Naming Chemical Compounds

Binary Ionic Compounds

Binary = 2 types of elements Ionic = made of ions Compound = atoms bonded

together

Ionic Compounds

Positive ions are attracted to Negative ions

FORMULA UNIT

Cation always comes first, then anion

Elemental anions

When an element becomes an anion, it starts to end in –ide Fluoride Chloride Bromide Oxide Sulfide Nitride Phosphide

Type I

The cation has a predictable charge Alkali Metals +1 Alkaline Earth Metals +2 Group 3A +3 Silver Ag+

Zinc Zn2+

Type II

The cation has a variable charge All Transition metals except for Ag and Zn (for

our purposes) The name will have a roman numeral to

denote the CHARGE on the cation

Fe2+

Fe3+

Cu+

Cu2+

Iron(II)

Iron(III)

Copper(I)

Copper(II)

Ferrous

Ferric

Cuprous

Cupric

Naming ionic compouds (Type I and II)

First name cation Just the name of element if Type I Name of element and roman numeral

with charge on cation if Type II Then name anion

Elemental anions end in “–ide”

When determining the formula, remember “swap ‘n’ drop”

Name the following:

Na3N

MgCl2 Al2O3

CuCl CuCl2 PbBr4

Sodium nitride Magnesium chloride Aluminum oxide

Copper(I) chloride Copper(II) chloride Lead(IV) bromide

Determine the formula of the following

Aluminum chloride Magnesium Oxide Sodium nitride Calcium chloride Copper(I) sulfide Lead (II) bromide Iron(III) oxide

AlCl3 MgO Na3N

CaCl2 Cu2S

PbBr2

Fe2O3

Polyatomic Ions

Many anions are not just ions of elements.

Polyatomic Ions = many atomed particle with an overall charge

Mostly nonmetals bonded to Oxygens

Polyatomic Ion Naming

Main polyatomic ion Ends in “–ate” Example: Chlorate ClO3

-

One fewer oxygens Ends in “-ite” Example: Chlorite ClO2

-

Even fewer oxygens Hypo = under Example: Hypochlorite ClO-

More oxygens than main ion Hyper = over, shortened to “per” Example: Perchlorate ClO4

-

Common Polyatomic Ions

NO2- Nitrite

NO3- Nitrate

SO32- Sulfite

SO42- Sulfate

PO43- Phosphate

PO33- Phosphite

Common Polyatomic Ions

Hydrogen can attach to the polyatomic ions as H+

This adds an H and reduces the overall charge by 1

PO43- Phosphate

HPO42- Hydrogen

Phosphate

H2PO41- Dihydrogen

Phosphate

CO32- Carbonate

HCO31-

Hydrogen carbonate

(bicarbonate)

Name these compounds with PAIs

AlPO4

Cu(NO3)2

Na2SO4

NaHCO3

Mg3(PO4)2

Aluminum phosphate Copper(II) nitrate Sodium sulfate Sodium bicarbonate Magnesium Phosphate

Molecular Compounds

Molecular compounds are not bonded by positive and negative ions

They SHARE electrons Made of two non-metals Cannot predict or explain charges

(no charges, because not LOSING or GAINING electrons – SHARING)

Naming Molecular Compounds (Type III)

Because there is no way to neutralize the compounds (like for ions) we must determine how many there are another way:

Use PREFIXES

How to tell if it’s Type III

Check the FIRST element – is it a non-metal?

If YES, it’s a Type III

Name the first element as the element

Name the second element ending in “-ide”

Prefixes

1 2 3 4 5 6 7 8 9 10

Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca

Using prefixes

If there is only one of the first element, you may omit the “mono”

You may not omit any other prefixes

The more electronegative element goes last (upper right hand corner)

F, O, N, Cl,

Name the following

PCl3 CO2

NO N2O4

N2F5

OF2

Phosphorus trichloride Carbon dioxide Nitrogen monoxide Dinitrogen tetroxide Dinitrogen pentafluoride Oxygen difluoride

Naming Practice! For each of the following compounds, determine whether it is type I, II, or III.

