Calculate the wavelengths of the first five emissi...

Question

Calculate the wavelengths of the first five emission lines of the Balmer series for hydrogen

Patrick Ford · Accepted Answer

For this problem, we need the equation for the emission of spectral lines.1λ=R(1nf2-1ni2) where R is the Rydberg constant. [readmore]R = 1.097 × 107 m-1 nf for the Balmer series  = 2First emission: ni = 3λ = [R(1/nf2 - 1/ni2)]-1 = [(1.097 × 107)(1/22 - 1/32)]-1 = 656nmSecond emission: ni = 4λ = [R(1/nf2 - 1/ni2)]-1 = [(1.097 × 107)(1/22 - 1/42)]-1 = 486nmThird emission: ni = 5λ = [R(1/nf2 - 1/ni2)]-1 = [(1.097 × 107)(1/22 - 1/52)]-1 = 433nmFourth emission: ni = 6λ = [R(1/nf2 - 1/ni2)]-1 = [(1.097 × 107)(1/22 - 1/62)]-1 = 410nmFifth emission: ni = 7λ = [R(1/nf2 - 1/ni2)]-1 = [(1.097 × 107)(1/22 - 1/72)]-1 = 397nmThe wavelengths of the first five emissions are 656nm, 486nm, 433nm, 410nm, and 397nm

Problem: Calculate the wavelengths of the first five emission lines of the Balmer series for hydrogen

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Problem Details

Problem: Calculate the wavelengths of the first five emission lines of the Balmer series for hydrogen

FREE Expert Solution

Problem Details

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