Final Answer:
To create an atomic model for sulfur, we utilize the electron configuration and orbital shapes. Sulfur has an atomic number of 16, indicating 16 electrons arranged in shells and subshells. The electron configuration of sulfur is 1s² 2s² 2p⁶ 3s² 3p⁴. The 's' and 'p' orbitals depict the electron distribution. The 's' orbital is spherical and holds up to 2 electrons, while 'p' orbitals come in three orientations (px, py, pz) and can hold a total of 6 electrons (2 in each orientation).
Step-by-step explanation:
1.Atomic Number and Electron Configuration:
Sulfur, with an atomic number of 16, has 16 electrons distributed across its energy levels. The electron configuration indicates the arrangement of these electrons within the orbitals. For sulfur, the electron configuration is 1s² 2s² 2p⁶ 3s² 3p⁴. This breakdown shows how electrons fill the different energy levels and sublevels, with 's' and 'p' orbitals being the primary focus for sulfur's atomic model.
2.Orbital Shapes 's' and 'p':
- 's' Orbital: It is spherical in shape and can accommodate a maximum of 2 electrons. In the sulfur atom, the 1s and 2s orbitals are 's' orbitals.
- 'p' Orbital: These orbitals have three orientations: px, py, and pz. Each 'p' orbital can hold a maximum of 2 electrons, and collectively, the 'p' orbitals can accommodate 6 electrons. For sulfur, the 2p and 3p orbitals are 'p' orbitals.
3.Three Orientations of 'p' Sublevels:
The 'p' orbitals have three distinct orientations along the x, y, and z axes:
- px: Aligned along the x-axis.
- py: Aligned along the y-axis.
- pz: Aligned along the z-axis.
By understanding the electron configuration and orbital shapes, we can visualize how the electrons are distributed in the different orbitals within the sulfur atom, particularly in the 's' and 'p' orbitals and their respective orientations.