Compound | dispersion | dipole | hydrogen-bonding |
carbon monoxide (CO) | Y | Y | N |
Cl2 chlorine | Y | N | N |
HBrO (hypobromous acid) | Y | Y | Y |
NOCl (nitrosyl chloride) | Y | Y | N |
* Y denotes Yes(Intermolecular force present) *N denotes Nil( Intermolecular force absent)
Dispersion Forces or London Forces
Atoms and nonpolar molecules are electrically symmetrical and have no dipole moment because their electronic charge cloud is symmetrically distributed. But a temporary dipole is created by the fluctuation in electronic arrangement in a molecule. Hence all molecules must show dispersion force.
Dipole forces
It can be dipole-dipole or dipole-induced dipole forces. Here a partial positive or partial negative charge is created on the atoms in a molecule due to its electronegativity difference. A polar molecule can induce a dipole on non polar molecule also.
Hydrogen bonding
It is a special case of dipole-dipole interaction. This is found in the molecules in which highly polar N-H, O-H or H-F bonds are present.
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