INORGANIC NOMENCLATURE

Binary Compounds

This type of compound contains only two different elements in any ratio. Since these compounds are ionic in nature, they typically contain a metal and a non-metal.

Rules for Writing a Name from a Formula

1. Write down the name of the element with the lower the electronegativity (usually a metal) first.

2. Remove the ending of the name of the second element (usually the non-metal) and add “ide” ending.

Examples:a)KI

potassium iodide

b)AlCl3

aluminum chloride

I

c)Na2S

sodium sulfide

0

H

+1 -1

II

III

IV

V

VI

VII

He

Li

+1

Be

+2

B

+3

C

+4 -4

N

-3

O

-2

F

-1

Ne

Na

+1

Mg

+2

Al

+3

Si

+4 -4

P

-3

S

-2

Cl

-1

Ar

K

+1

Ca

+2

Ga

+3

Ge

+4

As

-3

Se

-2

Br

-1

Kr

Rb

+1

Sr

+2

In

Sn

+4

Sb

-3

Te

-2

I

-1

Xe

Cs

+1

Ba

+2

Tl

Pb

+4

Bi

-3

Po

-2

At

-1

Rn

Fr

+1

Ra

+2

Rules for Writing Formula from a Name

1. Write down the symbols for the two elements, in the order they appear in the name.

2. Place the charge of the first element above the first symbol.

3. Place the charge o f the second element above the second symbol.

4. Use the “criss-cross” rule and write the numbers as subscripts.

5. Reduce the subscript numbers to the simplest ratio.

Examples:a)rubidium nitrideRb1N3 ( Rb3N

b)magnesium phosphideMg2P3 (Mg3P2

c)calcium oxide

Ca2O2 (Ca2O2 ( CaO

Binary Compounds

Give the correct formula for the following:

1. Sodium sulfide

16.Silver bromide

2. Calcium phosphide

17.Beryllium fluoride

3. Hydrogen iodide

18.Lithium bromide

4. Magnesium hydride

19.Potassium phosphide

5. Barium oxide

20.Aluminum hydride

6. Barium chloride

21.Lithium oxide

7. Aluminum oxide

22.Barium bromide

8. Cadmium oxide

23.Aluminum sulfide

9. Francium oxide

24.Strontium nitride

10. Potassium oxide

25.Cadmium bromide

11. Silver sulfide

26.Magnesium phosphide

12. Zinc chloride

27.Cesium nitride

13. Calcium iodide

28.Zinc nitride

14. Rubidium fluoride

29.Lithium selenide

15. Calcium chloride

30.Beryllium telluride

Give the correct name for the following:

1. NaCl

16.SrCl2

2. MgO

17.Na2O

3. CaO

18.K3N

4. BBr3

19.Li3P

5. MgS

20.BaF2

6. CaCl2

21.MgI2

7. AlBr3

22.K2S

8. Rb3P

23.SrO

9. Al2O3

24.Al2S3

10. Li2O

25.SrF2

11. NaBr

26.Ag2S

12. Be3P2

27.RbI

13. BeF2

28.AlF3

14. AlCl3

29.MgO

15. HCl

30.KBr

Stock Naming and Formulae-Use of Roman Numerals

Some elements have more than one valence they may use when bonding. The Stock System uses Roman Numeral to indicate which valence the element is using in a particular compound. This is the preferred method for naming binary compounds.

The Roman numeral represents the valence of the FIRST element, that is, the element with 2 or more positive valences.

Rules for Writing a Name from a Formula

1. Write down the name of the first element. The is the element that may have more than one valence.

2. Include the Roman numeral to represent the valence of the first element (reverse the “criss-cross” to deterring the valence).

3. Remove the ending on the name of the second element and add the “ide” ending.

Examples:a)FeCl2Fe2 Cl1Iron (II) chloride

b)FeCl3Fe3Cl1iron (III) chloride

c)SnOSn1O1tin (II) oxide

* This is a special case- reversing the criss-cross tells us that the valences of the oxide is 1, which is NOT possible- the valence of the oxide MUST be 2. This formula must have been reduced to a simplest ratio. Therefore, reversing the criss-cross should give us: Sn2 O2, giving us the name tin (II) oxide.

