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With a density of 12 g/cm 3, americium is less dense than both curium (13.52 g/cm 3) and plutonium (19.8 g/cm 3); but has a higher density than europium (5.264 g/cm 3)—mostly because of its higher atomic mass. Americium is relatively soft and easily deformable and has a significantly lower bulk modulus than the actinides before it: Th, Pa, U ...
Americium-242m has a mass of 242.0595492 g/mol. It is one of the rare cases, like 108m Ag, 166m Ho, 180m Ta, 186m Re, 192m Ir, 210m Bi, 212m Po and others, where a higher-energy nuclear isomer is more stable than the ground state, americium-242. [11] 242m Am is fissile with a low critical mass, comparable to that of 239 Pu. [12]
{{Infobox element}}; labels & notes: (Image) GENERAL PROPERTIES Name Symbol Pronunciation (data central) Alternative name(s) Allotropes Appearance <element> IN THE PERIODIC TABLE Periodic table Atomic number Standard atomic weight (data central) Element category (also header bg color) (sets header bg color, over 'series='-color) Group Period ...
This is a list of chemical elements and their atomic properties, ordered by atomic number (Z). Since valence electrons are not clearly defined for the d-block and f-block elements, there not being a clear point at which further ionisation becomes unprofitable, a purely formal definition as number of electrons in the outermost shell has been used.
A chemical element, often simply called an element, is a type of atom which has a specific number of protons in its atomic nucleus (i.e., a specific atomic number, or Z). [ 1 ] The definitive visualisation of all 118 elements is the periodic table of the elements , whose history along the principles of the periodic law was one of the founding ...
Americium-241 has a specific activity of 3.43 Ci/g (126.91 GBq/g). [3] It is commonly found in the form of americium-241 dioxide (241 AmO 2). This isotope also has one meta state, 241m Am, with an excitation energy of 2.2 MeV (0.35 pJ) and a half-life of 1.23 μs.
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In chemistry, the whole number rule states that the masses of the isotopes are whole number multiples of the mass of the hydrogen atom. [1] The rule is a modified version of Prout's hypothesis proposed in 1815, to the effect that atomic weights are multiples of the weight of the hydrogen atom. [ 2 ]