- This is what the inside

of a lithium-ion battery looks like.

It's not exactly high tech, just two meters of foil

coated in black paste,

all packed into this tiny 45 gram cylinder.

But these are some of the best batteries we have.

They power everything from laptops

and electric vehicles to orbiting satellites.

Yet when a battery fails,

all that energy can get released in the wrong way.

- Oh my God.

- [Reporter] The latest incident

involving a lithium-ion battery.

- So how did something so rudimentary looking

end up in almost every electronic device on the planet?

And why don't we have anything better?

In the early 1980s, most rechargeable batteries

were stuck at just 40 to 60 watt hours per kilogram,

meaning you would need a kilogram of battery

to power a 40 watt light bulb for just an hour.

As a result, when the first commercial

mobile phone launched in 1983, it was pretty unimpressive.

It took 10 hours to charge

for just 30 minutes of talk time.

Laptops, cameras, even medical devices

all suffered from the same bulky batteries.

Everyone from electronics giants

to oil companies were trying to make a better battery,

because they knew that even just doubling

the energy density could unlock

a new era of portable electronics

and power the digital revolution.

But what no one realized

is that someone had already found the solution.

In 1972, a 32-year-old British chemist

named Stanley Whittingham

was studying how different materials store energy

at Exxon's research lab in New Jersey.

Yes, that Exxon, the multinational oil giant,

then the largest oil company in the world.

They were researching batteries.

The next year, war broke out

between Egypt, Syria, and Israel.

When the US backed Israel,

Arab oil producers cut off oil exports in retaliation.

And on December 22nd, the price of crude oil

more than doubled from $5.12 a barrel to 11.65.

In response, President Nixon created policies

to try to keep oil prices down, but they backfired

and the shortage only got worse.

Americans were left queuing for hours at gas stations

as the government introduced a rationing program.

It got so bad that they even dropped

the national speed limit to 55 miles per hour

just to cut consumption.

At Exxon, executives were worried

that supplies would run out entirely,

so they started looking seriously at alternatives,

like electricity.

This wasn't a new idea.

In fact, in 1900 when cars were first taking off,

the top selling car was electric,

ahead of steam and gas powered cars.

But the problem with these electric cars

was their batteries.

They weighed 360 kilograms,

around 40% of the car's weight,

but they could only take you around 60 kilometers.

And the energy density wasn't just low,

it also degraded over time.

Every time you recharged, it got worse.

After fewer than 500 charges,

your range would've dropped to about 40 kilometers.

So by 1924, gas powered cars

outnumbered electric 10,000 to one.

But now that the oil supplies were running out,

it seemed to Exxon that there was no other solution

than to bring back the electric car,

and to do that, they needed a battery

with a much higher energy density.

So suddenly, Whittingham's side project

became a top priority.

Exxon poured in resources, giving him free rein to,

in his words, "Do pretty much what I wanted,

as long as it did not involve petroleum."

The very first battery dates back

to a curious incident in the 1780s

when Italian scientist Luigi Galvani

was dissecting a frog to study its anatomy.

He anchored one side of the frog on a brass hook

and went to cut it open with a steel scalpel.

But when he touched the scalpel to the frog's leg,

he noticed it suddenly twitched,

as if it had come back to life.

Galvani believed he'd discovered

a sort of animal electricity,

a living force produced by the tissue itself.

But Galvani's rival Alessandro Volta disagreed.

He thought it came from the metals themselves.

And you can see this with lots of different materials.

Veritasium producer Gregor set up a version

of this experiment, minus the frog, to test it out.

- [Gregor] I have zinc, magnesium, and iron here.

I can take any of these metals,

stick them into one side of a lemon

and stick some copper on the other side.

If I hook these up to a volt meter,

I should be getting a voltage.

And we got around 0.8 volts.

Now, the reason this happens

is because some elements want to get rid

of their electrons more than others.

So if you pair one that really doesn't want its electrons

with one that really wants some,

well, then the electrons are gonna be traveling across.

- [Narrator] Let's look at the zinc.

What's happening here is that zinc is losing its electrons.

