Chapert 6 Vocabulary - Chemical Bonding

Front 1

chemical bond

Back 1

mutual electrical attraction between nuclei and valence electrons of different atoms that binds the atoms together

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ionic bonding

Back 2

chemical bonding that results from the electrical attraction between cations and anions

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covalent bonding

Back 3

bonding that results from the sharing of electrons pairs between two atoms

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nonpolar-covalent bond

Back 4

bonding electrons are shared equally by the bonded atoms, resulting in a balaced distrubution of electrical charge

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polar

Back 5

an uneven distribution of electrical charge

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polar-covalent bond

Back 6

bonding electrons have an unequal attraction for the shared electrons

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molecule

Back 7

a neutral group of atoms that are held together by a colvent bond

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molecular compound

Back 8

a chemical compound whose simplest units are molecules

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chemical formula

Back 9

indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts

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molecular formula

Back 10

shows the types and number of atoms combined in a single molecule of a molecular compound

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bond energy

Back 11

the energy required to break a chemical bond and form neutral isolated atoms

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electron-dot notation

Back 12

is an electron-configuration notation in which only the valence electrons of an atom are shown by dots placed around the elements's symbol

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Lewis structure

Back 13

formulas in which atomic symbols represent nuclei and inner-shell electrons, dot-pairs or dashes b/t two atomic symbols represent electron pairs in covalent, and dots adjacent to only one atomic symbol represent unshared electrons

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structural formula

Back 14

indicates the kind, number, arrangement, and bonds but not the unshared pairs of the atoms in a molecule

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single bond

Back 15

a covalent bond in which one pair of electrons is shared between two atoms

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multiple bond

Back 16

double and triple bonds

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resonance

Back 17

bonding in molecules or ions that connot be correctly represented by a single Lewis structure

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ionic compound

Back 18

composed of (+) and (-) ions that are combined so that the numbers of (+) and (-) 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

Back 20

the energy released when one mole of an ionic crystalline compound is formed from gaseous ions

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polyatomic ion

Back 21

a charged group of covalently bonded atoms

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metallic bond

Back 22

bonding that results from the attraction between metal atoms and the surrounding sea of electrons

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malleability

Back 23

the ability of a substance to be hammered or beated into thin sheets

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ductility

Back 24

the ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire.

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VESPR theory

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states that repulsion b/t the sets of balance-level electrons surrounding an atom causes these sets to be oriented as far apart as possible

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hybridization

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mixing of two or more atomic orbitals of similar energies on the same atoms to produce new hybrid atomic 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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dipole

Back 28

created by equal but opposite charges that are separated by a short distance

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hydrogen bonding

Back 29

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 forces

Back 30

intermolecular attrations resulting from the constant motion of electrons and the creation of instantaneous dipoles