Question

Calculate the energy of the emitted photon as well as the wavelength and frequency of electromagnetic radiation emitted from the hydrogen atom when the electron undergoes the transition from n = 5 to n = 1. In what region of the spectrum does this line occur?

Answer #1

RH = redberg's constant = 1.0973 x 10^7 m-1

1 / = R_{H}
[1 / n1^2 - 1 / n2^2]

= 1.0973 x 10^7 [1 / 1 - 1 /5^2]

= 1.053 x 10^7 m-1

E = h C /

= 6.625 x 10^-34 x 3 x 10^8 x 1.053 x 10^7

= 2.09 x 10^-18 J

**energy of the emitted photon = 2.09 x 10^-18
J**

**wavelength = 9.50 x 10^-8
m = 95 nm**

**frequency = C / = 3 x 10^8 /
9.50 x 10^-8 = 3.16 x 10^15 Hz**

Calculate the shortest wavelength of the electromagnetic
radiation emitted by the hydrogen atom in undergoing a transition
from the n = 6 level

Q1)
Calculate the energy of an electron in the n =
2 level of a hydrogen atom.
Energy = _______Joules
Q2)
What would be the wavelength of radiation emitted from a
hydrogen atom when an electron moves from the n =
2 to n = 1energy level?
In what region of the spectrum does this radiation lie?
Wavelength = ________nm
Region = _________(ultraviolet or visible or infrared)

a. what is the energy of the emitted photon if an electron in
the hydrogen atom makes a transition from the n=7 state to the n=2
state?
b. Now, Imagine there is a photon with the same wavelength. What
is the speed of this photon?

Light is emitted from a hydrogen atom as an electron in the atom
jump from the n=9 orbit to the n=3 orbit.
What is the energy of the emitted photon in eV?
(b) What are the frequency and wavelength of the photon?
(c) In which frequency range (UV, visible, IR) is the emitted
electromagnetic radiation? Justify your answer.

4. [15] Light is emitted from a hydrogen atom as an electron in
the atom jump from the n=9 orbit
to the n=3 orbit.
(a) [7] What is the energy of the emitted photon in eV?
(b) [4] What are the frequency and wavelength of the photon?
(c) [4] In which frequency range (UV, visible, IR) is the
emitted electromagnetic radiation?
Justify your answer.

For a hydrogen atom, calculate the wavelength of an emitted
photon in the Lyman series that results from the transition n = 3
to n = 1. The Rydberg constant is 2.18 x 10^-18 J.

3. What is the wavelength (in nm) and frequency of light that is
emitted when an electron in a hydrogen atom drops from the n = 5 to
the n = 3 energy level

Determine the frequency (Hz) and wavelength (nm) of light
emitted when an electron in a Hydrogen atom makes a transition from
an orbital in n=6 to an orbital in n=5

Calculate the wavelength (in nm) of a photon emitted during a
transition corresponding to the first line in the Balmer series (nf
= 2) of the hydrogen emission spectrum.

) Describe the Bohr theory of the hydrogen atom and how it
explains the line spectrum of hydrogen. What is the
energy and wavelength of the
photon of energy that was emitted by hydrogen if one of its
electrons dropped from the n=6 state to the n=2 state. In what
region of the electromagnetic spectrum does this wavelength fall?
Which color line is this in the line spectra of hydrogen?

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