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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.
Chrome design nails. Oxygen is a chemical element with atomic number 8 which means there are 8 protons and 8 electrons in the atomic structure. The chemical symbol for Oxygen is O. Oxygen is a colourless, odourless reactive gas, the chemical element of atomic number 8 and the life-supporting component of the air.
1 Answer
The abundance of #'_8^16'O'# is 99.762 %, and the abundance of #'_8^18'O'# is 0.201 %.
- $ begingroup$ @Martin that is a good point, but I think that for the most part 'amu' is understood to be the unified atomic mass unit based on carbon-12, not oxygen-16. I at least have always seen 'amu' and not 'unified amu' in publications within the last couple of decades. $ endgroup$ – thomij Feb 25 '16 at 16:21.
- Atomic mass of Oxygen is 15.9994 u. The atomic mass is the mass of an atom. The atomic mass or relative isotopic mass refers to the mass of a single particle, and therefore is tied to a certain specific isotope of an element.
Assume you have 100 000 atoms of O. Then you have 37 atoms of #'_8^17'O'# and 99 963 atoms of the other isotopes.
Oxygen's Amu
Let x = the number of atoms of #'_8^16'O'# . Then the number of atoms of #'_8^18'O'# = 99 963 - x
The total mass of 100 000 atoms is
x × 15.995 u + (99 963 – x) × 17.999 u + 37 × 16.999 u = 100 000 × 15.9994 u
15.995 x + 1 799 234.037 – 17.999 x + 628.963 = 1 599 940
2.004 x = 199 123
x = 199 123/2.004 = 99 762
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Oxygen Amu
![Five uses for oxygen Five uses for oxygen](/uploads/1/3/7/3/137353452/441324459.png)
So there are 99 762 atoms of #'_8^16'O'# or 99.762 %.
The number of #'_8^18'O'# atoms is 99 963 – 99 762 = 201 atoms or 0.201 %.
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Related questions
The atomic mass of an element is the average mass of the atoms of an element measured in atomic mass unit (amu, also known as daltons, D). The atomic mass is a weighted average of all of the isotopes of that element, in which the mass of each isotope is multiplied by the abundance of that particular isotope. (Atomic mass is also referred to as atomic weight, but the term 'mass' is more accurate.)
For instance, it can be determined experimentally that neon consists of three isotopes: neon-20 (with 10 protons and 10 neutrons in its nucleus) with a mass of 19.992 amu and an abundance of 90.48%, neon-21 (with 10 protons and 11 neutrons) with a mass of 20.994 amu and an abundance of 0.27%, and neon-22 (with 10 protons and 12 neutrons) with a mass of 21.991 amu and an abundance of 9.25%. The average atomic mass of neon is thus:
Oxygen Amu Weight
0.9048 | × | 19.992 amu | = | 18.09 amu |
0.0027 | × | 20.994 amu | = | 0.057 amu |
0.0925 | × | 21.991 amu | = | 2.03 amu |
20.18 amu |
The atomic mass is useful in chemistry when it is paired with the mole concept: the atomic mass of an element, measured in amu, is the same as the mass in grams of one mole of an element. Thus, since the atomic mass of iron is 55.847 amu, one mole of iron atoms would weigh 55.847 grams. The same concept can be extended to ionic compounds and molecules. One formula unit of sodium chloride (NaCl) would weigh 58.44 amu (22.98977 amu for Na + 35.453 amu for Cl), so a mole of sodium chloride would weigh 58.44 grams. One molecule of water (H2O) would weigh 18.02 amu (2×1.00797 amu for H + 15.9994 amu for O), and a mole of water molecules would weigh 18.02 grams.
Oxygen Amu Atom
The original periodic table of the elements published by Dimitri Mendeleev in 1869 arranged the elements that were known at the time in order of increasing atomic weight, since this was prior to the discovery of the nucleus and the interior structure of the atom. The modern periodic table is arranged in order of increasing atomic number instead.