1) Covalent2) Ionic3) Organic

◦ Entire unit in Chem 30S

Generally a bond between 2 non-metal elements General Rules

◦ First element is named as listed on periodic table◦ Second element has the suffix –ide◦ Prefix used for each element to indicate the # of atoms

If only one atom of first element → No prefix used

Number Prefix

4 tetra

1 mono

2 di

3 tri

5 penta

6 hexa

7 hepta

8 octa

9 nona

10 deca

Name the following◦ CO2

◦ CO◦ CCl4◦ N2O4

◦ SF6

◦ P2Cl5◦ PI3◦ P5Cl8

Carbon dioxide

Carbon oxide

Carbon tetrachloride

Dinitrogen tetraoxideSulfur hexafluoride

Diphosphorus pentachloride

Phosphorus triodide

Pentaphosphorus octachloride

Write the formulas for the following◦ Tetranitrogen decaoxide◦ Disulfur pentafluoride◦ Hexaselenium tribromide◦ Nitrogen monoxide◦ Aluminum Chloride

N4O10

S2F5

Se6Br3

NO

IONIC

3 subcategories◦ Monatomic Ions◦ Polyatomic Ions◦ Transitional Metals

Can use both monatomic and polyatomic Rules

◦ Formula must be neutral◦ No # prefixes used as only one possible combination

with ions involved◦ Cation (+ve) listed first, Anion (-ve) listed second

Monatomic ions are ions that contain only 1 atom Anion has suffix –ide Examples

◦ NaCl◦ AlCl3◦ MgO◦ Ga2P3

◦ HF◦ NaH

Sodium Chloride

Aluminum Chloride

Magnesium Oxide

Gallium PhosphideHydrogen Fluoride

Sodium Hydride

Entire unit MUST be neutral◦ Add appropriate # of each ion to balance charges

Example Aluminum Fluoride

Al3+ F-

+3 -1 = +2

Al3+ 3F-

+3 -3 = 0

AlF3

Example Gallium Oxide

Ga3+ O2-

+3 -2 = +1

Ga3+ 2O2-

+3 -4 = -1

Ga2O3

2Ga3+ 2O2-

+6 -4 = +2

2Ga3+ 3O2-

+6 -6 = 0

Examples◦ Write the formulas for the following

Lithium Sulfide Magnesium Bromide Hydrogen Nitride Aluminum Phosphide Boron Sulfide

Li2S

MgBr2

H3N

AlPB2S3

Ions with more than one atom◦ Eg)

NO3- (Nitrate)

PO43- (Phosphate)

NH4+ (Ammonium)

◦ The entire item has a charge, not each element in the polyatomic ion

Look at page. 257 The exact ion name is used

Examples◦ NaBrO3

◦ Na2C2O4

◦ Ca(NO3)2

◦ NH4Cl

◦ Al2(SO3)3

Sodium Bromate

Sodium Oxalate

Calcium Nitrate

Ammonium ChlorideAluminum Sulfite

Entire unit MUST be neutral◦ Add appropriate # of each ion to balance charges

Example Potassium Permanganate

K+ MnO4-

+1 -1 = 0

KMnO4

Example Magnesium Nitrite

Mg2+ NO2-

+2 -1 = +1

Mg2+ 2NO2-

+2 -2 = 0

Mg(NO2)2

Transitional Metals can have different charges◦ Depends on the situation◦ Example

Fe2+

Fe3+

Ti2+

Ti4+

When naming, must determine what the charge is◦ Indicated by using Roman numerals

Must know Roman numerals 1-10

Example FeO

Fe2+ O2-

-2 = 0+2

Iron (II) Oxide

Example Fe2(CO3)3

2Fe 3CO32-

-6 = 0+6

Iron (III) Carbonate

3+

Write the names for the following◦ TiS2

◦ CuCl◦ AgNO3

◦ CuSO4

◦ V(ClO4)5

Titanium (IV) Sulfide

Copper (I) Chloride

Silver (I) Nitrate

Copper (II) SulfateVanadium (V) Perchlorate

The name indicates the charge◦ Balance as normal

Example Zinc (II) Chloride

Zn2+ Cl-

+2 -1 = +1

Zn2+ 2Cl-

+2 -2 = 0

ZnCl2

Examples◦ Nickel (II) Nitride◦ Chromium (IV) Oxalate◦ Iron (III) Cyanide◦ Mercury (I) Acetate (careful)

Ni3N2

Cr(C2O4)2

Fe(CN)3

Hg2(CH3COO)2

Peroxide◦ A polyatomic ion with 2 oxygen atoms with a 2- charge◦ Very reactive ion◦ Explosive in some cases

H20 Dihydrogen Monoxide (Covalent) H2O2 Hydrogen peroxide (Ionic)

Example MgO2

If the oxygen is an oxide ion, then we would have -4

The Mg is +2 This is not balanced Therefore the O2 item must have a -2 charge Peroxide (O2

2-)

P.282 #’s 65-70◦ Omit #67 d)& #69 i) & #66 h)