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Arrangement of Atoms

Electromagnetic Radiation Form of energy that exhibits wavelike behavior as it travels through space
Electromagnetic Spectrum Electromagnetic spectrum
Frequency Number of waves that pass a given point in a specific time, typically one second
Visible Light Spectrum that is used by most organisms to be able to see
Velocity of a Wave Product of wavelength and frequency part of the electromagnetic spectrum that is roughly in the middle
Photoelectric Effect Emission of electrons from a metal when light shines on the metal
Quantum Minimum quantity of energy that can be gained or lost by an atom
Planck’s Constant Fundamental physical constant; h=6.626 × 10-34 J⋅s
Photon Particle of electromagnetic radiation that has zero rest mass and carries a quantum of energy
Energy of a Photon E(photon)=hv
Ground State Lowest energy state of an atom
Excited State State in which an atom has a higher potential energy than it has in its ground state
Line-Emission spectrum Series specific wavelengths of emitted light created when the visible portion of light from excited atoms is shined through a prism
Continuous Spectrum Emission of continuous range of frequencies of electromagnetic radiation
Bohr Radius Radius of the s orbital in hydrogen
Interference Waves overlapping that results in a reduction of energy in some areas and an increase of energy in others
Heisenberg Uncertainty Principle “It is impossible to determine simultaneously both the position and velocity of an electron or any other particle”
Quantum Theory or Quantum Mechanics Mathematical description of the wave properties of electrons and and other very small particles
Orbital Three-dimensional region around the nucleus that indicates the probable location of an electron
Quantum Numbers Number that specifies the properties of atomic orbitals and the properties of electrons in orbitals
Principle Quantum Number (n) Quantum number that indicates the main energy level occupied by the electron
Angular Momentum Quantum Number (l ) Quantum number that indicates the shape of the orbital
Magnetic Quantum Number (m) Quantum number that indicates the orientation of an orbital around the nucleus
Spin Quantum Number (s) Spin quantum number (s)
Electron Configuration Arrangement of electrons in an atom
Pauli Exclusion Principle "No two electrons in the same atom can have the same set of four quantum numbers"
Hund’s Rule Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin
Valence Electron Electron that is available to be lost, gained, or shared in the formation of chemical compounds
Inner-Shell electrons Electron that is not in the highest occupied energy level
Highest Occupied level Electron-containing main energy level with the highest principal quantum number
Noble Gas Configuration Outer main energy level fully occupied, in most cases, by eight electrons
S Sublevel or Sub-Orbita Spherical shaped; only one sublevel is possible per n value
P Sublevel or Sub-Orbital Dumbbell shaped; three sub levels possible per n value (x, y, z axis)
F Sublevel or Sub-orbita More complex shaped; seven sub levels possible per n value
Created by: 30Leigh



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