H Chem – Chemistry – Flashcards

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Nucleons
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term used to collectively identify the subatomic particles in the nucleus of an atom
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Nuclide
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term used to identify the number of protons and neutrons in the nucleus of an atom
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Nuclear bonding energy
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the energy released when a nucleus is formed from neucleons
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Band of Stability
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a range of neutron-proton ratios that produce stable nuclei
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Nuclear Reaction
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a reaction that affects the nucleus of an atom
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Transmutation
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a change in the identity of a nucleus as a result of a change in the number of its protons
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Radioactive Decay
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the spontaneous disintegration of a nucleus into a slightly lighter nucleus, accompanied by emission of particles, electromagnetic radiation, or both
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Nuclear radiation
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the particles or electromagnetic radiation emitted from the nucleus during radioactive decay
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Radioactive Nuclide
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an unstable nucleus that undergoes radioactive decay
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Alpha Particle
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2 protons and 2 neutrons bond together and is emitted from the nucleus during some kinds of radioactive decay
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Beta Particle
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an electron emitted from the nucleus during some kinds of radioactive decay
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Gamma Rays
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high-energy electromagnetic waves emitted from a nuclues as it changes form an excited state to a ground energy state
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Half-life
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the time required for half the atoms of a radioactive nuclide to decay
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Decay Series
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a series of radioactive nuclides produced by successive radioactive decays until a stable nuclide is reached
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Parent Nuclides
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heaviest nuclide of each decay series
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Daughter Nuclides
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nuclides produced by the decay of the parent nuclide
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Artificial Transmutation
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occurs as a result of the bombardment of a stable nucleus with charged and uncharged particles
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Transuranium
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elements with more than 92 protons in their nuclei
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Radioactive dating
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process by which the approximate age of an object is determined based on the amount of certain radioactive nuclides present
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Radioactive tracers
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radioactive atoms that are incorporated into substances so that movement of the substances can be followed by radiation detectors
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Nuclear fission
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a very heavy nucleus splits into more-stable nuclei of intermediate mass
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Chain Reaction
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a reaction in which the material that starts the reaction is also one of the products and can start another reaction
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Critical mass
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minimum amount of nuclide that provides the number of neutrons needed to sustain a chain reaction
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Nuclear Reactors
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use controlled-fission chain reactions to produce energy or radioactive nuclides
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Nuclear Fusion
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light-mass nuclei combine to form a heavier, more stable nucleus
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Atom
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smallest particle of an element that retains the properties of that element
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Electrons
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negatively charged subatomic particles
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Protons
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positively charged subatomic particles
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Neutrons
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subatomic particles with no charge but with a mass nearly equal to that of a proton (Mass#- atomic#= number of neutron)
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nucleus
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central core of an atom and is composed of protons and neutrons
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atomic number (Z)
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of an element is the number of protons in the nucleus of an atom of that element
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Mass Number
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the total number of protons and neutrons in an atom
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Isotopes
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atoms that have the same number of protons but different numbers of neutrons
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Nuclide
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a general term for any isotope of any element
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Atomic Mass Unit
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one-twelfth the mass of a carbon-12 atom
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Average atomic mass
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a wighted avg. mass of the atoms in a naturally occurring sample of the element
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Periodic Table
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an arrangement of the elements according to similarites in their properties
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Periods
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horizontal rows of the periodic table
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Periodic Law
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states that when the elements are arranged in order of increasing atomic number, there is periodic repetition of their physical and chemical properties
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Groups/Families
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vertical columns of elements in ther periodic table
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Representative elements
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the groups of elements that exhibit a wide range of both physical and chemical properties
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Metals
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elements which have a high electrical conductivity and a high luster when clean. They are both ductile and malleable
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Ductile
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ability to be drawn into wires
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Malleable
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the ability to be beaten into thin sheets
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Alkali metals
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family name for the elements of group 1
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Alkaline Earth Metals
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family name for the element of group 2
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Transition metals
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elements found in group 3 through 12
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Inner transition metal (Rare Earth Metal)
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made up of both the lanthanide series and the actinide series
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Nonmetals
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elements that are generally non-lustrous and they are generally poor conductors of electricity
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Calcogens
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family name for the elements of group 16
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Calcogens
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family name for the elements of group 16
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Halogens
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family name for the elements of group 17
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Noble Gases
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fmaily name for the elements in group 18
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Metalloids
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elements with properties that are intermediate between those of metals and nonmetals
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Quantum Theory
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describes mathematically the wave properties of electrons and other small particles
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Heisenberg Uncertainty Principle
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states that it is impossible to determine simultaneously both the postition and velocity of an electron or any other particle
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Principal Energy Level
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a very narrow 3-dimensional region found at varying distances from the nucleus where there is the greatest probability of location electrons
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Sublevel
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a region within a principal energy level where equal energy level oribitals of a specific shape are located
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Orbital
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a 3-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 orbitsals
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Principal Quantum number
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symbolized by n, indicates the principal energy level occupied by the electrons
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Angular momentum quantum number
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symbolized by the letter l. indicates the shape of the orbital(sublevels)
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magnetic quantum number
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symbolized by the letter m, indicates the orientation of an orbital
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Spin quantum number
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symbolized bye letter s, has onlyl 2 possible values which indicate the 2 fundamental spin states of an electron in an orbital
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Electron Configuration
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indicates the arrangement of electrons in an atom
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ground-state electron configuration
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indicates the lowest-energy arrangement of the electrons for each element
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Aufbau Principle
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states that an electron occupies the lowest energy orbital that can receive it
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Pauli Exclusion Principle
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states that no 2 electrons in the same atom can have the same set of 4 quantum numbers
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Hund's Rule
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states that orbital 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
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Valence shell
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the electron-containing principal energy level with the highest principal quantum number
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Valence electrons
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electrons that are in the highest occupied energy level
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Inner shell electrons
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electrons that are not in the highest occupied energy level
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Noble gas configuration
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an outer principle energy level fully occupied, in most cases by 8 electrons
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Octet Configuration
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an outer principle energy level fully occupied by 8 electrons
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