Neither strontium (Sr) nor antimony (Sb) is shown in the activity series of Table 4.5. Based on their positions in the periodic table, which would you expect to be the better reducing agent? Will the following reaction occur? Explain.

Video transcript

Hello. Everyone in this video, we're given this reaction right over here, we're not taking into consideration their activity series. But we're looking at positions on the table. I was trying to identify if this reaction will occur and also to identify the better reducing agents. So when we're comparing rubidium and cadmium they're on the same period in the periodic table. So where rubidium is is in group one a. was gonna write this out. So Rubidium is in group one a. And then cadmium. So C. D. That's in that's the last element in the column in the transition metals. Let's just say in the deep block. Okay so the reason why we consider the position of these elements is because there's a pr day trend to kind of help us out to solve this problem. So let's recall that the tax property increases from right to left. So if this were to be the pr table, the metallic property increases from right to left. So this way and we're increasing here. So we're comparing rubidium to cadmium, rubidium is more metallic between the two because because there is a metallic significance between two, we can say that there's a detox reaction that occurs. So we have determined then that rubidium is a more metallic character compared to cadmium. So that that means that rubidium is going to be a better reducing agent in our case. That means out of these four different statements that we have. The correct statement is going to be be where we say that rubidium is the better reducing agent and the reaction will occur