Solution Found!
The visible emission lines observed by Balmer all involved
Chapter , Problem 6.41(choose chapter or problem)
The visible emission lines observed by Balmer all involved nf = 2. (a) Which of the following is the best explanation of why the lines with nf = 3 are not observed in the visible portion of the spectrum: (i) Transitions to nf = 3 are not allowed to happen, (ii) transitions to nf = 3 emit photons in the infrared portion of the spectrum, (iii) transitions to nf = 3 emit photons in the ultraviolet portion of the spectrum, or (iv) transitions to nf = 3 emit photons that are at exactly the same wavelengths as those to nf = 2. (b) Calculate the wavelengths of the first three lines in the Balmer seriesthose for which ni = 3, 4, and 5and identify these lines in the emission spectrum shown in Figure 6.11.
Questions & Answers
QUESTION:
The visible emission lines observed by Balmer all involved nf = 2. (a) Which of the following is the best explanation of why the lines with nf = 3 are not observed in the visible portion of the spectrum: (i) Transitions to nf = 3 are not allowed to happen, (ii) transitions to nf = 3 emit photons in the infrared portion of the spectrum, (iii) transitions to nf = 3 emit photons in the ultraviolet portion of the spectrum, or (iv) transitions to nf = 3 emit photons that are at exactly the same wavelengths as those to nf = 2. (b) Calculate the wavelengths of the first three lines in the Balmer seriesthose for which ni = 3, 4, and 5and identify these lines in the emission spectrum shown in Figure 6.11.
ANSWER:Problem 6.41The visible emission lines observed by Balmer all involved nf = 2. (a) Which of the following isthe best explanation of why the lines with nf = 3 are not observed in the visible portion of thespectrum: (i) Transitions to nf = 3 are not allowed to happen, (ii) transitions to nf = 3 emitphotons in the infrared portion of the spectrum, (iii) transitions to nf = 3 emit photons in theultraviolet portion of the spectrum, or (iv) transitions to nf = 3 emit photons that are at exactly thesame wavelengths as those to nf = 2. (b) Calculate the wavelengths of the first three lines in theBalmer seriesthose for which ni = 3, 4, and 5and identify these lines in the emissionspectrum shown in Figure 6.11. Step-by-step solution Step 1 of 11(a)The energy associated with the two orbits of the electron in the hydrogen atom is given by thefollowing equation. -18 1 1 E = (-2.18 x 10 J) ( n2 n2 ) ……..(1) f iWhere, E = Difference in energy between two states ni= Initial state nf= Final state