Nomenclature

Learn to name binary compounds of a metal and a nonmetal.

Learn how to name binary compounds containing only nonmetals.

Learn the names of common polyatomic ions and how to use them in naming compounds.

Learn names for common acids and how the anion composition determines the acids name.

Learn to write the formula of a compound, given its name.

Naming compounds

Common names are Epsom salts, milk of magnesia, laughing gas, and many more

There are over 4 million different compounds and more are discovered all the time

Memorizing the common names would be impossible so we have a system

Binary compounds

Compounds composed of 2 elements Two types:

Compounds that contain a metal and nonmetal

Compounds that contain 2 nonmetals

Naming Compounds That Contain a Metal

and a NonmetalTo learn to name binary

compounds of a metal and a nonmetal.

Binary Ionic Compound

Contain a positive ion (cation) and a negative ion (anion)

Two types of binary ionic compounds Type I: contain elements with only one

ion Na+, Cs+, Ca+2, etc

Type II: contain elements with 2 or more ions

Cr+2 or Cr+3, Cu+ or Cu+2

Type I Binary Ionic Compounds

The cation is always named 1st

The cation is named as the element name Na+ is sodium

The anion is named by taking the 1st part of the element name and adding –ide Cl- is chloride

Type I Binary Ionic Compounds

NaI sodium iodide

CaO calcium oxide

NaCl sodium chloride

KI potassium iodide

CaS calcium sulfide

CsBr cesium bromide

MgO magnesium oxide

CsF cesium fluoride

AlCl3 aluminum chloride

MgI2 magnesium iodide

Rb2O rubidium oxide

SrI2 strontium iodide

K2S potassium sulfide

Type II Binary Ionic Compounds

Some metals can produce 2+ ions When this happens, we use Roman

Numerals The Roman numerals only tell us the

charge, not how many of that ion there are in the compound

You do not need to use Roman numeral for metals that form only 1 cation

Type II Binary Ionic Compounds

What is FeCl2 made of? Fe+2 and two Cl-

What would we name it? Iron (II) chloride

What is PbO2 made of and what is its name? Pb+4 and 2 O-2 called lead (IV) oxide

Type II Binary Ionic Compounds

Write out the following and give their name CuCl

copper (I) chloride HgO

mercury (II) oxide Fe2O3

iron (III) oxide MnO2

manganese (IV) oxide PbCl4

lead (IV) chloride

Review Type I and II

CoBr2

Co+2 + Br- cobalt (II) bromide CaCl2

Ca+2 + Cl- calcium chloride Al2O3

Al+3 + O-2 aluminum oxide CrCl3

Cr+3 + Cl- chromium (III) chloride

Naming Binary Compounds That

Contain Only Nonmetals (Type III)

To learn how to name binary compounds containing only

nonmetals.

Rules for naming Type III The 1st element in the formula is named 1st and

the full element name is used. The 2nd element is named as though it were an

anion. Prefixes are used to indicate the # of atoms

present The prefix mono- is never used for the 1st

element

Prefixes for Type III mono- 1 di- 2 tri- 3 tetra- 4 penta- 5 hexa- 6 hepta- 7 octa- 8

Type III

BF3

notice they are both nonmetals Name the 1st element – boron Name the 2nd as an anion – fluoride Add prefixes

boron trifluoride

Practice Problems

NO nitrogen monoxide

N2O3 dinitrogen trioxide

CCl4 carbon tetrachloride

NO2 nitrogen dioxide

IF3 iodine trifluoride

I2O7 diiodine heptoxide

CO2 carbon dioxide

CF4 carbon tetrafluoride

NH3 nitrogen trihydride

PCl3 phosphorous trichloride

Naming Binary Compounds: A

ReviewTo review the naming of Type

I, II, and III binary compounds.

Naming binary compounds

Binary Compound?

Yes

Metal Present?

YesNo

Type III: Use prefixes Does the metal form more than one cation?

