Nomenclature

CH. 3

The Types of CompoundsIonic

salts, acids and bases (Electrolytes)

Minerals

Covalentinorganic from non living systems

organic/biological- hydrocarbons, from living systems

polymers - large hydrocarbons

Metallic compoundPure elements, alloys and amalgams

biometallic - proteins or large compounds with metal centers

N aC lsodium chloride

B inary

C aC O 3ca lc ium carbonate

Ternary

F ixed C harge M eta ls

F eOIron (II) oxide

B inary

P bS O 4lead (II) sulfa te

Ternary

M ultip le cha rge m eta ls

IO N IC C om pounds

H C lhydrochloric ac id

B inary

H 3P O 4phosphoric ac id

Ternary

A cids

N H 4N O 3am monium nitra te

terna ry

A m m onium sa lts

N 2S 4dinitrogen te trasulfide

b inary

inorgan ic

C 8H 18

octane

b inary

C H 3C O C H 3

acetone

terna ry

organ ic

C O V A LE N T com pounds

C om pounds

COVALENT CompoundsCovalent compounds usually form when two non metal

atoms which both have a desire to gain electrons create a bond by sharing the electrons between them.

Neither atoms has full possession of the electron; therefore neither atom is charged.

Most organic compounds or hydrocarbons would fit into this category.

With over 10 million compounds, organics comprise 90% of all the known matter.

IONIC CompoundsIonic Compounds involve the transfer of electrons

from one atom making a cation to another atom making an anion.

The bond forms when the cation with a positive charge is attracted to the anion with a negative charge.

This electrostatic attraction is the ionic bond and usually occurs between a metal and a non metal atom.

Balancing ChargeNa+ & O-2

Na+x O-2

y x(+1) + y(-2) = 0find the smallest common factor

Na2O

Ca+2 & N-3 x(+2) + y(-3) = 0

Ca3N2

Fixed Charge Metals

1A always carries a +1 charge.

Electron configuration - ns1

2A always carries a +2 charge

Electron configuration - ns2

3A metals and 3B always carries +3

electron configuration - ns2np1 or ns2nd1

Naming inorganic compoundsWhen an element forms only one compound

with a given anion.

name the cation

name the anion using the ending (-ide-ide)NaCl sodium chloride

MgBr2 magnesium bromide

Al2O3 aluminum oxide

K3N potassium nitride

Naming ionic compoundsMany metals form more than one compound with some anions.

For these, roman numerals are used in the name to indicate the charge on the metal.

Cu1+ + O2- = Cu2O copper(I) oxide copper(I) oxide

Cu2+ + O2- = CuO copper(II) oxide copper(II) oxide

Metals with multiple chargesTransition metals.Transition metals.

Here it is easier to list the ones that to only have a single common oxidation state.

All Group 3B - 3+

Ni, Zn, Cd - 2+

Ag - 1+

Lanthanides and actinides - 3+

Summary

Simple rules that will keep you out of trouble most of the time.

Groups IA, 2A, 3A (except Tl) only have a single oxidation state that is the same as the group number - don’t use numbers.

Most other metals and semimetals have multiple oxidation states - use numbers.

If you are sure that a transition group element only has a single state, don’t use a number.

Polyatomic Ions need to know

Nitrate NO31-

Carbonate CO3-2

Sulfate SO4-2

Phosphate PO4-3

Chlorate ClO31-

Hydroxide OH-

Cyanide CN-

Acetate C2H3O21-

Ammonium NH4+

Polyatomic ions

When a compound contains a polyatomic ion, you simply use the given name.

NH4Cl ammonium chloride

NaOH sodium hydroxide

KMnO4 potassium permanganate

(NH4)2SO4 ammonium sulfate

Acids and Bases

Acid

HCl HNO3 H2SO4 H3PO4

Base

NaOH KOH Ba(OH)2 Al(OH)3

The bases listed are metal hydroxides and therefore are named as an ionic compound

Acids

Binary acids– the anion is a single element ending in -IDE– the acid is named hydro - root - ic acid– HCl - Hydrogen Chloride or– hydro- chlor - ic acid

Ternary Acids

• Anion ends in -IDE– hydro - root - ic acid– HCN, hydrogen cyanide is hydro cyan ic acid

• anion ends in -ATE– root - ic acid

– HNO3, hydrogen nitrate is nitr ic acid

• anion ends in -ITE– root -ous acid

– H3PO3, hydrogen phosphite is phosphorous acid

Naming Covalent MoleculesA simple set of rules can be used.

name elements in the order they appear in the formula.

use prefixes to indicate how many atoms there are of each type.

mono = 1mono = 1 tetra = 4tetra = 4 hepta = 7hepta = 7di = 2di = 2 penta = 5penta = 5 octa = 8octa = 8tri = 3tri = 3 hexa = 6hexa = 6 deca = 10deca = 10

use the ending (-ide) for the second element listed in the formula.

Naming covalent compounds

The rule may be modified to improve how a name sounds.

ExampleExample - use monoxide not monooxide.

N2O5

CO2

COSiO2

ICl3P2O5

CCl4

dinitrogen pentoxidecarbon dioxidecarbon monoxidesilicon dioxideiodine trichloridediphophorous pentoxidecarbon tetrachloride

Naming Organic Compounds

• Contain Carbon and hydrogen atoms

• Use prefix to count number of carbons present in the compound

• functional groups

Nomenclature overviewNow that a large number of nomenclature rules

have been introduced, we need to review them.

Simple binary ionic compounds

Ionic compounds of metals with multiple charges

Compounds containing polyatomic ions

Simple molecular compounds

It’s useful to be able to identify which system to use by looking at the chemical.

A bit more on nomenclature

When the first element is a metal then usually:

If only one other element is present and the second element is a non-metal -name the metal first - as element.Name non-metal second with -ide-ide ending

If more than one other element is present -name the metal first - as element.The rest is most likely a polyatomic ionso use the name from the table in book.

A bit more on nomenclatureIs a metal presentas the first element?

Can the metal havemore than oneoxidation state?

Use prefixes(mono, di, tri ...)

Roman numeralsare not needed.

Use Roman numerals to indicate oxidation state of metal

NoNo

NoNo

YesYes

YesYes

Naming Activities

• Naming Flowchart