Question

to what element does the following electronic configuration belong? xe 6s²4f¹⁴5d¹⁰6p² po p cd pb ag

Explanation:

Step1: Determine the atomic number of Xe

Xe (Xenon) has an atomic number of 54.

Step2: Calculate the total number of electrons

The given electronic configuration is \([Xe]6s^{2}4f^{14}5d^{10}6p^{2}\).
The number of electrons from the part outside \([Xe]\) is \(2 + 14+10 + 2=28\).
The total number of electrons \(N=54 + 28=82\).

Step3: Match the atomic number with the elements

• Po (Polonium) has an atomic number of 84.
• P (Phosphorus) has an atomic number of 15.
• Cd (Cadmium) has an atomic number of 48.
• Pb (Lead) has an atomic number of 82.
• Ag (Silver) has an atomic number of 47.

Answer:

Pb