The zinc ions enter the juice,

and the electrons are forced to go through the circuit

to get to the other side.

There, hydrogen ions in the lemon juice

want those electrons,

so they receive them and turn into hydrogen gas.

You've got one side that gives up electrons,

that's the anode, and you've got one

that receives them, that's the cathode.

- But why do you need the lemon at all?

If there's no flow of the positive ions

through to the other side,

the electrons stop moving almost immediately.

This happens because all of the electrons

now get bunched up in the copper,

making it extremely negatively charged,

and that is just gonna push away any more electrons

from coming over to the other side.

- [Derek] That's because electrons

can't travel through lemon juice.

Liquids like this don't have

free electrons the way metals do,

so electrons stay in the wire.

They'll only leave the circuit at the copper side

if there's something in the juice,

like hydrogen ions ready to take them,

and if the reaction releases enough energy

to make that transfer happen.

But positive ions in the juice can move.

They travel across to balance the charge,

allowing the current to keep flowing.

A solution that carries charge this way

by moving ions is called an electrolyte.

- But we could also do this with the other metals

to get a similar reaction,

and we can actually quantify how much

each of these metals wants or doesn't want electrons.

With zinc, we already got around 0.9 volts,

but if you try it with iron, for example,

you get something lower, 0.5 or 0.6 volts.

Now, magnesium is tricky and it would be a bit higher,

but it oxidizes so quickly that even if I scrape

some of the oxide from the surface,

I'm still getting only around 0.7 volts.

The idea is that the larger the voltage on the volt meter,

the more energy each electron has to give

as it passes through the circuit.

But there's also a limit to this.

See, this beaker is full of lemon juice

from the lemons we used earlier,

and they're hooked up using spoons

and these wires to a variable power source.

Now look what happens when I up the voltage.

You'll actually start to see bubbles forming on both spoons,

and that's water in the lemon juice

actually being broken down into oxygen and hydrogen gas.

This already starts happening at 1.23 volts,

and that sets a limit on how much voltage

you can push through this electrolyte.

- Up until the early 1970s,

just about every commercial battery

used a water-based electrolyte, and as a result,

none of these battery cells could push

much beyond the 1.23 volt limit.

Now, the total energy a battery can store

depends on how much energy each charge has to give

times how much charge can move,

that is the battery's voltage times its capacity.

So if you can't increase the voltage,

your only option is to make more battery,

more cells or bigger cells,

but that won't increase the energy density.

And this is exactly the problem

Whittingham was trying to solve.

He was searching for materials

that could store large amounts of energy

in a compact space with light weight.

That led him to a class of compounds

called transition metal dichalcogenides.

He zeroed in on one in particular, titanium disulfide.

Titanium in this compound

has effectively lost four electrons,

two to each sulfur atom,

meaning it sits at a plus four oxidation state.

That leaves it very electron hungry,

exactly what you want in a battery cathode.

But titanium disulfide has a second key advantage,

this material is made of stacked layers

held together by weak Van der Waals forces.

This creates natural gaps between sheets of titanium

and sulfur atoms just wide enough

to let certain ions slip between the layers,

a process known as intercalation.

Better still, the structure can expand

and contract repeatedly without breaking down.

Now Whittingham just had to decide which ions to use.

He initially looked at potassium,

but it was just too reactive

and far too dangerous to work with.

Oh, yeah! (laughs)

- He turned to this,

a soft, silvery metal called lithium.

What makes lithium unique is not the fact

that it has one electron in its outer shell

that it wants to get rid of.

No, that it shares with the other elements in its group.

What sets it apart is how much energy

you can get out of lithium when it reacts in a battery.

See, when it loses that outer electron,

it forms a tiny, incredibly stable positive ion,

and so that reaction paired with the right cathode

releases more energy per electron than any other metal.

That's why it produces the highest voltage

of any metal used in batteries.

And because it's so small with just three protons,

lithium is also the least dense metal,

at just 0.53 grams per cubic centimeter.

This combination of low density and the tendency

to give away its electron made lithium perfect

for Whittingham's vision

of this high energy density battery.

