When a hydrogen atom is raised from the ground state to an excited state
Potential energy decreases and kinetic energy increases
Potential energy increases and kinetic energy decreases
Both kinetic energy and potential energy decrease
Absorption spectrum
The ionization energy of hydrogen atoms is 13.6 eV, the ionization energy of helium atom would be
13.6 eV
27. 2 eV
6.8 eV
54. 4 eV
The ionization energy of the electron in the hydrogen atom in its ground state is 13.6 eV. The atoms are excited to higher energy levels to wavelength of emitted radiation corresponds to the transition between
n = 3 to n = 2 states
n = 3 to n = 1 states
n = 2 to n = 1 states
n = 4 to n = 3 states
The spectrum obtained from a sodium vapour lamp is an example of
Band spectrum
Continuous spectrum
Emission spectrum
If the electron in a hydrogen atom jumps from an orbit with level n2 = 3 to an orbit with level n1 = 2, the emitted radiation has a wavelength given by
λ = 6/R
λ = R/6
To explain theory of hydrogen atom, Bohr considered
Quantisation of linear momentum
Quantisation of angular momentum
Quantisation of angular frequency
Quantisation of energy
Hydrogen atoms are excited from ground state to the principal quantum number 4. Then the number of spectral lines observed will be
3
6
5
2
The energy required to excite hydrogen atom from n = 1 to n = 2 state is 10.2 eV. What is the wavelength emitted when it returns to ground state?
1020 × 10-10 m
1220 × 10-10 m
1320 × 10-10 m
920 × 10-10 m
The total energy of electron in the ground state of hydrogen atom is -13.6 eV. The kinetic energy of an electron in the first excited state is
3.4 eV
1.7 eV
When hydrogen atom is in its first excited level, its radius is
Four times, its ground sate radius
Twice, its ground state radius
Same as its ground state radius
Half of its ground state radius
