REACTION PREDICTION Pre-AP CHEMISTRY

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REACTION PREDICTIONPre-APCHEMISTRY
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Reactants ? ProductsThe arrow means
yields or produces
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(s) solid(g) gas(l) liquid(aq) aqueous
(dissolved in water)? reversible reaction
catalyst (in this case, Pt is the catalyst)
heat is added heat is added
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Practice translating a word equationSolid
zinc metal reacts with aqueous copper(II) sulfate
to produce solid copper metal and aqueous zinc
sulfate.

• Zn(s) CuSO4(aq) ? Cu(s) ZnSO4(aq)

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Balancing EquationsBalancing is a trial and
error process and is best done in pencil!!We
balance an equation so that the reactants and
products each have the same number of atoms of
each element (conservation of mass).We must
correctly write the formulas for all reactants
and products before we balance.
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Coefficients Numbers placed in front of
reactants and products 2H2 O2 ? 2H2OThis
means that 2 moles or molecules of hydrogen gas
react with 1 mole or molecule of oxygen gas to
produce 2 moles or molecules of water. The
coefficients must be in the lowest ratio.
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Hints Balance elements one at a
time.Balance polyatomic ions that appear on
both sides of the equation as single units. (Ex.
Count sulfate ions, not sulfur and oxygen
separately)Balance H and O last.
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Zn HCl ? ZnCl2 H2

• Zn 2HCl ? ZnCl2 H2

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Al2(SO4)3 Ca(OH)2 ? Al(OH)3 CaSO4

• Al2(SO4)3 3Ca(OH)2 ?
• 2Al(OH)3 3CaSO4

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K H2O ? KOH H2

• 2K 2H2O ? 2KOH H2

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CH4 O2 ? CO2 H2O

• CH4 2O2 ? CO2 2H2O

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Fe Cl2 ? FeCl3

• 2Fe 3Cl2 ? 2FeCl3

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C6H14 O2 ? CO2 H2O

• 2C6H14 19O2 ? 12CO2 14 H2O

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Al4C3 H2O ? CH4 Al(OH)3

• Al4C3 12H2O ? 3CH4 4Al(OH)3

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Balance the following chemical equations.

• ___ Ca ____ H2O ? ____Ca(OH)2____H2
• Ca 2 H2O ? Ca(OH)2 H2
• 2. ____Cu2S _____O2 ? ____Cu2O ______SO2
• 2 Cu2S 3 O2 ? 2 Cu2O 2SO2
• 3. _____MnO2 _____HCl ? ______MnCl2 ______H2O
  _____Cl2
• MnO2 4 HCl ? MnCl2 2H2O Cl2
• 4. _____NH4NO3 _____NaOH ? _____NH3 _____H2O
  _____NaNO3
• NH4NO3 NaOH ? NH3 H2O NaNO3

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• 5. ____Fe(OH)3 ? _____Fe2O3 _____H2O
• 2Fe(OH)3 ? Fe2O3 3H2O
• 6. _____C3H6 _____O2 ? _____CO2 _____H2O
• 2C3H6 9O2 ? 6CO2 6H2O
• 7. __Zn(OH)2 __H3PO4 ? __Zn3(PO4)2 ___H2O
• 3 Zn(OH)2 2 H3PO4 ? Zn3(PO4)2 6H2O
• 8. _____CO _____Fe2O3 ? _____Fe _____CO2
• 3 CO Fe2O3 ? 2 Fe 3 CO2
• _ NH4Cl __Ca(OH)2 ? ___NH3 ___H2O __CaCl2
• 2NH4Cl Ca(OH)2 ? 2 NH3 2 H2O CaCl2
• ___HC2H3O2 ___NaHCO3 ? __CO2 __NaC2H3O2
  __H2O
• HC2H3O2 NaHCO3 ? CO2 NaC2H3O2 H2O

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Write a balanced chemical equation for each of
the following reactions. Include physical state
symbols.1. Copper metal heated with oxygen
gives solid copper(II) oxide.

• 2Cu(s) O2(g) ? 2CuO(s)

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2. Mixing ammonium nitrate and sodium hydroxide
solutions gives aqueous sodium nitrate, ammonia
gas, and water.

• NH4NO3(aq) NaOH(aq) ?
• NaNO3(aq) NH3(g) H2O(l)

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3. Mercury(II) nitrate solution reacts with
potassium iodide solution to give a mercury(II)
iodide precipitate and potassium nitrate
solution.

• Hg(NO3)2(aq) 2KI(aq) ? HgI2(s) 2KNO3(aq)

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4. Solutions of acetic acid and lithium hydroxide
produce water and aqueous lithium acetate.

• HC2H3O2(aq) LiOH(aq) ? H2O(l) LiC2H3O2(aq)

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5. Heating solid potassium chlorate in the
presence of manganese dioxide catalyst produced
potassium chloride and oxygen gas.

• 2KClO3(s) MnO2 2KCl(s) 3O2(g)

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DECOMPOSITION REACTIONS-Reaction where a
compound breaks down into two or more elements or
compounds. Heat, electrolysis, or a catalyst is
usually necessary.
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A compound may break down to produce two
elements.

