How do Lithium-ion Batteries Work? ||الليثيوم||البطاريات| nasıl||||| ||||batteries| ||litij||| Wie funktionieren Lithium-Ionen-Batterien? ¿Cómo funcionan las baterías de iones de litio? Comment fonctionnent les batteries au lithium-ion ? Come funzionano le batterie agli ioni di litio? リチウムイオン電池はどのように機能しますか? 리튬 이온 배터리는 어떻게 작동하나요? Kaip veikia ličio jonų baterijos? Jak działają baterie litowo-jonowe? Como funcionam as baterias de íons de lítio? Как работают литий-ионные аккумуляторы? Lityum-iyon Piller Nasıl Çalışır? Як працюють літій-іонні акумулятори? 锂离子电池如何工作？ 鋰離子電池如何工作？

Exploring Lithium-Ion Batteries: How they work, Recharge, and Degrade by: Branch Education |||||||||||branche| keşfetmek|||||||||||| |||||||Aufladen||||| |||||||||저하|||브랜치 교육 ||||||funzionano|||||| |||||||||Suirti||| استكشاف|||||||||||| 리튬 이온 배터리 살펴보기: 리튬 이온 배터리의 작동, 충전 및 분해 방법 작성자: 지사 교육

It's crazy every second you use your smartphone, there's a chemical reaction, |beprotiška|||||||||| ||||||||||substance| |||||쓰다|||||| 스마트폰을 사용하는 매 순간 화학 반응이 일어나고 있습니다, like a baking soda volcano happening inside of it. ||cuisson|||||| 처럼||베이킹||||안쪽|| ||||kaip ugnikalnis su soda|||| 베이킹소다 화산이 폭발하는 것처럼 말이죠.

It looks like a solid device without many moving parts, but its true! ||||tvirtas|||||||| Inside the battery there's chemical a reaction that is continuously running and without it, ||||||реакция|||||и|| |||||||that|||||| 안에||||||||||||| your phone would just be dead, which is something we're all familiar with. |||||||||우리는||| 우리 모두 익히 알고 있는 것처럼 휴대폰은 그냥 죽어버릴 것입니다. Let's investigate this lithium-ion battery. How does it power your smartphone, |дослідити||||||||||

what happens when you recharge it, and probably what we're all wonder |||||||||||نتساءل |||||||||||preguntamos o que||||||||||| Why does your battery die earlier and earlier in the day? |||||더 일찍||더 일찍||| To answer these questions, let's open up this battery and look inside. So first, how does your battery power your smartphone? Let's start from what we know.

All batteries have a positive terminal and a negative terminal |||||gnybtas|||| and supply power or electricity to our portable devices. |tiekia||||||| |fournir||||||| So, Electricity is essentially a flow of electrons and in our smartphone. |||본질적으로|||||||| 따라서 전기는 본질적으로 전자의 흐름이며 스마트폰에서도 마찬가지입니다. Electrons which are negatively charged flow from the negative terminal |||부정적으로|전하를 띤||||| |||||流れる|||| 음전하를 띤 전자는 음극 단자에서 흐릅니다.

and run things like the speakers or the display and then end up at the positive terminal. |||||스피커|||디스플레이|||||||| 스피커나 디스플레이와 같은 장치를 실행한 다음 양극 단자에 연결합니다. So then, where does this flow of electrons come from? ||어디||||||| 그렇다면 이 전자의 흐름은 어디에서 오는 것일까요?

Well, this is a lithium ion battery, so the electrons come from the element lithium. At the negative terminal, which is technically called the anode, |||||||||anode |||||||||陽極

lithium is stored between layers of carbon graphite, similar to the graphite in your pencil. ||||sluoksniai|||||||||| Graphite has a nifty crystal structure of layered planes |||pratique||||| |||šmaikštus||||| ||||||||면 グラファイト|||||||| 흑연은 층층이 쌓인 멋진 결정 구조를 가지고 있습니다.

that allows for the lithium to be wedged in between each of the layers. |||||||įspraustas|||||| |||||||끼어들다|||||| |||||||coincé|||||| The technical term for this is intercalation. ||||||삽입 ||||||挿入

Graphite functions as kind-of-like a stable storage space for lithium atoms. جرافيت|||||||||||| Ok- Moving on, one inherent property of the element lithium is that it doesn't like it's outer-most electron, ||||įgimtas|||||||||||||| ||||||||||||||||||전자 ||||固有の|||||||||||||| |||||властивість|||||||||||||

and it wants to give it up.

When there is an available path from the negative terminal to the positive terminal,

this electron separates from the lithium and starts heading to the other side. ||분리한다|||||||||| At the same time, the lithium leaves the graphite,

and becomes positively or +1 charged and is now called a lithium ion.

FYI- an ion is just fancy word for an atom |||||멋진|||| 참고로 이온은 원자의 멋진 단어일 뿐입니다.

who has lost or gained an electron, and thus is charged. ||||||||||전하를 띤

When a lot of lithium atoms leave the graphite at the same time, ||||||||||||같은 시간 많은 리튬 원자가 동시에 흑연을 떠나는 경우, a flow of electrons is built up. |||||형성된다| 전자의 흐름이 형성됩니다.

So, let's now jump to the positive terminal, which is technically called the cathode. |||||||||||||陰極

Here we have Cobalt that has lost some electrons to oxygen, thus making the Cobalt positive, or +4 charged.

As a result, it wants to gain back an electron.

So, when we connect the negative and positive terminals to our smartphone, the electrons flow from the lithium which wants to give up an electron, through the circuits and components in the smartphone

and to the cobalt which wants to gain an electron.

