1. Reaction Types

2. Nuclear Reactions Transmutations Fission and Fusion
Natural and Artificial
Alpha and Beta Decay, Positron Emission
Fission and Fusion

3. Transmutations
Any reaction where one element is transformed into a different element
Nuclear Reactions
Natural
Has one reactant
Alpha and Beta Decay, Positron Emission
Artificial
Has more than one reactant
Particle Accelerators

4. Radioactive Decay
Radioisotopes will undergo decay reactions to become more stable
Alpha Decay
Beta Decay
Positron Emission

5. Fission Splitting of a larger atom into two or more smaller pieces
Nuclear Power Plants
One Example:

6. Fusion Joining of two or more smaller pieces to make a larger piece
Sun, Stars
Examples

7. Chemical Reactions Synthesis Decomposition Single Replacement
Double Replacement
Neutralization
Combustion
Reduction-Oxidation
Organic Chemistry Reactions

8. Chemical Reactions Synthesis Decomposition 1 product 2Mg + O2  2MgO
1 reactant
2NaCl  2Na + Cl2

9. Chemical Reactions Single Replacement Double Replacement
Reactants - Element and Compound
Metal replaces metal, nonmetal replace nonmetal
Zn + 2HCl  ZnCl2 + H2
Double Replacement
Reactants – 2 compounds
Front pieces trade places
AgNO3 + NaCl  NaNO3 + AgCl

10. Neutralization Acid + Base  Water + Salt HA + BOH  HOH + BA
Double Replacement Reaction
HA + BOH  HOH + BA
Examples:
HCl + NaOH  H2O + NaCl
HNO3 + LiOH  H2O + LiNO3
H2SO KOH  2 H2O + K2SO4

11. Combustion
Chemical change in which an element or a compound reacts with oxygen, often producing energy in the form of heat and light
O2 is a reactant
2Mg + O2  2MgO

12. Redox Reactions
Reduction – Oxidation, or redox, involves the transfer of electrons
Reduction – gain of electrons
Oxidation – loss of electrons
LEO goes GER
Lose Electrons Oxidation
Gain Electrons Reduction

13. Net Ionic Equation
Shows only the ions involved in the redox reaction, not spectator ions
Still shows conservation of mass and charge
Zn + CuSO4  Cu + ZnSO4
Zn + Cu+2  Cu + Zn+2

14. Half Reactions
Only shows one element and how many electrons are gained or lost
Zn + CuSO4  Cu + ZnSO4
Zn  Zn e- Oxidation
Cu e-  Cu Reduction

15. Organic Chemistry Reactions
Saponification
Fermentation
Combustion
Addition
Substitution
Polymerization (2 types)
Esterification

16. Organic Chemistry Reactions
Saponification
Production of Soap
Fermentation
Production of ethanol and CO2 from sugar
C6H12O6  2C2H5OH + 2CO2

17. Combustion Complete Combustion of a Hydrocarbon Example:
CxHy + O2  CO2 + H2O
Example:
C3H8 + 5O2  3CO2 + 4H2O

18. Addition Addition of a halogen onto an alkene or alkyne Br Br │ │
│ │
H─ C≡ C─ H + Br─Br  H─ C= C─ H
Br Br Br Br
│ │ │ │
H─ C= C─ H + Cl─Cl  H─ C─ C─ H
│ │
Cl Cl

19. Substitution
Substitution of one halogen in place of a hydrogen on an alkane
H H H H
│ │ │ │
H─ C─ C─ H + Cl─Cl  H─ C─ C─ H H ─ Cl
H H H Cl
H H Br H
│ │ │ │
H─ C─ C─ H + Br─Br  H─ C─ C─ H H ─ Br
H Cl H Cl

20. Polymerization -(C2H4)n-
Connecting of smaller pieces into a long repeating chain
Plastics, starches, nylon
Two types:
Addition
Condensation
-(C2H4)n-

21. Esterification Production of an Ester from an alcohol and acid
Acid + Alcohol  Ester + Water
O H O H
ǁ │ ǁ │
H─ C─ O ─ H + H ─O ─C ─H  H─ C─ O ─ C─ H H2O
│ │
H H

22. Other Types
Entropy
Phase Changes
Ionic Dissociation

23. Entropy
Increasing Entropy
Solid  Liquid  Gas
Solid  Dissolved

24. Phase Changes
Substances change in phase only

25. Ionic Dissociation
Ions separate as solvent molecules mix