. Explain the difference between the 3
, 3
, and the 3
orbital of the same atom.
The Correct Answer and Explanation is:
The 3s3s3s, 3p3p3p, and 3d3d3d orbitals all belong to the same principal energy level (n = 3) in an atom, but they have different shapes, energy levels, and numbers of orbitals within that energy level. Here’s how they differ:
- Shape and Number of Orbitals:
- 3s3s3s orbital: The 3s3s3s orbital is spherical in shape, and it has one orbital. This means that within the third energy level, there is only one 3s3s3s orbital, which can hold up to two electrons.
- 3p3p3p orbitals: The 3p3p3p orbitals have a dumbbell shape and there are three of them (3px3p_x3px, 3py3p_y3py, 3pz3p_z3pz) in the third energy level. Each of these orbitals can hold two electrons, giving a total of six electrons for the 3p3p3p orbitals.
- 3d3d3d orbitals: The 3d3d3d orbitals have more complex shapes, often described as cloverleaf-like, and there are five 3d3d3d orbitals in the third energy level. These orbitals can collectively hold ten electrons.
- Energy Levels:
- The energy of orbitals increases as the angular momentum quantum number increases. Therefore, the 3s3s3s orbital has the lowest energy, followed by the 3p3p3p orbitals, and the 3d3d3d orbitals have the highest energy in the third principal energy level.
- Electron Configuration:
- Electrons will fill these orbitals in a specific order, starting with the lowest energy. The 3s3s3s orbital will fill first, followed by the 3p3p3p orbitals, and then the 3d3d3d orbitals, but only once the 3s3s3s and 3p3p3p orbitals are filled.
In summary, while all three orbitals (3s3s3s, 3p3p3p, and 3d3d3d) exist in the same energy level, they differ in shape, the number of available orbitals, and energy. The 3s3s3s orbital is spherical and holds 2 electrons, the 3p3p3p orbitals are dumbbell-shaped and hold 6 electrons, and the 3d3d3d orbitals are more complex and hold 10 electrons.
