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41 Cards in this Set
- Front
- Back
electromagnetic radiation
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a form of energy that exhibits wavelength behavior as it travels through space
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electromagnetic spectrum
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where all the forms of radiation form
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wavelength
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is the distance between corresponding points on adjacent waves
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frequency
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the number of waves that pass a given point in a specific time, usually one second
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photoelectric effect
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the emission of electrons from a metal when light shines on the metal
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quantum
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the minimum quantity of energy that can be lost or gained by an atom
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photon
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a particle of electromagnetic radiation having zero mass and carrying a quantum of energy
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ground state
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the lowest energy state of an atom
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excited state
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a state in which an atom is at a higher potential energy than it has in its ground state
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emission-line spectrum
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when a narrow beam of the emitted light was shined through a prism, it was separated into four specific colors of the visible spectrum
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continuous spectrum
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a continuous range of frequencies of electromagnetic radiation
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Heisenberg uncertainty principle
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states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle
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quantum theory
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describes mathematically the wave properties of electrons and other very small particles
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orbital
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a three-dimensional region around the nucleus that indicates the probable location of an electron
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quantum numbers
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specify the properties of atomic orbitals and the properties of electrons in orbitals
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principal quantum number
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symbolized by n, indicates the main energy level occupied by the electron
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angular momentum quantum number
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symbolized by l, indicates the shape of the orbital
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magnetic quantum number
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symbolized by m, indicates the orientation of an orbital around the nucleus
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spin quantum number
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has only two possible values-(+1/2,-1/2)- which indicate the two fundamental spin states of an electron
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electron configuration
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the arrangement of electrons in an atom
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Aufbau principle
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an electron occupies the lowest-energy orbital that can receive it
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Pauli exclusion principle
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no two electrons in the same atom can have the same set of four quantum numbers
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Hund's rule
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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
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noble gases
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group 18 elements
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noble-gas configuration
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refers to an outer main energy level occupied, in most cases, by eight electrons
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periodic law
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the physical and chemical properties of the elements are periodic functions of their atomic numbers
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periodic table
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an arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same group
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alkali metals
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elements of group 1
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alkaline-earth metals
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elements of group 2
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transition elements
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the d-block elements are metals with typical metallic properties
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main-group elements
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the p-block elements together with the s-block elements
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halogens
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the elements of group 17
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atomic radius
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one-half the distance between the nuclei of identical atoms that are bonded together
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ion
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an atom or group of bonded atoms that has a positive or negative charge
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ionization
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any process that results in the formation of an ion
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ionization energy
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the energy required to remove one electron from a neutral atom of an element
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electron affinity
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the energy change that occurs when an electron is acquired by a neutral atom
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cation
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a positive ion
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anion
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a negative ion
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valence electrons
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the electrons available to be lost, gained, or shared in the formation of chemical compounds
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electronegativity
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a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound
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