• Ex. Molten sodium chloride is electrolyzed.
  
• 2NaCl? 2Na Cl2

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A compound may break down to produce an element
and a compound.

• Ex. A solution of hydrogen peroxide is
  decomposed catalytically.
• 2H2O2 ? 2H2O O2

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A compound may break down to produce two
compounds.

• Ex. Solid magnesium carbonate is heated.
  
  MgCO3 ?MgO CO2

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Metallic carbonates break down to yield metallic
oxides and carbon dioxide.

• K2CO3 ? K2O CO2

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Metallic chlorates break down to yield metallic
chlorides and oxygen.

• 2RbClO3 ? 2RbCl 3O2

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Metallic sulfites break down to yield metallic
oxides and sulfur dioxide.

• BaSO3 ? BaO SO2

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Hydrogen peroxide decomposes into water and
oxygen.
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Sulfurous acid decomposes into water and sulfur
dioxide.
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Carbonic acid decomposes into water and carbon
dioxide.
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Hydrated salts decompose into the salt and water

• Sodium carbonate monohydrate is heated.
• Na2CO3.H2O ? Na2CO3 H2O

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Complete and balance the following reactions
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1. ZnCO3 ?

• ZnCO3 ? ZnO CO2

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2. KClO3 ?

• 2KClO3 ?2KCl 3O2

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3. HgO ?

• 2HgO ?2Hg O2

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4. H2CO3 ?

• H2CO3 ?H2O CO2

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5. NaCl electricity gt

• 2NaCl electricity gt 2Na Cl2

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6. H2SO3 ?

• H2SO3 ?H2O SO2

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7. CaCO3?

• CaCO3?CaO CO2

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8. H2O electricity gt

• 2H2O electricity gt 2H2 O2

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9. Na2SO4.10H2O ?

• Na2SO4.10H2O ? Na2SO4 10H2O

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10. H2O2 MnO2 gt

• 2H2O2 MnO2 gt2H2O O2

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11. CuSO4.5H2O ?

• CuSO4.5H2O ? CuSO4 5H2O

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ADDITION REACTIONS-also called synthesis,
combination or composition reactions-Two or more
elements or compounds combine to form a single
product.
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-A Group IA or IIA metal may combine with a
nonmetal to make a salt.

• Ex. A piece of lithium metal is dropped into a
  container of nitrogen gas.
• 6Li N2 ? 2Li3N

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-Two nonmetals may combine to form a molecular
compound. C O2 ? CO2
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-Two compounds combine to form a single product.

• Sulfur dioxide gas is passed over solid calcium
  oxide. SO2 CaO ? CaSO3

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-A metallic oxide plus carbon dioxide yields a
metallic carbonate. (Carbon keeps the same
oxidation state)

• Li2O CO2 ? Li2CO3

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-A metallic oxide plus sulfur dioxide yields a
metallic sulfite. (Sulfur keeps the same
oxidation state)

• K2O SO2 ? K2SO3

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-A metallic oxide plus water yields a metallic
hydroxide. CaO H2O ?Ca(OH)2
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-A nonmetallic oxide plus water yields an acid.
CO2 H2O ? H2CO3
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Complete and balance the following equations
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1. Li I2 ?

• 2Li I2 ? 2LiI

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2. Mg N2 ?

• 3Mg N2 ? Mg3N2

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3. SO3 H2O ?

• SO3 H2O ? H2SO4

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4. Sr S ?

• Sr S ? SrS

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5. Mg O2 ?

• 2Mg O2 ? 2MgO

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6. Ag O2 ?

• 4Ag O2 ? 2Ag2O

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7. Na2O H2O ?

• Na2O H2O ? 2NaOH

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8. SO2 H2O ?

• SO2 H2O ?H2SO3

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9. BaO CO2?

• BaO CO2? BaCO3

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10. CaO SO2 ?

• CaO SO2 ? CaSO3

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Double Replacement (metathesis)

• Two compounds react to form two new compounds.
• All double replacement reactions must have a
  "driving force" that removes a pair of ions from
  solution.
• Ions keep their same charges as reactants and
  products.

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Formation of a precipitate A precipitate is
an insoluble substance formed by the reaction of
two aqueous substances. Two ions bond together
so strongly that water can not pull them apart.
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SOLUBILITY SONG

• To the tune of My Favorite Things from The
  Sound of Music
• Nitrates and Group One and Ammonium,
• These are all soluble, a rule of thumb.
• Then you have chlorides, theyre soluble fun,
• All except Silver, Lead, Mercury I.
• Then you have sulfates, except for these three
• Barium, Calcium and Lead, you see.
• Worry not only few left to go still.
• We will do fine on this test. Yes, we will!
• Then you have the---
• Insolubles
• Hydroxide,
• Sulfide and Carbonate and Phosphate,
• And all of these can be dried!

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Ex. Solutions of silver nitrate and lithium
bromide are mixed.

