Polar covalent- due to the difference in electronegativity between H and Br.
There are dipole-dipole forces between the positive end (hydrogen) and the negative end of the other atom of a different molecule (hydrogen end. There are also LDFs, but no hydrogen bonds.
HBr is considered a polar covalent bond.
polar covalent
Br2 is covalently bonded
It will be a polar covalent bond.
It is a covalent bond.
This is an ionic bond.
It is a covalent bond.
an ion
Dipole
Dipole-dipole.
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.
HBr, H2O
an ion
Dipole
Dipole-dipole.
No, since its a polar compound its also considered to be polar. Therefore, it has dipole-dipole forces
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.
2.01 mol
HBr, H2O
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.
HBr
This is to do with the intermolecular forces in the two compounds. There are no hydrogen bonds between the molecules of either compound, since Br and I are not electronegative enough to polarise the molecules sufficiently. But since HI molecules contain more electrons than HBr, there are increased van der Waals forces in HI. For the same reason HBr has a higher boiling point than HCl, but HF has a higher boiling point than HCl, HBr or HI because of hydrogen bonding.
Hydrobromic acid HBr(aq)
HCL has a higher boiling point compared to HBr This is due to difference in electronegativity. H - 2.1 Cl - 3.0 Br - 2.8 The difference for HCl is 0.9, the difference for HBr is 0.7. The larger the difference in electronegavity means the stronger the bond. Large difference means greater attraction hence more energy is needed to overcome this bond.