In class we used valence bond theory to describe the bonding in CH2CH2, a planar molecule with HCH bond angles of 120. We assumed that CC and CH bonds would have the same s and p characters since their electronegativities are similar. For CF2CF2, however, F has a much larger electronegativity than C. Further, the available orbital bonding on F is a p-orbital and not an sorbital. Hence the C-F bonds have more "p-character" than C-H bonds, or said differently have less s-character than CH or CC bonds. a. Assume the molecule is in the xz plane and the s-character for the CC bond is twice the s-character for the C-F bonds. Determine the coefficients in the matrix below as we did for CH2CH2 in class. Assume 1 represents the CC bond directed along the z-axis. 123=s2pypxpy2s2px2p b. Determine the angles of FCF and FCC and rationalize the difference that now exists