But while lithium was easier to work with than potassium,

easier still didn't mean easy.

I mean, they only let me hold it in this glove box,

and matter of fact, here's what happens

to lithium if you put it in a glass of water.

(water bubbles) (tense music)

Safe to say, you don't want

this happening inside your battery.

- So, Whittingham had to switch out

the water-based electrolyte for something else,

and that change unlocked the possibility of higher voltages.

He turned to a solution of lithium salt

in an organic solvent, and it worked,

but it came with serious risks.

The solvent was volatile,

the lithium salt was chemically unstable.

Together, they formed a mixture that could explode

or release toxic fumes if mishandled.

Everything had to be done with extreme caution.

A stray spark or a trace of moisture

could destroy the experiment or start a fire.

But if you could get around the danger,

this new electrolyte was a huge perk.

It let lithium-ions shuttle

between electrodes without breaking down the solvent

or the cell, at least not until much higher voltages.

Whittingham had unlocked lithium's potential,

and in the process, he'd broken through

the 1.23 volt ceiling.

His new chemistry delivered nearly double,

a huge 2.4 volts per cell.

He now had a working prototype,

a metallic lithium anode on one side,

a titanium disulfide cathode on the other,

his new liquid electrolyte in between.

There was also a thin porous separator

that kept the electrodes apart,

so they couldn't touch and short circuit.

Here's how it works.

When you close the circuit,

lithium atoms at the anode give up their electrons.

Those electrons travel through the external circuit

toward the cathode, generating a current

that powers whatever's connected.

At the same time, the lithium-ions

are released into the electrolyte,

and then they pass through the porous separator

and migrate toward the cathode.

The electrons arriving through the circuit

are taken up by the titanium atoms

and the titanium disulfide.

The positive lithium-ions slide between the layers

to balance out the negative charge of the electrons,

and they become locked in place.

And this process is reversible.

When you apply a voltage to recharge,

the extra electrons are stripped from the titanium

and pulled back to the anode.

The lithium-ions are forced out

of the titanium disulfide layers into the electrolyte,

and they too migrate to the anode

where metallic lithium reforms.

What Whittingham had created here

was a rechargeable battery, one that worked reliably

cycle after cycle with incredible consistency.

I don't normally think about batteries this way,

but what they really are is tiny little contained

chemical reactions.

And in a chemical reaction,

if you could get a 60% yield,

that would be considered good.

But in a battery,

especially one that you wanna recharge 1000 times,

you need that reaction to be say 99.9% efficient,

because if it's not, the capacity of that battery

rapidly deteriorates.

If you have, say, a 95% yield,

then you'd lose a significant fraction

of lithium-ions every cycle.

After just 50 cycles, you'd only have 8%

of your original capacity left.

So that's pretty incredible

that every single lithium-ion

has to leave one electrode, pass through the electrolyte,

and slot neatly into the layered crystal structure

of titanium disulfide.

And then when you recharge it,

they have to leave again cleanly without incident,

without getting stuck, make their way

all the way back to the anode.

Amazingly, despite just being an early prototype,

Whittingham's battery came close to that 99%.

In the winter of 1973,

Exxon's managers summoned Whittingham

to the company's New York office.

Whittingham later said, "I went in there and explained it,

five minutes, 10 minutes at the most,

and within a week they said yes,

they wanted to invest in this."

They got to work at the Exxon laboratory,

but it wasn't all smooth sailing.

Firefighters had to be called out repeatedly.

They were called so often,

they threatened to start charging the lab

for the special chemicals needed

to extinguish the burning lithium.

- The problem was the anode.

Whittingham's design used pure lithium,

which worked brilliantly, until it didn't.

- [Billy] We've made a special cell.

We've made a transparent battery.

- [Gregor] That's so cool.

- But they're very, very small,

so we have a microscope lens

just to allow us to see it.

What you're seeing here is a piece of copper,

which we're gradually plating with lithium.

So this is analogous to the first generation

lithium metal batteries,

which use lithium metal as the anode.

On this side, we have a piece of lithium.

As we charge the battery, we're stripping the lithium

from that electrode and we're plating it.

