equations
Synthesis/Direct Combination
 A + B  AB
 2 elements combine to form a single compound
Decomposition
 AB  A + B
 Single compound is broken down
Single Replacement
 A + BX  AX + B
 An uncombined element replaces and element that is
part of a compound
Double Replacement
 AX + BY  AY + BX
 2 atoms or ions from 2 different compounds switch
places with each other
Identify the following equations:
3Mg + N2  Mg3N2
2K + 2 H2O  2KOH + H2
NH4OH  NH3 + H2O
3KOH + FeCl3  3KCl + Fe(OH)3
Complete the following:
CuS  _____________ + _____________
Br + Ag  ____________
Na + KOH  _________ + _____________
K2(CO3) + Ca(OH)2  _________ + _________
Equations/Reaction Type lab activity
SYNTHESIS

_______________
_______________
Equations/Reaction Type lab activity
DECOMPOSITION

_______________
_______________
Equations/Reaction Type lab activity
SINGLE REPLACEMENT

_______________
_______________
Equations/Reaction Type lab activity
DOUBLE REPLACEMENT

_______________
_______________
Balancing Equations
The Law of Conservation of Matter states that “matter
cannot be created nor destroyed”.
Therefore, in a balanced chemical equation, the
number of atoms of each element in the
reactants MUST EQUAL the number of atoms
of each element in the products!
CAUTION!!!!
When balancing equations, you can only add or
change coefficients (the big number in front of a
formula)! Never change the subscripts of a
balanced formula!!!
AIM
“Atom Inventory Method”
A strategy to help you determine the coefficients
needed to balance a chemical equation.
Remember to change your inventory every time you
add a coefficient!
AIM
Metal
Nonmetal
C
H
O
N2 + H2  NH3
CH4 + O2  CO2 + H2O
HCl + Fe2O3  FeCl3 + H2O
2C8H18 + O2  CO2 + H2O
Ca(OH)2 + H3PO4  Ca3(PO4)2 + H2O
Cu + H2SO4  Cu(SO4) + H2O + SO2
SiO2 + C  SiC + CO
(NH)3(PO4) + Ba(NO3)2  Ba3(PO4)2+ (NH4)(NO3)
(IP1)
____Mg + _____O2  _____MgO
(IP2)
____H2 + _____O2  _____H2O
(IP3)
___Cl2 +____KBr ____KCl +____Br2
(IP4)
__Al2(SO4)3 + __ZnCl2  __AlCl3 +__ZnSO4
(IP5)
___C3H8 + ____O2  ___CO2 + ___H2O
Writing Balanced Equations:
1.) IDENTIFY or NAME each REACTANT &
PRODUCT
2.)write CORRECTLY BALANCED FORMULAS for
each reactant and product
3.) adjust the COEFFICIENTS in the equation, using
AIM to have the same number of atoms of each
element on each side
2. iron + chlorine  iron (III) chloride
3. magnesium + nitrogen  magnesium nitride
6. nitrogen + oxygen  nitrogen (V) oxide
8. potassium chlorate potassium chloride + oxygen
1. hydrogen chloride + calcium hydroxide calcium chloride + water
4. silver nitrate+ aluminum chloride silver chloride + aluminum nitrate
7.
Iron(III)chloride+ sodium phosphate iron(III)phosphate + sodium chloride
5.
potassium phosphate+ calcium nitrate ___________ + _____________
Key to 9-16:
9. Ba(OH)2 + 2HCl  BaCl2 + 2H(OH)
10. 2Al + 3Br2  2AlBr3
11. Zn + 2HCl  ZnCl2 + H2
12. (NH4)(OH)  NH3 + H(OH)
13. 2Al2O3  4Al + 3O2
14. 2K + 2H(OH) 2 K(OH) + H2
15. 3Ba + N2  Ba3N2
16. SnCl4 + 2(NH4)2S  SnS2 + 4(NH4)Cl
Predicting if a SR rxn will Occur:
 a single replacement rxn WILL OCCUR if the free
metal is higher on ref. table J than the
combined metal
 Which SR rxn will occur?
Ca + Zn(NO3)2  Ca(NO3)2 + Zn
Ca + KNO3  Ca(NO3)2 + 2K
Predicting if a DR rxn will Occur:
 a double replacement rxn WILL OCCUR if the rxn
1.) forms a gas
Na2S(aq) + 2HCl(aq)  H2S(g) + 2NaCl(aq)
2.) forms water (1 molecule not both ionic)
NaOH(aq) + HCl(aq)  NaCl(aq) + H2O(l)
3.) forms a precipitate (Table F): form a solid
AgNO3(aq) + NaCl(aq)  AgCl(s) + NaNO3(aq)
Which DR rxn will occur?
KCl(aq) + AgNO3(aq)  AgCl + KNO3
KCl(aq) + NaNO3(aq)  NaCl + KNO3
Use reference table F to predict of the following
double replacement rxns will produce a ppt (occur):
Use reference table F to predict of the following
double replacement rxns will produce a ppt (occur):
Rxns hmwk: RB p. 40 #45, 48, 49-52, 54-59
45.) 3F2 + 2Ar  2ArF3
48.) 2Ni + O2 2NiO
49.) 2H2O 2H2 + O2
50.) 2Al2O3  4Al + 3O2
51.) 2NaCl  2Na + Cl2
52.) 2NH3  N2 + 3H2
54.) yes
55.) no
56.) yes
57.) yes
58.) yes
59.)
a. SR
b. D
c. S
d. DR
e. S
f. SR
g. DR
h. SR
i. DR
j. DR
Writing Equations II: Determining Products
1.
Aluminum reacts with magnesium sulfate
oxidation state of Mg:_____
oxidation state of Al: _____
oxidation state of (SO4) ion:_______
Writing Equations II: Determining Products
2. Calcium chloride reacts with aluminum hydroxide
oxidation state of Ca:_____
oxidation state of Al: _____
oxidation state of (SO4) ion:_______
oxidation state of (OH) ion:_______
Writing Equations II: Determining Products
3. Potassium oxide reacts with flourine gas
oxidation state of K:_____
oxidation state of F: _____
oxidation state of O:_______
Writing Equations II: Determining Products
4. Calcium reacts with hydrogen phosphate
oxidation state of Ca:_____
oxidation state of H: _____
oxidation state of (PO4) ion:_______
Writing Equations II: Determining Products
5. copper(I) sulfate reacts with barium chloride
oxidation state of Copper (I):_____
oxidation state of Ba: _____
oxidation state of (SO4) ion:_______
oxidation state of Cl ion:_______
Writing Equations II: Determining Products
6. Potassium thiocyanate reacts with iron(III) sulfate
oxidation state of K:_____
oxidation state of iron (III): _____
oxidation state of (SO4) ion:_______
oxidation state of thiosulfate ion:_______
Writing Equations III: Identification