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Hydrogen halide
 | This article needs additional citations for verification. (January 2025) |
In chemistry, hydrogen halides (hydrohalic acids when in the aqueous phase) are diatomic, inorganic compounds that function as Arrhenius acids. The formula is HX where X is one of the halogens: fluorine, chlorine, bromine, iodine, astatine, or tennessine.[1] All known hydrogen halides are gases at standard temperature and pressure.[2]
| Compound | Chemical formula | Bond length d(H−X) / pm (gas phase) |
model | Dipole μ / D |
Aqueous phase (acid) | Aqueous Phase pKa values |
|---|---|---|---|---|---|---|
| hydrogen fluoride (fluorane) |
HF |  |
 |
1.86 | hydrofluoric acid | 3.1 |
| hydrogen chloride (chlorane) |
HCl |  |
 |
1.11 | hydrochloric acid | -3.9 |
| hydrogen bromide (bromane) |
HBr |  |
 |
0.788 | hydrobromic acid | -5.8 |
| hydrogen iodide (iodane) |
HI |  |
 |
0.382 | hydroiodic acid | -10.4 [3] |
| hydrogen astatide astatine hydride (astatane) |
HAt |  |
 |
−0.06 | hydroastatic acid | ? |
| hydrogen tennesside tennessine hydride (tennessane) |
HTs |  |
 |
−0.24 ? | hydrotennessic acid | ? [4] |
- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ^ The Acidity of the Hydrogen Halides. (2020, August 21). Retrieved May 5, 2021, from https://chem.libretexts.org/@go/page/3699
- ^ Schmid, Roland; Miah, Arzu M. (2001). "The Strength of the Hydrohalic Acids". Journal of Chemical Education. 78 (1). American Chemical Society (ACS): 116. doi:10.1021/ed078p116. ISSN 0021-9584.
- ^ de Farias, Robson Fernandes (January 2017). "Estimation of some physical properties for tennessine and tennessine hydride (TsH)". Chemical Physics Letters. 667: 1–3. Bibcode:2017CPL...667....1D. doi:10.1016/j.cplett.2016.11.023.
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