TYPES OF REACTIONS. LAW OF CONSERVATION OF MASS Matter cannot be created nor destroyed just rearranged Chemical Equation- Represents, with symbols and.

TYPES OF REACTIONS

LAW OF CONSERVATION OF MASS Matter cannot be created nor destroyed just rearranged Chemical Equation- Represents, with symbols and formulas, the identities and relative amounts of the reactants and products in a chemical reaction

INDICATIONS OF A CHEMICAL REACTION Production of heat, light, or temperature change

Production of a gas Formation of a precipitate Color change Odor change

SYMBOLS USED IN CHEMICAL EQUATIONS

NH4OH(aq)  →   NH3(g) + H2O(l)

→→ Yields- indicates result of reaction

→→

←←

Indicates reversible reaction

(s)(s) solid

(l)(l) Liquid

(g)(g) Gas

(aq)(aq) Aqueous solution- dissolved in water

SYMBOLS USED IN CHEMICAL EQUATIONS

ºCºC

→→

Temperature at which reaction is carried out

PressurePressure

→→

Pressure exceeds normal atmospheric pressure

↑↑ (g) gaseous product

∆ ∆ heatheat

→→

→→

Reactants are heated

MnOMnO22

→→

Catalyst, alters rate of reaction

2H2O2 (l) 2H2O (l) + O2 (g) MnO2

7 DIATOMIC COVALENT MOLECULES The 7 elements are never alone in nature and are always a molecule. All of the following are Nonpolar Covalent Br2- liquid Bring =Bromine H2- gas Home =Hydrogen I2- solid Important =Iodine Cl2- gas Class =Chlorine N2- gas Notes =Nitrogen O2- gas Or =Oxygen F2- gas Fail =Fluorine

SYNTHESISA + B ABExamples:

2Mg + O2 2MgO

Sr + Br2 SrBr2

SYNTHESIS

+

+

DECOMPOSITION AB A + BExamples:

2H2O 2H2 + O2

2H2O2 2H2O + O2 Blood

Electrolysis of water- Decomposition of water using an electric current

DECOMPOSITION

+

+

SINGLE-REPLACEMENTA + BC AC + B

Examples: 2Na + 2H2O 2NaOH + H2

Zn + 2HCl ZnCl2 + H2

Fe + CuCl2 Cu + FeCl2

SINGLE-REPLACEMENT

+ +

+ +

DOUBLE-REPLACEMENTAB + CD AD + CB

Examples:KI + Pb(NO3)2 KNO3 + PbI2

AgNO3 + NaCl AgCl + NaNO3

DOUBLE-REPLACEMENTThey generally take place in an aqueous solution and they often produce a precipitate, gas, or a molecular compound.

COMBUSTIONA combustion reaction is where a substance reacts with

oxygen with the release of heat and usually the production of a flame.

A hydrocarbons will react with oxygen and combust into carbon dioxide and water.

C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(g)   A nonmetal will react with oxygen and combust into its nonmetal oxide and water SiH4 + 2O2 SiO2 + 2H2O

EXAMPLE PRACTICE AlBr3 + K KBr + Al

Single replacement

PRACTICE FeO + PdF2 FeF2 + PdO

Double replacement

P4 + Br2 PBr3

Synthesis

LiCl + Br2 LiBr + Cl2

Single replacement

PbBr2 + HCl HBr + PbCl2

Double replacement

C3H8 + 5O2 3CO2 + 4H2O

Combustion

CoBr3 + CaSO4 CaBr2 + Co2(SO4)3

Double replacement

Na3P + CaF2 NaF + Ca3P2

Single replacement

•SrBr2 Sr + Br2

Decomposition

Mn + HI H2 + MnI3

Single replacement

•SrBr2 Sr + Br2

Synthesis

Li3PO4 + NaBr Na3PO4 + LiBr

Double replacement

CaF2 + Li2SO4 CaSO4 + LiF

Single replacement