And actually what's happening right now

is the ideal reaction where it's very slow.

We're getting a dense plate.

The challenge then becomes if we go too fast.

- [Gregor] Oh, that is huge!

- Everything's fine

until all of a sudden it's not fine.

So we want the lithium to plate evenly across everywhere,

but instead, it forms in that one location,

and that is what is a lithium dendrite.

That lithium dendrite can grow.

The length scales of this is on the order of,

you know, millimeters,

so that would've easily short circuited the battery.

- [Gregor] And that dendrite can just keep growing,

and eventually it's gonna poke through the separator

and reach to the other side.

Now the electrons are gonna have a shortcut,

so instead of going through the circuit,

they race straight from the anode

to the cathode using the dendrite,

and that sudden surge of electrons cause intense heating,

and that can trigger a chain reaction inside the battery,

leading to a fire, or even an explosion.

- For all its promise,

Whittingham's battery was just too dangerous,

and then the oil crisis ended.

Prices dropped and Exxon's urgency evaporated.

The company shut down its lithium battery program.

Whittingham published his design in 1976,

and Exxon licensed the patent to a few manufacturers,

but with no funding and no momentum,

the first lithium battery revolution died

before it had a chance to take off.

Fortunately, a copy of Whittingham's paper

made it across the Atlantic

to Oxford University in England,

where it caught the attention of John B. Goodenough,

an American physicist leading a solid state chemistry group.

As he read the paper, one thing stood out,

the cell voltage was being held back.

The material Whittingham chose for the cathode,

titanium disulfide, capped the cell at just 2.4 volts,

but Goodenough believed that

with a better cathode material, he could do better.

He had previously worked

with compounds called transition metal oxides.

They were more stable than sulfides,

and some he knew were extremely hungry for electrons,

perfect for a cathode.

He tried one of these compounds in his battery,

and the voltage immediately spiked

from 2.4 volts to four volts.

This jump was incredible.

But what was even more surprising was the fact

that this compound already had lithium in it.

The material was lithium cobalt oxide.

Lithium cobalt oxide is arranged so that the cobalt

and oxygen atoms form tightly bonded layers,

with lithium-ions nestled in between.

This means that your supply of lithium-ions

doesn't just have to come

from the dangerous lithium metal on the anode side,

it's already there prebuilt into the cathode.

So theoretically, you don't even need lithium metal at all.

You could assemble the cell in a discharged state

with all your lithium-ions in the cathode,

then when you connect it to a charger,

these ions will get expelled

from the cathode crystal lattice and into the electrolyte.

At the same time, nearby cobalt atoms

will give up an electron to balance out the charge,

and those electrons then go through the wire

to the anode to meet with the ions.

If Goodenough could find an anode

that would replace lithium metal,

the battery would become safe enough to leave the lab

and actually power real world devices.

Goodenough was so excited about the potential of his design

that he reached out to battery companies across the US,

the UK and Europe, but incredibly, no one was interested.

So he asked Oxford to file a patent, but they refused.

So he took it to a government lab near Oxford,

the Atomic Energy Research Establishment,

and finally, they agreed to fund the patent,

but only if Goodenough signed away his financial rights.

Seeing no other option, he agreed,

and the lab patented the invention in 1981.

Now, this should have been a gold mine,

but the lab didn't realize what they had.

And so for the second time,

the lithium battery revolution was boxed up and shelved.

This should have been a turning point for battery science,

but bureaucracy and inertia stalled progress.

Every field has its bottlenecks.

For batteries, it was slow moving institutions.

For developers today, it's slow moving code reviews.

And I can relate.

When we make these videos,

especially the ones with simulations

or complex animations, it's rarely the ideas

that slow us down, it is the reviews.

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And now back to Goodenough's design,

a breakthrough with nowhere to go, yet.

While Goodenough's battery design was gathering dust,

10,000 kilometers away in Japan,

a 34-year-old chemist named Akira Yoshino

was trying to find a safer battery anode,

one that didn't require lithium metal.

Yoshino was actually looking at plastic.

Now, normally plastic is an insulator,

but the kind Yoshino was looking at is different.

