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Questions and Answers
Isotopes have the same number of protons but different numbers of electrons.
Isotopes have the same number of protons but different numbers of electrons.
False
The atomic mass of an element is solely based on the mass of protons in its nucleus.
The atomic mass of an element is solely based on the mass of protons in its nucleus.
False
The atomic mass unit (amu) is defined as 1/12 of the mass of one atom of hydrogen-1.
The atomic mass unit (amu) is defined as 1/12 of the mass of one atom of hydrogen-1.
False
Determining average atomic mass involves multiplying the exact atomic mass by its percent of natural abundance.
Determining average atomic mass involves multiplying the exact atomic mass by its percent of natural abundance.
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An atom's nuclear composition includes only protons since neutrons are not fixed within the nucleus.
An atom's nuclear composition includes only protons since neutrons are not fixed within the nucleus.
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Study Notes
Nucleus
- The nucleus of an atom contains protons and neutrons.
- The number of neutrons can vary for most elements.
Isotopes
- Atoms with the same number of protons (atomic number) but different numbers of neutrons are called isotopes.
Atomic Mass
- The atomic mass of an element is the average mass of its naturally occurring isotopes.
- To calculate average atomic mass, multiply the exact atomic mass of each isotope by its percent natural abundance and sum the results.
Atomic Mass Unit (amu)
- The relative masses of atoms are reported in atomic mass units (amu).
- 1 amu is defined as 1/12 of the mass of a single carbon-12 atom.
- Carbon-12 has 6 protons, 6 neutrons, and 6 electrons.
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Description
Explore the fundamental concepts of atomic structure, including the roles of protons, neutrons, and isotopes. This quiz covers atomic mass calculations and the significance of atomic mass units. Test your knowledge of how these concepts interplay within chemistry.
