8B.3 Why is the electronic configuration of the yttrium atom [Kr]4d15s2 and that of the silver atom [Kr] 4d 105s¹?

Explain, in terms of Coulombic energy and Exchange energy, why the ground-state electron configuration of Cr is [Ar]4s13d5 instead of [Ar]4s23d4.

What is the identity of the ion with an electron configuration [Xe]4f145d9 and has a charge of +4?

Write electron configurations for the following ions of d-block elements: (a) Zn2+, (b) Mn2+, and (c) Cr3+.

(a) As we go down the periodic table, which subshell is filled first, the 3d or the 4s subshell? (b) Which electronic configuration has a lower energy, [Ar]3d44s2 or [Ar]3d54s1? Note: The notation [Ar] represents the filled configuration for argon. Suggestion: Which has the greater number of unpaired spins? (c) Identify the element with the electronic configuration in part (b).

(1) What is the name of the element with a valence electron configuration of 2s22p3?fill in the blank 1(2) What is the name of the element with a valence electron configuration of 3s2?

An ion with a +4 charge has a ground state electron configuration of [Ar]3d3. What is the ion?

[Ar]4s23d2 is the electron configuration for Zirconium Titanium Vanadium Scandium

Which element has the following ground-state electron configuration? (Ne]3s23p3

[Ar]4s 23d 104p 3 is the electron configuration of a(n) O V atom. As Sb P Sn