You're more likely toĭeal with several grams of an actual substance. You're very unlikely to justīe dealing with one atom, or just a few atoms, or That we might actually see in a chemistry lab. But, what we're gonna do in this video is connect it to the masses Mass at an atomic level, or at a molecular level. Idea of average atomic mass, which we began to realizeĬould be a very useful way of thinking about a In a previous video, we introduced ourselves to the I hope this story/example helps out as a starting point for what can be a very difficult concept depending on how it is approached. Then I would go into the more specific and accurate details given by Just Keith to explain the concept thoroughly. Now, for Chemistry when dealing with atoms, compounds or particles of elements, the 'convenient number' is the mole, which makes the use of the atomic mass numbers on the Periodic table manageable and much easier to use both in theoretical calculations and practical experimentation with chemicals. ![]() The last item, the salt, it would not be feasible to count out grains or even to determine the grain size being consistent, but would be more like the problems encountered for the much smaller atom/compound/molecule. ![]() I would just like to add maybe an even more basic explanation that I would employ to start with: when going to the grocery store to shop for you and your family, you would not pick up eggs individually anymore, or say 27 mL of milk or a specific amount of grains of salt (say 5000 grains), you would get say a donzen eggs, a litre/gallon of milk and specific mass/weight in gram/ounce of salt depending upon which unit of measure you use, this being more convenient and manageable number(s) when shopping. I agree completely with Just Keith's answer of the over complication of this video along with his great detail on the background and mathematics of the mole and atomic mass unit.
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