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: 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 without changing the element.
However, by adding or subtracting neutrons, we can change an element's properties.
For an example:
This site goes into the different of H.
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An element has three naturally occurring isotopes with the following masses and abundances. How do you calculate the atomic mass of this element? What is the identity of the element?
The atomic mass is the weighted average of the atomic masses of each isotope. In a weighted average, we multiply each value by a number representing its relative importance. In...
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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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Do all isotopes of an element have the same atomic number?
If there is 1 positively charged particle in the atomic nucleus, 1 proton, then we have the element hydrogen; if 2, then helium; if 23, then vanadium etc. The atomic...
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Why is it necessary to use the average atomic mass of all isotopes, rather than the mass of the most commonly occurring isotope, when referring to the atomic mass of an element?
Why? Because accounting, and even more so chemistry, is a highly quantitative exercise. Mass is always conserved in a chemical reaction, and accurate masses, which are the weighted averages of...
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Do isotopes that have the same atomic number have the same atomic mass?
I'll assume by "atomic mass" you don't mean the "average mass of the naturally occurring isotopes", but rather the individual mass of the isotope itself. If multiple isotopes have...
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The atomic mass of element A is 63.6 atomic mass units. The only naturally occurring isotopes of element A are A-63 and A-65. What is the percent abundance in a naturally occurring sample of element A closest to?
The average isotopic mass is the weighted average of the mass of the individual . Because the quoted average, $63.6$ $"amu"$, is closer to $""^63A$ than $""^65A$, the $""^63A$...
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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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A fictitious element that has two isotopes has an average atomic mass of 117.3. If 65.43% of the atoms of the element have an atomic mass of 119.8, what is the atomic mass of the other isotope?
The weighted average of the is equal to $117.3*"amu"$. And thus.........with units of $"amu"$ $[65.43%xx119.8+34.57%xxchi] =117.3$ Where $chi-="mass of the other isotope"$.... And so we solve for $chi$.... $chi=(117.3-0.6543xx119.8)/(0.3457)=112.6*"amu"$
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All the atoms of a particle element have an equal number of protons and neutrons (Z=N). Which one is true?
A) The atomic weight must be a whole number.
B) The mass number must be exactly twice the atomic number for each atom.
The answer is B) The must be exactly twice the for each atom. The number of protons is the atomic number of an element. The mass number is the sum...
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