Dipole moment means how polar the molecule is, and since the hydrogen halides are diatomic and linear, this translates directly into how polar the bond is. The polarity of a bond depends on the electronegativity difference between the 2 atoms. The general trend in electronegativity is that it decreases down a column. This is because, while elements in the same column have the same effective nuclear charge (+7 in the case of halogens), they have larger electron clouds as you move down the Periodic Table. This means the valence (bonded) electrons are farther from the nucleus of Br than they are from the nucleus of F. Therefore, the attraction they feel for the nucleus is less for the larger atoms.
The hydrogen bond is not strong.
Hydrogen and dipole-dipole forces
Yes, water shows all three types of common intermolecular forces, namely dispersion forces, dipole-dipole forces and hydrogen bonds. Dispersion forces are present at any species which consists of movable charges that can be shifted with respect to one another. Thus a dipole emerges which on his part can induce dipoles in close-by molecules. The permanent dipole of water molecules leads to dipole-dipole forces. They can be distinguished from hydrogen bonds as they are present even at angles where no significant hydrogen bonds are expected any more.
no
Hydrogen has a positive charge.
Yes. Hydrogen bromide shows dipole-dipole interactions.
Hydrogen fluoride as it is a hydrogen bond.
The hydrogen bond is not strong.
hydrogen bonding is stronger.
Hydrogen bonds are stronger than dipole-dipole and Van der Waals forces.
a hydrogen bond
a hydrogen bond
Hydrogen and dipole-dipole forces
a hydrogen bond
CCl2F2 will have both Van der Waals forces and dipole-dipole forces.Hydrogen bonds only form from a Hydrogen atom, when a highly elecronegative atom (Nitrogen/Oxygen/Fluorine)
user-generated content: report abuseDipole-Dipole forces, Dispersion forces, and hydrogen bonding
hydrogen, London dispersion, and dipole - dipole