Common Ions and Nomenclature

Common Ions and Nomenclature

AP Nomenclature

Common Ions and Nomenclature

  • Memorize the AP Common Ions Memorizing the list of ions is not difficult, but it does take time. You are unlikely to pass the ion test if you wait until September to start memorizing. Many people like using flash cards.
  • Learn correct spellings, formulas and charges
  • Be able to read charges for type I ions from the periodic table
  • First test: Fri Sept 4. I will give you names of ions, you will write the formulas and charges.
  • Second test: Fri Sept 11. I will give you compound names (you write the formulas) and compound formulas (you write the names). Yes, spelling counts. Capitalization also counts.

1st year chemistry nomenclature notes [Summary is first, complete notes plus practice follow]

Compound TypesIdentify the type by looking at the first half of the compound

  1. Ionic: metal (known charge) + nonmetal
  • Name the metal, then the nonmetal
  • Nonmetal has –ide ending.

CaCl2: calcium chloride

Ca3(PO4)2: calcium phosphate

Ca3P2: calcium phosphide

  1. Ionic: metal (variable charge) + nonmetal
  • Identify the charge of the metal
  • Name the metal, put the charge in () as a Roman numeral
  • Name the nonmetal (-ide ending).

Fe2O3: iron(III) oxide

CuO: copper(II) oxide

Cu2O: copper(I) oxide

  1. Covalent: nonmetal + nonmetal
  • Use prefixes to identify the relative number of atoms in the compound.
  • First element: use element name; second: use –ide ending (like anions)
  • ‘Mono’ is not used for the first element.
  • Some names use contractions: monoxide, not monoxide.

1: mono

2: di

3: tri

4: tetra

5: penta

6: hexa

7: hepta

8: octa

9: nona

10: deca

BF3boron trifluoride

N2O5dinitrogen pentoxide

CCl4: carbon tetrachloride

NO2:nitrogen dioxide

  1. Acids: H + anion

Without oxygen:

HCl: hydrochloric acid

H2S: hydrosulfuric acid

With oxygen:

H2SO4: sulfate ion  sulfuric acid;

H2SO3: sulfite ion  sulfurous acid

5 NomenclatureLonger version

Early chemists made up names for compounds without a system:

sugar of lead; blue vitriol; quicklime; Epsom salts; milk of magnesia; gypsum; laughing gas

Nomenclature: naming system; name describes the composition of the compound

5.1 Naming Compounds

Binary compounds: compounds composed of two elements

Compound Types

  1. Ionic: metal (known charge) + nonmetal

Name the metal, then the nonmetal; nonmetal has –ide ending.

CaCl2: calcium chloride

Ca3(PO4)2: calcium phosphate

Ca3P2: calcium phosphide

CsF: cesium chloride

AlCl3: aluminum chloride

MgI2: magnesium iodide

  1. Ionic: metal (variable charge) + nonmetal

Identify the charge of the metal; name the metal, put the charge in () as a Roman numeral; name the nonmetal (-ide ending).

Copper has more than one possible charge. The charge must be added to the name.

CuO: copper(II) oxide

Cu2O: copper(I) oxide

Fe2O3: iron(III) oxide

5.2 Naming Binary Compounds that contain a Metal and a Nonmetal (Types I and II)

Some metal atoms can form two or more cations:.

Type I compounds: the metal present forms only one type of cation Na is always 1+

Type II compounds: the metal present can from two (or more) cations that have different charges

Cr can form Cr2+ and Cr3+; Cu can form Cu+ and Cu2+

Naming Type I Ionic Compounds

  1. Cation is first, then the anion.
  2. Cations (except the polyatomic one) take their names from the element name.
  3. Anions from a single atom are named by adding –ide to the root of the name.

Ex 5.1 Type I binary compounds

Compound formula ions ion names compound name

CsFCs+cesiumcesium fluoride

F-fluoride

AlCl3Al3+aluminumaluminum chloride

Cl-chloride

MgI2Mg2+magnesiummagnesium iodide

I-iodide

Type II binary compounds

When a cation has variable charges, the specific charge needs to be in the compound name.

Use roman numerals to give the charge.

ExFeCl2Fe2+ or Fe3+?[charge on Fe?] + 2(1-) = 0 charge is 2+

Cl-2+ + 2- = 0 [no net charge for compound]

Name: iron (II) chloride

Since there are two chloride ions, the iron must have a charge of 2+ to result in a neutral compound.

