Assuming that g orbitals fill according to Hund's rule, what is the atomic number of the first element to have a filled g orbital?

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Hello everyone today. We have the following problem. Following the off ball principle, identify the atomic number with a completed eight p orbital. So the off ball principle is just a method by which our orbital's or electrons are filled in to our orbital's and so generally we have our s orbital's RP orbital's our D orbital's and our f orbital's. And so we're gonna start off, we always start off with our one s orbital, that's the first energy level S is the first sub shell and then we're gonna say two because we're filling in those first two, electrons would move right across the periodic table. We move to the next row or the next period. So we have to s as well and then to move to the right hand side of the periodic table where we have two P six and it's important to note that S and P are going to have the same energy levels. So we moved from two P to three S two because we're filling in those first two electrons. Once again, we move straight across three P six because we're filling in all six of those electrons, we move into the four s orbital, we're filling in those first two. And this is when we encounter the transition metals and transition metals in the D orbital always starts at three D. And so we're going to say three D 10 because we're filling in all of those, we moved straight across and just as before we're gonna have four P six, we're gonna have fours for our S and P because they're in the same energy levels from four P six, we move to the next row, which is five S two after five, that's two, we're getting into the transition metals once again. And so we encounter three D 10. So next is four D 10. And so there is a simple pattern going on here. After our 40 10, we move right along to the right hand side of the periodic table where we encounter five P six, We move on to the 6th period, which is success to and then after six S two, we move into what's known as the f orbital And our f orbital can accommodate up to 14 electrons. And so after we moved to the f orbital, we moved right back to our d orbital. So as you said before, our d orbital is always going to be one less than R. S and p orbital's. And if you notice our f orbital is always going to be to less than R. S and R. P. So moving right along from R five D 10, we moved to the right hand side of the periodic table where we encounter six P six. We moved to the seventh energy level. So we have seven S two, we encountered four F 14. So next is five F 14 and that's gonna be it for the F series, there's only four F and five F. So once we move from F, we move right to our d orbital and our D orbital is going to be six D 10 because remember, but it was always one less than Rs and RP Once we do that, we move right on along to the right hand side of the periodic table where we have our seven p 6. Now we're in the 8th period. And so that's where we have our eight S 2. And so this is a new energy level That's going to be introduced and it's going to be known as the five G Orbital. And that can hold a maximum of 18 electrons. So we're going to add this one in as a special orbital. And so now that we enter the G After the G, we're going to enter six F and then after our six F 14, we go back to the D orbital's. So we have seven D 10 and last, but not least on the right hand side of the periodic table, we have our eight P six. And so if we add up all of these electrons here, all of our exponents here, they are going to give us the number of electrons that we are looking for for answer and plugging them into our calculator, We are going to get 168 electrons or the atomic number. And with that we've answered our question overall, I hope that this helped. And until next time

Assuming that g orbitals fill according to Hund's rule, what is the atomic number of the first element to have a filled g orbital?

Verified Solution

Key Concepts

Hund's Rule

Electron Configuration

Atomic Number and Periodic Table