Single Replacement Reactions:

A +BC AC + BAn element takes the place of another element in a compound. It could be a metal taking the place of another metal or hydrogen or a halogen taking the place of another halogen.

Mg(s) + FeSO4(aq)

Cl2(g) + KBr(aq)

Fe(s) + MgSO4 (aq) Br2 (aq) + KCl(aq)

MgSO4 (aq) + Fe(s)

KCl(aq) + Br2 (aq)

N.R.

N.R.

Magnesium is more active than Iron and

Chlorine is more active than Bromine!

Activity Series: For metals: Li

CsRbKBaSrCaNaLaMgBeAlMnZnCrFeCdCoNiSnPbH

ActivityDecreases

FClBrI

Lithium

Potassium

CalciumSodium

Magnesium

Aluminum

ZincChromiumIron

NickelTinLeadHydrogen

CopperMercurySilverPlatinumGold

Fluorine

ChlorineBromineIodine

ActivityDecreases

For halogens:

CesiumRubidium

HCuHgAgPtAu

Barium

CadmiumCobalt

Manganese

Beryllium

Lanthanum

Strontium

Hydrogen

AB +CD AD + CB

MgCO3(s) + FeSO4(aq)

BaCl2(aq) + KBr(aq)

Fe(NO3)3(aq)+Ca3(PO4)2(s) CuBr2 (aq) + KCl(aq)

It is a reaction between two ionic compounds in which the ions switch positions: The positive of the first combines with the negative of the second and the positive ofthe second with the negative of the first.

MgSO4 (aq) + FeCO3 (s)

BaBr2(aq) + KCl(aq)

Ca(NO3)2(aq)+ FePO3(s)

CuCl2 (aq) + KBr(aq)

2

22

23

2 2

Double Replacement Reactions :

One of the types of double-replacement reactions is when a precipitate is formed. When a precipitate is formed, the compound will be either insoluble or slightly soluble. An

example of this type of reaction is:

Pb(NO3)2(aq) + 2KI (aq) --> PbI2(s) + 2KNO3 (aq)

When one of the products is a gas, double-replacement

reactions also occur. For example:

FeS(s) + 2HCl(aq) -->

H2S(g) + FeCl2(aq)

An example of a double-replacement reaction where water is one of the products is:

HCl(aq)+ NaOH(aq) --> NaCl (aq) + H2O(l)

This is a neutralization reaction:

Acid + Base = Salt + Water

http://www.cameron.k12.wi.us/high/chemistry/drreac.html

Double-replacement reactions

Combustion of a hydrocarbon: Hydrocarbon+O2(g)C O2(g)+H2O(g)

When a substance combines with oxygen releasing a large amount of energy in the form of light and heat, it is a combustion

reaction. An example of a combustion reaction is: C3H8 + 5O2 --> 3CO2 + 4H2O

http://www.cameron.k12.wi.us/high/chemistry/comreac.htmlhttp://newtraditions.chem.wisc.edu/FPTS/fbeqns/eqncombf.htm

+ +

Decomposition Reactions: ABC… A +B +C …

Decomposition: the breaking down of a compound into one or more substances. (usually energy is required)

EXAMPLES: CO2 (g) ----- C(s) + O2(g)

2Fe2O3 (s)- 4Fe(s) + 3O2 (g)

Generalizations:1. A binary compound decomposes into two elements.2. A hydroxide of the metal decomposes into an oxide

of the metal and water.3. A ternary salt decomposes into an oxide of the metal

and an oxide of the non metal.4. A ternary or oxoacid decomposes into the oxide of a

non metal and water .