Hydrogen Emission Spectrum and Atomic Structure

Vocabulary flashcards covering the concepts of continuous vs. line spectra, electron energy level transitions, Bohr's model of the atom, and the specific transitions of the hydrogen emission spectrum.

Continuous Spectrum

A spectrum that shows all of the frequencies of light in the visible part of the spectrum, such as white light from a light bulb passed through a prism.

Line Spectrum

A spectrum that shows only specific frequencies of light, appearing as isolated lines of color rather than a continuous rainbow.

Hydrogen Emission Spectrum

The line spectrum produced when a gas lamp of hydrogen is excited by energy (such as electricity or heat), emitting light at specific frequencies.

Ground State

The lowest energy level or most stable state of an atom, where an electron resides prior to absorbing energy ($n = 1$ for a hydrogen atom).

Excited State

The state of an electron after it absorbs a specific frequency of energy corresponding exactly to the difference between energy levels and jumps to a higher level.

Red Line Transition (Hydrogen Spectrum)

The visible transition of lowest energy and frequency, produced when an electron drops from the third energy level ($n = 3$) to the second energy level ($n = 2$).

Green Line Transition (Hydrogen Spectrum)

The visible emission line representing an electron transition dropping from the fourth energy level ($n = 4$) to the second energy level ($n = 2$).

Blue Line Transition (Hydrogen Spectrum)

The visible emission line representing an electron transition dropping from the fifth energy level ($n = 5$) to the second energy level ($n = 2$).

Violet Line Transition (Hydrogen Spectrum)

The visible emission line of highest energy and frequency, produced when an electron drops from the sixth energy level ($n = 6$) to the second energy level ($n = 2$).

Visible Spectrum Transitions (Hydrogen)

Spectral lines in the visible region caused specifically by excited electrons dropping from higher energy levels down to the second energy level ($n = 2$).

Ultraviolet (UV) Transitions (Hydrogen)

High-energy spectral emissions caused by excited electrons dropping down to the first energy level ($n = 1$), which are invisible to the human eye.

Infrared Transitions (Hydrogen)

Low-energy spectral emissions caused by excited electrons dropping down to the third energy level ($n = 3$), which are invisible to the human eye.

Energy Level Convergence

The phenomenon where energy levels in an atom get closer together as you move outward from the nucleus, evidenced by spectral lines converging at higher energies.