Question
Neon consists primarily of two isotopes, with mass numbers 20 and $22,$ with a small amount of a third isotope, with mass number $21 .$ Write the nuclear symbols for each of these isotopes. How many neutrons does each of these isotopes contain?
Step 1
Therefore, the nuclear symbols for the isotopes of neon with mass numbers 20, 22, and 21 are $^{20}_{10}Ne$, $^{22}_{10}Ne$, and $^{21}_{10}Ne$ respectively. Show more…
Show all steps
Your feedback will help us improve your experience
Niamat Khuda and 81 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Neon has three naturally occurring isotopes, Ne-20, Ne-21, and Ne-22. Ne-20 has a mass of 19.9924356 amu and a natural abundance of 90.48%, and Ne-21 has a mass of 20.0038428 amu and a natural abundance of 0.27%. Calculate the percent abundance and atomic mass for the missing isotope.
Neon has three naturally occurring isotopes. They include Ne-20, atomic mass of 19.992 amu and percent abundance of 90.48%; Ne-21, atomic mass of 20.994 amu and percent abundance of 0.27%; Ne-22 has a mass of 21.991 amu and percent abundance of 9.25%. Calculate the average atomic mass of neon?
Neon is an inert gas with three stable isotopes. It is used in gas lasers and in advertising signs. Its isotopes and their abundances are: $\begin{array}{lll}\mathrm{Ne}-20 & 19.9924 \mathrm{amu} & 90.51 \%\end{array}$ $\begin{array}{lll}\text { Ne-21 } & 20.9938 \text { amu } & 0.27 \%\end{array}$ $\begin{array}{ll}\text { Ne-22 } & 21.9914 \text { amu } & 9.22 \%\end{array}$ What is the average atomic mass of neon?
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD