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Lesson 1
LIGHT AND QUANTIZED ENERGY
• electromagnetic radiation
• wavelength
• frequency
• amplitude
• electromagnetic spectrum
• quantum
• Planck’s constant
• photoelectric effect
• photon
• atomic emission spectrum
• All waves are defined by their wavelengths, frequencies,
amplitudes, and speeds.
c
= λν
• In a vacuum, all electromagnetic waves travel at the speed of light.
• All electromagnetic waves have both wave and particle properties.
• Matter emits and absorbs energy in quanta.
E
quantum
=
h
ν
• White light produces a continuous spectrum. An element’s
emission spectrum consists of a series of lines of individual colors.
Lesson 2
QUANTUM THEORY AND THE ATOM
• ground state
• quantum number
• de Broglie equation
• Heisenberg uncertainty principle
• quantum mechanical model of
the atom
• atomic orbital
• principal quantum number
• principal energy level
• energy sublevel
• Bohr’s atomic model attributes hydrogen’s emission spectrum to
electrons dropping from higher-energy to lower-energy orbits.
∆
E
=
E
higher-energy orbit
-
E
lower-energy orbit
=
E
photon
=
h
ν
• The de Broglie equation relates a particle’s wavelength to its mass,
its velocity, and Planck’s constant.
λ =
h
/
m
ν
• The quantum mechanical model assumes that electrons have
wave properties.
• Electrons occupy three-dimensional regions of space called
atomic orbitals.
Lesson 3
ELECTRON CONFIGURATION
• electron configuration
• aufbau principle
• Pauli exclusion principle
• Hund’s rule
• valence electron
• electron-dot structure
• The arrangement of electrons in an atom is called the atom’s
electron configuration.
• Electron configurations are defined by the aufbau principle, the
Pauli exclusion principle, and Hund’s rule.
• An element’s valence electrons determine the chemical properties
of the element.
• Electron configurations can be represented using orbital diagrams,
electron configuration notation, and electron-dot structures.
MODULE 4
STUDY GUIDE
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Module 4 • Study Guide