NAMING COMPOUNDS

TYPES OF COMPOUNDS Molecular compound (covalent bonds)

Compound made of two nonmetals NBr5

Ionic compound Compound made of a metal and a

nonmetal NaCl

Acid (ionic bonds) Compound that can donate a hydrogen ion HCl

MOLECULAR COMPOUND (TWO NONMETALS)

To name a molecular compound, you have two parts: The first element in the compound and The second element in the compound

NBr5

The first element is called by its normal name: N – nitrogen

The second name is called by its name and ends in –ide: Br – bromine bromide

PREFIXESIn addition to naming the

elements, you have to name how many they are. To do this you need prefixes.

The prefix goes in the front of the name of the element

PREFIXES (CONT)One – monoTwo – diThree – triFour – tetraFive - penta

Six – hexaSeven – hepta

Eight – octaNine – nonaTen - deca

MOLECULAR COMPOUND (CONT)

Therefore if you start with NBr5:Mononitrogen pentabromide

BUT wait, if you only have one element in the beginning part of the compound, you don’t have to put the prefix:Nitrogen pentabromide

TRY THESE

1. SCl62. N2O4

3. P3F5

4. CCl45. XeO

1. Trinitrogen hexaoxide

2. Boron pentabromide

3. Tetrasulfur decafluoride

4. Phosphorus octaiodide

ANSWERS1. Sulfur

hexachloride2. Dinitrogen

tetraoxide3. Triphosphorus

pentafluoride4. Carbon

tetrachloride5. Xenon monoxide

1. N3O6

2. BBr5

3. S4F10

4. PI8

SPECIAL CASEWhen naming some compounds, it is implied

that the compound is a DIATOMIC GASThere are only 7 diatomic molecules

HydrogenNitrogenOxygenFluorineChlorine IodineBromine

DIATOMIC MOLECULES If you ever see any of those molecules, you

write them as a compound with two of the atoms

Hydrogen – H2 Nitrogen – N2 Oxygen – O2 Fluorine – F2 Chlorine – Cl2 Iodine – I2 Bromine – Br2

IONIC COMPOUNDS (METAL AND NONMETAL)

The two parts of naming an ionic compound: The first element is always the metal The second element is the nonmetal

CaBr2 The first element is called by its normal

name: Ca Calcium The second element is named like a

molecular compound: Br bromideThe only difference is that you do

not use a prefix ever

IONIC COMPOUNDSTherefore if you start with

CaBr2:

Calcium Bromide

There is no prefix for bromide even though there is a 2

IONIC COMPOUNDSBefore we begin practice naming

ionic compounds, look at your ion sheet

Remember: To put ionic compounds together, you need to BALANCE THE CHARGE

EXAMPLE How would you show the following ionic

compound: Strontium iodide Strontium Sr (has a +2 charge: alkali earth

metal) Iodide (has a -1 charge: halogen) Just like before, cancel swap the charges

Sr+2 + 2I - SrI2

Your ion sheet gives you the names of several ions with the many possible charges of the transition metals

TRY THESE

1. BaCl22. K2O

3. AlF3

4. CaO

1. Magnesium oxide

2. Potassium sulfide

3. Sodium chloride

4. Beryllium iodide

ANSWERS1. Barium

chloride2. Potassium

oxide3. Aluminum

fluoride4. Calcium oxide

1. MgO2. K2S

3. NaCl4. BeI2

POLYATOMIC IONSAn ion that is composed of several

atomsFORMAL DEFINITION

Polyatomic ion: an electrically charged group of two or more chemically bonded atoms that function as a SINGLE ION

POLYATOMIC IONSSince the polyatomic ions are made of

more than 1 atom, their names are complicated

Example of some polyatomic ions:OH - hydroxideClO4 - perchlorateCO3

-2 carbonateNH4 + ammonium

POLYATOMIC IONS IMPORTANT NOTE: When combining

polyatomic ions, you still balance out the NET CHARGE:

Example: If you have sodium hydroxideSodium: Na+

Hydroxide: OH –

Na+ + OH - NaOH

POLYATOMIC IONWhat do you do if you have more than 1

polyatomic ion to balance out a charge?Example: If you have Magnesium acetate

Magnesium: Mg+2

Acetate: C2H3O2 –

Mg+2 + 2C2H3O2- Mg(C2H3O2)2

You put the entire polyatomic ion in brackets with the number of ions as a subscript

TRY THESE1. Lithium

oxalate2. Barium

bromate3. Sodium

Phosphate4. Aluminum

sulfate

1. K3BO3

2. Sr(NO2)2

3. Mg3(PO4)2

4. CaSO4

ANSWERS

1. Li2C2O4

2. Ba(BrO3)2

3. Na3PO4

4. Al2(SO4)3

1. Potassium borate

2. Strontium nitrite

3. Magnesium phosphate

4. Calcium sulfate

IONIC COMPOUNDS (TRANSITION METALS)

What do you do when you do not know the exact charge of the ion?

In other words, some of the transition metals can have more than 1 ionFe+2

Fe+3

You distinguish with Roman numerals

IONIC COMPOUNDS (TRANSITION METALS)

Solution: The name of the compound tells you the charge.

