Question

What is the wavelength of light (in m) emitted by a hydrogen atom when an electron relaxes from the 5 energy level to the 3 energy level?

Answer #1

1/ = RH(1/n1^2 - 1/n2^2)

RH = 109678cm^-1

n1 = 3

n2 = 5

1/ = 109678(1/(3)^2 -1/(5)^2)

1/ = 109678(1/9 -1/25)

1/ = 109678(0.11-0.04)

1/ = 7677.46

= 1/7677.46 = 0.00013cm = 1.3*10^-4cm

= 1.3*10^-6 m >>>>answer

A. 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=7. Express the wavelength in
nanometers to three significant figures.
B. An electron in the n=6 level of the hydrogen atom relaxes to
a lower energy level, emitting light of λ=93.8nm. Find the
principal level to which the electron relaxed. Express your answer
as an integer.
Can you explain it in...

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 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.

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 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

If the wavelength of light emitted when an electron relaxes from
n = 3 level is 102.6 nm, to what level did the electron relax
to?

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.

What is the wavelength of the photon emitted as the electron in
the hydrogen atom transitions from the 3rd to 2nd level? What is
the frequency of the photon and what is the energy carried by the
photon?
got -6606 A for the first one and I'm not sure if I'm doing it
right

The best answer for the wavelength of light emitted when an
electron transitions from the fourth energy level to the first
energy level in a hydrogen atom is:
a. 97.2 nm
b 972 nm
c. 9.72 nm
d. 9720 nm
e. .972 nm

Calculate the wavelength of a photon emitted when the electron
in a Li2+ ion relaxes from the n=8 energy level to the n=4 energy
level. (Use Bohr's model of the atom.)

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 17 minutes ago

asked 18 minutes ago

asked 18 minutes ago

asked 22 minutes ago

asked 48 minutes ago

asked 57 minutes ago

asked 57 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago