Emission spectra show bright lines at specific wavelengths when atoms emit photons. Absorption spectra show dark lines at specific wavelengths where atoms absorb photons.

Ground state: lowest energy level, highest binding energy. Excited states: higher energy levels, lower binding energy.

High-frequency photons have higher energy; low-frequency photons have lower energy. $E = hf$.

High-frequency photons have shorter wavelengths; low-frequency photons have longer wavelengths. $\lambda = \frac{c}{f}$.

Ground state electrons have higher binding energy, while excited state electrons have lower binding energy.

A photon is a discrete packet of light energy.

The minimum energy required to remove an electron from an atom.

The process where an electron is removed from an atom, creating an ion.

The unique set of frequencies of light emitted by an element when its electrons transition to lower energy levels.

The unique set of frequencies of light absorbed by an element when its electrons transition to higher energy levels.

The lowest energy level of an atom.

Emission spectra show bright lines at specific wavelengths emitted by an element. Absorption spectra show dark lines at specific wavelengths absorbed by an element.

Ground state: Highest binding energy, hardest to remove electron. Excited state: Lower binding energy, easier to remove electron.

High frequency photons: Larger energy transitions. Low frequency photons: Smaller energy transitions.

Absorption: Atom gains energy. Emission: Atom loses energy.

Emission spectra: Bright lines on a dark background. Absorption spectra: Dark lines on a continuous spectrum.