x

Electron Transitions

Calculate the wavelength of the photon released when an electron drops from energy level 3 to energy level 2


- \(3.4-1.5=1.9eV\)
- \(eV \to J\) = \(1.60\times 10^{-19}\)
- \(1.90\) \(eV\) \(\to\) \(3.04\times 10^{-19}J\)

- Use the equation \(E=\frac{hc}{\lambda}\)
- Rearrange to: \(\lambda=\frac{hc}{E}\)
- \(\frac{(6.63\times10^{-34})\times(3.00\times 10^8)}{3.04\times 10^{-19}}=6.54\times10^{-7}\)

Electron Transitions using Line Emission Spectrums
  • When an electron jumps down an energy level, a photon is released.
  • This photon has a wavelength that depends on how much energy is in it (how much energy was released from the electron)
    The equations
    • \[E=hf\]
    • \[E=\frac{hc}{\lambda}\]
    • \[\lambda=\frac{hc}{E}\]
  • These equations can be used to calculate energy, wavelength and freqency.
Ionisation
  • When an electron is removed from an atom, the atom is ionised.
  • The energy of each energy level shows the amount of energy required to remove an electron from that particular energy level.
  • The Ionisation energy shows how much energy is required to remove an electron from the ground state.
Left-click: follow link, Right-click: select node, Scroll: zoom
x