CH301/CH302: Atomic Structure, Periodic Table, and Quantum Mechanics

Vocabulary flashcards covering health resources and core atomic theory, periodic table concepts, and quantum mechanics topics from the notes.

Emission Spectra

Light emitted by excited atoms resulting in a line spectrum.

Rydberg Equation

Formula for hydrogen line wavelengths: 1/λ = R_H(1/n1^2 − 1/n2^2).

Bohr Model

Electrons orbit the nucleus in fixed, quantized energy levels.

Rutherford Model

Atom mostly empty space with a dense nucleus; positive charge in center.

Plum Pudding Model

Thomson’s model: electrons embedded in a positively charged sphere.

Dalton’s Atomic Theory

Atoms are indivisible; atoms of an element are identical; compounds form from atoms.

Nucleus

Dense center of the atom containing protons and neutrons.

Proton

Positively charged subatomic particle in the nucleus.

Electron

Negatively charged subatomic particle orbiting the nucleus.

Neutron

Electrically neutral subatomic particle in the nucleus.

Wave–Particle Duality

Idea that particles exhibit both wave-like and particle-like properties.

De Broglie Wavelength

Wavelength associated with a moving particle: λ = h/(mv).

Planck Constant (h)

Constant relating energy and frequency; h ≈ 6.626 × 10^−34 J·s.

λ = h/(mv)

De Broglie equation giving the wavelength of a moving particle.

Schrödinger Equation

Wave equation for nonrelativistic quantum mechanics; yields orbitals.

Wave Function ψ

Mathematical function whose square gives the probability density of finding an electron.

Orbitals

Regions in space with high probability of finding an electron; shapes defined by quantum numbers.

Probability Density ψ^2

Square of the wave function representing probability per unit volume.

Uncertainty Principle (Heisenberg)

Δx · Δp ≥ h/(4π); limits on simultaneous measurements of position and momentum.