Fe-N Bond Energy in Heme Group of Haemoglobin

In summary, the bond energy and length of the coordinate covalent bond between Fe2+ and N in the heme group of hemoglobin can be found through various sources, including calculations and spectroscopy. The optimized Fe-N bond distances have been determined to be 1.61 Å and 1.74 Å for the doublet and quartet states, respectively, and the average Fe-N bond distance in ligated forms of hemoglobin and cytochrome c is known to be 1.98 A. Further information and resources can be found through research and analysis.
  • #1
fomenkoa
47
0
I've been searching far and wide and simply cannot find any info on the BOND ENERGY of a Fe- N coordinate-covalent bond, like that found in the heme group of haemoglobin.


it looks like this:
... N
... |
N -- Fe2+ -- N
... |
... N

The Fe2+ ion also has 2 coordination sites perpendicular to that plane.

Where can I possibly find the bond energy/length of those coordinate covalent bonds?

Anton
 
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  • #2
In addition, the calculations show a rather large difference in the short Fe-N bond distance, giving optimized Fe-N bond distances of 1.61 Å and 1.74 Å for the doublet and quartet states, respectively.
from http://www-ssrl.slac.stanford.edu/research/highlights_archive/fev.html

Abstract - Structure-function relations in hemoglobin as determined by x-ray absorption spectroscopy.
http://www.ncbi.nlm.nih.gov/entrez/query.fcgi?cmd=Retrieve&db=PubMed&list_uids=1061148&dopt=Abstract
The ligated forms of hemoglobin, and cytochrome c at high pH, gave spectra which were very similar to the bis-imidazole complex, where the average Fe-N bond distance is known to be 1.98 A. By comparison it was possible to determine that the average Fe-N bond distances were 1.99 A in oxyhemoglobin, 1.98 A in carbonmonoxyhemoglobin, and 1.98 A in cytochrome c at pH less than 10.5, with an experimental accuracy of +/-0.02 A.

Don't know if this is of use -
http://www.udel.edu/chem/bahnson/Chem641/chime/HemeFe_2.htm
 
  • #3
Wow thanks you are a research genius!

Anton
 

Related to Fe-N Bond Energy in Heme Group of Haemoglobin

1. What is the Fe-N bond energy in the heme group of hemoglobin?

The Fe-N bond energy in the heme group of hemoglobin refers to the strength of the bond between the iron (Fe) ion and the nitrogen (N) atom in the porphyrin ring. This bond is essential for the function of hemoglobin as it allows for the binding and release of oxygen molecules.

2. How is the Fe-N bond energy measured?

The Fe-N bond energy can be measured using techniques such as X-ray crystallography, nuclear magnetic resonance (NMR) spectroscopy, and infrared (IR) spectroscopy. These methods allow scientists to determine the distance between the Fe and N atoms and the strength of their bond.

3. What factors affect the Fe-N bond energy in the heme group of hemoglobin?

The Fe-N bond energy can be affected by several factors, including the oxidation state of the iron ion, the surrounding amino acid residues, and the presence of other molecules such as carbon monoxide or nitric oxide. Changes in these factors can alter the strength of the bond and impact the function of hemoglobin.

4. How does the Fe-N bond energy contribute to the function of hemoglobin?

The Fe-N bond energy is essential for the function of hemoglobin as it allows for the reversible binding and release of oxygen molecules. The strength of this bond helps to maintain the structural integrity of the heme group and ensures that oxygen can be efficiently transported throughout the body.

5. Can the Fe-N bond energy be altered by mutations in the heme group of hemoglobin?

Yes, mutations in the heme group of hemoglobin can alter the Fe-N bond energy. This can result in structural changes that affect the ability of hemoglobin to bind and release oxygen, leading to conditions such as sickle cell anemia or thalassemia. Understanding the Fe-N bond energy is crucial for studying these disorders and developing treatments.

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