What is the electron configuration of sulfur (S)
The Correct Answer and Explanation is:
The electron configuration of sulfur (S), with an atomic number of 16, can be written as:
1s² 2s² 2p⁶ 3s² 3p⁴
Explanation:
- Atomic Number: The atomic number of sulfur is 16, which means it has 16 electrons. Electrons are arranged in shells around the nucleus in an order that minimizes energy.
- First Energy Level (n=1): The first shell can hold a maximum of 2 electrons. The first 2 electrons fill the 1s orbital, resulting in the configuration 1s².
- Second Energy Level (n=2): The second shell can hold up to 8 electrons. It first fills the 2s orbital with 2 electrons (2s²). Then, it fills the 2p orbitals with 6 electrons (2p⁶), as the 2p orbitals can accommodate up to 6 electrons.
- Third Energy Level (n=3): The third shell can also hold up to 8 electrons. It fills the 3s orbital with 2 electrons (3s²). After the 3s orbital is filled, there are 4 remaining electrons, which fill the 3p orbitals. This results in a 3p⁴ configuration, where 4 electrons are in the 3p orbitals.
Electron Configuration Breakdown:
- 1s²: 2 electrons in the 1st energy level’s s orbital.
- 2s²: 2 electrons in the 2nd energy level’s s orbital.
- 2p⁶: 6 electrons in the 2nd energy level’s p orbitals.
- 3s²: 2 electrons in the 3rd energy level’s s orbital.
- 3p⁴: 4 electrons in the 3rd energy level’s p orbitals.
Thus, the full electron configuration for sulfur is 1s² 2s² 2p⁶ 3s² 3p⁴. This notation shows how the electrons are distributed across the various orbitals. Since sulfur is in period 3 and group 16 of the periodic table, its outermost electrons are in the 3p orbitals, making it part of the chalcogen group.
