What is the Difference Between Bohr and Schrodinger Model?

The Bohr and Schrödinger models are two different approaches to understanding the structure of atoms and the behavior of electrons. Here are the main differences between the two models:

1. Dimensionality: The Bohr model is a one-dimensional model that used one quantum number to describe the distribution of electrons in the atom, with the only important information being the size of the orbit described by the n quantum number. On the other hand, Schrödinger's model allowed the electron to occupy three-dimensional space.
2. Electron Orbits: In the Bohr model, electrons occupy specific orbits or energy levels around the nucleus, with each orbit having a fixed energy. The Schrödinger model, however, describes electrons as standing waves with a greater probability of being in some areas of space, as described by the probability density function.
3. Applicability: The Bohr model is generally accurate for hydrogen atoms, which have a single electron and a small positively charged nucleus. The Schrödinger model, on the other hand, is more general and applicable to a wider range of atoms and molecules.
4. Uncertainty Principle: The Bohr model does not account for the Uncertainty Principle, while the Schrödinger model incorporates it.
5. Energy Levels: The Bohr model places electrons in specific energy levels, while the Schrödinger model allows electrons to have continuous energy values, as described by the energy eigenvalue equation.

In summary, the Bohr model is a simplified, one-dimensional model that accurately describes hydrogen-like atoms, while the Schrödinger model is a more general and comprehensive approach to understanding atomic structure and electron behavior.

Comparative Table: Bohr vs Schrodinger Model

Here is a table comparing the differences between the Bohr and Schrödinger models of atomic structure: