C O - Matteson School District 162 O 2 CO 2 ! Reactants (left ... A combustion reaction is when...

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Matter Cannot Be Created Nor Destroyed 1. Law of Conservation of Mass –atoms going into the reaction (reactants) must equal atoms coming out of the reaction (products)

C O2 CO2 Reactants (left) Products (right) Q: How many carbon on the left? Q:How many carbon on the right? A: 1 atom of carbon A: 1 atom of carbon

Q: How many oxygen on the left? Q:How many oxygen on the right? A: 2 atoms of oxygen A: 2 atoms of oxygen

“This chemical equation is balanced!”

2. To balance a chemical equation only add or change coefficients!

“Thou shalt NOT change subscripts when balancing chemical equations!”

Unit 8: Balancing and Identifying Chemical Reactions Packet

Name:___________________________________________

Again: Do Not Change Subscripts!!!! You can only change Coefficients!!

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T. Trimpe 2006 http://sciencespot.net/

Name __________________________ Atoms are not _______________ or _____________ during a chemical reaction.

Scientists know that there must be the ___________ number of atoms on each ___________ of

the ____________. To balance the chemical equation, you must add _______________ in front

of the chemical formulas in the equation. You cannot _______ or ___________ subscripts!

Mg + O2 MgO Try these: Ca + O2 CaO Ca = Ca =

O = O = N2 + H2 NH3 N = N =

H = H = Cu2O + C Cu + CO2 Cu = Cu =

O = O =

C = C = H2O2 H2O + O2 H = H =

O = O =

1) Determine number of atoms for each element.

2) Pick an element that is not equal on both sides of the equation.

3) Add a coefficient in front of the formula with that element and adjust your counts.

4) Continue adding coefficients to get the same number of atoms of each element on each side.

Mg = O =

Mg = O =

Balancing Act Notes + Practice

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Step-by-Step Example Problem: Step 1: Determine number of atoms for each element. Step 2: Pick an element that is not equal on both sides of the equation. Step 3: Add a coefficient in front of the formula with that element and adjust your counts. Step 4: Continue adding coefficients to get the same number of atoms of each element on each side.

Mg = 1 O = 2

Mg = 1 O = 1

Mg + O2 MgO

Mg = 1 O = 2

Mg = 1 O = 1

Mg + O2 MgO

Since the O atoms are not equal, we’ll target those first!

2 Mg + O2 2 MgO

Mg = 1 O = 2

Mg = 1 2 O = 1 2

Mg + O2 2 MgO Adding a 2 in front of MgO will change the number of atoms on the product side of the equation.

Now we need to increase the number of Mg atoms we have on the reactant side. Adding a 2 in front of Mg will give us 2 atoms of Mg and balance the equation.

Mg = 1 2 O = 2

Mg = 1 2 O = 1 2

Balancing Act Teacher Notes

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Name __________________________ Atoms are not _______________ or _____________ during a chemical reaction.

Scientists know that there must be the ___________ number of atoms on each ___________ of

the ____________. To balance the chemical equation, you must add _______________ in front

of the chemical formulas in the equation. You cannot _______ or ___________ subscripts!

Mg + O2 MgO Try these: Ca + O2 CaO Ca = Ca =

O = O = N2 + H2 NH3 N = N =

H = H = Cu2O + C Cu + CO2 Cu = Cu =

O = O =

C = C = H2O2 H2O + O2 H = H =

O = O =

1) Determine number of atoms for each element.

2) Pick an element that is not equal on both sides of the equation.

3) Add a coefficient in front of the formula with that element and adjust your counts.

4) Continue adding coefficients to get the same number of atoms of each element on each side.

Mg = O =

Mg = O =


Balancing Equations Practice Name ____________________________ Part A: Identify the following parts of each chemical formula by circling the subscripts and drawing a square around the coefficients.

H2 2 HCl 4 O2 CH4 3 CO3 2 NaOH

Part B: List the symbols for the atoms in each formula and give the number of each.

C2H6 2MgO 4P4O10 NH3 3 Al(OH)3 2 H2O2

Part C: Balance each of the following equations following the procedure described in class. Be sure to show your work.

