Honors Chemunit #6 Chemical Reactions Name ______

Honors ChemUnit #6 “Chemical Reactions”Name ______

I) Assignments / Handouts

A)Balancing chemical equations (info – pg 2)

B)Balancing equations ws(required – pg 3-4)

C)Chap 11 text asst(required – pg 5-6)

D)Word equations ws(required – pg 7-8)

E)Types of reactions notes and practice(required – pg 9-10)

F)Reaction types ws(required – pg 11-12)

G)Chemical reactions ws(required – pg 13-14)

H)Chemical reactions lab

I)Challenge problems

J)More TBA

II) Text Support (Chapter 11)

Section 11-1pg 344-355intro to chemical reactions
Section 11-2pg 356-368types of chemical reactions
Section 11-3pg 369-373reactions in aqueous solutions

Pearson Chemistry On-Line Text is now available at

(Log in as returning user near the upper right corner. Following is the common username and password for all honors chemistry students.)

Username:yetties

Password:sasquatch1 (the last symbol is the number “one” and not letter “l”)

Then choose from the following:

e-text (for on-line text)

practice (for support materials)

Standardized Test Prep Key for chapter 11 on page 381

1-B2-E3-C4P = Ca(NO3)24Q= K2CO34R = HCl

5 --- Ca+2(aq) + CO3-2(aq)  CaCO3(s)6 --- 2 H+(aq) + CO3-2(aq)  H2O(liq) + CO2(g) 7-D 8-decomposition 9-10 --- (NH4)2CO3(s)  2 NH3(g) + CO2(g) + H2O(liq)

11--- Ca(OH)2(aq) + CO2(g)  CaCO3(s) + H2O(liq)

Science Geek Website at (choose chemistry homepage from menu on left)

Interactive practice activities

Unit #4 – Periodic Behavior and Ionic Bonding (bullet points 4-7)

Identifying the reaction type

Does this reaction occur?

Predicting the names of products

Equation balancing

III) Learning Targets (I can…)

A) Balance chemical equations using appropriate coefficients.

B) Write balanced chemical equations from word equations.

C) Identify synthesis (composition), decomposition, single displacement, double displacement, and combustion reactions.

D) Given reactants --- predict reaction type and products. Write balanced chemical equations given those reactants.

E) Perform experiments. Determine reaction type and write balanced chemical equations for those experiments.

IV) Tentative Schedule

Thu12/10Biochem assignment

Fri12/11Balancing equations and word equations

Mon12/14Biochem day

Tue12/15Reactions Types

Wed 12/16Chemical reaction lab

Thu12/17Chemical reaction lab; challenge problems

Fri12/18Review

Mon12/21Written exam; Homework packets due

Tue12/22Lab Exam

Wed12/23TBA

Hint --- The following elements come in pairs: Br2 I2 N2 Cl2 H2 O2 F2

Assume other elements exist individually (unless directed otherwise)

V) On-line support

Mr. Guch’s website

(balancing equations, writing word equat, types of reactions)

This website may help you out in your quest to understand chemistry. Explanations are at the introductory level and give some detail --- but not too much.

ChemTeam

(chemical equations and reaction types)

This website may help you in your quest to understand chemistry. Explanations can get quite involved – depending on the topic. It may be helpful at the introductory level. It will be especially helpful if you are looking for extra detail.

Balancing chemical equations computer games

Classic Chembalancer, Review Chembalancer, Brain Boggle Chembalancer

Millionaire game – Can you earn your first million?

Balancing Chemical Equations --- Notes

Chemical Equation: Description of a chemical reaction using symbols and formulas.

C + O2  CO2

Reactant: Substance that enters into rection (left side)

Product: Produced by chemical reaction (right side)

Subscript: Little # describing amount of atoms

Coefficient: # in front describing amount of moles

Conservation of Mass Law-Atoms can be neither created nor destroyed during a chemical equation. So… The number of atoms on each side of the arrow has to be the same.

We have to add COEFFICIENTS to the front of the formulas to BALANCE an equation. Do NOT change the chemical formulas in the equation.

C + O2  CONot balanced (need O on right)

C + O2  2CO What else did that change?

2C + O2  2COPerfect.

Balancing Hints:

Start simple. What is different?
Group polyatomic ions if possible.
If in doubt, balance H2O last.
Check to make sure equation is correct (conservation of atoms)

Try these:

Mg+O2MgO

Na+Cl2NaCl

MgCO3+HClMgCl2+H2CO3

Balance These Equations:

