Chapter 4: Light & Electron Structure

Flashcards covering key concepts related to the structure of light and electrons based on the lecture notes.

Electromagnetic Radiation

A form of energy that travels in waves, produced when charged particles move or vibrate relative to each other.

Photon

A packet of light, existing in small increments.

Electromagnetic Spectrum

The broad continuum of electromagnetic energy, ranging from low-energy waves (TV and radio) to high-energy waves (X-rays and gamma rays).

Wavelength (λ)

The distance between two repeating points in a wave.

Frequency (ν)

The number of waves that pass through a point in one second, measured in hertz (Hz).

Ground State

The state of an atom when its electrons are in the lowest possible energy levels.

Excited State

The state of an atom when its electrons have jumped to higher energy levels.

Energy Levels

The allowed energies that electrons can have in an atom.

Bohr Model

A theory proposed by Niels Bohr that describes electrons orbiting the nucleus in defined energy levels.

Quantum Model

A more nuanced description of electron behavior, focusing on the probability locations of electrons.

Sublevel

Different energy levels found within a principal energy level, designated by letters s, p, d, and f.

Orbital

The region around the nucleus where electrons are most likely to be found.

Valence Electrons

Electrons in the outermost occupied energy level that play a key role in chemical bonding.

Octet Rule

The principle stating that atoms are stabilized by having eight electrons in their valence shell.

Noble Gas Notation

A shorthand way of writing electron configurations by using the nearest noble gas configuration.

Isoelectronic

Atoms or ions that have the same electron configuration.

Hund’s Rule

The principle that electrons will singly occupy orbitals of the same energy before pairing up.

Line Spectrum

A spectrum showing distinct lines of color, unique to the elements producing them.

Energy Sublevels

The divisions of principal energy levels, each containing a specific number of orbitals.

Spin

The property of electrons that gives them a tiny magnetic field.

Core Electrons

Inner electrons that are not involved in bonding.

Chemical Bonding

The interaction between outer electrons of different atoms that allows them to combine.