The three lowest energy levels of the electron in the Hydrogen atom have energies energies E₁= -21.8 x 10-19 J E₂= -5.45 x 10-1⁹ J E3= -2.43 x 10-1⁹ J Determine the wavelength of the spectral line due to the transition between levels E3 and E₁. -34 [Assume Planck's constant h = 6.6 x 10 J s, Speed of light c = 3 × 108 ms¯

11. In the Balmer series, during which of the following energy state changes of the hydrogen atom is the photon with the most energy emitted? (A) n = 5 directly to n = 2 (B) n = 4 directly to n = 2 (C) n = 2 directly to n = 4 (D) n = 2 directly to n = 5 12. What is the minimum energy needed to ionize a hydrogen atom when it is in the n = 2 state? (A) 1.9 eV (B) 3.4 eV (C) 12.2 eV (D) 13.6 eV

Which of these expressions would yield the wavelength of light in meters emitted when an electron drops from orbit n = 3 to n = 2 in a Bohr hydrogen atom? Given h = 4.14 x 10-15 eVs and c = 3.00 x 108 m/s.     a. 1.89/hxc   b. hc/1.89   c. 1.89 x h x c   d. (1.51 + 3.4)/hc   e. hc/3.4

II. Ordinary Notation 456,000 0.000457 Scientific Notation (6.) (7.) (8.) 23,700 (9.) (10.) (11.) (12.) 2.34 х 104 2.34 x 104 4.90 x 102 7.82 x 105

The ground state energy of hydrogen atom is -13.6 eV. (i) What is the potential energy of an electron in the 3rd excited state? (ii) If the electron jumps to the ground state from the 3rd excited state, calculate the wavelength of the photon emitted.