1. In the Bohr model for a hydrogen atom, an electron revolving in the third excited state. If the electron drops into second state, calculate the following: a. The total energy of the electron in the third excited state. b. The transition energy. c. The kinetic energy of electron in first excited state. DHA
Atomic Spectra
According to the Bohr model of an atom, the electron in an atom moves around a nucleus in fixed orbits with specific energies known as energy levels. The orbital energies are quantized. The electrons remain in these energy levels until they emit or absorb a photon of a particular wavelength, the quantum of energy. If the electron emits a photon, it then falls back to a lower energy level, and if it absorbs a photon, the electron rises to higher energy levels. The photons released or absorbed in these transitions of an electron are studied and analyzed on a screen as atomic spectra.
Ruby Lasers
Lasers are devices that emit light using atoms or molecules at a certain wavelength and amplify the light to produce a narrow beam of radiation. It works as per the principle of electromagnetic radiation. Their source of emission contains the same frequency and same phase. It was invented in the year 1960 by the great noble scientist, Theodore Maiman.
Balmer Series
The spectrum of frequency observed when electromagnetic radiation is emitted from an atom when it goes from higher energy state to lower state, is known as emission spectrum. This transition occurs when an excited electron moves from higher to lower state. It has many possible electron transitions and each transition has a specific energy difference.
Emission Spectrum
Every state of matter tries to be at minimum potential energy or it can be said that the atoms of element/ substance arrange themselves such that overall energy is minimum.
![Tutorial Sheet 01
1. In the Bohr model for a hydrogen atom, an electron revolving in the third excited
state. If the electron drops into second state, calculate the following:
a. The total energy of the electron in the third excited state.
b. The transition energy.
c. The kinetic energy of electron in first excited state.
2. Prove that the total energy of electron is measured in units of jou
CREDHA
3. Hydrogen atom electron moves from third orbit to the first orbit, calculate the wave
number of the radiated light. (Repeat using Rydberg equation).
4. Calculate the radius of orbit of an electron moving around a hydrogen atom with an
energy of -13.6ev. If a photon of energy 10.2ev hits electron and losses all its energy to
the electron, calculate the new radius of orbit. What frequency of light will be emitted
if the above electron changes it orbital radius to its old value?
5. An electron at rest
light of wavelength 4.96*10-7m. Calculate the velocity of
the electron.
6. An single electron orbits around a nucleus ofcharge (+Ze). It requires 47.2ev to excite
the electron from third Bohr orbit to the second orbit, calculate:
a. The value of Z.
b. The wavelength of electromagnetic radiation required to transferred the electron from
fourth to third orbit.
c. The radius of the first excited orbit.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcc93837e-b2e7-4f1b-8c8c-88a74806991f%2F7819d6aa-b5eb-44e1-ab4f-62a12013ec14%2Fszsvcbf_processed.jpeg&w=3840&q=75)
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