B onds between atoms are created when electrons are paired up by being transferred or shared. Atoms tend to form bonds that will allow it to obtain a full.

•Bonds between atoms are created when electrons are paired up by being transferred or shared.•Atoms tend to form bonds that will allow it to obtain a full valence shell.

Chemical Bonds

Two Types of Chemical Bonds:

Ionic Bonds Covalent Bonds

-Electrons are transferred from one atom to another

-Electrons are shared between atoms.

- Usually occurs between a metal and nonmetal

- Usually occurs between two nonmetals

CompoundsCompounds are formed when two or more kinds of atoms are bound together chemically. Compound can be either ionic or covalent.

Examples:

Why do these bonds occur?Remember: In a neutral atom the number of protons

and neutrons are equal but the atom might be unhappy because it does not have a complete outer shell of electrons(8 electrons). All atoms want to be happy like the Nobel gases!!!!!

How can atoms be happy?-By creating either an ionic or covalent bond.-If they create an ionic bond they either gain or

lose an electron.-Positive ion form by losing an electron-Negative ion form by gaining an

electron

Groups turning Ionic...

Positive Ions (cation)Group 1 Loses 1 electron Ion with a +1

Charge

Group 2 Loses 2 electrons

Ion with a +2 Charge

Group 13 Loses 3 electrons

Ion with a +3 Charge

Negative Ions (anion)Group 15 Gains 3

electronsIon with a -3 charge

Group 16 Gains 2 electrons

Ion with a -2 charge

Group 17 Gains 1 electron Ions with a -1 charge

Prefix number indicated

mono- 1di- 2tri- 3

tetra- 4penta- 5hexa- 6hepta- 7octa- 8nona- 9

deca- 10

Naming Binary Covalent Compounds

Formula Names

N2F6 Dinitrogen Hexafluoride

CO2

SiF4

CBr4

NCl3

P2S3

CO

NO2

SF2

PF5

SO2

NO

CCl4

P2O5

Examples:

Naming Binary Ionic CompoundsRules1. The Cation (positive ion) is named first, the Anion second.2. Monoatomic Cations take the element name                             Na+ --> Sodium                             Ca2+ --> Calcium3. Monoatomic Anions take the elements name and ends with "-ide"                             Cl- --> Chloride                             NaCl --> Sodium Chloride                             Li3N --> Lithium Nitride

Note** Greek prefixes are not used to indicate the number of atoms of each element in the formula unit for the compound (e.g., Na2O is named "sodium oxide" not "disodium oxide", or

"disodium monoxide").

Formula Name Formula Name

a. Li2O Lithium Oxide n. K2O

b. CsCl o. RbI 

c. MgS  p. Mg3N2

d. CaBr2 q. Ca3P2

e. BaI2 r. Al2S3

f. KH s. Ag2O

g. Na2S t. NaH

h. AlN u. CaO 

i. AgF v. Na2S

j. ZnO w. LiI

k. CdI2 x. CdS 

l. BaS y. ZnCl2

m. LiCl z. CsI

Examples:

Naming Ionic Compounds using Roman Numerals

(The Stock System of Naming)

How do we name compounds when the cation of variable charge is involved?

•Some elements have more then one oxidation number and when naming a compound these must be identified. •Roman numerals are shown after the cation in parenthesis(  ) to indicate the oxidation number.•To determine what the oxidation number is, you must use the anion (negative ion) to determine what the positive oxidation number is.

Example-  Pb(NO3)4   write the name  "lead nitrate".

Since lead has more than one oxidation state we must figure out which lead we have. Since each nitrate (4 of them) has a 1- charge, the Pb must be 4+. So our roman numeral will be (IV).

Pb(NO3)4  is named "lead(IV)  nitrate"

Formula Name Formula Name

 FeCl2 iron (II) chloride SnCl4

CoBr3 FeP

MnO2 Hg2S

NiBr2 PbO

HgO AuI

CuF2 SnS2

CuI FeBr3

SnBr2 Cr2O3

Au3P CoS

Cr2S3 MnI2

NiBr NiS

FeS PbO2

PbCl4 Mn2O5

II. Nonbinary Ionic compounds

(Use of Polyatomic Ions)

Nonbinary means more than two different elements

Step 1 First give the name of the metal, followed by the memorized polyatomic ion name.

Step 2 If the metal is to the right of group IIA, then aRoman numeral is used after the metal to describe the charge of the metal. Except Ag, Zn, and Al.

