Which of the following molecules will have the greatest dipole moment?Question 1Select one:a.HClb.H2Oc.NH3d.CH2Br2e.SiO2Clear my choice

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

a. HCl: This molecule is a diatomic molecule with a polar bond. However, it's dipole moment will be less than that of a polar molecule with more than two atoms.

b. H2O: Water is a bent molecule with two polar O-H bonds that add up to give a net dipole moment.

c. NH3: Ammonia is a trigonal pyramidal molecule with three polar N-H bonds. However, due to its geometry, the dipole moments do not cancel out completely, resulting in a net dipole moment.

d. CH2Br2: This molecule is tetrahedral with polar C-Br and C-H bonds. However, the dipole moments of the C-H bonds are less than those of the C-Br bonds, and they do not cancel out completely, resulting in a net dipole moment.

e. SiO2: Silicon dioxide is a linear molecule with two polar Si-O bonds. However, due to its linear geometry, the dipole moments of the two bonds cancel out, resulting in no net dipole moment.

Comparing these molecules, H2O (water) has the greatest dipole moment due to its bent shape and the high polarity of the O-H bonds. Therefore, the correct answer is b. H2O.