What is the electron configuration of a tin (Sn) atom (Z=50)?

The electron configuration of a tin (Sn) atom, which has an atomic number of 50, is:

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p2

This configuration tells us how the electrons are distributed across the various atomic orbitals.

The breakdown is as follows:

• 1s²: The first energy level can hold a maximum of 2 electrons, both of which fill the 1s orbital.
• 2s² 2p⁶: The second energy level consists of the 2s and 2p orbitals, filling them with 2 in 2s and 6 in 2p.
• 3s² 3p⁶: Similarly, the third energy level is filled with 2 electrons in the 3s and 6 in the 3p orbitals.
• 4s²: The 4s orbital is filled next with 2 electrons.
• 3d¹⁰: After 4s, the 3d orbital can hold up to 10 electrons, filling it completely.
• 4p⁶: The 4p orbital is filled with 6 electrons.
• 5s²: The 5s orbital also receives 2 electrons.
• 4d¹⁰: The 4d orbital fills completely with 10 electrons.
• 5p²: Finally, 2 electrons fill the 5p orbital.

Thus, the complete configuration reflects how the electrons are arranged to minimize energy and creates the chemical properties characteristic of tin.