The diagram shows the energy levels for an electron in a certain atom. Which transition shown represents the emission of a photon with the most energy?
What is the kinetic energy of the electron in an orbit of radius r in the hydrogen atom?
(e = electronic charge)
What happens whenever a hydrogen atom emits a photon in the Balmer series?
|1.||it may emit another photon in the Balmer series.|
|2.||it must emit another photon in the Lyman series.|
|3.||it may emit another photon in the Paschen series.|
|4.||it need not emit any more photon.|
The ionisation potential of hydrogen atom is
1. 13.60 volt
2. 8.24 volt
3. 10.36 volt
4. 14.24 bolt
Which source is associated with a line emission spectrum?
1. Electric fibre
2. Neon street Sign
3. Red traffic light
Ionisation potential of hydrogen atom is 13.6 eV. Hydrogen atoms in the ground state are excited by monochromatic radiation of photon energy 12.1 eV. According to Bohr's theory, the spectral lines emitted by hydrogen will be:
The frequency of the series limit of the Balmer series of hydrogen atoms in terms of Rydberg constant R and velocity of light C is:
Orbital acceleration of electron is
Consider the spectral line resulting from transition \(n=2\) to \(n = 1\) in the atoms and ions given below. The shortest wavelength is given by:
1. hydrogen atom
3. singly ionised helium
4. doubly ionised lithium
An particle of energy 5 MeV is scattered through by a fixed uranium nucleus. The distance of closest approach is of the order