Compare the intermolecular forces, dipole-dipole and hydrogen-bonding. What would you suggest is the biggest different between t
hem? A. Dipole-Dipole forces do not affect the properties of a substance as much as hydrogen-bonded forces do.
B. Dipole-Dipole forces are permanent; hydrogen-bonded forces are not.
C. Dipole-Dipole Forces can occur among both polar and nonpolar compounds, while hydrogen-bonded forces occur among only polar compounds.
D. Dipole-Dipole forces and hydrogen forces are essentially the same phenomena; hydrogen-bonded forces are just slightly stronger because they occur between hydrogen atoms and only the most electronegative atoms.
Both the dipole-dipole and hydrogen are essentially same because they result form formation of partial negative and positive charges on the atoms constituting a given molecule. in such molecule, one atom is more electronegative than the other and therefore pulls the shared electrons more to itself than the other atom. the atom that pulls a pair of electrons more to itself becomes partially negatively charged whereas the other atom becomes partially positively charge. the weak negative charges on one molecule attracts weak positive charge on the other molecule creating intermolecular forces referred to as dipole-dipole bonds. Hydrogen bonds form in the same manner they are stronger than typical dipole-dipole bonds. so according to the explanation above D is the correct answer.
Boron trifluoride only has six valence electrons and is one of the relatively rare second period covalent molecules that disobeys the octet rule. There are three bonded groups and so no lone pairs. Six electrons implies three electron pairs and therefore a trigonal geometry.
