Example Which hybrid orbitals are used by carbon atoms in the following molecules? ( HC-CH, () H C-CH=CH, (HE) CH CHO (c) CH-CH-OH Solution. (iv) CH COOH N.C.E.R.T

Compare Figs. 4-47 and 4-49. Why are they different? Because B2 is known to be paramagnetic, the 2p and 2p molecular orbitals must be switched from the first prediction. What is the rationale for this? Why might one expect the 2p to be lower in energy than the 2p? Why cant we use diatomic oxygen to help us decide whether the 2p, or 2p, is lower in energy?

Determine the hybridization for the indicated atoms in each structure below. C. D. :0: B. || CH;—CH,—C—OH CH3 CEN: Refer to the above structure, What is the hybridization of A, B, C and D na che ha se 2012

6.For the molecules shown below: L=molecule on left, R=molecule on the right H. CH3 at C H' ******* C%3Cd H -CH3 N. PCL R. (a) Add the lone pair of electrons to all atoms in both structures that have lone pairs (b) What hybrid orbital is used by the C in the CN group of L? (c) How many o (d) What is the approximate bond angle shown as “c" in L? - (e) What is the approximate bond angle shown as "f' in R? --- (f) What hybrid orbital is used by the O in the OCH3 group in R and how many t - bonds are there in L? --- -- -