Rules for writing a Formula From a Name

1. Write down symbols for the two element, ion the order they appear in the name.

2. Place the valence of the first element above the first symbol (Roman Numeral).

3. Place the valence of the second element above the second symbol.

4. Use the “criss-cross” rule and write the numbers as subscripts.

5. Reduce the subscript numbers to the simplest ratio.

Examples:a)Copper (II) oxide

Cu2O2( CuO

b)Chromium (III) sulfide

Cr3S2( Cr2S3

Stock Naming and Formulae – Using Roman Numerals

Give the correct formula for the following:

1. Copper (I) oxide

16.Manganese (III) oxide

2. Copper (II) oxide

17.Nickel (II) oxide

3. Tin (IV) chloride

18.Cobalt (III) fluoride

4. Mercury (II) bromide

19.Gold (I) bromide

5. Iron (III) fluoride

20.Lead (II) sulfide

6. Chromium (III) oxide

21.Iron (III) phosphide

7. Chromium (II) oxide

22.Antimony (III) bromide

8. Iron (II) chloride

23.Mercury (I) sulfide

9. Lead (IV) fluoride

24.Tin (II) phosphide

10. Iron (III) iodide

25.Nickel (III) sulfide

11. Lead (II) oxide

26.Tin (IV) oxide

12. Cobalt (II) nitride

27.Copper (I) iodide

13. Cobalt (III) sulfide

28.Tin (II) oxide

14. Antimony (III) chloride

29.Mercury (I) oxide

15. Bismuth (V) iodide

30.Bismuth (III) chloride

Give the correct name for the following:

1. SnF2

16. Cu2O

2. SnF4

17.HgI

3. Cu2S

18.Fe2S3

4. CuS

19.SbCl5

5. Cr2O3

20.CrCl2

6. SnS

21.Sb2S5

7. Fe2O3

22.Au2O3

8. HgCl2

23.NiO

9. CoCl3

24.SnF4

10. Co3N2

25.MnO2

11. PbO

26.NiCl2

12. Bi2S3

27.Cu3N2

13. CrCl3

28.Cu3N

14. Bi2O5

29.PbS

15. PbCl4

30.Ni2O3

The Prefix System

Another method of naming compounds in which the first element (usually P, S, C, N, Si) may have more than one valence is called the Prefix system. This method is used with compounds containing 2 non-metals.

Prefixes:

1mono-

6hexa-

2di-

7hepta-

3tri-

8octa-

4tetra-

9nona-

5penta-

10deca-

Rules for Writing a Name from a Formula

1. Write down the name as you did for binary compounds.

2. Include the prefix with the first element name that indicates how many of the first atoms are present. However, if there is only one atom, DO NOT use the mono- prefix!!

3. Include a prefix with the second element name that indicates how many of the second atom are present.

Examples:a)COcarbon monoxide

b)N2Odinitrogen monoxide

c)SO3sulfur trioxide

Rules for Writing a Formula from a Name

1. Just write what the name tells you.

Examples:a)dinitrogen tetroxide

N2O4

b)sulfur hexafluoride

SF6

c)diphophorous pentoxideP2O5

Give the correct formula:

Give the correct name:

1. Sulfur trioxide

1.CO2

2. Carbon monoxide

2.CO

3. Phosphorous triiodide

3.CS2

4. Silicon tetrafluoride

4.SO2

5. Sulfur dioxide

5.P2O3

6. Diphosphorous pentoxide

6.CCl4

7. Carbon tetraiodide

7.PCl3

8. Diphosphorous pentasulfide

8.SiO2

9. Sulfur hexabromide

9.P2O5

10. Silicon disulfide

10.SCl6

The “Ous” – “Ic” System

When the electropositive (first) element has 2 valences, “ous” denotes the LOWER and “ic” denotes the HIGHER. This system makes use of the Latin names of many of the metals.

