Question

1. What is the problem with Bohr's model of the atom?

2. How did Schrödinger resolve this problem?

Answer 1

Bohr's model of the atom had several problems, such as not being able to explain electron orbits and emission spectra for multi-electron atoms. Schrödinger resolved these problems by developing the wave equation, which describes the behavior of electrons in a hydrogen atom and introduces the concept of electron orbitals.

Step-by-step explanation:

Bohr's model of the atom had several problems:

1. It couldn't explain why electrons orbit at fixed distances and not in between.
2. It couldn't predict the emission spectrum for atoms with more than one electron.
3. It assumed simple circular paths for electron orbits, which doesn't match with the cloud-like nature of electron probabilities in quantum mechanics.

Schrödinger's resolved these problems by developing a complex mathematical equation called the wave equation. This equation accurately describes the behavior of the electron in a hydrogen atom and takes into account the wave-particle duality of electrons. It also quantizes electron energies and gives rise to the concept of electron orbitals, which are probability distributions of finding an electron in a specific region around the nucleus.

Answer 2

Below is the explanation

Step-by-step explanation:

Requirement 1

The main problem with Bohr's model is that it works very well for those atoms which have only one electron, like H or He+, but it didn't work for multi-electron atoms. Bohr was able to divine the difference in energy between each energy level, allowing us to intuit the powers of each line in the emission spectrum of hydrogen, and understand why electron energies are quantized.

Requirement 2

The application of Schrodinger's equation to atoms can explain the nature of electrons in atoms more accurately. Solving the Schrödinger equation gives us Ψ and Ψ2. With these, we can get the quantum number and the shapes and orientations of orbitals that characterize electrons in an atom or molecule.

There are two types of Schrodinger's equation: a time-dependent Schrödinger equation and a time-independent Schrödinger equation.