CHAPTER 5 - NOMENCLATURE IONIC COMPOUNDS NAMING Name the cation first, then name the anion second

CHAPTER 5 - NOMENCLATURE

IONIC COMPOUNDS

NAMINGName the cation first, then name the anion second

CATIONS1) Metals that form only one monatomic cation

Name as the elemental name

4A-1 (of 32)

Group 1 (1+)Group 2 (2+)

Al3+

Zn2+

Ag+

4A-2

Ca2+

calciumK+

potassiumAl3+

aluminum

4A-3

2) Metals that form more than one monatomic cationName as the elemental name, followed by their charge as a roman numeral in parenthesis

4A-4

Mn2+

manganeseMn3+

manganeseSn4+

tin (IV)

4A-5

George ForemanGeorge ForemanGeorge ForemanGeorge ForemanGeorge Foreman

(II) (III)

3) Cations that are polyatomic

NH4+

ammonium

UO22+

uranyl

Hg22+

mercury (I)

4A-6

ANIONS1) Nonmetals that form a monatomic anion

Name as the root of the elemental name, ending in -ide

4A-7

Group 17 (1-)Group 16 (2-)Group 15 (3-)

H (1-)

4A-8

O2-

oxideCl-

chlorideN3-

nitride

4A-9

S2- P3- H-

2) Anions that are polyatomicName polyatomic anions that contain oxygen as the root of the elemental name, ending in –ate or –ite

CO32-

carbonate

NO3-

nitrate

PO43-

phosphate

SO42-

sulfate

NO2-

nitrite

SO32-

sulfite

4A-10

Some elements can make 4 oxyions

ClO4- perchlorate

ClO3- chlorate

ClO2- chlorite

ClO- hypochlorite

4A-11

Name the following:

CaCl2

calcium chloride

Na2O

sodium oxide

MgS

4A-12

AuI3

1-1-1-

PbBr2

1-1-

Cu2O

gold (III) iodide

3+

lead (II) bromide

2+

4A-13

Cr2S3

2-2-2-

K2SO4 SnCO3

chromium (III) sulfide

3+3+

potassium sulfate

4A-14

FORMULASBase formulas on charge balance

barium fluorideBa2+ F-

(2+) + (1-) + (1-) = 0

potassium oxideK+ O2-

(1+) + (1+) + (2-) = 0

BaF2

Need 2 to make total charge 0


K2O

4A-15

lithium nitride aluminum sulfideAl3+ S2-

(3+) + (3+) + (2-) + (2-) + (2-) = 0

Makes 6+ Makes 6-

Al2S3

4A-16

cobalt (III) chlorideCo3+ Cl-

(3+) + (1-) + (1-) + (1-) = 0

CoCl3


lithium nitrateLi+ NO3

-

(1+) + (1-) = 0

LiNO3

4A-17

Sodium bicarbonateNa+ HCO3

-

(1+) + (1-) = 0

NaHCO3

barium hydroxideBa2+ OH-

(2+) + (1-) + (1-) = 0


BaOH2

4A-18

Ba(OH)2

NO!

zinc phosphateiron (III) nitrateFe3+ NO3

-

(3+) + (1-) + (1-) + (1-) = 0

Fe(NO3)2


4A-19

HYDRATESCompounds with water molecules trapped in their crystalsName ionic compound first, then a prefix for the number of waters, followed by -hydrate

1 mono2 di3 tri4 tetra5 penta

6 hexa7 hepta8 octa9 nona10 deca

4A-20

CuCl2.6H2O

copper (II) chloride hexahydrate

4A-21

iron (III) nitrate nonahydrateFe(NO3)3

.9H2O

COVALENT COMPOUNDS

NAMING BINARY COMPOUNDSName the 1st nonmetal as element name, using prefix if more than 1 atomName the 2nd nonmetal with –ide, always use a prefix

CO2

carbon dioxide

COcarbon monoxide

N2O

dinitrogen monoxide

4A-22

FORMULAS OF BINARY COMPOUNDSBase formulas on prefixes

Phosphorus triiodidePI3

diarsenic pentasulfide

4A-23

NAMING ACIDSARRHENIUS ACID – A compound that loses hydrogen ions in solutionARRHENIUS BASE – A compound that loses hydroxide ions in solutionOut of water – named as an ionic compound

HCl (g)hydrogen chloride

4A-24

Dissolved in water – name based on name of the acid’s anion

Anion in acid ends in –idehydro–root–ic acid

Anion in acid ends in –ateroot–ic acid

Anion in acid ends in –iteroot–ous acid

HBrBr-

bromide ionhydrobromic acid

4A-25




H2S

S2-

sulfide ionhydrosulfuric acid

4A-26




HNO3

NO3-

nitrate ionnitric acid

4A-27




H2SO4

SO42-

sulfate ionsulfuric acid

4A-28




H3PO3

PO33-

phosphite ionphosphorous acid

4A-29




FORMULAS OF ACIDS

hydrofluoric acidfluoride ionF-

HF

4A-30




FORMULAS OF ACIDS

carbonic acidcarbonate ionCO3

2-

H2CO3

4A-31




FORMULAS OF ACIDS

nitrous acidnitrite ionNO2

-

HNO2

4A-32

CHAPTER 5 - NOMENCLATURE IONIC COMPOUNDS NAMING Name the cation first, then name the anion second

Documents

Transcript of CHAPTER 5 - NOMENCLATURE IONIC COMPOUNDS NAMING Name the cation first, then name the anion second