1  

Chemical Nomenclature Contents: I. Types of Chemical Compounds 1. Classifying rules

2. Categorize: ionic or covalent 3. Categorize: binary or ternary

II. Naming Ions 1. Monatomic Anions* 2. Monatomic Cations* 3. Polyatomic Anions and Cations* III. Naming Ionic Compounds 1. Rules 2. Binary ionic compounds* 3. Ternary ionic compounds* 4. Random (binary and ternary) ionic compounds* IV. Naming Molecular Compounds 1. Rules 2. Practice* V. Naming Acids 1. Naming rules 2. Practice* VI. Naming Hydrates 1. Naming rules 2. Hydrate practice* * Determine name when given formula Determine formula when given name Chapter Review Problems

 2  

I. Types of Chemical Compounds Classifying rules Ionic compounds contain metal and non-metals Covalent (molecular) compounds contain only non-metals Classify the following compounds as ionic or molecular 1. CaCl2 _________________ 11. MgO __________________

2. CO2 _________________ 12. NH4Cl __________________

3. H2O _________________ 13. Sr(NO3)2 _________________

4. Na2SO4 _________________ 14. KI __________________

5. K2O _________________ 15. Ba(OH)2 _________________

6. NaF _________________ 16. NO2 __________________

7. Na2CO3 _________________ 17. Ca3(PO4)2 ________________

8. CH4 _________________ 18. FeCl3 __________________

9. Mg(NO3)2 ________________ 19. P2O5 __________________

10. LiBr _________________ 20. N2O3 __________________

Classifying rules Binary ionic compounds contain one atom (monatomic) ions only Example: Rb2O contains two Rb+ cations and one O2- anion Ternary ionic compounds contain at least one polyatomic ion Example: RbNO3 contains one Rb+ cation and one NO3

2- anion Classify the following as binary ionic or ternary ionic 21. KOH _________________ 26. Na2Cr2O7 ________________

22. CoO _________________ 27. MgSO4 __________________

23. Fe(NO3)2 ________________ 28. Cu2S ___________________

24. MgH2 __________________ 29. SnO2 ___________________

25. Cs2S _________________ 30. NH4NO3 _________________

  3  

II. Naming Ions   Rules for Monatomic Anions When naming, take the non-metal name, remove the ending and replace with it with “-ide” and then write the word “ion” When writing the formula, remove the “ide” and find the charge the atom will take as an ion on the periodic table. Write it as a superscript. Together 1. S2-

_________________ 3. bromide ion _____________

2. N3- _________________ 4. telluride ion _____________

You try it 5. F-

_________________ 7. iodide ion _________________

6. N3- _________________ 8. selenide __________________

Rules for Monatomic Cations Rule A When naming, if the atom only takes one charge when forming an ion, simply write the name of the atom and then write “ion” When writing the formula, look up the charge from the periodic table and write it as a superscript above the elements symbol. 9. Na+

_________________ 11. aluminum ion ____________

10. Mg2+ _________________ 12. silver ion ____________

Rule B When naming, if the atom can form more than one charge when forming an ion, take the name of the atom that the ion is formed from, place the charge as a Roman numeral in parentheses, and then add “ion”. When writing the formula, write the symbol with the positive charge as a superscript indicated in the parentheses. 13. Pb2+

_________________ 15. copper (I) ion ____________

14. Fe2+ _________________ 16. copper (II) ion___________

 4  

Monatomic ion and cation practice 1. N3-

_________________

2. lithium ion _________________

3. Ni+ _________________

4. oxide ion _________________

5. Cl- _________________

6. sulfide ion _________________

7. Ag+ _________________

8. zinc ion _________________

9. cobalt (II) ion _________________

10. fluoride ion _________________ Rules for Polyatomic Ions (both Anion and Cation) When naming, look up the name on the periodic table (often these names end in “-ite” or “-ate”, common exception is hydroxide OH-) When writing the formula, look up the formula on the periodic table 9. NO3

