Download Synthesis Reactions occur when two of more reactants combine to

NAME________________________________________Per______
Chemical Reactions
Balancing Equations, Reaction Types, Predicting Products, Solubility Rules, Activity Series
Vocabulary: reactant, product, balanced chemical reaction, state signifiers, aqueous, combustion,
decomposition, red flag, solubility, soluble, insoluble, dissociation, precipitate, single
replacement/displacement, reactivity, activity series, spectator ion, double replacement/displacement,
synthesis/combination, solute, solvent, oxidation number
In Class
Homework
Empirical/Molecular Practice:
1. Zinc form an ionic compound with an oxyanion. The formula is 44.97% Zn and 22.02% S. What
is the formula and the name of the compound?
2. Naphthalenedisulfonic acid is found to be 41.7% C, 2.8% H, 22.2% S, and 33.3% O. The molar
mass is 288 g/mol. Write the formula.
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BALANCING CHEMICAL EQUATIONS
Balance the following chemical equations and identify the reaction type for 1-20:
C = Combustion; D = Decomp.; S = Synthesis; SR = Single Replacement; DR = Double Replacement
Remember MINHO!
1. _____CH4 + _____O2  _____CO2 + _____H2O
2. _____Na + _____I2  _____NaI
3. _____N2 + _____O2  _____N2O
4. _____N2 + _____H2  _____NH3
5. _____KI + _____Cl2  _____KCl + _____I2
6. _____HCl + _____Ca(OH)2  _____CaCl2 + _____H2O
7. _____KClO3  _____KCl + _____O2
8. _____K3PO4 + _____HCl  _____KCl + _____H3PO4
9. _____S + _____O2  _____SO3
10. _____KI + _____Pb(NO3)2  _____KNO3 + _____PbI2
11. _____CaSO4 + _____AlBr3  _____CaBr2 + _____Al2(SO4)3
12. _____H2O2  _____H2O + _____O2
13. _____Na + _____H2O  _____NaOH + _____H2
14. _____C2H6 + _____O2  _____CO2 + _____H2O
15. _____Mg(NO3)2 + _____K3PO4  _____Mg3(PO4)2 + _____KNO3
16. _____NaCl + _____F2  _____NaF + _____Cl2
17. _____H2 + _____O2  _____H2O
18. _____AgNO3 + _____K2SO4  _____KNO3 + _____Ag2SO4
19. _____AlBr3 + _____K2SO4  _____Al2(SO4)3 + _____KBr
20. _____C3H8 + _____O2  _____CO2 + _____H2O
Rxn Type:_______
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Write the proper formula for each substance in the reaction, and balance these chemical equations:
(If the formula is incorrect, it won’t balance!! Remember Br2I2N2Cl2H2O2F2!)
21. Barium chloride + sodium sulfate  barium sulfate + sodium chloride
22. Calcium + hydrochloric acid  calcium chloride + hydrogen
23. Iron(II) sulfate + hydrochloric acid  iron(II) chloride + hydrogen sulfate
24. Magnesium + nitric acid  magnesium nitrate + hydrogen
25. Sodium iodide + bromine  sodium bromide + iodine
26. Sodium chlorate  sodium chloride + oxygen
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CHEMICAL REACTIONS
There are five common types of reactions we’ll be studying…for now! They are combustion,
decomposition, single displacement, double displacement, and synthesis reactions. Other types exist such
as equilibrium, redox, organic, and more!
TYPES OF CHEMICAL REACTIONS
Synthesis
Burning in oxygen, creates H2O + CO2
CH4 + O2  CO2 + H2O
Combustion Reactions occur when hydrocarbons or carbohydrates burn in oxygen. The products
are ALWAYS water and carbon dioxide.
btw:
Diatomic
Molecules:
Practice! Write combustion reactions (and balance them) for the following: C8H18 (octane),
C2H5OH (ethanol), C12H22O11 (sucrose):
Practice: Predict products and write balanced chemical reactions for the following.
1. Ethanoic acid (HC2H3O2) is burned in air.
2. Carbon tetrahydride (also known as methane) is burned.
3. A sample of 1-octanol (C8H17OH) is burned.
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Decomposition Reactions occur when a single reactant is broken down into two or more
products, sometimes spontaneously and sometimes with the addition of heat. About the phrasing below:
“metallic carbonate” means an ionic compound composed of a metal bonded to carbonate ion(s).
