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