what do i do for F my thing is RnCl4: determine the AXE formula and VSEPR shape around each central atom, draw each type of central atom once including bond angles and the name of the VSEPR shape
research the hybridization of the central atom, draw an energy level diagram demonstrating the hybrid orbitals
research and draw/provide an orbital overlap diagram of the molecule, labelling the hybrid orbitals, as well as sigma and pi bonds
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.
To determine the AXE formula, we need to first determine the number of atoms bonded to the central atom (Rn). From the formula RnCl4, we can see that there are 4 chlorine atoms bonded to the central Rn atom. This gives us an AX4E0 formula, where A represents the central atom, X represents the bonded atoms, and E represents the lone pairs on the central atom.
Next, we need to determine the VSEPR shape around the central atom. In this case, with 4 bonded atoms and 0 lone pairs, the VSEPR shape would be tetrahedral. The bond angles in a tetrahedral shape are approximately 109.5 degrees.
The hybridization of the central atom can be determined by looking at the steric number, which is the sum of the number of atoms bonded to the central atom and the number of lone pairs on the central atom. In this case, the steric number is 4. This corresponds to sp³ hybridization.
Drawing an energy level diagram demonstrating the hybrid orbitals would show the 4 sp³ hybrid orbitals originating from the central Rn atom.
For the orbital overlap diagram of the molecule, we would show the overlap of the sp³ hybrid orbitals with the p orbitals of the chlorine atoms to form sigma and pi bonds.
Adding bond dipoles to the VSEPR shapes and determining the overall dipole moment of the molecule would involve looking at the electronegativities of the atoms involved. If the bond dipoles do not cancel out due to symmetry, the molecule would be considered polar. If the bond dipoles do cancel out, then the molecule would be nonpolar.