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Cynthia Rodas 4H wrote:Hydrogen bonds are stronger than dipole-dipole. The strength for intermolecular forces arranged from lowest to highest is London forces, dipole-dipole, H-bonding, and ion-dipole.
Why are hydrogen bonds stronger than dipole dipole?
diople dipole interactions are constituted as van-der-waal attractions or london dispersion forces so they are inherently weaker than hydrogen bonds, but may or may not be more prevalent in a molecule than hydrogen bonds so cumulatively they could be larger. Individually however, no.
So the intermolecular forces are London Dispersions, Dipole-dipole, and Hydrogen Bonding. The intramolecular forces are ionic, metallic, and network solids. In terms of dipole-dipole and hydrogen bonding, a dipole-dipole bond is otherwise known as an attractive force between polar molecules, due to a difference in electronegativity. From my understanding, a hydrogen bond is a type of dipole, but it is way stronger than a dipole-dipole intermolecular force. Hydrogen can only be bonded to highly electronegative elements that Fluorine, Nitrogen, and Oxygen only.
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