sing the Rydberg equation, calculate the visible wavelength of light emitted as the electron drops back to the second energy level. Convert the units to nm. (Energy level for an excited electron in a hydrogen atom: 5). (Answer: 4.34x10^-4nm) b) What color would this correspond to? (Answer: Violet) c) Calculate the energy released by that electron. (Answer in scientific notation.) d) How much energy (in kJ) would be released if a mole of hydrogen atoms did this?
sing the Rydberg equation, calculate the visible wavelength of light emitted as the electron drops back to the second energy level. Convert the units to nm. (Energy level for an excited electron in a hydrogen atom: 5). (Answer: 4.34x10^-4nm) b) What color would this correspond to? (Answer: Violet) c) Calculate the energy released by that electron. (Answer in scientific notation.) d) How much energy (in kJ) would be released if a mole of hydrogen atoms did this?
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter5: Electrons In The Atom
Section5.1: Light And Quantized Energy
Problem 14SSC
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Using the Rydberg equation, calculate the visible
second energy level. Convert the units to nm. (Energy level for an excited electron in a hydrogen atom: 5). (Answer: 4.34x10^-4nm)
b) What color would this correspond to? (Answer: Violet)
c) Calculate the energy released by that electron. (Answer in scientific notation.)
d) How much energy (in kJ) would be released if a mole of hydrogen atoms did this?
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