In the Lewis structure of PCl5, phosphorus (P) is the central atom surrounded by five chlorine (Cl) atoms. Phosphorus is in Group 5A (Group 15) of the periodic table and has 5 valence electrons, while chlorine is in Group 7A (Group 17) and has 7 valence electrons.
To form the structure, you would start by placing the phosphorus atom in the center and then add the five chlorine atoms around it. Each chlorine atom will be connected to the phosphorus atom by a single bond (represented by a line). Additionally, each chlorine atom will have three lone pairs of electrons around it (represented by dots). The phosphorus atom will have no lone pairs of electrons in this case.
The Lewis structure of PCl5 would look like this: https://lewistructure.com/pcl5-lewis-structure/
In the Lewis structure of SF6, sulfur (S) is the central atom surrounded by six fluorine (F) atoms. Sulfur is in Group 6A (Group 16) of the periodic table and has 6 valence electrons, while fluorine is in Group 7A (Group 17) and has 7 valence electrons.
To form the structure, you would place the sulfur atom in the center and then add the six fluorine atoms around it. Each fluorine atom will be connected to the sulfur atom by a single bond (represented by a line). Additionally, each fluorine atom will have three lone pairs of electrons around it (represented by dots). The sulfur atom will have no lone pairs of electrons in this case.