- _________________ 13. perchlorate ion ____________

10. NH4+

_________________ 14. sulfate ion ____________

11. OH- _________________ 15. carbonate ion ____________

12. PO43-

_________________ 16. acetate ion ____________

  5  

Naming Ions Review Formula to name 1. Ca2+

_________________

2. O2- _________________

3. H+ _________________

4. Cu+ _________________

5. Fe3+ _________________

6. CO32+

_________________

7. NH4+

_________________

8. Zn2+ _________________

9. N3- _________________

10. Cl- _________________

11. F- _________________

12. Zr4+ _________________

Name to formula 13. sodium ion _________________

14. phosphide ion _________________

15. phosphate ion _________________

16. iron (II) ion _________________

17. strontium ion _________________

18. nickel (II) ion _________________

19. tin (II) ion _________________

20. sulfate ion _________________

21. sulfite ion _________________

22. sulfide ion _________________

23. iridium ion _________________

24. potassium ion _________________

 6  

III. Naming Ionic Compounds

When writing the formula: When ions combine, they form neutral compounds. These formulas are written in lowest, whole-number ratios. These formulas are called formula units. An ionic compound is referred to as a salt. One of the most common ionic compounds is NaCl, which is why we refer to it as salt or table salt. To determine the formula for an ionic compound you must determine the charge on each ion and then calculate how many of each ion must be brought together so that the charges are equal. Example: Aluminum oxide This compound is ionic (metal and non-metal) and, therefore is crystalline in structure. It contains aluminum ions (Al3+) and oxide ions (O2-) in a repeating three dimensional arrangement. Every repeating unit of aluminum oxide has two Al3+ ions and three O2- ions. 2 Al3+ ions contain a total positive charge of 2 x 3 = +6 3 O2- ions contain a total negative charge of 3 x 2 = - 6 This makes a neutral compound

Rules for Naming Ionic Compounds Rule A Example: CaI2 This compound contains one Ca2+ ion and two I- ions in a 1:2 ratio. According to the periodic table, the metal calcium only ever takes on a 2+ charge, naming this compound is simply Calcium Iodide. The non-metal drops its normal ending and you add “-ide”. Rule B Example: MnO2 This compound contains one Mn+4 ion and two O2- ions in a 1:2 ratio. According to the periodic table Mn could be +2 or +4. Since the two oxygens produce a combined -4 charge, the charge on Mn must be +4. Since it is +4 this must be indicated in the name: Manganese (IV) oxide.

  7  

Binary Ionic Compounds Formula to name 1. Cs2S _________________ 8. FeF3 __________________