Now here we run into a small issue. |||||||problema

With the flow of electrons from the negative to the positive terminal, the cobalt side grows more and more negatively charged,

and the other side positively charged.

Yes, the electrons do want to flow in this direction,

but at the same time electrons don't like to flow to an area

that is growing more and more negatively charged.

This is because opposite charges attract, and similar charges repel. |||||pritraukia||||atstumia

So, to fix this, we give the now positively charged lithium ions that recently left the graphite, a path to move to the other side. This path is called an electrolyte, and its function allows for lithium-ions to migrate over from one side to the other, while not allowing the electrons to move through it. When lithium gets to the cobalt side,

it again wedges itself, or intercalates with the cobalt and oxygen to become Lithium Cobalt Oxide. ||pleištai|||įsiterpia||||||||||

The lithium isn't regaining its electron- |||atgaunant||

that electron went to the cobalt, it's just balancing out the charge build up. ||||||||subalansuoja||||| Let's quickly recap. Here is a full battery. ||apžvelkime greitai||||| Throughout the day lithium atoms leave the graphite layers and separate from their electrons to become lithium ions. |atsiskirti|||||||

The electrons flow from the negative terminal through the circuits and components in the smartphone |||||||||grandinės||||| and into the positive terminal to join the cobalt atoms.

At the same time, the lithium-ions travel

through the electrolyte in order to neutralize the charge build up and keep the reaction going.

Here's the chemical formula for the reaction.

Thus, at the end of the day almost all of the lithium has left the graphite layers, and joined the cobalt to become lithium cobalt oxide, and your battery is now running on empty. Now that the battery is empty, let's recharge it.

We plug in our smartphone and when we do this the USB charger

applies a higher force on a flow of electrons in the opposite direction. ||||||||電子|||| Electrons are pulled out of the cobalt,

thus returning cobalt to its +4 state and kicking out the lithium ions. taigi|||||būseną||išstumti||||

On the other side, electrons are forced onto the graphite,

which pulls the lithium through the electrolyte, and back into the layers of graphite. As you see it's the exact opposite of the earlier reaction, which is why this battery is rechargeable. The lithium and its electrons move in one direction when you use the phone, and the opposite when you charge it back up.

Ok, so now let's rewind and add a few more details of note. ||||atsukti|||||||| First, these two sides can't touch, If the anode and cathode were to touch,

and if there were any lithium left in the graphite,

the chemical reaction would accelerate uncontrollably and cause a fire or often a small explosion. ||||||||||||||sprogimas

Thus, a non-conductive semipermeable separator |||laidus|puslaidžiai pralaidus|separator

that allows the lithium-ions to pass through is placed in the middle.

And this electrolyte isn't an effective barrier because it's a liquid

The second thing to note is that the graphite and cobalt peroxide ||||||||grafitas||| aren't good at collecting or distributing the electrons. |||||paskirstymo||

Thus, a conductive copper layer is added next to the graphite, |||varis|||||||

and a conductive aluminum layer next to the cobalt peroxide.

These two layers or sheets are called collectors.

Ok, onto third, these animations are showing 100% of the lithium moving from ||||animacijos||||||| the anode to the cathode, and back.

But in reality, there will always be some percentage

of lithium that remains in the anode, cathode, and electrolyte despite the battery being fully charged or discharged respectively. ||||||||atitinkamai Continuing to fourth, in order to maximize the capacity of the battery, and allow the battery to fit into your smartphone,

all these layers are folded and wrapped into a rectangular prism package. ||||sukrauti||supakuoti|||stačiakampis|| Ugh, I know this is a lot, but fifth and final,

in order to regulate the flow of electricity,

additional circuitry is added to the top of the battery. |cirkuliacija||||||||

This circuitry prevents overcharging and damage to the battery. So, then the final topic.

Why does your battery's max capacity reduce over time? There are several reasons,

one of which is that sometimes lithium and the incoming electron react with electrotye and organic solvent to form

compounds that are called a solid electrolyte interphase or SEI |||||||sąsaja|| SEI's irreversibly consume lithium and the electrolyte, |negrįžtamai|vartoti||||

thus reducing the overall quantity of lithium and

thereby reducing the max capacity of your battery. |mažinant||||||

Another reason is that when you fully discharge your battery until it's dead, it can result in too much lithium on the cobalt side,

which causes the irreversible generation of Lithium oxide and Cobalt (II) Oxide. These compounds are stuck in that state which thereby reduces the amount |||įstrigę|||||||| lithium and cobalt for future use.

So, one tip is to not let your battery run until its empty.

It's better to recharge your battery at

30 or 40% then to let it run until its dead. |tada|||||||

That about wraps it up.

When it comes to batteries,

there are hundreds of different chemistries and compounds that allow them to work,

but they all work on similar principles.

You just need three materials,

one that wants electrons,

one that wants to give up electrons,

and then a path for the build up of charge to neutralize.

Thanks for watching! Here are 3 questions I'm going to leave you with. Discuss them in the comments. Also, ask questions in the comments! If you do it I will pin the top questions for further discussion.

Don't forget to subscribe and tell your

friends and family about something you learned today.

This episode is about lithium ion smartphone batteries,

and it branches to electric vehicle batteries

discussed by Learn Engineering, we recommend you take a look! It also connects to galvanic and voltaic cells,

Chemical bonds & electronegativity

and lemon batteries.

Post your comments with further questions, answers, and thoughts. And Remember conceptual simplicity and structural complexity. ||konceptualus|paprastumas|||struktūrinė sudėtingumas