Chlorine reacts with molten sulfur to yield disulfur dichloride, a yellowish-red liquid. Propose a structure for disulfur dichloride.

Video transcript

Hi, everyone. Let's take a look at our next question. The reaction of oxygen with fluorine at very low temperatures yields di oxygen di fluoride, an orange colored solid, draw the structure of deoxy di fluoride. So to think of a possible structure, we'd want to start with how many valence electrons do we have here? So we have dye oxygen di fluoride. So 02 f two oxygen has six valence electrons. It's in group six A. So that would be six electrons multiplied by two atoms of oxygen and then fluorine has seven valence electrons. So seven electrons multiplied by two atoms of fluorine that's gonna give us 12 plus 14. So 26 valence electrons that we need to account for. So we've got our two oxygens and two floorings. So let's think about how they might be expected to bond. Well, fluorine with its seven valence electrons and high electronegativity would be expected to only make one bond. Whereas oxygen is quite comfortable having two bonds. So that leads us to assume that we'll have our oxygens bound to each other in the middle of the molecule and our fluorine on either end. So that gives us fluorine, oxygen, oxygen fluorine, we've got three bonds. So we take our 26 valence electrons and subtract six bonding electrons and we're left with 20 electrons to account for here. Well, our oxygen is in the middle, we give them two lone pairs each and that's going to be eight. So there's 12 left while giving each flooring three lone pairs, each picks up the last of those. So we've accounted for all of our electrons as well as put each of our atoms in a comfortable arrangement for them. The fourinth at the end with just one bond, they've got a complete shell and there are seven valence electrons, the oxygens in the middle, each with two bonds and two lone pairs. So surrounded by six electrons and also a complete octet. Now, we just need to think about the geometrical arrangement here. Our oxygens each have two lone pairs and two bonds. So they're going to form that bent structure, we only have single bonds. So we'll have sp three hybridization. So that will give us a tetrahedral geometry for our orbitals. But two of those orders will be filled with lone pairs. So just like water, there will be a bent structure there. So if we draw our expected structure with the geometrical arrangement, we'll have an oxygen with a fluorine and oxygen coming down from it and that bent structure and the two lone pairs, and we'd expect the other flooring to want to be as far away in space as possible from the first flooring. So we'll have it in sort of a or a double bond, you'd call it a trans arrangement going out the opposite side of the second oxygen and it having its two lone pairs to make another bent arrangement there. So we've got our structure with our two oxygens in the middle, the fluorine on the outside, all single bonds. And we have the bent arrangement of the two oxygens keeping the fluorine as far away from each other as possible. So there is our proposed structure for deoxy di fluoride. See you in the next video.