Everything about Actinides totally explained
The
actinoid (according to IUPAC terminology) (previously
actinide) series encompasses the 15
chemical elements that lie between
actinium and
lawrencium included on the
periodic table, with
atomic numbers 89 - 103. The actinoid series derives its name from the first element in the series, actinium, and ultimately from the
Greek ακτις (
aktis), "ray," reflecting the elements' radioactivity.
The actinoid series (
An) is included in some definitions of the
rare earth elements.
IUPAC is currently recommending the name
actinoid rather than actinide, as the suffix "-ide" generally indicates
ions (moreover, from
Latin, the suffix -ide means
"sons of actinium", while -oid means
"similar to actinium"). There are alternative arrangements of the periodic table that exclude actinium or lawrencium from appearing together with the other actinoids.
The actinoids display less similarity in their chemical properties than the
lanthanoid series (
Ln), exhibiting a wider range of
oxidation states, which initially led to confusion as to whether actinium, thorium, and uranium should be considered d-block elements. All actinoids are
radioactive.
Only thorium and uranium occur naturally in the earth's crust in anything more than trace quantities. Neptunium and plutonium have been known to show up naturally in trace amounts in uranium ores as a result of decay or bombardment. The remaining actinides were discovered in nuclear fallout, or were synthesized in particle colliders. The latter half of the series possess exceedingly short
half-lives.
The actinoids are typically placed below the main body of the periodic table (below the
lanthanoid series), in the manner of a footnote. The
full-width version of the periodic table shows the position of the actinoids more clearly.
An
organometallic compound of an actinoid is known as an
organoactinoid.
History of the actinoid series
From the earlier known chemical properties of actinium (89) up to uranium (92), indicating a relation to the
transition metals, it was generally assumed that the transuraniums would have similar qualities. During his
Manhattan Project research in
1944,
Glenn T. Seaborg experienced unexpected difficulty isolating americium (95) and curium (96). He began wondering if these elements more properly belonged to a different series than the transition metals, which would explain why the expected chemical properties of the new elements were different. In 1945, he went against the advice of colleagues and proposed the most significant change to
Mendeleev's
periodic table to have been accepted universally by the scientific community: the
actinide series.
In 1945, Seaborg published his
actinide concept of heavy element electronic structure, predicting that the actinides would form a transition series analogous to the rare earth series of lanthanoid elements.
In 1961, Antoni Przybylski discovered a
star that contained unusually high amounts of actinides.
Further Information
Get more info on 'Actinides'.
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