Elements Of General, Organic, And Biological Chemistry Chapter 3

Front 1

Chemical bond

Back 1

A net electrical force of attraction that holds atomic nuclei near each other within compounds.

Front 2

Molecule

Back 2

An electrically neutral particle made up of the nuclei and electrons of two or more atoms and held together by covalent bonds.

Front 3

Ionic compound

Back 3

A compound that consists of an orderly aggregation of oppositely charged ions that assemble in whatever ratio ensures overall electrical neutrality.

Front 4

Octet rule

Back 4

The atoms of the reactive representative elements tend to undergo those chemical reactions that most directly give them electron configurations of the nearest noble gas.

Front 5

Ion

Back 5

An electrically charged, atomic or molecular-sized particle.

Front 6

Li

Back 6

Lithium

Front 7

Na

Back 7

Sodium

Front 8

K

Back 8

Potassium

Front 9

Mg

Back 9

Magnesium

Front 10

Ca

Back 10

Calcium

Front 11

Ba

Back 11

Barium

Front 12

Al

Back 12

Aluminum

Front 13

O

Back 13

Oxygen

Front 14

S

Back 14

Sulfer

Front 15

F

Back 15

Fluorine

Front 16

F-

Back 16

Fluoride

Front 17

Cl

Back 17

Chlorine

Front 18

Cl-

Back 18

Chloride

Front 19

Br

Back 19

Bromine

Front 20

Br-

Back 20

Bromide

Front 21

I

Back 21

Iodine

Front 22

I-

Back 22

Iodide

Front 23

Ag

Back 23

Silver

Front 24

Zn

Back 24

Zinc

Front 25

Cu

Back 25

Copper

Front 26

Cu+

Back 26

Cuprous Ion

Front 27

Cu++

Back 27

Cupric Ion

Front 28

Fe

Back 28

Iron

Front 29

Fe++

Back 29

Ferrous Ion

Front 30

Fe+++

Back 30

Ferric Ion

Front 31

Oxidation

Back 31

A creaction in which the oxidation number of one of the atoms of a reactant becomes more positive.

Front 32

Reduction

Back 32

A reaction in which the oxidation number of an atom of one reactant becomes less positive or more negative.

Front 33

Oxidation number

Back 33

For monatomic ions, the quantity and sign of the electrical charge on the ion.

Front 34

Redox reaction

Back 34

A reaction in which oxidation numbers change.

Front 35

Reducing agent

Back 35

A substance that can cause another to be reduced.

Front 36

Oxidizing agent

Back 36

A substance that can cause an oxidation.

Front 37

Electrolyte

Back 37

Any substance whose solution in water conducts electricity.

Front 38

Covalent bond

Back 38

The net force of attraction that arises as two atomic nuclei share a pair of electrons.

Front 39

Covalence

Back 39

The number of covalent bonds that an atom can have in a molecule.

Front 40

Polyatomic Ion

Back 40

An ion made from two or more atoms.

Front 41

NH4+

Back 41

Ammonium ion

Front 42

H3O+

Back 42

Hydronium ion

Front 43

OH-

Back 43

Hydroxide ion

Front 44

CH3CO2-

Back 44

Acetate ion

Front 45

CO3--

Back 45

Carbonate ion

Front 46

HCO3-

Back 46

Bicarbonate ion

Front 47

SO4--

Back 47

Sulfate ion

Front 48

HSO4-

Back 48

Hydrogen sulfate ion (Bisulfate)

Front 49

PO4---

Back 49

Phosphate ion

Front 50

NO3-

Back 50

Nitrate ion

Front 51

NO2-

Back 51

Nitrite ion

Front 52

HSO3-

Back 52

Hydrogen Sulfite ion

Front 53

SO3--

Back 53

Sulfite ion

Front 54

CN-

Back 54

Cyanide ion

Front 55

MnO4-

Back 55

Permanganate Ion

Front 56

CrO4--

Back 56

Chromate ion

Front 57

Cr2O7--

Back 57

Dichromate ion

Front 58

Electron Cloud

Back 58

A mental model that views the one or two rapidly moving electrons of an orbital as creating a cloud-like distribution of negative charge.

Front 59

Electrical Dipole

Back 59

A pair of equal but opposite electrical charges separated by a small distance in a molecule.

Front 60

Polar bond

Back 60

A bond at which we can write beta plus at one end and beta minus at the other end.

Front 61

Electronegativity

Back 61

The ability of an atom joined to another by a covalent bond to attract the electrons of the bond toward itself.

Front 62

Polar Molecule

Back 62

A molecule that has sites of partial positive and partial negative charge and a permanent electrical dipole.