Chemistry Ch 6 Vocabulary

Front 1

chemical bond

Back 1

a mutual electrical attraction between the 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 large numbers of cations and anions

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covalent bonding

Back 3

results from the sharing of electron pairs between two atoms

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nonpolar-covalent bond

Back 4

a covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charge

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polar

Back 5

a bond that has an uneven distribution of charge

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polar-covalent bond

Back 6

a covalent bond in which the bonded atoms 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 covalent bonds

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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 numbers of atoms combined in a single molecule of a molecular compound

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diatomic molecule

Back 11

a molecule containing only two atoms

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bond length

Back 12

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

Back 13

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

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octet rule

Back 14

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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single bond

Back 15

a covalent bond produced by the sharing of one pair of electrons between two atoms

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Lewis structures

Back 16

formulas 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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double bond

Back 17

a covalent bond produced by the sharing of two pairs of electrons between two atoms

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triple bond

Back 18

a covalent bond produced by the sharing of three pairs of electrons between two atoms.

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resonance

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refers to 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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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

Back 21

the simplest collection of atoms from which an ionic compound's formula can be established

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lattice energy

Back 22

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

Back 24

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

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malleablity

Back 25

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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hybridization

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which is the mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies

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dipole

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

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dipole-dipole forces

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the forces of attraction between polar molecules

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hydrogen bonding

Back 30

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 forces

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

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molecular polarity

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uneven distribution of molecular charge

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VSEPR theory

Back 33

"valence shell electron pair repulsion -used to predict the shapes of molecules based on the fact that electron pairs strongly repel each other and tend to be oriented as far apart as possible

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atoms of metals bond _____ with atoms of nonmetals

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ionically

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atoms of metals bond ______ with each other

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metallically