• AgNO3(aq) LiBr(aq) ?AgBr(s) LiNO3(aq)

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Formation of a gas Gases may form directly in
a double replacement reaction or can form from
the decomposition of a product such as H2CO3 or
H2SO3. (Don't leave carbonic or sulfurous
acids, or ammonium hydroxide as products of
double replacement reactions, decompose them!)
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Ex. Excess hydrochloric acid solution is added
to a solution of potassium sulfite.

• 2HCl(aq) K2SO3(aq)?
• 2KCl(aq) H2O(l) SO2(g)

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Ex. A solution of sodium hydroxide is added to a
solution of ammonium chloride.

• NaOH(aq) NH4Cl(aq) ?
• NH3(g) H2O(l) NaCl(aq)

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Formation of a molecular substance When a
molecular substance such as water or acetic acid
is formed, ions are removed from solution and the
reaction "works".
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Ex. Dilute solutions of lithium hydroxide and
hydrobromic acid are mixed.

• LiOH(aq) HBr(aq) ?
• LiBr(aq) H2O

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Complete and balance the following equations
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1. NaOH CuSO4 ?

• 2NaOH CuSO4 ?
• Na2SO4 Cu(OH)2(s)

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2. NH4I AgNO3 ?

• NH4I AgNO3 ?
• NH4NO3 AgI(s)

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3. K2CO3 Ba(OH)2 ?

• K2CO3 Ba(OH)2 ?
• 2KOH BaCO3(s)

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4. KOH HI?

• KOH HI?KI H2O(l)

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5. K2CO3 HNO3 ?

• K2CO3 2HNO3 ?
• 2KNO3 H2O CO2

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6. (NH4)2SO4 BaCl2 ?

• (NH4)2SO4 BaCl2 ?
• 2NH4Cl BaSO4(s)

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7. Na2S NiSO4 ?

• Na2S NiSO4 ?
• NiS(s) Na2SO4

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8. Pb(NO3)2 KBr ?

• Pb(NO3)2 2KBr ?
• PbBr2(s) 2KNO3

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9. Fe2(SO4)3 Ba(OH)2 ?

• Fe2(SO4)3 3Ba(OH)2 ?
• 2Fe(OH)3(s) 3BaSO4(s)

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10. Hg2(NO3)2 KI ?

• Hg2(NO3)2 2KI ?
• 2KNO3 Hg2I2(s)

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Single ReplacementReaction where one element
displaces another in a compound.One element is
oxidized and another is reduced.
A BC ? B AC
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Active metals replace less active metals or
hydrogen from their compounds in aqueous
solution. Use an activity series to determine
the activity of metal.
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Ex. Magnesium turnings are added to a solution
of iron(III) chloride.

• 3Mg(s) 2FeCl3(aq) ? 2Fe(s) 3MgCl2(aq)

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Ex. Sodium is added to water.

• 2Na(s) 2H2O(l)?
• 2NaOH(aq) H2(g)
• Reactions of Alkali metals

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Ex. Fe H2O?

• Fe H2O? no reaction

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Active nonmetals replace less active nonmetals
from their compounds in aqueous solution. Each
halogen will displace heavier halogens from
their binary salts.
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Activity Series of NonmetalsMost Active
F2 Cl2
Br2 Least Active
I2
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Ex. Chlorine gas is bubbled into a solution of
potassium iodide.

• Cl2(g) 2KI(aq) ?
• I2(s) 2KCl(aq)

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Ex. I2 KCl ?

• I2 KCl ? no reaction

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Complete and balance the following equations
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1. Zn HCl ?

• Zn 2 HCl ?ZnCl2 H2

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2. Br2 NaCl ?

• Br2 NaCl ? No Reaction

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3. F2 NaBr ?

• F2 2NaBr ?2NaF Br2

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4. Al CuSO4 ?

• 2Al 3CuSO4 ?
• Al2(SO4)3 3Cu

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5. Cu AgNO3 ?

• Cu 2AgNO3 ?
• Cu(NO3)2 2Ag

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6. Cd CuSO4 ?

• Cd CuSO4 ?
• CdSO4 Cu

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7. K H2O ?

• 2K 2H2O ?
• 2KOH H2

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8. Mg H2SO4 ?

• Mg H2SO4 ?
• MgSO4 H2

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9. Ag HCl ?

• Ag HCl ?No Rxn

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10. I2 KCl ?

• I2 KCl ?No Rxn

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11. Ca H2O ?

• Ca 2H2O ?Ca(OH)2 H2

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12. Zn H2O ?

• Zn H2O ?No Rxn

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COMBUSTION REACTIONS
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In the presence of excess oxygen, most
hydrocarbons and alcohols can undergo complete
combustion reactions to form carbon dioxide and
water. The only tricky part is balancing the
reaction. Balance the C first, H second, and O
third.
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Ex. Ethane (C2H6) burns in air.

