How To Get Average Atomic Mass

Download Article

Average atomic mass is not a direct measurement of a single atom. Instead, it is the average mass per atom for a typical sample of a given element. If you could measure the mass of billions of individual atoms, you could calculate this value the same way you would find any average. Fortunately, there is a more practical method that relies on recorded information on the rarity of different isotopes.

1
Understand isotopes and atomic masses. Most elements can naturally occur in multiple forms, or isotopes. The mass number for each isotope is the sum of numbers of protons and neutrons in the nucleus. Each proton and each neutron weigh 1 atomic mass unit (amu).^[1] The only difference between two isotopes of the same element is the number of neutrons per atom, which affects the atom's mass.^[2] However, the element always has the same number of protons.
- The average atomic mass of the element takes the variations of the number of neutrons into account, and tells you the average mass per atom in a typical sample of that element.
- For example, the element silver (Ag) has two naturally occurring isotopes: Ag-107 and Ag-109 (or ¹⁰⁷Ag and ¹⁰⁹Ag).^[3] Isotopes are named after the "mass number," or the sum of protons and neutrons in one atom.^[4] This means Ag-109 has two more neutrons per atom than Ag-107, giving it slightly more mass.
2
Look up the mass of each isotope. You'll need two pieces of information for each isotope, which you can look up in a reference book or an online source such as webelements.com. The first is the atomic mass, or the mass of one atom of each isotope. Isotopes with more neutrons have more mass.
- For example, the silver isotope Ag-107 has an atomic mass of 106.90509 amu (atomic mass units). The isotope Ag-109 is slightly heavier with a mass of 108.90470.
- The last couple decimal places might be slightly different in different sources. Don't include any numbers in parentheses after the mass.
3
Write down the abundance of each isotope. The abundance tells you how common the isotope is, as a percentage of all atoms of the element. Each isotope contributes proportionally to its abundance (the more abundant the isotope, the more it will contribute to the average atomic mass). You can find this in the same source you found the mass. The abundances of all isotopes should add up to 100% (though it might be slightly off due to rounding errors).
- The isotope Ag-107 has an abundance of 51.86%. Ag-109 is slightly less common with an abundance of 48.14%. This means that a typical sample of silver is 51.86% Ag-107 and 48.14% Ag-109.
- Ignore any isotopes that do not have an abundance listed. These isotopes do not occur naturally on Earth.
4
Turn your abundance percentages into decimals. Divide the abundance percentage by 100 to get the same value as a decimal.
- In the sample problem, the abundance figures are 51.86 / 100 = 0.5186 and 48.14 / 100 = 0.4814.
5
Find the weighted average of the atomic mass of its stable isotopes. The average atomic mass of an element with n isotopes equals (mass_{isotope 1} * abundance_{isotope 1}) + (mass_{isotope 2} * abundance_{isotope 2}) + ... + (mass_{isotope n} * abundance_{isotope n} .^[5] This is an example of a "weighted average," meaning that more common (more abundant) masses have a greater effect on the result. Here's how to use this formula for silver:
- Average atomic mass_Ag = (mass_Ag-107 * abundance_Ag-107) + (mass_Ag-109 * abundance_Ag-109)
  =(106.90509 * 0.5186) + (108.90470 * 0.4814)
  = 55.4410 + 52.4267
  = 107.8677 amu.
- Look up the element on a periodic table to check your answer. The average atomic mass is usually written underneath the element symbol.^[6]

1

Convert mass to number of atoms. The average atomic mass tells you the relationship between mass and number of atoms in a typical sample of the element. This is useful in chemistry laboratories because it is almost impossible to count the number of atoms directly, but easy to measure mass. For example, you can weigh a sample of silver and predict that each 107.8677 amu of mass contains one silver atom.
2

Convert to molar mass . Atomic mass units are very small, so chemists typically weigh samples in grams instead. Fortunately, these concepts are defined to make the conversion as easy as possible. Just multiply the average atomic mass by 1 g / mol (the molar mass constant) to get an answer in g / mol instead. For example, 107.8677 grams of silver contain one mole of silver atoms on average.
3
Find average molecular mass. Since a molecule is just a collection of atoms, you can add the masses of the atoms together to find the mass of the molecule. If you use the average atomic masses (instead of the mass of a specific isotope), the answer is the average mass of the molecule as found in a naturally occurring sample. Here's an example:
- A molecule of water has the chemical formula H₂O, so it contains two hydrogen (H) atoms and one oxygen (O) atom.
- Hydrogen has an average atomic mass of 1.00794 amu. Oxygen atoms have an average mass of 15.9994 amu.
- The average mass of a molecule of H₂O equals (1.00794)(2) + 15.9994 = 18.01528 amu, equivalent to 18.01528 g/mol.

