Question

question 8 of 18
write the full electronic configuration for lead (pb).
electronic configuration:

Explanation:

Step1: Determine the atomic number of lead

Lead (Pb) has an atomic number of 82. This means it has 82 electrons.

Step2: Fill the electron shells following the Aufbau principle

Start filling the shells in the order \(1s\), \(2s\), \(2p\), \(3s\), \(3p\), \(4s\), \(3d\), \(4p\), \(5s\), \(4d\), \(5p\), \(6s\), \(4f\), \(5d\), \(6p\).

• \(1s\) can hold 2 electrons: \(1s^{2}\)
• \(2s\) can hold 2 electrons: \(2s^{2}\)
• \(2p\) can hold 6 electrons: \(2p^{6}\)
• \(3s\) can hold 2 electrons: \(3s^{2}\)
• \(3p\) can hold 6 electrons: \(3p^{6}\)
• \(4s\) can hold 2 electrons: \(4s^{2}\)
• \(3d\) can hold 10 electrons: \(3d^{10}\)
• \(4p\) can hold 6 electrons: \(4p^{6}\)
• \(5s\) can hold 2 electrons: \(5s^{2}\)
• \(4d\) can hold 10 electrons: \(4d^{10}\)
• \(5p\) can hold 6 electrons: \(5p^{6}\)
• \(6s\) can hold 2 electrons: \(6s^{2}\)
• \(4f\) can hold 14 electrons: \(4f^{14}\)
• \(5d\) can hold 10 electrons: \(5d^{10}\)
• \(6p\) can hold 2 electrons (since we have 82 electrons in total and after filling the previous shells we have 2 left for \(6p\)): \(6p^{2}\)

Answer:

\(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{2}\)