Isoptopes and Average Atomic Mass

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Presentation transcript:

Isoptopes and Average Atomic Mass Chemistry 11 Ms. McGrath

Atomic Mass Recall: The mass number, A, tells us the sum of protons and neutrons in the nucleus of an atom. The mass of an atom is expressed in atomic mass units (µ). Example: An oxygen that has 8 protons and 8 neutrons in its nucleus has a mass number of 16.

Atomic Mass Recall: All neutral atoms of the same element has the same number of protons and electrons. However, the number of neutrons can vary. Therefore, atoms of the same element do not necessarily have the same mass number.

oxygen-16 ( ), oxygen-17 ( ), oxygen-18 ( ) Isotopes Most oxygen atoms have a mass number of 16 (A = 16) There are, however, two other naturally occurring forms of oxygen. One of these has 9 neutrons, so A = 17 and the other has 10 neutrons, so A = 18. These forms are referred to as isotopes. These three isotopes of oxygen are called: oxygen-16 ( ), oxygen-17 ( ), oxygen-18 ( )

Isotopes - Oxygen Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. Isotopes of oxygen:

Isotopic Abundance The relative amount in which each isotope is present in an element is the isotopic abundance. Abundance can be expressed as a percent (100%) or as a decimal (1.00). For example, magnesium has three natural occurring isotopes. It is made up of 79% magnesium-24, 10% magnesium-25 and 11% magnesium-26.

Average Mass and the Periodic Table The average atomic mass on the periodic table is the average of the masses of all the element’s isotopes. The abundance of each isotope of the element must be taken into account when calculating the average atomic mass.

Calculating the Average Mass Natural occurring silver exists as two isotopes. From the mass of each isotope and the isotope abundance listed below, calculate the average atomic mass of silver. Isotope Atomic Mass (µ) Relative abundance (%) Ag 106.9 51.8 108.9 48.2