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vocab for atoms
| 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 |
Created by:
EllieKennamer
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