1. Metallic carbonates decompose into metallic oxides and carbon dioxide.
example
A sample of magnesium carbonate is heated.
MgCO3  MgO + CO2
2. Metallic chlorates and perchlorates decompose into metallic chlorides and oxygen.
example
A sample of iron(III) chlorate is heated.
2Fe(ClO3)3  2FeCl3 + 9O2
3. Metallic hydroxides (bases) decomposes into metallic oxides and water.
example
Solid potassium hydroxide is heated.
2KOH  K2O + H2O
4. A binary compound may break down to produce two elements.
example
Molten sodium chloride is electrolyzed.
2NaCl  2Na + Cl2
5. Hydrogen peroxide decomposes into oxygen and water.
example
2H2O2  2H2O + O2
6. Ammonium carbonate decomposes into ammonia, carbon dioxide, and water.
example
A sample of ammonium carbonate is heated.
(NH4)2CO3  2NH3 + CO2 + H2O
 7. Sulfurous acid decomposes into sulfur dioxide and water.
example
A sample of sulfurous acid is heated.
H2SO3  SO2 + H2O
=
 8. Carbonic acid decomposes into carbon dioxide and water.
example
A sample of carbonic acid is heated.
H2CO3  CO2 + H2O
 9. Ammonium hydroxide decomposes into ammonia and water.
example
NH4OH  NH3 + H2O
Practice for Combustion and Decomposition (Test questions will appear in this format. Write out the
chemical formulas for reactants from question, write formulas for products you predict, balance reaction):
1. _____A sample of calcium carbonate is heated.
2. _____Liquid hydrogen peroxide is warmed.
3. _____Dicarbon hexahydride is burned.
4. _____Molten aluminum chloride is electrolyzed.
5. _____A sample of carbonic acid is heated.
6. _____A sample of potassium perchlorate is heated.
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Single Replacement Reactions are reactions that involve an element replacing one part of a
compound. The products include the displaced element and a new compound. The more reactive element
(metal or nonmetal) will always end up as part of the compound; if the more reactive element is already in
the compound, no reaction will occur.
Single Replacement Reaction Lab (Completed in Lab Notebook) Behavior/safety and clean-up will be
considered part of the grade. Don’t forget titles for each section. Don’t cram everything on one page. Be
neat!
OBJECTIVE: Create a reactivity series for metals.
PROCEDURE: Perform reactions between each metal and each solution. Write down your observations.
Use 3 drops of solution, just enough to cover the piece of metal. Do not perform a reaction of a metal with
its own solution (ex. copper metal and CuCl2 solution)!! This creates unnecessary chemical waste.
DATA: Create a data table for observations of the reaction of each metal with each solution.
EQUATIONS: Write balanced chemical equations for each reaction observed. Write reactions for all 16 sets of
reactants. After the arrow, write products or ‘NR’. For example: Mg + 2AgNO3  Mg(NO3)2 + 2Ag. Assume that
copper and tin will have a charge of +1 when they form ionic compounds.
QUESTIONS: (Write the ENTIRE question, and answer directly beneath each question):
1. Considering the reactions you observed, under what circumstances will ‘no reaction’ occur?
2. Create an activity series for the 5 metals you observed using your data. Label most and least
reactive.
CONCLUSION: Write a conclusion (3-5 sentences) to justify the order of your activity series. Use complete
sentences.
After your lab, we will fill this in together:
General activity series for METALS
more reactive
General activity series for NONMETALS
less reactive
Metals have three types of reactions: metals with metals, metals with acid, metals with water (1-3 below):
1. Active metals replace less active metals from their compounds in aqueous solution.
example
Magnesium turnings are added to a solution of iron(III) chloride.
3Mg + 2FeCl3  2Fe + 3MgCl2
2. Active metals replace hydrogen in water.
example
Sodium is added to water.
2Na + 2HOH  H2 + 2NaOH
3. Active metals replace hydrogen in acids.
example
Lithium is added to hydrochloric acid.
2Li + 2HCl  H2 + 2LiCl
4. Active nonmetals replace less active nonmetals from their compounds in aqueous solution.
example
Chlorine gas is bubbled into a solution of potassium iodide.
Cl2 + 2KI  I2 + 2KCl
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If a less reactive element (metals and nonmetals) is combined with a more reactive element in compound
form, no reaction will occur.
example
Chlorine gas is bubbled into a solution of potassium fluoride.
