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What is the wavelength of the energy emitted when a hydrogen electron drops from the n equals 3 to n equals 2 electronic energy level?
That's the 'Lyman alpha' line, the least energetic transition to the n=1 level.
In order to calculate it, I'd need to look up the energy of the electron in the n=1 and
n=2 levels, as well as Planck's Konstant, or else the Rydberg Constant. And even then
I would have a difficult time of it, since I spilled an entire glass of Ginger Ale on my
calculator a couple of hours ago and the display is still blank.
So right now, it's a lot easier to look it up.
It's 122 nanometers.
What else can I help you with?
Why is a shorter wavelength of light emitted when an electron falls from n4 to n1 than when an electron falls from n2 to n1?
When an electron falls from n4 to n1, it releases more energy because it is transitioning between high energy states. This higher energy transition corresponds to a shorter wavelength of light being emitted, according to the energy of the photon being inversely proportional to its wavelength. In contrast, when an electron falls from n2 to n1, the energy released is less, resulting in a longer wavelength of light emitted.
What is the emission wavelength equation used to calculate the specific wavelength of light emitted by a substance?
The emission wavelength equation used to calculate the specific wavelength of light emitted by a substance is c / , where represents the wavelength, c is the speed of light in a vacuum, and is the frequency of the light emitted.
When an electron in atom changes energy states a photon is emitted If the photon has a wavelength of 550 nm how did the energy of the electron change?
The energy of the electron decreased as it moved to a lower energy state, emitting a photon with a wavelength of 550 nm. This decrease in energy corresponds to the difference in energy levels between the initial and final states of the electron transition. The energy of the photon is inversely proportional to its wavelength, so a longer wavelength photon corresponds to lower energy.
Determine the end value of n in a hydrogen atom transition if the electron starts in n equals 4 and the atom emits a photon of light with a wavelength of 486nm?
The wavelength of light emitted during a transition can be related to the energy levels involved using the Rydberg formula. Rearranging the formula for the final energy level, we find that the end value of n is 2 in this case. This means the electron transitions from the n=4 to the n=2 energy level in the hydrogen atom.
Is energy emitted or absorbed when an electron moves from an excited state to a ground state?
Emitted, and the precise amount of energy that is emitted will depend on what kind of atom, and moving from which excited state. That's how spectrographs can determine what element is present.
How do you calculate wavelength using the Bohr model for Hydrogen Atom?
You can calculate the wavelength of light emitted from a hydrogen atom using the Rydberg formula: 1/λ = R(1/n₁² - 1/n₂²), where λ is the wavelength, R is the Rydberg constant, and n₁ and n₂ are the initial and final energy levels of the electron.
Why is a shorter wavelength of light emitted when an electron falls from n4 to n1 than when an electron falls from n2 to n1?
When an electron falls from n4 to n1, it releases more energy because it is transitioning between high energy states. This higher energy transition corresponds to a shorter wavelength of light being emitted, according to the energy of the photon being inversely proportional to its wavelength. In contrast, when an electron falls from n2 to n1, the energy released is less, resulting in a longer wavelength of light emitted.
Why is a shorter wavelength of light emitted when an electron falls from n equals 4 to n equals 1 than when an electron falls from n equals 2 to n equals 1?
Shorter wavelength = more energy. The farther the electron falls, the more energy that will be emitted.
What is the energy in cm-1 of the photon emitted during the transition of an electron in a hydrogen atom from the n3 to n2 energy level?
The energy of the photon emitted during the transition of an electron in a hydrogen atom from the n3 to n2 energy level is approximately 364.5 cm-1.
What is the relationship between the light emitted by an atom in the energies of the electrons in the atom?
The more energy levels the electron jumps the more energy the emitted light will have. The more energy you have the shorter wavelength there is.
Which transition occurs when light wavelength of 486 nm is emitted by a hydrogen atom?
The transition from energy level 4 to energy level 2 occurs when a hydrogen atom emits light of 486 nm wavelength. This transition represents the movement of an electron from a higher energy level (n=4) to a lower energy level (n=2), releasing energy in the form of light.
What is the emission wavelength equation used to calculate the specific wavelength of light emitted by a substance?
The emission wavelength equation used to calculate the specific wavelength of light emitted by a substance is c / , where represents the wavelength, c is the speed of light in a vacuum, and is the frequency of the light emitted.
When an electron in atom changes energy states a photon is emitted If the photon has a wavelength of 550 nm how did the energy of the electron change?
The energy of the electron decreased as it moved to a lower energy state, emitting a photon with a wavelength of 550 nm. This decrease in energy corresponds to the difference in energy levels between the initial and final states of the electron transition. The energy of the photon is inversely proportional to its wavelength, so a longer wavelength photon corresponds to lower energy.
What is the wavelength of the photon emitted when a hydrogen atom goes from the second energy level to the first energy level?
The wavelength of the photon emitted can be calculated using the Rydberg formula: 1/wavelength = R(1/n1^2 - 1/n2^2), where R is the Rydberg constant, n1 is the initial energy level (2 in this case), and n2 is the final energy level (1 in this case). Plugging in the values gives the wavelength of the photon emitted.
What's the wavelength of the light emitted by the laser?
The wavelength of the light emitted by the laser is typically in the range of 400 to 700 nanometers.
Determine the end value of n in a hydrogen atom transition if the electron starts in n equals 4 and the atom emits a photon of light with a wavelength of 486nm?
The wavelength of light emitted during a transition can be related to the energy levels involved using the Rydberg formula. Rearranging the formula for the final energy level, we find that the end value of n is 2 in this case. This means the electron transitions from the n=4 to the n=2 energy level in the hydrogen atom.
Is energy emitted or absorbed when an electron moves from an excited state to a ground state?
Emitted, and the precise amount of energy that is emitted will depend on what kind of atom, and moving from which excited state. That's how spectrographs can determine what element is present.
