Final answer:
Compounds A) CHCl₃ and C) CH₂Cl₂ are likely to have a dipole moment, with the dipole moment pointing towards the more electronegative atoms.
Step-by-step explanation:
In order to determine which of the given compounds is likely to have a dipole moment, we need to consider the polarity of each individual bond in the molecule, as well as the overall molecular geometry.
A) CHCl₃: This molecule has polar covalent bonds due to the difference in electronegativity between carbon and chlorine. The molecule has a tetrahedral geometry, with the chlorine atoms positioned on three of the vertices and the hydrogen and carbon atoms on the remaining vertices. The dipole moment of CHCl₃ will point towards the more electronegative chlorine atoms.
B) H₂C=CH₂: This molecule has a linear geometry and nonpolar covalent bonds. The electronegativity difference between hydrogen and carbon is negligible, so the molecule does not have a dipole moment.
C) CH₂Cl₂: This molecule has polar covalent bonds between carbon and chlorine due to the difference in electronegativity. It has a tetrahedral geometry, with two chlorine atoms and two hydrogen atoms occupying the vertices. The dipole moments of the bonds do not cancel out, so the molecule has a net dipole moment pointing towards the more electronegative chlorine atoms.
D) SF₆: This molecule has nonpolar covalent bonds between sulfur and fluorine. It has an octahedral geometry, with the fluorine atoms positioned on the vertices. The dipole moments of the bonds cancel out, resulting in a molecule with no net dipole moment.
Based on these considerations, the compounds likely to have a dipole moment are A) CHCl₃ and C) CH₂Cl₂, with the dipole moment pointing towards the more electronegative atoms.