holt modernchem ch.6
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
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| bond energy | the energy required to break a chemical bond and form neutral isolated atoms
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| bond length | the distance between two bonded atoms at their minimum potential energy, that is, the average distance between two bonded atoms
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| chemical bond | a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together
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| chemical formula | a formula that indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numericalsubscripts
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| covalent bonding | a chemical bond resulting from the sharing of an electron pair between two atoms
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| diatomic molecule | a molecule containing only two atoms
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| dipole | equal but opposite charges that are separated by a short distance
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| dipole-dipole force | a force of attraction between polar molecules
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| double bond | a covalent bond produced by the sharing of two pairs of electronsbetween two atoms
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| ductility | the ability of a substance to be drawn, pulled, or extruded through asmall opening to produce a wire
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| electron-dot notation | an electron-configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element’s symbol
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| formula unit | the simplest collection of atoms from which an ionic compound’s formula can be established
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| hybrid orbitals | orbitals of equal energy produced by the combination of two or more orbitals on the same atom
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| hybridization | the mixing of two or more atomic orbitals of similar energies onthe same atom to produce new orbitals of equal energies
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| hydrogen bonding | the intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair ofelectrons of an electronegative atom in a nearby molecule
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| intermolecular force | the force of attraction between molecules
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| ionic bonding | the chemical bond resulting from electrical attraction between large numbers of cations and anions
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| ionic compound | a compound composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal
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| lattice energy | the energy released when one mole of an ionic crystalline compound is formed from gaseous ions
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| Lewis structure | a formula in which atomic symbols represent nuclei and innershell electrons, dot-pairs or dashes between two atomic symbols representelectron pairs in covalent bonds, and dots adjacent to only one atomic symbolrepresent unshared electrons
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| London Dispersion Force | an intermolecular attraction resulting from thec onstant motion of electrons and the creation of instantaneous dipoles
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| lone pair | a pair of electrons that is not involved in bonding and that belongs exclusively to one atom
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| malleability | the ability of a substance to be hammered or beaten into thin sheets
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| metallic bonding | chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons
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| molecular compound | a chemical compound whose simplest units are molecules
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| molecular formula | a formula showing the types and numbers of atoms combined in a single molecule of a molecular compound
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| molecular polarity | the uneven distribution of molecular charge
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| molecule | a neutral group of atoms that are held together by covalent bonds
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| multiple bond | a double or triple bond
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| nonpolar-covalent bond | a covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution ofelectrical charge
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| octet rule | chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its highest occupiedenergy level
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| polar | having an uneven distribution of charge
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| polar-covalent bond | a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons
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| polyatomic ion | a charged group of covalently bonded atoms
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| resonance | the bonding in molecules or ions that cannot be correctly representedby a single Lewis structure
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| single bond | a covalent bond produced by the sharing of one pair of electronsbetween two atoms
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| structual formula | a formula that indicates the kind, number, arrangement, andbonds but not the unshared electron pairs of the atoms in a molecule
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| triple bond | a covalent bond produced by the sharing of three pairs of electrons between two atoms
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| unshared pair | a pair of electrons that is not involved in bonding and that belongs exclusively to one atom
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| VSEPR Theory | repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart aspossible
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| Ionic compounds have (low, high) melting points | high
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| boxes are used to demonstrate ______ | sharing
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| unshared electrons exert | a very powerful repulsive force.
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| what determines bond length | potential energy
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