CHEMISTRY OF THE MAIN GROUP 2 ELEMENTS, GROUP 15, 16, 17, 18 AND HYDROGEN

Question

What is the valence electron configuration for Group 5A elements? Metallic character increases when going down a group. Give some examples illustrating how Bi and Sb have metallic characteristics not associated with N, P, and As. Elemental nitrogen exists as N2, whereas in the gas phase the elements phosphorus, arsenic, and antimony consist of P4, As4, and Sb4 molecules, respectively. Give a possible reason for this difference between N2 and the other Group 5A elements. White phosphorus is much more reactive than black or red phosphorus.

Answer 1

The valence electrons for group 5A would be 3 electrons found in the p orbital. Conductibility and melting points could provide the necessary metal-non metal distinction between Bi and Sb and the other group 5A elements. The presence of a d orbital that could be used or is used for P4, As4 and Sb4 could explain why Nitrogen Gas has two atoms while the other gases in the 5a group have 4 atoms each.