• 2C2H6 7O2 ? 4CO2 6H2O

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Ethanol (C2H5OH) burns

• C2H5OH 3O2 ? 2CO2 3H2O

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Complete and balance the reactions for the
combustion of the following compounds
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1. CH4

• CH4 2O2 ? CO2 2H2O

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2. C2H2

• 2C2H2 5 O2 ? 4CO2 2H2O

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3. CH3OH

• 2CH3OH 3O2 ? 2CO2 4H2O

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4. C6H12O6

• C6H12O6 6O2 ? 6CO2 6H2O

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5. C8H18

• 2C8H18 25O2 ? 16CO2 18H2O

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6. C3H8

• C3H8 5O2 ? 3CO2 4H2O

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7. C6H6

• 2C6H6 15O2 ? 12CO2 6H2O

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8. C2H4

• C2H4 3O2 ? 2CO2 2H2O

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9. C35H72

• C35H72 53O2 ? 35CO2 36 H2O

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10. C3H7OH

• 2C3H7OH 9O2 ? 6CO2 8H2O

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SYNTHESIS AND DECOMPOSITION REACTIONS
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Complete and balance the following equations
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1. Sr O2 ?

• 2Sr O2 ?2SrO

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2. Na O2 ?

• 4Na O2 ?2Na2O

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3. K Cl2 ?

• 2K Cl2 ?2KCl

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4. Ca F2 ?

• Ca F2 ?CaF2

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5. sodium iodine ?

• 2Na I2 ?2NaI

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6. magnesium oxygen ?

• 2Mg O2 ?2MgO

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7. hydrogen chlorine ?

• H2 Cl2 ? 2HCl

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8. silver sulfur ?

• 2Ag S ? Ag2S

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9. calcium oxide water ?

• CaO H2O ? Ca(OH)2

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10. sulfur trioxide water ?

• SO3 H2O ? H2SO4

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11. MgBr2?

• MgBr2? Mg Br2

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12. AlCl3 ?

• 2AlCl3 ?2Al 3Cl2

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13. H2O ?

• 2H2O ?2H2 O2

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14. KI ?

• 2KI ?2K I2

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15. NaCl ?

• 2NaCl ?2Na Cl2

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16. nickel(II) chlorate ?

• Ni(ClO3)2 ? NiCl2 3O2

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SINGLE AND DOUBLE REPLACEMENT REACTIONS
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Write and balance the following reactions
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1. Zn(s) CuSO4(aq) ?

• Zn(s) CuSO4(aq) ?ZnSO4(aq) Cu(s)

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2. Cl2(g) KI(aq) ?

• Cl2(g) 2KI(aq) ?2KCl(aq) I2(s)

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3. Ni(s) MgSO4(aq) ?

• Ni(s) MgSO4(aq) ?No Reaction

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4. Br2(l) CaCl2(aq) ?

• Br2(l) CaCl2(aq) ?No Rxn

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5. zinc copper(II) nitrate ?

• Zn(s) Cu(NO3)2(aq) ? Cu(s) Zn(NO3)2(aq)

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6. calcium hydrochloric acid ?

• Ca(s) 2HCl(aq) ? CaCl2(aq) H2(g)

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7. copper(II) nitrate silver ?

• Cu(NO3)2(aq) Ag(s) ? No Rxn

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8. sodium iodide bromine ?

• 2NaI(aq) Br2(l) ? 2NaBr(aq) I2(s)

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9. sodium water ?

• 2Na(s) 2H2O(l) ? 2NaOH(aq) H2(g)

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10. FeCl2 K2S ?

• FeCl2(aq) K2S(aq) ?
• FeS(s) 2KCl(aq)

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11. ZnCl2 Pb(NO3)2 ?

• ZnCl2(aq) Pb(NO3)2(aq)?
• Zn(NO3)2(aq) PbCl2(s)

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12. CaCl2 Na2CO3 ?

• CaCl2(aq) Na2CO3(aq) ? 2NaCl(aq) CaCO3(s)

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13. (NH4)2SO4 BaCl2 ?

• (NH4)2SO4(aq) BaCl2(aq) ? 2NH4Cl(aq) BaSO4(s)

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14. sodium hydroxide acetic acid ?

• NaOH(aq) HC2H3O2(aq) ? NaC2H3O2(aq) H2O(l)

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15. copper(II) sulfate ammonium sulfide ?

• CuSO4(aq) (NH4)2S(aq) ? CuS(s) (NH4)2SO4(aq)

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MIXED EQUATION WORKSHEET 1Complete the word
equation, write the formula equation, balance it
and identify the type of reaction. You many
abbreviate as S, D, SR, DR, and C.
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1. Magnesium hydroxide nitric acid ?

• magnesium hydroxide nitric acid ?
• magnesium nitrate water
• Mg(OH)2 2HNO3 ? Mg(NO3)2 2H2O
• DR

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2. Complete combustion of methane (CH4)

• methane oxygen ?
• carbon dioxide water
• CH4 2O2 ? CO2 2H2O
• Combustion

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3. Chlorine sodium bromide ?

• chlorine sodium bromide ?
• bromine sodium chloride
• Cl2 2NaBr ? Br2 2NaCl
• Single Replacement

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4. Aluminum sulfuric acid ?

• aluminum sulfuric acid ?
• aluminum sulfate hydrogen
• 2Al 3H2SO4 ?Al2(SO4)3 3H2
• Single replacement

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5. Sulfuric acid sodium acetate ?

