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Chap4_Electron_Arng
Chapter 4: Arrangement of Electrons in Atoms (Holt Modern Chemistry)
| Question | Answer |
|---|---|
| A form of energy that exhibits wavelike behavior as it travels through space | Electromagnetic radiation |
| All forms of electromagnetic radiation form this | Electromagnetic spectrum |
| The distance between corresponding points on adjacent waves | Wavelength |
| The number of waves that pass a given point in a specific time, usually one second | Frequency |
| The emission of electrons from a metal when light shines on the metal | Photoelectric effect |
| The minimum quantity of energy that can be lost or gained by an atom | Quantum |
| A particle of electromagnetic radiation having zero mass and carrying a quantum of energy | Photon |
| The lowest energy state of an atom | Ground state |
| A state in which an atom has a higher potential energy than it has in its ground state | Excited state |
| When a narrow beam of the emitted light is shined through a prism, it separates into specific colors of the visible spectrum, producing this | Emission-line spectrum |
| The emission of a continuous range of frequencies of electromagnetic radiation | Continuous spectrum |
| It is impossibl3 to determine simultaneously both the position and the velocity of an electron or any other particle | Heisenburg uncertainty principle |
| A theory that mathematically describes the wave properties of electrons and other very small particles | Quantum theory |
| A three-dimensional region around the nucleus that indicates the probably location of an electron | Orbital |
| Numbers that specify the properties of atomic orbitals and properties of electrons in orbitals | Quantum numbers |
| Symbolized by n, indicates the main energy level occupied by the electron | Principle quantum number |
| Symbolized by l, indicates the shape of the orbital | Angular momentum quantum number |
| Symbolized by m, indicates the orientation of an orbital around the nucleus | Magnetic quantum number |
| Has only two values (+1/2 or -1/2), indicates the two fundamental spin states of an electron in an orbital | Spin quantum number |
| The arrangement of electrons in an atom | Electron configuration |
| An electron occupies the lowest-energy orbital that can receive it | Aufbau principle |
| No two electrons in the same atom can have the same set of four quantum numbers | Pauli exclusion principle |
| 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 state | Hund's rule |
| The Group 18 elements (helium, neon, argon, krypton, xenon, and radon) | Noble gases |
| An outer main energy level occupied, in most cases, by eight electrons | Noble-gas configuration |
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