ELEMENTS atomic number = Z = number of protons = p mass number = number of nucleons = p + n atomic mass = experimental measurement of the mass of the.

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Presentation transcript:

ELEMENTS atomic number = Z = number of protons = p mass number = number of nucleons = p + n atomic mass = experimental measurement of the mass of the element

ISOTOPES same element with different masses change number of neutrons stable and radioactive

RADIOACTIVITY The simultaneous decay of one element usually into another element with the emission of energy and usually a decay particle. The decay particle and energy are released from the nucleus. The decay particle is a very high energy particle (emitted at high velocity and can cause great damage).

THE CHEMICAL ELEMENTS

THE STABLE ISOTOPES

COSMIC ABUNDANCE OF THE ELEMENTS extreme abundance of hydrogen and helium from the big bang general decrease in abundance with increasing atomic number (Z) some low abundance (Li, Be, B) and some high (Fe, Ni, Pb) greater abundance of even Z than odd Z elements

IMPORTANT EXOTHERMIC NUCLEAR PROCESSES  splitting of the atom  heavy elements  examples- U, Pu  U.S. commercial nuclear reactors Fusion  joint two atoms  light elements  examples- H, He, Li  Sun’s energy source Fission

BINDING ENERGY

IRON High cosmic abundance Highest binding energy per nucleon A very stable nuclide in the solar system