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Chem Ch. 4 VOC

Stack #155221

a form of energy that exhibits wavelike behavior as it travels through space Electromagnetic Radiation
all the forms of electromagnetic radiation 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 was shined through a prism, it was separated into a series of specific frequencies (and therefore specific wavelengths) of visible light – the bands of light are part of the line-emission spectrum Line-emission spectrum
the emission of a continuous range of frequencies of electromagnetic radiation Continuous spectrum
states that it is impossible to determine simultaneously both the position and the velocity of an electron or any other particle Heisenberg uncertainty principle
describes mathematically the waves properties of electrons and other very small particles Quantum theory
a three-dimensional region around the nucleus that indicates the probable location of an electron Orbital
specify the properties of atomic orbitals and the properties of electrons in orbitals Quantum numbers
symbolized by n, indicates the main energy level occupied by the electron Principal 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 possible values(+1/2, -1/2) which indicate the two fundamental spin states of an electron 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 2 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 b a second electron, and all electrons in singly occupied orbitals must have the same spin Hund’s rule
electrons that are not in the highest occupied energy level Inner-shell electrons
the Group 18 elements (helium, neon, argon, krypton, xenon, and radon) Noble gasses
outer main energy level fully occupied [most cases-by 8 electrons] Noble-gas configuration
Created by: ElizabethI