How Electron in hydrogen atom is put into higher energy state
To generate hydrogen spectral lines, electrons are excited to higher energy states within hydrogen atoms. This process is typically achieved by providing energy to the hydrogen atoms in one of the following ways:
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Electromagnetic Radiation (Light): When a hydrogen atom is exposed to electromagnetic radiation, such as visible or ultraviolet light, the energy from the radiation can be absorbed by an electron, causing it to move to a higher energy level. This process is known as excitation. The electron jumps from its ground state (lowest energy level) to an excited state (higher energy level). The specific wavelength or energy of the incoming light must match the energy difference between the two energy levels for the excitation to occur.
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Electric Discharge: In laboratory settings, hydrogen gas can be excited by passing an electric current through it. The electrons gain energy from the electric field and move to higher energy levels. When they return to lower energy levels, they emit energy in the form of light. The emitted light consists of discrete spectral lines, each corresponding to a specific transition between energy levels.
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Collision with Other Particles: In some natural processes, such as in stars, high-temperature plasmas, or particle collisions, hydrogen atoms may collide with other particles, transferring energy to the electrons and exciting them to higher energy levels. Subsequent de-excitations of the electrons result in the emission of spectral lines.
Once the electrons have been excited to higher energy states, they are unstable in those states and tend to return to lower energy levels. When they do so, they release the excess energy in the form of electromagnetic radiation (light). This emitted light consists of spectral lines that are unique to hydrogen and are characteristic of the transitions between the different energy levels of the hydrogen atom.
The energy of the emitted light corresponds to the energy difference between the excited state and the lower energy state to which the electron returns. The specific wavelengths of the spectral lines in the hydrogen spectrum are a result of these energy differences and are often associated with the Balmer, Lyman, and Paschen series, each corresponding to different series of transitions within the hydrogen atom.