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draw lewis structures for each of the following molecules and use their intermolecular forces to compare them: bf3, cf3h, and ch3oh
draw lewis structures for each of the following molecules and use their intermolecular forces to compare them: bf3, cf3h, and ch3oh
To drawLewis structuresfor each of the following molecules and use their intermolecular forces to compare them, we need to first understand the structure and bonding of each molecule.BF3:Boron trifluoride, BF3, is a molecule with atrigonal planar geometry. It has three covalent bonds with three fluorine atoms, and a vacant p-orbital on boron. The Lewis structure for BF3 is:F F| |F--B--FBF3 is a nonpolar molecule with no net dipole moment. The intermolecular forces in BF3 are London dispersion forces, which are relatively weak compared to other intermolecular forces.CF3H:Trifluoromethane, CF3H, is a molecule with atetrahedral geometry. It has three covalent bonds with three fluorine atoms, and one covalent bond with a hydrogen atom. The Lewis structure for CF3H is:F F| |F--C--F|HCF3H is a polar molecule with a net dipole moment. The intermolecular forces in CF3H include dipole-dipole forces and London dispersion forces.CH3OH:Methanol, CH3OH, is a molecule with a tetrahedral geometry. It has three covalent bonds with three hydrogen atoms, one covalent bond with an oxygen atom, and a lone pair of electrons on the oxygen atom. The Lewis structure for CH3OH is:H H| |H--C--O|HCH3OH is a polar molecule with a netdipole moment. The intermolecular forces in CH3OH include hydrogen bonding, dipole-dipole forces, and London dispersion forces.In summary, BF3 is a nonpolar molecule with only London dispersion forces, CF3H is a polar molecule with dipole-dipole forces and London dispersion forces, and CH3OH is a polar molecule with hydrogen bonding, dipole-dipole forces, and London dispersion forces. Therefore, CH3OH has the strongest intermolecular forces among the three molecules.To know more aboutLewis structure, referbrainly.com/question/20300458#SPJ11...