Determine the Lewis Structure of the molecule? BCI3 (no Cl-Cl bonds) C3H;CI (C's are central atoms) COF2 (C is central atom) CIO,- (no O-0 bonds) PBrs (no Br-Br bonds)

a) Draw the Lewis structure for the molecule on the left (labeled as Molecule A above). Draw the Lewis structure which has minimum formal charges.  b) Draw the correct Lewis structure for the molecule on the right (labeled as Molecule B above). Draw the Lewis structure which has minimum formal charges. c) Select the three TRUE statements from those provided below. The molecule on the right (Molecule B) is planar (all atoms lie within the same plane). The molecule on the left (Molecule A) is planar (all atoms lie within the same plane). The molecule on the right (Molecule B) has polar bonds. The molecule on the left (Molecule A) has polar bonds. We can distinguish between the two molecules (Molecule A and Molecule B) based upon their dipole moment.

Notes April In this exercise we have nitrogen, water, carbonate, carbon tetra chloride, ammonium, carbon monoxide, dinitrogen monoxide, nitrate, chlorite, phosphate, NF3, F2, SO42- and OCL2 !! Conclusion All of the compounds in this exercise are what kind of compound? Explain why this is important to VSEPR. Conclusion Explain why it is important to consider both VSEPR shape and bond polarity to determine the overall polarity of a molecule. Use the HF (hydrogen fluoride) and CO₂ (carbon dioxide) as examples.

Please don't provide handwritten solution ....