What is the Difference Between 1s and 2s Orbital?

The main differences between 1s and 2s orbitals are:

1. Energy level: 1s orbital has a lower energy than the 2s orbital. Electrons fill lower energy orbitals first, so the 1s orbital is filled before the 2s orbital.
2. Size and shape: Both 1s and 2s orbitals are spherically symmetrical. However, the 2s orbital is larger in size than the 1s orbital. The radius of the 1s orbital is smaller, making it the smallest spherical shape among orbitals.
3. Probable regions: The 2s orbital has two most probable regions, while the 1s orbital has only one most probable region.
4. Nodal plane: The 2s orbital has one node, while the 1s orbital has no nodes.

In summary, the 1s orbital is closer to the nucleus, has a lower energy, and is smaller in size compared to the 2s orbital. The 2s orbital has a larger size, two most probable regions, and a nodal plane, while the 1s orbital has only one most probable region and no nodes.

Comparative Table: 1s vs 2s Orbital

The main difference between 1s and 2s orbitals is their energy levels, with the 1s orbital having a lower energy than the 2s orbital. Both orbitals have a spherical shape and can accommodate a maximum of two electrons. Here is a table summarizing their differences and similarities:

The 1s orbital is the closest to the nucleus and has the lowest energy among other orbitals. The 2s orbital, on the other hand, is farther from the nucleus and has a higher energy level. Electrons fill low energy orbitals (closer to the nucleus) before they fill higher energy ones.