• Sulfuric acid sodium acetate ?
• sodium sulfate acetic acid
• H2SO4 2NaC2H3O2 ?
• Na2SO4 2HC2H3O2
• Double replacement

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6. Heating calcium carbonate ?

• calcium carbonate ?
• calcium oxide carbon dioxide
• CaCO3 ? CaO CO2
• Decomposition

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7. Heating mercuric oxide ?

• mercuric oxide ?
• mercury oxygen
• 2HgO ? 2Hg O2
• Decomposition

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8. Zinc silver nitrate ?

• Zinc silver nitrate ?
• zinc nitrate silver
• Zn 2AgNO3 ? Zn(NO3)2 2Ag
• Single Replacement

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9. Burning sulfur

• Sulfur oxygen ?
• sulfur dioxide
• S O2 ? SO2
• synthesis

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10. Heating sodium chlorate

• sodium chlorate ?
• sodium chloride oxygen
• 2NaClO3 ? 2NaCl 3O2
• Decomposition

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11. Zinc chloride ammonium sulfide ?

• Zinc chloride ammonium sulfide ?
• zinc sulfide ammonium chloride
• ZnCl2 (NH4)2S ? ZnS 2NH4Cl
• double replacement

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12. Aluminum hydroxide hydrochloric acid ?

• Aluminum hydroxide hydrochloric acid ? aluminum
  chloride water
• Al(OH)3 3HCl ? AlCl3 3H2O
• Double replacement

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13. Calcium steam ?

• Calcium steam ?
• calcium hydroxide hydrogen
• Ca 2H2O ? Ca(OH)2 H2
• Single replacement

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14. Heating carbonic acid

• carbonic acid ?
• water carbon dioxide
• H2CO3 ? H2O CO2
• Decomposition

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15. Electrolysis of sodium chloride ?

• Sodium chloride ?
• sodium chlorine
• 2NaCl ? 2Na Cl2
• Decomposition

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16. Combustion of propane (C3H8)

• Propane oxygen ?
• Carbon dioxide water
• C3H8 5O2 ? 3CO2 4 H2O
• Combustion

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17. Bromine potassium iodide ?

• Bromine potassium iodide ?
• Iodine potassium bromide
• Br2 2KI ? I2 2KBr
• Single Replacement

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18. Magnesium hydrochloric acid ?

• Magnesium hydrochloric acid ?
• magnesium chloride hydrogen
• Mg 2HCl ? MgCl2 H2
• Single replacement

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19. Sodium hydroxide acetic acid ?

• Sodium hydroxide acetic acid ?
• sodium acetate water
• NaOH HC2H3O2 ? NaC2H3O2 H2O
• Double replacement

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20. Burning hydrogen ?

• hydrogen oxygen ? water
• 2H2 O2 ? 2H2O
• Synthesis or combustion

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21. Zinc sulfuric acid ?

• Zinc sulfuric acid ?
• zinc sulfate hydrogen
• Zn H2SO4 ? ZnSO4 H2
• single replacement

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22. Heating magnesium carbonate

• magnesium carbonate ?
• magnesium oxide carbon dioxide
• MgCO3 ? MgO CO2
• Decomposition

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23. Sodium chlorine ?

• Sodium chlorine ?
• sodium chloride
• 2Na Cl2 ? 2NaCl
• Synthesis

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24. Lead(II) nitrate sodium iodide ?

• Lead(II) nitrate sodium iodide ?
• lead (II) iodide sodium nitrate
• Pb(NO3)2 2NaI ? PbI2 2NaNO3
• Double replacement

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25. Silver nitrate sodium sulfide ?

• Silver nitrate sodium sulfide ?
• silver sulfide sodium nitrate
• 2AgNO3 Na2S ? Ag2S 2NaNO3
• Double replacement

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26. Iodine potassium chloride ?

• Iodine potassium chloride ?
• No Reaction

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27. Magnesium oxide water ?

• Magnesium oxide water ?
• magnesium hydroxide
• MgO H2O ? Mg(OH)2
• synthesis

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MIXED EQUATION WORKSHEET 2
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Complete the word equation, write the formula
equation, balance it and identify the type of
reaction. You many abbreviate as S, D, SR, DR,
and C.
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1. sodium hydrogen carbonate hydrochloric
acid ?

• sodium hydrogen carbonate hydrochloric acid ?
  sodium chloride water carbon dioxide
• NaHCO3 HCl ? NaCl H2O CO2
• double replacement

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2. Complete combustion of ethanol (C2H5OH)

• Ethanol oxygen ?
• carbon dioxide water
• C2H5OH 3O2 ? 2CO2 3H2O
• Combustion

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3. sulfurous acid magnesium hydroxide ?

• sulfurous acid magnesium hydroxide ?
• water magnesium sulfite
• H2SO3 Mg(OH)2 ? 2H2O MgSO3
• double replacement

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4. carbonic acid lithium hydroxide ?

