Unit 1: Quantum Mechanics, Spectral Series, and Quantum Numbers

Vocabulary practice flashcards defining key atomic models, spectral series, equations, and quantum numbers discussed in the lecture.

Bohr model

A simplified model of the atom explaining that electrons exist at discrete, quantized energy levels ($n = 1, 2, 3$) and are not found in between.

Emission spectrum

The unique pattern of discrete wavelengths of light emitted when an atom of a specific element is energized.

Absorption

The process where an electron absorbs an incoming photon whose energy corresponds exactly to an energy gap to move up to a higher energy level.

Emission

The process where an electron falls down to a lower energy level, releasing a photon with a wavelength corresponding exactly to that energy gap.

Balmer series

A series of spectral emission lines for the hydrogen atom that occur when an excited electron falls back down to the $n = 2$ energy level.

Lyman series

A series of spectral emission lines in the ultraviolet region resulting from electron transitions that fall down to the $n = 1$ energy level.

Paschen series

A series of spectral emission lines in the infrared region resulting from electron transitions that fall down to the $n = 3$ energy level.

Rydberg equation

A mathematical formula used to calculate the energy, frequency, or wavelength of light emitted or absorbed during electron transitions between any two integer energy levels in a hydrogen atom.

De Broglie equation

An equation showing wave-particle duality by relating the wavelength of matter to Planck's constant divided by the mass and velocity of the object.

Atomic orbitals

Three-dimensional regions around a single nucleus where electron density is most likely to be located, derived as solutions to Schrödinger's equations.

Principal quantum number ($n$)

The quantum number representing the shell and average distance of an electron from the nucleus, which can only be a positive integer ($n = 1, 2, 3, \text{etc.}$).

Angular momentum quantum number ($l$)

The quantum number representing the subshell and the specific spatial shape of an atomic orbital, ranging in values from $0$ up to $n - 1$.

Magnetic quantum number ($m_l$)

The quantum number that designates the specific orbital orientation within a subshell.

Spin quantum number ($m_s$)

The quantum number describing the intrinsic angular momentum of an electron within an orbital, corresponding to spin up or spin down.