Isotopes, Percent Abundance, Atomic Mass | How to Pass Chemistry
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- Опубликовано: 20 сен 2017
- 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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