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A battery is a device that converts chemical energy contained within its active materials directly into electric energy by means of an electrochemical oxidation-reduction (redox) reaction. Battery can be defined as an electrochemical device (consisting of one or more electrochemical cells) which can be charged with an electric current and discharged whenever required. Batteries are usually devices that are made up of multiple electrochemical cells that are connected to external inputs and outputs. Batteries are widely employed in order to power small electric devices such as mobile phones, remotes, and flashlights. Historically, the ‘term’ battery has always been used in order to refer to the combination of two or more electrochemical cells. However, the modern definition of the term ‘battery’ is believed to accommodate devices that only feature a single cell.

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Batteries and similar devices accept, store, and release electricity on demand. Batteries use chemistry, in the form of chemical potential, to store energy, just like many other everyday energy sources. For example, logs and oxygen both store energy in their chemical bonds until burning converts some of that chemical energy to heat. Gasoline and oxygen mixtures have stored chemical potential energy until it is converted to mechanical energy in a car engine. Similarly, for batteries to work, electricity must be converted into a chemical potential form before it can be readily stored. Batteries consist of two electrical terminals called the cathode and the anode, separated by a chemical material called an electrolyte. To accept and release energy, a battery is coupled to an external circuit. Electrons move through the circuit, while simultaneously ions (atoms or molecules with an electric charge) move through the electrolyte. In a rechargeable battery, electrons and ions can move either direction through the circuit and electrolyte. When the electrons move from the cathode to the anode, they increase the chemical potential energy, thus charging the battery; when they move the other direction, they convert this chemical potential energy to electricity in the circuit and discharge the battery. During charging or discharging, the oppositely charged ions move inside the battery through the electrolyte to balance the charge of the electrons moving through the external circuit and produce a sustainable, rechargeable system. Once charged, the battery can be disconnected from the circuit to store the chemical potential energy for later use as electricity.

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Battery types

Batteries can be broadly divided into two major types.

Primary Cell / Primary battery

Secondary Cell / Secondary battery

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These are batteries where the redox reactions proceed in only one direction. The reactants in these batteries are consumed after a certain period of time, rendering them dead. A primary battery cannot be used once the chemicals inside it are exhausted.

An example of a primary battery is the dry cell – the household battery that commonly used to power TV remotes, clocks, and other devices. In such cells, a zinc container acts as the anode and a carbon rod acts as the cathode. A powdered mixture of manganese dioxide and carbon is placed around the cathode. The space left in between the container and the rod are filled with a moist paste of ammonium chloride and zinc chloride.

The redox reaction that takes place in these cells is:

At Anode

Zn(s) –> Zn²⁺ (aq) + 2e–

At Cathode

2e– + 2 NH₄⁺ (aq) –> 2 NH3 (g) + H₂ (g)

2 NH3 (g) +Zn²⁺ (aq) –> [Zn (NH₃)₂] 2+ (aq)

H₂ (g) + 2 MnO₂ (S) –> Mn₂O₃ (S) + H₂O (l)

Thus, the overall cell equation is:

Zn(s) + 2 NH₄⁺ (aq) + 2 MnO₂ (S) –> [Zn(NH₃)₂] 2+ (aq) + Mn₂O₃ (S) + H₂O (l)

Another example of the primary cell is the mercury cell, where a zinc-mercury amalgam is used as an anode and carbon is used as a cathode. A paste of HgO is used as an electrolyte. These cells are used only in devices that require a relatively low supply of electric current (such as hearing aids and watches).

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These are batteries that can be recharged after use by passing current through the electrodes in the opposite direction, i.e. from the negative terminal to the positive terminal.

For example, a lead storage battery that is used in automobiles and inverters can be recharged a limited number of times. The lead storage battery consists of a lead anode and the cathode is a lead grid packed with lead dioxide. Sulphuric acid with a concentration of 38% is used as an electrolyte. The oxidation and reduction reaction involved in this process are listed below.

At Anode

Pb –> Pb²⁺+ 2 e–

Pb+ SO₄ 2– –>PbSO₄(electrode) + 2 e–

At Cathode

2 e–+ PbO₂+ 4 H⁺ –> Pb²⁺+ 2 H₂O

2 e–+ PbO₂+ 4 H⁺+ SO₄ ²⁻ –> PbSO₄(electrode) + 2 H₂O

In order to recharge these batteries, the charge is transferred in the opposite direction and the reaction is reversed, thus converting PbSO₄ back to Pb and PbO2.

