1. Chapter 7
CHEMICAL REACTIONS

2. Reactions happen everyday in and around us!!
Digesting food Photosynthesis Baking cookies

3. All chemical reactions involve changing substances!!
Reactants  Products
Word Equations
Describing a chemical reaction using words
water  hydrogen + oxygen

4. Practice!! Write word equations for the following:
Pure copper can be produced by heating copper (II) sulfide with oxygen. Sulfur dioxide is also produced in this reaction.
Copper (II) sulfide + Oxygen  Copper + Sulfur dioxide

5. Describing Chemical Change
Formula or Skeleton Equation
Translate the words to formulas
Skeleton equations do not indicate the relative amounts of the reactants and products
water  hydrogen + oxygen
H2O  H2 + O2

6. To write an equation, you must write the correct formula first
To write an equation, you must write the correct formula first!! Finding Formulas Review
Elements
Is it an atom or a diatomic molecule (HON FClBrI)?
Atom  single atom
Silver Ag
Diatomic  subscript 2
Chlorine
Cl2

7. Finding Formulas Review
Compounds
Is it molecular (nonmetals) or ionic (metal or ammonium)?
Molecule  Translate prefix
Carbon dioxide
CO2
Ionic  find charges, criss-cross, reduce
Barium nitrate
Ba2+ and NO3-
Ba(NO3)2

8. Finding Formulas Review
Common names
Water
H2O
Ammonia
NH3
Salt
NaCl
Sugar
C12H22O11

9. Symbols Used in Chemical Equations+
(s)
(l)
(g)
(aq)
Used to separate two reactants or two products
“Yields” separates reactants from products
reversible reaction
solid
liquid
gas
dissolved in water
heat must be added to reaction
heat
catalyst added Pt

10. Practice!! Write a skeleton equation for the following:
When calcium carbonate is heated, calcium oxide and carbon dioxide are produced.
CaCO3 (s) CaO (s) + CO2 (g)
When solid mercury (II) sulfide is heated with oxygen, liquid mercury metal and gaseous sulfur dioxide are produced
HgS (s) + O2 (g) Hg (l) + SO2 (g)

11. Balancing Equation Rules
Make sure you have the right formulas.
Balance the atoms by changing the coefficients.
Start with atoms that appear only once on each side. Usually you will do hydrogen and oxygen last.
If a polyatomic ion is on both sides of the equation, treat it as one unit and balance it as a single unit.
Balancing tricks
If you are having trouble getting it to balance, double the first compound and try again.
Double check to make sure all atoms and ions are balanced and the coefficients are in the lowest possible ration.

12. Make sure you have the right formulas.
___H2 + ___O2  ___H2O 2 1 2
___H2 + ___O  ___H2O 1 1 1

13. Balance the atoms by changing the coefficients.
___H2 + ___O2  ___H2O 2 2
Can’t erase the 2
Can’t add a 2

14. ___H2SO4 + ___NaOH  ___Na2SO4 + ___H2O 1 2 1 2
Start with atoms that appear only once on each side. Usually you will do hydrogen and oxygen last.
___H2SO4 + ___NaOH  ___Na2SO4 + ___H2O 1 2 1 2
Do Na and S first.
2. Do H next.
3. Do O last.

15. ___Mg + ___AgNO3  ___Mg(NO3)2 + ___Ag 2
If a polyatomic ion is on both sides of the equation, treat it as one unit and balance it as a single unit. 2
___Mg + ___AgNO3  ___Mg(NO3)2 + ___Ag 2
The anion, NO3 , is on both sides 2 3 3 2
___H3PO4 + ___(NH4)2CO3  ___H2CO3 + ___(NH4)3PO4
NH4 , CO3 , and PO4 appear on both sides

16. ___C2H6 + ___O2  ___CO2 + ___H2O 2 3
If you are having trouble getting it to balance, double the first compound and try again.
___C2H6 + ___O2  ___CO2 + ___H2O 2 3
How can you make this = 7 ?
4 + 3 = 7
___C2H6 + ___O2  ___CO2 + ___H2O 2 7 4 6
8 + 6 = 14

17. 6. More Practice!
___Pb(OH)4 + ___H2SO4  ___Pb(SO4)2 + ___H2O

18. ___H2 + ___O2  ___H2O ___H2 + ___O2  ___H2O 4 2 4 2 1 2
Double check to make sure all atoms and ions are balanced and the coefficients are in the lowest possible ratio.
___H2 + ___O2  ___H2O 4 2 4
___H2 + ___O2  ___H2O 2 1 2

19. There are five different types of reactions that we will study!
Five Reaction Types
There are five different types of reactions that we will study!
Synthesis
Decomposition
Combustion
Single Replacement
Double Replacement

20. Five Reaction Types Mg + O2 
Synthesis (combination) Reactions - 2 or more substances combining to make a single product.
A + B  AB
2K + Cl2  2KCl
CaO + H2O  Ca(OH)2
Mg + O2 

21. Synthesis + 

22. Five Reaction Types Ag2O 
Decomposition Reaction - single reactant breaking down into simpler substances.
AB  A + B
2H2O  2H2 + O2
CaCO3  CaO + CO2
Ag2O 

