The unit cell of nickel arsenide is shown here. (b) What is the empirical formula?

Video transcript

Hello everyone today we have a falling problem. Consider the unit cell of titanium for oxide. So in a unit cell Adams had different contributions depending on their location. So for example, we may have corner atoms. Corner atoms would be this example here. So this will be a corner adam And that's going to contribute 1/8 to the cell. We may have atoms inside such as this right here. This would be considered atoms that are inside and that would contribute 1 to the cell or we may have atoms in the face of cube. And so an example of that would be this molecule here. This would go ahead and be an oxygen. That is a face in the queue And that's going to contribute 1/2. And so we're gonna examine each of these atoms differently. So with oxygen, oxygen is positioned as a face adam within the cell and so we actually have four of those and they each contribute 1/2 and so that's going to equal to oxygen also has inside atoms And there's two of those. So two times the one contribute contribution they give gives us two as well. So this is going to give us four overall for titanium. We noticed that we have inside tight teams and we have two of those and so that example is going to be this one here. This is going to be an inside titanium and we have two of those and those each contribute one, so that's going to equal to and so we put the formula together, that's going to be titanium to oxygen four, which simplifies to t i 02 as our final answer. And this is our empirical formula. Overall, I hope this helped, and until next time.