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chapter 4 chem vocab
vocab
| Question | Answer |
|---|---|
| Electromagnetic radiation | A form of energy that exhibits wavelike behavior as it travels through space |
| Electromagnetic spectrum | All forms of electromagnetic radiation |
| Wavelength | The distance between corresponding points on adjacent waves |
| Frequency | The number of waves that pass a specific point in a certain amount of time |
| Visible Light | Electromagnetic radiation that can produce a visual image that can be seen with the naked eye |
| Velocity of a wave | Measure of the rate of change of a wave |
| Photoelectric effect | The emission of an electron from a metal when light shines on the metal |
| quantum | The minimum amount of energy that can be lost or gained by an atom |
| Planck’s Constant | This relates the energy of a photon to the frequency of that photon. Its value is approximately 6.626 × 10 -34 joule-seconds |
| Photon | A particle of electromagnetic radiation that has zero rest mass and carries a quantum of energy |
| Energy of a Photon | The capability to transfer heat to a photon |
| Ground State | Lowest energy state of an atom |
| Excited State | A state where an atom has a higher potential energy than it has in its ground state |
| Line-emission spectrum | A series of specified wavelenghts of emitted light is separated into a series of specific frequencies of visible light |
| continuous spectrum | Emission of a continuous range of frequencies of electromagnetic radiation |
| Bohr radius | The radius of the n=1 orbital in hydrogen |
| Interference | Waves overlap which causes a reduction of energy in some areas and an increase in others |
| Heisenberg Uncertainty Principle | States it is impossible to determine the position and velocity of an electron or other particle |
| Quantum Theory or Quantum Mechanics (same definition for both of these so list them together) | Describes wave properties of electrons and other particles |
| Orbital | 3-D region around the nucleus and the probable place of an electron |
| Quantum numbers | specify the properties of atomic orbitals and the properties of electrons in orbitals |
| Principle Quantum number (n) | Indicates the main energy level occupied by electrons |
| Angular momentum quantum number (l ) | Indicates shape of the orbital |
| Magnetic quantum number (m) | Indicates the orientation of an orbital around the nucleus |
| Spin quantum number (s) | Indicates the two fundamental spin states of an electron in a orbital |
| Aufban Principle | An electron occupies the lowest energy orbital that can receive it |
| Electron Configuration | 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 orbitals must have the same spin |
| Valence Electron | the electrons of an atom that can participate in the formation of chemical bonds with other atoms |
| Inner-shell electrons | Electrons that are not in the highest energy level |
| Highest occupied level | The electron containing main energy level with the highest principal quantum number |
| Noble Gas Configuration | Outer main energy level fully occupied in most cases by 8 electrons |
| s sublevel or sub-orbital | A spherically symmetrical atomic orbital |
| p sublevel or sub-orbital | The orbital of an atomic electron with an orbital angular momentum quantum number of unity |
| f sublevel or sub-orbital | corresponds to an electron orbital with angle momentum quantum number l = 3. |
Created by:
j.millsdar4
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