Quantum Model, Electron Configurations, Light, Spectroscopy, Coffee Lab, and PES

Vocabulary practice flashcards covering quantum mechanics, atomic structure, electron configurations, light principles, spectroscopic techniques, standard curves, and photoelectron spectroscopy.

Bohr Model

An atomic model that places electrons in defined circular orbits with specific quantized energies around the nucleus.

Quantum Mechanical Model

An atomic model that describes regions of high probability for finding an electron, known as orbitals, rather than exact physical paths.

Blackbody Radiation

A physical phenomenon demonstrating that energy is emitted in discrete amounts rather than any arbitrary continuous amount.

Photoelectric Effect

The ejection of electrons from a material when light with a frequency above a specific threshold strikes it.

Atomic Emission Spectra

Characteristic patterns of specific light wavelengths emitted by atoms, revealing discrete electron energy states.

Orbital

A region of space where there is a high probability of finding an electron, holding a maximum of two electrons with opposite spins.

Sublevel

A group of equal-energy orbitals of the same type ($s$, $p$, $d$, or $f$) within a principal energy level.

Principal Energy Level

A major electron energy shell represented by the principal quantum number $n = 1, 2, 3\text{...}$, with higher levels generally farther from the nucleus and higher in energy.

$s$ Sublevel

A spherical sublevel consisting of 1 orbital that holds a maximum of 2 electrons.

$p$ Sublevel

A dumbbell-shaped sublevel consisting of 3 orbitals that holds a maximum of 6 electrons.

$d$ Sublevel

A complex-shaped sublevel consisting of 5 orbitals that holds a maximum of 10 electrons.

$f$ Sublevel

A complex-shaped sublevel consisting of 7 orbitals that holds a maximum of 14 electrons.

Noble-Gas Configuration

A shorthand electron configuration that replaces the inner completed electron shell with the bracketed symbol of the preceding noble gas.

Hund's Rule

The rule stating that electrons occupy equal-energy orbitals singly with parallel spins before any orbital receives a second electron.

Aufbau Principle

The rule stating that electrons occupy the available orbitals of lowest energy first before filling higher-energy orbitals.

Principal Quantum Number ($n$)

The quantum number that indicates the principal energy level or major electron shell ($n = 1, 2, 3\text{...}$).

Angular Momentum Quantum Number ($l$)

The quantum number that identifies the sublevel type, defined as $s=0$, $p=1$, $d=2$, and $f=3$.

Magnetic Quantum Number ($m_l$)

The quantum number that designates a specific orbital within a sublevel, ranging from $-l$ through $+l$.

Electron Spin Quantum Number ($m_s$)

The quantum number that describes the spin orientation of an electron, taking values of $+\frac{1}{2}$ or $-\frac{1}{2}$.

Heisenberg Uncertainty Principle

The fundamental limit stating that it is impossible to simultaneously measure both the exact position and exact momentum of an electron.

Wave-Particle Theory of Light

The model stating that light exhibits both wave characteristics (wavelength, frequency) and particle characteristics (photons).

Amplitude

The height of a wave measured from its equilibrium position, which corresponds to the wave's intensity.

Frequency ($ u$)

The number of wave cycles that pass a given point per second, measured in hertz ($\text{Hz}$ or $\text{s}^{-1}$).

Wavelength ($rac{}{} ext{lambda}$ or $ u$)

The distance between equivalent points on consecutive waves, typically expressed in meters ($\text{m}$).

Speed of Light ($c$)

The physical constant representing the speed of light in a vacuum, equal to $3.00 \times 10^8\text{ m/s}$.

Planck's Constant ($h$)

The proportionality constant relating photon energy to frequency, equal to $6.626 \times 10^{-34}\text{ J}\text{s}$.

Electromagnetic Spectrum

The full range of electromagnetic radiation ordered from longest wavelength to shortest: radio, microwave, infrared, visible, ultraviolet, X-ray, and gamma ray.

Photon

A discrete packet or particle of electromagnetic radiation carrying energy equal to $E = h \times \text{frequency}$.

Quantum

The minimum discrete amount or packet of energy that can be absorbed or emitted by an atom.

Valence Electron

An electron located in the outermost occupied principal energy level of an atom that participates in chemical bonding.

Octet Rule

The tendency of main-group atoms to gain, lose, or share electrons to achieve a full outer shell of 8 valence electrons.

Continuous Spectrum

A spectrum that displays an uninterrupted continuum of all wavelengths across a given range.

Emission Spectrum

A spectrum composed of discrete bright lines at specific wavelengths emitted when excited electrons transition to lower energy levels.

Absorption Spectrum

A continuous spectrum containing dark lines caused by the absorption of specific light wavelengths as electrons transition to higher energy levels.

Standard Curve

A reference graph plotting known concentrations against measured responses used to calculate unknown sample concentrations using $x = \frac{y - b}{m}$.

Photoelectron Spectroscopy (PES)

An experimental technique that utilizes the photoelectric effect to determine electron binding energies and deduce electron configurations.

Binding Energy Peak

A peak in a photoelectron spectrum whose position indicates electron binding energy and whose area corresponds to the relative number of electrons in that sublevel.