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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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  • intermolecular forces - Why does fluorine form only one hydrogen bond . . .
    6 Fluorine in hydrogen fluoride can form only a limited amount of hydrogen bonds because there is only one (protic) hydrogen atom per fluorine Ammonium fluoride has enough protic hydrogens to form hydrogen bonds with all four electron pairs on each fluorine — and so they do, in a wurtzite-type arrangement of the ions
  • 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 See this, archived here
  • Spontaneity and nature of attack of fluorine gas on aluminum
    What is the nature of the reaction of attack of fluorine gas on aluminium metal? Is it spontaneous in nature? I have studied reactions of halogens on aluminium, but it had no information about fluo
  • Oxidation state of fluorine in HOF - Chemistry Stack Exchange
    What should be the oxidation state of $\\ce{F}$ in $\\ce{HOF}$ As fluorine is the most electronegative element in the periodic table, it should be $-1$ But when I googled it, I found that many so
  • inorganic chemistry - Why is fluorine the most electronegative atom . . .
    Fluorine is the most electronegative element because the definition of electronegativity makes it so The electronengativity scales are defined based on experimentally determined properties of the elements
  • How is fluorine gas contained and transported, why arent the metal . . .
    It was made from the video Fluorine - Periodic Table of Videos I noticed that the cylinder containing the fluorine gas "filled up on the roof" in the video looks like it is made out of metal, as is the tube feeding the gas to the combustion sample The liquification experiment also shown in the video uses a flexible tube that appears to be
  • periodic trends - If fluorine has a lower electron affinity than . . .
    I have read that fluorine has a lower electron affinity than chlorine despite its lower atomic radius because its electron cloud is extremely dense If this is the case, shouldn't the ionization energy of fluorine be lower than that of chlorine, since fluorine's dense electron cloud should eagerly repel its electrons?
  • inorganic chemistry - Why is fluorine more reactive than chlorine . . .
    This is shielding Lastly, fluorine is much smaller molecule than chlorine, and the shorter distance, or radius, between the nucleus and the electron again makes it more likely to attract the electron and react to gain a noble gas configuration
  • Why does fluorine atom have a higher ionization energy than oxygen atom?
    Both oxygen and fluorine (and nitrogen, carbon, boron and neon) have a $\mathrm {2p}$ orbital as their highest occupied, so we expect to ionise from that If you draw a trend of the ionisation energies, you observe that the energy rises from boron to nitrogen, is lower for oxygen and rises from oxygen to neon
  • Does fluorine have 5 or 7 active valence electrons?
    Fluorine is listed as 5 "active" valence electrons, implying perhaps that the 2s electrons do not participate in bonding Why is fluorine treated differently than oxygen (or does oxygen make compounds where the 2s electrons are more involved in bonding than those of fluorine)?





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