Oxidation state of fluorine in HOF
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
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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
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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
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7 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
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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
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In this case, the formation of fluorine-containing products is generally much more thermodynamically favourable than that of the corresponding iodine-containing products.
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It seems related to the atomic size but hydrogen has a smaller atomic size than fluorine. Why is fluorine the most electronegative atom?
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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
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Fluorine atoms might quantum-tunnel just as hydrogen ones, minding that their radii closely resemble each other, and because of it nonrigidity of $ce {PF5}$ via Berry pseudorotation
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I know fluorine is the most electronegative element but can we humans ever synthesize fluorine in a positive oxidation state like +1?
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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
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