Question

Two isomers of the planar compound $1,2$ -dichloroethylene are shown here. Which of the following statements best explains these data? (a) The larger the dipole moment, the stronger the intermolecular forces, and therefore the boiling point is lowest for the molecule with the largest dipole moment. (b) The dispersion forces increase from F to Clt to Br; since the boiling point also increases in this order, the dispersion forces must make a far greater contribution to intermolecular interactions than dipole-dipole interactions. (c) The trend in electronegativity is $\mathrm{F}>\mathrm{Cl}>\mathrm{Br} ;$ therefore, the most ionic compound (CH_{2} \mathrm { F } _ { 2 } ) has the lowest boiling point, and the most covalent compound

          Two isomers of the planar compound $1,2$ -dichloroethylene are shown here. Which of the following statements best explains these data? (a) The larger the dipole moment, the stronger the intermolecular forces, and therefore the boiling point is lowest for the molecule with the largest dipole moment. (b) The dispersion forces increase from F to Clt to Br; since the boiling point also increases in this order, the dispersion forces must make a far greater contribution to intermolecular interactions than
dipole-dipole interactions. (c) The trend in electronegativity is $\mathrm{F}>\mathrm{Cl}>\mathrm{Br} ;$ therefore, the most ionic compound (CH_{2} \mathrm { F } _ { 2 } ) has the lowest boiling point, and the most covalent compound

Added by Brandon P.

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