Copper Cuprum

LeadPlumbum

Gold Aurum

IronFerrum

TinStannum

Rules for Writing a Name from a Formula

1. Write the name for the first element. Remove the ending and add either ‘-ous’ (if the element is using the lower valence) or ‘-ic’ (if the element is using the higher valence)

2. Write the name of the second element. Remove the ending and add ‘-ide’.

Examples:

a)PbBr2

plumbous bromide

b)PbBr4

plumbic bromide

Rules for Writing the Formula from the Name

1. Write down the symbols for the 2 elements, in the order they appear in the name.

2. Place the valence of the first element above the first symbol (‘-ous’ = lower valence, ‘-ic’ = higher valence).

3. Place the valence of the second element above the second symbol.

4. Use the ‘criss-cross’ rule and write the numbers as subscripts.

5. Reduce the subscript numbers to the simplest ratio.

Examples:

a)Stannous chlorideSn2 Cl1 ( SnCl2

b)Stannic chlorideSn4 Cl1 (SnCl4

Give the correct formula for the following

1. Mercuric oxide

11.Manganous sulfide

2. Cupric iodide

12.Arsenic oxide

3. Stannous chloride

13.Stannic iodide

4. Ferric chloride

14.Cuprous chloride

5. Aurous sulfide

15.Auric oxide

6. Plumbic fluoride

16.Chromic iodide

7. Nickelic oxide

17.Aurous bromide

8. Colbaltic chloride

18.Ferrous sulfide

9. Antimonic oxide

19.Mercurous oxide

Stannic oxide

20.Ferrous oxide

Give the correct name for the following:

1. CrO

11.NiO

2. Sb2O5

12.Fe2O3

3. PbCl4

13.FeS

4. Ni2O3

14.AuBr

5. PbF4

15.CrI3

6. As2S3

16.Au2O3

7. FeN

17.SnI4

8. SnCl2

18.MnS

9. CuI2

19.As2O5

10. HgO

20.CuCl2

Try These:

1. Stannous iodide

21.Antimonic oxide

2. Tin (IV) oxide

22.Bismuth (v) oxide

3. Manganous chloride

23.Arsenious bromide

4. Manganese (IV) sulfide

24.Copper (II) fluoride

5. Chromic oxide

25.Ferrous oxide

6. Phosphorous triiodide

26.Tin (II) bromide

7. Cuprous sulfide

27.Ferric oxide

8. Copper (II) oxide

28.Gold (III) sulfide

9. Mercuric oxide

29.Mercurous hydride

10. Silicon dioxide

30.Manganese (IV) oxide

11. Mercurous sulfide

31.Mercuric bromide

12. Iron (III) oxide

32.Copper (I) iodide

13. Cupric fluoride

33.Plumbous oxide

14. Antimony (V) oxide

34.Lead (IV) sulfide

15. Stannous fluoride

35.Plumbic sulfide

16. Antimony (III) oxide

36.Arsenic (V) oxide

17. Diphosphorous pentoxide

37.Bismuthous fluoride

18. Tin (IV) sulfide

38.Carbon monoxide

19. Manganic sulfide

39.Arsenious sulfide

20. Lead (II) chloride

40.Phosphorous pentafluoride

SOME EXCEPTIONS….

a) PEROXIDES

To write the formula of a peroxide, simply write the formula of the ordinary oxide (1.e. cover up the prefix “per”). Cancel as usual if necessary, then add one oxygen atom and after adding the one extra oxygen atom DO NOT CANCEL!!

Examples:a)Sodium oxide

Na2O

c)hydrogen oxide

H2O

Sodium peroxide Na2O2

hydrogen peroxideH2O2

b)Barium oxide

BaO

d)lead (II) oxide

PbO

Barium peroxideBaO2

lead (II) peroxidePbO2

b) VALENCE OF FIRST ELEMENT NOT INDICATED

In compounds of copper, lead and manganese, the valence of the metal is often not revealed in the name of the compound. In such a case, use the most common valence which is +2 for Cu, Pb, and Mn ONLY!!

Examples:a)Manganese bromideMnBr2 (Mn has a most common valence of +2)

b)Copper chlorideCuCl2(Cu has a most common valence of +2)

c)Lead iodide

PbI2(Pb has a most common valence of +2)

** REMEMBER when finding the valence from the formula, you should keep in mind that the formula may be in reduced form.

Example:PbO2

What is the valence of Pb?

