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 | a kind of electromagnetic radiation |
Velocity of a wave | the velocity at which the crests of a wave move. |
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 | emission of an electron from a metal when light shines on the metal |
Photon | a particle of electromagnetic radiation that has zero rest mass and carries a quantum of energy |
Energy of a Photon | depends on the frequency of 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 its 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 | the radius of the n=1 orbital in hydrogen. .529exp(-10) m |
Interference | when waves overlap |
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 | 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 | numbers that specify 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 recieve 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 eighteen electrons |
s sublevel or sub-orbital | empty orbital of the lowest energy |
p sublevel or sub-orbital | next available vacant orbitals |
f sublevel or sub-orbital | filled in the 6th and 7th period |