Cl2 + KF  no reaction (NR)
example
Zinc is added to a solution of sodium chloride.
Zn + NaCl  no reaction (NR)
***Note: On the AP reaction prediction section, all reactions “work”; in other words there will be no “No
reaction” on the AP Exam.
Practice! (beware: combustion and decomposition….):
1. _____A piece of copper is dropped into a container of water.
2. _____An aluminum strip is immersed in a solution of silver nitrate.
3. _____Zinc pellets are added to a sulfuric acid solution.
4. _____Ammonium carbonate is gently heated over a Bunsen burner.
5. _____Fluorine gas is bubbled into a solution of aluminum chloride.
6. _____Magnesium turnings are added to a solution of lead(II) acetate.
7. _____Iodine crystals are added to a solution of sodium chloride.
8. _____Propane (C3H8) is burned in air.
9. _____Calcium metal is added to a solution of nitrous acid.
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10. _____A pea-sized piece of lithium is added to water.
11. _____A solution of iron(III) chloride is poured over a piece of platinum wire.
Solubility means the ability of something to dissolve in a solvent. Usually our solvent is water.
Mainly Water Soluble (will dissolve into ions in water)
All nitrates, chlorates, & perchlorates.
All ionic compounds containing alkali metal cations (group IA) and ammonium.
All acetates except silver acetate.
All chlorides, bromides, and iodides except mercury, silver, and lead(II).
All sulfates except mercury, silver, lead(II), calcium, barium, and strontium.
Mainly Water Insoluble (will NOT dissolve into ions in water; will remain as a solid “precipitate”)
All carbonates, phosphates, and sulfites except Group IA and ammonium.
All sulfides except Group IA and IIA and ammonium.
All hydroxides except Group IA, ammonium, calcium, strontium, and barium.
What is “ion soup?”
(s)=
(l)=
(g)=
(aq)=
Practice! Make up 5 examples of soluble compounds, and 5 examples of insoluble compounds.
Double Replacement Reactions
In order to predict double replacement reactions yielding precipitates, one must memorize the solubility
rules listed on page 6. Also memorize the five common gases and seven strong acids, listed below:
Common gases: H2S, CO2, SO2, NH3, HCN (g)as
Strong acids (dissociate completely): HCl, HBr, HI, HClO3, HClO4, HNO3, H2SO4  (aq)ueous
Title:
DOUBLE DISPLACEMENT LAB
Purpose: to use your knowledge of solubility rules to predict reactions that will create solids and gases
Materials:
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Copper(II) sulfate
Silver nitrate
Ammonium carbonate
strontium nitrate
sodium hydroxide
iron(III) nitrate
cobalt(II) chloride
nickel(II) chloride
sodium bicarbonate
phosphoric acid
Pre-lab (due tomorrow; -10 pts on your lab grade if incomplete)
1. Write the names for each substance
2. Write balanced double displacement reactions to create 3 different solids and 1 gas
3. Copy the data table below, but leave it blank. There should be room for eight different reactions (The goal
is to product 5 solids and 1 gas; there are two extra columns in case you predict incorrectly.)
Before Going to Lab
Sit with your group and choose 5 sets of chemical reactants that will produce solids and 1 set that will produce a
gas (bubbles or smell). Write the reactants in the data table.
Reactants
Observations (include color,
smell, bubbles, precipitate, etc.)
Procedure
Place one to two drops of each chemical reagent in the well plate. Make observations. You may need to move the
well plate onto black and white backgrounds to observe the precipitate. Do not be wasteful with chemicals. One
or two drops is sufficient. Points will be deducted from teams who waste chemicals.
Clean-Up
Rinse everything down the drain. Dry the well plate. Close all bottles and return caps. Clean up any spills. Return
your basket. Wash your hands.
Lab Write-Up (TO BE DONE INDIVIDUALLY)
For each of the 6 reactions:
~neatly write the balanced reaction (using s, l, g, aq) and name all products
Practice! What will happen if the substances below are mixed? Write balanced chemical reactions (watch
out for other reaction types!):
1. _____Silver nitrate and potassium bromide
2. _____Ammonium chloride and cobalt(II) sulfate
3. _____Cadmium carbonate is electrolyzed
4. _____Lithium hydroxide and sodium chromate
5. _____Zinc acetate and cesium hydroxide
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6. _____Ammonium sulfide and lead(II) nitrate
7. _____Iron(III) sulfate and barium iodide
8. _____Magnesium and tin(I) nitrate
9. _____Chromium(III) bromide and sodium nitrate
10. _____Rubidium phosphate and titanium(IV) nitrate
11. _____Ammonium carbonate and nickel(II) chloride
12. _____Tin(IV) nitrate and potassium sulfite
13. _____ dicarbon hexohydride is burned.
