Otis Singleton
Electric batteries are a source of electric power, consisting of one or more electrochemical cells with external connections that power electrical devices. They are divided into two groups: primary batteries, which are designed to be used until they no longer have enough voltage to operate a device and are then discarded, and secondary batteries, which can be recharged. The capacity of a battery refers to the amount of electric charge it can deliver, and batteries with higher energy density are generally better as they can be more compact. Electric batteries are used in a wide range of applications, from small electric watches to large power grids, and they play a crucial role in electric vehicles (EVs) and the transition to a more sustainable economy.
Characteristics and Values of Electric Batteries:
| Characteristics | Values |
|---|---|
| Definition | A source of electric power consisting of one or more electrochemical cells with external connections for powering electrical devices. |
| Types | Primary (single-use) and Secondary (rechargeable) |
| Composition | Electrodes, Electrolyte, Anode, Cathode |
| Capacity | The amount of electric charge it can deliver at a voltage that does not drop below the specified terminal voltage. |
| Energy Density | The amount of energy a device can hold per unit volume. |
| Self-Discharge | The rate at which a battery loses its charge when not in use, due to internal chemical reactions. |
| Lifespan | The number of charge/discharge cycles possible before the cells fail to operate satisfactorily. |
| Environmental Impact | The extraction process of lithium and cobalt for batteries can cause environmental damage and health issues for nearby people and animals. |
| Applications | Electric vehicles, renewable energy storage, mobile phones, lamps, watches, etc. |
| Advancements | Faster charging, longer-lasting, safer, and higher-capacity batteries are being developed. |
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What You'll Learn
Electric batteries are a source of electric power
The history of electric batteries dates back to 1749 when Benjamin Franklin first used the term "battery" in his experiments with electricity. However, it was Italian physicist Alessandro Volta who built the first electrochemical battery, the voltaic pile, in 1800. This battery consisted of a stack of copper and zinc plates separated by brine-soaked paper disks, which could produce a steady current. The term "battery" originally referred to a device composed of multiple cells, but now includes devices with a single cell.
Primary batteries, also known as single-use or disposable batteries, are used once and discarded as the electrode materials are irreversibly changed during discharge. Examples include alkaline batteries used in flashlights and portable electronic devices. On the other hand, secondary batteries, or rechargeable batteries, can be discharged and recharged multiple times using an applied electric current. Lead-acid batteries used in vehicles and lithium-ion batteries used in portable electronics are examples of secondary batteries.
Electric batteries have a wide range of applications, from powering small electronic devices such as watches and hearing aids to providing propulsion for electric vehicles and stabilizing electrical grids. Electric vehicles, or BEVs (Battery Electric Vehicles), rely solely on electricity from onboard battery packs to power their motors. This technology has environmental benefits, as it can reduce city pollution and dependence on fossil fuels. However, the manufacturing and disposal of electric vehicle batteries can have negative environmental impacts, particularly regarding the extraction of materials such as lithium and cobalt.
The performance and lifespan of electric batteries are influenced by various factors, including temperature, charge and discharge rates, and the number of charge cycles. At lower temperatures, the available capacity of batteries decreases, and some batteries can be damaged by freezing. Additionally, high-rate charging and discharging can lead to a disordered crystal structure, resulting in reduced battery efficiency.
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They consist of electrochemical cells
An electric battery is a source of electric power that consists of one or more electrochemical cells with external connections for powering electrical devices. Electrochemical cells are devices that convert chemical energy into electrical energy or vice versa.
Electrochemical cells are made up of two half-cells, each consisting of an electrode dipped in an electrolyte. The half-cells are connected by a salt bridge, which allows for ionic contact between them without the two solutions mixing. One of the half-cells loses electrons through oxidation, while the other gains electrons through a reduction process. This process is called a redox reaction.
The two primary types of electrochemical cells are galvanic cells and electrolytic cells. A galvanic cell, also known as a voltaic cell, generates electrical energy from spontaneous redox reactions. It consists of two different metals connected by a wire, with each metal in a separate solution. A salt bridge or porous membrane connects the two solutions, allowing the reaction to occur until equilibrium is reached.
Electrolytic cells, on the other hand, are electrochemical cells in which applied electrical energy drives a non-spontaneous redox reaction. They are often used to decompose chemical compounds through electrolysis, such as decomposing water into hydrogen and oxygen.
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They can be primary or secondary
Electric batteries are devices that consist of one or more electrochemical cells with external connections that power electrical devices. They can be primary or secondary.
Primary batteries, also known as disposable batteries, are designed to be used once until they are depleted and then discarded. They cannot be recharged once exhausted. Common examples include alkaline batteries like AA and AAA batteries, which are widely used in remote controls, smart meters, and smoke detectors. Primary batteries are ideal for devices that need reliable power for a long period but use little energy over time. They are cheaper to produce and purchase but can be more expensive in the long run due to the need for frequent replacements.
