Thus, the valence shell electronic arrangement for these elements becomes ns2 np3. Since this matches the electron configuration given to you, you can say that this unknown element is located in group 13. The separating electron in the elements of group 15 enters the n p subshell. The electron configuration for the outermost electrons of an element located in group 13 will thus be

period in the periodic table, the first element located the #p# block is placed in group 13 and the last is placed in group 18. This places the element in the #p# block, which as you can see covers elements located in groups 13 to 18.įor any energy level, i.e. Now, the highest-energy electron is located in a #p# orbital, more specifically in an #np# orbital, which is simply a #p# orbital located on the #n# energy level. Details in the p block are best known for their semiconductor properties.

The p block elements are characterised as being poor metals. the electron configuration in the outermost energy level, ns2np3, where n is the period number. The p block elements are the six elements in the periodic table located below group 3A and above group 5A, namely, carbon (C), silicon (Si), germanium (Ge), tin (Sn), lead (Pb), and flerovium (Fl). valence electrons, in an atom looks like this Similarly, all elements in Group 5A/15 have the general configuration ns2np3, and they have five valence electrons. 9.6: Electron Configurations for Group 5A Elements. In your case, the electron configuration of the outermost electrons, i.e. As you know, the periodic table is organized in blocks that correspond to the location of an element's highest-energy electrons.Įlements that have their highest-energy electrons in the #s# orbital are located in the #s# block, elements that have their highest-energy electrons in a #p# orbital are located in the #p# block, and so on.

Ns2 np3 valence shell group 5a