Question

Calculate the wavelength and frequency of light emitted when an electron changes from n=5 to n=2 in the H atom.

Wavelength = ???m

Frequency = ??? s^-1

Answer #1

Here photon will be emitted

1/wavelength = R* (1/nf^2 - 1/ni^2)

R is Rydberg constant. R = 1.097*10^7

1/wavelength = R* (1/nf^2 - 1/ni^2)

1/wavelength = 1.097*10^7* (1/2^2 - 1/5^2)

wavelength = 4.341*10^-7 m

wavelength = 434 nm

we have:

wavelength = 4.341*10^-7 m

we have below equation to be used:

frequency = speed of light/wavelength

=(3.0*10^8 m/s)/(4.341*10^-7 m)

= 6.911*10^14 Hz

wavelength = 4.341*10^-7 m

frequency = 6.911*10^14 s-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

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

Calculate the wavelength of the photon emitted when an electron
makes a transition from n=5 to n=3. You can make use of the
following constants: h=6.626×10−34 J⋅s c=2.998×108 m/s 1 m=109
nm

Calculate the wavelength of the photon emitted when an electron
makes a transition from n=5 to n=3. You can make use of the
following constants: h=6.626×10−34 J⋅s c=2.998×108 m/s 1 m=109
nm

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?

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?

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?

Determine the wavelength of light emitted when an electron drops
from n=3 to n=2 where E1 = -10eV, E2 = -5eV, and E3 = -2.5eV

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.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 2 minutes ago

asked 3 minutes ago

asked 3 minutes ago

asked 8 minutes ago

asked 12 minutes ago

asked 20 minutes ago

asked 27 minutes ago

asked 27 minutes ago

asked 28 minutes ago

asked 33 minutes ago

asked 37 minutes ago

asked 40 minutes ago