For the `beta^+` (positron) emission from a nucleus, there is another competing process known as electron capture (electron from an inner orbit, say, the K emitted). `e^+` + `"_Z^AX` `rarr` `"_(Z-1)^AY` + `v` . Show that if `beta^+` emission is energetically allowed, electron capture is necessarily allowed but not vice-versa

Which of the following processes causes the emission of X-ray? a) alpha -emission b) beta -emission c) beta^(+) (Positron) emission d) electron capture

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:

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)) When an electron jumps from higher to lower orbit energy is:

Bohr model is a system consisting of small, dense nucleus surrounded by orbiting electrons. The electrons travel is defined circular orbits around the nuclues which orbital angular moementum is an integral multiple of h/(2pi) . While rotating in allowed orbits (stationary orbits) the electron does not radiate energy. electromagnetic radiations are emitted when the electron jumps from a higher orbit (E_(ni)) to a lower orbit (E_(nf)) . The total energy of the electron in an atom is negative. It suggests that

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)) Balmer series lies in:

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 . 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 . 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