Chemistry Chapter 6

Front 1

bond energy

Back 1

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

Front 2

bond length

Back 2

the distance between two bonded atoms at their minimum potential energy, that is, the average distance between two bonded atoms

Front 3

chemical bond

Back 3

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

Front 4

chemical formula

Back 4

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

Front 5

covalent bonding

Back 5

a chemical bond resulting from the sharing of an electron pair between two atoms

Front 6

diatomic molecule

Back 6

a molecule containing only two atoms

Front 7

dipole

Back 7

equal but opposite charges that are separated by a short distance

Front 8

dipole-dipole force

Back 8

a force of attraction between polar molecules

Front 9

double bond

Back 9

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

Front 10

ductility

Back 10

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

Front 11

electron-dot notation

Back 11

an electron-configuration notation in which only the valenge electrons of an atom of a particular element are shown, indicated by dots placed around the element's symbol

Front 12

formula unit

Back 12

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

Front 13

hybrid orbitals

Back 13

orbitals of equal energy produced by the combination of two or more orbitals on the same atom

Front 14

hybridization

Back 14

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

Front 15

hydrogen bonding

Back 15

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

Front 16

intermolecular force

Back 16

the force of attraction between molecules

Front 17

ionic bonding

Back 17

the chemical bond resulting from electrical attraction between large numbers of cations and anions

Front 18

ionic compound

Back 18

a compound composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal

Front 19

lattice energy

Back 19

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

Front 20

Lewis structure

Back 20

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

Front 21

London dispersion force

Back 21

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

Front 22

lone pair

Back 22

a pair of electrons that is not involved in bonding and that belongs exclusively to one atom

Front 23

malleability

Back 23

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

Front 24

metallic bonding

Back 24

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

Front 25

molecular compound

Back 25

a chemical compound whose simplest units are molecules

Front 26

molecular formula

Back 26

a formula showing the types and numbers of atoms combined in a single molecule of a molecular compound

Front 27

molecular polarity

Back 27

the uneven distribution of molecular charge

Front 28

molecule

Back 28

a neutral group of atoms that are held together by covalent bonds

Front 29

multiple bond

Back 29

a double or triple bond

Front 30

nonpolar-covalent bond

Back 30

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

Front 31

octet rule

Back 31

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

Front 32

polar

Back 32

having an uneven distribution of charge

Front 33

polar-covalent bond

Back 33

a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons

Front 34

polyatomic ion

Back 34

a charged group of covalently bonded atoms

Front 35

resonance

Back 35

the bonding in molecules or ions that cannot be correctly represented by a single Lewis structure

Front 36

single bond

Back 36

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

Front 37

structural formula

Back 37

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

Front 38

triple bond

Back 38

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

Front 39

unshared pair

Back 39

a pair of electrons that is not involved in bonding and that belongs exclusively to one atom

Front 40

VSEPR theory

Back 40

repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible