Stenberg Basic Chemistry Ch 6

Front 1

chemical bond

Back 1

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

Front 2

ionic bonding

Back 2

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

Front 3

covalent bonding

Back 3

chemical bonding that results from the sharing of electron pairs between two atoms

Front 4

polar

Back 4

bonds that have an uneven distribution of charge

Front 5

molecule

Back 5

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

Front 6

chemical formula

Back 6

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

Front 7

octet rule

Back 7

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 8

Lewis structure

Back 8

formulas in which atomic symbols represent nuclei and inner-shell electrons, dashes between atoms represent shared electrons, and pairs of dots represent unshared electrons

Front 9

valence electrons

Back 9

electrons available to be lost, gained, or shared in an atom

Front 10

formula unit

Back 10

simplest collection of atoms from which an ionic compound’s formula can be derived

Front 11

metallic bonding

Back 11

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

Front 12

malleability

Back 12

ability to be hammered into thin sheets

Front 13

ductility

Back 13

ability to be extruded through a small opening and made into a wire

Front 14

intermolecular forces

Back 14

forces of attraction between different molecules

Front 15

polyatomic ion

Back 15

a charged group of covalently bonded atoms