Question

A certain hydrogen-like atom emits light with a frequency of 2.2x10^16 Hz associated with the n=2 to n=1 transition. What frequency light will be emitted for the n=3 to n=2 transition for this atom?

Answer #1

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

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.

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.

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.

Determine the end (final) value of n in a hydrogen atom
transition, if the electron starts in n = 2 and the atom absorbs a
photon of light with a frequency of 4.57 × 10 14 Hz. (This question
has already been posted, however, the answers for it dont match the
options).

An electron in a hydrogen atom undergoes a transition from the n
= 6 level to some lower energy level. In doing so, energy is
released in the form of light. a) Calculate the frequency in s-1
(to 3 significant figures) of a photon of light associated with the
highest frequency transition (i.e. largest difference in frequency)
possible from the n = 6 to a lower level. (HINT: Try drawing a
picture first…) b) Calculate the wavelength (in nm) of...

2.) Which transition in a hydrogen atom would absorb the photon
of greatest frequency?
n = 3 to n = 1
n = 6 to n = 2
n = 2 to n = 9
n = 35 to n = 2
n = 12 to n = 6
n = 1 to n = 4
***NOT n=2 to n=9***

A hydrogen atom undergoes a transition from n = 5 to n = 2.
Considering the fact that it may go through intermediate steps
between 5 and 2 (for example, 5 → 3 → 2),
a) what is the shortest possible wavelength for emitted
photons?
b) what is the longest possible wavelength for emitted
photons?

Consider the electronic transition from n = 4 to n = 1 in a
hydrogen atom, and select the correct statement below: A photon of
97 nm wavelength and 2.05x10-18 J energy was emitted from the
hydrogen atom in this electronic transition. A photon of 97 nm
wavelength and 2.05x10-18 J energy was absorbed by the hydrogen
atom in this electronic transition. A photon of 122 nm wavelength
and 1.64x10-18 J energy was emitted from the hydrogen atom in this...

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