What is wrong with the following electron configurations?a. Ni 1s...

Question

What is wrong with the following electron configurations?a. Ni 1s^2 2s^2 2p^6 3s^2 3p^6 3d^10b. N 1s^2 2p^5c. Si 1s^2 2s^2 2p d. Mg 1s^2 2s^2 2p^6 3s

Accepted Answer

Hello everyone. So in this video, we want to identify the rule which is out ball principle. Hunt's rule or poly exclusion principle that violates or violated by the following electron configurations. So we have three different electron configurations, each breaking one of these rules. So let's first write out what each of these rules is starting off with the alphabetic principle. So we'll do this in red at pillow red start here. So the principle, this means that the electrons occupied orbital's in increasing energy. Now, for the second row, the hunt's role, do this in green. So for our Hunt's role, this means that electrons must single filled the degenerates orbital's before double filling them art. And the last rule that we have is the poly exclusion principle. So what the states is that two electrons in the same orbital must have opposite opposite spins. All right, let's take a look at the first one talking about lithium. Here, we have 21 S one and two P one. So this breaks the golf ball principle because the two S must be filled before the two P. So basically, they kind of just skip the two S and went straight to A two P and that's incorrect. And here again, we're violating the principle. Alright. For the second one, for oxygen we see here, we have been condensed electron configuration with the noble gas being helium. Then we go to S 22 P and then this right here. So what's going on here? And what's wrong about this is that we're breaking the poly exclusion principle room because we have two electrons here in the shell or in the same orbital being the identical spin, we usually want one, something like this one going up, one going down. In this case here, we only have two going up. So that is incorrect. And again, we're breaking the poly exclusion principle. All right. And lastly for P here, for our phosphorus, we again have a condensed electron configuration here. So we are starting with neon going to three S two and three P. So why this is wrong is that we're breaking huns rule. It states that the, again, the electrons must fill, must Singley fill the degenerate orbital's before double filling them. So instead of putting this down electron here, which have put one here before we go back to the first one here. Again, we're breaking hands, bro. Alright. So now that we have successfully identified all the rules that each of these examples broke, we go ahead and look at these answer choices and figuring out which kind of order is the correct one, we can see that since the first one. So number one is out about two is Polly and three is huns. The one that matches our determination, our determined answer is going to be answer choice. A so that's going to be this one right here. So as a choice is going to be my final answer for this problem.

What is wrong with the following electron configurations?a. Ni 1s^2 2s^2 2p^6 3s^2 3p^6 3d^10b. N 1s^2 2p^5c. Si 1s^2 2s^2 2p d. Mg 1s^2 2s^2 2p^6 3s

Key Concepts

Electron Configuration

Pauli Exclusion Principle

Hund's Rule

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