In their physical and chemical properties, actinium, thorium, protactinium, and uranium are respectively similar to lanthanum, hafnium, tantalum, and tungsten, and thus would seem to belong respectively to the third, fourth, fifth, and sixth columns of the periodic table. Only with neptunium does this horizontal progression (arguably) break down. So why aren't elements 89 to 92 distributed across columns 3 to 6 of the table?
Tell me more
×
Physics Stack Exchange is a question and answer site for
active researchers, academics and students of physics. It's 100% free, no registration required.
|
|
||||
|
|
The position of the Lanthanides and Actindes in the periodic table is due to their electronic orbital position. While the group number of an element does correlate with physical and chemical properties, it primarily informs you of the electronic configuration. In the case of elements 90-92, they have electrons in the f-orbital, so sit comfortably in the Actinides. Element 89 however is 'like' a group 3 element, with electrons only in s and d orbitals. Read-up here for more information. |
|||
|
