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The most common stable nitrogen isotope is
The other, less common, stable nitrogen isotope is
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Oxygen is composed of three isotopes 16/8 O (15.995 u), 17/8 O (16.999 u) and 18/8 O (17.999 u). One of these isotopes, 17/8 O, comprises of 0.037% of oxygen. What is the percentage abundance of the other two isotopes, using the average atomic mass of 15.9994 u.
The abundance of $""_8^16"O"$ is 99.762 %, and the abundance of $""_8^18"O"$ is 0.201 %. Assume you have 100 000 atoms of O. Then you have 37 atoms of $""_8^17"O"$...
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Vanadium has two naturally occurring isotopes, 50-V with an atomic mass of 49.9472 amu and 51-V with an atomic mass of 50.9440. The atomic weight of vanadium is 50.9415. What is the percent abundance of the vanadium isotopes?
The idea with that have two naturally occurring is that the percent abundances of those two must add up to give $100%$. In calculations, it is often easier to...
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What is the difference in stable and unstable isotopes?
Usually, what makes an isotope unstable is the large nucleus. If a nucleus becomes larger enough from the number of neutrons, since the neutron count is what makes , it...
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What are the stable isotopes of carbon?
There are many isotopes of carbon, most of them shntheric and highly unstable. A complete list is given at . Both stable isotopes of carbon occur in nature, carbon-12 being...
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Silver has two naturally occurring isotopes with the following isotopic masses 106.90509 and 108.9047. The average atomic mass of silver is 107.8682 amu. What is the fractional abundance of the lighter of the two isotopes?
We know that: $x_(1)106.9059 + x_(2)108.9047 = 107.8682$ $(i)$ $x_(1) + x_(2) = 1$ $(ii)$ We assume that silver has only the 2 , which for a first approximation...
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Bromine consists of two isotopes with masses of 78.92 and 80.92 amu. What is the abundances of these two isotopes?
$color(white)(XX)$mass(amu)$color(white)(X)$Isotopic abundance Br-79$color(white)(XXXX)$78.92$color(white)(XXXXXXX)$? Br-81$color(white)(XXXX)$80.92$color(white)(XXXXXXX)$? $"average atomic mass"=("mass*%"+"mass*%"+"mass*%"...)$ Let x be % abundance of Br-79 Let 1-x be % abundance of Br-81 Br is 79. 904g/mol on $color(orange)"(average atomic mass)"$ $79.904%=x+(1-x)$...
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Isotopes are considered stable when the strong overcomes the electrostatic repulsion between force positively charged what?
You might get a more nuanced answer in the Physics section, because the strong nuclear force is something that chemists don't have much of a handle on. As far as...
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Why do you think isotopes of $N$ are used in medicine as opposed to other elements with stable isotopes like boron, neon or sodium?
Isotopes, $""^15N$, $""^13C$, are the same chemically as the isotope they replace. They are not the same spectroscopically. Mass spectroscopy would certainly differentiate between the isotopes. In addition, there might...
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All isotopes of a particular element have the same atomic number. How then do the isotopes of a particular element differ?
: The number of protons in an atom, NOT the number of neutrons Isotope: An element with a varying number of neutrons Remember, we CANNOT change the number of protons...
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How do you calculate the atomic mass of element X if there are two isotopes of this element (x-24 and x-28) and 75% of all x atoms are x-28 isotopes?
$75%$ of all X atoms are X-28, which means that $25%$ of all X atoms are X-24 as there are only 2 . Then, you do the multiplied by...
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