Emission & Absorption Spectrum (DP IB Physics) : Revision Note

Katie M

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Katie M

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Spectra & Atomic Energy Levels

  • Atomic spectra are observed when atoms emit or absorb light of certain wavelengths

    • These are known as emission spectra and absorption spectra

  • Atomic spectra provide evidence that electrons in atoms can only transition between discrete atomic energy levels

Emission Spectra

  • Emission spectra can be produced by heating a low-pressure gas

    • Heating provides energy to excite electrons to higher energy levels

    • When an electron transitions back to a lower energy level, it emits a photon

  • Each transition corresponds to a specific wavelength of light which correlates to an observable spectral line

  • The resulting emission spectrum contains a set of discrete wavelengths, represented by coloured lines on a black background

Emission spectrum of hydrogen gas

hydrogen-emission-spectra

A typical hydrogen emission spectrum contains several spectral lines in the visible region of the electromagnetic spectrum

Absorption Spectra

  • Absorption spectra can be produced by passing white light through a cool, low-pressure gas

    • Only photons with the exact energy required to excite electrons will be absorbed

  • Each absorbed photon corresponds to a specific wavelength of light which correlates to an observable dark line in a continuous spectrum of wavelengths

  • The resulting absorption spectrum contains a set of discrete wavelengths, represented by dark lines on a coloured background

    • These lines correspond to the same lines observed on an emission spectrum for the same element

Absorption spectrum of hydrogen gas

hydrogen-absorption-spectra

A typical hydrogen absorption spectrum is the inverse of its emission spectrum

Spectra & Chemical Composition

  • The chemical composition of a substance can be investigated using emission and absorption spectra

  • Each element produces a unique pattern of spectral lines

  • No two elements produce the same set of spectral lines, therefore, elements can be identified by their atomic spectrum

Emission spectra of different elements

Reference-Spectra

Emission line spectra are unique to each element, like a fingerprint

  • For example:

    • Hydrogen is known to produce strong spectral lines in the red portion of the visible spectrum, at 656 nm

    • When sodium is burned, a characteristic yellow flame is observed due to it producing strong spectral lines in the yellow portion of the spectrum, at 589 nm

    • When mercury is burned, most of the emission lines are below 450 nm, which produces a characteristic blue light

  • Elements such as sodium and mercury are known for their use in street lights, as well as neon for its use in colourful signs

  • This can be achieved when

    • An electrical discharge is applied to the vapourised substance

    • The energy supplied excites orbital electrons within individual atoms to a higher energy state

    • When the electrons move back down to the ground state, a specific wavelength of light is emitted 

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Katie M

Author: Katie M

Expertise: Physics Content Creator

Katie has always been passionate about the sciences, and completed a degree in Astrophysics at Sheffield University. She decided that she wanted to inspire other young people, so moved to Bristol to complete a PGCE in Secondary Science. She particularly loves creating fun and absorbing materials to help students achieve their exam potential.

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