Question

use the periodic table to determine the electron configuration for dysprosium (dy) and americium (am) in noble - gas notation.
dy:
xe6s²6f¹⁰
xe6s²4f¹⁰
rn6s²6f¹⁰
rn6s²4f¹⁰

Explanation:

Step1: Determine the noble - gas core

Dysprosium (Dy) has an atomic number of 66. The noble gas with an atomic number less than 66 is Xenon (Xe) which has an atomic number of 54.

Step2: Determine the remaining electrons

The number of remaining electrons is \(66 - 54=12\). The electron configuration after the noble - gas core is filled as follows: The \(6s\) orbital can hold 2 electrons (\(6s^{2}\)), and the \(4f\) orbital (since it is in the lanthanide series, the \(4f\) orbitals are being filled) can hold 10 electrons (\(4f^{10}\)).

Answer:

\([Xe]6s^{2}4f^{10}\)