Average Atomic Mass and Isotopes

Vocabulary flashcards covering key concepts related to average atomic mass and isotopes.

Average Atomic Mass

The weighted average mass of an element's isotopes, calculated based on their natural abundances.

Isotopes

Atoms of the same element that have different numbers of neutrons and therefore different atomic masses.

Abundance

The relative occurrence of a particular isotope of an element, often expressed as a percentage.

(85Rb)

An isotope of rubidium with an atomic mass of 85.

(87Rb)

An isotope of rubidium with an atomic mass of 87.

(234U)

An isotope of uranium with an atomic mass of 234.

(235U)

An isotope of uranium with an atomic mass of 235.

(238U)

An isotope of uranium with an atomic mass of 238.

Average atomic mass of Rubidium

85.556 amu, calculated using the abundances of its isotopes.

Average atomic mass of Uranium

237.9783 amu, calculated using the abundances of its isotopes.

Average atomic mass of Titanium

47.923 amu, calculated from the weighted contributions of its isotopes.

Why do isotopes exist?

Atoms have different isotopes due to varying numbers of neutrons.