Pb2 O1

This indicates that the oxide has a valence of -1. We know that this is not true, as oxide has a valence of -2. The formula MUST be in reduced form, and therefore, Pb must have a valence of +4.

Write formulas for the following:

1. Antimony (III) oxide

11.Beryllium peroxide

2. Stannous fluoride

12.Silver peroxide

3. Ferrous phosphide

13.Mercury (II) hydride

4. Iron (III) sulfide

14.Iron (II) nitride

5. Mercurous oxide

15.Lead (IV) fluoride

6. Iron (II) nitride

16.Aluminum chloride

7. Manganese (IV) sulfide

17.Magnesium oxide

8. Copper sulfide

18.Sulfur dioxide

9. Manganese fluoride

19.Carbon dioxide

10. Copper iodide

20.Manganese dioxide

Name the following:

1. H2O2

18.MnO2

2. P2O5

19.PbO

3. P2S3

20.Sn3N4

4. CO2

21.Pb3P2

5. SO2

22.Mg3N2

6. CuS

23.K2O2

7. MnO

24.Na2O2

8. CaO2

25.BeI2

9. CO

26.P2S3

10. HgO

27.CuO

11. AgBr

28.MnBr4

12. PbS

29.SO3

13. Fe2S3

30.PbO

14. BeS

31.HgI

15. MgO

32.CuBr

16. AlI3

33.MgO2

17. HF

34.Sb3P5

SOME EXTRA PRACTICE……

1. Silver fluoride

8.Lead fluoride

2. Arsenic (V) sulfide

9.Copper bromide

3. Copper (II) peroxide

10.Manganese chloride

4. Copper oxide

11.Magnesium sulfide

5. Magnesium peroxide

12.Aluminum peroxide

6. Lead oxide

13.Calcium peroxide

7. Copper sulfide

14.Tin (II) peroxide

THE OXY ACIDS

Points to remember…..

1. All acids contain the element hydrogen (H)

2. All oxy acids contain the element oxygen in addition to hydrogen

3. All oxy acids contain 3 elements

4. All oxy acids have derivatives and are members of a family of acids.

5. The main oxy acids are those listed below:

OXY ACIDS

1. Sulphuric acid – H2SO4

5.Chloric acid – HClO3

2. Phosphoric acid – H3PO4

6.Fluoric acid – HFO3

3. Nitric acid – HNO3

7.Bromic acid – HBrO3

4. Carbonic acid – H2CO3

8.Iodic acid – HIO3

The above acids are the SECOND member of a family of acids all of which are derived from the main oxy acid listed above. Examples:

Persulphuric acid- H2SO5

Perchloric acid

- HClO4

*sulphuric acid - H2SO4

* chloric acid

- HClO3

Sulphurous acid- H2SO3

chlorous acid

- HClO2

Hyposulphurous acid- H2SO2

hypochlorous acid- HClO

Hydrosulphuric acid - H2S

hydrochloric acid - HCl

NOTE: All HYDRO acids contain NO OXYGEN

RADICALS OR IONS FROM OXY ACIDS

A RADICAL is a group of atoms acting as one unit which contains an electrical charge.

An ION is an electrically charged particle which may consist of a group of atoms or single atoms with either a positive electrical charge (deficiency of electrons) or a negative electrical charge (surplus of electrons).

If an acid loses all or part of its hydrogen either an ion or radical remains. These ions or radicals have names and valences. The valences of these ions or radicals need NOT be remembered because the valence of these ions or radicals is always equal to the number of hydrogen atoms which the ion or radical was combined in the original parent acid from which it was formed.

