Properties of Light and Quantum Mechanics

Flashcards covering essential vocabulary from the topics of light properties, quantum mechanics, electron configurations, and chemical bonding.

Electromagnetic spectrum

Range of all types of electromagnetic radiation.

Wave property of light

Describes light behavior as waves, including interference and diffraction.

Double-slit experiment

Demonstrates the wave nature of light through interference patterns.

c = νλ

In this formula, c represents the speed of light, ν is the frequency, and λ is the wavelength.

Particle property of light

Refers to the behavior of light as particles called photons.

Quantization of light energy

Energy of light is quantized and can only exist in discrete amounts.

Photoelectric effect

Phenomenon where light causes the emission of electrons from a material.

E=hf

Energy of a photon is equal to Planck's constant (h) multiplied by its frequency (f).

Line spectrum of the H-atom

Spectrum consisting of discrete line emissions corresponding to electron transitions.

Bohr model

Model of the atom that describes electron orbits around the nucleus.

Ground state

Lowest energy state of an atom.

Excited state

Higher energy state of an atom when an electron absorbs energy.

De Broglie relation

Wavelength of a particle is inversely proportional to its momentum.

Wave property of matter

Describes particles as waves, explaining electron behavior in atoms.

Orbitals (ψ)

Mathematical functions that describe the wave-like behavior of electrons in an atom.

Born interpretation

States that the square of the wave function gives the probability density of finding an electron.

Quantum numbers

Set of values that describe the energies and positions of electrons in atoms.

Aufbau principle

Electrons fill orbitals in order of increasing energy.

Pauli Exclusion Principle

No two electrons in an atom can have the same set of quantum numbers.

Hund’s rule

Electrons will fill degenerate orbitals singly before pairing up.

Electron configuration of ions

Arrangement of electrons in an ion's atomic orbitals.

Atomic radius

Distance from the nucleus to the outermost electron shell.

Ionization energy

Energy required to remove an electron from an atom.

Electron affinity

Energy change that occurs when an electron is added to a neutral atom.

Electronegativity

Measure of the ability of an atom to attract electrons in a bond.

Lewis structures

Diagrams that represent the bonding between atoms of a molecule and the lone pairs of electrons.

Bond order

Number of shared electron pairs between two atoms.

Resonance

Concept where a molecule can be represented by two or more valid Lewis structures.

Polar covalent bonds

Bonds with unequal sharing of electrons due to differences in electronegativity.