Using only the elements P, Br, and Mg, give formulas for the following. (b) A molecular compound with polar covalent bonds that obeys the octet rule and has no formal charges

Video transcript

Hello everyone today. We have the following problem using only sulfur and flooring draw the structure of a compound with an expanded octet and no lone pairs on the sulfur and zero formal charges. So the very first thing we want to note is which one of these is going to expand its octet. So we're going to find out which one has an expanded octet or which one can add more electrons to it than normal? That's going to be sulfur. Why? Because sulfur has an empty D. Orbital. And in fact this is the case for any atom from period three and below. They all have an empty D orbital where electrons can be brought into under normal circumstances, sulfur can form six bonds when it expanded octet. Excuse me. On the other hand we have flooring and flooring can only form one bond. So we have floor informing one bond and we have sulfur forming six bonds. With that information. We know that we're going to have one sulfur in the middle surrounded by six different florins. And this aligns with what we just said that sulfur can form six bonds with its expanded octet. And flooring can only form one bond in which it is doing now. We need to see how many elements or how many electrons we can add around each atom here. So we're gonna go ahead and actually calculate the formal charge. And we'll start with flooring, our formal charge equation is going to be the number of valence electrons minus the number of bond lines that we see around an atom minus the number of electrons that we see surrounding each atom. And so for flooring it was that it has a has zero formal charge. The number of valence electrons because it is a group seven a Element, it has seven valence electrons bond lines. There's only one bond line around each flooring and we need to find out how many electrons we have. We can actually solve for that, solving for that. We get zero equals six minus electrons And we get the number of electrons is six. So there should be six electrons around each flooring. We're gonna go ahead and draw those in. All right next we're going to have the formal charge for our sulfur. So we're gonna have a formal charge for sulfur. It's gonna be the same equation. The number of valence electrons minus the bond lines minus the electrons surrounding each sulfur. So we know that must have a formal charge of zero Sulfur is in the group six a. So it has six valence electrons. The group number corresponds with the number of valence electrons. There are six bond lines around each Around that one sulfur. And we need to solve how many electrons we need solving for this, we get zero equals zero minus electrons and we get that the number of electrons is going to equal zero. So as the question stated, there should be no lone pairs on sulfur. And what we just solved for says that confirms it. And so this is going to be our overall diagram for that structure. Overall, I hope that this helped, and until next time.