There is a chemical interact between the hydrogen halides and water that allows all but HF to fully dissociate, but the molecules in their pure form are not ionic.īy the way, hydrogen is not the only element that unexpectedly doesn't make many ionic compounds. Some mistakenly think that just because some compounds of hydrogen easily dissociate in water (the strong acids) then they must be ionic. There is an article on eHow that really messes this up. I think I should note that some websites get this wrong. There are a few such compounds (some of the hydrides are ionic), but it is unusual. So, it is rather usual for hydrogen to be involved in an ionic bond. HF is a weak acid and HCl, HBr, and HI are strong acids. However, when dissolved in water to form acids, the chemistry is a bit different.
Thus a polar covalent bond results in F and H both having what they want.Īnd, in fact, all of the hydrogen halides in their pure form have polar covalent or covalent bonds.
So, for H to achieve its full two electrons (remember that H seeks 2, not 8, electrons) then the only way to do that with F is by sharing the electron. If you want to think in terms of the octet rule, H would have no electrons whatsoever if it gave its electron to F.
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