2. BaO _________________ 9. Mg3N2 __________________

3. AlI3 _________________ 10. Ni3P2 __________________

4. MnO2 _________________ 11. UO2 __________________

5. Tc3P4 _________________ 12. HF __________________

6. CdBr2 _________________ 13. CoN __________________

7. NaCl _________________ 14. K2S __________________

Name to formula 15. rubidium sulfide _________________

16. mercury (II) oxide _________________

17. calcium nitride _________________

18. zinc bromide _________________

19. uranium (VI) fluoride _________________

20. silver phosphide _________________

21. platinum (II) selenide _________________

22. europium (II) nitride _________________

23. cesium phosphide _________________

24. lead (II) chloride _________________

25. cadmium oxide _________________

26. tin (IV) fluoride _________________

27. iron (II) oxide _________________

28. iron (III) oxide _________________

29. copper (II) sulfate _________________

30. chromium (III) chloride _________________

 8  

More Binary Ionic Compounds 1. KBr _________________

2. V2O5 _________________

3. cobalt (III) oxide _________________

4. barium phosphide _________________

5. cadmium nitride _________________

6. Cu3P _________________

7. Ag2S _________________

8. Sn3N4 _________________

9. radium iodide _________________

10. beryllium selenide _________________

11. Fe2S3 _________________

12. SrO _________________

13. CrCl2 _________________

14. mercury (II) fluoride _________________

15. lead (IV) bromide _________________

16. CuSe _________________

17. FeP _________________

18. lithium oxide _________________

19. cobalt (III) fluoride _________________

20. CdI2 _________________

  9  

Ternary Ionic Compounds 1. calcium nitrite _________________

2. BaSO4 _________________

3. silver acetate _________________

4. SrSO3 _________________

5. nickel (II) phosphate _________________

6. Na2CO3 _________________

7. LiHCO3 _________________

8. ammonium phosphate _________________

9. Be(ClO)2 _________________

10. aluminum oxalate _________________

11. rubidium dichromate _________________

12. KHSO3 _________________

13. calcium hydroxide _________________

14. manganese (II) silicate _________________

15. HCN _________________

16. cesium hydrogen sulfate _________________

17. Ti(OH)4 _________________

18. ammonium chloride _________________

19. Ca(ClO3)2 _________________

20. rubidium cyanate _________________

21. copper (II) sulfate _________________

22. CuCl _________________

23. iron (II) arsenate _________________

24. NH4OH _________________

 10  

IV. Molecular Compounds Rules for Molecular Compounds Molecular compounds are composed of individually covalently bonded

atoms. The simplest unit of a molecular compound is called a “molecule”.

The compounds are composed only of non-metals. The are sometimes

called covalent compounds since the bond between the atoms is formed by

shared “co”, valence “valent” electrons.

These prefixes are used to indicate the number of each atom in simple

molecular compounds:

mono- one hexa- six

di- two hepta- seven

tri- three octa- eight

tetra- four nona- nine

penta- five deca- ten

The prefix that indicates the number of each atom is placed before the name

of the element. Exception: mono is not used for the first element if there is

only one of them (see Example 2). ALL molecular compounds end in “-ide” Example 1: N2O is dinitrogen monoxide

NOT dinitride monoxide (the first element does not end in “–ide”)

NOT dinitrogen monoxygen (the second element does end in “-ide”)

NOT dinitrogen monooxide (the “o” is dropped before a vowel)

Example 2: CO is carbon monoxide NOT monocarbon monoxide (see exception above)

NOT carbon oxide (mono is necessary to indicate the quantity of O)

  11  

Molecular Compound Practice

1. CF4 _________________

2. N2O5 _________________

3. CS2 _________________

4. SO3 _________________

5. P4O8 _________________

6. iodine tribromide _________________

7. chlorine dioxide _________________

8. sulfur hexafluoride _________________

9. difluorine octachloride _________________

10. tribromine nonatelluride _________________

11. H2O _________________

12. P2S4 _________________

13. N2O4 _________________

14. XeF4 _________________

15. SI4 _________________

16. carbon dioxide _________________

17. trinitrogen hexabromide _________________

18. diiodine heptaselenide _________________

19. CO _________________

20. dicarbon octafluoride _________________

21. P4O10 _________________

22. Si3N4 _________________

23. Cl2S7 _________________

24. NBr5 _________________

 12  

V. Naming Acids

Rules for Acids Acids are often referred to as proton donors. There are many chemicals that have

acidic properties but we will stick to naming acids that begin with an H in their

formula. When such a compound is mixed with water, the hydrogen atom breaks

off. Chemists say it “dissociates”. It leaves its only electron attached to its former

molecule. The only thing remaining of the hydrogen atom then is a proton, hence

“proton donor”. This small ion is written H+ the more of them an acid produces, the

stronger the acid.

Acids are aqueous, meaning they are compounds dissolved in water. They should

be, but are not always, written with an (aq) subscript.

Binary acid: an acid that contains a hydrogen and one other element.

Example: HCl(aq) hydrochloric acid

Oxyacid: an acid that contains a hydrogen an oxygen and a third element.

Example: HNO3(aq) nitric acid

Acid naming rules (formula to name) First determine the name of the anion (the part that comes after the H).

For HCl(aq) Cl- is the anion and it would be chloride. Ending in “-ide”

For HClO2(aq) ClO2- is the anion and it would be chlorite. Ending in “-ite”

For HClO3(aq) ClO3- is the anion and it would be chlorate. Ending in “-ate”

If ion ends in “-ide” then the acid begins with “hydro” and ends in “-ic”.

