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Non Life Sciences => Chemistry => Topic started by: pluvam on 19/09/2009 22:15:02

Title: Why do some transition metals have variable oxidation numbers?
Post by: pluvam on 19/09/2009 22:15:02

I know that the answer lies in their electron configurations but what exactly?

For example Fe, Fe(+2) and Fe(+3)

And also how do i know which oxidation number is the most common for any transition metal?

Thanks for any help

Title: Why do some transition metals have variable oxidation numbers?
Post by: Chemistry4me on 20/09/2009 00:53:59

The various oxidation states correspond to the involvement of the 4s and unpaired 3d electrons in transition metals. For example, Mn has 5 unpaired 3d electrons and two 4s electrons. It's highest oxidation state is +7 when it uses all seven of these electrons. Then there is Mn²⁺ which is +2 and it has lost the two 4s electrons. In between all theses you have, MnCl₂ (+2), Mn₂O₃ (+3), MnO₂ (+4), +5 can't think of one [:-X], and MnO₄^2- (+6). There is also +1 which is not very common. All of these have different numbers of electrons involved in bonding hence the different oxidation states.

Title: Why do some transition metals have variable oxidation numbers?
Post by: yor_on on 23/10/2009 03:47:26

nice explanation.
Ah, just what is transition metal's?

Title: Why do some transition metals have variable oxidation numbers?
Post by: EvilFrog on 23/10/2009 16:08:33

transition metals are the elements in between group 2 to group 3(i mean between the group that start with Be to the group that start with B). can i say like that? Is it an explanation?

Title: Why do some transition metals have variable oxidation numbers?
Post by: yor_on on 04/11/2009 19:41:18

Possibly :)

But chemistry is a field if its own