Post on 31-Dec-2015
ObjectivesObjectives
1) Write and balance equations1) Write and balance equations 2) Identifying the types of reactions2) Identifying the types of reactions
Reactants and ProductsReactants and Products
Gallium + Sulfuric acid → Gallium Sulfate + Gallium + Sulfuric acid → Gallium Sulfate + HydrogenHydrogen
Reactants- left side of the arrowReactants- left side of the arrow
-starting materials-starting materials Products-right side of the arrowProducts-right side of the arrow
-the substance made, produced-the substance made, produced The number of atoms on the reactant side The number of atoms on the reactant side
must equal the number of atoms on the must equal the number of atoms on the product side.product side.
BalancingBalancing
Rules:Rules: 1) Write the correct chemical formula for the 1) Write the correct chemical formula for the
reactants and the products.reactants and the products. 2) Adjust the coefficients (the numbers that 2) Adjust the coefficients (the numbers that
appear in front of the formulas) only and evenly.appear in front of the formulas) only and evenly. 3) Never change the subscripts (the small 3) Never change the subscripts (the small
numbers in a formula)numbers in a formula) 4) When counting atoms, multiply the 4) When counting atoms, multiply the
coefficients by the subscript for each element.coefficients by the subscript for each element. 5) There are seven elements, that when left 5) There are seven elements, that when left
alone, exist as diatomic molecules. alone, exist as diatomic molecules. BrBr22 I I22 N N22 Cl Cl22 HH22 OO22 FF22
Balancing ExampleBalancing Example
Ga + HGa + H22SOSO44 → Ga → Ga22(SO(SO44))33 + H + H22
Balanced:Balanced: 2Ga + 3H2Ga + 3H22SOSO4 4 → Ga → Ga22(SO(SO44))33 + 3H + 3H22
Identifying ReactionsIdentifying Reactions
The five types of reactions:The five types of reactions:
-Synthesis or Combination-Synthesis or Combination
-Single Replacement-Single Replacement
-Double Replacement-Double Replacement
-Combustion-Combustion
-Decomposition (6 types)-Decomposition (6 types)
SynthesisSynthesis
element + element → compoundelement + element → compound Occurs when two or more elements are Occurs when two or more elements are
combined to form a new substancecombined to form a new substance Also called CombinationAlso called Combination
Synthesis or Synthesis or CombinationCombination
Example:Example:
2 Na + Cl2 Na + Cl22 → 2NaCl → 2NaCl
Jayhawk says: Here’s an example of synthesis:
+ = Rivalry
Single ReplacementSingle Replacement
Occurs when one element displaces another Occurs when one element displaces another in a compound.in a compound.
A + BC → B + ACA + BC → B + ACelement + compound → element + compoundelement + compound → element + compound
Single ReplacementSingle Replacement
Example:Example:
Na + LiCl → NaCl + LiNa + LiCl → NaCl + Li
Listen up ,class, it’s time for an example.
Double ReplacementDouble Replacement
Occurs when the positive and negative ions of the two Occurs when the positive and negative ions of the two reactants are interchangedreactants are interchanged
AB + CD → AD + CBAB + CD → AD + CB compound + compound→compound compound + compound→compound
+compound+compound Never put two metals togetherNever put two metals together
Double ReplacementDouble Replacement
Example:Example:
2NaCl + Li2NaCl + Li22O → NaO → Na22O + 2LiClO + 2LiCl
Did you know? Double replacement is also referred to as metathesis.
DecompositionDecomposition Occurs when energy in the form of heat, light, Occurs when energy in the form of heat, light,
electricity, or mechanical shock is supplied. A electricity, or mechanical shock is supplied. A compound may decompose to form simpler compound may decompose to form simpler compounds and/or elements. compounds and/or elements.
compound → 2 or more substancescompound → 2 or more substances→→
DecompositionDecomposition There are 6 different types of decompositionThere are 6 different types of decomposition
Did you know? You might also know decomposition by analysis.
Electrical DecompositionElectrical Decomposition
AB → A + BAB → A + B
2NaCl → 2Na + Cl2NaCl → 2Na + Cl22
Decomposition: Oxy-AcidDecomposition: Oxy-Acid
Oxy-Acid → Water + Nonmetal Oxy-Acid → Water + Nonmetal OxideOxide
HH22SOSO4 4 → H→ H22O + SOO + SO33
Examples:Examples: HNOHNO33
HH33POPO44
HClOHClO22
Decomposition: Metallic Decomposition: Metallic HydroxideHydroxide
Metallic Hydroxide → Metal Oxide Metallic Hydroxide → Metal Oxide + Water+ Water
2LiOH → Li2LiOH → Li22O + HO + H22OO
Fe(OH)Fe(OH)2 2 → FeO + H→ FeO + H22OO
Decomposition: Metallic Decomposition: Metallic CarbonateCarbonate
Metallic Carbonate → Metal Oxide Metallic Carbonate → Metal Oxide +Carbon Dioxide+Carbon Dioxide
MgCOMgCO33 → MgO + CO → MgO + CO22
FeFe22(CO(CO33))22 → Fe → Fe22OO33 + 3CO + 3CO22
Decomposition: Metallic Decomposition: Metallic ChlorateChlorate
Metallic Chlorate → Metal Chloride Metallic Chlorate → Metal Chloride + Oxygen+ Oxygen
2LiClO2LiClO22 → 2LiCl + 3O → 2LiCl + 3O22
Ca(ClOCa(ClO33))22 → CaCl → CaCl22 + 3O + 3O22
Decomposition: Metallic Decomposition: Metallic OxideOxide
Metallic Oxide → Metal + Metallic Oxide → Metal + OxygenOxygen
2Li2Li22O → 4Li + OO → 4Li + O22
2BaO → 2Ba + O2BaO → 2Ba + O22