Chemistry 1-2: chapter 4 vocabulary flashcards
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27 terms
Terms | Definitions |
|---|---|
 Electromagnetic radiation | form of energy that exhibits wavelike behavior as it travels through space. |
| Electromagnetic spectrum | collective term given to all forms of electromagnetic radiation. |
| Wavelength | distance between corresponding points on adjacent waves. |
| Frequency | number of waves that pass through a given point in a specific time (usually one second). |
| Photoelectric effect | effect that refers to the emission of electrons from a metal when light shines on the metal. |
| Quantum | minimum quantity of energy that can be lost or gained by an atom. |
| Photon | particle of electromagnetic radiation having zero mass and carrying a quantum of energy. |
| Ground state | lowest energy state of an atom. |
| Excited state | state in which an atom has a higher potential energy than it has in its ground state |
| line-emission spectrum | bands of light produced when a narrow beam of emitted light shines through a prism, separating the light into a series of specific frequencies. |
| continuous spectrum | emission of a continuous range of frequencies of electromagnetic radiation. |
| Heisenberg uncertainty principle | idea that states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle. |
| Quantum theory | theory that mathematically describes the wave properties of electrons and other very small particles. |
| Orbital | 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. |
| Principal quantum number | a number, symbolized by n, that indicates the main energy level occupied by an electron. |
| Angular momentum quantum number | a number, symbolized by L, that indicates the shape of the orbital. |
| Magnetic quantum number | a number, symbolized by m, that indicates the orientation of an orbital around the nucleus. |
| Spin quantum number | a number which only has two possible values (-0.5 and 0.5) and indicates the two fundamental spin states of an electron in an orbital. |
| Electron configuration | arrangement of electrons in an atom. |
| Aufbau principle | principle that states that an electron occupies the lowest-energy orbital that can receive it. |
| Pauli exclusion principle | principle that states that no two electrons in the same atom can have the same set of four quantum numbers. |
| Hund's rule | rule that states that orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and that all electrons in singly occupied orbitals must have the same spin. |
| Highest occupied level | electron-containing main energy level with the highest principle quantum number. |
| Inner-shell electrons | electrons that are not in the highest occupied energy level. |
| Noble gases | Group 18 elements, which include helium, neon, argon, krypton, xenon, and radon. |
| Noble-gas configuration | outer main energy level fully occupied by eight electrons. |
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