Compare the dipole moments of the following pairs of molecules and determine whether the first is "Greater Than", "Less Than" or "Equal to" the second.
O The dipole moment of ClO2 is ___ the dipole moment of SO2
O The dipole moment of SiF4 is _ the dipole moment of SF4
O Dipole moment of SO2 is __the dipole moment of SO3
O The dipole moment of BeCl2 is _ the dipole moment of SCl2
O The dipole moment of H2O is ____ the dipole moment of H2S

The dipole moment is the difference of electronegativity between the atoms in a molecule, and the total is the sum of the dipole moments of the bonds. So, it depends on the geometry of the molecule. When the dipole moment is 0 the molecule is nonpolar, when it is different from 0 the molecule is polar.

Both ClO₂ and SO₂ have angular geometry because there are lone pairs of electrons in the central atom (Cl and S), but Cl has a higher value of electronegativity than S, so the dipole moment must be greater.

SiF₄ is a nonpolar molecule, which has tetrahedral geometry and no lone pairs at the central atom. SF₄ has lone pairs at the central atom, and then the molecule is polar, so the dipole moment of SiF₄ is less than of SF₄.

The SO₃ molecule has no lone pairs at the central atom and has trigonal geometry, so it's a nonpolar molecule. SO₂ has angular geometry and it's a polar molecule, so the dipole moment of SO₂ is greater.

BeCl₂ has a linear geometry and is a nonpolar molecule. SCl₂ has an angular geometry, and it's a polar molecule, so the dipole moment of BeCl₂ is less than the dipole moment of SCl₂.

Oxygen has a higher electronegativity than the sulfur, and both molecules are polar with angular geometry, so the dipole moment of H₂O is greater.