No Yes

Type I: Use the element name for the

cation

Type II: Determine the charge of the

cation; use a Roman numeral after the

cation

Type I, II, III

AsF3 arsenic trifluoride

Al2S3 aluminum sulfide

SnBr4 tin (IV) bromide

CS2 carbon disulfide

CdS cadmium sulfide

AgCl silver chloride

KI potassium iodide

NO nitrogen monoxide

P2O5 diphosphorous pentoxide

FeCl3 iron (III) chloride

Naming compounds with polyatomic ions

Simply write the name of the polyatomic ion No change is needed

What would NH4C2H3O2 be called? Look at the table

NH4 – ammonium C2H3O2 – acetate

Put the them together in the same order as the formula

Ammonium acetate

Naming compounds with polyatomic ions

If using a cation with more than one charge, use Roman numerals Fe(NO3)3

The 2nd 3 tells us that there are 3 NO3 in the formula

Looking on our chart we see NO3 has a charge -1

If they’re totaled, that makes our total charge -3

Fe must be +3 to cancel it out Iron (III) nitrate

Polyatomic Practice

Na2SO4

sodium sulfate

KH2PO4

potassium dihydrogen phosphate

Mn(OH)2

Manganese (II) hydroxide

Na2SO3

sodium sulfite

Cu(NO3)2

Copper (II) nitrate

PbCO3

Lead (II) carbonate

KHSO4

potassium hydrogen sulfate

NH4I ammonium iodide

NaCN sodium cyanide

Naming Chemical Compounds

Binary Compound?

Yes

Metal Present?

YesNo

Type III: Use

prefixes

Does the metal form more than one cation?

NoYes

Type I: Use the element

name for the cation

Type II: Determine the charge of the

cation; use a Roman numeral after the cation

No

Polyatomic Ion or Ions Present?

No Yes

We will learn this

procedure

later.

Name the compound similar to naming binary

compounds but use the polyatomic chart for

their names

Name the following chemical compounds to be turned in for

a grade1. Na2CO3

2. FeBr3

3. PCl3

4. CsClO4

5. CuSO4

6. NaHCO3

7. BaSO4

8. CsClO4

9. BrF5

10. NaBr11. KOCl12. Zn3(PO4)2

13. Ca(HCO3)2

14. MgI2

15. KMnO4

16. Sb2O3

17. Fe(OH)2

1. Na2CO3 sodium carbonate

2. FeBr3 iron (III) bromide

3. PCl3 phosphorous trichloride

4. CsClO4 cesium perchlorate

5. CuSO4 copper (II) sulfate

6. NaHCO3 sodium hydrogen carbonate

7. BaSO4 barium sulfate

8. CsClO4 cesium perchlorate

9. BrF5 bromine pentafluoride

10. NaBr sodium bromide

11. KOCl potassium hypochlorite

12. Zn3(PO4)2 zinc (II) phosphate

13. Ca(HCO3)2 calcium hydrogen carbonate

14. MgI2 magnesium iodide

15. KMnO4 potassium permanganate

16. Sb2O3 antimony (III) oxide

17. Fe(OH)2 iron (II) hydroxide

Naming Acids

To learn how the anion composition determines the

acid’s nameTo learn names for common

Acids

A molecule w/ one or more H+ ions attached to an anion

The rules for naming acids depend on whether it has oxygen

Rules for naming acids

If no oxygen is present Add prefix hydro- and suffix –ic to the root

word and the word acid to the end HCl

hydro + chlorine + ic + acid hydrochloric acid

Rules for naming acids

If oxygen is present Named after the anion present

When anion ends in –ate Add suffix –ic and the word acid H2SO4 sulfate becomes sulfuric acid

When anion ends in –ite Add suffix –ous and the word acid HNO2 nitrite becomes nitrous acid

Naming AcidsDoes the anion contain oxygen?

YesNo

hydro-+anion root+ -ic hydro(anion root)ic acid

Check the ending of the anion name

-ite -ate

anion or element root+ -ous(root)ous acid

anion or element root+ -ic(root)ic acid

Acid Practice HF

Hydrofluoric acid H3PO3

Phosphorous acid HNO3

Nitric acid HBrO3

Bromic acid H2S

Hydrosulfuric acid

Writing Formulas from Names

To learn to write the formula of a compound, given its

name

Formulas from names So far you were given a name and you

gave the formula A lot of times the reverse is also

necessary calcium hydroxide

Ca+2 OH-

You will need 2 hydroxide ions to cancel out the +2 charge of Ca

Ca(OH)2

iron (II) oxide Fe+2 O-2

The +2 and -2 cancel each other out FeO