Which solid in each pair has the higher melting point and why? c. Kr(s) or Xe(s)

Video transcript

hey everyone in this example, we need to determine which of these atoms has a lower melting point. And we need to explain our answer. So what we should recognize is that we have the atoms sodium and RB for rubidium which are located both in group one A of our periodic tables which we should recognize as our alkali metal group. So these are alkali metals. And when we recall our trend for atomic radius on our periodic table, we would recall that atomic radius is going to be increasing as we go towards the bottom left of our periodic table. So looking at first sodium on the periodic table again, we started seeing group but it's across period three vs rubidium we would see is also in group one a. But across period five. And so we would say that because rubidium is in period five, it's going to therefore be a larger adam because it has a larger atomic radius based on the trend that we've recalled and so therefore the ions or the ion. We should say that rubidium forms being in group one A. It should form a plus one ion. Well have a decreased ion density or we can say a decreased charge density, weakening the metallic bonds and decreasing its melting point. And so to overall explain our answer, we would say that rubidium has the lower melting point, sorry, lower melting point due to its weaker metallic bonds. And so this statement here is our final answer. As long or as well as our explanation as to why it has the lower melting point. I hope that everything I reviewed was clear. If you have any questions, please leave them down below, and I will see everyone in the next practice video.