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- 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
- 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
- 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
- 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)?
- 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
- Are there stronger oxidizing agents than fluorine gas?
Are there stronger oxidizing agents than fluorine gas, so it could oxidize fluoride to fluorine? Also, in case of oxygen, fluorine gas can oxidize oxygen gas to the exotic dioxygenyl ion
- 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 best oxidising agent, but . . .
Fluorine is the most electronegative element But due to its high effective nuclear charge it holds up its electron density very tightly, moreover its a non-metal so preferably accepts electron to form stable (F–) ion which has configuration of Ne F2 ------> F+ + e- is very favorable therefore it gets reduced very easily (reduced form F- is very stable than F2) and so it oxidises other
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