For each central atom, go back to the VSEPR shapes in Part c and add the bond dipoles and the overall dipole moment of that area of the molecule (if there is one). Explain whether the entire molecule is polar or not.
how do i do this question tell me steps by steps for RnCl4
Step 1: Identify the central atom in RnCl4. In this case, the central atom is Rn (radon).
Step 2: Determine the VSEPR shape for RnCl4, which is square planar.
Step 3: Add the bond dipoles to the VSEPR shape. In RnCl4, there are four Cl (chlorine) atoms bonded to the central Rn atom. The bond dipoles between Rn and Cl are directed towards the Cl atoms.
Step 4: Find the overall dipole moment of the molecule. In a square planar molecular geometry, if the bond dipoles cancel each other out (i.e. if they are symmetrically arranged in opposite directions), the molecule will be nonpolar.
Step 5: Since the bond dipoles in RnCl4 are symmetrically arranged in opposite directions, they cancel each other out, resulting in a nonpolar molecule.
In conclusion, RnCl4 is a nonpolar molecule due to the symmetric arrangement of bond dipoles in a square planar geometry.