Unit 4: Chemical Bonding

Front 1

Chemical Bond

Back 1

A link between atoms that results from the mutual attraction between the nuclei and valence electrons of both atoms

Front 2

Ionic Bond

Back 2

a chemical bond resulting from electrical attraction between large numbers of positive and negative ions, cations & anions

Front 3

Covalent Bond

Back 3

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

Front 4

Polar Covalent Bond

Back 4

a covalent bond where the united atoms have an unequal attraction for the shared electrons

Front 5

Nonpolar Covalent Bond

Back 5

a covalent bond in which the bonding electrons are shared equally by bonded atoms with a resulting balanced distribution of charges

Front 6

Ionic Compound

Back 6

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

Front 7

Formula Unit

Back 7

simplest collection of atoms from which a compound's formula can be established

Front 8

Crystal Lattice

Back 8

an orderly arrangement of ions

Front 9

Lattice energy

Back 9

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

Front 10

Molecule

Back 10

the smallest unit quanity of matter which can exist by itself and retain all the properties of the original substance

Front 11

Molecular Compound

Back 11

a chemical compound whose simplest units are molecules

Front 12

The 7 diatomic molecules

Back 12

hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, iodine

Front 13

Bond Energy

Back 13

the energy required to break a chemical bond and fomr neutral atoms

Front 14

Bond Length

Back 14

the average distance between two bonded atoms

Front 15

Octet Rule

Back 15

chemical compounds will form so that each atom, by gaining, losing or sharing electrons, has an octet of electrons in its highest occupied energy level

Front 16

Unshared Pair

Back 16

a pair of electrons that is not involved in bonding, but instead belongs exclusively to one atom

Front 17

Structural Formula

Back 17

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

Front 18

Isomers

Back 18

compounds with the same formula but a different arrangement of atoms

Front 19

Chemical Formula

Back 19

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

Front 20

Molecular Formula

Back 20

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

Front 21

Single Bond

Back 21

covalent bond produced by sharing one pair of electrons between 2 atoms

Front 22

Double Bond

Back 22

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

Front 23

Covalent Networking Bond

Back 23

a continuous, 3D network of covalently bonded atoms

Front 24

Coordinate Covalent Bond

Back 24

a bond where just one atom contributes electrons

Front 25

Triple Bond

Back 25

a covalent bond with the sharing of three pairs of electrons

Front 26

Polyatomic Ion

Back 26

a charged group of covalently bonded atoms

Front 27

Resonance

Back 27

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

Front 28

Delocalized Electrons

Back 28

valence electrons that are free to move about

Front 29

Metallic Bond

Back 29

a chemical bond resulting from the attraction between metal atoms and surrounding mobile electrons

Front 30

Heat of Vaporization

Back 30

the amount of heat needed to change a metal in solid state to a gas

Front 31

VSEPR Theory

Back 31

used for predicting molecular geometry

Front 32

Main assumption of the VSEPR Theory

Back 32

electrons in molecules will repel one another; therefore causing the bonds and long pairs of electrons to orient themselves as they do

Front 33

VSEPR Theory

Back 33

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

Front 34

Hybridization

Back 34

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

Front 35

Hybrid Orbitals

Back 35

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

Front 36

Intermolecular Forces

Back 36

the forces of attraction between molecules

Front 37

Intramolecular Forces

Back 37

the forces of attraction within a molecule

Front 38

Dipole

Back 38

equal, but opposite charges separated by a short distance

Front 39

Dipole-Dipole Forces

Back 39

forces of attraction between polar molecules

Front 40

Hydrogen Bonding

Back 40

an intermolecular attraction between a hydrogen atom and an unshared pair of electrons on a strongly electronegative atom in another molecule

Front 41

London Dispersion Forces

Back 41

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