If you are given the wavelengths of light observed by a particular student for the hydrogen emission spectrum you should be able to (a) determine the frequencies and energies associated with these wavelengths, (b) be able to use the Bohr equation to calculate the wavelengths expected for the Balmer series of the hydrogen atom, (c) be able to quantitatively compare the results from (a) and (b) - i.e., know how to calculate the % difference between a students results and Bohrs.

If you are given the wavelengths of light observed by a particular student for the hydrogen emission spectrum you should be able to (a) determine the frequencies and energies associated with these wavelengths, (b) be able to use the Bohr equation to calculate the wavelengths expected for the Balmer series of the hydrogen atom, (c) be able to quantitatively compare the results from (a) and (b) - i.e., know how to calculate the % difference between a students results and Bohrs.

If you are given the wavelengths of light observed by a particular student for the hydrogen emission spectrum you should be able to (a) determine the frequencies and energies associated with these wavelengths, (b) be able to use the Bohr equation to calculate the wavelengths expected for the Balmer series of the hydrogen atom, (c) be able to quantitatively compare the results from (a) and (b) - i.e., know how to calculate the % difference between a students results and Bohrs.



(a) ∙frequency= speed of light/wavelength

∙energy= frequency x Planck's constant.

(b) ΔE= -Rn x (1/nf^2 - 1/ni^2)


(c) % difference = [(actual - theoretical)/ actual] x 100%


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