Unit 6 Test: Types of Reactions

How to: tell if reaction will occur

- balance total molecular equation - complete total ionic equation (species of solid compounds are not separated) - complete net ionic equation ***reaction will not occur if all species are spectator ions (aka all the species cancel out)

Name the type of reaction: CaCO3 --> CaO + CO2

- decomposition

Redox Reaction

- oxidation and reduction occur at the same time - oxidized (more positive) - reduction (more negative) - single, synthesis, decomposition and combustion

Name the type of reaction: 2AgNO3 + Cu --> Cu(NO3)2 + 2Ag

- single

Name the type of reaction: Pb + FeSO4 --> PbSO4 +Fe

- single

Diatomic Elements (make a block 7 on periodic table)

- subscript of 2 when written alone in a chemical equation Elements: Hydrogen, Oxygen, Fluorine, Bromine, Iodine, Nitrogen, Chloride

How to: determine if compound is soluble or insoluble

- use table F

Is it a good idea to store hydrofluoric acid HF2 in an Al container?

- Table J no because Al is more reactive than H2. - Al pushes valence electrons onto Hydrogen ion to make that neutral - hydrofluoric will react in container

Things to note when predicting products:

- The compounds form must be neutral ionic compounds (which means you'll be paying attention to their charges) - You do NOT carry subscripts from the reactants to the product (unless they are polyatomic ions - You always balance your equation LAST Steps: 1) write the products 2) balance equation 3) check my making sure charges on each side of equations are equal 4) identify type of reaction

Insoluble Compounds

- Will precipitate - (s)

Soluble Compounds

- Won't precipitate - (aq)

Synthesis example

2Mg + O2 → 2MgO

Balance the reaction and name type: NH3 + H2SO4 --> (NH4)2SO4

2NH3 + 1H2SO4 --> 1(NH4)2SO4 - synthesis

Balance the reaction and name type: NaBr + Ca(OH)2 --> CaBr2 + NaOH

2NaBr + 1Ca(OH)2 --> 1CaBr2 + 2NaOH - double

Balance the reaction and name type: C5H9) + O2 --> CO2 + H20

4C5H9O + 27O2 --> 20CO2 + 18H20 - combustion

Combustion example

6O2 + C6H12O6 → 6CO2 + 6H2O

Basic Equation: Synthesis

A + B --> AB

Basic Equation: Single Replacement

AB + C --> AC + B (nonmetals switch) AB + C --> BC + A (metals switch)

Basic Equation: Double Replacement

AB + CD --> AD + BC *either the metals switch or the nonmetals switch

Basic Equation: Decomposition

AB --> A + B

Single Replacement example

Cu(SO4) + Al → Al2SO4 + Cu - metals replaced

Basic Equation: Combustion

CxHy + O2 --> CO2 + H2O

Decomposition example

H2O2 → H2 + O2

Table J: predict reactions

Metal X and Ion Y^+2 will react if Metal X is more reactive than Ion Y according to Table J - table J (top to bottom ---most reactive to least reactive)

Total and Net ionic: Chromium (III) nitrate (aq) + iron (II) sulfate (aq) --> chromium (III) sulfate (aq) + iron (II) nitrate (aq)

Molecular Equation: 2 Cr(NO3)3(aq) + 3 FeSO4(aq) --> 3Fe(NO3)2(aq) + Cr2(SO4)3 (aq) Total Ionic: 2 Cr^+3 + 6 NO3^-1 + 3 Fe^+2 + 3 SO4^-2 --> 2 Cr^+3 + 3 SO4^-2 + 6 NO3^-1 + 3 Fe^+2 Net Ionic: 0 = no reaction

Acid-Base Neutralization example

NH3 + H2CO → H2O + NH3CO2

Double Replacement example

Na2CO3 + Ni(NO)3→ 2Na(NO)3 + NiCO3

6 types of chemical reactions

Synthesis Decomposition Single Replacement Double Replacement Combustion Acid-Base Neutralization

Total and Net ionic: AgNO3 (aq) + KCl (aq) --> AgCl (s) + KNO3 (aq)

Total ionic: Ag^+1 + NO3 ^-1 + K^+1 + Cl^-1 --> AgCl (s) + K^+1 + NO3 ^-1 Net Ionic: Ag^+1 + Cl^-1 --> AgCl (s) - will react

Redox Reaction example: Pb + H3PO4 --> H2 + Pb3(PO4)3

_3_ Pb + _2_H3PO4 --> _3_H2 + _1_Pb3(PO4)3 ***PO4 is not included in redox reaction because it is a spectator ion Pb^0 --> Pb^+2 + 2e^- (oxidized) H^+1 + 1e^- --> H^0 (reduced) 2H^+1 + 2e^- --> 2H^0 Pb^0 + 2H^+1 + 2e^- --> 2H^0 +Pb^+2 + 2e^- Pb^0 + 2H^+1 --> 2H^0 +Pb^+2

Soluble or Insoluble: Copper (II) Sulfide

insoluble

Soluble or Insoluble: PbCO3

insoluble

Soluble or Insoluble: KBr

soluble

Soluble or Insoluble: Silver acetate

soluble