ACID NAME

ACID FORMULA

ION NAME

ION FORMULA

Perchloric acid

Chloric acid

Chlorous acid

Hypochlorous acid

Hydrochloric acid

Pernitric acid

Nitric acid

Nitrous acid

Persulphuric acid

Sulphuric acid

Sulphurous acid

Hyposulphurous acid

Hydrosulphuric acid

Perphosphoric acid

Phosphoric acid

Phosphorous acid

Hypophosphorous acid

Hydrophosphoric acid

Perfluoric acid

Fluoric acid

Fluorous acid

Hypofluorous acid

Hydrofluoric acid

ACID NAME

ACID FORMULA

ION NAME

ION FORMULA

Perbromic acid

Bromic acid

Bromous acid

Hypobromous acid

Hydrobromic acid

Percarbonic acid

carbonic acid

carbonous acid

Periodic acid

Iodic acid

Iodous acid

Hypoiodous acid

Hydroiodic acid

CONGRATULATIONS! You’ve made it to the half way point

A. SYMBOLS AND VALENCES – Do you know them? To be successful in nomenclature, knowing your symbols is absolutely essential.

B. Simple Binary Compounds

1. Sodium oxide

4.Potassium sulphide

2. Aluminum chloride

5.Barium nitride

3. Lithium phosphide

6.Magnesium fluoride

C.More Complex Binary Compounds

Use of Roman Numerals

1. Nickel (II) chloride

4.Manganese (II) iodide

2. Lead (IV) sulphide

5.Gold (III) oxide

3. Copper (II) oxide

6.Antimony (III) phosphide

Use of Prefixes

1. Sulphur dioxide

4.Carbon disulphide

2. Phosphorous pentoxide

5.Phosphorous trioxide

3. Phosphorous trichloride

6.Sulphur trioxide

Peroxides and valences of the first element not indicated

1. Sodium peroxide

5.Hydrogen peroxide

2. Calcium peroxide

6.Copper (II) peroxide

3. Copper sulphide

7.Lead oxide

4. Manganese nitride

8.Copper chloride

D.The Oxy Acids – DO YOU KNOW THE BIG FIVE? You MUST learn them.

1. Sulphuric acid

2. Nitric acid

3. Carbonic acid

4. Phosphoric acid

5. Chloric acid

HOW ABOUT

1. Fluoric acid

2. Bromic acid

3. Iodic acid

** For practice, write out the names and formulae for the complete series of the phosphoric acid family, the carbonic acid family, and the nitric acid family. Beside each formula also write: The radical formula, the radical name, and the radical valence.

NOTE: The nitric and carbonic acid families are incomplete and only the first 3 members need be written, the others don’t actually exist.

SALTS OF THE OXY ACIDS

A SALT is a compound formed by replacing all or part of the available hydrogen of an acid by a METAL or an ELECTROPOSITIVE RADICAL.

e.g. Calcium phosphate

Ca2++ PO43- (Ca3(PO4)2

(from H3PO4)

Examples:

Name

Formula

Name

Formula

Calcium sulfate

CaSO4

Arsenic Phosphate

As3(PO4)5

Sodium chlorite

NaClO2

Antimony (III) HypochloriteSb(ClO)3

Aluminum nitrate

Al(NO3)3

Cupric nitrite

Cu(NO2)2

Ferric sulphate

Fe2(SO4)3

Mercurous perchlorate

HgClO4

Zinc carbonate

ZnCO3

Potassium chlorate

KClO3

Lead sulfate

PbSO4

stannic phosphite

Sn3(PO3)4

Manganese nitrite

Mn(NO2)2

Bismuth (V) sulfite

Bi2(SO3)5

Write the formulae for:

