O2
Dipole
Dispersion forces and Dipole-Dipole Source: Mastering Chemistry
Dipole-dipole.
HBr is a polar molecule: dipole-dipole forces. There are also dispersion forces between HBr molecules. The hydrogen bond is a special dipole-dipole interaction between the hydrogen atom in a polar N-H, O-H, or F-H bond and an electronegative O, N, or F atom.
O2
Dipole
Dispersion forces and Dipole-Dipole Source: Mastering Chemistry
Dipole-dipole.
HBr is a polar molecule: dipole-dipole forces. There are also dispersion forces between HBr molecules. The hydrogen bond is a special dipole-dipole interaction between the hydrogen atom in a polar N-H, O-H, or F-H bond and an electronegative O, N, or F atom.
No, since its a polar compound its also considered to be polar. Therefore, it has dipole-dipole forces
There are two different atoms.So it is polar.
Polar covalent- due to the difference in electronegativity between H and Br.
HBr
There is no hydrogen bonding in HBr and HI. The intermolecular forces are London dispersion forces- HI has more electrons, so more instantaneous induced dipole-dipole interaction- more intermolecular force- and therefore a higher boiling point.
Ka = [H+].[Br-] / [HBr] However the value of this expression is very high, because HBr is a STRONG acid, meaning that much more than 99.9% of the HBr molecules in water are protolized (ionized), making [H+] and [Br-] equal to the original (added) HBr amount, and the [HBr]-value nearly zero.
yes HBr is an electrolyte