write the electron configuration of an atom of the element highlighted in this outline of the periodic…
write the electron configuration of an atom of the element highlighted in this outline of the periodic table:\n\n1\n2\n3\n4\n5\n6\n7\n\nhe\nne\nar\nkr\nxe\nrn\n\nhint: you do not need to know the name or symbol of the highlighted element!
Answer
Explanation:
Step1: Identify the period of the element
The highlighted element is located in the 4th horizontal row. $$n = 4$$
Step2: Identify the block and group
The element is in the $d$-block (transition metals), specifically the 8th column of the $d$-block. $$d\text{-block, 8th element}$$
Step3: Determine the noble gas core
The noble gas preceding the 4th period is Argon. $$\text{Core: } [Ar]$$
Step4: Write the valence configuration
For the 4th period $d$-block, electrons fill the $4s$ and $3d$ orbitals. $$4s^{2} 3d^{8}$$
Step5: Combine for full configuration
Combine the noble gas core with the valence electrons. $$[Ar] 4s^{2} 3d^{8}$$
Answer:
$[Ar] 4s^{2} 3d^{8}$