Fluorine
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| Fluorine | |||||||||||||||||||||||||
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| General Info | |||||||||||||||||||||||||
| Atomic Symbol | F | ||||||||||||||||||||||||
| Atomic Number | 9 | ||||||||||||||||||||||||
| Atomic Weight | 18.9984 g/mol18.998 amu | ||||||||||||||||||||||||
| Chemical series | Halogens | ||||||||||||||||||||||||
| Appearance | Yellowish brown gas 
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| Group, Period, Block | 7, 2, p | ||||||||||||||||||||||||
| Electron configuration | 1s2 2s2 2p5 | ||||||||||||||||||||||||
| Electrons per shell | 2, 7 
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| CAS number | 7782-41-4 | ||||||||||||||||||||||||
| Physical properties | |||||||||||||||||||||||||
| Phase | gas | ||||||||||||||||||||||||
| Density | 0.0017 g/ml | ||||||||||||||||||||||||
| Melting point | 53.53 K-219.62 °C -363.316 °F 96.354 °R | ||||||||||||||||||||||||
| Boiling point | 85.03 K-188.12 °C -306.616 °F 153.054 °R | ||||||||||||||||||||||||
| Isotopes of Fluorine | |||||||||||||||||||||||||
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| All properties are for STP unless otherwise stated. | |||||||||||||||||||||||||
Fluorine (Latin: fluere, meaning "to flow") is the 9th element. Fluorine is poisonous gas,(toxic), and highly corrosive. It has a yellow-green tint to it. This element has high electronegativity and extremely reactive with other chemicals. It burns with a bright flame[1] It reacts with all organic and inorganic substances. When it reacts with water, it is very dangerous. Fluorine is very useful, so it is used for many things in our daily lives. For example, the toothpaste that we use everyday contains fluorine. Freon also contains fluorine. During World War II, America used 'uranium hexafluoride (UF6)' to separate the isotopes of Uranium to make the atomic bomb.
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Properties
Fluorine is in the halogens group. The atomic mass is 18.9984 g/mol. The natural phase of Fluorine is gas. The odor of Fluorine is somewhat in doubt. Fluorine's Electron configuration is 1s2 2s2 2p2. The melting point of Fluorine is -219.62℃ and the boiling point is -188℃. Fluorine is the most electronegative and reactive element on the periodic table, so it can be easily combined with any other element. Fluorine can react with noble gases such as krypton and xenon. The reaction can be explosive. The reaction is very dangerous especially with water. And when the temperature becomes high, it reacts stongly. In addition, because it is highly reactive, it also can react with hydrogen.
Compounds
Because Fluorine is one of the reactive element in the periodic table, it makes a lot of compounds with almost every element. The many forms of Chlorides, Bromides and Oxides are examples of compounds of Fluorine. There are many forms even within them; it can be "chlorine (I) fluoride", and "chlorine (II) fluoride".[2] Therefore, Fluorine has a very large number of compounds. Because of its unusual reactivity, Fluorine can react even with noble gases. Noble gases such as Xenon and Krypton, are not usually reactive due to their outer shell of electrons being full; they do not have much affinity to gain or lose an electron, so it is not common to react with noble gases. An aromatic ring is reactive, but if the Fluorine atom attached to it, the aromatic ring can be quite unreactive. It reduces reactivity of the molecule as a whole.
Occurrences
Fluorine can be found in many places, but the main areas where Fluorine is found is in China, Mexico, and Western Europe. About 4 million tons of Fluorine are produced annually. Mostly, Fluorine can be found in common rock forming minerals, including fluorite (CaF2). It occurs in both igneous and sedimentary rocks. It also occurs as minerals such as apatite, topaz, simple halides, also in silicates such as muscovite and a range of amphibole and mica minerals. Fluorine is the 13th most abundant element in the earth’s crust. Some soils can hold approximately 330 ppm of Fluorine. There are about 0.6 ppb of Fluorine present in the atmosphere.[3]
Uses
Because of the special properties of Fluorine, it can be used for many purposes. Fluoride (the ionic form of fluorine) is excellent against tooth decay. Fluoride covers teeth with thin layers, so it protects from forming cavities. In addition, Fluorine is very toxic, it kills bacteria in water, so many nations add Fluorine into the city water as a disinfectant. Hydrofluoric acid (HF) is used to etch glass, including most of the glass used in light bulbs. Crystals of calcium fluoride (CaF2), also known as fluorite and fluorspar, are used to make lenses to focus infrared light. Fluorides are ingredients in such household products as cleaning solutions for metal, tile, brick, and cement. During World War II, America wanted to make the Atomic bomb. To make it, scientists needed to separate some isotopes of uranium. To separate the isotopes, the uranium was processed as 'uranium hexafluoride (UF6)'.[4] Fluorine(dichlorodifluoromethane (CF2C2)), is also used in the manufacture of Freon, which is used in the refrigerator. Unfortunately, freon stays in the atmosphere for a long time and reacts with ozone, decreasing the Ozone layer. [5]
Isotopes
- Main Article: Isotopes
Although fluorine (F) has multiple isotopes, only one of these isotopes is stable; as such, it is considered a monoisotopic element. Standard atomic mass: 18.9984032(5) u
The main isotopes of Fluorine are 18F, 19F. The nuclide 18F is an important source of positrons. The natural abundance for 19F is 100% and 18F is 0%. 19F is stable and half-life of 18F is 109.7 mins. Several other isotopes have been discovered ranging in a variety of different half-lifes
Table
| nuclide symbol | Z(p) | N(n) | isotopic mass (u) | half-life | nuclear spin | representative isotopic composition (mole fraction) | range of natural variation (mole fraction) |
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| excitation energy | |||||||
| 14F | 9 | 5 | 14.03506(43)# | 2-# | |||
| 15F | 9 | 6 | 15.01801(14) | 410(60)E-24 s [1.0(2) MeV] | (1/2+) | ||
| 16F | 9 | 7 | 16.011466(9) | 11(6)E-21 s [40(20) keV] | 0- | ||
| 17F | 9 | 8 | 17.00209524(27) | 64.49(16) s | 5/2+ | ||
| 18F | 9 | 9 | 18.0009380(6) | 109.771(20) min | 1+ | ||
| 18mF | 1121.36(15) keV | 162(7) ns | 5+ | ||||
| 19F | 9 | 10 | 18.99840322(7) | STABLE | 1/2+ | 1.0000 | |
| 20F | 9 | 11 | 19.99998132(8) | 11.163(8) s | 2+ | ||
| 21F | 9 | 12 | 20.9999490(19) | 4.158(20) s | 5/2+ | ||
| 22F | 9 | 13 | 22.002999(13) | 4.23(4) s | 4+,(3+) | ||
| 23F | 9 | 14 | 23.00357(9) | 2.23(14) s | (3/2,5/2)+ | ||
| 24F | 9 | 15 | 24.00812(8) | 400(50) ms | (1,2,3)+ | ||
| 25F | 9 | 16 | 25.01210(11) | 50(6) ms | (5/2+)# | ||
| 26F | 9 | 17 | 26.01962(18) | 9.6(8) ms | 1+ | ||
| 27F | 9 | 18 | 27.02676(40) | 4.9(2) ms | 5/2+# | ||
| 28F | 9 | 19 | 28.03567(55)# | <40 ns | |||
| 29F | 9 | 20 | 29.04326(62)# | 2.6(3) ms | 5/2+# | ||
| 30F | 9 | 21 | 30.05250(64)# | <260 ns | |||
| 31F | 9 | 22 | 31.06043(64)# | 1# ms [>260 ns] | 5/2+# | ||
From Wikipedia [6]
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