Warm-Up
Balance the following equations
1) When sulfur trioxide gas reacts with water, a
solution of sulfuric acid (H2SO4) is formed
2) Copper metal reacts with hot concentrated sulfuric
acid(H2SO4) solution to form aqueous copper (II)
sulfate, and sulfur dioxide gas and water
3) C6H6 + O2  CO2 + H2O
Practice
•
Boron sulfide reacts violently with water to form
dissolved boric acid (H3BO3) and hydrogen sulfide
gas.
• When liquid phosphorus trichloride is added to
water, it reacts to form aqueous phosphorous
acid (H3PO3) and aqueous hydrochloric acid (HCl).
Practice Writing Skeleton Equations
• Solid Carbon reacts with Chlorine gas to form
solid Carbon Tetrachloride
• Solid Magnesium metal reacts with solid Zinc
Carbonate to form solid Magnesium Carbonate
and solid Zinc metal
Write and balance the following
equations
•When Isopropanol Alcohol (C3H8O) is burned in
excess oxygen it produces carbon dioxide and
water.
•When aqueous sodium hydroxide reacts with
sulfuric acid (H2SO4), aqueous sodium sulfate
and water are produced.
Write out the Skeleton Equation and
balance
• Gaseous hydrogen reacts with gaseous chlorine
to form aqueous hydrogen chloride
• Carbon monoxide gas reacts with gaseous
oxygen to form solid carbon dioxide
Types of Reactions
•There are five general types of reactions:
•Synthesis
•Decomposition
•Single Displacement
•Double Displacement
•Combustion
1) Synthesis Reactions
•Synthesis reactions are also called combination
reactions
•A synthesis reaction occurs when two substances
combine to form a new compound
Synthesis Reaction Continued
•The general form of a synthesis reaction is:
• A + B  AB
•Substance “AB” is the only substance formed
Examples of Synthesis Reactions
•2 Mg (s) + O2 (g)  2 MgO (s)
•Fe (s) + Cl2 (g)  FeCl2 (s)
•U (s) + 3 F2 (g)  UF6 (g)
Practice
Write the synthesis reaction for the following
•The synthesis of KCl
•The synthesis of barium fluoride
2) Decomposition Reaction
•In decomposition reactions, one substance
breaks down (decomposes) into two or more
simpler substances
Decomposition Reactions Cont.
• General Form of Decomposition Reaction
(Binary):
•
AB  A + B
Examples of
Decomposition Reactions
•2 HgO (s)  2 Hg (l) + O2 (g)
•Ca(OH)2  CaO (s) + H2O (g)
•H2SO4 (aq)  SO3 (g) + H2O (l)
• 1.
The decomposition of ammonia (NH3)
•2. The decomposition of Aluminum Oxide
•3. The decomposition Iron (III) Chloride
Warm-Up
•Name/ Write the following compounds:
•Fe2O3
•N2O5
•Lithium Chloride
•Copper (I) Sulfate • tetrahydrate
•SF6
•Phosphorous Acid
•HF(aq)
•Dinitrogen pentafluoride
Write Correct Balance Equations
•
The decomposition of magnesium oxide
• The decomposition of hydrogen peroxide (H2O2)
into oxygen and water
• The decomposition of Mg(OH)2 into magnesium
oxide and water
• The decomposition of NaHCO3
Write Correct Balance Chemical Equations for the
following reactions
•1. The synthesis of barium fluoride
•2. The decomposition of NaOH
•3. The decomposition of CaCO3
3) Single Replacement Reaction
•In a single replacement reaction (also called a
displacement reaction), an element reacts with a
compound
•A + BC  AC + B
Examples of Single
Replacement Reactions
•Mg + Zn(NO3)2  Mg(NO3)2 + Zn
•Mg + 2 AgNO3  Mg(NO3)2 (aq) + 2 Ag
Rules for Single
Replacement Reactions
•NOT ALL single replacement reactions occur
•You can determine if a reaction will occur by
knowing the activity series of metals or the
activity series of Halogens
(See Reference Guide)
Rules for Single Replacement
•The activity series tell you if one metal can
replace another metal in a reaction
•The Activity Series is ordered
•Any metal that is above another metal in the
activity series WILL REPLACE the less reactive
metal
Activity Series
• Li
•K
• Ca
• Na
• Mg
• Al
• Zn
• Fe
• Pb
•H
• Cu
• Hg
• Ag
Predict if the following
reactions will occur
• 1. Li + PbSO4
• 2. Mg + LiNO3
• 3. Na + AgCl
•4.
•5.
•6.
•7.
Write balanced equations for
the following reactions
Li + NaCl 
Au + Fe2O3 
Fe + ZnO 
Br2 + MgI2 
•Write and Balance the following equations:
•1) The decomposition of Iron (III) Chlorate
•2) Li2CO3 
•3) Li + BaS 
•4) Ag + SrSO4 
4) Double Displacement Reactions
•In a double displacement reaction, two
compounds react
•The compounds swap elements with each
other
•The General Formula
AB + CD  AD + CB
Double Displacement Cont
•Compounds contain a positive and negative part
•In a double displacement, the positive parts
swap places with each other as do the negative
parts
Examples
•PbCl2 + Li2SO4  PbSO4 + 2 LiCl
•ZnBr2 + 2 AgNO3  Zn(NO3)2 + 2 AgBr
Predict the Products of the following
reactions and balance
•BaCl2 (aq) + KClO3 (aq) 
A B
C D
AD
CB
•HCl (aq) + NaOH (aq) 
•RbBr (aq) + AgCl (aq) 
Predict the Products of the following
reactions and balance
•AgNO3 + NaCl 
•NaCl + H2SO4 
•FeS + HCl
•KOH + H2SO4 