2. Determine the energy of an electron for the following scenarios. a, n=20f He* b, n=30f...
Using the Bohr model, determine the energy in joules of the photon produced when an electron in a Li2+ ion moves from the orbit with n = 2 to the orbit with n = 1
Using the Bohr model, determine: a. The lowest possible energy, in joules, for the electron in the Lition. b. The lowest possible energy for the electron in the He ion. c. The energy of an electron with n=6 in a hydrogen atom. d. The energy of an electron with n=8 in a hydrogen atom.
9- Determine the wavelength necessary to ionize H, He+, and Li2+. 10- Determine the energy of the electron in the second excited state of a B4+ ion. How much energy is required to remove the electrons from one mole of B4+ ions in this state? Calculate the corresponding frequency and wavelength of the light emitted in a transition from the second excited state to the first excited state energy level of this ion.
Using the Bohr model, determine the lowest possible energy, in joules, for the electron in the Li2+ ion. En = -kZ2/n2 (k = 2.179×10–18 J, n is the quantum number of an orbital, Z is the nuclear charge; this equation applies to an atom with only one electron; please note that the nuclear charge is different from the atom charge)
2. Determine the ionization energy (in kJ mol-1) of a He+ ion with its electron in its lowest energy orbital.
An electron in the n=2 energy level makes a transition to the n=7 energy level after absorbing a 397 nm photon. What is the energy difference between these levels in electron volts (1 eV = 1.6 x 10-19 J)? A. 5.00 eV B. 4.74 eV C. 3.97 eV D. 3.13 eV E. 2.35 eV
How much energy would be required to ionize(remove the final electron from) a He+ ion if the electron was in the n=2 level? Would it require more or less energy if the electron was in the n=4 level? (a) 2.18 x 10-18 J, more (b) 2.18 x 10-18 J, less (c) - 5.45x 10-19 J, more (d) 5.45x 10-19J, less (e) 5.45x 10-19 J, same
The single electron on a Li2+(g) atom is excited to the n=7 orbital. When the electron falls to the n=3 orbital a photon of light is emitted by the atom. What is the wavelength of this photon of light? (a) 496 nm (b) 1005 nm (c) 112 nm (d) 91.2 nm (e) 4468 nm ** solutions says answer is (C) but not sure how they got that
CALCULATOR FULL SCREEN PRINTER VERSION BACK NEXT SPECTROSCOPY AND REACTIVITY T04/S07 The energy levels the electron can occupy in the Li2+ ion can be calculated using the energy level equation. A Li2+ ion emitted a photon with a frequency of 5.55 x 1015 Hz to reach an energy level with n=2. What was the value of n for its initial energy level? Speed of Light c=3.00x108 m/s Planck's Constant h=6.63x10-34 J s Rydberg's Constant Rh=2.18x10-18 ] Avogadro's No. NA=6.02x1023mol-1 Energy...
2. Calculate the energy of an electron in the n=2 energy level of hydrogen. Calculate the energy of an electron in the n=3 energy level. What is the difference in energy of these two levels? If a photon of -2,18 X/ 08 2427 light had this energy, what would its wavelength be?