I am a Mole

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Ask min4u about Park Grand Paddington Court. Reviewed 5 March Afternoon tea for the second time. Reviewed 3 weeks ago via mobile. Travellers who viewed Park Grand Paddington Court also viewed. Terrace Restaurant at the Blakemore Hotel. All restaurants in London Been to Park Grand Paddington Court? Preparing to study chemistry. Atomic weight and atomic mass. The mole and Avogadro's number. Atomic number, mass number, and isotopes. Counting protons, electrons, and neutrons. Identifying isotopes and ions. Video transcript Let's talk about a concept that probably confuses chemistry students the most on some level.

But on some level it's also one of the simplest concepts. And that's the idea of a mole, which in chemistry is different than the thing digging up your backyard, or the thing you want to get removed from your left eye. A mole in chemistry is just a number.

See a Problem?

It's just a number, and the number is 6. So it's a very huge number. And this is also called Avogadro's number. Maybe I will do a video on Avogadro. But that's all you need to know. A mole is just a number. There are kind of more Byzantine definitions of a mole. This actually is not-- actually, let me copy and paste it from Wikipedia.

This is Wikipedia's definition of a mole. And you hopefully at the end of this video you'll see that they're equivalent.

But if you're just getting exposed to the concept, this to me, it's just not an easy concept. Basically, a "a mole is defined as the amount of substance of a system that contains as many elemental entities as there are atoms in 12 grams of carbon So if you just take the last part, atoms in 12 grams of carbon So that means that there are 1 mole of carbon let me write it like that-- carbon There are 1 mole of carbon 12 atoms in 12 grams of carbon.

And so that's why a mole is useful. So I could have just instead of writing 1 mole, I could have replaced this as there's 6.

How do you figure that out? Or I guess, what else does this mean? I mean, we just added in carbon, they said it's the amount of substance of any molecule, if you convert between atomic mass units and grams.

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This I find very confusing. How can we apply this in other places? So the first thing to realize is a mole is just a way of translating between grams and atomic mass units. One carbon 12 atom is what? What's its mass number? That's why it's called carbon 12 instead of carbon So its mass is 12 atomic mass units.



So if you have something that has a mass of 12 atomic mass units and you have a mole of them, or you have 6. So another way to think about it is 1 gram is equal to 1 mole of atomic mass units.

A Mole Is A Unit

I'll write amu's like that. Or you can write 1 gram is equal to 6. And the reason why this is useful-- and it's kind of addressed in this Wikipedia definition there-- is it helps us translate between the atomic world-- where we deal with atomic mass units and we deal with, oh, we've got an extra neutron now, let's add one to our atomic mass number-- and translating between that atomic world and our everyday world where we deal in grams.

And just so you know, a gram is still a pretty small amount of mass. A kilogram is about 2 pounds.

The Southlanders

So this is not much. So there's a ton of atoms in a very small amount of-- in 1 gram of carbon, or at least in 12 grams of carbon, you have a ton of atoms. And just to hit the point home, I probably should have talked about this in the atom. This is a huge number.