Chapter 6: Electronic Structure of Atoms

These flashcards cover key concepts related to the electronic structure of atoms, including the wave and particle nature of light, quantum mechanics, and electron configuration.

Wave Nature of Light

Refers to the wavelike characteristics of electromagnetic radiation.

Wavelength (λ)

Distance between corresponding points on adjacent waves.

Frequency (ν)

The number of complete waves passing a given point per unit of time.

Electromagnetic Spectrum

Types of electromagnetic radiation arranged by wavelength.

Speed of Light (c)

Velocity at which all electromagnetic radiation travels, approximately 3.00 × 10^8 m/s.

Max Planck

Introduced the concept that energy is absorbed or released in discrete packets called quanta.

Photon

A packet of energy that carries electromagnetic radiation.

Photoelectric Effect

Phenomenon where photons transfer their energy to electrons in a metal.

Line Spectrum

A spectrum that consists of discrete wavelengths emitted by gases.

Bohr’s Model of the Atom

Describes electrons as occupying orbits of fixed radii with specific energies.

Ground State

The lowest energy state of an atom.

Excited State

Higher-energy states of an atom where electrons occupy orbits further from the nucleus.

Quantum Mechanics

A branch of physics describing the wave and particle nature of matter.

Quantum Numbers

Set of numbers that describe the unique quantum state of an electron in an atom.

Principal Quantum Number (n)

Indicates the energy level of an electron in an atom.

Angular Momentum Quantum Number (l)

Describes the shape of the electron's orbital.

Magnetic Quantum Number (ml)

Describes the 3-D orientation of an orbital.

Pauli Exclusion Principle

States that no two electrons in the same atom can have the same set of quantum numbers.

Hund’s Rule

Lowest energy is attained when the number of electrons with the same spin is maximized.

Condensed Electron Configuration

Representation of an atom's electron configuration using the nearest noble gas.