Isotopes, Percent Abundance, Atomic Mass | How to Pass Chemistry
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- Опубліковано 8 вер 2024
- Finally, Isotopes are explained using simple real-life examples! Find out what isotopes of the same element have in common and how they are different. This video explains percent abundance and average atomic mass broken into easy steps.
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Practice problems with step by step answers:
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TIMESTAMPS
0:32 What are Isotopes
2:22 Average Atomic Mass Example
6:26 Percent Abundance Example
10:58 Practice problems
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Sorry Madame I've a question
Nitrogen is made by two isotopes N-14 and N-15 .given nitrogens atomic weigh of 14.007.what is the percent abundance of each of isotope
@@happinessnyamete4242 well i dont know the exact value so i used 14 and 15 as amu for the n-14 and n-15
step1. 14.007 = (y x 14) + ((1-y) x 15)
step2. 14.007 = 14y +15 - 15y
step3. 14.007 - 15 = 14y - 15y
step4. -0.993 = -1y
step5. -0.993/-1 = y
n-14= 0.993 x 100 n-15= (1- 0.993) x 100
n-14= 99.3% n-15= 0.7%
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Wait, what if there's three isotopes for finding percent abundance?
If it were three isotopes then you would label the first two as x and the last one as 1-2x. So the formula would be:
Average Atomic Mass= ( X ⋅weight of isotope) + ( X ⋅weight of isotope) + [(1-2X) ⋅ weight of isotope]
@@melissamaribel Why would the first 2 be labeled as X? I am just struggling to understand the "why" behind using 1-2x as opposed to another mathematical phrase in this formula. Thanks for your videos! I'm gathering so much information :)
@@melissamaribel if we put x same for upper two isotopes then their relative abundance will be same... Then it will be wrong
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Hey Melissa! I was just wondering why for the isotope abundance the first x was 63cu and not 65cu? Thank you!
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when it comes to finding % abundance, since we don't know the %, instead of substituting % with x, can't we just take the given mass of each isotope, divide it by the average atomic mass, and multiply by 100 for the percent abundance? Thanks for the help!
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