* Note that the II refers to the charge, not the subscript number*

FeCl3 = iron (III) chloride

Ex. PbO2O2-Pb?+ + 2(2-) = 0; Pb4+

Lead (IV) oxide

Alternate system: The ion with the higher charge has a name ending in –ic;

The ion with the lower charge has a name ending in –ous.

Fe3+ = ferricFe2+ = ferrous

Ex. 5.2 Type II binary

  1. CuClCu?+Cu+copper (I) chloride

Cl-

  1. HgOHg?+Hg2+mercury (II) oxide

O2-

  1. Fe2O3Fe?+6+Fe3+iron (III) oxide

O2-6-

  1. MnO2Mn?+ 4+Mn4+manganese (IV) oxide

O2-4-

  1. PbCl4Pb?+4+Pb4+lead (IV) chloride

Cl-4-

Rules: 1. Cation first, then anion 2. Because the cation can have more than one charge, specify the charge with a roman numeral in parentheses.

5.3 Naming Binary Compounds that Contain Only Nonmetals (Type III)

Covalent: nonmetal + nonmetal

What would make good names for NO and NO2?  need a way to distinguish these two ‘nitrogen oxides’

Rules for Naming Type III Binary Compounds

  1. The first element in the formula is named first (full element name).
  2. The second element is named as though it were an anion.
  3. Prefixes are used to denote the numbers of atoms present.
  4. The prefix mono- is never used for naming the first element. For example, CO is called carbon monoxide, not monocarbon monoxide.

BF3boron trifluoride

NOnitrogen monoxide [aka nitric oxide]

N2O5dinitrogen pentoxide

CCl4: carbon tetrachloride

NO2:nitrogen dioxide

IF3:iodine trifluoride

1: mono2: di3: tri4: tetra5: penta

6: hexa7: hepta8: octa9: nona10: deca

5.4 Naming Binary Compounds: Strategy / Review

* Use the periodic table to determine which elements are metals, nonmetals and transition metals.

5.5 Naming Compounds that Contain Polyatomic Ions

Polyatomic ions: several atoms bound together (covalently) that have a charge

Oxyanions

=Polyatomic ions that contains an atom of an element, and different numbers of oxygen

The ion with a smaller number of oxygen atoms has an –ite ending

The ion with a bigger number of oxygen atoms has an –ate ending

If there are more than 2 oxyanions in a series, hypo- (less than) and per- (more than) are used as prefixes to indicate the ion with the fewest number of oxygen, and the one with the most

Ex.

ClO-hypochlorite

ClO2-chlorite

ClO3-chlorate

ClO4-perchlorate

5.6 Naming Acids

Acids: compounds that produce H+ ions when dissolved in water (~ molecules with H+ attached to anions)

Rules for naming acids (depend on whether the anion contains oxygen)

  1. If the anion does not contain oxygen, the acid is named with the prefex hydro- and the suffix –ic attached to the root name for the element.
  2. HCl (hydrogen chloride), when dissolved in water forms hydrochloric acid
  3. HCN (hydrogen cyanide), when dissolved in water forms hydrocyanic acid
  4. H2S (hydrogen sulfide), when dissolved in water forms hydrosulfuric acid
  5. When the anion contains oxygen, the acid name is formed from the root name of the central element of the anion or the anion name, with a suffix of –ic or –ous. When the anion name ends in –ate, the suffix –ic is used; when the anion name ends in –ite, the suffix –ous is used.
  6. H2SO4SO42- sulfatesulfuric acid
  7. H3PO4PO43- phosphatephosphoric acid
  8. HC2H3O2C2H3O2- acetateacetic acid
  9. H2SO3SO32- sulfitesulfurous acid
  10. HNO2NO2- nitritenitrous acid

Acids: starts with H

Without oxygen:

HCl: hydrochloric acid

H2S: hydrosulfuric acid

With oxygen:

H2SO4: sulfate ion  sulfuric acid;

H2SO3: sulfite ion  sulfurous acid

Nomenclature practice

Write the names for these compounds.

