All polar molecules have a permanent dipole moment, but London dispersion forces in non-polar molecules can cause temporary dipole moments as well.
Generally if a molecule contains polar bonds and the bond dipole moments do not cancel each other out then that molecule will have an overall dipole moment. Bond dipoles arise when there is a significant difference in electronegativity between the atoms in the bond. There some cases such as phosphine PH3 where the lone pair can make a significant contribution to the molecular dipole moment.
Symmetric molecules have no dipole moment. An example is carbon tetrachloride, CCl4 , which has no dipole moment yet the C-Cl bonds are polar, (chlorine is more electronegative than carbon). The chlorine atoms each have a small negative charge but because the molecule is tetrahedral there is no dipole and therefore no dipole moment
The molecular dipole moment is a measure of the separation of positive and negative charges within a molecule. It is a vector quantity that indicates the overall polarity of a molecule. It is determined by the individual dipole moments of the bonds within the molecule and their spatial arrangement.
Every polar molecule has a permanent dipole.
KrF2 is a linear molecule and therefore there is no dipole moment.
This is not a naturally occuring compound. If it exists, it would not have a dipole moment as it would be a linear molecule.
It is a symmetrical tetrahedral molecule so has zero dipole moment.
dipole moment of water is 1.85 Debye
Carbon dioxide has a zero dipole moment. The C=O bonds are polar, but because the molecule is linear, the polarities cancel one another and the molecule has a zero dipole moment. Click on the related link for an illustration of the carbon dioxide molecule showing its dipole moment.
Dipole moment of CO2 molecule is zero,becoz it is linear molecule,whereas SO2 is angular molecule having dipole moment 1.61 D....:)
No. H2 molecule does not have any dipole moment.
NH3 is an asymmetrical compound.So it is exhibits.