Synthesis Reactions occur when two or more reactants combine to form a single product. There
are several common types of synthesis reactions.
1. A metal combines with a nonmetal to form a binary salt.
example
A piece of lithium metal is dropped into a container of nitrogen gas.
6Li + N2  2Li3N
2. Metallic oxides and water form bases (metallic hydroxides).
example
Solid sodium oxide is added to water.
Na2O + HOH  2NaOH
Solid magnesium oxide is added to water.
MgO + HOH  Mg(OH)2
3. Nonmetallic oxides and water form acids. The nonmetal retains its oxidation number.
example
Carbon dioxide is bubbled into water.
CO2 + H2O  H2CO3
Dinitrogen pentoxide is bubbled into water.
N2O5 + H2O  2HNO3
4. Metallic oxides and nonmetallic oxides form salts. The nonmetal retains its oxidation number.
example
Solid sodium oxide is added to carbon dioxide.
Na2O + CO2  Na2CO3
Solid calcium oxide is added to sulfur trioxide.
CaO + SO3  CaSO4
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Practice!
1. _____Sulfur trioxide is bubbled into water.
2. _____chlorine gas is added to magnesium.
3. _____Nickel (II) perchlorate is warmed.
4. _____Solid sodium is combined with iodine gas.
5. _____Aluminum foil is added to sulfuric acid.
6. _____Solid calcium oxide is added to water.
7. _____Solutions of silver nitrate and zinc chloride are mixed.
Practice Test
REVIEW: Write the reaction type in the line. Write formulas for reactants and products of the following
reactions. Name the products.
1. _____Sodium chlorate is warmed.
2. _____C3H6 is burned.
3. _____Solutions of copper (II) hydroxide and acetic acid are mixed.
4. _____Iron (II) sulfate + Aluminum sulfide 
5. _____Calcium hydroxide + Phosphoric acid 
6. _____Iron(II) + copper (II) nitrate 
7. _____Magnesium + Oxygen 
8. _____Magnesium carbonate 
9. _____Hydrogen + Chlorine 
10. _____Barium carbonate 
11. _____Zinc hydroxide 
12. _____Iron (III) hydroxide 
13. _____Silver + Sulfur 
14. _____Potassium iodide + chlorine 
15. _____Sodium iodide + Bromine 
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TEACHER PAGES!!!!
Exercise 9-2: Predict and balance the following double replacement reactions. Use the abbreviations (s),
(l), (g), and (aq) for the reactants and products. All reactions are aqueous unless otherwise stated.
1. ammonium sulfate and potassium hydroxide are mixed together
2. ammonium sulfide is reacted with hydrochloric acid
3. cobalt (II) chloride is combined with silver nitrate
4. solid calcium carbonate is reacted with sulfuric acid
5. potassium sulfite is reacted with hydrobromic acid
6. potassium sulfide is reacted with nitric acid
7. ammonium iodide + magnesium sulfate
8. solid titanium (IV) carbonate + hydrochloric acid
9. solid calcium sulfite + acetic acid
10. strontium hydroxide + ammonium sulfide
Exercise 9-3: Predict and balance the following reactions. Use the abbreviations (s), (l), (g), and (aq) for
the reactants and products. All reactions are aqueous unless otherwise stated.
1. carbon dioxide gas is bubbled through a solution of lithium hydroxide
2. sodium nitrite is reacted with hydrochloric acid
3. ammonium bromide + sodium hydroxide
4. carbon dioxide gas is reacted with solid potassium oxide
5. solid magnesium oxide is reacted with hydrochloric acid
6. equal numbers of moles of potassium hydroxide and phosphoric acid react
7. sodium fluoride reacts with dilute nitric acid
8. ammonium carbonate + potassium bromide
9. oxalic acid (0.1 M) reacts with an equal volume of cesium hydroxide (0.1 M)
10. silver nitrate + sodium chromate
1. iron filings added to copper (II) sulfate in solution
2. aluminum in hydrochloric acid
3. potassium metal added to cold water
4. zinc metal added to mercury (II) nitrate
5. silver metal added to copper (II) sulfate
6. chlorine gas bubbled through a solution of calcium bromide
7. potassium iodide added to lead (II) nitrate
8. sodium sulfite combined with acetic acid
9. sodium chloride added to sulfuric acid
10. barium nitrate added to sodium oxalate
11. sodium bicarbonate added to hydrochloric acid
Part 1: Write and balance in chemical equation from the following sentences. Include states.