1. FeCl32. NaCl3. Cu(OH)2

4. N2O

5. BaSO4

6. PO5

7. (NH4)CO3

8. SnBr2

Naming Practice! For each of the following compounds, determine the CHARGE on the cation (+1, +2, +3, or +4)

1. FeCl32. Cu(OH)2

3. Cr2S3

4. NiS5. Pb(NO3)2

6. SnCl4

1. 3

2. 2

3. 3

4. 2

5. 2

6. 4

Acids

All acids have the H+ ion in them as the cation.

All acids have “acid” in their name

Consider Hydrochloric Acid HCl

Naming Acids

If the anion DOES NOT CONTAIN OXYGEN: Prefix hydro- Root name of anion element Suffix –ic

Examples HF H2S

Hydrofluoric Acid

Hydrosulfuric Acid

Hydrooxygenic acid

Naming Acids

If the anion CONTAINS OXYGEN (ie: is a polyatomic ion) Root name of the PAI If anion ends in -ate,

acid ends in –ic If anion ends in –ite,

acid ends in –ous

Naming Acids Examples

H2SO4

H2SO3

HNO3

HNO2

HC2H3O2

Phosphoric Acid Carbonic Acid

Sulfuric Acid Sulfurous Acid Nitric Acid Nitrous Acid Acetic Acid

H3PO4

H2CO3

Organic Molecules

Carbon based Naming is based on number of

carbons Functional groups

Sets of molecules attached to the carbons

Naming is also based on what functional groups are where

Alkanes

The simplest organic molecules are Alkanes.

Carbons are all single bonded to each other

When not bonded to another carbon, bonded to a Hydrogen

All alkanes end in -ane

Prefixes

Note that the prefixes pertain to all types of carbon based molecules with any types of functional groups or chains

•Meth•Eth•Prop•But

•Pent•Hex•Hept•Oct

Alkenes and Alkynes

A functional group can be a set of atoms, or the way they are bonded.

Alkenes Carbons have double bonds between

them Alkynes

Carbons have triple bonds between them

Alkenes and Alkynes

To Name All alkenes end with –ene. All alkynes end with –yne Number the carbons in the longest

chain. Carbon 1 is at the end of the chain

closest to the first functional group Put the number that the bond is on,

then the chain length (some name by putting the number

BEFORE the functional group ending)

Isomer = molecule with SAME formula but DIFFERENT structure

Alcohols

Have an –OH group attached Name the carbon chain (prefix and

bond) End in –ol Indicate which carbon the –OH is on

2-propanol 1-Butanol 3-Octenol

What are the formulas for these alcohols?

Alcohols

Some alcohols have common names like glycerol

Branched Hydrocarbons

The longest continuous chain of carbon atoms gives the root name/prefix.

Substituent is named by the number of carbons.

Specify location of substituent by numbering carbon atoms in longest chain.

Substituent often referred to as R or R’ (for second substituent)

Substituent often referred to as R or R’ (for second substituent)

If more than one alkyl group, use prefix di, tri, etc. to alkyl name

Substituents listed in alphabetical order (disregarding prefix)

Branched Hydrocarbon SubstituentAlkyl groups

What is the name of the compound?

Hints

•Number Carbon chain from on side closest to first alkyl group

•Single carbon branch called methyl, triple carbon group called propyl

•More than one branch, use prefixes di-, tri-, etc.

2,4 dimethyl hexane 4 ethyl,5 methyl heptane

Tricky ones!!!

Each END of a line is a Carbon atom. No H’s are indicated, but they are assumed

See if you can name these.

Halohydrocarbons

Functional group is a halogen (X = F, Cl, Br, I)

General Formula R – X

Naming Select longest chain containing halogen Number so that C with halogen gets

lowest number

Ethers

Functional group - O –

General Formula R – O – R’

Naming Name the R group as an alkyl Name the R’ group as an alkyl End in ether

Aldehydes

Functional group - C – H

General Formula R – C – H

Naming Name the R group Change the ending to -al

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