Hydrobromic acid (HBr) is classified as a molecular compound rather than an ionic compound. This classification stems from the fact that HBr is formed from non-metals: hydrogen (H) and bromine (Br). In a molecular compound, atoms are held together by covalent bonds, where electrons are shared between the atoms. In the case of HBr, the hydrogen atom shares an electron with bromine, creating a polar covalent bond due to the difference in electronegativity between the two elements.
Furthermore, HBr is classified as an acid. In aqueous solution, it dissociates completely into H+ and Br– ions, which is characteristic of strong acids. This ability to donate protons (H+) makes it an acid in the Brønsted-Lowry acid-base theory. Thus, we can conclude that HBr is a molecular compound and behaves as a strong acid when dissolved in water.