To determine which of the given molecules has the greatest net dipole, we need to consider both the polarity of the individual bonds and the shape of the molecule.

a. PCl3: Phosphorus trichloride is a polar molecule. The chlorine atoms are more electronegative than the phosphorus atom, creating polar bonds. The molecule is also pyramidal in shape, which means the dipoles do not cancel out.

b. CCl4: Carbon tetrachloride is a nonpolar molecule. Although the C-Cl bonds are polar, the molecule is tetrahedral, so the bond dipoles cancel each other out.

c. H2O: Water is a polar molecule. The oxygen atom is more electronegative than the hydrogen atoms, creating polar bonds. The molecule is also bent in shape, which means the dipoles do not cancel out.

d. BeF2: Beryllium difluoride is a nonpolar molecule. Although the Be-F bonds are polar, the molecule is linear, so the bond dipoles cancel each other out.

e. BF3: Boron trifluoride is a nonpolar molecule. Although the B-F bonds are polar, the molecule is trigonal planar, so the bond dipoles cancel each other out.

Therefore, out of the given options, water (H2O) has the greatest net dipole due to its polar bonds and bent shape.

Question

To determine which of the given molecules has the greatest net dipole, we need to consider both the polarity of the individual bonds and the shape of the molecule.

a. PCl3: Phosphorus trichloride is a polar molecule. The chlorine atoms are more electronegative than the phosphorus atom, creating polar bonds. The molecule is also pyramidal in shape, which means the dipoles do not cancel out.

b. CCl4: Carbon tetrachloride is a nonpolar molecule. Although the C-Cl bonds are polar, the molecule is tetrahedral, so the bond dipoles cancel each other out.

c. H2O: Water is a polar molecule. The oxygen atom is more electronegative than the hydrogen atoms, creating polar bonds. The molecule is also bent in shape, which means the dipoles do not cancel out.

d. BeF2: Beryllium difluoride is a nonpolar molecule. Although the Be-F bonds are polar, the molecule is linear, so the bond dipoles cancel each other out.

e. BF3: Boron trifluoride is a nonpolar molecule. Although the B-F bonds are polar, the molecule is trigonal planar, so the bond dipoles cancel each other out.

Therefore, out of the given options, water (H2O) has the greatest net dipole due to its polar bonds and bent shape.

Knowee AI · Accepted Answer

To determine which of the given molecules has the greatest net dipole, we need to consider both the polarity of the individual bonds and the shape of the molecule.

a. PCl3: Phosphorus trichloride is a polar molecule. The chlorine atoms are more electronegative than the phosphorus atom, creating polar bonds. The molecule is also pyramidal in shape, which means the dipoles do not cancel out.

b. CCl4: Carbon tetrachloride is a nonpolar molecule. Although the C-Cl bonds are polar, the molecule is tetrahedral, so the bond dipoles cancel each other out.

c. H2O: Water is a polar molecule. The oxygen atom is more electronegative than the hydrogen atoms, creating polar bonds. The molecule is also bent in shape, which means the dipoles do not cancel out.

d. BeF2: Beryllium difluoride is a nonpolar molecule. Although the Be-F bonds are polar, the molecule is linear, so the bond dipoles cancel each other out.

e. BF3: Boron trifluoride is a nonpolar molecule. Although the B-F bonds are polar, the molecule is trigonal planar, so the bond dipoles cancel each other out.

Therefore, out of the given options, water (H2O) has the greatest net dipole due to its polar bonds and bent shape.

Which of the following has the greatest NET dipole?Question 10Select one:a.PCl3b.CCl4c.H2Od.BeF2e.BF3

Question

Which of the following has the greatest NET dipole?

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