Questions: Write the electron configuration of an atom of the element highlighted in this outline of the Periodic Table: Hint: you do not need to know the name or symbol of the highlighted element! [Kr] 6s^2 5d^10 6p^6

Write the electron configuration of an atom of the element highlighted in this outline of the Periodic Table:

Hint: you do not need to know the name or symbol of the highlighted element!
[Kr] 6s^2 5d^10 6p^6

Transcript text: Write the electron configuration of an atom of the element highlighted in this outline of the Periodic Table: Hint: you do not need to know the name or symbol of the highlighted element! \[ [\mathrm{Kr}] 6 s^{2} 5 d^{10} 6 p^{6} \]

Solution

Solution Steps

Step 1: Locate the highlighted element

The highlighted element is located in the 6th row and the 18th column (last column) of the periodic table.

Step 2: Determine the electron configuration

The noble gases are located in the last column of the periodic table. The highlighted element is in the 6th row. The noble gas in the 5th row is Xenon (Xe), so we begin the electron configuration with [Xe].

The sixth row begins by filling the 6s orbital. Since the highlighted element is in the 18th column and the first two columns correspond to the s-block, there are two electrons in the 6s orbital.

Next, the f-orbitals are filled. Since there are 14 elements in the f-block, we add 4f¹⁴ to the configuration.

After the f-orbitals, the d-orbitals are filled. Since the d-block has 10 elements, we add 5d¹⁰. (Note that the d-orbitals are one less than the current row, hence the 5d.)

Finally, the p-orbitals are filled. The highlighted element is in the 18th column, which is the sixth column in the p-block, therefore we add 6p⁶ to the configuration. (The p-orbitals correspond to the same row number as the element, hence 6p.)

Final Answer:

[Xe] 6s² 4f¹⁴ 5d¹⁰ 6p⁶

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