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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.
Which gas has electronic transitions involving the largest energy change?
The gas with electronic transitions involving the largest energy change is typically hydrogen. In hydrogen, transitions between energy levels correspond to significant differences in energy due to its simple atomic structure. The energy changes are most pronounced in the ultraviolet region of the spectrum, particularly for transitions from the ground state to higher excited states. Other gases may exhibit electronic transitions as well, but hydrogen's transitions involve the largest energy changes relative to its electronic structure.
Why is the flame of beryllium colourless?
The flame of beryllium is colorless because beryllium does not emit visible light when it is heated. Unlike other metallic elements that can produce characteristic flame colors due to electronic transitions, beryllium’s electronic structure does not allow for such transitions in the visible spectrum. Instead, any energy absorbed may result in excitation of electrons to higher energy states, but these transitions involve higher energy photons, which are outside the visible range. As a result, beryllium appears to burn without producing a colorful flame.
Which one of the following series of lines in the hydrogen spectrum arises from transitions down to n2?
The series of lines in the hydrogen spectrum that arises from transitions down to n=2 is known as the Balmer series. This series includes visible light emissions when electrons fall from higher energy levels (n≥3) to the n=2 level. The Balmer lines are characterized by wavelengths that fall within the visible range, producing colors such as red, green, and blue in the spectrum.
What is the common feature among transitions where the resulting radiation lies within the visible light range of the electromagnetic spectrum?
The common feature among transitions that result in radiation within the visible light range of the electromagnetic spectrum is that they typically involve electronic transitions between energy levels in atoms or molecules. Specifically, these transitions occur when electrons move from a higher energy level to a lower one, emitting photons with wavelengths between approximately 400 nm (violet) and 700 nm (red). The energy difference between these levels corresponds to the energy of visible light photons, making it possible for the emitted radiation to fall within this range.
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.
Why it is not possible to observe the n7 to n2 transition in the Balmer Series?
The Balmer Series describes the transitions of electrons in a hydrogen atom from higher energy levels (n ≥ 3) down to the n = 2 level, resulting in visible light emissions. The n = 7 to n = 2 transition falls within the ultraviolet range, which is not part of the visible spectrum typically associated with the Balmer Series. Consequently, while such transitions can occur, they cannot be observed as part of the Balmer Series since they emit wavelengths that are outside the visible range. Thus, the n = 7 to n = 2 transition is not considered part of the series.
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.