Another example of the secondary cell is the nickel-cadmium cell. These cells have high storage capacities and their lifespan is relatively long (compared to other secondary cells). However, they are difficult to manufacture and maintain.

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Based on the application of the battery, they can be classified again. They are:

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Based on the application of the battery, they can be classified again. They are:

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Household Batteries

These are the types of batteries which are more likely to be known to the common man. They find uses in a wide range of household appliances (such as torches, clocks, and cameras). These batteries can be further classified into two subcategories:

Rechargeable batteries Nickel
Examples: Cadmium batteries, Lithium-Ion

Non-rechargeable batteries
Examples: Silver oxide, Alkaline & carbon zinc

Industrial Batteries

These batteries are built to serve heavy-duty requirements. Some of their applications include railroad, backup power and more for big companies. Some examples are:
Nickel Iron
Wet Nickel Cadmium (NiCd)

Vehicle Batteries

These are more user-friendly and a less complicated version of the industrial batteries. They are specifically designed to power cars, motorcycles, boats & other vehicles. An important example of a vehicle battery is the lead-acid battery.

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A Battery is a device consisting of one or more electrical cells that convert chemical energy into electrical energy. Every battery is basically a galvanic cell where redox reactions take place between two electrodes which act as the source of the chemical energy.

Battery types

Batteries can be broadly divided into two major types.

Primary Cell / Primary battery

Secondary Cell / Secondary battery

Based on the application of the battery, they can be classified again. They are:

Household Batteries

These are the types of batteries which are more likely to be known to the common man. They find uses in a wide range of household appliances (such as torches, clocks, and cameras). These batteries can be further classified into two subcategories:

Rechargeable batteries Nickel
Examples: Cadmium batteries, Lithium-Ion

Non-rechargeable batteries
Examples: Silver oxide, Alkaline & carbon zinc

Industrial Batteries

These batteries are built to serve heavy-duty requirements. Some of their applications include railroad, backup power and more for big companies. Some examples are:
Nickel Iron
Wet Nickel Cadmium (NiCd)

Vehicle Batteries

These are more user-friendly and a less complicated version of the industrial batteries. They are specifically designed to power cars, motorcycles, boats & other vehicles. An important example of a vehicle battery is the Lead-acid battery.

Primary Cell

These are batteries where the redox reactions proceed in only one direction. The reactants in these batteries are consumed after a certain period of time, rendering them dead. A primary battery cannot be used once the chemicals inside it are exhausted.

An example of a primary battery is the dry cell - the household battery that commonly used to power TV remotes, clocks, and other devices. In such cells, a zinc container acts as the anode and a carbon rod acts as the cathode. A powdered mixture of manganese dioxide and carbon is placed around the cathode. The space left in between the container and the rod are filled with a moist paste of ammonium chloride and zinc chloride.

The redox reaction that takes place in these cells is:
Zn(s) -> Zn²⁺ (aq) + 2e⁻2e- + 2 NH₄⁺ (aq) -> 2 NH3 (g) + H₂ (g)2 NH3 (g) +Zn²⁺ (aq) -> [Zn (NH₃)₂] 2+ (aq)H₂ (g) + 2 MnO₂ (S) -> Mn₂O₃ (S) + H₂O (l)
Thus, the overall cell equation is:
Zn(s) + 2 NH₄⁺ (aq) + 2 MnO₂ (S) -> [Zn(NH₃)₂] 2+ (aq) + Mn₂O₃ (S) + H₂O (l)
Another example of the primary cell is the mercury cell, where a zinc-mercury amalgam is used as an anode and carbon is used as a cathode. A paste of HgO is used as an electrolyte. These cells are used only in devices that require a relatively low supply of electric current (such as hearing aids and watches).

Secondary Cell

These are batteries that can be recharged after use by passing current through the electrodes in the opposite direction, i.e. from the negative terminal to the positive terminal.