Examples

NaOH Fe(NO3)3

Fe(SO4)2Zn(C2H3O2)2

Formula Name Formula Name

NH4+ Ammonium O2

2- Peroxide

C2H3O2- Acetate NO3

- Nitrate

CO32- Carbonate NO2

- Nitrite

HCO31- Hydorgen

carbonateSO4

2- Sulfate

ClO4- Perchlorate SO3

2- Sulfite

ClO3- Chlorate PO4

3- Phosphate

ClO2- Chlorite PO3

3- Phosphite

ClO- Hypochlorite CrO42- Chromate

CN- Cyanide Cr2O72- Dichromate

OH- Hydroxide MnO41- Permanganate

Memorized Polyatomic Ion List

II. Nonbinary Ionic compoundsNonbinary means more than two different elements

Step 1

First give the name of the metal, followed by the memorized polyatomic ion name.

Step 2

If the metal is to the right of group IIA, then aRoman numeral is used after the metal to describe the charge of the metal. Except Ag, Zn, and Al.

Examples

NaOH Fe(NO3)3

Fe(SO4)2Zn(C2H3O2)2

Sodium hydroxide

CO

II. Nonbinary Ionic compoundsNonbinary means more than two different elements

Step 1

First give the name of the metal, followed by the memorized polyatomic ion name.

Step 2

If the metal is to the right of group IIA, then aRoman numeral is used after the metal to describe the charge of the metal. Except Ag, Zn, and Al.

Examples

NaOH Fe(NO3)3

Fe(SO4)2Zn(C2H3O2)2

Sodium hydroxide

Iron(III) nitrate

II. Nonbinary Ionic compoundsNonbinary means more than two different elements

Step 1

First give the name of the metal, followed by the memorized polyatomic ion name.

Step 2

If the metal is to the right of group IIA, then aRoman numeral is used after the metal to describe the charge of the metal. Except Ag, Zn, and Al.

Examples

NaOH Fe(NO3)3

Fe(SO4)2Zn(C2H3O2)2

Sodium hydroxide

Iron(III) nitrate

Iron(II) sulfate

II. Nonbinary Ionic compoundsNonbinary means more than two different elements

Step 1

First give the name of the metal, followed by the memorized polyatomic ion name.

Step 2

If the metal is to the right of group IIA, then aRoman numeral is used after the metal to describe the charge of the metal. Except Ag, Zn, and Al.

Examples

NaOH Fe(NO3)3

Fe(SO4)2Zn(C2H3O2)2

Sodium hydroxide

Iron(III) nitrate

Iron(II) sulfate Zinc acetate

NOMENCLATURE

COVALENT BONDS(non-metal with non-

metal)

IONIC BONDS(metal with non-metal)

POLYATOMIC ION(more than 2 elements in

the compound)

Rules:• Use pre-fixes (mono-, di-, tri-, tetra-, penta-, etc…)• Second element ends

with the suffix “-ide)

Rules:• Find polyatomic ion

on the cheat sheet.• If the polyatomic ion

is listed first, then the second element ends with the suffix “-ide)

• If the polyatomic ion is listed last, then simply name the first element.

Rules:• No pre-fixes!• Second element ends

with the suffix “-ide)

If there is a TRANSITION METAL (groups 3-12) present, then use roman numerals (I, II, III, IV, V)

Balancing Chemical Equations

Recall: •The law of Conservation of Matter (mass). Matter can not be created or destroyed only changed.•A chemical equation is a way to show matter being changed from one compound to another.

For example:H + O ------> H O

•This equations show when hydrogen and oxygen combine it makes water. But look closer.... In the first half of the equation you have one hydrogen and one oxygen and in the second you have two hydrogen and one oxygen. You must balance this equation due to the law of conservation of matter. With the equation the way it is, you are saying that you created another hydrogen and you can not create matter.

2H + O-----> H ONow it is Balanced!!! Two hydrogen on each side and one oxygen on each side.

2

2

PRACTICE:

PRACTICE:

4 Types of Chemical Reactions

1. Single Replacement Reaction- Occurs when one element replaces another element in a

compound.A + BC -----> B +AC

2. Double Replacement Reaction- Occurs when cations of two compounds switch places.

AB + CD ----> CB + AD3. Decomposition Reaction

-Occurs when a single compound breaks down into simpler compounds.

AB -----> A + B4. Synthesis Reaction

-Occurs when two of more substances combine to form a single substance.

A + B ----> AB