P + O2 P4O10 Mg + O2 MgO P = P = Mg = Mg =

O = O = O = O =

HgO Hg + O2 Al2O3 Al + O2 Hg = Hg = Al = Al =

O = O = O = O =

BaCl2 + H2SO4 BaSO4 + HCl

Ba = Ba =

Cl = Cl =

H = H =

S = S =

O = O =

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Name _______________________________________ Class ____________ Date ___________________________

Balancing Chemical Equations Worksheet For the following:

1. Draw a circle around each subscript. 2. Draw a square around each coefficient.

H2O 5Cl2 2Mg 3H2O2

For the following

1. List the chemical symbols of each element. 2. Give the number of atoms of each element.

HCl CO2 Na2SO4

Balance the following chemical equations. 1. ____ Cu2O + ____ C g ____ Cu + ____ CO2 2. ____ H2O2 g ____H2O + ____O2 3. ____ Al + ____Fe3N2 g ___ AlN + ____ Fe 4. ____Ag2S g ____Ag + ____ S8

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5. ____ ZnS + ____AlP g ____Zn3P2 + ____Al2S3 6. ____ Fe(OH)3 g ____ Fe2O3 + ____H2O Given the two chemical equations, circle the one that is balanced. 7. a. 2Na + Cl2 g 2NaCl b. 2Na + 2Cl2 g 2NaCl 8. a. C3H8 + 5O2 g 3CO2 + 4H2O b. 2C3H8 + 5O2 g 3CO2 + 8H2O 9. a. 2NH3 + 5O2 g 2NO + 3H2O b. 4NH3 + 5O2 g 4NO + 6H2O 10. a. Y(NO3)2 + GaPO4 g YPO4 + Ga(NO3)2 b. 2Y(NO3)2 + 2GaPO4 g 2YPO4 + Ga(NO3)2

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Balancing Act Practice Name ____________________________ Balance each equation. Be sure to show your lists! Remember you cannot add subscripts or place coefficients in the middle of a chemical formula. 1. Na + MgF2 NaF + Mg 2. Mg + HCl MgCl2 + H2 3. Cl2 + KI KCl + I2 4. NaCl Na + Cl2 5. Na + O2 Na2O 6. Na + HCl H2 + NaCl 7. K + Cl2 KCl Challenge: This one is tough! C2H6 + O2 CO2 + H2O

`

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Chapter 7 Worksheet #1 Balancing Chemical Equations

Balance the equations below: 1) ____ N2 + ____ H2 Æ ____ NH3 2) ____ KClO3 Æ ____ KCl + ____ O2 3) ____ NaCl + ____ F2 Æ ____ NaF + ____ Cl2 4) ____ H2 + ____ O2 Æ ____ H2O 5) ____ Pb(OH)2 + ____ HCl Æ ____ H2O + ____ PbCl2 6) ____ AlBr3 + ____ K2SO4 Æ ____ KBr + ____ Al2(SO4)3

7) ____ CH4 + ____ O2 Æ ____ CO2 + ____ H2O 8) ____ C3H8 + ____ O2 Æ ____ CO2 + ____ H2O 9) ____ C8H18 + ____ O2 Æ ____ CO2 + ____ H2O 10) ____ FeCl3 + ____ NaOH Æ ____ Fe(OH)3 + ____NaCl 11) ____ P + ____O2 Æ ____P2O5 12) ____ Na + ____ H2O Æ ____ NaOH + ____H2 13) ____ Ag2O Æ ____ Ag + ____O2 14) ____ S8 + ____O2 Æ ____ SO3 15) ____ CO2 + ____ H2O Æ ____ C6H12O6 + ____O2 16) ____ K + ____ MgBr2 Æ ____ KBr + ____ Mg 17) ____ HCl + ____ CaCO3 Æ ____ CaCl2 + ____H2O + ____ CO2 18) ____ HNO3 + ____ NaHCO3 Æ ____ NaNO3 + ____ H2O + ____ CO2 19) ____ H2O + ____ O2 Æ ____ H2O2 20) ____ NaBr + ____ CaF2 Æ ____ NaF + ____ CaBr2 21) ____ H2SO4 + ____ NaNO2 Æ ____ HNO2 + ____ Na2SO4

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Chapter 7 Worksheet #1 Balancing Chemical Equations

Balance the equations below: 1) ____ N2 + ____ H2 Æ ____ NH3 2) ____ KClO3 Æ ____ KCl + ____ O2 3) ____ NaCl + ____ F2 Æ ____ NaF + ____ Cl2 4) ____ H2 + ____ O2 Æ ____ H2O 5) ____ Pb(OH)2 + ____ HCl Æ ____ H2O + ____ PbCl2 6) ____ AlBr3 + ____ K2SO4 Æ ____ KBr + ____ Al2(SO4)3

