If you mean a dipole which only lasts for an instant, then you have to picture the electrons of the molecule surrounding the nuclei. In a non-polar molecule the electrons are shared evenly on average, but at any one second they may be distributed so that there is a greater density at one end than another, i.e. there is a temporary dipole.
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An instantaneous dipole can occur when the electron distribution in a molecule is momentarily uneven, creating a temporary dipole moment. This can happen due to random fluctuations in electron distribution within the molecule. These instantaneously induced dipoles can lead to London dispersion forces, which are a type of weak intermolecular force.
Dipole-dipole is between two polar molecules, that would be polar anyway. Dipole-induced dipole is between a polar molecule and a non-polar molecule that is now polar due to the proximity of a polar molecule.
A dipole develops in a molecule when there is an unequal distribution of electron density, causing one end of the molecule to be more negatively charged and the other end to be more positively charged. This occurs due to differences in electronegativity between atoms within the molecule, leading to a separation of charge and the formation of a dipole moment.
For an ammonia molecule to be IR active, it must have a changing dipole moment, which is caused by the asymmetric stretching and bending vibrations of its bonds. This is because IR spectroscopy detects changes in the dipole moment of a molecule as it absorbs infrared radiation. In the case of ammonia, its stretching and bending vibrations result in a non-zero dipole moment change, making it IR active.
Yes, sulfur dioxide (SO2) is a polar molecule and has a dipole moment. This is because of the difference in electronegativity between the sulfur and oxygen atoms, causing an unequal distribution of electron density within the molecule.
The dipole moment of hydrogen bromide is expected to be in the direction from hydrogen to bromine. This is because bromine is more electronegative than hydrogen, causing an uneven distribution of electron density in the molecule.