Add New Question

Question

How do you find weighted average mass if you don't have one of the amu?

Meredith Juncker is a PhD candidate in Biochemistry and Molecular Biology at Louisiana State University Health Sciences Center. Her studies are focused on proteins and neurodegenerative diseases.

Scientific Researcher

Expert Answer

An atomic mass unit is the same thing as grams per mole (1 amu = 1 g/mol). It is also the same thing as a dalton (1 amu = 1 Da). so if you don't know the amu for one of your elements, you can search for this particular isotope online to find the amu and natural abundance specific to that particular isotope.
Question

What's the atomic weight of platinum?

Meredith Juncker is a PhD candidate in Biochemistry and Molecular Biology at Louisiana State University Health Sciences Center. Her studies are focused on proteins and neurodegenerative diseases.

Scientific Researcher

Expert Answer

The atomic weight of platinum is 195.078 amu. Check out "How to Calculate Atomic Mass" for more information.
Question

Why do we need to know average atomic mass?

Meredith Juncker is a PhD candidate in Biochemistry and Molecular Biology at Louisiana State University Health Sciences Center. Her studies are focused on proteins and neurodegenerative diseases.

Scientific Researcher

Expert Answer

It's important to know average atomic mass because different isotopes of an element exist at different abundances on Earth, so different isotopes contribute to the average atomic mass at different proportions.
Question

How do I find the atomic weight?

The atomic weight is just another term for the average atomic mass.
Question

Can you give another example of average atomic mass?

Neon has three natural isotopes: 90.48% of Neon is Ne-20 with a mass of roughly 19.992 amu; 9.25% is Ne-22 with a mass of 21.991 amu; and 0.27% is Ne-21 with a mass of 20.993 amu. The average atomic mass of Neon is (19.992)(0.9048) + (21.991)(0.0925) + (20.993)(0.0027) = about 20.180 amu.
Question

As the atomic number increases within a group of elements, the atomic radius usually does what?

We can assume the atomic radius increases with the atomic number.
Question

How can I find average mass of bromine?

Go to socratic.org/chemistry, and search "atomic mass of bromine."

Ask a Question

200 characters left

Include your email address to get a message when this question is answered.

Submit

Video

The term relative atomic mass is sometimes used as a synonym for average atomic mass. There is a slight difference since the relative atomic mass has no units; it is a measure of mass relative to the carbon-12 atom. As long as you use atomic mass units in your average mass calculation, however, the two values are numerically identical.
With rare exceptions, elements later on the periodic table have a higher average mass than the elements before it. This is a quick way to check whether your answers make sense.
1 atomic mass unit is defined as 1/12 the mass of one carbon-12 atom.
The isotope abundances are based on samples that naturally occur on Earth. Unusual substances such as a meteorite or a sample created in a laboratory might have different ratios of isotopes, and therefore a different average atomic mass.
The parenthetical number after an atomic mass tells you the uncertainty in the final digit. For example, an atomic mass of 1.0173 (4) means that typical samples vary within a range of 1.0173 ± 0.0004. You don't need to take this into account unless the problem requires it.
Use the average atomic mass when doing mass calculations involving elements and compounds.^[7]

Atomic masses are almost always written in terms of atomic mass units (amu or u), sometimes called the dalton (Da). Never add a different unit of mass (such as kilograms) after the number without converting it.

Things You'll Need

Pencil
Paper
Calculator
Isotope abundance data
Isotope atomic mass unit data

About This Article

Article SummaryX

If you need to find the average atomic mass of an element, you will need to look up the atomic mass and the abundance of each isotope in that element. The abundance of all of the isotopes should add up to 100%. Multiply the mass times the abundance for each isotope, then add all of the results together to get the average atomic mass. For tips from our reviewer on how to convert the mass to the number of atoms, keep reading!

Did this summary help you?

Thanks to all authors for creating a page that has been read 413,684 times.