Naming Compounds

Chapter 6(Chapter 9)

Rules for Naming CompoundsFormula begins with a metal Formula does NOT begin with a metal

‘H’ in front NO ‘H’ in front

1)Metal name *

2) Polyatomic name

1) Metal name *

2) Non metal ROOT + IDE

Only 2 elements More than 2 elements

1) Name 1st element

2) 2nd element ROOT + IDE

3) Prefix needed for subscripts

(di, tri, tetra, penta, hexa, hepta, octa, nona, deca)

Only 2 elements More than 2 elements

1) Write HYDRO

2) 2nd element ROOT + IC

3) Write ACID

Polyatomic ends with ATE

Polyatomic ends with ITE

1) Polyatomic ROOT + IC

2) Write ACID

1)Polyatomic ROOT + OUS

2)Write ACID

Classic Names: add –OUS for lower charge/ -IC for higher charge to these roots

(NH4+ acts like a metal)

*These metals use a Roman Numeral after their name to indicate it’s charge

Copper (I) – Cu+1

Copper (II)- Cu+2

Mercury(I) – Hg2+2

Mercury(II) – Hg+2

Iron(II) – Fe+2

Iron (III) – Fe+3

Chromium (II) – Cr+2

Chromium(III) – Cr+3

Manganese(II) – Mn+2

Manganese(III) – Mn+3

Cobalt(II) – Co+2

Cobalt(III) – Co+3

Lead(II) – Pb+2

Lead(IV) – Pb+4

Tin(II) – Sn+2

Tin(IV) – Sn+4

Cupr -Mercur -

Ferr -Chrom -Mangan -Cobalt -

Plumb -Stann -

K2SO4

Potassium sulfate

CaC2O4

Calcium oxalate

H2SO3

Sulfurous acid

(NH4)2S

Ammonium sulfide

Mg(HCO3)2

Magnesium hydrogen carbonate

CCl4

Carbon tetrachloride

P2O5

Diphosphorous pentoxide

NO2

Nitrogendioxide

SF6

sulfurhexafluoride

H2C2O4

Oxalic acid

Al(C2H3O2) 3

Aluminumacetate

H3PO4

Phosphoric Acid

HF

Hydrofluoric Acid

Ba(ClO)2

Barium hypochlorite

LiBr

Lithium bromide

HClO4

Perchloric acid

Rb2O

Rubidium oxide

Sr(OH)2

Strontium hydroxide

KMnO4

Potassium permanganate

NaCN

Sodium cyanide

Ca(HSO3)2

Calcium hydrogen sulfite

Ba(NO3)2

Barium nitrate

H3PO3

Phosphorous acid

Ag2CrO4

Silver chromate

ZnCO3

Zinc carbonate

SO3

Sulfur trioxide

BeSe

Beryllium selenide

AlN

Aluminum nitride

NH4C2H3O2

Ammonium acetate

PCl3

Phosphorous trichloride

K2HPO3

Potassium hydrogen phosphite

H2SO4

Sulfuric acid

H2S

Hydrosulfuric acid

(NH4)2C2O4

Ammonium oxalate

HNO2

Nitrous acid

Al2(SO4)3

Aluminum sulfate

LiClO2

Lithium chlorite

Ag2Cr2O7

Silver dichromate

Hl

Hydroiodic acid

NaClO

Sodium hypochlorite

NI3

Nitrogen triodide

H2CrO4

Chromic acid

Rules for Naming CompoundsFormula begins with a metal Formula does NOT begin with a metal

‘H’ in front NO ‘H’ in front

1)Metal name *

2) Polyatomic name

1) Metal name *

2) Non metal ROOT + IDE

Only 2 elements More than 2 elements

1) Name 1st element

2) 2nd element ROOT + IDE

3) Prefix needed for subscripts

(di, tri, tetra, penta, hexa, hepta, octa, nona, deca)

Only 2 elements More than 2 elements

1) Write HYDRO

2) 2nd element ROOT + IC

3) Write ACID

Polyatomic ends with ATE

Polyatomic ends with ITE

1) Polyatomic ROOT + IC

2) Write ACID

1)Polyatomic ROOT + OUS

2)Write ACID

Classic Names: add –OUS for lower charge/ -IC for higher charge to these roots

(NH4+ acts like a metal)

*These metals use a Roman Numeral after their name to indicate it’s charge

Copper (I) – Cu+1

Copper (II)- Cu+2

Mercury(I) – Hg2+2

Mercury(II) – Hg+2

Iron(II) – Fe+2

Iron (III) – Fe+3

Chromium (II) – Cr+2

Chromium(III) – Cr+3

Manganese(II) – Mn+2

Manganese(III) – Mn+3

Cobalt(II) – Co+2

Cobalt(III) – Co+3

Lead(II) – Pb+2

Lead(IV) – Pb+4

Tin(II) – Sn+2

Tin(IV) – Sn+4

Cupr -Mercur -

Ferr -Chrom -Mangan -Cobalt -

Plumb -Stann -

CuBr2

Copper(II) bromide

Cupric bromide

Fe(NO3)3

Iron (III) nitrate

Ferric nitrate

SnF2

Tin(II) fluoride

Stannous fluoride

PbI2

Lead(II) Iodide

Plumbous Iodide

Co(NO2)2

Cobalt(II) nitrite

Cobaltous nitrite

FeO

Iron(II) oxide

Ferrous oxide

Fe2(SO4)3

Iron(III) sulfate

CuC2O4

Cupric oxalate

PbO2

Lead(IV) oxide

When +4 and -2 charges are paired up, REDUCE the subscripts to ‘1’ and ‘2’