It's called polyacetylene,

and its carbon atoms are arranged in a repeating chain

of single and double bonds,

a structure that gives it unusual electronic properties.

If you tweak polyacetylene by adding or removing electrons,

electrons can actually move along this carbon chain.

So the plastic conducts electricity like a metal.

And that got Yoshino thinking,

what if polyacetylene could work as a battery anode?

During charging, it could absorb lithium-ions and electrons,

and then during discharge, it would give up those electrons

to the circuit, just like lithium metal does.

If it worked, it could eliminate the most dangerous part

of the battery, the metallic lithium.

But for months, Yoshino struggled.

Obviously, since he removed lithium metal from the anode,

he had to get lithium-ions from somewhere else

and he couldn't figure it out.

And then just as he was losing hope,

on the last workday of 1982 while cleaning out his office,

he stumbled upon a 1980 paper by John B. Goodenough.

It described a cathode made of lithium cobalt oxide,

a cathode that already contained lithium.

This was the missing piece.

He sketched out the reaction between lithium cobalt oxide

and his lithium free anode,

and then built a test cell using the two materials.

It worked safely and reliably,

but Yoshino wasn't satisfied.

The material he used for the anode,

the polyacetylene had an extremely low density.

I mean, it couldn't pack in enough lithium,

so the energy density of the battery was terrible.

Yoshino needed something more lightweight, compact,

conductive, and crucially,

something that could reversibly accept

and release lithium-ions within its structure

without breaking down.

He tested material after material,

and every single one failed,

until a breakthrough came from within his own company.

Another team had developed a new form of carbon

with a unique crystalline structure.

They called it vapor grown carbon fiber.

He got his hands on a sample,

tried it in the lab, and it worked.

To prove it, he placed a test cell

containing metallic lithium into a safety rig,

one that's designed to test explosives.

Then he dropped a heavy iron rod onto it.

It exploded violently.

Then he ran the same test again,

but this time with his new design,

using carbon as the anode.

He charged the cell, placed it in the rig,

and dropped the rod but nothing happened.

The contrast was undeniable.

Later, Yoshino would say,

"That was the moment when the lithium-ion battery was born."

But his employer, Asahi Chemical,

well, they weren't a battery company,

and they didn't know how to make batteries.

So in 1986, Asahi executive Isao Kuribayashi

flew to Boston on a top secret mission,

carrying three jars containing cathode,

anode and electrolyte materials.

He handed them to a tiny firm called Battery Engineering,

working out of a converted truck garage,

and he asked them to turn the materials

into cylindrical cells,

like the kind you might buy for a flashlight.

The team did just that,

completely unaware of what they were handling.

It wasn't until 2020 that employees learned the truth

that they had helped assemble the world's first

pre-production lithium-ion batteries.

Two weeks later, Kuribayashi returned to Japan

with 200 finished perfectly functioning cells.

Even then, Asahi's leadership hesitated.

Kuribayashi refused to give up.

On the 21st of January, 1987,

he visited Sony and he took one of the prototype cells

and rolled it across the conference table to the Sony execs,

and at last, they saw its potential.

They reworked the design,

swapping out Yoshino's carbon material

for graphite that could better intercalate lithium-ions

between its layers.

And in 1991, Sony launched

the first commercial lithium-ion battery

inside this, the Sony Handycam.

Their battery was compact, rechargeable, powerful,

and crucially, free of unstable lithium metal.

It was Sony who first coined the name

lithium-ion and it stuck.

But this wasn't just about one camcorder.

Competing companies like Panasonic

and Sanyo raced to catch up.

Lithium-ion batteries started appearing

in phones, CD players, laptops.

Manufacturers actually began to advertise

the use of lithium-ion batteries

as a key selling point of their products.

- I'm showing my age here.

I joined the industry when lithium-ion cells

were first introduced,

and there was a Sony camcorder that was introduced,

and then there was Dell computer.

And I still remember the ads when Dell computer

introduced their lithium-ion battery,

and they had eight hours of runtime,

so they had an advertisement in a magazine

and it was eight pages long.

