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chapter 4 vocab for


Electromagnetic radiation a form of energy that exhibits wavelike behavior as it travels through space.
Electromagnetic spectrum all the forms of electromagnetic radiation.
Wavelength the distance between corresponding points on adjacent waves
Visible Light light that can be saw by the naked eye.
Velocity of a wave the speed at which a wave travels
photoelectric effect the emission of electrons from a metal when light shines on the metal
quantum the minimum quantity of energy that can be gained or lost by an atom.
Planck’s Constant h
Photon a particle of electromagnetic radiation that has zero rest mass and carries a quantum of energy.
Energy of a Photon (Ephoton
Ground State the lowest energy state of an atom
Excited State a state in which an atom has a higher potential energy than it has in its ground state.
Line-emission spectrum a series of specific wavelengths of emitted light created when the visible portion of the light from excited atoms is shined through a prism.
continuous spectrum the emission of a continuous range of frequencies of electromagnetic radiation.
Bohr radius the radius of the n
Interference when waves overlap resulting 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 particles.
Quantum Theory or Quantum Mechanics (same definition for both of these so list them together) a mathematical description of the wave properties of electrons and other very small particles.
Orbital a three-dimensional region around the nucleus that indicates the probable location of an electron.
Quantum numbers a number that specifies the properties of atomic orbitals and the properties of electrons in orbitals.
Principle Quantum number (n) the quantum number that indicates the main energy level occupied by the electron.
Angular momentum quantum number (l ) the quantum number that indicates the shape of thew orbital.
Magnetic quantum number (m) the quantum number that indicates the orientation of an orbital around the nucleus.
Spin quantum number (s) the quantum number that has only two possible values, +1/2 and -1/2, which indicate the two fundamental spin states of an electron in an orbital.
Aufban Principle an electron occupies the lowest-energy orbital that can receive it.
Electron Configuration the 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 an electron that is available to be lost,gained,or shared in the formation of chemical compounds.
Inner-shell electrons an electron that is not in the highest occupied energy level.
Highest occupied level the electron-containing main energy level with the highest principal quantum number.
Noble Gas Configuration an outer main energy level fully occupied, in most cases,by eight electrons.
s sublevel or sub-orbital 1st energy level contains 2 electrons
p sublevel or sub-orbital 2nd energy level contains 6 electrons.
f sublevel or sub-orbital 4th energy level contains 14 electrons.
Created by: charliewalker