The HBr molecule is linear (obviously, since it contains only two atoms). The dipole moment is a vector, parallel to the bond, pointing toward the partially positively charged atom, which is, in this case, the hydrogen. The magnitude of the dipole moment is the difference in the partial electrical charges on each atom times the spatial separation of the atoms in the bond. In a molcule with more than two atoms (more than one bond), the dipole moment of each bond must be added vectorially and the resultant vector will determine the dipole moment of the molecule. For instance, carbon dioxide has two carbon-oxygen double bonds of high polarity, but because the molecule is linear, and the individual dipoles oppose each other, the carbon dioxide molecule has no net dipole moment.
no, although the c - cl bond is a polar bond due to the difference in pauling's electronegativity values the actual molecule is not a polar molecule due to the symmetry of the chlorine atoms surrounding the central carbon atom. therefor there is no dipole (Difference in charge) present in the molecule. however, there is induced dipole interactions due to the constant movement of electrons around the molecule giving temporary dipole moments which in turn induces neighboring molecules to also exibit these dipole moments. (Van der Walls forces)
It has no net dipole moment, therefore, it is non polar.
Hydrogen fluoride as it is a hydrogen bond.
Yes it is a dipole but i do not know the direction of movement of the dipole.
dipole-dipole
No, Nitrogen TriFluoride has dipole-dipole forces
A hydrogen bond is a very strong dipole-dipole bond. A hydrogen bond can only form between hydrogen and a strong electromagnetic atom; fluorine, oxygen or chlorine.
Yes. Hydrogen bromide shows dipole-dipole interactions.
It should be pointed towards the oxygen.
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.
Hydrogen fluoride as it is a hydrogen bond.
hydrogen bonding is stronger.
The hydrogen bond is not strong.
There are two different atoms.So it is polar.
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.
Hydrogen bonds are stronger than dipole-dipole and Van der Waals forces.
a hydrogen bond
1 D (Debye) ~ 3.34 x 10^-30 C m (Coulomb meters), therefore the dipole moment of HF =1.91 x 3.34 x 10^-30 = 6.38 x 10^-30 C m
Amides have some hydrogen bonding, between the lone pair on the nitrogen and the hydrogen on the nitrogen in the next molecule. There will also be van der Waals forces and a little dipole-dipole attraction.