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Germanium is a chemical element; it has symbol Ge and atomic number 32. ... At least 27 radioisotopes have also been synthesized, ranging in atomic mass from 58 to 89.
Average atomic mass Electronegativity (Pauling) First Ionization Energy Radii Valence electrons; Atomic ... Germanium: Ge: 72.63(1) 2.01: 7.8994: 125 ...
Germanium (32 Ge) has five naturally occurring isotopes, 70 Ge, 72 Ge, 73 Ge, 74 Ge, and 76 Ge. Of these, 76 Ge is very slightly radioactive, decaying by double beta decay with a half-life of 1.78 × 10 21 years [4] (130 billion times the age of the universe). Stable 74 Ge is the most common isotope, having a natural abundance of approximately 36%.
The atomic mass (relative isotopic mass) is defined as the mass of a single atom, which can only be one isotope (nuclide) at a time, and is not an abundance-weighted average, as in the case of relative atomic mass/atomic weight. The atomic mass or relative isotopic mass of each isotope and nuclide of a chemical element is, therefore, a number ...
It contains a table of main isotopes and eventually the standard atomic weight. This template is reused in {{Infobox <element>}} as a child Infobox (|child=yes). As of Jan 2023, a 'Main isotope' is conforming MOS:MAINISOTOPE (under construction, see WP:ELEMENTS What is a "Main_isotope"?) Each isotope has its own row, with decay modes:
Its first ionization energy should be about 400 kJ/mol and its metallic radius approximately 170 picometers. With a relative atomic mass of around 445 u, [4] it should be a very heavy metal with a density of around 26 g/cm 3.
The standard atomic weight (A r °(Cu)) for copper is the average, weighted by their natural abundance, and then divided by the atomic mass constant m u. [ 1 ] The standard atomic weight of a chemical element (symbol A r °(E) for element "E") is the weighted arithmetic mean of the relative isotopic masses of all isotopes of that element ...
The standard atomic weight (commonly called "atomic weight") of an element is the average of the atomic masses of all the chemical element's isotopes as found in a particular environment, weighted by isotopic abundance, relative to the atomic mass unit.