Look at the location in the periodic table of elements A, B, C, and D. What is the electron configuration of the transition metal in each of the following ions?

(c) C3+

(d) DO42-

Video transcript

Examine the position of element A in the periodic table for the ion below determine the electron configuration of the transition metal. So if we were to reference a periodic table, we could note that A is in the Cobalt position. So Cobalt is a member of the D lock on a periodic table and has an atomic number of 27. And so to determine its electron configuration, we first need to reference the noble gas that precedes it, which is argon. So we put that in brackets and then we continue to fill the next row. So once we have filled the argon, we move on to the next row, which is the four s section of the periodic table, we have forest two and then we enter in the forest two is to represent the first two electrons in the S block, we then move into the D block and we have 123456 and seven. So that is what A is if we were to determine a two plus, this means that we have lost two electrons. And so transition metals typically lose their highest shell number first when forming cations. And So when Cobalt will lose two electrons to form a two plus, we will remove electrons from the four s orbital first, since it is highest shell number. And so once we do that, we simply have argon in brackets followed by 3d 7 or answer choice. A as our final answer overall, I hope this helped. And until next time.