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Chem Ch. 5

Electromagnetic Radiation A form of energy exhibiting wavelike behavior as it travels through space; can be described by wavelength, frequency, amplitude, and speed and includes visible light, microwaves, X rays, and radio waves.
Wavelength Distance between points on two consecutive waves.
Frequency The number of waves that hit this point in one second.
Amplitude The intensity of a wave.
Electromagnetic Spectrum Includes all forms of electromagnetic radiation,with the only differences between the types of radiation being their frequencies and wavelengths.
Quantum The minimum amount of energy (in Joules) that can be gained or lost by an atom.
Planck’s Constant h = 6.63 x 10-34 J*s
Photoelectric Effect A phenomenon in which photo electrons are emitted from a metal's surface when light of a certain frequency shines on the surface.
Photon A particle of electromagnetic radiation with no mass that carries a quantum of energy.
Atomic Emission Spectrum A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors.
Ground State Electrons in their lowest allowable energy levels are in ther _____________.
De Broglie Equation The velocity of a mass, mv, is a particle property, whereas lambda is a wave property or lambda=h/mv.
Heisenberg Uncertainty Principle States that it is not possible to know precisely both the velocity and the position of a particle at the same time.
Quantum Mechanical Model of the Atom An atomic model in which electrons are treated as waves.
Atomic Orbitals A three-dimensional region around the nucleus of an atom that describes an electron's probable location.
Principal Quantum Number Number which the quantum mechanical model assigns to indicate the relative sizes and energies of atomic orbitals.
Principal Energy Levels The major energy levels of an atom.
Energy Sublevels The energy levels contained within a principal energy level.
Electron Configuration The arrangements of electrons in the atom.
Aufbau Principle States that electrons fill up the lowest energies possible first.
Pauli Exclusion Principle States that a maximum of two electrons may occupy a single orbital, but only if the electrons have opposite spins.
Hund’s Rule States that for sublevels with multiple orbitals, an electron with the same spin occupies each orbital before a 2nd electron with the opposite spin enters each orbital.
Valence Electrons The electrons in an atom's outermost orbitals.
Electron Dot Structure Consists of an elements symbol, representing the atomic nucleus and inner-level electrons, that is surrounded by dots, representing the atom's valence electrons.
Created by: monopoly10



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