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Why does excited hydrogen atoms always produce the same line emission spectrum?
Excited hydrogen atoms produce the same line emission spectrum because they have specific energy levels associated with their electron transitions. When an electron falls from a higher energy level to a lower one, it emits a photon with a specific energy, corresponding to a specific wavelength of light. This results in the characteristic line emission spectrum of hydrogen.
Bohr used the emission spectrum of hydrogen to support his idea that?
Each energy level corresponds to an exact amount of energy needed by the electron to orbit the nucleus. Transitions from a higher energy level to a lower energy level correspond to the difference in the energy needed for an electron to occupy those two energy levels. This difference creates the emission spectrum.
Which model of an atom explains why excited hydrogen gas gives off certain colors of light?
The Bohr model of the atom explains why excited hydrogen gas gives off certain colors of light. When an electron transitions from a higher energy level to a lower one, it emits light with specific wavelengths corresponding to the difference in energy levels, producing the characteristic spectral lines of hydrogen such as the Balmer series.
Why does hydrogen atom contain many lines?
When the energy is supplied to the atom of hydrogen it will be exited then its single electron will jump from its ground state to some higher energy level. Now,when it de exites from higher level to ground level by several jumps pectral lines of different wavelengths are emitted. That is why the spectrum of hydrogen contains many lines.
What happens to excess energy when the electron jumps from a higher energy orbit to a lower energy orbit in the hydrogen atom?
The electron emits a photon of light which we can see in a spectrograph as color. Four colors are normally seen in a hydrogen atom subjected to energy.
Absorption of what type of electromagnetic radiation results in electronic transitions?
Absorption of ultraviolet (UV) or visible light results in electronic transitions in atoms or molecules. This energy causes electrons to move to higher energy levels, leading to the absorption of specific wavelengths of light by the substance.
The lines at the ultraviolet end of the hydrogen spectrum are known as the lyman series wich electron transitions within an atom are responsible for these lines?
The series of lines in an emission spectrum caused by electrons falling from energy level 2 or higher (n=2 or more) back down to energy level 1 (n=1) is called the Lyman series. These emission lines are in the ultra-violet region of the spectrum.
Is visible light higher than ultavoilet waves?
If you are talking about energy then no, UV has higher energy than visible light.
Why are the hydrogen Balmer lines strong in the spectra of medium-temperature stars and weak in the spectra of hot and cool stars?
They are like this due to the fact that most hydrogen atoms are ionized which makes a weaker balmer line. The strength of the Balmer line is sensitive to temperature so that's why it occurs more in the middle. The hot end of the hydrogen is low Balmer line due to them being in the ground state. Hope that's answers it =] -CRS
Is Balmer series only present in hydrogen atom?
No, the Balmer series is observed in hydrogen-like atoms, which have one electron orbiting a nucleus. It consists of the spectral lines produced when the electron transitions from higher energy levels to the second energy level. Other atoms with similar electron configurations can also exhibit Balmer-like series in their spectra.
Compare the frequency and energy of infrared waves to the frequency energy of the visible light?
Visible light has a higher frequency, a higher energy per photon, and a smaller wavelength, compared to infrared.
What has more energy a visible light or infrared light?
Visible light. It has a higher frequency so more energy.
Why were transitions which ended at energy level 1 not studied by the unaided eye?
Transitions that end at energy level 1 are in the UV or X-ray range, which is outside the visible spectrum detectable by the human eye. Our eyes can only perceive electromagnetic radiation within a certain range of wavelengths, typically from about 400 to 700 nanometers, corresponding to the colors of light in the visible spectrum. UV and X-ray wavelengths are much shorter and higher in energy, making them invisible to the naked eye.
Is ultraviolet radiation a higher or lower energy radiation than visible light?
Ultraviolet radiation is of higher energy than visible light. Ultra-violet suggests that it is above violet in the spectrum, and the colour violet is the uppermost region of visible light.
What is the starting energy in the sun is?
The nuclear energy available in the hydrogen. This is a kind of potential energy. Hydrogen has a higher energy level than helium.
What happens when an electron in a hydrogen atom moves from higher energy level to the lowest level?
When an electron in a hydrogen atom moves from a higher energy level to the lowest level, it emits a photon of energy equal to the difference in energy between the two levels. This photon is released as light, and the electron transitions to the ground state. This process is known as an electron transition or de-excitation.
Gamma radiation is of lower energy than visible radiation?
No. Gamma radiation is of higher energy than visible (light) radiation.
