1 mole of a substance equals the amount of grams needed for that substance to have 6.0221413e+23 (Avogadro's number) atoms in it, isn't it? In order to determine how many grams one mole of a substance is, I've learned that you just need to check the atomic mass number on your periodic table, take that number and put "gram" at the end. The thing I don't understand is, how come it's that simple? The atomic mass number is the number of protons and electrons (nucleons) in the atom, right? So how come 6.0221413e+23 times the mass of all nucleons ALWAYS amounts to the number of nucleons in grams for any substance? For example, carbon has an atomic mass number of 12 so 1 mole of carbon equals 12 grams of carbon. Hydrogen has an atomic mass number of 1 so 1 mole of carbon equals 1 gram of hydrogen. Is this some great coincidence? Or is there a link that I'm not seeing? I'm not sure I understood what a mole is and my research on it just confuses me, so there's why I'm asking. Thank you for reading and (hopefully) helping!
Can you please explain how they did? 1 amu is the mass of 1 nucleon. The mass of a nucleon can't be chosen, it's fixed, it's a fact of nature that we can merely observe. This source explains that scientists couldn't directly measure the mass of a nucleon so they created the relationship: 1 amu = 1/6.0221415 x 10^23 grams I understand that 1 mole of 12 amu equals 12 grams following this relationship 6.0221415 x 10^23 = N = 1 mole 1 amu = 1/N g N x 12 x 1 amu = N x 12 x 1/N g <=> N x 12 x 1 amu = 12 x 1 g <=> N x 12 amu = 12 g But what I still don't get is, how did they know that the mass of a nucleon was equal to 1/6.0221415 x 10^23 grams ? The gram is a fixed quantity too, so they couldn't just arbitrarily choose that relationship to fit their needs, right?
Welcome to PF You are a critical thinker, and your question is a nice one and it proves that you don't just take knowledge as constant information but a "why" question always pops in your mind Avogadro's is a selected number, it's not a coincidence at all that the mass of Avogadro's number is equal to the mass number, Avogadro's was precisely selected because they certainly knew that the mass of his number for any element atoms will be equal to its mass number, how come? That seems so weird!! But it's actually very simple, let's do some math to get to the bottom of this. But first lets just point to some impotent things Atoms consist of protons, neutrons and electrons 1 - protons and neutrons roughly have equal masses 2 - electrons' mass is negligible So the mass of an atom = mass of neutrons + mass of protons = a.m.u x Mass number Mass of "n" atoms = a.m.u x mass number x n If n = the reciprocal of a.m.u then Mass of " n " atoms = Mass number bingo !!! That reciprocal is Avogadro's number, Avogadro's number = 1/a.m.u So mass of Avogadro's number of atoms = mass of proton or neutron x mass number x Avogadro's number = a.m.u x mass number x 1/a.m.u = mass number So it's not a coincidence, Avogadro's number was selected to be the mass of one a.m.u reciprocal so that one mole of any substance becomes equal to its mass number, thanks to Avogadro, chemical calculations are very Simple.
That's not true. Mass of neutron is 1.674927351×10^{-27} kg Mass of proton is 1.672621777×10^{-27} kg Mass of alpha particle (helium nucleus) is 6.64465675×10^{-27} kg Alpha particle is two neutrons and two protons, so its mass should be 2*1.674927351×10^{-27} + 2*1.672621777×10^{-27} = 6.695098256×10^{-27} Where is the missing 0.050441506×10^{-27} kg?
Thank you. I think I understand the logic behind it: Having n times the mass of an atom is practical in that it enables us to cancel out the number of nucleons in the equation (they're equal to 1) mass of Avogadro's number of atoms = [strike]mass of proton or neutron[/strike] x mass number x [strike]Avogadro's number[/strike] My only issue now is that this should be correct: Avogadro's number = 1/mass of proton or neutron But it isn't by my calculations mass of proton = 1.6726×10^-24 g (according to wiki) avogadro's number = 6.0221413x10^23 (according to google) 6.0221413x10^23 != 1/1.6726×10^-24 (the answer to 1/1.6726×10^-24 is 5.9787157718...x10^23 , going by my calculator). Did I make a mistake in my calculations? Or did I actually not understand the logic that you explained?
They didn't KNEW it, they DEFINED it as 1g/N_{A}. What they really did was they defined first 1 mole to be the number of atoms in exactly 12 grams of C-12. Selection of C-12 and 12 is arbitrary (actually in the past it was O-16 and 16 g). That allowed them to determine N_{A}. Once they had N_{A}, they calculated amu value - and this way it was guaranteed to work the way it does.
I was thinking about that too, and I also did some calculations and I find out that there something going wrong, as I said before my reply isn't accurate 100% but it got the main logical idea I hope someone on the forum could edit a correction, I did my best
Simple summation won't work for two reasons, First, mass of the nucleus is lower than the sum of masses of all nucleons by so called binging energy. Second, molar mass is the weighed average of masses of all isotopes present. That's why it was important to choose an isotope (C-12) and not an element (C) for the definition.
