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 | reflect IR light and transmit visible. |
Velocity of a wave | distance traversed by a periodic, or cyclic, motion per unit time (in any direction). |
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 | is a physical constant reflecting the sizes of quanta in quantum mechanics. |
Photon | a particle of electromagnetic radiation that has zero rest mass and carries a quantum of energy. |
Energy of a Photon | symbolized by hv. |
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 shines through a prism. |
continuous spectrum | the emission of a continuous range of frequencies of electromagnetic radiation. |
Bohr radius | the radius of the ground state orbit of the hydrogen atom in the bohr theory. |
Interference | in physics the superpostion of two or more waves resulting in a new wave pattern. |
Heisenberg Uncertainty Principle | it is impossible to determine simultaneously both the position and velocity of an electron or any other particle. |
Quantum Theory | a mathematical description of the wave properties of electrons and other very small particles. |
Quantum Mechanics | a mathematical description of the wave properties of electrons and other very small particles. |
Orbital | a threedimensional 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 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, + ½ and |
Aufban Principle | an electron occupies the lowest |
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 in 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 |
Highest occupied level | the electron containing main energy lecel 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 suborbital | is the lowest energy. |
p sublevel or suborbital | middle level |
f sublevel or suborbital | highst energy level |