write the electron configuration of an atom of the element highlighted in this outline of the periodic…

Explanation:

Step1: Identify the element's position

The highlighted element is in Period 4 and is the second element in the d-block (Group 4).

Step2: Determine the noble gas core

The noble gas preceding Period 4 is Argon ($Ar$).

Step3: Fill the remaining orbitals

Period 4 starts with the $4s$ orbital (2 electrons). The d-block starts filling the $(n-1)d$ orbital, which is $3d$. Being the second element in the d-block, it has 2 electrons in the $3d$ orbital.

Step4: Combine the components

The full configuration is $[Ar] 4s^{2} 3d^{2}$ or $1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2} 3d^{2}$.

Answer:

$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2} 3d^{2}$ (or $[Ar] 4s^{2} 3d^{2}$)