1) Consider the Bohr model of the hydrogen model (Z=1) in which an electron is in thesmallest possible orbit (n=1).a) Find the acceleration of the electron in this orbit.b) Classical electromagnetic theory predicts that an electron with acceleration a willradiate energy. The power loss is given by = -2e²a²/(3(4¹c³)). Evaluate thisformula for this atom where c is the speed of light in vacuum.c) If the electron continues to radiate at this rate how long will it take to reduce theenergy from -13.6 eV to twice this value.

Answered: Image /qna-images/answer/179d4ee9-03cc-410a-8ea9-a30410e4d45d.jpg

Answered: 1) Consider the Bohr model of the…

Similar questions

The gravitational attraction between electron and proton in a hydrogen atom is weaker than the coulomb attraction by a factor of about 10-40. An alternative way of looking at this fact is to estimate the radius of the first Bohr orbit of a hydrogen atom if the electron and proton were bound by gravitational attraction. You will find the answer interesting.
QUESTION 45 In the Bohr model what is the ratio of the radius of orbit n = 2 to the radius of orbit n = 8? a. one/64 b. one-sixteenth In the Bohr model what is the ratio of the energy of orbit n = 12 to the energy of orbit n = 3? a. one/64 b. one-sixteenth
3. The ground state wavefunction for a hydrogen atom can be written as µ=Be*/a where B is a constant and a is the Bohr radius. (a) Show that the probability density of this wavefunction is: P(r)=Cre 2r/0 where C is a constant. (b) Calculate the value of r for which this is a maximum.
The so-called Lyman-a photon is the lowest energy photon in the Lyman series of hydrogen and results from an electron transitioning from the n = 2 to the n = 1 energy level. Determine the energy in eV and the wavelength in nm of a Lyman-a photon. HINT (a) the energy in eV eV (b) the wavelength in nm nm
Energy changes of -1.8167 x 10-19 is recorded when an electron jump from n=6 in an unknown series of hydrogen line spectra. a) calculate the value of nf- [ RH = 2.18 x 10-19]b) identify the line spectra for this radiation
An electron in a hydrogen atom is excited from the ground state to the n = 3 state. True or false?a) The wavelength of light emitted when the electron drops from n=3 to n = 1 is longer than that from n = 3 to n = 2.
Determine the wavelengths of the photons from the transition of hydrogen electron from n1 = 2 to n2 = 7.
M2
A particular Bohr orbit in a hydrogen atom has a total energy of-0.85 eV. What are (a) the kinetic energy of the electron in thisorbit and (b) the electric potential energy of the system?
an electron in a hydrogen atom is in a state with principal quantum number n = 3. a) what is the largest orbital angular momentum it can have? b) which values of the z - component of the angular momentum are allowed with this total momentum? (leave answers in units of h bar) c) the electron transitions to the n = 2 energy level, emitting a photon. what is that photon's length?
5) A metal with work function 9.05 eV is used for a photoelectric effect lab. Find the energy of the electrons if light with 200nm wavelength is used. 6) Energy levels for a particular system is given as En = 10.5 n(n+1)/n^3 in eV. Find the energy for electron transition from n=2 to n=4. Determine if this transition is an absorption that requires energy or it is an emission that releases photon.
A hydrogen atom initially in the ground level absorbs a photon, which excites it to the n = 4 level. Determine the wavelength and frequency of photon.

SEE MORE QUESTIONS