CHEM101 Lecture Notes - Lecture 7: Paramagnetism, Bond Energy, Vsepr Theory

• School: University of Alberta
• Department: Chemistry
• Course: CHEM101
• Professor: Sai Yiu

Document Summary

But for b2, c2 and n2, the order is: *you are responsible for applying the correct mo diagram to appropriate diatomic molecules. There are a total of 2 x 4 = 8 valence electrons. Therefore, the structure of c2 according to the mo theory is: The electron configuration of n = [he] 2s2 2p3. There are a total of 2 x 5 = 10 valence electrons. Since there is no unpaired electron, n2 is diamagnetic. There are a total of 2 x 6 = 12 valence electrons. Consider the mo diagram: y g r e n. For the formation of o2 ( 2s)2 ( *2s)2 ( 2p)2 ( 2p)4 ( *2p)2. Since there are two unpaired electron, o2 is paramagnetic. The vb theory and vsepr cannot explain the paramagnetic properties of o2 because there is no unpaired electron in its lewis structure: The molecular orbital diagrams for the 2nd period diatomic molecule are shown below: