Histidine

Not to be confused with histamine.
L-Histidine
Names
IUPAC name
Histidine
Other names
2-Amino-3-(1H-imidazol-4-yl)propanoic acid
Identifiers
71-00-1 Yes
ChEBI CHEBI:57595 Yes
ChEMBL ChEMBL17962 Yes
ChemSpider 6038 Yes
DrugBank DB00117 Yes
Jmol-3D images Image
KEGG D00032 Yes
PubChem 773
UNII 4QD397987E Yes
Properties
Molecular formula
 C6H9N3O2
Molar mass 155.15 g·mol−1
4.19g/100g @ 25 °C [1]
Hazards
MSDS External MSDS
NFPA 704
Flammability code 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g., canola oil Health code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentine Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
1
1
0
Supplementary data page
Refractive index (n),
Dielectric constant (εr), etc.
Thermodynamic
data
 Phase behaviour
solid–liquid–gas
UV, IR, NMR, MS
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Histidine (abbreviated as His or H)[2] is an α-amino acid with an imidazole functional group. It is one of the 23 proteinogenic amino acids. Its codons are CAU and CAC. Histidine was first isolated by German physician Albrecht Kossel in 1896. Histidine is an essential amino acid in humans and other mammals. It was initially thought that it was only essential for infants, but longer-term studies established that it is also essential for adult humans.[3]

Chemical properties

The conjugate acid (protonated form) of the imidazole side chain in histidine has a pKa of approximately 6.0. This means that, at physiologically relevant pH values, relatively small shifts in pH will change its average charge. Below a pH of 6, the imidazole ring is mostly protonated as described by the Henderson–Hasselbalch equation. When protonated, the imidazole ring bears two NH bonds and has a positive charge. The positive charge is equally distributed between both nitrogens and can be represented with two equally important resonance structures.

Aromaticity

The imidazole ring of histidine is aromatic at all pH values.[4] It contains six pi electrons: four from two double bonds and two from a nitrogen lone pair. It can form pi stacking interactions,[5] but is complicated by the positive charge.[6] It does not absorb at 280 nm in either state, but does in the lower UV range more than some amino acids.[7][8]

Biochemistry

The imidazole sidechain of histidine is a common coordinating ligand in metalloproteins and is a part of catalytic sites in certain enzymes. In catalytic triads, the basic nitrogen of histidine is used to abstract a proton from serine, threonine, or cysteine to activate it as a nucleophile. In a histidine proton shuttle, histidine is used to quickly shuttle protons. It can do this by abstracting a proton with its basic nitrogen to make a positively charged intermediate and then use another molecule, a buffer, to extract the proton from its acidic nitrogen. In carbonic anhydrases, a histidine proton shuttle is utilized to rapidly shuttle protons away from a zinc-bound water molecule to quickly regenerate the active form of the enzyme. Histidine is also important in haemoglobin in helices E and F. Histidine assists in stabilising oxyhaemoglobin and destabilising CO-bound haemoglobin. As a result, carbon monoxide binding is only 200 times stronger in haemoglobin, compared to 20,000 times stronger in free haem.

Certain amino acids can be converted to intermediates of the TCA cycle. Carbons from four groups of amino acids form the TCA cycle intermediates α-ketoglutarate, succinyl CoA, fumarate, and oxaloacetate. Amino acids that form α-ketoglutarate are glutamate, glutamine, proline, arginine, and histidine. Histidine is converted to formiminoglutamate (FIGLU). The formimino group is transferred to tetrahydrofolate, and the remaining five carbons form glutamate. Glutamate can be deaminated by glutamate dehydrogenase or transaminated to form α-ketoglutarate.[9]

NMR

When protonated, the 15N chemical shifts of the side-chain nitrogens are similar (about 200 ppm, relative to nitric acid on the sigma scale, on which increased shielding corresponds to increased chemical shift). As the pH increases past approximately 6, the protonation of the imidazole ring is lost. The remaining proton of the now-neutral imidazole can exist on either nitrogen, giving rise to what is known as the N-1 or N-3 tautomers. NMR shows that the chemical shift of N-1 drops slightly, whereas the chemical shift of N-3 drops considerably (about 190 vs. 145 ppm). This indicates that the N-1-H tautomer is preferred, it is presumed due to hydrogen bonding to the neighboring ammonium. The shielding at N-3 is substantially reduced due to the second-order paramagnetic effect, which involves a symmetry-allowed interaction between the nitrogen lone pair and the excited pi* states of the aromatic ring. As the pH rises above 9, the chemical shifts of N-1 and N-3 become approximately 185 and 170 ppm. It is worth noting that the deprotonated form of imidazole, imidazolate ion, would be formed only above a pH of 14, and is therefore not physiologically relevant. This change in chemical shifts can be explained by the presumably decreased hydrogen bonding of an amine over an ammonium ion, and the favorable hydrogen bonding between a carboxylate and an NH. This should act to decrease the N-1-H tautomer preference.[10]

Metabolism

The amino acid is a precursor for histamine and carnosine biosynthesis.

