Niels Bohr Model: Exploring Hydrogen Orbits

[Milind_shyani]

Hi,
we know that we can find the radius and energy of the orbits of hydrogen.now why is it so that we cannot apply the same formulas for other elements by using the equations given by bohr.if there are complications what are they?

 

[lalbatros]

Main complication is that the Bohr model is rather far from reality even if it illustrates very simply the fundamentals of quantum mechanics.

However, for most of atomic physics the full quantum mechanics is needed.

For example, orbitals describe stationary waves of electrons in the atom in a very precise way. This description is much more elaborated than the Bohr model. Without, you could never explain chemistry.

As another example you should think to the Pauli exclusion principle: no more than two electron can manage to eccupy the same orbital if they have oppiste spins. Again this is not included in the Bohr model.

 

[sir-pinski]

The Niels Bohr model was a groundbreaking theory in understanding the structure of atoms, particularly the orbits of electrons within them. However, it is important to note that the model was developed specifically for hydrogen atoms and cannot be applied to other elements in the same way. This is because each element has a unique atomic structure, with different numbers of protons, neutrons, and electrons.

The Bohr model was based on the concept of quantized energy levels, where electrons occupy specific orbits around the nucleus at fixed distances. These orbits are determined by the balance between the attractive force of the positively charged nucleus and the repulsive force of the negatively charged electrons. For hydrogen, the equation for calculating the radius and energy of these orbits is relatively simple, as it only involves the mass and charge of the electron and the nucleus.

However, for other elements, the equations become much more complex due to the presence of multiple electrons and the interactions between them. The electrons in an atom do not move independently, but rather influence each other's behavior. This means that the energy levels and orbital shapes are not as well-defined as in the Bohr model.

Moreover, the Bohr model was developed in the early 20th century and has since been replaced by more accurate models such as the quantum mechanical model. This model takes into account the wave-like nature of electrons and provides a more detailed understanding of atomic structure.

In summary, while the Bohr model was a significant step in understanding the behavior of electrons in atoms, it is limited to hydrogen and cannot be applied to other elements with the same simplicity. The complexities of atomic structure and the advancements in scientific understanding have led to the development of more accurate models.