Question

How does the Bohr’s model of atoms differ from the quantum mechanical model?

Answer 1

Hint: We need to understand the Bohr’s atomic model and the quantum mechanical model of atoms to distinguish between them. The Bohr’s model is the closest model which describes the atomic structure in the classical mechanical approach.

Complete answer:
We know that there were numerous models of atoms which tried to explain the existence of the neutral atoms in material using the classical mechanical approach. Bohr's model is the one which is the closest model which could explain the atomic existence in the most acceptable manner before quantum mechanical theory.
The Bohr’s model has the following conditions –
1.The atoms consist of discrete energy states in which the electrons orbit around the nuclei. These are stationary states in which the electrons do not radiate energy.
2.When the electrons undergo transition from one energy level to the other, a specific radiation of a discrete frequency is produced, which is given as –
$$f={\displaystyle \frac{E_1-E_2}{h}}$$
3. The angular momentum of the electron in each of the state is quantised must be an integral multiple of $${\displaystyle \frac{h}{2\pi }}$$ given by –
$$mvr={\displaystyle \frac{nh}{2\pi }}$$
The Bohr Model gives the atomic model in a one-dimensional view, whereas the Schrodinger’s quantum model represents the probability of occurrence of the electrons in a three-dimensional space. This makes the solution of the Schrodinger’s equation nearly impossible for atoms of a larger number of electrons. The correct solution for the Schrodinger equation is found in a standard and simple way only hydrogen atom.
This is the required solution.

Note:
The Bohr model of the atom gave the idea about the discrete energy levels which was an important conclusion that is extended even into the Schrodinger solution. All the preceding hypotheses gave enough information to move forward in making an apt model.