Secondary batteries, on the other hand, are rechargeable batteries that can be used, depleted, and then recharged repeatedly through an applied external electrical current. Examples include lithium-ion batteries found in smartphones and laptops, as well as lead-acid batteries used in automotive applications. The electrochemical reactions in secondary batteries are reversible, and the chemical reactants can be restored by running a charging current into the battery. They are more costly to purchase but more economical to use over time. Secondary batteries are more suited for applications where high power and frequent recharging are feasible and economical, such as mobile phones, laptops, electric vehicles, and renewable energy storage systems.
The choice between primary and secondary batteries depends on the specific needs of the application, including cost, energy requirements, lifespan, and environmental impact. While primary batteries are suitable for low-power, long-term use in inaccessible devices, secondary batteries are key to supporting high-energy applications where recharging is more practical.
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They can be recharged by applying direct current
Electric batteries are a source of electric power consisting of one or more electrochemical cells with external connections for powering electrical devices. They are used in a wide range of applications, from small devices like electric watches to large systems like electric grids and vehicles.
Rechargeable batteries, also known as secondary cells, can be recharged by applying direct current (DC) using a DC power supply. This process involves adjusting the voltage and current to the appropriate levels specified by the battery manufacturer. The battery holder plays a crucial role in this setup, providing two leads (one negative and one positive) that facilitate the connection to the DC power supply via alligator clips.
When recharging a battery, it is essential to follow safety precautions and refer to the manufacturer's instructions. The first step is to ensure that no current is flowing through the battery before connecting the charger. Next, connect the positive lead from the charger to the positive terminal of the battery, typically marked with a "+" or a red colour. Similarly, connect the negative lead to the negative terminal, usually marked with a "-" or a black colour.
The duration of the recharging process can vary depending on the battery type and charger settings. Some chargers offer different modes, such as "jumpstart" or "quick charge," which can provide a faster recharge in as little as 15 minutes. However, a full recharge can take several hours or even overnight. It is important to monitor the charging process and shut off the charger when the battery is fully charged to avoid overcharging.
It is worth noting that the performance of rechargeable batteries tends to degrade over time due to the gradual disordering of the battery's crystal structure. This phenomenon, known as the "memory effect," results in a loss of performance and an increased tendency for self-discharge. Despite these limitations, rechargeable batteries remain a crucial component of modern technology, powering everything from mobile phones to electric vehicles.
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They are used in electric vehicles
Electric vehicles (EVs) use batteries to store and deliver electricity, powering one or more electric traction motors on which the vehicle relies for propulsion. They are a clean, quiet, and smooth alternative to traditional combustion engines. The most common type of battery used in EVs is the lithium-ion battery, which offers a high power-to-weight ratio, high energy efficiency, good high-temperature performance, and a long life.
The capacity of a battery refers to the amount of electric charge it can deliver at a voltage that does not drop below the specified terminal voltage. The more electrode material contained in the cell, the greater its capacity. The rated capacity of a battery is usually expressed as the product of 20 hours multiplied by the current that a new battery can consistently supply for 20 hours at 20 °C (68 °F), while remaining above a specified terminal voltage per cell.
The lithium-ion battery has variants, including Li-NMC, LFP, and Li-NCA, which dominate the EV market. LFP batteries, in particular, reached a 41% global market share by capacity for BEVs in 2023. They are heavier but cheaper and more sustainable than other options. Sodium-ion batteries are also becoming more popular due to their affordability, safety, and similar power delivery characteristics to lithium-ion batteries.
In addition to lithium-ion and sodium-ion batteries, other types of batteries used in EVs include lead-acid batteries, nickel-metal hydride batteries, and Zebra batteries. Lead-acid batteries were more commonly used in early modern EVs, such as the 1996 EV1, but their low specific energy, poor cold-temperature performance, and short calendar and lifecycle impede their use in newer models. Nickel-metal hydride batteries are considered a mature technology but are less efficient in charging and discharging than lead-acid batteries. Zebra batteries use a molten sodium chloroaluminate (NaAlCl4) salt as the electrolyte, providing a specific energy of 120 W·h/kg. However, they have poor specific power and require heating the electrolyte to high temperatures, wasting energy and presenting potential hazards.
The type of battery used in an EV will depend on various factors, including the vehicle's size, performance, and cost. As EV technology continues to evolve, we can expect advancements in battery technology, such as solid-state batteries and lithium-sulfur batteries, to further improve the performance and sustainability of electric vehicles.
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Frequently asked questions
An electric battery is a source of electric power consisting of one or more electrochemical cells with external connections for powering electrical devices.
When a battery is supplying power, its positive terminal is the cathode and its negative terminal is the anode. The terminal marked negative is the source of electrons. When a battery is connected to an external electric load, those negatively charged electrons flow through the circuit and reach the positive terminal, thus causing a redox reaction by attracting positively charged ions, or cations. Thus, higher energy reactants are converted to lower energy products, and the free-energy difference is delivered to the external circuit as electrical energy.
Electric batteries are used in a wide range of applications, from small, everyday items such as watches and torches, to larger applications such as cars, buses, trucks, boats, and even stabilising an electrical grid and powering submarines.
