1. Look back at your notes or in the book if you don’t know the answers:
Starter 11/21/13
Look back at your notes or in the book if you don’t know the answers:
What is the difference between a physical and a chemical change?
List three examples of each.

2. What type of reaction occurs when you burn something?
Monday March 14th, 2016
Starter:
Name the following compounds
AgNO3
N3O7
Ca(OH)2
SiF4
AlPO4
CrSO4
Write the formulas
Iron (III) sulfide
Strontium nitride
Disilicon octahydride
Potassium phosphide
By the end of the day, Scholars will be able to:
Identify the three major parts of a reaction equation.
Classify a reaction based on its reactants and products
And answer a question like this:
What type of reaction occurs when you burn something?
Topic: Chemical Reactions
8-10 minutes

3. Chemical Reactions
Day 1

4. Requires a chemical change to occur.
Chemical reaction
the process by which one or more substances is changed into one or more different substances
Requires a chemical change to occur.

6. Painting

7. Phase changes (solid, liquid, gas)

8. Bleach Spots

9. Rust

10. Burning

11. A new hair cut

12. House on Fire

13. Folding paper

14. Rusty car

15. Sugar dissolving in water

16. Chocolate melting

17. Permanent Hair dye

18. Crumpling paper

19. Crystal light and water

20. Sanding down wood

21. Boiling Water

22. Sour Milk

23. Chemical equation
Chemical reactions are described using a chemical equation:
Zn + 2HCl  ZnCl2 + H2
There are three parts to a chemical equation
Reactants
Yield Sign
Products

24. Reactants
The starting substances or molecules that participates in a chemical reaction.
Reactants are found on the left side of a chemical equation.

25. Yield Sign Arrow that separates the reactants from the products.
Read as: yields, forms, or produces

26. Products A substance that forms in a chemical reaction
Found on the right side of the yield sign.

27. Types of Reactions
There are 5 main types of reactions that we will discuss in this class:
Synthesis
Decomposition
Single Replacement
Double Replacement
Combustion

28. Composition/synthesis
Two or more substances combine to form one new substance.
Many salts are prepared through a synthesis reaction.
Most synthesis reactions are exothermic.
An exothermic reaction gives out energy in the form of heat or light.
Usually written in the form:
A + B  AB
Example
2 Mg + O2 2 MgO

29. Decomposition
When a compound or molecule breaks up into simpler substances.
Decomposition reactions require heat or energy in order to break the bonds in the compound. This means that they are endothermic.
An endothermic reaction takes in energy from the surroundings.
Usually written in the form:
AB  A + B
Example
2 H2O ---> 2 H2 + O2

30. Single Replacement One element replaces another element in a compound.
Usually written in the form:
A + BC  AC + B
Example
Mg + 2 H2O ---> Mg(OH)2 + H2

32. Double Replacement
The cations and anions for each compound are switched to form two new compounds
Usually written in the form:
AB + CD  AD + CB
Example
Pb(NO3)2 + 2 KI  PbI2 + 2 KNO3

35. Combustion
Hydrocarbon reacts with oxygen to form carbon dioxide and water.
Usually written in the form:
CxHy + O2 H2O +CO2
Example
C10H O2 ---> 10 CO2 + 4 H2O

36. Sample Problems List what type the following reactions are:
NaOH + KNO3 --> NaNO3 + KOH
CH4 + 2 O2 --> CO2 + 2 H2O
2 Fe + 6 NaBr --> 2 FeBr3 + 6 Na
CaSO4 + Mg(OH)2 --> Ca(OH)2 + MgSO4
Pb + O2 --> PbO2
Na2CO3 --> Na2O + CO2

37. Solution to Sample Problems
Solutions to the Sample Problems
double displacement
Combustion
single displacement
Synthesis
decomposition

38. Group Work/Skit
With your group, produce a short scene that you can act out to describe one of the following types of reactions:
Synthesis
Decomposition
Single Replacement
Double Replacement

39. Describe the chemical reaction illustrated below :
___________________________________________ ___________________________________________ ____________
Type of reaction: ________________________________

40. Describe the chemical reaction illustrated below :
____________________________________________ ____________________________________________ __________
Type of reaction: ________________________________

41. Describe the chemical reaction illustrated below :
____________________________________________ ____________________________________________ __________
Type of reaction: ________________________________

42. Describe the chemical reaction illustrated below :
____________________________________________ ____________________________________________ __________
Type of reaction: ________________________________

43. Writing chemical equations
Two types of chemical equations:
Word equations
Symbol equations

44. Word Equations
Word equations are link together the names of the reactants with those of the products formed.
These equations do not need to be balanced.
Examples:
magnesium + oxygen  magnesium oxide
hydrogen + oxygen hydrogen dioxide

45. Symbol Equations
Symbol equations are shorthand notation used to explain a chemical reaction
They use the given element symbols found on the period table
These equations MUST be balanced
Examples:
Cl2 + 2KI  2KCl + I2
Zn + CuSO4  ZnSO4 + Cu

46. Writing Chemical Equations
STEP 1:
Determine the reactants and the products
STEP 2:
Assemble the equation
STEP 3:
Balance the equation (get the same # of atoms of each element on each side)

47. Examples: Write the word equation: Write the symbol equation:
CH4 + 2O2  CO2 + 2H2O
C6H12O6 + 6O2  6CO2 + 6H2O
Write the symbol equation:
Copper + oxygen  copper (II) oxide
Dihydrogen monoxide  hydrogen + oxygen

48. Chemical Equation Examples
Write the word equation for the following:
2K + 2H2o  2KOH + H2
CaCO3  CaO + CO2
Mg + 2HCl  MgCl2 + H2
Write the symbol equation for the following:
Iron + sulfur  Iron(II)sulfide
Aluminum + iodine  aluminum iodide
Carbon dioxide + water  glucose + oxygen