Atomic Mass: Introduction
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- Опубликовано: 7 окт 2012
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What is atomic mass? It is a weighed average of the different isotopes of an element. It is sometimes referred to as atomic weight, relative atomic mass, or average atomic mass. We look at how to calculate and determine the weighed average of elements using atomic mass units.
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Hey everyone, I'm here to help. If you have any questions or just want to learn more, click on the link in the description above. It'll take you to a page where you can ask me questions.
Hey can You please tell me How do we know exact number of electron, proton, neutron, and exact atomic mass when we cant even see atom?
I can't see the discription sir
I am a student working toward a PhD in science education. This is a great video - you use several techniques that have been shown to help people learn difficult material
1) define vocabulary in common language
2) compare and contrast (weighted vs. non weighted average)
3) build on/activate prior knowledge (beginning with average before moving on to weighted average and the use of the car analogy
4) use of multiple representations (illustrations, science terms, number sentences)
5) solved a simpler problem working toward the problem using isotopes
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I'm happy to answer this question. Just do me a favor and ask it by clicking on the link in the video description above (vsepr.org); it will take you to a page where you can ask and answer questions.
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These videos are really interesting so thanks for creating them. I came here just by googling what are isotopes after reading about heavy water and not really understanding it.
One question I have is what is the point of knowing the weighted average mass of an element? That number completely depends on how much of it is out there, which I presume is done by some sort of sampling?
Whatever the reason, how can we sure this is correct in the full universe and if our sampling of the element is wrong, doesn't that impact the above uses quite significantly?
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great video but you did not explain the concept of carbon 12 isotop as base for calculating relative atomic mass. It says 1/12 of C-12 = 1 amu. It is very confusing. Did you have a video on that ?
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I don't know if this might help people but working out the "regular average" or (4000 + 5000)/2 = 4500 is actually just a different version of 4000 x (0.5) + (5000 x 0.5) = 4500. Both equations are saying there are 50% of lemona GX and lemona GXL.
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