EDITED POST So you're contradicting ElmorshedyDr's logic? You're saying that they came up with Avogadro's number first and then calculated the amu value? So the number of Avogadro isn't actually the reciprocal of the mass of a nucleon (chosen to make the mass of the nucleon cancel out in the equations so that the atomic number would remain)? If that's correct, then how come their arbitrary choice (of the number of atoms in 12 grams of C-12) causes the mass of the atom to equal the atomic number in grams? I'm sorry, I'm really doing my best, but I'm not sure I understand what you mean...
Yes. Exactly. They defined mole, not the Avogadro's number. Once they defined mole, it was enough to count atoms in a mole (remember, exactly 12 g of C-12) to determine N_{A}. There is a plan to redefine the mole, and express it in terms of N_{A} - that is, to define N_{A} as being equal to some arbitrary value. But so far Avogadro's constant is not defined, but determined.
Some of the answer to your queries is in the link below. The thing to realise is scientists had got the mass proportions in which atoms combine and could work with moles about a century before they could get the mass of an atom (and so Avogadro's number). In traditional school courses they used to emphasise these laws of combinations and drilled you with endless calculations concerning them. Telling us really anything known about atoms was left till University. But now they reckon that's boring so they tell it earlier. But it sounds like they haven't told you how things like the mass of the atom are found out. The teachers in my time were instructed not to do that, to be scientific you had to grasp the reason for believing something. Now you can see that dealing with 10^{22}, say, atoms that is something you can see and weigh and so verify these laws of constant proportion in combinations etc. that were in fact the original experimental basis for atomic theory and all chemistry in a school lab. Hence the boring calculations - 'chemistry is not all fireworks' was a saying of one of my teachers - which students still have to do - it's called 'stoichoimetry' - and that we get many questions on here and that have an undeserved reputation for difficulty. You asked, almost, how did they determine the mass of an atom or molecule in grams also opposed to its relative mass I.e. the mass of one relative to another which is what I was just talkng about. There were several ways (all interesting stories) but the most key one historically was this: although the atoms and molecules are too small to see in any ordinary simple setup, these atoms are in constant motion and give kicks to other particles such as the fat globules of milk which are big enough to see by microscope moving as a result of these kicks ('Brownian motion'). Studying that, in brief, they got to Avogadro's number. The theory of it was the work of Einstein. Link https://www.physicsforums.com/showpost.php?p=4680146&postcount=7
I think you were answering me while I was editing my post, so you didn't see the change, but I'm still confused on: how come their arbitrary choice (of the number of atoms in 12 grams of C-12) causes the mass of the atom to equal the atomic number in grams? How can something arbitrary fit so perfectly? I don't understand how they could "define" the mass of a nucleon and not "know" it, given that grams are a fixed quantity of mass and the mass of a nucleon is a fixed quantity in nature that they could merely observe not choose, too... If you're not seeing my problem, here's an example: I "define" that the ball I'm holding has a mass of 2 kg. But when I lay it on my balance, it says that it weighs 9.81 newton here on earth. If the acceleration on earth equals 9.81 then the ball must have a mass of 1 kg (regardless of what I "defined"/chose earlier), it's not me who "defines" its mass, its mass is a fact of reality which I "know" because I calculated it. I've read it, but it defines avogadro's number as the reciprocal of the mass of a nucleon (on the second page) which our calculations and Borek contradicts. :/
Wait, if 1 amu equals 1g/Avogadro's number (as defined), then Avogadro's number equals 1g/1 amu, right? And 1g/1amu is the reciprocal of 1 amu, right? And 1 amu is 1/12 of the mass of a C-12 atom, so it's the mass of one nucleon. So that definition does say that Avogadro's number is the reciprocal of the mass of 1 amu, right? Ugh, this is so confusing :(
It is not mass of a nucleon that is defined, it is a UNIT used to measure it (amu) that is defined. It is defined to be 1/12 of the mass of the C-12 atom. Close to the mass of the nucleon, but different.
But if 1 amu does not equal the mass of a nucleon, then the mass of the nucleon can't be canceled out in the equaltion: 1 amu = 1 g/N_{A} N_{A} = 1g/1 amu Mass of atom = number of nucleons x mass of 1 nucleon N_{A} x Mass of atom = N_{A} x number of nucleons x mass of 1 nucleon 1g/1 amu x mass of atom = 1g/1 amu x number of nucleons x mass of 1 nucleon You can't say: Mass of nucleon/amu x number of nucleons = 1g x number of nucleons So N_{A} x mass of atom = number of nucleons g So how come having an Avogadro number (N_{A}) of atoms of an element equals the number of nucleons of that element in grams anyway? Why didn't they use the reciprocal of the mass of a nucleon instead of Avogadro's number although the former fits the equation perfectly (and the latter does not)?
Reflect, all measurements are comparisons. It is essential to have some standard to compare that back to, and since the nineteenth century the standards have been internationalised. And it is good to make them as convenient as reasonably possible. When you ask in #what a coincidence! how come it worked out that simple it's like saying hey a litre of water turns out to weigh exactly one kilo, incredible coincidence!