For example, a lead storage battery that is used in automobiles and inverters can be recharged a limited number of times. The lead storage battery consists of a lead anode and the cathode is a lead grid packed with lead dioxide. Sulphuric acid with a concentration of 38% is used as an electrolyte. The oxidation and reduction reactions involved in this process are listed below.

In order to recharge these batteries, the charge is transferred in the opposite direction and the reaction is reversed, thus converting PbSO ₄ back to Pb and .

Another example of the secondary cell is the nickel-cadmium cell. These cells have high storage capacities and their lifespan is relatively long (compared to other secondary cells). However, they are difficult to manufacture and maintain.

To learn more about batteries and other related topics, register with BYJU'S and download the App.

Read more:

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Types Of Battery - Different Types of Batteries and Their Uses & Applications

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A Battery is a device consisting of one or more electrical cells that convert chemical energy into electrical energy. Every battery is basically a galvanic cell where redox reactions take place between two electrodes which act as the source of the chemical energy. Batteries can be broadly divided into two major types.

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Batteries and similar devices accept, store, and release electricity on demand. Batteries use chemistry, in the form of chemical potential, to store energy, just like many other everyday energy sources. For example, logs store energy in their chemical bonds until burning converts the energy to heat. Gasoline is stored chemical potential energy until it is converted to mechanical energy in a car engine. Similarly, for batteries to work, electricity must be converted into a chemical potential form before it can be readily stored. Batteries consist of two electrical terminals called the cathode and the anode, separated by a chemical material called an electrolyte. To accept and release energy, a battery is coupled to an external circuit. Electrons move through the circuit, while simultaneously ions (atoms or molecules with an electric charge) move through the electrolyte. In a rechargeable battery, electrons and ions can move either direction through the circuit and electrolyte. When the electrons move from the cathode to the anode, they increase the chemical potential energy, thus charging the battery; when they move the other direction, they convert this chemical potential energy to electricity in the circuit and discharge the battery. During charging or discharging, the oppositely charged ions move inside the battery through the electrolyte to balance the charge of the electrons moving through the external circuit and produce a sustainable, rechargeable system. Once charged, the battery can be disconnected from the circuit to store the chemical potential energy for later use as electricity.

Batteries were invented in 1800, but their chemical processes are complex. Scientists are using new tools to better understand the electrical and chemical processes in batteries to produce a new generation of highly efficient, electrical energy storage. For example, they are developing improved materials for the anodes, cathodes, and electrolytes in batteries. Scientists study processes in rechargeable batteries because they do not completely reverse as the battery is charged and discharged. Over time, the lack of a complete reversal can change the chemistry and structure of battery materials, which can reduce battery performance and safety.

DOE Office of Science & Electrical Energy Storage

Research supported by the DOE Office of Science, Office of Basic Energy Sciences (BES) has yielded significant improvements in electrical energy storage. But we are still far from comprehensive solutions for next-generation energy storage using brand-new materials that can dramatically improve how much energy a battery can store. This storage is critical to integrating renewable energy sources into our electricity supply. Because improving battery technology is essential to the widespread use of plug-in electric vehicles, storage is also key to reducing our dependency on petroleum for transportation.

BES supports research by individual scientists and at multi-disciplinary centers. The largest center is the Joint Center for Energy Storage Research (JCESR), a DOE Energy Innovation Hub. This center studies electrochemical materials and phenomena at the atomic and molecular scale and uses computers to help design new materials. This new knowledge will enable scientists to design energy storage that is safer, lasts longer, charges faster, and has greater capacity. As scientists supported by the BES program achieve new advances in battery science, these advances are used by applied researchers and industry to advance applications in transportation, the electricity grid, communication, and security.

Electrical Energy Storage Facts

The 2019 Nobel Prize in Chemistry was awarded jointly to John B. Goodenough, M. Stanley Whittingham, and Akira Yoshino "for the development of lithium-ion batteries."

The Electrolyte Genome at JCESR has produced a computational database with more than 26,000 molecules that can be used to calculate key electrolyte properties for new, advanced batteries.

Resources and Related Terms
Scientific terms can be confusing. DOE Explains offers straightforward explanations of key words and concepts in fundamental science. It also describes how these concepts apply to the work that the Department of Energy's Office of Science conducts as it helps the United States excel in research across the scientific spectrum.

