3) Draw the orbital diagram for the ground state, excited state (if needed), and the hybrid.

Select only individual atoms, and not the bonds between them. Double bonds may be conjugated, meaning that there is one single bond between them. Identify all the atoms in the structure below that must lie in the same plane.

3) Determine whether CH3CI is polar. To do this, you must: draw the 3D structure of the molecule, use arrows to indicate polar bonds, and either use an arrow to indicate the net dipole moment or state that the molecule is non-polar.

Draw the Lewis structures for the following molecules. For each molecule, determine its (a) electronic geometry, (b) number of nonbonding domains on the central atom, and (c) polarity of the molecule. Remember, that molecules that have zero nonbonding domains on the central atom AND have all of the outer atoms the same are NONPOLAR. Generally, molecules with different outer atoms or with more than one nonbonding domain are POLAR. However, these may be NONPOLAR ONLY IF the dipoles cancel each other due to a symmetrical arrangement. CIF3 (a) electronic geometry: -Select-- (b) number of nonbonding domains on central atom: -Select-v (c) molecule polarity: -Select- SO2 .(a) electronic geometry: --Select- (b) number of nonbonding domains on central atom: -Select---V (c) molecule polarity: --Select--v SF5 (a) electronic geometry: [-Select- (b) number of nonbonding domains on central atom: --Select--- ♥ (c) molecule polarity: --Select-- v IFS (a) electronic geometry: -Select-- (b) number of…