7) ____ CH4 + ____ O2 Æ ____ CO2 + ____ H2O 8) ____ C3H8 + ____ O2 Æ ____ CO2 + ____ H2O 9) ____ C8H18 + ____ O2 Æ ____ CO2 + ____ H2O 10) ____ FeCl3 + ____ NaOH Æ ____ Fe(OH)3 + ____NaCl 11) ____ P + ____O2 Æ ____P2O5 12) ____ Na + ____ H2O Æ ____ NaOH + ____H2 13) ____ Ag2O Æ ____ Ag + ____O2 14) ____ S8 + ____O2 Æ ____ SO3 15) ____ CO2 + ____ H2O Æ ____ C6H12O6 + ____O2 16) ____ K + ____ MgBr2 Æ ____ KBr + ____ Mg 17) ____ HCl + ____ CaCO3 Æ ____ CaCl2 + ____H2O + ____ CO2 18) ____ HNO3 + ____ NaHCO3 Æ ____ NaNO3 + ____ H2O + ____ CO2 19) ____ H2O + ____ O2 Æ ____ H2O2 20) ____ NaBr + ____ CaF2 Æ ____ NaF + ____ CaBr2 21) ____ H2SO4 + ____ NaNO2 Æ ____ HNO2 + ____ Na2SO4

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Chemical Reaction Types All chemical reactions can be placed into one of six categories. Here they are, in no particular order: 1) Combustion: A combustion reaction is when oxygen combines with another compound to form water and carbon dioxide. These reactions are exothermic, meaning they produce heat. An example of this kind of reaction is the burning of napthalene:

C10H8 + 12 O2 ---> 10 CO2 + 4 H2O

2) Synthesis: A synthesis reaction is when two or more simple compounds combine to form a more complicated one. These reactions come in the general form of:

A + B ---> AB One example of a synthesis reaction is the combination of iron and sulfur to form

iron (II) sulfide: 8 Fe + S8 ---> 8 FeS

3) Decomposition: A decomposition reaction is the opposite of a synthesis reaction - a complex molecule breaks down to make simpler ones. These reactions come in the general form:

AB ---> A + B One example of a decomposition reaction is the electrolysis of water to make

oxygen and hydrogen gas: 2 H2O ---> 2 H2 + O2

4) Single displacement: This is when one element trades places with another element in a compound. These reactions come in the general form of:

A + BC ---> AC + B

One example of a single displacement reaction is when magnesium replaces hydrogen in water to make magnesium hydroxide and hydrogen gas:

Mg + 2 H2O ---> Mg(OH)2 + H2

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5) Double displacement: This is when the anions and cations of two different molecules switch places, forming two entirely different compounds. These reactions are in the general form:

AB + CD ---> AD + CB

One example of a double displacement reaction is the reaction of lead (II) nitrate with potassium iodide to form lead (II) iodide and potassium nitrate:

Pb(NO3)2 + 2 KI ---> PbI2 + 2 KNO3

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13

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YOUTUBE EXAMPLES:

1. Synthesis: EX:

Artwork taken from an unknown source (a worksheet acquired second-hand many years ago).

Types of Reactions

Chemical reactions can be categorized into a variety of types. Five common types that we will study are synthesis, decomposition, combustion, single replacement and double replacement. Be familiar enough with the description of each type so that you are able to classify a reaction if given a chemical equation or verbal description. Synthesis: Synthesis reactions involve the formation of more complex compounds (many atoms) from simpler compounds and/or elements. The most common synthesis reaction involves the formation of a compound from its elements.

Examples:

2 H2(g) + O2(g) 2 H2O(g)

3 H2(g) + N2(g) 2 NH3(g)

General: A + B AB Synthesis reactions are also referred to as combination, formation, and addition reactions.

Decomposition: Decomposition reactions involve the breaking down of more complex compounds (larger, more atoms) into simpler compounds and/or elements. These reactions can often be thought of as being the opposite of synthesis reactions. Decomposition reactions often require heating in order to occur.

