review of ionic and molecular formula writing:. chapter 8 outline 8.1 – chemical equations the...
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Review of Ionic and Review of Ionic and Molecular Formula Molecular Formula Writing:Writing:
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Chapter 8 Outline
8.1 – Chemical Equations
The symbols and formulas used to represent reactants
and products
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Reading and Writing Chemical Equations:
1. Represent the Facts
2. Use correct formulas for compounds
-Ionic – SWAPPING
-Molecular – PREFIXES
-Diatomics – AUTOMATICALLY get a subscript “2”
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Diatomics:
Silly Phrase:HairyNinjasOftenFightCleanBrightItalians
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Reading and Writing Chemical Equations:
Metals are the symbol only:
Magnesium metal = Mg
Copper metal = Cu
**No numbers or charges!!*
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Reading and Writing Chemical Equations:
3. Law of Conservation of Mass:
Nature balances the reactions, so we must too! We will use COEFFICIENTS which match what nature does.
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Types of Equations
Word Equation
-Shows reactants and products in WORDS
-For now these will be given to you
Example:
Methane Gas + Oxygen Gas -> Carbon dioxide + Water
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Types of Equations
Formula Equation
-Uses Formulas
Example:
CH4 + O2 -> CO2 + H2O
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Types of Equations
Balanced Equation
-Number of each atom on the left matches the number on the right
-THIS IS WHAT NATURE DOES!
Example:
CH4 + 2O2 -> CO2 + 2H2O
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Other Symbols
s=solid
l=liquid
g=gas
aq=aqueous=dissolved in water
Reversible Reaction
Add Heat
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Significance of an Equation
-Will give us information about the amounts of reactants and products
-That’s Chapter 9!
Reversible Reactions – Can proceed in either direction.
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Balancing Reactions
• Most can be done by inspection
• STEPS1. Write the WORD EQUATION (for now given)
Ex. Water -> Hydrogen Gas + Oxygen Gas(this is called the Electrolysis of Water)
2. Replace words with formulas
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Water -> Hydrogen Gas + Oxygen Gas
H2O -> H2+
O2
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3. Balancing
-Balance one atom at a time
-Start with elements that are on each side one time only
-Balance polyatomics (like NO3) as an entire group when possible
-Balance O and H last
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Water -> Hydrogen Gas + Oxygen Gas
H2O O2-> +H2
H
O
Count atoms to check!
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Electrolysis of Water
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Practice Problems
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More Practice Problems
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More Practice Problems
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8.2 – Types of Reactions
1. Synthesis
-Combining 2 or more reactants to form one product
A + X -> AX
Example:Magnesium + Oxygen Gas -> Magnesium oxide
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8.2 – Types of Reactions2. Decomposition
-Breaking down 1 reactant into 2 or more products
AX -> A + X
Example:
Hydrogen peroxide -> Water + Oxygen gas
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8.2 – Types of Reactions
3. Single Displacement
-One element replacing another in a compound
A + BX -> B + AX
-A replaces the one it is most similar to!
Example:aluminum + iron (III) oxide -> iron + aluminum oxide
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Single Displacement
Honors must be able to predict products.
Examples:
1.copper (II) nitrate + zinc ->
2.Sodium chloride + fluorine gas ->
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8.2 – Types of Reactions
4. Double Displacement
-Two elements switch places in compounds
AX + BY -> AY + BX
Example:Sodium chloride+Silver(I) nitrate->Sodium nitrate+Silver(I) chloride
4 Types of Reactions Review:
(Stop after Dbl Disp)
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8.2 – Types of Reactions
4. Double Displacement
-You must be able to predict products for this type of reaction!
Example:
Iron (II) sulfide + Hydrogen chloride ->
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Activity Series
• Activity = Ability to react
• Activity Series = List of elements by activity
• High on the list means the element can replace those below it
• Helps us determine whether a reaction will or will not happen
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Activity SeriesLiKCaNaMgAlZnFeCoNiSnPbCuHgAg
Most active on this list
Least active on this list
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Activity SeriesLiKCaNaMgAlZnCrFeCoNiSnPbCuHgAg
For a single displacement reaction to occur, the SINGLE REACTANT must be HIGHER than the one in the compound
Example: 2Al + 3ZnCl2 -> 3Zn + 2AlCl3
Example: Co + 2NaCl -> CoCl2 + 2Na
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Solubility
• Solubility = Ability to dissolve
• Soluble = DissolvesIn Water = Aqueous – aq
• Insoluble = Does NOT DissolveSolid = s = precipitate
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SolubilitySolubility Rules (these will be given to you on test):– Group 1 and Ammonium compounds ARE soluble– Acetate, Nitrate, and chlorate compounds ARE
soluble– Group 17 (other than F) ARE soluble EXCEPT
when with Ag, Hg2+2, and Pb– Sulfates ARE soluble EXCEPT when with Ba, Sr,
Pb, Ca, Ag, Hg2+2– Carbonates, Hydroxides, Oxides, Sulfides,
Phosphates, Oxalates are INSOLUBLE**Start at the top and work down. STOP when you hit
the first rule that applies to ANY PART of you compound**
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Solubility
Examples:
Cu(NO3)2 =
Silver nitrate + sodium chloride ->