1. Mercurous perphosphate

39.Arsenious sulphate

2. Arsenious persulphate

40.Antimonic perchlorate

3. Bismuth (V) sulphate

41.Lead (II) iodate

4. Calcium percarbonate

42.Silver sulphide

5. Stannous perchlorate

43.Magnesium nitride

6. Silver hyposulphite

44.Iron (III) phosphide

7. Barium chlorite

45.Copper (I) hyposulphite

8. Lithium chlorate

46.Stannic nitrate

9. Magnesium sulphite

47.Hydrogen sulphate

10. Manganese hypophosphite

48.Hydrogen nitrate

11. Copper sulphate

49.Lithium carbonate

12. Lead (II) carbonate

50.Barium pernitrate

13. Aluminum sulphite

51.Silver persulphate

14. Lithium nitrate

52.Lead sulphide

15. Barium phosphate

53.Copper phosphate

16. Magnesium sulphide

54.Manganese perphosphate

17. Copper phosphide

55.Antimony (III) nitrate

18. Cupric sulphite

56.Aurous nitrate

19. Mercurous hypochlorite

57.Bismuth (III) sulphate

20. Tin (II) carbonate

58.Lead nitrate

Nomenclature – Part II

21. Lead (IV) chlorite

59.Arsenic (V) iodate

22. Plumbous carbonite

60.Tin (IV) fluorate

23. Stannic percarbonate

61.Ferrous periodate

24. Potassium hypochlorite

62.Stannic sulphate

25. Silver phosphite

63.Mercuric hypobromite

26. Iron (II) hyposulphite

64.Bismuth (III) sulphite

27. Sodium pernitrate

65.Radium percarbonate

28. Potassium chlorate

66.Zinc iodate

29. Magnesium nitrate

67.Barium carbonate

30. Sodium carbonate

68.Calcium carbonate

31. Stannous sulphate

69.Stannous sulphite

32. Ferric sulphite

70.Copper sulphide

33. Manganese (IV) nitrate

71.Lead phosphate

34. Sodium hypochlorite

72.Lead phosphide

35. Calcium phosphate

73.Manganese sulphide

36. Aluminum nitrate

74.Potassium bromate

37. Cupric phosphate

75.Aurous fluoride

38. Copper (I) hyposulphite

76.Boron nitrite

Give the name for the following compounds:

1. AsPO3

11.NiSO3

2. Al(NO3)3

12.Fe(ClO2)3

3. MnSO3

13.Sn3(PO4)4

4. AgClO

14.Pb(ClO)2

5. AuF3

15.Ba(ClO3)2

6. Mg(ClO4)2

16.Al(ClO3)3

7. LiNO3

17.K2CO4

8. PbCO3

18.Ag2SO3

9. AgFO

19.KClO

10. MgCO4

20.NaNO2

1. AMMONIUM RADICAL: NH4+; Valence of +1. Derivative of ammonia gas (NH3)

Examples:Ammonium chloride

NH4Cl

Ammonium sulphate

(NH4)2SO4

Ammonium phosphate

(NH4)3PO4

Ammonium nitrate

NH4NO3

2. HYDROXIDE RADICAL: OH-; Valence of -1. A component of ALL bases.

Examples:Sodium hydroxide

NaOH

Ammonium hydroxide

NH4OH

Iron (II) hydroxide

Fe(OH)2

Copper (I) hydroxide

CuOH

3. ACETATE RADICAL:CH3COO-; Valence of -1

Derived from the oxy acid, Acetic acid (CH3COOH)

Examples: Calcium acetate

(CH3COO)2Ca

Iron (II) acetate

(CH3COO)2Fe

Tin (IV) acetate

(CH3COO)4Sn

Ammonium acetate

CH3COONH4

4. PERMANGANATE RADICAL: MnO4-; Valence of -1

Examples: Potassium permanganateKMnO4

Mercury (II) permanganateHg(MnO4)2

5. DICROMATE RADICAL: Cr2O72-; Valence of -2

Examples: Potassium dichromate

K2Cr2O7

Ammonium dichromate

(NH4)2Cr2O7

6. CHROMATE RADICAL: CrO42-; Valence of -2

Examples: Copper (I) chromate

Cu2CrO4

Mercury (II) chromate

HgCrO4

7. CYANIDE RADICAL:CN-1; Valence of -1

Examples: Copper (I) cyanide

CuCN

Mercury (II) cyanide

Hg(CN)2

Give the name for the following compounds:

