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Chemistry Unit 3 Voc

Chemistry Unit 3 Vocabulary - Chemical Bonding

QuestionAnswer
the configuration (order of filling) of the s, p, d, and f orbitals; electrons fill the lowest energy levels first Aufbau Principle
a bond in which electrons are shared, equally or unequally Covalent Bond
energy released when an electron is added to an atom to form an ion Electron Affinity
the different energy levels filled by electrons within an atom Electron Orbitals (s,p,d,f)
electrons fill empty orbitals before they pair up Hund's Rule
a negatively or positively charged atom (monatomic) or group of atoms (polyatomic) Ion
a bond in which one or more electrons are given by one atom to another Ionic Bond
an atomic symbol with dots showing valence electrons Lewis Dot Structure
a bond in which the valence electrons are shared among all of the atoms in the metal Metallic Bond
the 3D shape of a covalent molecule, as determined by shared and unshared electrons Molecular Geometry
elements, other than transition metals, that tend to react so that each atom has eight electrons in its outer (valence) shell (e.g., orbitals are full) Octet Rule
for atoms of pure elements, the oxidation number is zero; for monatomic ions, it is the charge on the ion; Oxidation Number
in polyatomic ions, the oxidation numbers of the component atoms add up to the charge on the ion; in a neutral molecule, the oxidation numbers add up to zero Oxidation Number
electrons in the same orbital, and the value must have opposite spins Pauli's Exclusion Principle
because of differences in electronegativity, different types of atoms in covalent molecules do not share electrons equally Polar & Nonpolar Molecules
unshared electron pairs of atoms in covalent molecules repel each other; thus, the shape of the molecule will tend to minimize the net repulsions VSEPR - Valence Shell Electron Repulsion Theory
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