IIIIIIIV Chemical Nomenclature I. Ions to Know II. Molecular Compounds III. Ionic Compounds IV.Acids.

I II III IV

Chemical Nomenclature

I. Ions to KnowII. Molecular Compounds

III. Ionic CompoundsIV.Acids

I. Ions to Know

+1   -1   -2   -3  

NH4+ Ammonium ion OH- Hydroxide ion C2O4

-2 Oxalate ion PO4-3 Phosphate ion

H3O+ Hydronium ion CN- Cyanide ion CrO4-2 Chromate ion PO3

-3 Phosphite ion

Hg2+2 Mercury (I) ion HCO3

- Bicarbonate ion Cr2O7-2 Dichromate ion AsO4

-3 Arsenate ion

    C2H3O2- Acetate ion O2

-2 Peroxide ion    

    NO3- Nitrate ion CO3

-2 Carbonate ion    

    NO2- Nitrite ion SO4

-2 Sulfate ion    

    ClO4- Perchlorate ion SO3

-2 Sulfite ion    

    ClO3- Chlorate ion        

    ClO2- Chlorite ion        

    ClO- Hypochlorite ion        

    BrO4- Perbromate ion        

    BrO3- Bromate ion        

    BrO2- Bromite ion        

    BrO- Hypobromite ion        

    IO4- Periodate ion        

    IO3- Iodate ion        

    IO2- Iodite ion        

    IO- Hypoiodite ion    

II. Molecular Nomenclature

Prefix System (binary compounds)

1. Less e-neg atom comes first.

2. Add prefixes to indicate # of atoms. Omit mono- prefix on first element.

3. Change the ending of the second element to -ide.

PREFIXmono-di-tri-tetra-penta-hexa-hepta-octa-nona-deca-

NUMBER123456789

10

II. Molecular Nomenclature

CCl4

N2O

SF6

carbon tetrachloride

dinitrogen monoxide

sulfur hexafluoride

II. Molecular Nomenclature

arsenic trichloride

dinitrogen pentoxide

tetraphosphorus decoxide

AsCl3

N2O5

P4O10

II. Molecular Nomenclature

N O F

Cl

Br

I

H

II. Molecular Nomenclature

The Seven Diatomic Elements

Br2 I2 N2 Cl2 H2 O2 F2

III. Ionic Nomenclature

Ionic Formulas

Write each ion, cation first. Don’t show charges in the final formula.

Overall charge must equal zero. If charges cancel, just write symbols. If not, use subscripts to balance charges.

Use parentheses to show more than one polyatomic ion.

Stock System - Roman numerals indicate the ion’s charge.

III. Ionic Nomenclature

Ionic Names

Write the names of both ions, cation first.

Change ending of monatomic ions to -ide.

Polyatomic ions have special names.

Stock System - Use Roman numerals to show the ion’s charge if more than one is possible. Overall charge must equal zero.

III. Ionic Nomenclature

Consider the following: Does it contain a polyatomic ion?

-ide, 2 elements no-ate, -ite, 3+ elements yes

Does it contain a Roman numeral?Check the table for metals not in Groups 1 or 2.

No prefixes!

Common Ion Charges

1+

2+ 3+ NA 3- 2- 1-

0

III. Ionic Nomenclature

potassium chloride

magnesium nitrate

copper(II) chloride

K+ Cl

Mg2+ NO3

Cu2+ Cl

KCl

Mg(NO3)2

CuCl2

III. Ionic Nomenclature

NaBr

Na2CO3

FeCl3

sodium bromide

sodium carbonate

iron(III) chloride

III. Ionic Nomenclature

IV. Acid Nomenclature

Acids – What are they?

Compounds that form H+ in water.

Formulas usually begin with ‘H’.

Examples:

HCl (aq)– hydrochloric acid

HNO3 (aq)– nitric acid

H2SO4 (aq)– sulfuric acid

Anion Ending Acid Name

-ide hydro-(stem)-ic acid

-ate (stem)-ic acid

-ite (stem)-ous acid

IV. Acid Nomenclature

IV. Acid Nomenclature

h yd ro - p re fix-ic en d in g

2 e lem en ts

-a te en d in gb ecom es-ic en d in g

-ite en d in gb ecom es

-o u s en d in g

n o h yd ro - p re fix

3 e lem en ts

AC ID Ss ta rt w ith 'H '

HBr

H2CO3

H2SO3

2 elements, -ide

3 elements, -ate

3 elements, -ite

hydrobromic

acid

carbonic

acid

sulfurous

acid

IV. Acid Nomenclature

hydrofluoric acid

sulfuric acid

nitrous acid

2 elements

3 elements, -ic

3 elements, -ous

HF (aq)

H2SO4

HNO2

IV. Acid Nomenclature

H+ F-

H+ SO42-

H+ NO2-

(aq)

(aq)