Isotopes, Percent Abundance, Atomic Mass | How to Pass Chemistry

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

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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

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@@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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So when you are calculating to find average atomic mass, do you wait until the end to round for sig figs, or do you do that throughout the problem as you go?

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Hello Melissa I love your channel you have already inspired me to feel like I can accomplish Chemistry! I don't understand why you round some of the answers within the average atomic mass formula answers? Is it because of the given Sig Figs? some of them in the first example had more Sig Figs in given do you just do the least amount?

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5:19 Why do you round with significant figures at the very end when you add, but you don't when you multiply the given isotopic mass with the percent abundance?

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I just wonder at 5.34. you said they given 4 sig figs then the answer should be 4, but they are adding not dividing or multiple, so we should choose the lowest decimal places for the answer, am I correct?

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I'm curious why did you write down 0.469915 when finding the atomic mass instead of using the number shown on the calculator? is this related to sig figs?