fluorine isotope with 10 neutrons

The least stable is 29Ar with a half-life of approximately 4×10−20 seconds. number of protons identifies the element to be fluorine (F). [2] The half-life of 26mF is 2.2(1) milliseconds; it decays mainly to the ground state of 26F or (rarely, via beta-minus decay) to one of high excited states of 26Ne with delayed neutron emission. It has a half-life of 4.158 seconds. Its abundance is 100%; no other isotopes of fluorine exist in significant quantities. Its half-life has been determined to be approximately 150 years, and it decays by beta emission to 32P and then to 32S. Its major value is in the production of the radiopharmaceutical fludeoxyglucose, used in positron emission tomography in medicine. Its specific radioactivity is 4.78 × 109 TBq/g. [6] Fluorine-19.

With the exception of those two, all other isotopes have half-lives under a minute, most under a second. There are 13 radioisotopes that have been discovered, with mass numbers from 7 to 21, all with short half-lives, the longest being that of 8B, with a half-life of only 770 milliseconds (ms) and 12B with a half-life of 20.2 ms. All other isotopes have half-lives shorter than 17.35 ms. Those isotopes with mass below 10 decay into helium while those with mass above 11 mostly become carbon. The longest-lived is 24Ne with a half-life of 3.38 minutes. Fluorine-21, as with fluorine-20, is also one of unstable isotopes of this element. The longest-lived radioisotope is 18F; it has a half-life of 109.739 minutes. On the Earth, 40Ar makes up 99.6% of natural argon. Because in each fluorine nucleus, there are necessarily "9 protons", why necessarily?, there must be 10 neutrons, neutral massive particles, in the fluorine nucleus. 24.56 amu. Fluorine-19 is NMR-active with spin of 1/2, so it is used in fluorine-19 NMR spectroscopy. How do isotopes of carbon differ from one another? The least stable is 25P with a half-life shorter than 30 nanoseconds. Silicon (14Si) has 23 known isotopes, with mass numbers ranging from 22 to 44. Tables, graphs, and references", https://en.wikipedia.org/w/index.php?title=Isotopes_of_fluorine&oldid=972131413#Fluorine-18m, Creative Commons Attribution-ShareAlike License, This page was last edited on 10 August 2020, at 09:55. All other isomers have half-lives under a year, most under a day. Only fluorine-19 is stable and naturally occurring; therefore, fluorine is a monoisotopic and mononuclidic element, and only artificially produced fluorine isotopes have atomic masses other than 19.

In either case, 18F decays into 18O. Like all positron-emitting radioisotopes, 18F also may decay by electron capture. Fluorine (9 F) has 17 known isotopes, with atomic masses ranging from 14 F to 31 F (with the exception of 30 F), and two isomers (18m F and 26m F). The least stable isotope is 8C, with a half-life of 2.0 x 10−21 s. Boron (5B) naturally occurs as isotopes 10B and 11B, the latter of which makes up about 80% of natural boron. After 32Si, 31Si has the second longest half-life at 157.3 minutes. Three of those isotopes occur naturally: the two stable forms 39K (93.3%) and 41K (6.7%), and a very long-lived radioisotope 40K (0.012%). 28Si, 29Si (4.67%), and 30Si (3.1%) are stable. For this reason 18F is a commercially important source of positrons. The longest-lived radioisotope is 18F; it has a half-life of 109.739 minutes. Only two nuclear isomers (long-lived excited nuclear states), fluorine-18m and fluorine-26m, have been characterized.

This is also the only carbon radioisotope found in nature—trace quantities are formed cosmogenically by the reaction 14N + 1n → 14C + 1H. Oxygen is composed of three isotopes 16/8 O (15.995 u), 17/8 O (16.999 u) and 18/8 O (17.999 u).... Copper is listed on the periodic table as having a relative atomic mass of 63.55.

[6]. Its abundance is 100%; no other isotopes of fluorine exist in significant quantities. It has two decay modes, of which the main one is positron emission.

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