CHEMICAL REACTIONS:

1
CHAPTER 6 CHEMICAL REACTIONS CLASSIFICATION AND
MASS RELATIONSHIPS
2
(No Transcript)
3
DEFINITIONS REACTANT PRODUCT BALANCED
EQUATION
4
(No Transcript)
5
BALANCED EQUATIONS
6
(No Transcript)
7
(No Transcript)
8
HINTS FOR BALANCINGCHEMICAL EQUATIONS
9
PRACTICE EQUATIONS Al(s) O2(g) ?
Al2O3(s) C3H8 O2 ? CO2 H2O Pb(NO3)2
NaCl ? PbCl2 NaNO3
10
In the lab, we usually weigh our reagents. But it
is individual atoms or molecules that react, not
grams of atoms or molecules.
11
MOLECULAR WEIGHT
12
MOLE CONCEPT AND ELEMENTS
13
One mole of compound
14
(No Transcript)
15
In the lab, we usually weigh our reagents. But it
is individual atoms or molecules that react, not
grams of atoms or molecules.
16
(No Transcript)
17
(No Transcript)
18
(No Transcript)
19
WHEN INDOUBT, CONVERT TO MOLES!!!
20
(No Transcript)
21
(No Transcript)
22
(No Transcript)
23

• REACTION CALCULATIONS
• Now we have everything we need to be able
• to calculate the moles and mass involved
• in chemical reactions.
• EXAMPLE
• Acetylene burns in oxygen
• 2 C2H2 5 O2 ? 4 CO2 2 H2O
• How many grams of carbon dioxide are
• produced when 22.0 g of C2H2 are burned?

24

• REACTION YIELDS

25
PERCENT YIELD We burn 22.0 g of acetylene and 65
g of CO2 are produced. What is the yield?
26
CLASSES OF CHEMICAL REACTIONS 1) 2) 3)
27

Group 1A

Halides
28
OXIDATION-REDUCTION (redox) REACTIONS
29
REDOX REACTIONS
30
(No Transcript)
31
(No Transcript)
32
REDOX REACTIONS
33
REDOX REACTIONS
34
REDOX REACTIONS
Zn(s) CuSO4(aq) ? Cu(s) ZnSO4(aq)
35
(No Transcript)
36
REDOX REACTIONS In photographic film 2 AgBr
light ? 2 Ag Br2
37

• REDOX REACTIONS
• EXAMPLES
• 4 Fe 3 O2 ? 2 Fe2O3
• 4 Al 3 O2 ? 2 Al2O3
• S O2 ? SO2
• CH3OH ? H2CO H2
• 2 H2CO O2 ? 2 H2CO2
• 2 H2CO2 O2 ? 2 CO2 2 H2O

38
(No Transcript)
39
OXIDATION NUMBERS Rule 1 Rule 2 Rule 3 Rule
4 Rule 5
40
Rule 6 Rule 7
41
RULE 1
42
RULES 2 and 3
43
RULES 4-7
44
RULES 5-7
45
RULE 6
46
USING OXIDATION NUMBERS TO DETERMINE WHAT IS
OXIDIZED OR REDUCED
47

• IONIC EQUATIONS

48

• MOLECULAR EQUATIONS
• TOTAL IONIC EQUATIONS
• NET IONIC EQUATIONS

49

• EXAMPLE
• Write the following molecular equation in total
  ionic and net ionic forms. Soluble substances
  are indicated by (aq) after their formulas and
  non soluble solids are indicated by (s) after
  their formulas.
• BaCl2 (aq) Na2S(aq) BaS(s) 2NaCl(aq)