmium (NiCd) battery was the cutting edge battery for portable devices, however the Li-ion battery boasts nearly 2x the energy capacity of the NiCd (3 volt/cell compared to 1.7 volt/cell with NiCd), making it a clear choice for devices such as phones and cars.

The lithium-ion battery is composed

of a series of cells, surrounded by a

sheath of metal, typically aluminum.

A cell is a space in which the chemical

reactions that create power occur.

Single lithium-ion cell

Electrochemical reaction

In a battery, the reactants of a redox reaction are physically separated, and the electrons are transferred through a wire or circuit creating electrical current.

Breaking it down further:

Lithium cobalt oxide

cathode

moles Lithium ion

electron charge

moles of Lithium ion

graphite (carbon)

moles of lithium bonded to carbon

(anode)

In a rechargeable battery, such as a Li-ion battery, this reaction is reversed when an external source (commonly a wall outlet) provides the electrons to reset the reaction.

The reaction

Positive electrode half-reaction (DISCHARGING):

Negative electrode half-reaction (CHARGING):

*when both half-reactions are combined, the equation is balanced

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