Atomic Structure & Electromagnetic Energy

Vocabulary flashcards covering atomic models, electron behavior, and electromagnetic energy relationships discussed in the lecture notes.

Wave-Mechanical (Quantum) Model

Currently accepted atomic model where electrons occupy probability clouds (orbitals) rather than fixed paths.

Valence Electrons

Electrons in an atom’s outermost orbitals that control chemical reactivity because they are accessible to other atoms.

Core Electrons

Inner electrons held close to the nucleus; they generally do not participate in reactions because other atoms cannot easily reach them.

Bohr Model

Early atomic model with fixed circular orbits; accurately describes hydrogen due to its single electron but fails for multi-electron atoms.

Energy Level (Orbit)

Discrete distance from the nucleus where an electron can reside; higher numbers mean the electron is farther from the nucleus and has more energy.

Electron Transition (Toward Nucleus)

Movement to a lower energy level; electron loses energy and emits a photon of light.

Electron Transition (Away From Nucleus)

Movement to a higher energy level; electron absorbs energy to move farther from the nucleus.

Photon

Packet of electromagnetic energy released or absorbed when an electron changes energy levels.

Wavelength–Frequency Relationship

Wavelength and frequency are inversely proportional; longer wavelength equals lower frequency.

Frequency–Energy Relationship

Frequency and energy are directly proportional; higher frequency equals higher photon energy.

Electromagnetic Spectrum (Increasing Wavelength)

Gamma rays, X-rays, UV light, visible light, IR light, microwaves, radio waves.

Visible Spectrum Order

Violet, blue, green, yellow, orange, red as wavelength increases.

Red Light Wavelength

Approximately 625–700 nm within the visible spectrum.

Orange Light Wavelength

Approximately 575–625 nm within the visible spectrum.

Violet Light Wavelength

Approximately 400–425 nm within the visible spectrum.