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Batteries and similar devices accept, store, and release electricity on demand. Batteries use chemistry, in the form of chemical potential, to store energy, just like many other everyday energy sources. For example, logs store energy in their chemical bonds until burning converts the energy to heat.

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Imagine a world without batteries. All those portable devices we're so dependent on would be so limited! We'd only be able to take our laptops and phones as far as the reach of their cables, making that new running app you just downloaded onto your phone fairly useless.

Luckily, we do have batteries. Back in 150 BC in Mesopotamia, the Parthian culture used a device known as the Baghdad battery, made of copper and iron electrodes with vinegar or citric acid. Archaeologists believe these were not actually batteries but were used primarily for religious ceremonies.

The invention of the battery as we know it is credited to the Italian scientist Alessandro Volta, who put together the first battery to prove a point to another Italian scientist, Luigi Galvani. In 1780, Galvani had shown that the legs of frogs hanging on iron or brass hooks would twitch when touched with a probe of some other type of metal. He believed that this was caused by electricity from within the frogs' tissues, and called it 'animal electricity'.

Luigi Galvani found that the legs of frogs suspended on brass hooks would twitch when prodded with a probe made of another type of metal. He thought this response was caused by 'animal electricity' from within the frog. Image source: Luigi Galvani / Wikimedia Commons.

Volta, while initially impressed with Galvani's findings, came to believe that the electric current came from the two different types of metal (the hooks on which the frogs were hanging and the different metal of the probe) and was merely being transmitted through, not from, the frogs' tissues. He experimented with stacks of layers of silver and zinc interspersed with layers of cloth or paper soaked in saltwater, and found that an electric current did in fact flow through a wire applied to both ends of the pile.

Alessandro Volta's battery: a pile of zinc and silver sheets interspersed with cloth or paper soaked in saltwater. Imagine using that to power your phone. Image source: Luigi Chiesa / Wikimedia Commons.

Volta also found that by using different metals in the pile, the amount of voltage could be increased. He described his findings in a letter to Joseph Banks, then president of the Royal Society of London, in 1800. It was a pretty big deal (Napoleon was fairly impressed!) and his invention earned him sustained recognition in the honour of the 'volt' (a measure of electric potential) being named after him.

I myself, joking aside, am amazed how my old and new discoveries of ... pure and simple electricity caused by the contact of metals, could have produced so much excitement. Alessandro Volta

So what exactly was happening with those layers of zinc and silver, and indeed, the twitching frogs' legs?

The chemistry of a battery

A battery is a device that stores chemical energy, and converts it to electricity. This is known as electrochemistry and the system that underpins a battery is called an electrochemical cell. A battery can be made up of one or several (like in Volta's original pile) electrochemical cells. Each electrochemical cell consists of two electrodes separated by an electrolyte.

So where does an electrochemical cell get its electricity from? To answer this question, we need to know what electricity is. Most simply, electricity is a type of energy produced by the flow of electrons. In an electrochemical cell, electrons are produced by a chemical reaction that happens at one electrode (more about electrodes below!) and then they flow over to the other electrode where they are used up. To understand this properly, we need to have a closer look at the cell's components, and how they are put together.

Electrodes

To produce a flow of electrons, you need to have somewhere for the electrons to flow from, and somewhere for the electrons to flow to. These are the cell's electrodes. The electrons flow from one electrode called the anode (or negative electrode) to another electrode called the cathode (the positive electrode). These are generally different types of metals or other chemical compounds.

In Volta's pile, the anode was the zinc, from which electrons flowed through the wire (when connected) to the silver, which was the battery's cathode. He stacked lots of these cells together to make the total pile and crank up the voltage.

But where does the anode get all these electrons from in the first place? And why are they so happy to be sent off on their merry way over to the cathode? It all comes down to the chemistry that's going on inside the cell.

There are a couple of chemical reactions going on that we need to understand. At the anode, the electrode reacts with the electrolyte in a reaction that produces electrons. These electrons accumulate at the anode. Meanwhile, at the cathode, another chemical reaction occurs simultaneously that enables that electrode to accept electrons.

