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31 Cards in this Set
- Front
- Back
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bond energy
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energy required to break a given chemical bond
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ionic bonding
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the electrostatic attraction between oppositely charged ions
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ionic compound (binary)
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a compound that results when a metal reacts with a nonmetal to form a cation and an anion
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Coloumb's Law
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constant where E is the energy of interaction between a pair of ions, expressed in joules; r is the distance between the ion centers in nm; and Q1 and Q2 are the numerical ion charges.
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bond length
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the distance between the nuclei of the two atoms connected by a bond; the distance where the total energy of a diatomic molecule is minimal
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covalent bonding
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a type of bonding in which electrons are shared by atoms
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polar covalent bonding
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a covalent bond in which the electrons are not shared equally because one atom attracts them more strongly than the other
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electronegativity
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the tendency of an atom in a molecule to attract shared electrons to itself
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dipolar
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a molecule that has a center of positive charge and a center of negative charge
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dipolar moment
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a property of a molecule whose charge distribution can be represented by a center of positive share and a center of negative charge
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isoelectronic ions
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ions containing the same number of electrons
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lattice energy
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the energy change occurring when separated gaseous ions are packed together to form an ionic solid
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single bond
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a bond in which one pair of electrons is shared by two atoms
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double bond
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a bond in which two pairs of electrons are shared by two atoms
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triple bond
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a bond in which three pairs of electrons are shared by two atoms
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localized electron (LE) model
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a model which assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
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lone pair
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an electron pair that is localized on a given atom; an electron pair not involved in bonding
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bonding pair
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an electron pair found in the space between two atoms
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Lewis structure
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diagram of a molecule showing how the valence electrons are arranged among the atoms in the molecule
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duet rule
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elements that form stable molecules where they share two electrons (hydrogen)
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octet rule
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the observation that atoms of nonmetals tend to form the most stable molecules when they are surrounded by eight electrons (to fill their valence orbitals)
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resonance
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a condition occurring when more than one valid Lewis structure can be written for a particular molecule. The actual electronic structure is not represented by any one of the Lewis structures but by the average of them all
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formal charge
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the charge assigned to an atom in a molecule or polyatomic ion derived from a specific set of rules
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molecular structure
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the 3d arrangement of atoms in a molecule
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VSEPR model
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a model whose main postulate is that the structure around a given atom in a molecule is determined principally by minimizing electron pair repulsions
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hybridization
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a mixing of the native orbitals on a given atom to form special atomic orbitals for bonding
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hybrid orbitals
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a set of atomic orbitals adopted by an atom in a molecule different from those of the atom in the free state
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sigma bond
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a covalent bond in which the electron pair is shared in an area centered on a line running between the atoms
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pi bond
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a covalent bond in which parallel p orbitals share an electron pair occupying the space above and below the line joining the atoms
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bond order
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the difference between the number of bonding electrons and the number of antibonding electrons, divided by two. Its an index of bond strength.
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coordinate covalent bond
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a metal-ligand bond resulting from the interaction of a Lewis base (the ligand) and a Lewis acid (the metal ion)
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