When electron jumps from n = 4 to n = 2 orbit, we get :
second line of Lyman series
second line of Balmer series
second line of Paschen series
an absorption line of Balmer series
Ionization 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 :
2
3
4
1
Hydrogen atoms are excited from ground state of the principal quantum number 4. Then the number of spectral lines observed will be
6
5
Consider an electron in the nth orbit of a hydrogen atom in the Bohr model. If the circumference of orbit can be expressed in terms of de-Broglie wavelength λ ,then find out it's value ?
( 0.529 ) n λ
√ n λ
( 13.6 ) λ
n λ
When a hydrogen atom is raised from the ground state to an excited state.
PE decreases and KE increases
PE increases and KE decreases
Both KE and PE decreases
Absorption spectrum
The radius of hydrogen atom in its ground state is 5.3 x 10 -11 m. After collision with an electron it is found to have a radius of 21.2 x 10 – 11 m. What is the principal quantum number n of the final state of the atom ?
n = 4
n = 2
n = 16
n = 3
The ionization energy of hydrogen atom is 13.6 eV. Following Bohr’s theory, the energy corresponding to a transition between 3rd and 4th orbit is
3.40 eV
1.51 eV
0.85 eV
0.66 eV
In Rutherford scattering experiment, what will be the correct angle for α- scattering for an impact parameter, b = 0 ?
90o
270 o
0o
180o
The ground state energy of hydrogen atom is -13.6 eV. When its electron is in the first excited state, its excitation energy is
3.4 eV
6.8 eV
10.2 eV
Zero
The spectrum obtained from a sodium vapour lamp is an example of
band spectrum
continuous spectrum
emission spectrum
absorption spectrum