The technical chemical term for a reaction that involves the exchange of electrons is a reduction-oxidation reaction, more commonly called a redox reaction. The entire reaction can be split into two half-reactions, and in the case of an electrochemical cell, one half-reaction occurs at the anode, the other at the cathode. Reduction is the gain of electrons, and is what occurs at the cathode; we say that the cathode is reduced during the reaction. Oxidation is the loss of electrons, so we say that the anode is oxidised.

Each of these reactions has a particular standard potential. Think of this characteristic as the reaction's ability/efficiency to either produce or suck up electrons-its strength in an electron tug-of-war.

Any two conducting materials that have reactions with different standard potentials can form an electrochemical cell, because the stronger one will be able to take electrons from the weaker one. But the ideal choice for an anode would be a material that produces a reaction with a significantly lower (more negative) standard potential than the material you choose for your cathode. What we end up with is electrons being attracted to the cathode from the anode (and the anode not trying to fight very much), and when provided with an easy pathway to get there-a conducting wire-we can harness their energy to provide electrical power to our torch, phone, or whatever.

The difference in standard potential between the electrodes kind of equates to the force with which electrons will travel between the two electrodes. This is known as the cell's overall electrochemical potential, and it determines the cell's voltage. The greater the difference, the greater the electrochemical potential, and the higher the voltage.

To increase a battery's voltage, we've got two options. We could choose different materials for our electrodes, ones that will give the cell a greater electrochemical potential. Or, we can stack several cells together. When the cells are combined in a particular way (in series), it has an additive effect on the battery's voltage. Essentially, the force at which the electrons move through the battery can be seen as the total force as it moves from the anode of the first cell all the way through however many cells the battery contains to the cathode of the final cell.

When cells are combined in another way (in parallel) it increases the battery's possible current, which can be thought of as the total number of electrons flowing through the cells, but not its voltage.

Electrolyte

But the electrodes are just part of the battery. Remember Volta's bits of paper soaked in salty water? The salty water was the electrolyte, another crucial part of the picture. An electrolyte can be a liquid, gel or a solid substance, but it must be able to allow the movement of charged ions.

Electrons have a negative charge, and as we're sending the flow of negative electrons around through our circuit, we need a way to balance that charge movement. The electrolyte provides a medium through which charge-balancing positive ions can flow.

As the chemical reaction at the anode produces electrons, to maintain a neutral charge balance on the electrode, a matching amount of positively charged ions are also produced. These don't go down the external wire (that's for electrons only!) but are released into the electrolyte.

At the same time, the cathode must also balance the negative charge of the electrons it receives, so the reaction that occurs here must pull in positively charged ions from the electrolyte (alternatively, it may also release negative charged ions from the electrode into the electrolyte).

So, while the external wire provides the pathway for the flow of negatively charged electrons, the electrolyte provides the pathway for the transfer of positively charged ions to balance the negative flow. This flow of positively charged ions is just as important as the electrons that provide the electric current in the external circuit we use to power our devices. The charge balancing role they perform is necessary to keep the entire reaction running.

Now, if all the ions released into the electrolyte were allowed to move completely freely through the electrolyte, they would end up coating the surfaces of the electrodes and clog the whole system up. So the cell generally has some sort of barrier to prevent this from happening.

When the battery is being used, we have a situation where there is a continuous flow of electrons (through the external circuit) and positively charged ions (through the electrolyte). If this continuous flow is halted-if the circuit is open, like when your torch is turned off-the flow of electrons is halted. The charges will pile/build up and the chemical reactions driving the battery will stop.

As the battery is used, and the reactions at both electrodes chug along, new chemical products are made. These reaction products can create a kind of resistance that can prevent the reaction from continuing with the same efficiency. When this resistance becomes too great, the reaction slows down. The electron tug-of-war between the cathode and anode also loses its strength and the electrons stop flowing. The battery slowly goes flat.

Recharging a battery

Some common batteries are single use only (known as primary or disposable batteries). The trip the electrons take from the anode over to the cathode is one-way. Either their electrodes become depleted as they release their positive or negative ions into the electrolyte, or the build-up of reaction products on the electrodes prevents the reaction from continuing, and it's done and dusted. The battery ends up in the bin (or hopefully the recycling, but that's a whole other Nova topic).