Each one was an hour longer, so it was a big deal.

- But what's crazy is that even after all this,

these batteries should never have worked.

See, when you charge the battery for the first time,

lithium-ions move from the cathode to the graphite anode.

And here, they react with the electrolyte

to form this weird complex patchwork of compounds

that build up on the anode's surface.

These parasitic side reactions

should keep going on indefinitely,

using up all the lithium

and destroying the cell but they don't.

Instead they form a thin protective layer

known as the solid electrolyte interface, or SEI.

It's a kind of chemical shield

protecting both the graphite anode

and the electrolyte from further reactions.

But crucially, lithium-ions can still slip through it.

When the SEI originally forms

during the first charging cycle,

around 5% of the lithium in the cell

actually gets stuck in this layer,

decreasing the battery's capacity.

But this little trade off

is what makes the battery stable enough

to be used for years or even decades,

which is why today lithium-ion batteries

are virtually everywhere.

From 1991 to 2023, the price per kilowatt hour

dropped by 99% from nearly $9,000 to just $100.

At the same time, energy density and cycle life,

how many times a battery can be charged

and discharged before it wears out, improved dramatically,

crossing a critical threshold.

Lithium-ion batteries had become powerful enough

and finally cheap enough for something bigger,

the return of the electric car.

Today, lithium-ion powers a $100 billion industry.

In 2019, Whittingham, Goodenough

and Yoshino finally received

the Nobel Prize in chemistry for an invention

that in the committee's words

"Revolutionized our way of life."

This made Goodenough the oldest Nobel laureate in history,

receiving the award at the age of 97.

But lithium-ion isn't perfect.

- Scary moments aboard a JetBlue plane,

a fire erupting after a passenger's backpack

suddenly exploded.

- Every week, inside an airplane,

there is at least one event of a battery,

of a phone, of an iPad or a toy or something

that catches fire.

- What, every week?

- Yeah, every week.

- It's just the latest incident aboard a plane

involving lithium-ion batteries.

- [Reporter] So far this year,

60 onboard battery incidents through early October.

- Every flight in the US has a bag, a specialized bag

with very thick non-flammable materials

where you put the phone inside,

and you close it, and you still have a hazard

and you have to deal with these gases,

but now you have put the fire ignition away

from anything else.

And if it burst into fireworks,

then at least it's in a container.

And then you tell the captain,

"We need to land immediately."

- [Derek] So what is actually happening

when a battery fails like that?

- This is a classic lithium-ion battery,

and today we're gonna do something I always wanted to do.

We're gonna tear one down.

I guess safe to say don't do this at home.

But what would happen if you were to do this

outside of the gloved box?

- If you charged up the cell

and then you tried to tear it up,

then you could accidentally short it,

and then it could burn

and it could even explode or fire.

If you discharged it and you opened it up,

you'd release all the different gases

and really toxic chemicals, and if you inhale those,

then you'd probably end up in hospitals.

So at this point, we have what we call the jelly roll.

So that's a roll off the cathode,

separates that anode.

- [Gregor] Yeah.

- Stuck together with bit of tape.

So Li Ren's just gonna scalpel off the tape,

and then we should be able to unroll it into a nice sheet.

- [Gregor] So these little patches are the electrolyte or?

- Yeah. - Okay.

- [Derek S.] So as time goes by, it'll start evaporating out.

- That is so cool.

It's so obvious when you see it,

but I don't think anyone intuitively thinks

that it's a rolled up like sheet

of anode and cathode inside.

But these layers inside the battery,

they're not gonna stay perfect forever.

Here's an electrode from a new cell

compared to one from an old one.

You can see that the lithium is building up

in all of the wrong places,

and if this sort of degradation gets out of hand,

well, we're about to push the cell

past its breaking point.

How do we blow up a battery?

- So today we've got a prismatic battery.

It's a small battery from sort of a power tool

or a phone or something similar.

We're gonna wrap it in some nichrome wire,

so we pass current through this wire.

Something like 200 watts we pass through-

- That's a lot. - This wire.

Yeah, and it's a significant battery.

We want it to go and we want it

to go pretty spectacularly.

