Monthly Archives: October 2016

Tara Wood of Augusta, Georgia, was with two of her kids on a routine trip to the grocery store. It was Norah, her 4-year-old’s, birthday.

That’s when they ran across Dan Peterson, known as Mr. Dan. 

“As Mr. Dan walked by, she (Norah) smiled and waved. ‘Hi old person! It’s my birthday!’” said Wood. “He stopped in his tracks, smiled, and said, ‘Well hello, little lady! How old are you today?’ They chatted for a couple of minutes, and we went our separate ways.”

<Read the rest of the story>

October 23^rd is Mole Day—you know, because 10/23 is like 10²³.

THE EARLY HISTORY of chemistry has many interesting stories. Just consider the problems scientists had 200 years ago as they tried to figure out some of the most basic ideas of chemistry. It was clear that there were different substances—for instance, water is different than coal. But it wasn’t so clear what these substances were made of. You could take something like nitrogen gas (N₂) and oxygen gas (O₂) and combine them together to make another gas (in this case NO₂). It thus seemed reasonable to suppose that stuff (molecular gas) was made of smaller stuff (atoms). But the evidence isn’t so easy to see. The primary difficulty is that humans can’t see molecules or atoms. All the scientific ideas have to be built on indirect evidence.

This is where Amedeo Avogadro comes into the picture (of course his real name is Lorenzo Romano Amedeo Carlo Avogadro di Quaregna e di Cerreto—but everyone just calls him Avogadro for obvious reasons). Avogadro developed the following idea:

Avogadro’s Law: If you have two gasses at the same temperature and pressure, they will occupy the same volume only if they contain the same number of molecules.

If you are thinking this is just a version of the Ideal Gas Law, you are correct—but let’s move on to a useful example. Suppose you take water (which is H₂O) and run an electric curent through it—called electrolysis. This can break the water molecules into hydrogen gas and oxygen gas (which you could collect). If you had these two gases at the same temperature and pressure, the hydrogen gas would take up twice the volume compared to the oxygen gas. Why? Well, when you break up the water molecule, you get twice as much hydrogen as oxygen. Yes, hydrogen doesn’t just float around as a single atom. Instead it forms a bond with another hydrogen to make H₂—but oxygen does the same thing (O₂).

In the end, you would know that water is made of both hydrogen and oxygen and that there is twice as much hydrogen as oxygen. That’s a pretty big piece to the whole elements puzzle and you need an idea like Avogadro’s Law to figure it out.

Avogadro’s Number

But what about this number of Avogadro? Why is it important and why didn’t Amedeo know what it was? Let’s start with a definition. If I have 12 grams of carbon-12 (not any other isotopes of carbon) then it would have exactly Avogadro’s number of atoms in it. We can write this number as (approximately):

So we would call this number of carbon atoms, one mole (sort of like 12 eggs is one dozen).

Why is important? Avogadro’s number is sort of like a bridge. It bridges chemistry and atomic physics. In chemistry we measure things based on their bulk properties. Things like mass (total mass), pressure, volume, temperature. However, when we consider these things from an atomic perspective we look at individual atoms and the momentum, velocity of these particles. Avogadro’s number connects these two ideas and allows us to explore atomic-level things by measuring macroscopic level quantities. It’s a big deal.

But why didn’t Avogadro know this number? Because he didn’t directly come up with the idea. Chemists named the number after Avogadro to honor his contributions to chemistry.

Determining a Value for Avogadro’s Number

If you had a carton with a dozen eggs, you could open up the package and count the number of eggs to find out that one dozen equals twelve. You can’t really do the same thing with a mole of carbon. Carbon atoms are too tiny to see and there are too many to count. We have to find another way to get a value for Avogadro’s number. There are quite a few ways to determine this magic number, but let me go over a simple method.

Start with two pieces of copper placed in a solution of copper-sulfate. When you run an electric current through the system, copper is removed from one plate and deposited on the other plate. This means that one of the plates gains mass and the other loses mass (should be by the same amount).

When the copper atom is removed from one plate, it acts as a charge carrier in the complete circuit (battery, wires, copper, solution). If I measure the current in this circuit and record the time, I can use the definition of current to find the total transfer of charge (which would be the transfer of copper ions).

Let’s put this all together.

• Run current through the copper and copper sulfate.
• Positive copper ions are transferred from one plate to the other making a change in mass (which I can measure).
• I can measure the current and time and calculate the total transfer of charge from one plate to another.
• Since a copper ion has a positive charge of 1 e (charge of an electron), I can get the number of ions transferred.
• Knowing that 1 mole of copper is 63.546 grams, I should be able to get a relationship between the change in mass and the number of moles—which will give me Avogadro’s number.

In my rough experiment, I had an electric current of 0.42 Amps for 10 minutes. This gives a total change in charge of 252 Coulombs. Dividing this by the charge of one ion (1.6 x 10^-19 C) I get 5.575 x 10²¹ ions. The change in mass of one plate is 0.344 grams. That’s all I need. Now I can write:

That’s not a terrible value for Avogadro’s number. Really, it’s not. If you take the accepted value of 6.022 x 10²³, then my estimate is just off by less than a factor of 2. I call that close enough. The idea works even if my method was a little bit sloppy. Still, my value is better than no value.