But. The nifty thing about that flow of ions and electrons as it takes place in some types of batteries that have appropriate electrode materials, is that it can also go backwards, taking our battery back to its starting point and giving it a whole new lease on life. Just as batteries transformed the way we've been able to use various electrical devices, rechargeable batteries have further transformed those devices' utility and lifespans.

When we connect an almost flat battery to an external electricity source, and send energy back in to the battery, it reverses the chemical reaction that occurred during discharge. This sends the positive ions released from the anode into the electrolyte back to the anode, and the electrons that the cathode took in also back to the anode. The return of both the positive ions and electrons back into the anode primes the system so it's ready to run again: your battery is recharged.

The process isn't perfect, however. The replacement of the negative and positive ions from the electrolyte back on to the relevant electrode as the battery is recharged isn't as neat or as nicely structured as the electrode was in the first place. Each charge cycle degrades the electrodes just a little bit more, meaning the battery loses performance over time, which is why even rechargeable batteries don't keep on working forever.

Over the course of several charge and discharge cycles, the shape of the battery's crystals becomes less ordered. This is exacerbated when a battery is discharged/recharged at a high rate-for example, if you drive your electric car in big bursts of speed rather than steadily. High-rate cycling leads to the crystal structure becoming more disordered, with a less efficient battery as a result.

Memory effect and self discharge

The almost-but-not-quite completely reversible discharge and recharge reactions also contribute to something called the 'memory effect'. When you recharge some types of rechargeable batteries without sufficiently discharging them first, they 'remember' where they were up to in earlier discharge cycles and don't recharge properly.

In some cells, it is caused by the way the metal and the electrolyte react to form a salt (and the way that salt then dissolves again and metal is replaced on the electrodes when you recharge it). We want our cells to have nice, uniform, small crystals of salt coating a perfect metal surface, but that's not what we get in the real world! The way some crystals form is very complex, and the way some metals deposit during recharge is also surprisingly complex, which is why some battery types have a bigger memory effect than others. The imperfections mainly depend on the charge state of the battery to start with, the temperature, charge voltage and charging current. Over time, the imperfections in one charge cycle can cause the same in the next charge cycle, and so on, and our battery picks up some bad memories. The memory effect is strong for some types of cells, such as nickel-based batteries. Other types, like lithium-ion, don't suffer from this problem.

Another aspect of rechargeable batteries is that the chemistry that makes them rechargeable also means they have a higher tendency towards self-discharge. This is when internal reactions occur within the battery cell even when the electrodes are not connected via the external circuit. This results in the cell losing some of its chemical energy over time. A high self-discharge rate seriously limits the life of the battery-and makes them die during storage.

The lithium-ion batteries in our mobile phones have a pretty good self-discharge rate of around 2-3 per cent per month, and our lead-acid car batteries are also pretty reasonable-they tend to lose 4-6 per cent per month. Nickel-based batteries lose around 10-15 per cent of their charge per month, which is not very good if you plan to store a torch for a whole season when you don't need it! A non-rechargeable alkaline battery only loses around 2-3 per cent of its charge per year.

Voltage, current, power, capacity ... what's the difference?

All these words basically describe the strength of a battery, right? Well, sort of. But they're all subtly different.

Voltage = force at which the reaction driving the battery pushes electrons through the cell. This is also known as electrical potential, and depends on the difference in potential between the reactions that occur at each of the electrodes, that is, how strongly the cathode will pull the electrons (through the circuit) from the anode. The higher the voltage, the more work the same number of electrons can do.

Current = the number of electrons that happen to be passing through any one point of a circuit at a given time. The higher the current, the more work it can do at the same voltage. Within the cell, you can also think of current as the number of ions moving through the electrolyte, times the charge of those ions.

Power = voltage x current. The higher the power, the quicker the rate at which a battery can do work-this relationship shows how voltage and current are both important for working out what a battery is suitable for.

Capacity = the power of the battery as a function of time, which is used to describe the length of time a battery will be able to power a device for. A high-capacity battery will be able to keep going for a longer period before going flat/running out of current. Some batteries have a sad little quirk-if you try and draw too much from them too quickly, the chemical reactions involved can't keep up and the capacity is less! So, we always have to be careful when we talk about battery capacity and remember what the battery is going to be used for.