1. HgO+Cl2HgCl+O2

2. Na+Br2NaBr

3.Al2O3Al+O2

4. CuCl2+H2SCuS+HCl

5. Cl2+NaBrNaCl+Br2

6.NaOH+HClNaCl+H2O

7. KClO3KCl+O2

8.Na2O+CO2Na2CO3

9. H2O+FeFe2O3+H2

10. Ca(OH)2+HNO3Ca(NO3)2+H2O

Name

Balancing Chemical Equations

1)____ N2 + ____ H2  ____ NH3

2)____ KClO3  ____ KCl + ____ O2

3)____ NaCl + ____ F2  ____ NaF + ____ Cl2

4)____ H2 + ____ O2  ____ H2O

5)____ Pb(OH)2 + ____ HCl  ____ H2O + ____ PbCl2

6)____ AlBr3 + ____ K2SO4  ____ KBr + ____ Al2(SO4)3

7)____ CH4 + ____ O2  ____ CO2 + ____ H2O

8)____ C3H8 + ____ O2  ____ CO2 + ____ H2O

9)____ FeCl3 + ____ NaOH  ____ Fe(OH)3 + ____NaCl

10)____ P + ____O2  ____P2O5

11)____ Na + ____ H2O  ____ NaOH + ____H2

12)____ Ag2O  ____ Ag + ____O2

13)____ S8 + ____O2  ____ SO3

14)____ CO2 + ____ H2O  ____ C6H12O6 + ____O2

15)____ HCl + ____ CaCO3  ____ CaCl2 + ____H2O + ____ CO2

16)____ H2O + ____ O2  ____ H2O2

17)____ H2SO4 + ____ NaNO2  ____ HNO2 + ____ Na2SO4

18)____ C8H18 + ____ O2  ____ CO2 + ____ H2O

Chapter 11 Book Assignment (p. 344-373)

1 – Chemystery: Why should Maria not place sodium hydroxide next to sulfuric acid?

2 – Define catalyst.

3 – Write the balanced chemical equation for the decomposition of hydrogen peroxide into water and oxygen gas using MnO2 as a catalyst. Include proper placement of the MnO2 catalyst in the equation.

4 – What do each of the following subscripts represent: (s), (l), (g), (aq)

5 – In a balanced chemical equation, which of the following are always true?

Sum of reactant coeffifiencts = sum of product coefficients

Sum of reactant atoms of any element = sum of product elements of the same element

Mass of reactant atoms = mass of product atoms

6 – Does the loss of mass when a candle burns violate the law of conservation of mass? Explain.

7 – Write a balanced chemical equation for each of the following general reaction types listed below:

Combination (synthesis)

Decomposition

Single replacement

Double replacement

Combustion

8 – What “triggers” many decomposition reactions.

9 – What is the activity series for metals?

10 – The reactivity series for halogens helps us identify ______as the most reactive halogen.

11 – Which of the following would react with HCl (hydrochloric acid): Zn, Cu, Ag, Mg Explain.

12 – The solid product formed when 2 aqueous solutions combine is called a ______.

13 – Does gasoline that burns in a car undergo complete combustion? Explain.

14 – Write the balanced equation for the detonation of nitroglycerin. What type of reaction is this?

15 – What chemical makes up stalagmites and stalactites in many caves?

16 – Write the net ionic equation for the reaction of barium nitrate and sodium carbonate.

17 – Identify the spectator ions in the reaction in #16.

18 – Which of the following are not soluble? Na2CO3 NaCl PbCl2 CuSO4 BaSO4

19 – Why does chlorinated tap water get cloudy in the presence of silver nitrate.

20 - Write the net ionic equation for the precipitate that forms in #19.

Word Equations Name ______

Directions:

Write out and balance the following chemical equations.
Identify each reaction as synthesis (composition), decomposition, single displacement, double displacement, or combustion. (Hint: See pages 356-368 in text and/or class notes)

The following elements come in pairs: Cl2, H2, O2, Br2, F2, I2, N2

Assume other elements exist individually (unless directed otherwise)

Zinc and lead (II) nitrate react to form zinc nitrate and lead.

Potassium metal and bromine gas combine to form potassium bromide.

Aluminum bromide and chlorine gas react to form aluminum chloride and bromine gas.

Sodium oxide and calcium chloride react to form calcium oxide and sodium chloride.

Hydrogen gas and nitrogen monoxide react to form water and nitrogen gas.

Aluminum and hydrogen chloride (hydrochloric acid) react to form aluminum chloride and hydrogen gas.

Sodium hydroxide and aluminum nitrate react to form sodium nitrate and aluminum hydroxide.

Tin (IV) iodide + barium nitride  barium iodide + tin (IV) nitride.

Aluminum chloride decomposes into aluminum and chlorine gas.

Tricarbon octahydride (propane) burns in oxygen gas to form carbon dioxide and water vapor.

Part II – Answer the questions 1-5 using pages 356-368 in text and/or class notes.

What is the difference between a synthesis and a decomposition reaction?

What is the difference between a single and a double displacement reaction?

What two compounds are formed during a combustion reaction involving a hydrocarbon?

Can all chemical reactions written actually take place? (p. 361) Explain.