Examples:

2 H2O(l) 2 H2(g) + O2(g)

2 KClO3(s) 2 KCl(s) + 3 O2(g)

General: AB A + B

Combustion: Combustion reactions involve the reaction of a substance with oxygen gas (O2). It is often referred to as burning. The products of the reaction are oxides of the elements in the reactants. Hydrocarbon combustion leads to the formation of carbon dioxide gas and water vapor. Examples:

2 Mg(s) + O2(g) 2 MgO(s)

CH4(g) + 2 O2(g) CO2(g) + 2 H2O(g)

General: AB + O2(g) AxOy + BwOz Some combustion reactions are also synthesis reactions. For instance, the combustion of magnesium leads to the formation of magnesium oxides

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Yours:

2. Decomposition: EX: Yours:

3. Single Replacement: EX: Yours:

4. Double Replacement: EX: Yours:

5. Combustion:

EX: Yours:

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Synthesis

Worksheet #2: Synthesis Reactions 1. calcium + oxygen → calcium oxide Ca + O2 → 2. copper + sulfur → copper(II) sulfide Cu + S8 → 4. hydrogen + nitrogen → ammonia H2 + N2 → 5. hydrogen + chlorine → hydrogen chloride H2 + Cl2 → 6. silver + sulfur → silver sulfide Ag + S8 → 7. chromium + oxygen → chromium(III) oxide Cr + 3O2 → 8. aluminum + bromine → aluminum bromide Al + Br2 → 9. sodium + iodine → sodium iodide Na + I2 → 10. hydrogen + oxygen → water H2 + O2 →

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Worksheet #2: Synthesis Reactions In synthesis reactions, two or more reactants come together to form one compound.

A + B � AB Complete the following word equations, and write and balance the formula equation. 1. calcium + oxygen � 2. copper + sulfur � copper(II) sulfide 3. calcium oxide + water � calcium hydroxide 4. hydrogen + nitrogen � 5. hydrogen + chlorine � 6. silver + sulfur � 7. chromium + oxygen � 8. aluminum + bromine � 9. sodium + iodine � 10. hydrogen + oxygen � 11. aluminum + oxygen �

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Decomposition Reaction Practice

1) Ni(ClO3)2 --->

2) Ag2O --->

3) HNO2 --->

4) Fe(OH)3 --->

5) ZnCO3 --->

6) Cs2CO3 --->

7) Al(OH)3 --->

8) H2SO4 --->

9) RbClO3 --->

10) RaCl2 --->

CHEMISTRY DECOMPOSITION REACTION WORKSHEET

DECOMPOSITION

REACTION GUIDELINE EXAMPLES

1. 2 NaCl ----> 2 Na + Cl22. Na2CO3 ----> Na2O + CO23. Ba(ClO3)2 ----> BaCl2 + O24. Ca(OH)2 ----> CaO + H2O5. 2 H3PO4 ----> P2O5 + 3 H2O

1. Binary compounds breakdown into their elements.

2. Carbonates break down into an oxide and carbon dioxide

3. Chlorates break down to a binary salt and oxygen.

4. Bases break down to the oxide of the metal and water.

5. Acids break down to the oxide of the nonmetal plus water.

AB ------> A + B

During decomposition, one compound splits apart into two or more substances. These substances can be elements or simpler compounds.

REACTION GUIDELINES

REACTION FORMAT

REACTION DESCRIPTION

REACTION CATEGORY

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Synthesis and Decomposition Reactions

Synthesis reactions are chemical reactions in which two or more substances react to form a new product. The general form of a synthesis reaction is written as: A + B à AB

Decomposition reactions are chemical reactions in which a reactant breaks down into two or

more products. The general form of a decomposition reaction is written as: AB à A + B Balance the following reactions and identify whether the reaction is a synthesis or decomposition reaction.

Balance the Reactions: Synthesis or Decomposition?

1. ___Ca + ___O2 à ___CaO ________________________

2. ___H2 + ___N2 à ___NH3 ________________________

3. ___H2O2 à ___H2O + ___O2 ________________________

4. ___H2 + ___O2 à ___H2O ________________________

5. ___CaCO3 à ___CaO + ___CO2 ________________________

6. ___H2 + ___Cl2 à ___HCl ________________________

7. ___Al + ___Br2 à ___AlBr3 ________________________

8. ___Zn(OH)2 à ___ZnO + ___H2O ________________________

9. ___HgO à ___Hg + ___O2 ________________________

10. ___Cr + ___O2 à ___Cr2O3 ________________________

11. ___Na + ___I2 à ___NaI ________________________

12. ___Ag2O à ___Ag + ___O2 ________________________

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Balancing Equations

Balance the reactions: Synthesis or Decomposition?