23. Decomposition

24. 2C8H18(l) + 25O2(g)  16CO2(g) + 18H2O(g)
Five Reaction Types
Combustion Reactions - an element or compound reacting with oxygen(O2), often producing heat or light.
A + O2(g)  AO or CO2 + H2O
Element Combustion - also a combination reaction.
2Mg(s) + O2(g)  2MgO(s)
Hydrocarbon Combustion - oxygen reacting with a substance containing hydrogen and carbon. In complete hydrocarbon combustion, the products will always be CO2 and H2O.
2C8H18(l) + 25O2(g)  16CO2(g) + 18H2O(g)
C3H8(g) O2(g) 

25. Combustion

26. Five Reaction Types
Single Replacement Reaction - atoms of an element replacing the atoms of a second element in a compound. Only occurs if the elemental atoms are more reactive (chemically active) than the atoms they are attempting to replace in the compound.
A + BX  B + AX
X + AY  Y + AX

27. Single Replacement
Copper is added to silver nitrate

28. Zn + AlCl3  NR (No Reaction)
Five Reaction Types
Activity Series Li K Ca Na Mg Al Zn
Single Replacement cont.
Li is higher (more reactive) than Na atoms so the following reaction would occur.
Li + NaOH  Na + LiOH
Zn is lower (less reactive) than Al and is therefore not active enough to replace the Al in the compound and a reaction would NOT occur.
Zn + AlCl3  NR (No Reaction)

29. Five Reaction Types Mg + LiNO3  Na + Zn(NO3)2  Br2 + NaI 
Activity Series Li K Ca Na Mg Al Zn
Single Replacement cont.
Mg + LiNO3 
Na + Zn(NO3)2 
Br2 + NaI 

30. Double Replacement

31. Five Reaction Types Na2S(aq) + Cd(NO3)2(aq)  CdS(s) + 2NaNO3(aq)
Double replacement - exchange of two positive ions between two compounds.
AX + BY  AY + BX
A and B are trading places
Na2S(aq) + Cd(NO3)2(aq)  CdS(s) + 2NaNO3(aq)
Ca(OH)2(aq) + HCl(aq) 

32. Practice!
Li3N + NH4NO3 
HBr + Al(OH)3 

33. Predicting Products To predict the products of a chemical reaction, you must recognize the possible type of reaction that the reactants can undergo!
Hydrocarbon Combustion - Are O2 and a hydrocarbon the reactants?
 CO2 and H2O
Decomposition - Only 1 reactant
 break apart into elements
Synthesis - Reactants are both elements?
 combine to make one product
Single replacement - Reactants an element (not O2) and a compound
 check the activity series, replace like ions or NR
Double Replacement - Reactants are both compounds?
 trade the like ions

34. Steps to finding net ionic equations
Predict Products
Balance
Find states (not soluble= (s), soluble = (aq))
Write ionic equations (separate aqueous into ions)
Write net ionic equation by canceling spectator ions (can be NR)

35. Net Ionic Equations AgNO3 (aq) + NaCl (aq)  AgCl (s) + NaNO3 (aq)
We can write this equation more realistically if we recognize that most ionic compounds dissociate or separate into cations and anions when they dissolve in water.
Complete Ionic Equation- An equation that shows dissolved ionic compounds as their free ions.
Ag+(aq) + NO3-(aq)+Na+(aq) + Cl- (aq) AgCl(s)+Na+(aq)+ NO3- (aq)
This equation can be simplified and made more useful by eliminating the ions that do not participate in the reaction. You do this by canceling the ions that appear on both sides of the equation.

36. Net Ionic Equations
Spectator Ions- Ions that are not directly involved in a reaction.
What are the spectator ions in the previous problem?
Rewrite the equation leaving out the spectator ions.
Net Ionic Equation- indicates only the particles that actually take part in the reaction.
Ag+ (aq) + Cl- (aq)  AgCl (s)

37. Net Ionic Equations
In writing balanced net ionic equations, you must also balance the electric charge.
What is the net ionic equation of the following? (First write the complete ionic equation)
Pb (s) + AgNO3 (aq)  Ag (s) + Pb(NO3)2
Pb (s) + Ag+ (aq)  Ag(s) + Pb2+ (aq)
Although this equation is balanced with respect to atoms, the electrical charges do not balance.
Pb (s) + 2Ag+ (aq)  Ag(s) + Pb2+ (aq)

38. Solubility Rules and Activity Series
SOLUBILITY RULES
 1.      Alkali metal compounds, acetates, nitrates, and ammonium compounds are all soluble. 
 2.      Hydroxides of alkali metals and NH4+1, Ca+2, Sr+2, and Ba+2 are soluble.  All others are insoluble.
 3.      All halides (chlorides etc.) are soluble except for those containing Ag+1, Pb+2, and Hg2+2.
 4.      Most sulfates are soluble, except for BaSO4, SrSO4, Ag2SO4, PbSO4, and CaSO4.
 5.      Most phosphates, carbonates, chromates and sulfides are insoluble (except those of the alkali metals and ammonium). 
 6.      In addition, all acids are soluble!