• carbonic acid lithium hydroxide ?
• water lithium carbonate
• H2CO3 2LiOH ? 2H2O Li2CO3
• Double replacement

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5. gold sulfuric acid ?

• gold sulfuric acid ?
• No Reaction

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6. aluminum fluorine ?

• aluminum fluorine ? aluminum fluoride
• 2Al 3F2 ? 2AlF3
• Synthesis

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7. calcium oxide water ?

• calcium oxide water ?
• calcium hydroxide
• CaO H2O ? Ca(OH)2
• Synthesis

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8. acetic acid sodium hydroxide ?

• acetic acid sodium hydroxide ?
• water sodium acetate
• HC2H3O2 NaOH ? H2O NaC2H3O2
• Double replacement

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9. potassium chloride lead(II) nitrate ?

• potassium chloride lead(II) nitrate ?
• potassium nitrate lead(II) chloride
• 2KCl Pb(NO3)2 ? 2KNO3 PbCl2
• Double replacement

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10. carbon monoxide oxygen ?

• carbon monoxide oxygen ?
• carbon dioxide
• 2CO O2 ? 2CO2
• Synthesis

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11. sodium chlorine ?

• sodium chlorine ?
• sodium chloride
• 2Na Cl2 ? 2NaCl
• Synthesis

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12. dinitrogen pentoxide water ?

• dinitrogen pentoxide water ?
• nitric acid
• N2O5 H2O ? H2N2O6 2HNO3
• Synthesis

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13. bromine sodium chloride ?

• bromine sodium chloride ?
• No rxn

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14. potassium chloride mercury(I) nitrate?

• potassium chloride mercury(I) nitrate?
• potassium nitrate mercury(I) chloride
• 2KCl Hg2(NO3)2 ? 2KNO3 Hg2Cl2
• Double replacement

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15. sulfur dioxide water ?

• sulfur dioxide water ?
• sulfurous acid
• SO2 H2O ? H2SO3
• Synthesis

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16. lithium oxide water ?

• lithium oxide water ?
• lithium hydroxide
• Li2O H2O ? 2LiOH
• Synthesis

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17. heating zinc carbonate

• zinc carbonate ?
• zinc oxide carbon dioxide
• ZnCO3 ? ZnO CO2
• Decomposition

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18. silver nitrate sodium chloride ?

• silver nitrate sodium chloride ?
• silver chloride sodium nitrate
• AgNO3 NaCl ? AgCl NaNO3
• Double replacement

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19. heating beryllium chlorate

• beryllium chlorate ?
• beryllium chloride oxygen
• Be(ClO3)2 ? BeCl2 3O2
• Decomposition

209
20. electrolysis of water?

• water? hydrogen oxygen
• 2H2O ? 2H2 O2
• Decomposition

210
21. complete combustion of butane (C4H10)

• Butane oxygen ?
• carbon dioxide water
• 2C4H10 13O2 ? 8CO2 10H2O
• Combustion

211
22. iron(II) sulfate ammonium sulfide ?

• iron(II) sulfate ammonium sulfide ?
• iron(II) sulfide ammonium sulfate
• FeSO4 (NH4)2S ? FeS (NH4)2SO4
• Double replacement

212
23. lithium water?

• lithium water?
• lithium hydroxide hydrogen
• 2Li 2H2O ? 2LiOH H2
• Single replacement

213
24. potassium oxide water?

• potassium oxide water?
• potassium hydroxide
• K2O H2O ? 2KOH
• Synthesis

214
25. silver sulfur?

• silver sulfur? silver sulfide
• 2Ag S ? Ag2S
• Synthesis

215
26. sodium water?

• sodium water?
• sodium hydroxide hydrogen
• 2Na 2H2O ? 2NaOH H2
• Single replacement

216
27. calcium hydroxide ammonium sulfate?

• calcium hydroxide ammonium sulfate?
• calcium sulfate ammonia water
• Ca(OH)2 (NH4)2SO4 ?
• CaSO4 2NH3 2H2O
• Double replacement

217
NET IONIC EQUATIONS
218
Net ionic equations show only the species
actually involved in the reaction. As you first
learn to write net ionic equations, you will
write three different equations for each
reaction.
219
Steps in writing net ionic equations
220
1. Write the complete molecular equation. (This
is the type of equation that you are accustomed
to writing.)
221
2. Write the complete ionic equation. To do
this, you must ionize everything that is soluble
and ionized in solution. Everything else is left
together. Do not ionize solids, gases or weak
electrolytes.
222
3. Write the net ionic equation. To do this,
cancel out all ions that are not participating in
the reaction (spectator ions) and rewrite the
equation.
223
Sodium chloride silver nitrate

• 1. NaCl(aq) AgNO3(aq) ?
• NaNO3(aq) AgCl(s)
• 2. Na Cl- Ag NO3- ?
• Na NO3- AgCl(s)
• 2. Na Cl- Ag NO3- ?
• Na NO3- AgCl(s)
• 3. Cl- Ag? AgCl

224
Ex. HCl Ba(OH)2 ?
1. 2HCl Ba(OH)2 ? 2H2O BaCl2 2. 2H 2Cl-
Ba2 2OH- ? 2H2O Ba2 2Cl- 2. 2H
2Cl- Ba2 2OH- ? 2H2O Ba2
2Cl- 3. 2H 2OH- ? 2H2O H OH-
? H2O
225
Write net ionic equations for the following
reactions
226
1. KCl(aq) Pb(NO3)2(aq)?