Conversion of histidine to histamine by histidine decarboxylase

The enzyme histidine ammonia-lyase converts histidine into ammonia and urocanic acid. A deficiency in this enzyme is present in the rare metabolic disorder histidinemia. In Actinobacteria and filamentous fungi, such as Neurospora crassa, histidine can be converted into the antioxidant ergothioneine.[11]

Supplementation

Supplementation of histidine has been shown to cause rapid zinc excretion in rats with an excretion rate 3 to 6 times normal.[12][13]

Additional images

See also

References

  1. ↑ http://prowl.rockefeller.edu/aainfo/solub.htm[]
  2. ↑ IUPAC-IUBMB Joint Commission on Biochemical Nomenclature. "Nomenclature and Symbolism for Amino Acids and Peptides". Recommendations on Organic & Biochemical Nomenclature, Symbols & Terminology etc. Retrieved 2007-05-17.
  3. ↑ Kopple, J D; Swendseid, M E (1975). "Evidence that histidine is an essential amino acid in normal and chronically uremic man". Journal of Clinical Investigation 55 (5): 881–91. doi:10.1172/JCI108016. PMC 301830. PMID 1123426.
  4. ↑ Mrozek, Agnieszka; Karolak-Wojciechowska, Janina; Kieć-Kononowicz, Katarzyna (2003). "Five-membered heterocycles. Part III. Aromaticity of 1,3-imidazole in 5+n hetero-bicyclic molecules". Journal of Molecular Structure 655 (3): 397. doi:10.1016/S0022-2860(03)00282-5.
  5. ↑ Wang, Lijun; Sun, Na; Terzyan, Simon; Zhang, Xuejun; Benson, David R. (2006). "A Histidine/Tryptophan π-Stacking Interaction Stabilizes the Heme-Independent Folding Core of Microsomal Apocytochrome b5Relative to that of Mitochondrial Apocytochrome b5". Biochemistry 45 (46): 13750–9. doi:10.1021/bi0615689. PMID 17105194.
  6. ↑ Blessing, Robert H.; McGandy, Edward L. (1972). "Base stacking and hydrogen bonding in crystals of imidazolium dihydrogen orthophosphate". Journal of the American Chemical Society 94 (11): 4034. doi:10.1021/ja00766a075.
  7. ↑ Katoh, Ryuzi (2007). "Absorption Spectra of Imidazolium Ionic Liquids". Chemistry Letters 36 (10): 1256. doi:10.1246/cl.2007.1256.
  8. ↑ A. Robert Goldfarb; Saidel, LJ; Mosovich, E (1951-11-01). "The Ultraviolet Absorption Spectra of Proteins". Journal of Biological Chemistry 193 (1): 397–404. PMID 14907727.
  9. ↑ Board review series (BRS)-- Biochemistry, Molecular Biology, and Genetics (fifth edition): Swanson, Kim, Glucksman
  10. ↑ Roberts, John D. (2000). ABCs of FT-NMR. Sausalito, CA: University Science Books. pp. 258–9. ISBN 978-1-891389-18-4.
  11. ↑ Fahey, Robert C. (2001). "Novelthiols Ofprokaryotes". Annual Review of Microbiology 55: 333–56. doi:10.1146/annurev.micro.55.1.333. PMID 11544359.
  12. ↑ R M Freeman; Taylor, PR (1977-04-01). "Influence of histidine administration on zinc metabolism in the rat". The American Journal of Clinical Nutrition 30 (4): 523–7. PMID 851080.
  13. ↑ Wensink, Jan; Hamer, Cornelis J. A. (1988). "Effect of excess dietary histidine on rate of turnover of65Zn in brain of rat". Biological Trace Element Research 16 (2): 137–50. doi:10.1007/BF02797098. PMID 2484542.

External links