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  • inorganic chemistry - Why is the Si-F bond one of the strongest single . . .
    I honestly have no clue where to begin explaining why the Si-F bond is one of the strongest single covalent bonds of them all I would actually predict the bond to be relatively weak on account of the relatively large size of the Si atom leading to a relatively long bond length and hence poor orbital overlap
  • Reaction of Silicon Dioxide with Hydrofluoric Acid
    Although H-F has a stronger bond than H-Cl and other halogen acids, the Si-F bond is one of the strongest single bonds known, so forming four of them in the product makes the reaction thermodynamically favorable Si-Cl bonds are not nearly as strong, and the difference is greater than 4x the difference between HF and HCl $\endgroup$ –
  • If a molecule has both polar and ionic bonds in it, is it polar or . . .
    1) The silicon to fluoride bond is polar covalent Even though an electronegativity difference of more than 2 0 generally indicates an ionic bond, the cutoff rises as the average electronegativity of the two combining species rises
  • polarity - without using electronegativity, which one of these . . .
    $\begingroup$ Yes, but for the purposes of the homework, I doubt they were looking for students to know that It's hard to find examples of trigonal bypyramidal molecules without using the same ones over and over, so this one ends up being in lots of assignments
  • Will Triflic Acid Damage PTFE? - Chemistry Stack Exchange
    To answer your question about using glass vials, it is safe to store triflic acid in glass vials bottles as factors afecting ability of acid to dissolve through glass are if it is a VERY strong superacid or any strongly fluorine donating compounds that will break S = O bonds in Silica to form Si - F bonds like hydrofluoric acid
  • How exactly does UV light break bonds? - Chemistry Stack Exchange
    For example, in the photochemical decomposition of hydrogen peroxide, the weak $\\ce{O-O}$ bond is broken by UV light Ultraviolet light can also dissociate relatively strong bonds such as the double
  • Why do non-metals not form Ionic bonds(Ti-C, Sc-P) and instead form . . .
    As Poutnik describes in his answer, low-electronegativity nonmetallic such as boron form bonds with low ionic character because in general, their atoms are not strongly electronegative enough to fully withdraw electrons even from highly electropositive metals (which still do require some ionization energy)
  • How much can we extend the Finkelstein reaction?
    They need something like a silane to activate them because the Si–F bond is of a competitive strength Yes, the Finkelstein can work in other solvents, especially with the correct activators You can even do the Finkelstein on aromatic rings if you add catalytic copper (I) iodide and a diamine to activate it





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