Isotopes, Percent Abundance, Atomic Mass | How to Pass Chemistry
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- เผยแพร่เมื่อ 22 ส.ค. 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]
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@@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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@@ilyasjamei1413 At 8:10, why should we give 'x' to 1st isotope why not to another one?
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