1. Manganese dichromate

21.Calcium carbonate

2. Gold (I) permanganate

22.Potassium cyanide

3. Iron (III) chromate

23.Barium carbonate

4. Antimony (III) acetate

24.Zinc permanganate

5. Iron (II) hydroxide

25.Ammonium percarbonate

6. Calcium acetate

26.Bismuth (III) sulphite

7. Lithium hydroxide

27.Mercury (II) hypobromite

8. Aluminum acetate

28.Tin (IV) sulphate

9. Sodium hydroxide

29.Iron (II) cyanide

10. Ammonium acetate

30.Tin (IV) fluorate

11. Silver acetate

31.Arsenic (V) iodate

12. Silicon fluoride

32.Lead permanganate

13. Iron (II) cyanide

33.Bismuth (III) sulphate

14. Zinc bromide

34.Silver nitrate

15. Potassium dichromate

35.Zinc hydroxide

16. Manganese sulphide

36.Mercury (II) hydroxide

17. Lead phosphide

37.Ammonium hydroxide

18. Lead cyanide

38.Beryllium permanganate

19. Copper sulphide

39.Tin (II) acetate

20. Tin (II) sulphite

40.Lead (IV) hydroxide

Give the name for the following compounds:

1. (NH4)3PO2

13.CaSO5

2. SnCr2O7

14.Ag2CrO4

3. (CH3COO)2Ca

15.NH3

4. Ni(MnO4)3

16.CuSO4

5. CuOH

17.Pb(FO3)2

6. Pb(CrO4)2

18.NH4NO3

7. (NH4)2S

19.Ca(OH)2

8. NH4ClO

20.Fe2(Cr2O7)3

9. Mn(OH)2

21.NH4ClO3

10. (CH3COO)3Al

22.Pb(OH)4

11. Sb(OH)5

23.CH3COONa

12. Na3PO2

24.CH3COOAg

ACID SALTS (Use of the Prefix “bi”

ACID SALT – and acid salt is one which contains hydrogen in its radical

Acid salts result when dibasic acids (one containing 2 hydrogen atoms like H2SO4) or tribasic acids (like H3PO4) do not always lose all of their hydrogen atoms when forming a salt. Examples:

ACID FORMULA

IONS OR RADICALS

VALENCE OF ION OR RADICAL

COMMON NAME OF ION OR RADICAL

PREFERRED NAME OF ION OR RADICAL

H2SO4

SO4

HSO4

-2

-1

Sulphate

Bisulphate

Sulphate

Hydrogen sulphate

H2SO3

SO3

HSO3

-2

-1

Sulfite

Bisulfite

Sulfite

Hydrogen sulfite

H2CO3

CO3

HCO3

-2

-1

Carbonate

bicarbonate

Carbonate

Hydrogen carbonate

H3PO4

PO4

HPO4

H2PO4

-3

-2

-1

Phosphate

Monohydrogen phosphate

Dihydrogen phosphate

Phosphate

Monohydrogen phosphate

Dihydrogen phosphate

H3PO3

PO3

HPO3

H2PO3

-3

-2

-1

Phosphite

Monohydrogen phosphite

Dihydrogen phosphite

Phosphite

Monohydrogen phosphite

Dihydrogen phosphite

H3PO2

PO2

HPO2

H2PO2

-3

-2

-1

hypophosphite

Monohydrogen hypophosphite

Dihydrogen hypophosphite

hypophosphite

Monohydrogen hypophosphite

Dihydrogen hypophosphite

SOME ACID SALTS – Examples

Sodium bicarbonate – NaHCO3

Iron (II) bisulphite – Fe(HSO3)2

Copper hydrogen carbonate – Cu(HCO3)2

Tin (IV) bisulphate – Sn(HSO4)4

Potassium monohydrogen hypophosphite – K2HPO2

Lead bicarbonate – Pb(HCO3)2

Ammonium dihydrogen perphosphate – NH4H2PO5

Lithium hydrogen carbonate – LiHCO3

Give names for the following formulae:

1. Pb(HCO3)4

6.Pb(HSO5)2

2. As(HSO3)3

7.(NH4)2HPO5

3. Sn(HSO4)4

8.NaHCO3

4. Fe2(HPO2)3

9.KHSO3

5. Mn(H2PO3)2

10.LiHCO3

Give formulae for the following compounds:

