the ground-state electron configuration of Y3+ is
Y3+: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6
When you are determining the electronic configuration of a transition metal ion, you have to be careful be the last electrons added to the configuration for the neutral atom are not the first to be removed upon ionization. You should, however, start with the electronic configuration of the neutral metal atom.
In the case if yttrium,
Y: [Kr] 5s2 4d1
The first electrons to be removed are the 5s electrons. So if the charge were less than +3, you should focus on removing those electrons first. However, in the case if a Y+3 ion, you should remove all three valence electrons (those outside of the [Kr] core. The resulting ion will be isoelectronic with Krypton.
digital configuration of Carbon (C), Nitrogen(N), Oxygen(O) are as follows: C(6)- 1s2 2s2 2Px1 2Py1 N(7)- 1s2 2s2 2Px1 2Py1 2Pz1 O(8)- 1s2 2s2 2Px2 2Py1 2Pz1 the following, Carbon has 2 electrons in its 2p subshell. So, there is an chance to make strong 1/2-crammed P orbital in the perfect shell of Carbon by gaining a million electron. So, to achieve stability Carbon can honestly income a million electron. on the otherhand, Nitrogen has already 1/2-crammed P orbital in the perfect shell. So, it received’t settle for more suitable electrons via the indisputable fact that is robust adequate. to achieve extra electrons it has to break its stability. because of this, Nitrogen is a lot less positive(extra effective) than that of Carbon In case of Oxygen, there r 4 electrons in P orbital. that is neither 1/2-crammed nor complete-crammed. So it isn’t strong adequate to achieve extra electrons. So, oxygen can also income extra electrons in its outermost shell ensuing in a extra perfect eelectronic affinity than Nitrogen. for this reason, digital affinity of Nitrogen> Carbon & Oxygen
1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 is the electron configuration for Y3+
what element is Y….????? Are u leaving part of the question…???
Source(s): Am a born chemist