In this video we'll write the electron configuration for Ag and AG, plus this is silver and the silver ion. So when we do this silvers a bit of an exception, so we have to be careful, let's, take our time and get this right. So we have the periodic table here, and it's divided up into these orbital blocks. This will be real helpful for us. We can see silver, right here, that's 47 so silver on the periodic table that has an atomic number of 47. All these elements are neutral. That means that the number of.

Protons and electrons they'll be the same 47 is the atomic number that's, the number of protons. So we have 47 electrons for just silver neutral, atom silver so let's write the electron configuration for silver. So we'll start here we have 1s 1. So we have 1. S, 1 1. S, 2, that's full, so we're, just going to write 1. S, 2 to s, 1 to s, 2, that's full.

We go 2 to P 1 2, 3, 4 5, 6, P holds up to 6. So we have 2 P, 6 and let's stop for a second, because where should we end based on this table? If we follow over here, we. Have 4 D 1 2, 3, 4 5, 6, 7, 8 9. So we should end in 4d 9, so it's helpful to think about that. And this is why this is really a helpful table. Let's go on.

We had 2p6, 3s2, 3p6 4s2. And then we go from the 4 s to the 3. D. D can hold up to 10, so we'll, put 3 D 10 and remember silver has atomic number 47. So 47 protons 47. Electrons.

All these numbers are going to need to add up to 47. So I have 3 D. Then 4 p, 6 5, s, 2 and then 4d nine, which is where we wanted to end up. This is the electron configuration for AG. Just. Based on using this table, if you used one of these electron configuration charts, you'd get the same answer. So all these numbers add up to 47 silver, though is an exception. So we have to think about this a little more.

This is not correct. This is not what we see in the lab or in our experiments. So let's write the correct electron configuration for silver, and then it'll be easy to do it for the silver ion.

So the first thing we need to correct is with transition metals. Those d-block elements, the.3D is written before the 4s, so we'll replace that and then over here. So this is a little better, it's more accurate. So we have this now as our electron configuration, which still isn't correct when we look at the diagram here, we have our 1s1 1s2 they're in opposite directions. So this is full we go to two s, two.

And so on. If we go out here and look at the 4d in the 5s, we see this 4d it's 49. So two, four, six, eight, nine, electrons, it's, not full. And what experiments have told us is that half filled. Or completely filled D orbitals, they are more stable.

So here, if we had one more electron here, this would be much more stable. So we could take this electron here and move it over from the 5s to that 4d, and we could fill this out. Now, this is a full D orbital. This is full. And now we have one here.

So we should update these numbers here. Now we have that 3 D 10, and we have the 5. S, 1. And this is the correct electron configuration for AG for silver. So we needed to understand that this 4d, if we had. This full or just 1 in each one of these little sub orbitals here that would be much more stable using that information let's do the electron configuration for just AG, plus so here's silver again and to become positive. We need to lose an electron.

We need negative charge. So this goes away here, this becomes positive. And this is the electron configuration for AG.

Plus we just lost this one 5s, one electron so that's it. So these are the electron configurations for AJ here and then AG, plus this is Dr. B, and thanks for watching.