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TEParrangedatoms
| 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 |
Created by:
Tessa Elise
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