The position of each element in the table gives important information about its structure, properties, and behavior in chemical reactions. Diagram Radioisotopes Isotopes that emit, or kick out, subatomic particles to reach a more stable, lower-energy, configuration Decay the process in which radioisotopes release particles and energy Isotope's Half-Life the period over which half of the material will decay to a different, relatively stable product Purpose of the Periodic Table Similar to a filing system.
The relative atomic masses given in periodic table entries-like the one for hydrogen, below-are calculated for all the naturally occurring isotopes of each element, weighted by the abundance of those isotopes on earth. Relative Atomic Mass an average of the atomic masses of all the different isotopes in a sample, with each isotope's contribution to the average determined by how big a fraction of the sample it makes up. In general, an atom's atomic mass will be very close to its mass number, but will have some deviation in the decimal places. By definition, an atom of carbon with six neutrons, carbon-12, has an atomic mass of 12 amu. Atomic Mass The atomic mass of a single atom is simply its total mass and is typically expressed in atomic mass units or amu.
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