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fluorine    音标拼音: [fl'ʊr,in] [fl'ɔr,in]
n. 氟[非金属元素]

氟[非金属元素]

fluorine
n 1: a nonmetallic univalent element belonging to the halogens;
usually a yellow irritating toxic flammable gas; a powerful
oxidizing agent; recovered from fluorite or cryolite or
fluorapatite [synonym: {fluorine}, {F}, {atomic number 9}]

Fluorine \Flu"or*ine\ (fl[=u]"[o^]r*[i^]n or fl[=u]"[o^]r*[=e]n;
104), n. [NL. fluorina: cf. G. fluorin, F. fluorine. So
called from its occurrence in the mineral fluorite.] (Chem.)
A non-metallic, gaseous element of atomic number 9, strongly
acid or negative, and associated with chlorine, bromine, and
iodine, in the halogen group of which it is the first member.
It always occurs combined, is very active chemically, and
possesses such an avidity for most elements, and silicon
especially, that it can neither be prepared nor kept in glass
vessels, but may be contained in lead vessels. If set free it
immediately attacks a containing glass vessel, so that it was
not isolated until 1886. It is a pungent, corrosive,
colorless gas. Symbol F. Atomic weight 19.00.
[1913 Webster]

Note: Fluorine unites with hydrogen to form hydrofluoric
acid, which is the agent employed in etching glass. It
occurs naturally, principally combined as calcium
fluoride in fluorite, and as a double fluoride of
aluminium and sodium in cryolite.
[1913 Webster]


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  • inorganic chemistry - Why is fluorine the most electronegative atom . . .
    Fluorine has a high electron affinity (easy to gain an electron) and a high ionization energy (hard to lose an electron) There are other scales, including the Allred-Rochow scale , based on effective nuclear charge and covalent radius , the Sanderson scale based on atomic size, and the Allen scale based on the average energy of the valence
  • inorganic chemistry - Why is fluorine more reactive than chlorine . . .
    Fluorine molecule has a small atomic radius with 5 electron in 2p orbital This means it has a high charge density on its atom When fluorine molecule breaks up into F- ions it remains highly unstable and just wants to bond with other element Due to this charge density fluorine has high polarizability which makes it more reactive
  • inorganic chemistry - Why doesnt fluorine harm the ozone layer the way . . .
    Fluorine atoms released are quickly sequestered into carbonyl compounds and subsequently into hydrogen fluoride by reacting with water and methane molecules which is very stable in the stratosphere As such, CFCs are now being replaced with Hydrofluorocarbons (HFCs) according to Montreal protocol (but they do contribute to global warming)
  • halides - Can fluorine ever have a positive oxidation state . . .
    Rather, the gold is bonded octahedrally to five individual fluorine atoms and a difluorine ($\ce{F2}$) ligand, the latter attached end on and rotated so that in the most stable conformation (according to most of the several optimization schemes used), the remote fluorine atom is eclipsed with one of the other ligands as if attracted to it (a
  • Spontaneity and nature of attack of fluorine gas on aluminum
    Fluorine is one of the most dangerous substances out there, and one of the presumed products, $\ce{OF2}$, is also terrifying If you can calculate the free energy change for a reaction, you will know whether it is spontaneous
  • Is F2 two fluoride ions or just one? - Chemistry Stack Exchange
    A fluorine atom can share electrons with another nonmetal to form a covalent bond When sharing electrons in a covalent bond, the fluorine is still called an atom, because it has not gained complete control over the electron that is completing its $2p$ orbital In the $\ce{F2}$ molecule, there are to fluorine atoms
  • Why does chlorine have a higher electron affinity than fluorine?
    Fluorine, though higher than chlorine in the periodic table, has a very small atomic size This makes the fluoride anion so formed unstable (highly reactive) due to a very high charge mass ratio Also, fluorine has no d-orbitals, which limits its atomic size As a result, fluorine has an electron affinity less than that of chlorine
  • Why exactly is a fluoride anion a stronger base than iodine anion?
    The high oxidising ability of fluorine can be thought of as a side effect of its high electronegativity: it has a tendency to strongly attract electrons since it has a highly positively charged nucleus that is shielded by only two core and seven valence electrons Adding an eighth electron is comparatively easy
  • Why are there more fluoride compounds formed with xenon?
    Noble gases form compounds with fluorine and oxygen only because fluorine and oxygen are the most electronegative elements Heavier noble gases (xenon and krypton) are able to form compounds with other elements because xenon and krypton, both have low ionisation enthalpies as compared to helium and neon
  • Why is fluorine a oxidising agent? - Chemistry Stack Exchange
    We also know that fluorine has very high charge mass ratio as it is very small in size and its electron gain enthalpy is know to be very high, i e gain of electron is favourable thermodynamically Also, many sources state that: Fluorine has low bond dissociation enthalpy and high hydration enthalpy due to which fluorine is a good oxidizing agent





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