If you have a compound of iron and oxygen, an example would be: Iron (III) oxide

This means that iron has a +3 charge2Fe+3 + 3O-2 Fe2O3

IONIC COMPOUNDS (TRANSITION METALS)

This means that if you’re given the formula, you have to figure out the charge of the metal ion:

Example: MnO2

What you know: O has a -2 chargeTherefore the total negative is -4This means that you need a +4 to

balanceYou get Manganese (IV) oxide

TRY THESE1. Nickel (III)

iodate2. Lead (II)

chloride3. Gold (I)

Sulfate4. Vanadium (III)

chlorate

1. W(PO4)2

2. AuBO3

3. Tl3PO4

4. Sn(NO3)4

ANSWERS

1. Ni(IO3)3

2. PbCl23. Au2SO4

4. V(ClO3)3

1. Tungsten (VI) phosphate

2. Gold (III) borate

3. Thallium (I) phosphate

4. Tin (IV) nitrite

ACIDS What is an acid?

For now: An acid is a compound that will donate a proton (H+)

How do you recognize an acid Any compound that begins with H+

There are two basic types of acids for naming Binary acid Polyatomic acid

BINARY ACID A binary acid has a hydrogen ion and a single

halide Examples: HCl, HF, HBr, HI

Naming these acids takes the following format: Hydro-(root of the name of the halide)-ic acid

Therefore HCl becomes Hydrochloric acid

BINARY ACID What would be the names of the

following:1. HF2. HBr3. HI

ANSWERS

1. Hydrofluoric acid2. Hydrobromic acid3. Hydroiodic acid

POLYATOMIC ACIDSSimilar convention to binary acids

(Base name of the polyatomic ion)-ic acid

HC2H3O3

This is an H+ with a C2H3O3-

The name of the polyatomic ion is acetate

The name is Acetic acid

POLYATOMIC ACIDSThe differencesWhat if you have H2SO4 and

H2SO3

What’s the difference in these two names?: only one can be sulfuric acid

POLYATOMIC ACIDS If the ion ends in the name “-ate”

Sulfate, nitrate, chlorate The name of the acid is (root of ion)-ic acid Sufuric acid, nitric acid, chloric acid

If the ion ends in the name “-ite” Sulfite, nitrite, chlorite The name of the acid is (root of ion)-ous acid Sulfurous acid, nitrous acid, chlorous acid

TRY THESE

1. H2CO3

2. HNO2

3. HIO3

4. H3PO4

1. Oxalic acid2. Sulfurous

acid3. Sulfuric

acid4. Bromic acid

ANSWERS1. Carbonic

acid2. Nitrous acid3. Iodic acid4. Phosphoric

acid

1. H2C2O4

2. H2SO3

3. H2SO4

4. HBrO3

SUMMARYBefore you start naming,

determine the type of compound Molecular, ionic or acid

Naming molecular compounds (nonmetal and nonmetal) Name of the first element Base name of the second element + ide Make sure you use the prefix indicating

number of atoms

SUMMARY (CONT) Naming ionic compounds (metal and

nonmetal) Name of the first element

Name of the second element + ide or

Name of the second polyatomic ion

Make sure you balance the charges of each ion

If the metal has more than 1 possible charge, indicate the charge with a Roman numeral

SUMMARY (CONT)Acids (the compound has a

hydrogen ion H+) Binary acids Hydro (base name of the halogen)-ic acid

Polyatomic acids (Base name of the polyatomic ion w/

“-ate”) – ic acid (Base name of the polyatomic ion w/

“-ite”) – ous acid

WRITE THE SYMBOL OR NAME

1. Calcium chloride2. Lead (IV) sulfate3. Carbon

tetrachloride4. Hydroiodic acid5. Sulfuric acid6. Dinitrogen

hexachloride

7. HBr8. NH4NO3

9. S3Br8

10. NO11. HNO2

12. Mn(C2H3O2)3

13. Pb(SO3)2

ANWERS

1. CaCl22. Pb(SO4)2

3. CCl44. HI5. H2SO4

6. N2Cl6

7. Hydrobromic acid8. Ammonium nitrate9. Trisulfur

octabromide10. Nitrogen monoxide11. Nitrous acid12. Manganese (III)

acetate13. Lead (IV) sulfite

PUTTING THIS IN A CHEMICAL REACTION

General Format: Reactants Products

Steps Translate the chemical into its symbol and

then put the state of matter AFTER the chemical symbol

Put a “+” between each set of reactants and products

STATES OF MATTER Symbols for states of matter:

Solid (s) Liquid (l) Gas (g) Aqueous (aq)

EXAMPLE Solid sodium is mixed with chlorine gas

to form aqueous sodium chloride Solid sodium = ? is mixed with = ? chlorine gas = ? to form = ? aqueous sodium chloride = ?

FINAL ANSWER

Na(s) + Cl2(g) NaCl(aq)

TRY THESE1. Solid iron is combined with oxygen gas

to produce solid iron(III) oxide.2. Aqueous magnesium nitrate is

combined with solid zinc to form aqueous zinc nitrate and solid magnesium.

ANSWERS

1. Fe(s) +O2(g) Fe2O3(s)

2. Mg(NO3)2(aq) + Zn(s) Zn(NO3)2(aq) + Mg(s)