Chemists synthesize Fe-VI compound

[phantom power]

The form that the metal takes is dependent on the number of electrons in the iron atom's outermost shell, known as valence electrons (there are eight in an ordinary iron atom). Iron can occur in different ionized forms determined by the number of valence electrons, which are essential for forming chemical bonds with other atoms.

"The valence electrons of an ion are those mainly responsible for how the ion reacts," Berry explains.

The new species of iron found by Berry and his colleagues is designated iron VI, which means the atom has just two valence electrons and is highly reactive as it seeks to regain iron's eight-electron stable configuration by grabbing electrons from atoms of other elements. The new form is so reactive it can only be studied at low temperatures, in this case minus 40 degrees F.

(...)

"We hope that this complex will have practical advantages over other iron compounds, and we might expect that it does based on its structure," Berry says. "Whereas the ferrate ion easily transfers an oxygen atom to organic substrates, we might expect that our complex may transfer a nitrogen atom instead. This sort of reactivity is becoming more important in organic synthesis since it allows new synthetic pathways to nitrogen-containing organic molecules which are very important and have widespread utility."



http://www.sciencedaily.com/releases/2006/06/060601220415.htm

[JDPriestly]

1. Please translate for those of us who do not understand the

language of science.

[phantom power]

5. I'll take a stab (chemists, please set me straight)

First of all, that article goofed a bit. Iron does not "normally" have 8 electrons in it's outer shell. It's more common oxidation states are:

Fe-II (6 electrons), Fe-III (5 electrons) and Fe-IV (4 electrons).

Now, a lot of chemistry is driven by the fact that atoms "want" to have 8 electrons in their outer shell. In order to accomplish that, they can either take them (or give them) to another atom, in an ionic bond, or they can share them, in a covalent bond (organic chemistry, the kind that drives most biology, is mostly covalent bonds).

So, Fe-VI (if I'm reading that diagram right), is taking 6 electrons to complete it's shell, and it's got an ionic bond with 6 other atoms. In that compound it looks like 5 nitrogens and an oxygen.

What does it mean? It means that new kinds of chemical reactions are possible. What those are, I don't know. But it seems that they are interested in the reactions involving nitrogen.

[Kagemusha]

6. Thanks, I knew there was something fishy.

Only stuff with 8 electrons in the outer shell naturally are the inert gases... the reporter goofed there.

[Ready4Change]

8. A translation for Car Manufacturers.

A car made out of iron VI will rust out in half the time, thus increasing sales.

[Xipe Totec]

9. It is a good nitrogen donor

It is highly reactive, and likely to transfer a nitrogen atom in a chemical reaction. Thus, if someone is trying to construct a molecule that requires a nitrogen atom at a specific location, this compound may be the ideal donor reagent.

PS: Odd coincidence, your on-line name is the same of the discoverer of Oxygen.

http://www.woodrow.org/teachers/ci/1992/Priestley.html

[Kagemusha]

2. Widespread utility, but only useable at -40F?

(Well which is the same as -40C in this case...)

I'm curious what they plan to do with it.

Edit: Not that hardcore chem is my thing but, in English, it means that they've created a form of iron in a lab that wants to join with other substances very badly. Joining with oxygen produces plain old rust. Now if it joins with nitrogen instead, then it's.. different, and something else. And beyond that I'm waiting for details. ^^;

Sounds like if they tried studying it at room temperature it'd just turn to rust like, instantly.

[sutz12]

3. That means that they can handle the pure stuff at that temp

Once it is alloyed or bonded with other elements, I'm sure it could be used at normal temps. :)

It sounds very active, so that would indicate that at room temp it is difficult to keep it pure

[displacedtexan]

4. Whee! Let's all ride...

The Ferrous Wheel!

[eppur_se_muova]

7. This is a new compound of Iron(VI), but Iron(VI) is not new.

BaFeO4 and SrFeO4 have been known for some time and can be prepared on a fairly large scale. They are of interest as possible electrical cell ("battery") components; a few years ago a group (in Spain, IIRC) discovered that the instability of these two compounds, which made use in batteries impractical, was actually due to contamination by chloride. In the absence of chloride, they were much more stable. Haven't seen ferrate(VI) batteries yet.

K2FeO4 is being explored for use as a disinfectant. Google Ferrate(VI): http://www.google.com/search?hl=en&q=ferrate+%28VI%29&btnG=Google+Search

There is some evidence that an iron Fe(VI) species may have been known as far back as the Middle Ages, though obviously not recognized as such.