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chapter 4 vocab for
definitions
Question | Answer |
---|---|
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 |
Frequency | the number of waves that pass a given point in a specific time, usually one second. |
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. |