Each ball-and-stick model shows the electron and molecular geometry of a generic molecule. Explain what is wrong with each molecular geometry and provide the correct molecular geometry, given the number of lone pairs and bonding groups on the central atom. (c)

Video transcript

Hey everyone in this example, we need to select which Damon below correctly describes the molecular geometry and electron geometry for our given molecule, sulfur tetro fluoride. We should recognize that to predict these two geometries. We can use our A. X. E. Notation where we recall that A represents our central atom. In this case sulfur X. Represents any bonding regions. So that will include bonds attached to our central atom as well as lone pairs for a total of five bonding regions. So we would say so far that we have a X5 for our notation, which therefore tells us our electron geometry. And we would recognize a X5 notation as the following electron geometry, which is tribunal by pyramidal for our given molecule. Now to continue on with our notation, we have E. Which represents electron regions on our central atom and we would recognize that we have a lone pair attached to our central atom. So that would as a whole mean we have a X five E one notation and because we have this as a notation, we can therefore now predict our molecular geometry where we would recognize that because we have one electron pair on our central atom, we would recognize that we have seesaw molecular geometry for sulfur tetra fluoride. And so that means that the only correct choice to complete this example is choice A. As our final answer for the electron geometry and molecular geometry of sulfur tetra fluoride, I hope this helps if you have any questions, please leave them down below. Otherwise, I'll see everyone in the next practice video