Explain, with the help of an appropriate labelled sketch diagram, how a hydrogen atom, which has only one electron, has so many spectral lines.
The diagram of the energy levels follows:
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An electron may reside in any of the energy levels. When it falls to a lower level, light is emitted with an energy that is the difference between the two energy levels. There are many energy levels and many combinations from which the electron can fall "from/to" so there are many different wavelengths emitted by the single electrons.
Atoms and glucose are being used for energized...
To explain how a hydrogen atom, which has only one electron, can produce so many spectral lines, we need to understand the concept of energy levels and electron transitions.
In a hydrogen atom, the electron is located in specific energy levels surrounding the nucleus. These energy levels are represented by the diagram you provided, with the nucleus at the center and the energy levels arranged in increasing energy from the inside to the outside.
When the electron is in its ground state or the lowest energy level, it is in the most stable configuration. However, the electron can absorb energy and move to a higher energy level, known as an excited state. This absorption of energy can happen due to external factors such as heat or light.
Once the electron is in an excited state, it is no longer stable and tends to return to its ground state, releasing the excess energy it gained. This release of energy occurs in the form of electromagnetic radiation or light. The energy of this emitted light is directly related to the energy difference between the two energy levels involved in the transition.
The diagram you provided shows the various energy levels, and each transition between these levels produces a specific wavelength or color of light. The more energy levels an atom has, the greater the number of possible transitions, and hence a greater number of spectral lines.
In the case of a hydrogen atom, which has a single electron, there are many available energy levels for the electron to transition between. This results in a large number of spectral lines appearing in the hydrogen emission or absorption spectrum.
By studying the wavelengths of these spectral lines, scientists can gain insights into the energy levels and electronic structure of atoms, which in turn helps in understanding various aspects of atomic physics and chemistry.