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Chapter 6 Review Packet 11-14-02[1]

A mole of photons of wavelength 725 nm has kj of

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10. A mole of photons of wavelength 725 nm has ______ kJ of energy. a. 2.74 x 10 -19 b. 4.56 x 10 -46 c. 6.05 x 10 -3 d. 165 e. 227 11. It takes 254 kJ/mol to eject electrons from a certain metal surface. What is the longest wavelength of light (nm) that can be used to eject electrons from the surface of this metal via the photoelectric effect? 12. An electron in a Bohr hydrogen atom has an energy of -1.362 x 10 -19 J. The value of n for this electron is __________. 13. Calculate the energy (J) change associated with an electron transition from n=2 to n=5 in a Bohr hydrogen atom. 14. In the Bohr model of the atom, _____. a. electrons travel in circular paths called orbitals b. electrons can have any energy c. electron energies are quantized d. electron paths are controlled by probability e. both a and c 15. The n=2 to n=6 transition in the Bohr hydrogen atom corresponds to the _________ of a photon with a wavelelngth of ______ nm. 16. The wavelength of a particle is given by __________.
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