307138 If the energy of an electron in the second Bohr orbit of H-atom is \({\rm{ }} - {\rm{E}}\) , what is the energy of the electron in the Bohr's first orbit ?

307170 The ionisation energy of a hydrogen atom is 13.6 eV. The energy of the third-lowest electronic level in doubly ionised lithium ion \({\rm{(Z = 3)}}\) is

307139 Based on the equation:
\({\rm{\Delta E = - 2}}{\rm{.0 \times 1}}{{\rm{0}}^{{\rm{ - 18}}}}{\rm{J}}\left( {\frac{{\rm{1}}}{{{\rm{n}}_{\rm{1}}^{\rm{2}}}}{\rm{ - }}\frac{{\rm{1}}}{{{\rm{n}}_{\rm{2}}^{\rm{2}}}}} \right){\rm{,}}\) the wavelength of the light that must be absorbed to excite hydrogen electron from level \({\rm{n = 1}}\) to level \({\rm{n = 2}}\) will be:
\({\rm{(h = 6}}{\rm{.625 \times 1}}{{\rm{0}}^{{\rm{ - 34}}}}{\rm{Js,c = 3 \times 1}}{{\rm{0}}^{\rm{8}}}\,{\rm{m}}{{\rm{s}}^{{\rm{ - 1}}}}{\rm{)}}\)

307140 If potential energy of an electron in hydrogen atom is \({\rm{ - x}}\,{\rm{eV}}\), then its kinetic energy will be

307138 If the energy of an electron in the second Bohr orbit of H-atom is \({\rm{ }} - {\rm{E}}\) , what is the energy of the electron in the Bohr's first orbit ?

307170 The ionisation energy of a hydrogen atom is 13.6 eV. The energy of the third-lowest electronic level in doubly ionised lithium ion \({\rm{(Z = 3)}}\) is

307139 Based on the equation:
\({\rm{\Delta E = - 2}}{\rm{.0 \times 1}}{{\rm{0}}^{{\rm{ - 18}}}}{\rm{J}}\left( {\frac{{\rm{1}}}{{{\rm{n}}_{\rm{1}}^{\rm{2}}}}{\rm{ - }}\frac{{\rm{1}}}{{{\rm{n}}_{\rm{2}}^{\rm{2}}}}} \right){\rm{,}}\) the wavelength of the light that must be absorbed to excite hydrogen electron from level \({\rm{n = 1}}\) to level \({\rm{n = 2}}\) will be:
\({\rm{(h = 6}}{\rm{.625 \times 1}}{{\rm{0}}^{{\rm{ - 34}}}}{\rm{Js,c = 3 \times 1}}{{\rm{0}}^{\rm{8}}}\,{\rm{m}}{{\rm{s}}^{{\rm{ - 1}}}}{\rm{)}}\)

307140 If potential energy of an electron in hydrogen atom is \({\rm{ - x}}\,{\rm{eV}}\), then its kinetic energy will be

307138 If the energy of an electron in the second Bohr orbit of H-atom is \({\rm{ }} - {\rm{E}}\) , what is the energy of the electron in the Bohr's first orbit ?

307170 The ionisation energy of a hydrogen atom is 13.6 eV. The energy of the third-lowest electronic level in doubly ionised lithium ion \({\rm{(Z = 3)}}\) is

307139 Based on the equation:
\({\rm{\Delta E = - 2}}{\rm{.0 \times 1}}{{\rm{0}}^{{\rm{ - 18}}}}{\rm{J}}\left( {\frac{{\rm{1}}}{{{\rm{n}}_{\rm{1}}^{\rm{2}}}}{\rm{ - }}\frac{{\rm{1}}}{{{\rm{n}}_{\rm{2}}^{\rm{2}}}}} \right){\rm{,}}\) the wavelength of the light that must be absorbed to excite hydrogen electron from level \({\rm{n = 1}}\) to level \({\rm{n = 2}}\) will be:
\({\rm{(h = 6}}{\rm{.625 \times 1}}{{\rm{0}}^{{\rm{ - 34}}}}{\rm{Js,c = 3 \times 1}}{{\rm{0}}^{\rm{8}}}\,{\rm{m}}{{\rm{s}}^{{\rm{ - 1}}}}{\rm{)}}\)

307140 If potential energy of an electron in hydrogen atom is \({\rm{ - x}}\,{\rm{eV}}\), then its kinetic energy will be

307138 If the energy of an electron in the second Bohr orbit of H-atom is \({\rm{ }} - {\rm{E}}\) , what is the energy of the electron in the Bohr's first orbit ?

307170 The ionisation energy of a hydrogen atom is 13.6 eV. The energy of the third-lowest electronic level in doubly ionised lithium ion \({\rm{(Z = 3)}}\) is

307139 Based on the equation:
\({\rm{\Delta E = - 2}}{\rm{.0 \times 1}}{{\rm{0}}^{{\rm{ - 18}}}}{\rm{J}}\left( {\frac{{\rm{1}}}{{{\rm{n}}_{\rm{1}}^{\rm{2}}}}{\rm{ - }}\frac{{\rm{1}}}{{{\rm{n}}_{\rm{2}}^{\rm{2}}}}} \right){\rm{,}}\) the wavelength of the light that must be absorbed to excite hydrogen electron from level \({\rm{n = 1}}\) to level \({\rm{n = 2}}\) will be:
\({\rm{(h = 6}}{\rm{.625 \times 1}}{{\rm{0}}^{{\rm{ - 34}}}}{\rm{Js,c = 3 \times 1}}{{\rm{0}}^{\rm{8}}}\,{\rm{m}}{{\rm{s}}^{{\rm{ - 1}}}}{\rm{)}}\)

307140 If potential energy of an electron in hydrogen atom is \({\rm{ - x}}\,{\rm{eV}}\), then its kinetic energy will be