The term "quantised energy levels" refers to the concept in quantum mechanics where the energy of an electron in an atom is not continuous, but discrete. This means that the energy an electron can have is not a range, but specific, fixed values.

This concept is applied to the hydrogen atom (H atom) in the following way:

1. The hydrogen atom consists of a single proton and a single electron. The electron moves around the proton in specific orbits.

2. According to the Bohr model of the atom, these orbits correspond to certain energy levels. The electron can exist in any of these orbits, but nowhere in between.

3. When the electron absorbs a specific amount of energy (in the form of a photon), it can 'jump' from a lower energy level to a higher one. This is called excitation.

4. Conversely, when the electron falls from a higher energy level to a lower one, it emits a photon with a specific energy. This is called de-excitation.

5. The energy of the photon absorbed or emitted is exactly equal to the difference in energy between the two levels. This is why the energy levels are said to be 'quantised' - they can only take on specific values, and the energy changes in discrete 'jumps', not continuously.

6. The specific energy levels that the electron can occupy in a hydrogen atom are calculated using the Rydberg formula. This formula gives the wavelengths of the spectral lines of the hydrogen atom, which correspond to the energy differences between the levels.

In summary, the term 'quantised energy levels' in the context of the hydrogen atom refers to the specific, discrete energy levels that the electron in the atom can occupy, and the discrete 'jumps' in energy that occur when the electron absorbs or emits energy.

Question

The term "quantised energy levels" refers to the concept in quantum mechanics where the energy of an electron in an atom is not continuous, but discrete. This means that the energy an electron can have is not a range, but specific, fixed values.

This concept is applied to the hydrogen atom (H atom) in the following way:

1. The hydrogen atom consists of a single proton and a single electron. The electron moves around the proton in specific orbits.

2. According to the Bohr model of the atom, these orbits correspond to certain energy levels. The electron can exist in any of these orbits, but nowhere in between.

3. When the electron absorbs a specific amount of energy (in the form of a photon), it can 'jump' from a lower energy level to a higher one. This is called excitation.

4. Conversely, when the electron falls from a higher energy level to a lower one, it emits a photon with a specific energy. This is called de-excitation.

5. The energy of the photon absorbed or emitted is exactly equal to the difference in energy between the two levels. This is why the energy levels are said to be 'quantised' - they can only take on specific values, and the energy changes in discrete 'jumps', not continuously.

6. The specific energy levels that the electron can occupy in a hydrogen atom are calculated using the Rydberg formula. This formula gives the wavelengths of the spectral lines of the hydrogen atom, which correspond to the energy differences between the levels.

In summary, the term 'quantised energy levels' in the context of the hydrogen atom refers to the specific, discrete energy levels that the electron in the atom can occupy, and the discrete 'jumps' in energy that occur when the electron absorbs or emits energy.

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