Question | Answer |
Electromagnetic radiation | A form of energy that exhibits wavelike behavior as it travels through space |
Electromagnetic spectrum | All forms of electromagnetic radiation |
Wavelength | The distance between corresponding points on adjacent waves |
Frequency | The number of waves that pass a specific point in a certain amount of time |
Visible Light | Electromagnetic radiation that can produce a visual image that can be seen with the naked eye |
Velocity of a wave | Measure of the rate of change of a wave |
Photoelectric effect | The emission of an electron from a metal when light shines on the metal |
quantum | The minimum amount of energy that can be lost or gained by an atom |
Planck’s Constant | This relates the energy of a photon to the frequency of that photon. Its value is approximately 6.626 × 10 -34 joule-seconds |
Photon | A particle of electromagnetic radiation that has zero rest mass and carries a quantum of energy |
Energy of a Photon | The capability to transfer heat to a photon |
Ground State | Lowest energy state of an atom |
Excited State | A state where an atom has a higher potential energy than it has in its ground state |
Line-emission spectrum | A series of specified wavelenghts of emitted light is separated into a series of specific frequencies of visible light |
continuous spectrum | Emission of a continuous range of frequencies of electromagnetic radiation |
Bohr radius | The radius of the n=1 orbital in hydrogen |
Interference | Waves overlap which causes a reduction of energy in some areas and an increase in others |
Heisenberg Uncertainty Principle | States it is impossible to determine the position and velocity of an electron or other particle |
Quantum Theory or Quantum Mechanics (same definition for both of these so list them together) | Describes wave properties of electrons and other particles |
Orbital | 3-D region around the nucleus and the probable place of an electron |
Quantum numbers | specify the properties of atomic orbitals and the properties of electrons in orbitals |
Principle Quantum number (n) | Indicates the main energy level occupied by electrons |
Angular momentum quantum number (l ) | Indicates shape of the orbital |
Magnetic quantum number (m) | Indicates the orientation of an orbital around the nucleus |
Spin quantum number (s) | Indicates the two fundamental spin states of an electron in a orbital |
Aufban Principle | An electron occupies the lowest energy orbital that can receive it |
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 orbitals must have the same spin |
Valence Electron | the electrons of an atom that can participate in the formation of chemical bonds with other atoms |
Inner-shell electrons | Electrons that are not in the highest energy level |
Highest occupied level | The electron containing main energy level with the highest principal quantum number |
Noble Gas Configuration | Outer main energy level fully occupied in most cases by 8 electrons |
s sublevel or sub-orbital | A spherically symmetrical atomic orbital |
p sublevel or sub-orbital | The orbital of an atomic electron with an orbital angular momentum quantum number of unity |
f sublevel or sub-orbital | corresponds to an electron orbital with angle momentum quantum number l = 3. |