Question

using the drop down choices below, complete the ground state electron configuration for an atom of nickel. note: if an orbital doesnt contain electrons, select a value of \0\ from the list (for the purposes of this question only). ar 4s 3d 4p

Explanation:

Step1: Determine the atomic number of nickel

Nickel (\(Ni\)) has an atomic number \(Z = 28\). Argon (\(Ar\)) has an atomic number \(Z=18\).

Step2: Calculate the number of electrons after \([Ar]\)

The number of electrons remaining is \(28 - 18=10\).

Step3: Fill the \(4s\) and \(3d\) orbitals

The \(4s\) orbital fills before the \(3d\) orbital. The \(4s\) orbital can hold a maximum of \(2\) electrons. After filling \(4s\) (\(2\) electrons), we have \(10 - 2 = 8\) electrons left for the \(3d\) orbital. The \(4p\) orbital has \(0\) electrons in the ground - state of nickel.

Answer:

\([Ar]4s^{2}3d^{8}4p^{0}\)