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Fluorine-18 (18F) is a fluorine radioisotope which is an important source of positrons. It has a mass of 18.0009380(6) u and its half-life is 109.771(20) minutes. It decays by positron emission 97% of the time and electron capture 3% of the time. Both modes of decay yield stable oxygen-18.

Fluorine-18,  18F
Fluorine-18 decay.svg
Decay over 24 hours
General
Name, symbolFluorine-18,18F
Neutrons9
Protons9
Nuclide data
Natural abundanceRadioisotope
Half-life109.771(20) min
Decay products18O
Isotope mass18.0009380(6) u
Spin1+
Excess energy873.431± 0.593 keV
Binding energy137369.199± 0.593 keV
Decay modes
Decay modeDecay energy (MeV)
Positron emission (97%)0.6335
Electron capture (3%)1.6555
Complete table of nuclides

Contents

SynthesisEdit

In the radiopharmaceutical industry, fluorine-18 is made using either a cyclotron or linear particle accelerator to bombard a target, usually of pure or enriched [18O]water [1] with high energy protons (typically ~18 MeV protons). The fluorine produced is in the form of a water solution of [18F]fluoride, which is then used in a rapid chemical synthesis of the radiopharmaceutical. The organic oxygen-18 pharmaceutical molecule is not made before the production of the radiopharmaceutical, as high energy protons destroy such molecules. Radiopharmaceuticals using fluorine must therefore be synthesized after the fluorine-18 has been produced.

ChemistryEdit

Fluorine-18 is often substituted for a hydroxyl group in a radiotracer parent molecule, due to similar steric and electrostatic properties. This may however be problematic in certain applications due to possible changes in the molecule polarity.

ApplicationsEdit

Fluorine-18 is one of the oldest tracers used in positron emission tomography (PET), having been in use since the 1960s.[2] Its significance is due to both its short half-life and the emission of positrons when decaying.

Tracers include sodium fluoride which can be useful for skeletal imaging as it displays high and rapid bone uptake accompanied by very rapid blood clearance, which results in a high bone-to-background ratio in a short time[3] and fluorodeoxyglucose (FDG), where the 18F substitutes a hydroxyl. New dioxaborolane chemistry enables radioactive fluoride (18F) labeling of antibodies, which allows for positron emission tomography (PET) imaging of cancer.[4]

ReferencesEdit

  1. ^ Fowler J. S. and Wolf A. P. (1982) The synthesis of carbon-11, fluorine-18 and nitrogen-13 labeled radiotracers for biomedical applications. Nucl. Sci. Ser. Natl Acad. Sci. Natl Res. Council Monogr. 1982.
  2. ^ Blau, Monte; Ganatra, Ramanik; Bender, Merrill A. (January 1972). "18F-fluoride for bone imaging". Seminars in Nuclear Medicine. 2 (1): 31–37. doi:10.1016/S0001-2998(72)80005-9.
  3. ^ Ordonez, A. A.; DeMarco, V. P.; Klunk, M. H.; Pokkali, S.; Jain, S.K. (October 2015). "Imaging Chronic Tuberculous Lesions Using Sodium [18F]Fluoride Positron Emission Tomography in Mice". Molecular Imaging and Biology. 17 (5): 609–614. doi:10.1007/s11307-015-0836-6. PMC 4561601. PMID 25750032.
  4. ^ Rodriguez, Erik A.; Wang, Ye; Crisp, Jessica L.; Vera, David R.; Tsien, Roger Y.; Ting, Richard (2016-04-27). "New Dioxaborolane Chemistry Enables [18F]-Positron-Emitting, Fluorescent [18F]-Multimodality Biomolecule Generation from the Solid Phase". Bioconjugate Chemistry. 27 (5): 1390–1399. doi:10.1021/acs.bioconjchem.6b00164. PMC 4916912. PMID 27064381.


Lighter:
fluorine-17
Fluorine-18 is an
isotope of fluorine
Heavier:
fluorine-19
Decay product of:
neon-18
Decay chain
of fluorine-18
Decays to:
oxygen-18