For the following pairs of elements, circle the one that is MORE REACTIVE (p.361).

sodiumorpotassium

zinc or hydrogen

fluorineor chlorine

5 Types of Reactions --- NotesName ______

Synthesis (or composition): 2 or more reactants join to form 1 product.

sodium+chlorinesodium chloride

2Na+Cl22NaCl

Magnesium+fluorine

Decomposition: Substances are broken apart into smaller pieces.

Calcium carbonatecalcium oxide +carbon dioxide

CaCO3CaO+CO2

Mercury (II) oxide

Single Displacement: One single element takes the place of another in a compound.

Copper (II) chloride + iron  copper + iron (II) chloride

CuCl2+FeCu+FeCl2

Copper+silver nitrate

Double Displacement: Two compounds exchange ions.

Sodium hydroxide + potassium chloride  sodium chloride + potassium hydroxide

NaOH +KCl NaCl+ KOH

Potassium hydroxide + barium fluoride 

Combustion: A hydrocarbon combines with O2, forming CO2 and H2O.

Tricarbon tetrahydride + oxygen  carbon dioxide + water

C3H8+5 O2 3 CO2+ 4 H2O

Dicarbon dihydride + oxygen  carbon dioxide + water

Identify the type of reaction

For the following reactions, indicate whether the following are examples of synthesis, decomposition, combustion, single displacement, or double displacement:

1)Na3PO4 + 3 KOH  3 NaOH + K3PO4 ______

2)MgCl2 + Li2CO3  MgCO3 + 2 LiCl ______

3)C6H12 + 9 O2  6 CO2 + 6 H2O ______

4)Pb + FeSO4  PbSO4 + Fe ______

5)CaCO3  CaO + CO2 ______

6)P4 + 3 O2  2 P2O3 ______

7)2 RbNO3 + BeF2  Be(NO3)2 + 2 RbF ______

8)2 AgNO3 + Cu  Cu(NO3)2 + 2 Ag ______

9)C3H6O + 4 O2  3 CO2 + 3 H2O ______

10)2 C5H5 + Fe  Fe(C5H5)2 ______

11)SeCl6 + O2  SeO2 + 3Cl2 ______

12)2 MgI2 + Mn(SO3)2  2 MgSO3 + MnI4 ______

13)O3  O. + O2 ______

14)2 NO2  2 O2 + N2______

Reaction TypesName ______

Directions:

Complete each word equation by predicting which product(s) are formed.
Then, write out and balance each chemical equation.

The following elements come in pairs: Cl2, H2, O2, Br2, F2, I2, N2

Assume other elements exist individually (unless directed otherwise)

Synthesis or Composition (assume elements combine to form a balanced ionic compound unless stated otherwise)

1.lithium + fluorine 

2.calcium + oxygen 

3.aluminum + oxygen 

4.carbon + oxygen  carbon monoxide

Decomposition (assume compound breaks up into its component elements unless stated otherwise)

5.sodium chloride 

6.dihydrogen monoxide (water) 

7.silver oxide 

8.potassium chlorate  potassium chloride + oxygen

Single Displacement

9.zinc + copper (II) chloride 

10.chromium (III) sulfite + calcium 

11.magnesium + hydrogen chloride (hydrochloric acid) 

12.fluorine + sodium chloride 

Double Displacement

13.silver nitrate + sodium chloride 

14.sodium hydroxide + hydrogen chloride (hydrochloric acid) 

15.potassium chloride + calcium hydroxide 

16.potassium phosphate + calcium chloride 

Combustion (assume hydrocarbons combine with oxygen to form carbon dioxide and water vapor unless stated otherwise)

17.carbon tetrahydride (methane) + oxygen 

18.dicarbon tetrahydride + oxygen 

19.pentacarbon octahydride + oxygen 

20.ethanol (C2H6O) + oxygen 

Name______Hour ______

Chemical Reactions

Predict the products of the following reactions, and then balance them.

Identify the type of each reaction.

1)__ Ag + __CuSO4 

Type:______

2)__ NaI + __ CaCl2 

Type:______

3)__ O2 + __ H2 

Type:______

4)__ NaNO3 + __ Mn(OH)2 

Type:______

5)__ AgNO2 + __ BaSO4 

Type:______

6)__ K2CrO4+ __ CuSO4 

Type:______

7)__ CaCO3 + __ AgI 

Type:______

8)__ C6H12 + __O2 

Type:______

9)__ LiBr + __ Pb(SO3)2 

Type:______

10)__ LiNO3 + __Ag 

Type:______

11)__ Fe (II) + __ O2 

Type:______

12)__ CaCl2 

Type:______

13)__ AlCl3 + __ Cs 

Type:______

14)__ Al(NO3)3 + __ Ga 

Type:______

15)__ CH4O2 + __ O2 

Type:______

16)__ C4H8 + __ O2 

Type:______

17)__ KCl + __ Mg(OH)2 

Type:______

18)__ Zn + __ Hg(NO2)2 

Type:______

19)__ H2 + __ O2 

Type:______

20)__ Na2O 

Type:______