HCl Hydrochloric acid

If ion ends in “-ite” then the acid ends in “-ous”. HClO2 Hydrochlorous acid

If ion ends in “-ate” then the acid ends in “-ic”. HClO3 Chloric acid

If the anions are sulfate, sulfite, phosphate you don’t call the acids sulfic,

sulfous or phosphic. They are sulfuric, sulfurous and phosphoric.

  13  

Acid naming rules (name to formula) Combine the appropriate amount of H+ with the anion to make a neutral

compound.

Example: What is the formula for phosphoric acid?

Since it ends in “-ic” it indicates an “-ate” ion, phosphate to be exact.

The phosphate ion is PO43- with a -3 charge. 3 H+ are needed to balance.

Answer: H3PO4(aq)

What is the formula for citric acid? (hint: citrate ion is C6H5O73-)

Acid Practice

1. hydrocyanic acid _________________ 2. dichromic acid _________________ 3. hydrobromic acid _________________ 4. nitrous acid _________________ 5. sulfuric acid _________________ 6. HF(aq)

_________________

7. H3PO4(aq) _________________ 8. H2CO3(aq) _________________ 9. H2S(aq) _________________ 10. acetic acid _________________ 11. sulfurous acid _________________ 12. perchloric acid _________________ 13. carbonic acid _________________ 14. HClO(aq) _________________ 15. HClO2(aq) _________________ 16. H2C2O4(aq) _________________ 17. H3P(aq) _________________ 18. HMnO4(aq) _________________ 19. hydrochloric acid _________________ 20. chromic acid _________________ 21. phosphoric acid _________________ 22. HCl(aq) _________________

 14  

VI. Naming Hydrates Hydrates are compounds with water molecules trapped within them. These

compounds release water when heated.

Naming Rules

Greek prefixes are used to indicate the number of water molecules that are

trapped.

Example: MgSO4�7H2O

Formula Mg SO4 � 5 H2O

Name magnesium sulfate hepta hydrate

Remember your ionic compound naming rules for elements which take more

than one charge as ions such as copper (which can take a +1 or +2 charge).

Example: CuSO4�5H2O

Formula Cu SO4 � 5 H2O

Name copper (II) sulfate penta hydrate

Hydrate Practice (formula to name) 1. MgCl2�6H2O _________________ 2. Cd(NO3)2�4H2O _________________ 3. ZnCl2�6H2O _________________ 4. Na2S2O3�5H2O _________________ 5. CaCl2�2H2O _________________ Hydrate Practice (name to formula) 1. barium hydroxide octahydrate _________________ 2. sodium sulfate decahydrate _________________ 3. lithium chloride tetrahydrate _________________ 4. cobalt (II) chloride hexahydrate _________________ 5. sodium carbonate decahydrate _________________

  15  

Chapter Review Problems

1. cadmium nitrate _________________ 2. chromate ion _________________ 3. dinitrogen monoxide _________________ 4. NO2

- _________________ 5. nitrous acid _________________ 6. HPO4

2-

_________________

7. PCl3 _________________ 8. HC lO4(aq) _________________ 9. BaSO4 _________________ 10. sulfur hexafluoride _________________ 11. hydrogen peroxide _________________ 12. sulfuric acid _________________ 13. carbonate ion _________________ 14. BaO _________________ 15. HClO2(aq) _________________ 16. SrSO3 _________________ 17. Fe _________________ 18. acetic acid _________________ 19. CBr4 _________________ 20. hypochlorite ion _________________ 21. (NH4)2SO4�H2O _________________ 22. calcium hydroxide _________________ 23. Na2CO3 _________________ 24. Cu3P _________________ 25. HI _________________ 26. lead (II) acetate _________________ 27. O2

2- _________________

28. ammonium ion _________________ 29. CO3

2- _________________

30. H3O+ _________________

 16