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A sample of H-atoms having electrons in the ground state is exposed to high energy rays of quantum energy 13.3875 eV. The H-atoms absorb the energy and get excited. When the electron drops from excited state to the ground state, how many lines are seen in the emission spectrum of hydrogen?
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A sample of H-atoms having electrons in the ground state is exposed to...
Number of Lines in Emission Spectrum of Hydrogen
- When H-atoms absorb high-energy rays, their electrons get excited to higher energy levels.
- The excited electrons eventually drop back to the ground state, emitting energy in the form of light.
- During the de-excitation process, the electron transitions from higher energy levels to the ground state.
- Each transition corresponds to the emission of a specific wavelength of light.
- The emission spectrum of hydrogen consists of multiple spectral lines representing these transitions.
- The number of lines in the emission spectrum is determined by the number of possible transitions between energy levels.
- The energy levels of hydrogen are quantized, with the energy difference between levels corresponding to specific wavelengths.
- The formula for calculating the energy of a photon is E = hc / λ, where E is the energy, h is Planck's constant, c is the speed of light, and λ is the wavelength.
- By considering the energy of the absorbed photons (13.3875 eV) and the energy differences between energy levels in hydrogen, the number of lines in the emission spectrum can be determined.
- In the case of hydrogen atoms excited by 13.3875 eV energy rays, the emission spectrum will consist of a specific number of spectral lines corresponding to the transitions of electrons from higher energy levels back to the ground state.
- When H-atoms absorb high-energy rays, their electrons get excited to higher energy levels.
- The excited electrons eventually drop back to the ground state, emitting energy in the form of light.
- During the de-excitation process, the electron transitions from higher energy levels to the ground state.
- Each transition corresponds to the emission of a specific wavelength of light.
- The emission spectrum of hydrogen consists of multiple spectral lines representing these transitions.
- The number of lines in the emission spectrum is determined by the number of possible transitions between energy levels.
- The energy levels of hydrogen are quantized, with the energy difference between levels corresponding to specific wavelengths.
- The formula for calculating the energy of a photon is E = hc / λ, where E is the energy, h is Planck's constant, c is the speed of light, and λ is the wavelength.
- By considering the energy of the absorbed photons (13.3875 eV) and the energy differences between energy levels in hydrogen, the number of lines in the emission spectrum can be determined.
- In the case of hydrogen atoms excited by 13.3875 eV energy rays, the emission spectrum will consist of a specific number of spectral lines corresponding to the transitions of electrons from higher energy levels back to the ground state.
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A sample of H-atoms having electrons in the ground state is exposed to high energy rays of quantum energy 13.3875 eV. The H-atoms absorb the energy and get excited. When the electron drops from excited state to the ground state, how many lines are seen in the emission spectrum of hydrogen?
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A sample of H-atoms having electrons in the ground state is exposed to high energy rays of quantum energy 13.3875 eV. The H-atoms absorb the energy and get excited. When the electron drops from excited state to the ground state, how many lines are seen in the emission spectrum of hydrogen? for UPSC 2024 is part of UPSC preparation. The Question and answers have been prepared according to the UPSC exam syllabus. Information about A sample of H-atoms having electrons in the ground state is exposed to high energy rays of quantum energy 13.3875 eV. The H-atoms absorb the energy and get excited. When the electron drops from excited state to the ground state, how many lines are seen in the emission spectrum of hydrogen? covers all topics & solutions for UPSC 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A sample of H-atoms having electrons in the ground state is exposed to high energy rays of quantum energy 13.3875 eV. The H-atoms absorb the energy and get excited. When the electron drops from excited state to the ground state, how many lines are seen in the emission spectrum of hydrogen?.
A sample of H-atoms having electrons in the ground state is exposed to high energy rays of quantum energy 13.3875 eV. The H-atoms absorb the energy and get excited. When the electron drops from excited state to the ground state, how many lines are seen in the emission spectrum of hydrogen? for UPSC 2024 is part of UPSC preparation. The Question and answers have been prepared according to the UPSC exam syllabus. Information about A sample of H-atoms having electrons in the ground state is exposed to high energy rays of quantum energy 13.3875 eV. The H-atoms absorb the energy and get excited. When the electron drops from excited state to the ground state, how many lines are seen in the emission spectrum of hydrogen? covers all topics & solutions for UPSC 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A sample of H-atoms having electrons in the ground state is exposed to high energy rays of quantum energy 13.3875 eV. The H-atoms absorb the energy and get excited. When the electron drops from excited state to the ground state, how many lines are seen in the emission spectrum of hydrogen?.
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