chapters 6 and 7 chemical reactions are solid!!faculty.orangecoastcollege.edu/mappel/chem 130/fall...
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1
Chapters 6 and 7
Chemical Reactions Are SOLID!!
Chapter 6
I. Chemical Reactions and Equations
A. When has a Reaction Occurred?
B. Representing Reactions with
Chemical Equations
C. Balancing Chemical Equations
Chapter 7
I. Precipitation Reactions
A. Ionic Compounds in
Solutions
B. Double Displacement Reactions
II. Acid Base Reactions
III. Oxidation Reduction Reactions
IV. Combustion Reactions
2
I. Chemical Reactions and
Equations
A) When has a Reaction Occurred?
B) Representing Reactions with Chemical
Equations
What is a Chemical Equation?
1. 2. 3. 4.
3
Information Provided by Recipes and
Chemical Equations
- Ratios of ingredients to each other
and to product(s) provide conversion
factors
Difference Between Recipes and Chemical Equations Chemistry - forward and reverse directions of equation
are possible
- for a specific set of conditions one
direction is favored
www.smallstepsproject.org
4
How do we treat chemical reactions?
Law of Conservation of Mass
- total mass of all substances after a
chemical rxn is the same as the total mass
before the rxn
http://www3.delta.edu/bernadetteharkness/Ch4AtomicTheoryPart1/Ch4AtomicTheoryPart1_print.html
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Method For Balancing Chemical Equations
1. Convert statement into chemical
equation and balance the atoms Sulfuryl chloride(SO2Cl2) reacts with hydroiodic acid to form
hydrosulfuric acid, dihydrogen monoxide, hydrochloric acid, and
iodine.
i. Start with elements in only one compound
on either side of the equation
ii. Finish with elements that exist as
monoatomic atoms, diatomic molecules,
triatomic molecules, etc.
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2. Adjust the coefficients to smallest
whole number coefficients
3. Check Answer
4. Specify the states of Matter
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Example (balance)
1. Solid aluminum reacts with aqueous
hydrochloric acid to form aqueous
aluminum chloride and hydrogen gas.
10
2. Aqueous calcium phosphate reacts
with solid silicon dioxide and solid carbon
(C(s)) to form solid phosphorus, solid
calcium silicate (SiO32-
), and gaseous carbon
monoxide.
3. Fe(OH)3(s) + H2SO4(aq) Fe2(SO4)3(aq) + H2O(l)
12
Chapter 7 Reactions in Aqueous Solution
WHICH IONIC COMPOUNDS WILL DISSOLVE?
Ionic (in water)
Soluble Insoluble
Dissociates into cations and anions
Stays intact
Molecular (in water)
Acids
(soluble)
Bases (N)
(soluble)
Neither Acid or Base
(soluble or insoluble)
Strong Acid Weak Base Weak Acid
Stays Intact H3O
+ + anion Stays Intact
Stays Intact
Solubility Rules for Common Ionic Compounds
SOLUBLE COMPOUNDS
group 1 cations + any anion soluble
ammonium ion + any anion soluble
Any cation + nitrate, perchlorate, soluble
or acetate ions
MOSTLY SOLUBLE COMPOUNDS
Any cation + chloride, bromide, soluble
or iodide ions (except lead(II), silver, mercury(I) insoluble)
Any cation + sulfate ions soluble (except strontium, calcium, barium, lead(II), mercury(I) insoluble)
INSOLUBLE COMPOUNDS
Any cation + hydroxide ions insoluble (except group I, ammonium, calcium*, barium*, strontium* soluble)
Any cation + sulfide ions Insoluble (except group I, ammonium, group II* soluble)
Any cation + carbonate or Insoluble
phosphate ions (except group I, ammonium soluble)
* - slightly soluble (for chem 130 = soluble)
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