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jade ch 4 vocab
| Question | Answer |
|---|---|
| Visible Light | one type of electromagnetic radiation that moves at a constant speed |
| *Velocity of a wave | |
| photoelectric effect | emission of electrons from a metal when a light shines in the metal |
| quantum | the minimum quantity of energy that can be gained or lost by an atom |
| *Planck’s Constant | the constant of proportionality relating the energy of a photon to its frequency |
| Photon | particle of electromagnetic radiation that has zero rest mass and carries a quantum of energy |
| *Energy of a Photon | |
| Ground State | lowest energy state of an atom |
| Excited State | state where an atom has a higher potential energy than it has in its ground state |
| Line | emission spectrum |
| continuous spectrum | emission of a continuous range of frequencies of electromagnetic radiation |
| Bohr radius | the radius of the n=1 orbital in hydrogen |
| *Interference | |
| Heisenberg Uncertainty Principle | in is impossible to determine simultaneously to both the position and vilocity of an electron or any other particle |
| Quantum Theory or Quantum Mechanics (same definition for both of these so list them together) | mathmatical description of the wave properties of electrons and other very small particles |
| Orbital | 3 |
| Quantum numbers | a number that specifies the properties of atomic orbitals and the properties of electrons in orbitals |
| Principle Quantum number (n) | quantum number that indicates the main energy level occupied by the electron |
| Angular momentum quantum number (l ) | quantum number that indicates the shape of the orbital |
| Magnetic quantum number (m) | quantum number that indicates the orientation of an orbital around the nucleus |
| Spin quantum number (s) | quantum number that has only 2 values, which indicate the 2 fundamental spin states of an electron in an orbital |
| Aufban Principle | an electron occupies the lowest energy orbital that can recieve it |
| Electron Configuration | arrangement of electrons in an atom |
| Pauli Exclusion Principle | No two electrons in the same atom may have identical sets 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 | electron that is avalible to be lost gained or shared in the formation of chemical compounds |
| Inner | shell electrons |
| Highest occupied level | 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 8 electrons |
| s sublevel or sub | orbital |
| *p sublevel or sub | orbital |
| *f sublevel or sub | orbital |
| orbital | |
| Electromagnetic radiation | form of energy that exhibits wavelike behavior as it travels through space |
| Electromagnetic spectrum | all the forms of electromagnetic radiation |
| Wavelength | distance between corresponding points on adjacent waves |
| Frequency | number of waves that pass a given point in a specific time normally one second |
| Wavelength | distance between corresponding points on adjacent waves |
| Frequency | number of waves that pass a given point in a specific time normally one second |
Created by:
mahalie.jade
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