Question

Part B

Using equation E=(hcRH)(1n2)=(−2.18×10−18J)(1n2), calculate the energy of an electron in the hydrogen atom when n= 5.

Part C

Calculate the wavelength of the radiation released when an electron moves from n= 5 to n=2.

Answer #1

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)

1. The energy of the electron in the lowest level of the
hydrogen atom (n=1) is -2.179×10-18 J. What is the energy of the
electron in level n=5? -8.716×10-20 J 2.The electron in a hydrogen
atom moves from level n=6 to level n=4.
a) Is a photon emitted or absorbed?
b) What is the wavelength of the photon?

Calculate the wavelength, in nm, of the photon that is released
from a hydrogen atom when the atom's electron moves from n=8 to
n=2. Please show all work.

Using the Rydberg formula, calculate the initial energy level
when an electron in a hydrogen atom transitions into n=2 and emits
a photon at 410.1 nm. Note: the Rydberg constant = 1.097 x
107 m-1

6.
a) For a hydrogen atom, if the emission energy associated when
the electron starts at n = 8 is 2.65 x 10-20 J, at what
energy level does the photon finish at?
b) What type of electromagnetic radiation is associated with
this change

A photon is incident on a hydrogen atom. The photon
moves the electron from an n = 5 energy level to an n = 10 energy
level.
A: Is this an absorption or emission process? Choose
one.
B: What is the wavelength, in nanometers, of the
incident photon?

Determine the wavelength of the light absorbed when an electron
in a hydrogen atom makes a transition from an orbital in which
n = 2 to an orbital in which n =
5. Determine the wavelength 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.

9) a. Explain what is happening inside an atom when it emits
light.
9) b. Explain what is happening inside an atom when it absorbs
light.
10) An excited hydrogen atom emits light with a frequency of
1.141 x 1014 Hz for its electron to reach the n=4 energy level. In
which energy level did the electron begin? Big hint: what is the
sign (neg or pos) of the electron’s energy change? (Remember, it
says “emits”) Use this sign when...

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.

A photon is emitted from a hydrogen atom when an electron goes
from the n = 6 to the n = 2 state. What kind of electromagnetic
radiation is this? Select one:
a. Visible Light
b. Ultraviolet Light
c. Infrared Radiation
d. X-Ray Radiation
e. Microwave Radiation

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