Chapter 6 – Chemical Bonding – Flashcards
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| chemical bond |
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| a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together |
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| ionic bonding |
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| the chemical bond resulting from electrical attraction between large numbers of cations and anions |
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| covalent bonding |
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| a chemical bond resulting from the sharing of an electron pair between two atoms |
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| nonpolar-covalent bond |
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| a covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balance of electrical charge |
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| polar |
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| having an uneven distribution of charge |
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| polar-covalent bond |
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| a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons |
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| molecule |
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| a neutral group of atoms that are held together by covalent bonds |
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| molecular compound |
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| a chemical compound whose simplest units are molecules |
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| chemical formula |
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| a formula that indicates the relative numbers of atoms of each kind in a chemical compund by using atomic symbols and numerical subscripts |
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| molecular formula |
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| a formula showing the types and numbers of atoms combined in a single molecule of a molecular compound |
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| diatomic molecule |
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| a molecule containing only two atoms |
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| bond length |
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| the distance between two bonded atoms at their minimum potential energy, that is, the average distance between two bonded atoms |
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| bond energy |
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| the energy required to break a chemical bond and form neutral isolated atoms |
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| octet rule |
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| chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its highest occupied energy level |
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| electron-dot notation |
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| 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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| unshared pair |
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| a pair of electrons that is not involved in bonding and that belongs exclusively to one atom |
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| lone pair |
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| a pair of electrons that is not involved in bonding and that belongs exclusively to one atom |
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| Lewis structure |
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| a formula in which atomic symbols represent nuclei and inner-shell electrons, dot-pairs or dashes between two atomic symbols represent electron pairs in covalent bonds, and dots adjacent to only one atomic symbol represent unshared electrons |
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| structural formula |
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| a formula that indicates the kind, number, arrangement, and bonds but not the unshared electron pairs of the atoms in a molecule |
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| single bond |
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| a covalent bond produced by the sharing of one pair of electrons between two atoms |
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| double bond |
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| a covalent bond produced by the sharing of two pairs of electrons between two atoms |
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| triple bond |
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| a covalent bond produced by the sharing of three pairs of electrons between two atoms |
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| multiple bond |
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| a double or triple bond |
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| resonance |
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| the bonding in molecules or ions that cannot be correctly represented by a single Lewis structure |
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| ionic compound |
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| 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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| formula unit |
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| the simplest collection of atoms from which an ionic compound's formula can be established |
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| lattice energy |
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| the energy released when one mole of an ionic crystalline compound is formed from gaseous ions |
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| polyatomic ion |
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| a charged group of covalently bonded atoms |
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| metallic bonding |
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| chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons |
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| malleability |
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| the ability of a substance to be hammered or beaten into thin sheets |
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| ductility |
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| the ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire |
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| molecular polarity |
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| the uneven distribution of molecular charge |
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| VSEPR theory |
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| repulsion between the sets of valence-level electrons surrounding an atom causes these sets to oriented as far apart as possible |
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| hybridization |
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| the mixing of two or more atomic oribitals of similar energies on the same atom to produce new orbitals of equal energies |
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| hybrid orbitals |
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| orbitals of equal energy produced by the combination of two or more orbitals on the same atom |
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| intermolecular forces |
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| the force of attraction between molecules |
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| dipole |
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| equal but opposite charges that are separated by a short distance |
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| dipole-dipole force |
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| a force of attraction between polar molecules |
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| hydrogen bonding |
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| the intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule |
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| London dispersion force |
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| an intermolecular attraction resulting from the constant motion of electrons and the creation of instantaneous dipoles |
