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Choose the element with the more negative (more exothermic) electron affinity from each of the following pairs:a. $mathrm{Mg}$ or $mathrm{S}$b. $mathrm{K}$ or $math...

Question

Choose the element with the more negative (more exothermic) electron affinity from each of the following pairs:a. $mathrm{Mg}$ or $mathrm{S}$b. $mathrm{K}$ or $mathrm{Cs}$c. Si or $mathrm{P}$d. Ga or $mathrm{Br}$

Choose the element with the more negative (more exothermic) electron affinity from each of the following pairs: a. $mathrm{Mg}$ or $mathrm{S}$ b. $mathrm{K}$ or $mathrm{Cs}$ c. Si or $mathrm{P}$ d. Ga or $mathrm{Br}$



Answers

Choose the element with the higher first ionization energy in each pair.

a. P or I
b. Si or Cl
c. P or Sb
d. Ga or Ge

Okay. What we want to do is we want to talk about electronic affinity and electron affinity is really um is kind of talking about the energy released on on adding an electron to an atom. Okay. Um and um these are called there is an electronic affinity trend um based off of the periodic table um that um it increases as we look from left to right so increases as we go from left to right. It also increases as we look from down to up and increases means it actually gets more negative. Okay. Um so that electron affinity is really talking about um you know when we add or release an electron there's energy that is released. And it has to do with a Adams uh affinity to be able to attract or not attract that electron. Okay. So we want to kind of look at pairs of pears and see determine which one has the more negative electron affinity which one has the greatest electron affinity. Um So we have sodium or rubidium. So we have it. We noticed that sodium is here group idioms is two steps down so we know that it increases or gets more negative as we look from down to up. So that means sodium will have the more. Okay. Um And so now my second pair is going to be bore on or sulfur. So now I've got to find boron and sulfur. So here is born right here and here is sulfur. And so remember it gets more negative if I look from left to right and then also from down to up. And so even though boron is above, he's also a little bit more to the left of sulfur. Um So I would almost say that sulfur has some more. Okay. Um and now we're gonna do um carbon lips carbon or nitrogen. Um So that is up here. So remember carbon um we have more negative or the electronic infinity increases from left to right. So of course that's going to be nitrogen. That one was easier because it was on the same road. And then the last warned you is lithium or flurry. Um And it really is. Um this flooring right here, right, listens over here Florence way over here. Um So of course it's gonna be a flurry.

Right, Theis question as us between these elements, which one has ah, more negative electron affinity. Um, so between magnetism and so far. So for a little affinity. If you move from the left to the right off the periodic table, the affinity, uh, electron affinity will increase in another word. Um, the electron affinity will be more negative. And so silver is this this position and he s mechanism. So for sure so far will have a more negative electron definitive compare with him between potassium and cesium. So for the first road for the first column, if you move now, the electoral affinity actually decrease, which mean that, um the lower the element, it will have my positive electron affinity. And so, in this case, potassium will have a more negative electron affinity between silicon and force for force for us. So silicon and force for us force for us is the exception with this train because it has 1/2 filled Alberto. An addition off any electron to its half their orbital will increase the repulsion of the two electrons. And in as a consequence, um, it has, uh, weaker electron affinity as compared with silica on dso between the two Silicon should have the more negative electron affinity on the last one would be gallium and roaming. So this is, uh, roaming. And this is ah, gallium where? Wait a minute. And if I talk here, So we have followed the same train. If you move to the right of the periodic table, the elements on the right will have a stronger electron affinity compared with the one on the left. So roaming should have, um, are negative, uh, Mark after an affinity compared with gallium

Depending on the different group of Adam and its location on the you're gonna take over to answer these questions. So, for a we're looking at A versus RV. They're both in the same column with the periodic table. But they're in one's RV is to hose down, or they are Panay. And so for this one, we're interested in the one that is further up that periodic tables. The correct answer is any for a for be there, um, in different chemical groups are different. Come, punk. Oops. I'm so for for this case, we're more interested and be who we are us because they're in different groups. First, he we have CNN horseshit both next to each other based on the different group of therein the Martian sea trip. Um, Mrs Good there. Indeed I am. A lie and a fracture in the same column of bare table on complete opposite sides and sense of has a charge off. Just one minus, huh? It really wants that extra electron. It has the higher affinity in this case

So now I work on problem 80 from chapter eight. In this problem, we were asked to choose the element with the more negative, which means more X, a thermic electron affinity from each pair. So our trend four electron affinity here will be a increases As you go from left to right. This is a general trend and from bottom to top. So here we want the one that is more electron affinity by saying more negative, they mean which we're talking about in Philippi. We're talking about the heat released and since the ones that are more likely to join with an electrons will be the ones that release energy and doing so. So we want to see the ones we wantto see the element that follows this trend here. And so the first, um, pair that we have is magnesium and sulfur. We can see that sulfur as much farther to the right, so sulfur will be the one that has the higher electron affinity, which means more X, a thermic electron affinity When that makes sense, because sulfur should want to gain electrons to get noble gas configuration, whereas magnesium would want to lose them to obtain noble gas configuration. Then we have potassium or cesium, which are in the same column. But potassium is much higher, and based on the trend here, potassium will be the one that has a higher electron affinity. This is because the balance orbital's are much closer to the nucleus and more likely to attract a new electron and part C were given silicone or phosphorus. Now, this one here is tricky, because phosphorus is higher up on the periodic table there farther to the right, it's farther to the right, so it that has more electron affinity. However, the answer is silicon. And the reason for this is because P has 1/2 filled UH, P sub shell. Bosphorous has 1/2 filled P show, so that makes it a little more stable, so it's a little less likely to add an electron to pair with one of its P electrons. Then it would be otherwise. So you see this trend here is the general trend and and we always have to look at the specific problem to see if there any exceptions, such as stability that we get here from having the half lp social. The fourth part here is gallium or bro mean in here. We can easily see The romaine is farther to the right on this periodic table. So Romain is the one that has a higher electron affinity.


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