Chapter 6: Electronic Structure of Atoms

Flashcards covering key vocabulary and concepts from the lecture notes on electronic structure of atoms.

Electronic Structure

The arrangement and energy of electrons within an atom.

Electromagnetic Radiation

Moves as waves through space at the speed of light.

Wavelength

The distance between corresponding points on adjacent waves.

Frequency (ν)

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

Speed of Light (c)

The speed at which all electromagnetic radiation travels.

Blackbody Radiation

The emission of light from hot objects.

Photoelectric Effect

The emission of electrons from metal surfaces when light is shone on them.

Quanta

The packets in which energy comes, according to Max Planck.

Atomic Emissions Spectra

The spectra observed from energy emitted by atoms and molecules.

Line Spectrum

A spectrum of discrete wavelengths observed for atoms and molecules.

Bohr Model

Stated that only orbits of certain radii, corresponding to specific energies, are permitted for the electron in a hydrogen atom.

Ground State

The lowest energy state for an electron.

Excited State

Any energy state higher than the ground state.

Wave Nature of Matter

If light can have material properties, matter should exhibit wave properties.

Uncertainty Principle

The more precisely the momentum of a particle is known, the less precisely its position is known.

Quantum Mechanics

Mathematical treatment into which both wave and particle nature of matter could be incorporated.

Electron Density

The square of the wave function, representing the probability of finding an electron at a given time.

Orbital

Describes a spatial distribution of electron density.

Principal Quantum Number (n)

Describes the energy level on which the orbital resides.

Angular Momentum Quantum Number (l)

Defines the shape of the orbital.

Magnetic Quantum Number (ml)

Describes the three-dimensional orientation of the orbital.

Electron Shell

Orbitals with the same value of n.

Subshells

Different orbital types within a shell.

Spin Quantum Number (ms)

The "spin" of an electron which describes its magnetic field.

Pauli Exclusion Principle

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

Electron Configuration

The way electrons are distributed in an atom.

Ground State (electron configuration context)

The most stable electron configuration; has the lowest possible energy.

Hund’s Rule

When filling degenerate orbitals, the lowest energy is attained when the number of electrons having the same spin is maximized.

Valence Electrons

Electrons in the outermost shell.

Core Electrons

Filled inner shell electrons.

Lanthanide Elements

Elements with electrons entering the 4f sublevel.

Actinide Elements

Elements with electrons entering the 5f sublevel.

Main-Group Elements

Elements in the s and p blocks of the periodic table.