Worksheet: Atomic Emission Spectra

In this worksheet, we will practice labeling the lines in atomic emission spectra and linking their positions to electronic transitions in hydrogenic atoms.

Q1:

The atomic emission spectrum of cesium contains lines at frequencies of 3 . 4 5 × 1 0 1 4 Hz and 6 . 5 3 × 1 0 1 4 Hz. Calculate the difference in energy between these two lines.

Q2:

The atomic emission spectrum of rubidium contains lines at wavelengths of 780.0 nm and 424.4 nm. Calculate the difference in energy between these two lines.

  • A 2 . 9 2 1 × 1 0 1 9 J
  • B 2 . 5 4 7 × 1 0 1 9 J
  • C 3 . 2 2 0 × 1 0 1 9 J
  • D 2 . 1 3 4 × 1 0 1 9 J
  • E 5 . 5 8 6 × 1 0 1 9 J

Q3:

The visible lines of the atomic emission spectrum for hydrogen are produced by electronic transitions to a common energy level. What is the principal quantum number 𝑛 for this energy level?

Q4:

Which of the following series of electronic transitions in the hydrogen atom produces spectral lines with the shortest wavelengths?

  • APaschen series
  • BBalmer series
  • CBrackett series
  • DLyman series
  • EPfund series

Q5:

In which series of electronic transitions in the hydrogen atom does the lower energy level have the principal quantum number 𝑛 = 4 ?

  • ABalmer series
  • BLyman series
  • CPaschen series
  • DBrackett series
  • EPfund series

Q6:

Which series of electronic transitions in the hydrogen atom produces spectral lines with ultraviolet wavelengths?

  • APaschen series
  • BBalmer series
  • CBrackett series
  • DLyman series
  • EPfund series

Q7:

Which series of electronic transitions in the hydrogen atom is responsible for all visible lines in its emission spectrum?

  • APaschen series
  • BLyman series
  • CBrackett series
  • DBalmer series
  • EPfund series

Q8:

Which series of electronic transitions in the hydrogen atom produces spectral lines with infrared wavelengths?

  • ABalmer series
  • BLyman series
  • CBrackett series
  • DPaschen series
  • EPfund series

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