(tense music)

(scientists laughing)

- [Gregor] Good luck, Harry.

What we're simulating here

is a catastrophic battery failure,

the kind that could happen

if a cell is damaged or overheated,

or even just badly manufactured.

It starts around 80 degrees Celsius

when the protective SEI layer

on the anode starts to break down.

It's gonna try to reform,

but these reactions are gonna release more heat,

and if that heat can escape,

the temperature is gonna keep rising.

How close is it to exploding now?

What do you think?

- It should burst very soon. - Seconds.

- [Gregor] At roughly 130 degrees Celsius,

the polymer separator is gonna melt,

and now the anode and cathode can come into direct contact,

and a massive internal short follows.

The cathode itself starts to decompose.

And because transition metal oxides

release oxygen from their crystal structure,

they're gonna fuel the combustion,

and now the fire is just feeding itself.

Oh. - Yes!

- Oh, oh my God.

(dramatic music)

That's really violent.

This is insane, from one small battery like that.

- And it's only 50% state of charge.

- What we call ignition happens

inside the battery, not outside the battery,

and it requires a fuel

or a substance that will undergo a reaction,

it requires an oxidizer

or the equivalent oxidizer and it requires heat.

The battery contains these three inside,

so it has its own equivalent to an oxidizer,

its own equivalent to a fuel

and its own source of heat.

- Yeah. - All of it in one device.

- So it's not actually lithium that burns.

A modern lithium-ion battery

like this one here contains

very little lithium, ironically.

It's actually everything else inside here that's dangerous.

It must be really hard putting out a battery fire

if it really has everything that it needs.

- Yeah, exactly.

So you can still put the blanket

and stop the oxygen from arriving,

but you will not, the fire will not go to zero.

It will still, it will be smaller,

but it will still be there.

And then with water,

yeah, water has the ability to take heat away,

so it is possible to take the heat away

from the battery with water.

The best thing is to put and immerse the battery

into a bath of water.

- Yeah.

- It's brutal.

You can do it with one battery, with 10 batteries,

with 15 batteries,

but when you have very large packs of batteries

with thousands of batteries,

you cannot physically put that under water.

- Yeah, one thing that is popping up recently as a threat

to cities is electric car fires.

- [Guillermo] Well, we know a lot of water works.

- Yeah, well, if there's a water source

nearby, I guess, yeah.

- Yeah, I mean, this is what they do

in some countries around the world.

They have a truck, a specialist truck

full of water, and you just take the car

that has been involved in electric fire

and they dump it into it.

- No way. - Yeah, they do.

But, and actually it works.

- [Derek] So, how dangerous is it really?

- It's very rare.

Every million batteries, there is a fire.

- Okay. - Right.

So that's very safe, that in the standards

of engineering, that's like, oh, you have a good system.

One out of a million, that's fine.

But batteries are everywhere.

We don't even think about it.

So within our lifetimes, we are going to reach a point

where we would have been exposed

to more than a million batteries,

so we would be all of us experiencing

a fire of a battery.

- With billions of batteries in circulation,

even rare failures become inevitable.

Meanwhile, demand is skyrocketing.

By 2030, we're projected to need

over 17 million tons of battery grade materials,

and making lithium-ion batteries comes at a cost.

Lithium only makes up

around 20 parts per million of Earth's crust.

It's expensive and water intensive to extract,

and 70% of cobalt, another key ingredient

in many lithium-ion designs

comes from the Democratic Republic of Congo,

much of it mined under hazardous,

often exploitative conditions.

We need more batteries and we need them fast.

We can't just rely on lithium alone.

- So it's not like lithium's as good as we're gonna get.

Like that we're gonna get much better

batteries in the future.

If our priorities are about

saving the planet from runaway climate change,

we need to have massive scale energy storage system

and electrify almost everything else that we do.

- The hunt is still on for safer batteries,

for cheaper ones, ones that last longer,

charge faster, and ones that store far more energy.

The lithium-ion battery changed the world,

but the future of energy storage

won't be about just conquering one element,

it'll be about mastering many.

(whooshing)