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TERM
Bonding Electron Pair
Ionic Crystals Metallic Crystals Metallic Bonding Electron Sea Theory Molecular crystals
Covalent Network Crystal Dipole Dipole-dipole Force Electron Configuration Valence Shell Electron-Pair Repulsion (VSEPR) Theory Quantum Number Three-dimensional Structure |
DEFINITION
Is two electrons that are working together in forming a nonpolar covalent bond between atoms.
Solids that have positive and negative ions arrange in a crystal lattice structure, with alternating packing of the positive and negative ions.
Solids with closely packed atoms, they held together by electrostatic interactions and free moving electrons.
bonding that holds the nuclei and electrons of metals together.
Electrons in a metallic crystal move freely around the positively charged nuclei. Solids composed of individual
molecules held together by intermolecular forces of attraction. Solid in which the atoms form covalent bonds in an
interwoven network. positive and negative charges that are seperated in a region in space.
Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule.
Electrons that have the lowest energy are found closest to the nucleus. and the electrons that have higher energy are found away from the nucleus. Method to determine the geometry of a molecule based on the idea that electron pairs are as far apart as possible.
Any of a set of real numbers assigned to a physical system that individually characterize the properties and collectively specify the state of a particle or of the system.
is the shape that depends on the preferred spatial orientation of covalent bond to atoms having two or more bonding partners.
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Wave Function
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Mathematical probability of finding an electron in a certain region of space
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Valence Electron
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Electron in the outermost principal quantum level of an atom
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van der Waals Forces
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Many types of intermolecular forces, including dipole-dipole forces, London dispersion forces, and hydrogen bonding
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Magnetic Quantum Number (m)
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Quantum number that describes the orientation of an atomic orbital in space relative to other orbitals in the atom, with whole-number values between +l and -l, including 0
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London-dispersion Forces
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Intermolecular forces that exist in non-polar molecules; they increase as the molecular mass increases
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Lewis Structure
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A Lewis Dot Structure is a symbol of description of the valence electrons in a molecule. The dots are used to represent individual electrons and lines represent covalent bonds.
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Orbital
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Region around the nucleus where an electron has a high
probability of being found |
Principal Quantum Number
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Quantum number that describes the size and energy of an atomic orbital
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Secondary Quantum Number (l)
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Quantum number that describes the shape and energy of an
atomic orbital, with whole-number values from 0 to n -1 for each value of n |
Spin Quantum Number (ms)
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Quantum number that relates to the spin of the electron
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Shell
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Atom's main energy level, where the shell number is given by the principal quantum number, n = 1, 2,3,4,...
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