• 2KCl(aq) Pb(NO3)2(aq)?
• 2KNO3(aq) PbCl2(s)
• 2K 2Cl- Pb2 2NO3- ?
• 2K 2NO3- PbCl2
• Pb2 2Cl- ? PbCl2

227
2. HCl(aq) CaSO3(s)?

• 2HCl(aq) CaSO3(s)?
• H2O(l) SO2(g) CaCl2(aq)
• 2H 2Cl- CaSO3 ?
• H2O SO2 Ca2 2Cl-
• 2H CaSO3 ?
• H2O SO2 Ca2

228
3. Zn(s) O2(g) ?

• 2Zn(s) O2(g) ?2ZnO(s)

229
4. Li(s) H2O(l) ?

• 2Li(s) 2H2O(l) ?
• 2LiOH(aq) H2(g)
• 2Li(s) 2H2O(l) ?
• 2Li 2OH-(aq) H2(g)

230
5. Na2SO4(aq) BaBr2(aq)?

• Na2SO4(aq) BaBr2(aq)?
• 2NaBr(aq) BaSO4(s)
• 2Na SO42- Ba2 2Br- ?
• 2Na 2Br- BaSO4
• SO42- Ba2 ? BaSO4

231
6. MgCO3(s)?

• MgCO3(s)? MgO(s) CO2(g)

232
7. AgNO3(aq) Na2CO3(aq) ?

• 2AgNO3(aq) Na2CO3(aq) ?
• Ag2CO3(s) 2NaNO3(aq)
• 2Ag 2NO3- 2Na CO32- ?
• Ag2CO3 2Na 2NO3-
• 2Ag CO32- ? Ag2CO3

233
8. Na2S(aq) HCl(aq) ?

• Na2S(aq) 2HCl(aq) ?
• 2NaCl(aq) H2S(g)
• 2Na S2- 2H 2Cl- ?
• 2Na 2Cl- H2S
• S2- 2H ? H2S

234
9. H2SO3(aq) ?

• H2SO3(aq) ?H2O(l) SO2(g)

235
10. Cl2(g) NaI(aq) ?

• Cl2(g) 2NaI(aq) ?I2(s) 2NaCl(aq)
• Cl2 2Na 2I- ?I2 2Na 2Cl-
• Cl2 2I- ?I2 2Cl-

236
EXTRA EQUATION WORKSHEETPRE-AP CHEMISTRY
237
Complete the word equation, write the formula
equation, balance it and identify the type of
reaction. You many abbreviate as S, D, SR, DR,
and C.
238
1. heating magnesium carbonate

• magnesium carbonate ?
• magnesium oxide carbon dioxide
• MgCO3 ? MgO CO2
• Decomposition

239
2. complete combustion of propanol (C3H7OH)

• propanol oxygen ?
• carbon dioxide water
• 2C3H7OH 9O2 ? 6CO2 8H2O
• Combustion

240
3. sulfur oxygen ?

• sulfur oxygen ?sulfur dioxide
• S O2 ? SO2
• Synthesis

241
4. sulfuric acid cadmium ?

• sulfuric acid cadmium ?
• cadmium sulfate hydrogen
• H2SO4 Cd ? CdSO4 H2
• Single Replacement

242
5. sulfur dioxide water ?

• sulfur dioxide water ?
• sulfurous acid
• SO2 H2O ? H2SO3
• Synthesis

243
6. hydrochloric acid(aq) calcium carbonate(s) ?

• hydrochloric acid(aq) calcium carbonate(s) ?
• carbon dioxide(g) water(l) calcium
  chloride(aq)
• 2HCl CaCO3 ? CO2 H2O CaCl2
• Double replacement

244
7. net ionic equation for 6

• 1. 2HCl(aq) CaCO3(s) ?
• CO2(g) H2O(l) CaCl2(aq)
• 2. 2H 2Cl- CaCO3 ?
• CO2 H2O Ca2 2Cl-
• 3. 2H CaCO3 ?
• CO2 H2O Ca2

245
8. silver nitrate (aq) hydrochloric acid (aq)?

• silver nitrate (aq) hydrochloric acid (aq)?
• silver chloride(s) nitric acid(aq)
• AgNO3 HCl ? AgCl HNO3
• Double replacement

246
9. net ionic equation for 8

• 1. AgNO3(aq) HCl(aq) ?
• AgCl(s) HNO3(aq)
• 2. Ag NO3- H Cl- ?
• AgCl(s) H NO3-
• 3. Ag Cl- ? AgCl(s)

247
10. barium nitrate(aq) potassium sulfate (aq)?