  1. I2O7
  2. CO2
  3. CF4
  4. NH3
  5. PCl3
  6. PCl5
  7. P4O6
  8. SF6
  9. SO3
  10. SO2
  11. N2O3
  12. CO
  13. NO2
  14. SeF6
  15. SiO2
  16. H2O
  17. CuO
  18. SrO
  19. B2O3
  20. K2S
  21. AsF3
  22. Al2S3
  23. SnBr4
  24. CS2
  25. CdS
  26. AgCl
  27. KI
  28. NO
  29. P2O5
  30. FeCl3
  31. ClF3
  32. CuCl
  33. MnO2
  34. MgO

Naming Practice

  1. Ca(OH)2
  2. Na3PO4
  3. KMnO4
  4. (NH4)2Cr2O7
  5. Co(ClO4)2
  6. KClO3
  7. Cu(NO2)2
  8. PbCO3
  9. KHSO4
  10. NH4I
  11. NaCN

  1. H3PO3
  2. Na2CO3
  3. FeBr3
  4. HF
  5. CsClO4
  6. PCl3
  7. H2S
  8. CuSO4
  9. Ca(HCO3)2
  10. MgI2
  11. KMnO4
  12. HBrO4
  13. Fe(OH)2
  14. NaHCO3
  15. BaSO4
  16. HNO3
  17. BrF5
  18. NaBr
  19. Zn3(PO4)2

Naming Practice

  1. Fe2O3
  2. CsCl
  3. NaCN
  4. P2S3
  5. H2S
  6. Cu(NO3)2
  7. Ag2S
  8. SnBr4
  9. Ca3(PO4)2
  10. Ba(OH)2
  11. HF
  12. MgCO3
  13. PbO
  14. NH4NO3
  15. BaSO4
  16. Li2CO3
  17. H3PO4
  18. K2Cr2O7
  19. HNO3
  20. MnSO4

  1. Diboron trioxide
  2. Hydrochloric acid
  3. Calcium acetate (calcium ethanoate)
  4. Sodium hydroxide
  5. Copper (II) permanganate
  6. Aluminum phosphate
  7. Silicon dioxide
  8. Magnesium oxide
  9. Ammonium hydroxide
  10. Sodium carbonate
  1. Cobalt (III) nitrate
  2. Sulfuric acid
  3. Calcium chloride
  4. Lead (IV) oxide
  5. Dinitrogen pentoxide
  6. Silver chloride
  7. Iron (II) oxide
  8. Hydrosulfuric acid
  9. Ammonium sulfate
  10. Sulfur hexafluoride

Name Compound Types I, II, III and acids

  1. KClO3
  2. NaBr
  3. SrO
  4. B2O3
  5. HBr
  6. PbCO3
  7. NH4I
  8. H2SO4
  9. CuSO4
  10. Ca(HCO3)2
  11. MgI2
  12. BrF5

Write formulas from names

For ionic compounds, write ions with charges, then combine, using subscripts and parentheses as necessary.

  1. barium carbonate
  1. hydrochloric acid
  1. potassium hydroxide
  1. sodium carbonate
  1. cobalt (III) nitrate
  1. calcium chloride
  1. lead (IV) oxide
  1. dinitrogen pentoxide
  1. ammonium phosphate
  1. ammonium sulfate
  1. disulfur dichloride
  1. nitric acid
  1. lithium iodide
  1. aluminum oxide
  1. sodium nitrate
  1. ammonium hydroxide
  1. magnesium bromide
  1. carbon disulfide
  1. cobalt (II) chloride
  1. cesium fluoride

Nomenclature: Types I, II and IIIch 5

Write the names for the following compounds.

  1. KCl
  2. CO2
  3. CoCl3
  4. CaO
  5. PbBr4
  6. CO
  7. CsCl
  8. PCl5
  9. CuI2
  10. SF6
  11. Fe2O3
  12. PbS
  13. FeO
  14. SnBr4
  15. LiH
  16. SO3
  17. CaI
  18. NO
  19. KI
  20. P4O6
  21. NaF
  22. CuCl
  23. BaCl
  24. N2O3
  25. Al2S3

Nomenclaturech 5

Write the names for the following compounds.

  1. Ca(OH)2
  2. K2S
  3. MgO
  4. HBr
  5. P2O5
  6. NaCN
  7. NO
  8. FePO4
  9. HC2H3O2
  10. Al2S3
  11. PbBr4
  12. CuSO4
  13. HCl
  14. PCl3
  15. CuNO3


Write the chemical formulas. (For types I and II, write the ions with charges first, then combine)

  1. Sodium sulfide
  2. Nitrogen monoxide
  3. Dinitrogen trioxide
  4. Copper (II) chloride
  5. Aluminum bromide
  6. Iron (III) hydroxide
  7. Carbon tetrafluoride
  8. Potassium nitrate

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