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Chapter 4: Arrangement of Electrons in Atoms (Holt Modern Chemistry)

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
Created by: SavioScience



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