Emission Spectra and the Bohr Model of the Atom (Leaving Cert Physics): Flashcards

Unique light patterns emitted by excited atoms

All wavelengths present; smooth rainbow red to violet

Hot solids or liquids (e.g. tungsten filaments)

Specific wavelengths as distinct lines on dark background

Hot gases or electric discharge through gas

Electrons exist only in specific energy levels, not in between

$n = 1$, lowest energy level where electrons normally exist

$n = 2, 3, 4$, etc.; higher energy levels above ground state

A fixed energy value that an electron in an atom can have

Electron falls to lower level, energy released as photon

$E = hf$ where $h$ is Planck's constant, $f$ is frequency

$h = 6.63 \times 10^{-34}$ J·s

$c = f\lambda$ where $c = 3.00 \times 10^8$ m/s

Inversely related: higher energy = shorter wavelength (bluer)

Visible spectral lines from transitions ending at $n = 2$