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What is the wavelength of light emitted when the electron in hydrogen atom undergoes transition from an energy level with N to an energy level with n 2?
Wiki User
∙ 9y ago
This can be calculated using the following procedure: 1 / w = (Rh / hc)(1/nf^2 - 1/ni^2); 1 / w = ((2.18 x 10^-18) / (6.63 x 10^-14)(3.00 x 10^8))(1/(1^2) - 1/(6^2)); 1 / w = (1.10 x 10^7)(0.972); 1 / w = 1.07 x 10^7; w = 9.35 x 10^-8 m = 93.5 nm. The emission by the hydrogen atom is of wavelength 93.5 nm.
Wiki User
∙ 9y ago
Wiki User
∙ 11y ago2.48 x 10^15 Hz. The energy of these photons is 1.64 x 10^-18 J (-5.4 x 10^-19 J - -2.18x 10^-18 J). Using equation 8.5, the frequency is found to be 2.48 x 10^15 Hz by dividing the photon energy by Planck's Constant (1.64 x 10^-18 J / 6.63 x 10^-34 J*s). They are ultraviolet.
Wiki User
∙ 14y agoA bit dicy for me since it has been a long time, but I have the formula sheet. Attend.
This formula to find Hertz: ( v = Hertz )
v = (3.29 X 10^15 s^-1) * Z^2 * (1/n final - 1/n initial )
Z = 1 for hydrogen
v = ( 3.29 X 10^15 ) * 1^2 * (1/2^2 - 1/4^2 )
= 6.169 X 10^14 Hertz
Now to convert Hertz into wavelength use this; Wavelength = Speed of light/Hertz
2.998 X 10^8/6.169 X 10^14 = 4.86 X 10^-7 meters (speed of light has m/s units while Hertz has s units, so meters come out )
to get nanometers; 4.86 X 10^-7 times 10^9 = 486 nanometers of wavelength.
( look up that color of visable light )
Wiki User
∙ 13y agoBeen awhile, so long answer.
a) Frequency (v) = (3.29 X 10^15 s^-1)(Z^2)(1/Nf^2-1/Ni^2)
Z = 1 for H
Hertz = (3.29 X 10^15)(1^2)(1/2^2-1/3^2)
= 4.569 X 10^14 Hertz
Energy = Planck's constant * frequency in hertz
= (6.626 X 10^-34 J*s)(4.569 X 10^14 Hertz)
= 3.027 X 10^-19 Joules
b) Energy = Planck's constant * speed of light/wavelength in meters
3.027 X 10^-19 J = (6.626 X 10^-34)(2.998 X 10^8 m/s)/wavelength
= 6.563 X 10^-7 meters
which is 656.3 nanometers
Wiki User
∙ 9y agoYou need to look up the Rydberg equation, which can be used to solve problems of this form.
The typesetting functionality here isn't really good enough to show the equation, so I've added a link in the Related Links section to the Wikipedia article on it.
Add your answer:
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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 end value of "n" is 2.
Quantum-mechanical model for the hydrogen atom which of the following transitions would produce light with the longer wavelength 3p2s or 4p3p?
A transition from 4p to 3p will produce light with a longer wavelength. This is because this transition is a smaller energy exchange than that of 3p to 2s (longer wavelength = less energy.)
To which series would the emitted light belong if an electron in a hydrogen atom underwent a transition from level n 5 to level n 1?
Lyman
Hydrogen sometimes is ________________ an electron and sometimes it has an _____________ electron.?
dd
What is the wavelength of the hydrogen atom in the 2nd line of the Balmer series?
With reference to the wikipedia article on this topic: The Balmer series predicts visible light wavelengths with high accuracy. The limiting transition wavelength predicted by the formula, inf -> 2, would be 364.6 nm.
What color is the wavelength of light in the balmer series that results from the transition of an electron from n4 to n2?
The n4-n2 transition of hydrogen is in the cyan, with wavelength of 486.1 nm. blue = als
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 end value of "n" is 2.
Which particle is emitted from a hydrogen-3 nucleus when it undergoes radioactive decay?
beta, aka an electron.
Quantum-mechanical model for the hydrogen atom which of the following transitions would produce light with the longer wavelength 3p2s or 4p3p?
A transition from 4p to 3p will produce light with a longer wavelength. This is because this transition is a smaller energy exchange than that of 3p to 2s (longer wavelength = less energy.)
Can you make the hydrogen a metal?
Yes. Although hydrogen is a non-metal, there is metallic hydrogen. It is formed when hydrogen is sufficiently compressed and undergoes a phase change; it is an example of degenerate matter. Solid metallic hydrogen consists of a crystal lattice of protons with a spacing which is significantly smaller than a Bohr radius. Indeed, the spacing is more comparable with an electron wavelength. The electrons are unbound and behave like the conduction electrons in a metal. As is the dihydrogen molecule H2, metallic hydrogen is an allotrope. In liquid metallic hydrogen, protons do not have lattice ordering.
What is the wavelength of a photon that will induce a transition from the ground state to the n equals 4 state in hydrogen?
That is the "gamma" line of the Lyman series: 94.97 nanometers.
What do Each of the colored lines in hydrogen's emission spectrum corresponds with?
transition of an electron from a higher energy level to a lower energy level.
To which series would the emitted light belong if an electron in a hydrogen atom underwent a transition from level n 5 to level n 1?
Lyman
Is hydrogen a transition metal?
No, hydrogen is a gas.
Hydrogen sometimes is ________________ an electron and sometimes it has an _____________ electron.?
dd
What are the Electron Configuration of hydrogen?
Hydrogen electron configuration will be 1s1.
What is the difference between hydrogen and an electron?
Hydrogen is an element, the electron is a subatomic particle.
