chapter 3 ~ chemical reactions

Chapter 3 ~ Chemical Reactions

Balancing Combustion ReactionsWrite a balanced equation for the

combustion of butane.

Chemical Equilibrium

Solution Terms• Solvent• Solute• Homogeneous mixture• Aqueous• Electrolyte (strong / weak)• Nonelectrolyte

Solubility of Ionic Compounds in Water

Exercise 3.4 ~Predict the solubility of the following

compounds:

LiNO3

CaCl2

CuONaC2H3O2

List as many types of chemical reactions as you can.

Give an example of each type of reaction

Precipitation Reactions aka: Double Replacement Rxns

Exercise 3.5 ~ Will precipitation reactions occur between:

Sodium carbonate and copper (II) chloride

Potassium carbonate and sodium nitrate

Nickel(II) chloride and potassium hydroxide

Writing Net Ionic EquationsExercise 3.6Write balanced net ionic equations for:Aluminum chloride and sodium

phosphate

Iron(III) chloride and potassium hydroxide

Lead(II) nitrate and potassium chloride

Acid / Base ReactionsCharacteristics of Characteristics

of Acids Bases

HCl + Zn

Using the Activity Series

Al + CuCl2

Cu + NaCl

Zn + HCl

Cu + HCl

Ca + H2O

Naming Acids

Binary Acids

Oxyacids

Acids and BasesDefinitions:Arrhenius Acid: an acid is a substance that

ionizes in water to produce H+ or H3O+ ionsHCl + H2O

Arrhenius Base: a base produces OH- ions in water

NaOH

Bronsted-Lowry Acids and BasesAcid: a substance that donates a proton to

any other substanceBase: a substance that accepts a proton

from another substanceHNO3 + H2ONH4

+ + H2OFe(H2O)6

3+ + H2O

NH3 + H2O

Amphiprotic Substances

Act as a Bronsted acid OR a Bronsted baseHCO3 + H2O H3O+ + CO3

2-

OR HCO3 + H2O H2CO3 + OH-

Conjugate Acid-Base Pairs

HCO3 + H2O H3O+ + CO32-

Conjugate acid-base pairs differ by the presence of a _____________________________

Ionization of Acids and Bases

Strong Acids

Weak Acids

Diprotic and polyprotic acids

Ionization of bases

Common Acids and Bases

Metal and Nonmetal Oxides

• CO2• SO2• SO3• NO2• CaO• MgO

Reactions of Strong Acids and Strong Bases

HCl + NaOH

HNO3 + NaOH

H2SO4 + Ca(OH)2

Mg(OH)2 + HCl

Reactions of Weak Acids

• Acetic Acid and sodium hydroxide

Gas Forming Reactions

Acids + CarbonatesCalcium carbonate + HCl

Calcium carbonate + HC2H3O2

Acids + bicarbonatesNaCO3 + HC4H5O6

Gas Forming Reactions

• Acids + sulfidesNa2S + HCL

Gas Forming Reactions

• Acids + sulfitesNa2SO3 + HCl

• Ammonium salts + basesNH4Cl + NaOH

Exercise 3.11

Write the equation for the reaction of barium carbonate and nitric acid

Write a balanced equation for the reaction of ammonium sulfate and sodium hydroxide

Driving Forces for Reactions

• Precipitation Reactions

• Gas forming reactions

• Acid-base reactions

• Oxidation-reduction reactions

TEST TUBE WITH NAIL -OBSERVATIONS:

EXPLANATIONS?????

CuSO4 and NaCl combine:

Activity Series: Fe, Cu

Iron ions react with oxygen and water:

New Concepts:

Complex ion ~

Redox Reactions ~

Base Anhydride ~

Oxidation Numbers

• As opposed to valence number:

Rules for Assigning Oxidation Numbers1. Pure elements have oxidation numbers of 02. Single element ions have oxidation numbers

equal to their charges3. F always an oxidation number = -14. Cl, Br, I always = -1 except in compounds with

O or F5. H has an oxidation number of +1 unless it is a

hydride ion (-1)6. O has an oxidation number of -2 unless it is a

peroxide (-1) or superoxide7. Oxidation numbers of elements in polyatomic

ions always = the charge of the ion8. Oxidation numbers in compounds always add

to 0.

Determining Oxidation Numbers

• Fe2O3

• CO32-

• H2SO4

• NO21+

Oxidation-Reduction Reactions

Fe2O3(s) + 3CO(g) 2Fe(s) + 3CO2(g)

Redox Reactions

• Element oxidized

• Element reduced

• Oxidizing agent

• Reducing agent

Breathalyzer Reaction

3CH3CH2OH + 2Cr2O72- + 16 H3O+

3CH3CO2H + 4 Cr3+ +27H2O

9 Oxidation States of N

• NO31- NO2

• NH4 1+ N2H4

• NH2OH N2

• N2O NO• N2O3

H2O2 + Blood

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