1. Chemical Reactions
Unit7

2. Chemical Reactions Reflect: What is a chemical reaction?
Why do they occur?

3. Chemical Reactions A Chemical Reaction is:
A rearrangement of atoms creating a new substance

4. Chemical Reactions A Chemical Reaction is:
Indicated by a color change, bubbles (a gas) or a precipitate (a solid formed).

5. Chemical Reactions A Chemical Reaction is:
Made up of reactants that change into products w/ different properties.

6. Chemical Reactions A Chemical Reaction is:
A rearrangement of atoms creating a new substance
Indicated by a color change, bubbles (a gas) or a precipitate (a solid formed).
Made up of reactants that change into products w/ different properties.

7. Word Equations Zn(s) + Pb(NO3)2(aq) -> Zn(NO3)2(aq) + Pb (s)
Directions: Write the word equations below as a
correct chemical equation.
1). Zinc (s) + Lead (II) Nitrate (aq) yields Zinc Nitrate (aq) + Lead (s)
Zn(s) Pb(NO3)2(aq) > Zn(NO3)2(aq) + Pb (s)

8. Word Equations 4Al(s) + 3O2(g) -> 2Al2O3 (aq)
4 Aluminum (s) + 3 Oxygen (g) yields 2 Aluminum Oxide(s)
4Al(s) O2(g) > Al2O3 (aq)

9. Conservation of Matter
Chemical Reactions
Conservation of Matter
All balanced chemical equations show a conservation of matter by the use of coefficients.
For mass to remain constant before and after a chemical reaction the number of atoms of each element must be the SAME before and after a chemical reaction.

10. Counting Atoms in a Reaction

11. Chemical Reactions
All balanced chemical reactions show a conservation of mass, energy and charge by the use of coefficients in front of each the molecular formulas.

12. Chemical Reactions
For mass to remain constant before and after a chemical reaction the number of atoms of each element must be the same before and after a chemical reaction.  These two statements demonstrate the Law of Conservation of Matter!

13. Balancing Equations
Example 1: Ca + O2  CaO

14. Balancing Equations
Example 2: Na + Cl2  NaCl

15. Balancing Equations
Example 3: FeCl2 + Na3PO4  NaCl + Fe3(PO4) 2

16. Balancing Equations Example 4:
Methane (CH4) reacts with oxygen to make carbon dioxide and water

17. Balancing Equations
Example 5: Fe(s) + O2(g)  Fe2O3(s)

18. Cu(s) + H2SO4(aq)  CuSO4(aq) + H2O(l) + SO2(g)
Balancing Equations
Example 6:
Cu(s) H2SO4(aq)  CuSO4(aq) H2O(l) SO2(g)

19. Balancing Equations Example 7:
Calcium hydroxide + Phosphoric Acid  Calcium Phosphate + water

20. Balancing Equations
Chemical equations can also include the physical states: (S) indicates a ___Solid_______ (l) indicates ____Liquid________ (g) indicates ____Gas________ (aq) indicates __Aqueous (dissolved in water)

21. Types of Chemical Reactions
Reflect:
When looking at a chemical equation what side are the reactants on?
What side are the products on?
What does the “” mean?

22. 4 Major Types of Chemical Reactions
2H2 + O2 -> 2H2O
Two reactants make one product
Synthesis = to make something

23. 4 Major Types of Chemical Reactions
2NaCl -> 2Na + Cl2
4 Major Types of Chemical Reactions
One reactant breaks up into multiple products
Decomposition = breakdown

24. 4 Major Types of Chemical Reactions
Mg + CuCl2 -> MgCl2 + Cu
The reactant metal that is by itself is more reactive than the metal in the ionic compound
4 Major Types of Chemical Reactions
The lone metal is more reactive than the metal in the ionic compound
Single replacement= single element switching places with bonded cation
Table J

25. 4 Major Types of Chemical Reactions
NaCl + Ag(NO3) -> Na(NO3) + AgCl
A solid (ppt), gas or water is created in the product
4 Major Types of Chemical Reactions
A solid (ppt), gas, or water is created in the products
Double replacement = two elements switching places
Table f

26. Single Replacement Reactions
Reflect:
Look at Table J in your Reference Tables.
What is the most reactive metal?
What is the most reactive nonmetal?
What is the least reactive metal?
What is the least reactive nonmetal?

27. Remember ?

28. Single Replacement Reactions
Single Replacement Reactions: *Where part of an ionic compound is removed and replaced by a new more reactive element.

29. Single Replacement Reactions
Practice comparing the reactivity of elements on Table J: K & Ba Cr & Zn Au & Na F2 & Br2 Cl2 & I2 Al & Br2

30. Single Replacement Reactions
 Single Replacement
Reactions will occur if:
The element that is by itself is more reactive than the
element you are comparing it to in the ionic
compound.

31. Single Replacement Reactions
Predicting Single Replacement Reactions:
Directions: Use Table J to predict if the single replacement reaction
will occur and balance the equation if necessary.
Mg(s) Pb(NO3)2 (aq) 

32. Single Replacement Reactions
Ag(s) Pb(NO3)2 (aq) 

33. Single Replacement Reactions
Zn(s) HCl (aq) 

34. Single Replacement Reactions
F2 (g) + NaCl (aq) 

35. Single Replacement Reactions
5. Cl2 (g) NaF (aq) 

36. Applications of Single Replacement Reactions
Jewelry! Silver and Gold are prized elements for making jewelry. One reason they make good jewelry is that they are not very reactive. They are above hydrogen on Table J. That’s a good thing so when it rains your jewelry will not be ruined (oxidize)!

37. Double Replacement Reactions
Reflect:
What does the word soluble mean?
What does the word insoluble mean?

38. Double Replacement Reactions
* Ionic compounds dissolved in water switch partners
Double Replacement Reactions will occur if:
You make a gas, water or a precipitate
Using Table F to predict solubility:
Soluble Compounds: Insoluble Compounds:
Compounds that dissolve in Compounds that are solids
Water (stay aq) and DO NOT dissolve in water

39. Using Table F NaNO3: AgCl: CaSO4: MgSO4: Na2CO3: Ba(OH)2: Ca3(PO4)2:
HOH:
(NH4)OH:
PbBr2:

40. Practice
1. NaI (aq) + Pb(NO3)2 (aq)  2. K2CO3 (aq) + CaSO4 (aq)  3. BaCl2 (aq) + Na2SO4 (aq)  4. BaCl2 (aq) + NaOH (aq) 

41. Practice
5. Cu(OH)2 (aq) + H2SO4 (aq)  6. Cu(NO3)2 (aq) + NaOH (aq)  7. NiSO4 (aq) + Li3PO4 (aq)  8. MgCl2(aq) + Na2CO3 (aq) 

42. Practice
9. H2SO4 (aq) + NaOH (aq)  10. NaNO3 (aq) + NH4Cl (aq) 