Question | Answer |
Electromagnetic radiation-a form of energy that exhibits wavelike behavior as it travels trough 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-Electromagnetic radiation in this range of wavelengths | |
Velocity of a wave- | |
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-a physical constant reflecting the sizes of quanta in quantum mechanics 6.626068 × 10-34 m2 kg / s | |
Photon-a paricles of electromagnetic radiation that has zero rest mass and carries a quantum of energy | |
Energy of a Photon-depends on the frequency or the radiation | |
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 it's ground state | |
Line-emission spectrum-a series of specific wavelengths of emitted light created when the visible portion of light from excited atoms is shined through a prism | |
continuous spectrum-the emission of a continuous range of frequencies of electromagnetic radiation | |
Bohr radius- | |
Interference-The wave properties of light lead to interference, but certain conditions of coherence must be met for these interference effects to be readily visible | |
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 (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 locationof 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 the 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 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 electrons | |
s sublevel or sub-orbital-n=1,in an nth main energy level there are n Sublevels | |
p sublevel or sub-orbital-n=2,,in an nth main energy level there are n Sublevels | |
f sublevel or sub-orbital-n=4,in an nth main energy level there are n Sublevels | |