Learning ObjectiveCalculate the typical atomic fixed of an element given the isotopes and their natural abundance
Key PointsAn element can have differing number of neutron in that nucleus, however it constantly has the same variety of protons. The version of an aspect with different neutrons have different masses and also are called isotopes.The average atomic mass for an facet is calculate by summing the masses of the element’s isotopes, each multiplied by its herbal abundance on Earth.When doing any type of mass calculations involving facets or compounds, constantly use average atomic mass, which have the right to be found on the periodic table.

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Termsnatural abundanceThe variety of a certain isotope naturally discovered on the planet.average atomic massThe fixed calculated through summing the masses of an element’s isotopes, each multiplied by its organic abundance on Earth.mass numberthe total variety of protons and also neutrons in an atom nucleus.

The atomic variety of an element defines the element’s identity and signifies the variety of protons in the nucleus of one atom. For example, the facet hydrogen (the lightest element) will always have one proton in that is nucleus. The element helium will always have two protons in that nucleus.

Isotopes

Atoms that the same facet can, however, have actually differing numbers of neutrons in your nucleus. Because that example, secure helium atoms exist that contain either one or 2 neutrons, yet both atoms have two protons. This different types of helium atoms have various masses (3 or 4 atomic mass units), and also they are referred to as isotopes. For any type of given isotope, the amount of the numbers of protons and neutrons in the cell nucleus is dubbed the mass number. This is since each proton and each neutron weigh one atom mass unit (amu). By including together the number of protons and also neutrons and multiplying through 1 amu, you deserve to calculate the mass of the atom. All facets exist together a arsenal of isotopes. Words ‘isotope’ originates from the Greek ‘isos’ (meaning ‘same’) and also ‘topes’ (meaning ‘place’) due to the fact that the facets can occupy the same location on the periodic table when being different in subatomic construction.

Lithium AtomStylized lithium-7 atom: 3 proton (red), 4 neutron (blue), and also 3 electron (black). (Lithium additionally has another, rarer isotope with just 2 neutrons. )

Calculating average Atomic Mass

The typical atomic massive of an element is the amount of the masses the its isotopes, every multiplied by its organic abundance (the decimal linked with percent of atoms of that element that room of a given isotope).

Average atomic mass = f1M1 + f2M2 + … + fnMn where f is the portion representing the herbal abundance that the isotope and M is the massive number (weight) the the isotope.

The median atomic mass of an element can be uncovered on the periodic table, commonly under the element symbol. Once data space available regarding the herbal abundance of miscellaneous isotopes of one element, that is basic to calculation the typical atomic mass.

For helium, there is around one isotope of Helium-3 for every million isotopes of Helium-4; therefore, the mean atomic mass is really close come 4 amu (4.002602 amu).Chlorine is composed of two major isotopes, one with 18 neutron (75.77 percent of herbal chlorine atoms) and one with 20 neutrons (24.23 percent of herbal chlorine atoms). The atomic variety of chlorine is 17 (it has 17 protons in that nucleus).

To calculate the median mass, first convert the percentages right into fractions (divide them by 100). Then, calculate the fixed numbers. The chlorine isotope through 18 neutron has wealth of 0.7577 and a mass variety of 35 amu. To calculate the mean atomic mass, multiply the fraction by the mass number for each isotope, then include them together.

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Average atomic mass the chlorine = (0.7577 cdot 35 amu) + (0.2423 cdot 37 amu) = 35.48 amu

Another example is to calculation the atomic mass the boron (B), which has actually two isotopes: B-10 v 19.9% organic abundance, and also B-11 with 80.1% abundance. Therefore,

Average atomic mass of boron = (0.199cdot

10 amu) + (0.801cdot

11 amu) = 10.80 amu

Whenever we carry out mass calculations involving facets or compounds (combinations that elements), we always use average atomic masses.


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