Both vanadium and its 3+ ion are paramagnetic. Refer to their electron configurations to explain this statement.

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hey everyone in this example, we need to think of the electron configurations of titanium two plus carry on. And the titanium neutral atom and we need to explain why based on these electron configurations, this pair are both para magnetic. So we want to go ahead and we can express our electron configurations through orbital diagrams. So we want to recall that titanium is located across period four in group four B. of Our Transition Metal Block. And we would recall that the transition metal block is located in the D block, which is our sub level for our two atoms here. So to write out our orbital diagram and our electron configuration, we would start out with the lowest sublevel number and that would be the fourth energy level at the S sub level because it's the smallest sub level. We should recall that R. S. Sublevel only has one orbital. So we can draw in one box here to represent our single orbital in the S sublevel. And then we want to recognize that titanium again is in the D block corresponding to the D sublevel. So we would move on to our D. Block which across the fourth period will begin at the third energy level, three D. And we should recall that our D block contains a total of five orbital's. So we would draw in five boxes Which can hold a maximum of 10 electrons. So we can even this out and just draw three D. In the midst of these five orbital's now because we recognize that we have two types of titanium atoms are first being a titanium two plus Catalan and our second being a neutral titanium atom. We're going to draw in two of these orbital diagrams because they're going to have different orbital diagrams based on that difference in charge. Now, when we go to our fourth period or the fourth energy level on our periodic tables to land on titanium, we're going to count four counts where we would land on the titanium atom. And so that corresponds to a total of four electrons that we would need to fill in our orbital diagram here. So we want to recall our ALF about principle which states that we should fill in our lowest energy sub level first before moving on to fill in our higher energy sublevel. And we also want to recall hans rule which states that we should fill in an electron within the orbital first within the direction of a arrow facing up and then with a direction of another electron represented by a downward arrow. And this is for each orbital. So beginning with our titanium neutral atom here will start here, we're going to fill in our four electrons which correspond to the count of four, which allows us to land on the titanium atom first in our lowest energy sub level where again we have one electron represented by an upward arrow. And then following Hunt's rule, we would place our second electron in the first orbital of the s sub level in a downward arrow direction. So this represents the two of the four electrons that we should fill in for our titanium orbital diagram. And so we have two more electrons to fill in. And to honor Hunt's Rule, we will fill in the last two electrons where we have an upward arrow in the first orbital and then another upward arrow in the second orbital. And this would honor both huns rule and our ALF about principle which we recalled above. We should recognize that in our titanium two plus ion R two plus charge or a positive charge tells us that we will lose that number of electrons. So in this case we're going to lose two electrons. And in order to remove these two electrons, we want to remove them from the lowest energy sublevel. And so that would leave us with two electrons in which we would go ahead and fill in our outermost sub level, which is our three D sublevel here. So we would honor huns rule by drawing in these two electrons first in an upward direction arrow and then in the second orbital also in an upward direction arrow. And this would complete our orbital diagram for the titanium two plus carry on because we would have removed the two electrons that would have been in our original for us orbital. And so the next step is to recall our definition of para magnetic, which states that we would have a weak magnetic attraction between our atoms, two magnets that are externally applied, which would therefore form an induced internal magnetic attraction that is parallel to the direction of the externally applied magnetic force. And so we would go ahead and confirm that para magnetic is also defined other than by that formal direction. It's also defined by the presence of unpaid electrons in our orbital's. And so because we do have unpaid electrons in our three D sub level here, that would correspond to a para magnetic property between our two medals, the titanium Catalan and the titanium neutral atom. And so based on these facts we've outlined, we can go ahead and confirm that choice. A is going to be the most accurate answer choice to define as to why based on our electron configurations. In our diagrams here, The titanium two plus carry on. And the titanium neutral atom are both para magnetic. And that again is due to the fact that they both have unpaid electrons in their configuration. So A will complete this example as our final answer. And if you have any questions, just leave them down below. Otherwise, I'll see everyone in the next practice video

Both vanadium and its 3+ ion are paramagnetic. Refer to their electron configurations to explain this statement.

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Key Concepts

Electron Configuration

Paramagnetism

Ionization and Electron Loss