Another popular term is 'energy density'. This is the amount of energy a device can hold per unit volume, in other words, how much bang you get for your buck in terms of power vs. size. With a battery, generally the higher the energy density the better, as it means the battery can be smaller and more compact, which is always a plus when you need it to power something you want to keep in your pocket. It's even a plus for electric cars-the battery has to fit in the car somehow!

For some applications, such as storing electricity at a renewable power plant like a wind or solar farm, a high energy density isn't so much of a problem, as they will most likely have ample space to store the batteries. The main goal for this use would be to simply store as much electricity as possible, as safely and cheaply as possible.

Why so many types?

A range of materials (it used to be just metals) can be used as the electrodes in a battery. Over the years, many, many different combinations have been tried out, but there are only a few that have really gone the distance. But why use different combinations of metals anyway? If you've got a pair of metals that work well together as electrodes, why bother messing around with others?

Different materials have different electrochemical properties, and so they produce different results when you put them together in a battery cell. For example, some combinations will produce a high voltage, very quickly, but then drop off rapidly, unable to sustain that voltage for long. This is good if you need to produce, say, a sudden flash of light like a camera flash.

Other combinations will only produce a trickle of current, but they'll keep that trickle going for ages. We don't need a huge amount of current to power a smoke detector, for example, but we do want our smoke detectors to keep going for a long time.

Another reason to use different combinations of metals is that often two or more battery cells need to be stacked to obtain the required voltage, and it turns out that some electrode combinations stack together much more happily than other combinations. For example, the lithium iron phosphate batteries (a type of lithium-ion battery) used in electric cars stack together to make high voltage systems (100 or even more volts), but you'd never do that with those NiCad Walkman batteries that get hot!

Our different needs over time have led to the development of a huge array of battery types. To read more about them, and what the future holds for battery power, check out our other Nova topics.

This topic is part of our four-part series on batteries. For further reading see types of batteries, lithium-ion batteries and batteries of the future.

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Imagine a world without batteries. All those portable devices we're so dependent on would be so limited! We'd only be able to take our laptops and phones as far as the reach of their cables, making that new running app you just downloaded onto your phone fairly useless.

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An appropriate reduction electrode and an oxidation electrode are combined to create a galvanic cell, which uses a redox process to transform chemical energy into electrical energy. Through a porous diaphragm or a salt bridge, two electrolytic solutions, in which electrodes are submerged, are connected to one another. A device that makes use of the electrical energy generated in the outer circuit is linked to the two electrodes.

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At the oxidation electrode, oxidation takes place. A negative potential is produced by the accumulation of these electrons on the electrode. Due to the reduction process taking place there, a positive potential forms at the reduction electrode. Due to a difference in potential between these two electrodes when they are linked, electrons begin to flow from the oxidation electrode to the reduction electrode in the outer circuit. As a result, an electric current is generated.

The electrode where oxidation takes place is referred to as the anode, while the electrode where reduction occurs is referred to as the cathode. The cathode and anode in a galvanic cell each have a positive and negative polarity.

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1. Electrodes: a combined name given to anode and cathode where oxidation and reduction take place respectively.

2. Electrolyte: aqueous solution of compounds that help the movement of ions.

3. Salt bridge: A concentrated solution of an inert electrolyte is contained in a U-shaped tube known as a salt bridge. Examples of electrolytes are KCl,KNO₃,K₂SO₄ etc., or solidified solution of such an electrolyte in Agar-Agar and gelatin. These inert electrolytes do not take part in the reduction reaction. The function of the salt bridge is to allow the movement of ions from one solution to the other without mixing two solutions. Thus, electron flow in the outer circuit in the wire and the inner circuit are completed by the flow of ions from one cell to the other through the salt bridge. The salt bridge maintains the electrical neutrality of the solution in the two half-cells.

4. Voltmeter: A device used to measure voltage in the closed circuit.

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They are commonly used as a source of electrical power, such as in batteries.

They can also be used in electroplating, where one metal is coated with another metal using an electric current.

Galvanic cells are used in certain types of medical devices, such as heart pacemakers.

They are also used in water treatment systems to control the acidity of water.

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Galvanic Cell- Overview, Definition, Diagram, Example, FAQs

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Galvanic Cell: Read and learn about Galvanic Cell overview, meaning,diagram, examples and working concept of the cell, summarized notes and FAQs in detail.