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- What is the electronic configuration of Fe(II) ion?
The electronic configuration of Fe is [Ar] 3dX6 4sX2 [A r] 3 d X 6 4 s X 2 So after removing two electrons the configuration becomes: [Ar] 3dX6 [A r] 3 d X 6 But why can't the electrons rearrange themselves to give a more stable [Ar] 3dX5 4sX1 [A r] 3 d X 5 4 s X 1 configuration?
- Differences between Fe3+ and Fe2+ - Chemistry Stack Exchange
For eg , Fe2+ F e 2 + forms a red-orange compound with amine lignads Fe3+ F e 3 + forms blood red solution with thiocyanate ions, which is used as fake blood in movies, dramas and so on Ferrous ions normally have paramagnetic properties, but can become diamagnetic due to the formation of low-spin complexes
- About Fe (III) and Fe (II) coordination complexes
Why does Fe(III) form octahedral coordination complexes if it has 5 electrons in its d-orbitals? I understand that Fe(II) has 6 electrons in its d-orbitals and 6 lone pairs from 6 ligands as the 12
- Why Fe 3+ is more common than Fe 2+ - Chemistry Stack Exchange
I heard that Fe(III) F e (I I I) is more common than Fe(II) F e (I I) but I've not heard a very clear explanation Could someone please explain this incorporating electron configurations in their answer?
- Is there an iron–iron bond in diiron nonacarbonyl?
Diiron nonacarbonyl, $\\ce{[Fe2(CO)9]}$, is often depicted with an Fe–Fe bond as shown at the left-hand side: The Fe—Fe bond is usually invoked in order to (1) explain the observed diamagnetism and
- inorganic chemistry - Is iron (III) carbonate stable in water . . .
The resulting precipitate is sometimes written as FeX2OX3 ⋅aq F e X 2 O X 3 a q Adding an excess of sodium carbonate solution may lead to the formation of HCOX3X− H C O X 3 X ions in the resulting solution Explanation Iron (III) carbonate is a weak electrolyte since it is formed by a weak acid and a weak base so it gets readily hydrolysed especially in the presence of a mineral acid:
- Why do iron (II) ions and chromium have different electronic . . .
What I don't understand: I know [Ar] 3dX6 [A r] 3 d X 6 is correct for iron (II), but I don't understand why Why don't iron ions adjust themselves as Cr does to achieve the extra stability? Is it because, in this case, it needs to excite an electron to an orbital of higher energy, whereas, in Cr, the 4s electron just moves down to an orbital of lower energy?
- Why is Cr(2+) a stronger reducing agent than Fe(2+) in water?
According to me, F e X 2 + should be a better reducing agent because F e X 2 + - after being oxidized - will attain a stable d X 5 configuration, whereas C r X 2 + will attain a d X 3 configuration I think the half filled d X 5 configuration is more stable than the d X 3 configuration Why is this not so?
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