Chemistry Unit 6 Vocabulary

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 cations and anions.

Front 3

Covalent Bonding

Back 3

Bonding that results from the sharing of electron pairs between two atoms.

Front 4

Non-Polar Covalent Bond

Back 4

A covalent bond in which the bonding electrons are shared equally by the bonded atoms.

Front 5

Polar

Back 5

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

Front 8

Chemical Formula

Back 8

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

Front 9

Molecular Formula

Back 9

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

Front 10

Bond Energy

Back 10

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

Front 11

Octet Rule

Back 11

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 12

Electron-Dot Notation

Back 12

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

Front 13

Lewis Structures

Back 13

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 14

Structural Formulas

Back 14

Indicates the kind, number, arrangement, and binds but not the unshared pairs of the atoms in a molecule.

Front 15

Single Bond

Back 15

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

Front 16

Multiple Bonds

Back 16

Double and triple bonds.

Front 17

Resonance

Back 17

Refers to bonding in molecules or ions that cannot be correctly represented by a single Lewis Structure.

Front 18

Ionic Compound

Back 18

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

Front 19

Polyatomic Ion

Back 19

A charged group of covalently bonded atoms.

Front 20

Metallic Bonding

Back 20

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

Front 21

Malleability

Back 21

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

Front 22

Ductility

Back 22

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

Front 23

VSEPR Theory

Back 23

This states that repulsion between the sets of valence electrons surrounding an atom causes these sets to be oriented as far apart as possible.

Front 24

Dipole

Back 24

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

Front 25

Hydrogen Bonding

Back 25

The IMF 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 26

London Dispersion Forces

Back 26

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