What's the Difference between Mass Number and Atomic Mass?
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- เผยแพร่เมื่อ 22 ส.ค. 2024
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What's the difference between mass number and atomic mass? Mass number is the number of protons and neutrons in an atom, and it tells us about the mass of the atom in amu, or atomic mass units. Atomic mass is the average mass of all the isotopes of a certain type. It is a weighted average that takes into account the abundances of all of the different isotopes.
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Good question! You can look it up in a textbook or on the web, or (usually) it will be given to you in a problem. But the point is, there's no way you can know what the abundance percentages are just off the top of your head, so don't worry if you didn't know where they'd come from.
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This was incredibly helpful, I feel far more confident in my ability to calculate this now. Thank you!!!!!
Thankyou very much! I passed my chemistry exam with 21/25 and its because of you . But i also have some doubt in atomic mass can you explain me how to find it
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Hey do yo have another video explaining differences between Relative Atomic And Molecular Masses? Thx
This is the most unequivocal explanation of Atomic and Mass number. Crystal clear explanation.
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Very precise explanation...Thank you
Your videos are fantastic but in this case your description of relative atomic mass is misleading- misleading because the MOST important concept to understand is the RELATIVE part of "relative atomic mass". If you understand its relativity to 1/12 of the mass of Carbon and the use of ratios to simplify the Math, we are ultimately able to relate mass to moles (and vice versa), moles to atoms/ions/compounds. It demystifies chemistry calculations... I can forward some info to assist- I home school by kids and formally lectured at University. If you have dealt with this elsewhere- my apologies...
Meto Leach You bring up a good point. But I don't think it's necessarily applicable to this video. It's true that I'm not talking about the *relative* part in this video, but I'm trying not to confuse the students. For me, by far the most important part of relative atomic mass is the idea that it's a weighed average of the masses of different isotopes. 99% of students don't understand that. The C-12 relative issue is, in my mind, much more relevant to the issue of relative *isotopic* mass, in other words, the mass of each individual isotope. Once we have masses for those, it's important to understand that the relative atomic mass for an element is fundamentally a weighed average of those isotopic masses.
Tyler DeWitt Can I encourage you to take time to understand this concept not from the perspective of "weighed averages" to get exact weights but how we produce simple numbers (Ar, relative to C-12), and how the mole (defined as exactly 12gms of C-12 containing x units) and relative atomic mass enables us to relate these simple numbers (Ar, Mr) to the physical property of mass, and enables us to compare products and reactants using stoichiometry. These concepts transformed chemistry because it took chemistry from a textbook (theory) to hands-on chemistry (calculating mass, yields, quantitative analysis, concentrations..etc). Students rarely struggle with relative atomic mass from the perspective of adding up numbers from a table, they just accept whatever they're given. However they struggle when they ask why can I use relative atomic masses to calculate a mole, why can I add Ar's to give Mr's, why can I use Ar's for ions, elements...etc Most teachers will simply say that "by definition". But if you were to show why these definitions were written the way they were (its not random) and not just show how to use it, you would understand this aspect of chemistry as a natural continuum and not as unrelated parts of puzzle. A piece-meal approach to teaching only leads to confused minds (PS-I'm not saying that this is what you do!)
Meto Leach I totally completely agree with you. I think that is a beautiful way to teach Chemistry.
+Meto Leach I'm still trying to figure out how to explain the idea of 'relative' atomic mass involving this definition: relative atomic mass = mass of one atom of the element / (1/12 x mass of one atom of C-12)...this definition is often found in chemistry textbook..students find it difficult to understand and teachers find it difficult to explain..so this is usually 'touch-and-go' and students basically simply go back to the numbers provided in the Periodic Table without really understanding how they come about! If you have any materials to share that can close this gap, it would be most valubale when I'm teaching this topic to my students!
A Chemistry teacher from Singapore
+Tyler DeWitt
Thank you for all your amazing videos! As a teacher myself, I'm learning a lot from you!
Based on my reply to Meto Leach shown below:
I'm still trying to figure out how to explain the idea of 'relative' atomic mass involving this definition: relative atomic mass = mass of one atom of the element / (1/12 x mass of one atom of C-12)...this definition is often found in chemistry textbook..students find it difficult to understand and teachers find it difficult to explain..so this is usually 'touch-and-go' and students basically simply go back to the numbers provided in the Periodic Table without really understanding how they come about! If you have any materials to share that can close this gap, it would be most valubale when I'm teaching this topic to my students!
Would you have an idea or would even make a video to address this issue? Thanks so much for your help! :)
A Chemistry teacher from Singapore
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Excellence explanation. My teacher told me: mass of an element as compared with the mass of an atom C taken as 12. He confused us but now i get it
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Why are carbon limited to just boron 10 and 11? Why cant there be boron 50 and boron 100?
+Leopold Vincent Medley good point you raised
There can be but they would be so unstable that they would have half lifes that we couldn't even count. Boron 11 and Boron 10 are much more stable. Furthermore because Boron-11 has a abundance of 80% it has a much more stable amount of neutrons and protons.
Leopold...boron 10 and 11 is just what is found in nature. If there really was a boron 50 in nature then you would calculate that in. How scientists found out what is in nature percentage wise is another question.
Ernie Estrada Using mass spectrometry....
Ernie Estrada you are correct.
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