Atomic spectra

Definition

Atomic spectra are the distinct lines of color, or wavelengths of light, emitted or absorbed by atoms. These spectra result from transitions between different energy levels within an atom.

5 Must Know Facts For Your Next Test

1. Atomic spectra can be emission or absorption spectra, depending on whether the atom emits or absorbs photons.
2. Each element has a unique atomic spectrum, acting like a fingerprint for that element.
3. The lines in an atomic spectrum are due to electron transitions between quantized energy levels in an atom.
4. The Rydberg formula can predict the wavelengths of hydrogen spectral lines.
5. $E = h\nu$ relates the energy of emitted/absorbed light to its frequency $\nu$ and Planck's constant $h$.

Review Questions

• What causes the distinct lines in an atomic spectrum?
• How can you use atomic spectra to identify elements?
• What is the relationship between energy levels and spectral lines?

Related terms

Quantization: The concept that energy exists in discrete units called quanta rather than a continuous range.

$E = h\nu$: A formula expressing that the energy ($E$) of a photon is equal to Planck's constant ($h$) multiplied by its frequency ($\nu$).

Rydberg Formula: An equation used to predict the wavelengths of all spectral lines of hydrogen.