For any H like system, the ratio of velocities of electron in I, II & III orbit e.e.,`V_(1):V_(2):V_(3)` will be:
For any H like system, the ratio of velocities of electron in I, II & III orbit e.e.,`V_(1):V_(2):V_(3)` will be:
A
`1:2:3`
B
`1:1//2:1//3`
C
`3:2:1`
D
`1:1:1`
Text Solution
Verified by Experts
Topper's Solved these Questions
Similar Questions
Explore conceptually related problems
If photons of frequency v are incident on the surface of metals A and B of threshold frequencies v/2 and v/3 respectively, the ratio of the maximum kinetic energy of electrons emitted from A to that from B is:
Define the term work function of a metal. The threshold frequency of a metal is 2f_0 is incident on the metal plate, the maximum velocity of electrons emitted is v_1 , when the frequency of the incident radiation is increased of 5f_0 the maximum velocity of electrons emitted is v_2 . Find the ratio of v_1 to v_2 .
Bohr's model of hydrogen atom In order to explain the stability of atom and its line spectra, Bohr gave a set of postulates: An electron in an atom revolves in certain circular orbit around the nucleus. These are the orbits for which mvr=(nh)/(2pi) In these allowed orbits, the electron does not radiate energy. When an electron jumps from higher energy level E_(n_2) to lower energy orbit E_(n_1) , radiation is emittd and frequency of emitted electron is given by v=(E_(n_2)-E_(n_1))/h . Further the radius of the n^(th) orbit of hydrogen atom is r=(n^2h^24piepsilon_0)/(4pi^2me^2) and energy of the n^(th) orbit is given by E_n=-13.6/n^2 eV . The angular momentum of the orbital electron is integarl multiple of
Bohr's model of hydrogen atom In order to explain the stability of atom and its line spectra, Bohr gave a set of postulates: An electron in an atom revolves in certain circular orbit around the nucleus. These are the orbits for which mvr=(nh)/(2pi) In these allowed orbits, the electron does not radiate energy. When an electron jumps from higher energy level E_(n_2) to lower energy orbit E_(n_1) , radiation is emittd and frequency of emitted electron is given by v=(E_(n_2)-E_(n_1))/h . Further the radius of the n^(th) orbit of hydrogen atom is r=(n^2h^24piepsilon_0)/(4pi^2me^2) and energy of the n^(th) orbit is given by E_n=-13.6/n^2 eV . If 13.6 eV energy is required to ionise the hydrogen atom, then enegy required to remove an electron from n=2 is:
Bohr's model of hydrogen atom In order to explain the stability of atom and its line spectra, Bohr gave a set of postulates: An electron in an atom revolves in certain circular orbit around the nucleus. These are the orbits for which mvr=(nh)/(2pi) In these allowed orbits, the electron does not radiate energy. When an electron jumps from higher energy level E_(n_2) to lower energy orbit E_(n_1) , radiation is emittd and frequency of emitted electron is given by v=(E_(n_2)-E_(n_1))/h . Further the radius of the n^(th) orbit of hydrogen atom is r=(n^2h^24piepsilon_0)/(4pi^2me^2) and energy of the n^(th) orbit is given by E_n=-13.6/n^2 eV . What would happen, if the electron in an atom is stationary?
Bohr's model of hydrogen atom In order to explain the stability of atom and its line spectra, Bohr gave a set of postulates: An electron in an atom revolves in certain circular orbit around the nucleus. These are the orbits for which mvr=(nh)/(2pi) In these allowed orbits, the electron does not radiate energy. When an electron jumps from higher energy level E_(n_2) to lower energy orbit E_(n_1) , radiation is emittd and frequency of emitted electron is given by v=(E_(n_2)-E_(n_1))/h . Further the radius of the n^(th) orbit of hydrogen atom is r=(n^2h^24piepsilon_0)/(4pi^2me^2) and energy of the n^(th) orbit is given by E_n=-13.6/n^2 eV . The ground state energy of hydroen atom is -13.6 eV. The KE and PE of the electron in this state are
Define the term work function of a metal. The threshold frequency of a metal is f_0 when the light of frequency 2f_0 is incident on the metal plate, the maximum velocity of electrons emitted is v_1 , when the frequency of the incident radiation is increased to 5f_0 , the maximum velocity of electrons emitted is v_2 . Find the ratio of v_1 and v_2 .
Bohr's model of hydrogen atom In order to explain the stability of atom and its line spectra, Bohr gave a set of postulates: An electron in an atom revolves in certain circular orbit around the nucleus. These are the orbits for which mvr=(nh)/(2pi) In these allowed orbits, the electron does not radiate energy. When an electron jumps from higher energy level E_(n_2) to lower energy orbit E_(n_1) , radiation is emittd and frequency of emitted electron is given by v=(E_(n_2)-E_(n_1))/h . Further the radius of the n^(th) orbit of hydrogen atom is r=(n^2h^24piepsilon_0)/(4pi^2me^2) and energy of the n^(th) orbit is given by E_n=-13.6/n^2 eV . When hydrogen atom is the first excited level, it radius is:,
Bohr model is a system consisting of small, dense nucleus surounded by orbting electrons. The electrons travel in defined circular orbits around the nucleus for which orbital angular momentum is an itnegral multiple of h/(2pi) . While rotating in allowed orbits the electrons does not raidate energy. Electromagneitc radiations are emitted when the electrons jumps from a higher orbit (E_(n_i)) to a lower orbit (E_(n_f)) Allowed energy of hydrogen atom in the n^(th) orbit is:
Bohr model is a system consisting of small, dense nucleus surounded by orbting electrons. The electrons travel in defined circular orbits around the nucleus for which orbital angular momentum is an itnegral multiple of h/(2pi) . While rotating in allowed orbits the electrons does not raidate energy. Electromagneitc radiations are emitted when the electrons jumps from a higher orbit (E_(n_i)) to a lower orbit (E_(n_f)) The radius of first orbit out of the allowed of its is: