# Review I Constants I Periodic Table You may want to reference (Pages 85 - 88) Section 2.3 while completing this problem. Part A Calculate the frequency of the light emitted when an electron in a hydrogen atom makes each of the following transitions. Then, calculate the energy emitted from each transition. n 4-n 3 Express the frequency in inverse seconds. 1.60x1014 s-1 Previous Answers Submit Correct To calculate the frequency, you should have started by using the equation -18 J 1 1 AE=-2.18x 10 where AE is the change in energy and n is the energy level. Once you had the energy in joules, you could solve for frequency v using the equation E hv where h is Planck's constant. Part B What is the energy emitted from n = 4->n= 3 transition in J? V0 ΑΣφ ? J Submit Request Answer

Question help_outlineImage TranscriptioncloseReview I Constants I Periodic Table You may want to reference (Pages 85 - 88) Section 2.3 while completing this problem. Part A Calculate the frequency of the light emitted when an electron in a hydrogen atom makes each of the following transitions. Then, calculate the energy emitted from each transition. n 4-n 3 Express the frequency in inverse seconds. 1.60x1014 s-1 Previous Answers Submit Correct To calculate the frequency, you should have started by using the equation -18 J 1 1 AE=-2.18x 10 where AE is the change in energy and n is the energy level. Once you had the energy in joules, you could solve for frequency v using the equation E hv where h is Planck's constant. Part B What is the energy emitted from n = 4->n= 3 transition in J? V0 ΑΣφ ? J Submit Request Answer fullscreen

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