Chem Ch. 6

Front 1

Chemical bond

Back 1

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

Front 2

ionic bonding

Back 2

chemical bonding that results from the electrical attraction between large numbers of cations and anions.

Front 3

covalent bonding

Back 3

results from the sharing of electron pairs between two atoms.

Front 4

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.

Front 5

polar

Back 5

bonds that have an uneven distribution of charge.

Front 6

polar-covalent bond

Back 6

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

Front 7

molecule

Back 7

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

Front 8

molecular compound

Back 8

a chemical compound whose simplest units are molecules.

Front 9

chemical formula

Back 9

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

Front 10

molecular formula

Back 10

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

Front 11

diatomic molecule

Back 11

a molecule containing only 2 atoms.

Front 12

bond length

Back 12

the distance between 2 bonded atoms at their minimm potential energy, that is, the average distance between two bonded atoms.

Front 13

bond energy

Back 13

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

Front 14

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 energy level.

Front 15

electron-dot notation

Back 15

an electron-configuration notation in which only the valence electrons of an atom of a particular element are shown.

Front 16

unshared pair / lone pair

Back 16

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

Front 17

lewis structures

Back 17

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.

Front 18

structural formula

Back 18

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

Front 19

single bond

Back 19

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

Front 20

double bond

Back 20

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

Front 21

triple bond

Back 21

a covalent bond produced by the sharing of 3 pairs of electrons between 2 atoms.

Front 22

multiple bonds

Back 22

what you call double and triple bonds.

Front 23

resonance

Back 23

refers to bonding in molecules or ions that cannot be correctly represented by a single lewis structure.

Front 24

ionic compound

Back 24

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

Front 25

formula unit

Back 25

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

Front 26

lattice energy

Back 26

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

Front 27

polyatomic ions

Back 27

charged group of covalently bonded atoms.

Front 28

metalic bonding

Back 28

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

Front 29

malleability

Back 29

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

Front 30

Ductility

Back 30

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

Front 31

molecular polarity

Back 31

the uneven distribution of molecular charge.

Front 32

VSEPR

Back 32

states that repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible.Valence shell electron pair repulsion

Front 33

hybridization

Back 33

the mixing of 2 or more atomic orbitals of similar energies on the same atoms to produce new orbitals of equal energies.

Front 34

hybrid orbitals

Back 34

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

Front 35

intermolecular forces

Back 35

the forces of attraction between molecules.

Front 36

dipole

Back 36

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

Front 37

dipole-dipole forces.

Back 37

the forces of attraction between polar molecules.

Front 38

hydrogen bonding

Back 38

the intermolecular forces 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 is a nearby molecule.

Front 39

London dispersion forces

Back 39

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