a. Solid magnesium hydroxide reacts with aqueous nitric acid
b. Aqueous strontium chloride reacts with aqueous lead (II)
c. Aqueous potassium phosphate and aqueous calcium bromide react.
d. The reaction of solid lithium with liquid
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Part 2: Using the activity series table and the halogen activity rules, predict whether a reaction would
occur in the following reactions. If a reaction does occur, write the products in the correct formulas, then
balance the equation. If no reaction occurs, write “NR.”
a. Fe(s) + SnCl2(aq) 
b. NaCl(aq) + Br2(l) 
c. Ag(s) + CuCl2(aq) 
d. Zn(NO3)2(aq) + Mg(s) 
e. CuCl(aq) + Cd(s) 
Part 3: Predict the products for the following reactions. Give the states for each of the products. Balance
the equations.
a. Pb(NO3)2(aq) + KI(aq) 
b. NiCO3(s) + HCl(aq) 
c. MgSO4(aq) + Na3PO4(aq) 
d. Ba(OH)2(aq) + MgSO4(aq) 
e. C4H10(l) + O2(g) 
General activity series for METALS
(most active) Li Ca Na Mg Al Zn Fe Pb [H2] Cu Ag Pt (least active)
General activity series for NONMETALS
(most active) F2 Cl2 Br2 I2 (least active)
Single
Sulfur dioxide gas is bubbled through water.
A pea-sized piece of sodium is added to a container of iodine vapor.
Solid magnesium oxide is added to sulfur trioxide gas.
Solid potassium oxide is added to a container of carbon dioxide gas.
Solid lithium oxide is added to water.
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Chemical Reactions
Balancing Equations, Reaction Types, Predicting Products, Solubility Rules, Activity Series
Back to the basics: We’re going back to the old style of homework. I will check homework every day for
a completion grade. No late work will be accepted, so get to work each night and stay on top of your
chemistry!
Thursday
Friday
1/22
1/23
Monday
Tuesday
1/26
1/27
In Class
Balancing, Intro to Types of Reactions
Combustion, Decomposition
Homework (due next day)
Pg 1, 1-20
Finish pg 1-2, comb prob,
decomp probs
decomp probs
Single replacement reactions
Single Replacement Lab
Lab Debriefing, Activity Series, Double
Replacement Reaction, Solubility Rules
Wednesday 1/28 Review HW, Review 4 types of Reactions,
Double replacement reactions
Double Replacement Lab
Thursday
1/29 Nomenclature Quiz, Double Replacement
Reactions: Will they happen?
Friday
1/30 Synthesis Reactions, Review 5 types of
Pg 10
Reactions
Monday
2/2
Review
Tuesday
2/3
Next Unit
Wednesday 2/4
Next Unit
Thursday
2/5
Next Unit
Finish packet, study for test 
Friday
2/6
Test
***This is a tentative schedule and may change as needed. Be flexible!
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NAME___________________________Per______
Chemical Reactions
Balancing Equations, Reaction Types, Predicting Products, Solubility Rules, Activity Series
Back to the basics: We’re going back to the old style of homework. I will check homework every day for
a completion grade. No late work will be accepted, so get to work each night and stay on top of your
chemistry!
Thursday
1/22
In Class
Balancing, Intro to Types of Reactions
Friday
1/23
Combustion, Decomposition
Monday
1/26
Single Replacement Lab
Tuesday
1/27
Wednesday
1/28
Thursday
1/29
Friday
1/30
Monday
2/2
Lab Debriefing, Activity Series, Double
Replacement Reaction, Solubility Rules
Review HW, Review 4 types of Reactions,
Double Replacement Lab
Nomenclature Quiz, Double Replacement
Reactions: Will they happen?
Synthesis Reactions, Review 5 types of
Reactions
Review
Homework (due next day)
Tuesday
2/3
Next Unit
Wednesday 2/4
Next Unit
Thursday
2/5
Next Unit
Finish packet, study for test 
Friday
2/6
Test
***This is a tentative schedule and may change as needed. Be flexible!
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