• barium nitrate(aq) potassium sulfate (aq)?
• barium sulfate(s) potassium nitrate(aq)
• Ba(NO3)2 K2SO4 ? BaSO4 2KNO3
• Double Replacement

248
11. net ionic equation for 10

• 1. Ba(NO3)2 (aq) K2SO4(aq) ? BaSO4(s)
  2KNO3(aq)
• 2. Ba2 2NO3- 2K SO42- ?
• BaSO4 2K 2NO3-
• 3. Ba2 SO42- ? BaSO4

249
12. sodium hydroxide phosphoric acid ?

• sodium hydroxide phosphoric acid ?
• sodium phosphate water
• 3NaOH H3PO4 ? Na3PO4 3H2O
• Double replacement

250
13. iodine rubidium chloride ?

• iodine rubidium chloride ? No Rxn

251
14. magnesium(s) copper(II) sulfate(aq)?

• magnesium(s) copper(II) sulfate(aq)?
• magnesium sulfate(aq) copper(s)
• Mg CuSO4 ? MgSO4 Cu
• Single replacement

252
15. net ionic equation for 14

• 1. Mg(s) CuSO4(aq) ? MgSO4(aq) Cu(s)
• 2. Mg Cu2 SO42- ?
• Mg2 SO42- Cu
• 3. Mg Cu2 ? Mg2 Cu

253
16. ammonium nitrate(aq) sodium hydroxide(aq) ?

• ammonium nitrate(aq) sodium hydroxide(aq) ?
  ammonia (g) water (l) sodium nitrate (aq)
• NH4NO3 NaOH ?
• NH3 H2O NaNO3
• Double replacement

254
17. net ionic equation for 16

• 1. NH4NO3(aq) NaOH(aq) ?
• NH3(g) H2O(l) NaNO3(aq)
• 2. NH4 NO3- Na OH- ?
• NH3 H2O Na NO3-
• 3. NH4 OH- ? NH3 H2O

255
18. potassium(s) water(l) ?

• potassium(s) water(l) ?
• potassium hydroxide(aq) hydrogen(g)
• 2K 2H2O ? 2KOH H2
• Single Replacement

256
19. net ionic equation for 18

• 1. 2K(s) 2H2O(l) ?
• 2KOH(aq) H2(g)
• 2. 2K 2H2O ? 2K 2OH- H2

257
20. sodium bromide(aq) chlorine(g)?

• sodium bromide(aq) chlorine(g)?
• sodium chloride bromine
• 2NaBr Cl2 ? 2NaCl Br2
• Single replacement

258
21. net ionic equation for 20

• 1. 2NaBr(aq) Cl2(g) ? 2NaCl(aq) Br2(l)
• 2. 2Na 2Br- Cl2 ?
• 2Na 2Cl- Br2
• 3. 2Br- Cl2 ? 2Cl- Br2

259
22. aluminum nitrogen?

• aluminum nitrogen?
• aluminum nitride
• 2Al N2 ? 2AlN
• Synthesis

260
23. sodium sulfide(aq) hydrochloric acid(aq)?

• sodium sulfide(aq) hydrochloric acid(aq)?
  sodium chloride (aq) hydrogen sulfide (g)
• Na2S 2HCl ? 2NaCl H2S
• Double replacement

261
24. net ionic equation for 23

• 1. Na2S(aq) 2HCl(aq) ? 2NaCl(aq) H2S(g)
• 2. 2Na S2- 2H 2Cl- ?
• 2Na 2Cl- H2S
• 3. S2- 2H ? H2S

262
25. heating magnesium sulfate heptahydrate

• magnesium sulfate heptahydrate ?
• magnesium sulfate water
• MgSO4.7H2O ? MgSO4 7H2O
• Decomposition

263
26. heating mercury(II) oxide?

• mercury(II) oxide ?
• mercury oxygen
• 2HgO ? 2Hg O2
• Decomposition

264
27. bromine strontium chloride?

• bromine strontium chloride? No Rxn

265
1. Dilute hydrochloric acid is added to a
solution of potassium sulfite.

• 2HCl(aq) K2SO3(aq) ?H2O(l) SO2(g) 2KCl(aq)
• 2H 2Cl- 2K SO32-?
• H2O(l) SO2(g) 2K 2Cl-
• 2H SO32-? H2O(l) SO2(g)

266
2. A solution of sodium sulfide is added to a
solution of zinc nitrate.

• Na2S(aq) Zn(NO3)2(aq) ? 2NaNO3(aq) ZnS(s)
• 2Na S2- Zn2 2NO3- ? 2Na 2NO3- ZnS
• S2- Zn2 ? ZnS

267
3. Chlorine gas is bubbled into a solution of
potassium iodide.

• Cl2(g) 2KI(aq) ? 2KCl(aq) I2(s)
• Cl2 2K 2I- ? 2K 2Cl- I2
• Cl2 2I- -gt 2Cl- I2

268
4. Magnesium metal is burned in nitrogen gas.

• 3Mg(s) N2(g) ? Mg3N2(s)

269
5. Solid sodium oxide is added to water.

• Na2O(s) H2O(l) ? 2NaOH(aq)
• Na2O(s) H2O(l) ?2Na(aq) 2OH-(aq)