1. Silver hydrogen sulphate

2. Potassium bicarbonate

3. Lead (IV) monohydrogen phosphite

4. Iron (II) dihydrogen phosphate

5. Potassium carbonate

6. Tin (II) phosphite

7. Iron (II) phosphite

8. Magnesium persulphate

9. Sodium monohydrogen perphosphate

10. Ammonium hypofluorite

11. Tin (II) permanganate

12. Manganese nitrite

13. Copper sulphate

14. Ammonium dihydrogen hypophosphite

15. Bismuth (III) hydrogen carbonate

16. Potassium hydrogen persulphate

17. Aluminum hydrogen sulphite

18. Copper (II) bicarbonate

19. Antimony (V) monohydrogen perphosphate

20. Tin (IV) hydrogen sulphite

21. Iron (III) hydrogen percarbonate

22. Calcium bicarbonate

23. Aluminum bisulphate

24. Manganese bicarbonate

25. Lead monohydrogen phosphate

26. Copper dihydrogen phosphite

27. Nickel (II) monohydrogen perphosphate

28. Zinc monohydrogen hypophosphite

29. Mercury (I) dihydrogen phosphite

30. Ammonium monohydrogen hypophosphite

31. Ammonium dihydrogen hypophosphite

32. Barium bisulphate

33. Arsenic (III) bisulphite

Hydrates

Hydrate:a compounds containing water of hydration (a definite, chemically combined proportion of water)

Examples:

Copper sulphate pentahydrate

CuSO4 ( 5H2O

Sodium sulphate decahydrate

Na2SO4 ( 10H2O

Magnesium sulphate heptahydrte

MgSO4 ( 7H2O

Give the name for the following formulae:

1. Fe2(HPO2)3 ( 5H2O

2. Mn(H2PO3)2 ( 6H2O

3. Pb(HSO5)2 ( 2H2O

4. (NH4)2HPO5 ( 7H2O

5. Sn(MnO4)2 ( 2H2O

6. KHSO5 ( H2O

7. Al(HSO3)3 ( 8H2O

8. Cu(HCO3)2 ( 3H2O

9. NH4H2PO2 ( 3H2O

10. (NH4)2HPO2 ( 4H2O

Give the formulae for the following compounds:

1. Potassium carbonate monohydrate

2. Tin (II) phosphite heptahydrate

3. Ferrous phosphite hexahydrate

4. Magnesium persulphate tetrahydrate

5. Sodium perphosphate nonahydrate

6. Ammonium hypofluorite trihydrate

7. Manganese nitrite octahydrate

8. Cupric sulphate pentahydrate

9. Ammonium dihydrogen perphosphate hexahydrate

10. Bismuth (III) hydrogen carbonate dihydrate

THE DIATOMIC GASES

The molecules of these gases (elemental) consist of pairs of identical atoms. KNOW THEM!!

Remember CHINBOF or the “Seven Sisters”

Chlorine gasCl2 (g)

Bromine vapour

Br2 (g)

Hydrogen gas H2 (g)

Oxygen gas

O2 (g)

Iodine gas

I2 (g)

Fluorine gas

F2 (g)

Nitrogen gas N2 (g)

MONATOMIC GASES – THE INERT NOBLE GASES

Because of their stable electron configurations, these gases remain as discrete monatomic particles (** Some of them have been made to react in a laboratory)

Helium

He (g)

Krypton Kr (g)

Neon

Ne (g)

Xenon

Xe (g)

Argon

Ar (g)

Radon

Rn (g)

BINARY ACIDS

Certain gases dissolve in water to form acids have the SAME formula

NAME OF GAS

FORMULA

NAME OF ACID

FORMULA

Hydrogen chloride

HCl (g)

Hydrochloric acid

HCl (aq)

Hydrogen bromide

HBr (g)

Hydrobromic acid

HBr (aq)

Hydrogen iodide

HI (g)

Hydroiodic acid

HI (aq)

Hydrogen fluoride

HF (g)

Hydrofluoric acid

HF (aq)

Hydrogen sulphide

H2S (g)

Hydrosulfuric acid

H2S (aq)

Hydrogen cyanide

HCN (g)

Hydrocyanic acid

HCN (aq)

** Formation of the salts for these acids has been covered under “Binary Compounds”.

THE END!!!

OTHER RADICALS

1