How Do You Relate An Elements Periodic Table Position To Its Quantum Electron Configuration And Reactivity?
All elements withing the same group (Alkali metals for example) will have an electron configuration that ends the same way (s1 for alkali metals, s2 for Alkaline earth, Groups 3-8 end in p1, p2, p3, p4… so on. The trasition metals end with d orbitals of an energy level one less than the period the element is found in. Lanthanides and actinides end in f orbitals with an energy level equal to its period # minus 2.) The periodic table can be divided up into a “block” for each of the orbital shapes. Groups 1and 2 make the s block. 3-8 make the p block. Trans metals make the d block. Lant/Actinides make the f block. Simply count over the # of spaces that the element is within that block to determine the number of electrons in the last orbital of the electron config. I’m not sure what you mean by “reactivity.” Lots of things affect that. But elements are usually more stable with full or half full orbitals in the OUTER (highest number) energy levels. So, elements ending in s1 will generally
