Question

What are the common (usual) oxidation states of the Lanthanides??

Answer 1

+3

Answer 2

http://www.chem.ox.ac.uk/icl/heyes/LanthAct/A7.html

Answer 3

umm pls give me a good table
like +2 -> [lanthanides]
then +3 -> [lanthanides]
etc..

Answer 4

sorry the link was for the actinides :P let me find something for lanth

Answer 5

I see they both exhibit a common oxidation state of +3

Answer 6

yeah.. i know that.. i require a detailed table of naturally occuring stable oxidation states of the Lanthanides..

Answer 7

Oke gimme a few minutes, i'll make a table

Answer 8

ookay..

Answer 9

for most of the lanthanides the ionsiation energy to lose a fourth electron will be so large that it cannot be compensated for by bond formation,this is due to the 4f electrons which are shielded and can be regarded as "core electrons".in general it can be said that I4~2(I3)~4(I2)~8(I1)

however for Eu and Yb +2 will be the favoured O.S. due to the presence of a half filled(7e) and a filled 4f shell(14e) respectively

the +4 oxidation state is also possible

Answer 10

tks.. it was known.. Lanthanides, for this reason, also form chelting complexes only..

Answer 11

Ion
La3+ Tb3+
Ce3+ Dy3+
Pr3+ Ho3+
Nd3+ Er3+
Pm3+ Tm3+
Sm3+ Yb3+
Eu3+ Lu3+
Gd3+

Answer 12

every lanthanide element forms a +3 oxidation state which is
very stable to oxidation or reduction. In keeping with its stability, this oxidation state is
very easily made. For example, the metals all dissolve readily in acid to form tri-positive
aqueous ions. But going beyond +3 is very difficult. There are a few scattered examples
of the +4 state, cerium(IV) being much the most stable example, but oxidation states of five or above have never been made.

Answer 13

yeah so please post all possible stable oxidation states..
thanks for the effort

Answer 14

\(
\begin{array}{|c|c|c|c|c|c|c|c|c|c|c|c|c|c|c|c|}
\hline
\sf 4&&X&X&&&X&&&X&&&&X&\\
\hline
\sf 3&X&X&X&X&X&X&X&X&X&X&X&X&X&X&X\\
\hline
\sf 2&X&X&X&X&&X&X&X&X&X&X&X&X&X&X\\
\hline
\sf 1&&X&&X&&X&X&X&X&X&X&X&&X&X\\
\hline
&\sf La&\sf Ce&\sf Pr&\sf Nd&\sf Pm&\sf Sm&\sf Eu&\sf Gd&\sf Tb&\sf Dy&\sf Ho&\sf Er&\sf Tm&\sf Yb&\sf Lu\\
\hline

\end{array}\)