1. ___Cu + ___S8 à ___CuS ________________________

2. ___NaClO3 à ___NaCl + ___O2 ________________________

3. ___MgCO3 à ___MgO + ___CO2 ________________________

4. ___Al2O3 à ___Al + ___O2 ________________________

5. ___Ag + ___S8 à ___Ag2S ________________________

6. ___P + ___O2 à ___P2O5 ________________________

7. ___S8 + ___O2 à ___SO3 ________________________

8. ___H2O à ___H2 + ___O2 ________________________

9. ___CO + ___O2 à ___CO2 ________________________

10. ___H2SO4 à ___H2 + ___SO3 ________________________

11. ___KClO3 à ___KCl + ___O2 ________________________

12. ___AlCl3 à ___Al + ___Cl2 ________________________

13. ___Cu + ___O2 à ___CuO ________________________

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1 Replacement Worksheet-Chem 121

CHEMISTRY REPLACEMENT REACTION WORKSHEET DISCRIPTION During double replacement, the cations and anions of two different compounds switch places. AB + CD -----> AD + CB REACTION GUIDELINE 1. It is important that the formulas of the products be written correctly. If they are correct, balancing the equation is a simple task; if not, the equation will probably never balance. 2. In these reactions, there is never a change in oxidation state (in other words, the charges stay the same). EXAMPLES AgNO3 + NaCl ---> AgCl + NaNO3 Silver nitrate + sodium chloride silver chloride + sodium nitrate Pb(NO3)2 + CuSO4 ---> PbSO4 + Cu(NO3)2 Lead (II) nitrate + copper (II) sulfate lead (II) sulfate + copper (II) nitrate DOUBLE REPLACEMENT PRACTICE REACTIONS For each reaction predict the products and balance the equation. State the reaction in chemical formulas and in symbols. For example: AgNO3 + NaCl --->

Silver nitrate + sodium chloride silver chloride + sodium nitrate AgNO3 + NaCl ---> AgCl + NaNO3

1) Ca(OH)2 + H3PO4 --->

2) K2CO3 + BaCl2 --->

3) Cd3(PO4)2 + (NH4)2S --->

4) Co(OH)3 + HNO3 --->

14. ___Fe + ___O2 à ___Fe2O3 ________________________

Double Replacement Reaction

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2 Replacement Worksheet-Chem 121

5) AgNO3 + KCl --->

6) Na2CO3 + H2SO4 --->

7) Al(OH)3 + HC2H3O2 --->

8) Al2(SO4)3 + Ca3(PO4)2 --->

9) Cr2(SO3)3 + H2SO4 --->

10) AgC2H3O2 + K2CrO4 --->

11) FeBr2 + K2CO3 --->

Single Replacement Reaction Chart

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Activity Series Chart

Metals Non-Metals

Name Symbol Name Symbol

Lithium Li Fluorine F Potassium K Chlorine Cl Barium Ba Bromine Br Strontium Sr Iodine I Calcium Ca

Sodium Na Magnesium Mg Aluminum Al Manganese Mn Zinc ZnIron Fe Cadmium CdCobalt Co Nickel Ni Tin Sn Lead Pb Hydrogen HCopper Cu Silver Ag Mercury HgGold Au

***Elements CANNOT replace anything ABOVE them. The reaction DOES

NOT OCCUR in this situation.***

Least Active

Most Active

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Name:

Single Replacement Reactions Worksheet

A. Predict the products and balance the following single replacement reactions. If no reaction occurs write N.R. For transition metals use the following charges: Iron: Fe3+ Mercury: Hg2+ Lead: Pb4+ Copper: Cu1+ Gold: Au+3

1) Fe + CuCl2 o

2) Hg + Sn(SO4)2 o

3) Ba + Ni3(PO4)2 o

4) Pb + Au(NO3)3 o

5) Li + HOH o

6) K + AgCl o

7) Ca + NaOH o

8) Cu + Fe(OH)3 o

9) Fe + Cu(OH)2 o

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Single Replacement Practice

Name___________________________

1. Ag + K(NO3) à

2. Zn + 2 Ag(NO3) à

3. Al + H2(SO4) à

4. Cl2 + KI à

5. Li + H2O à

6. Cu + Fe(SO4) à

7. Na + H2O à

8. Cu + H2O à

9. Cl2 + NaI à

10. Al + CuCl2 à

11. Br2 + CaI2 à

12. Al + HCl à

13. Cl2 + MgI2 à

14. Fe + Cu(SO4) à

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15. Cl + Cu(SO4) à

Types of Reactions Worksheet

Balance the following equations and indicate the type of reaction taking place: 1) ____ NaBr + ____ H3PO4 à ____ Na3PO4 + ____ HBr

Type of reaction: ____________________

2) ____ Ca(OH)2 + ____ Al2(SO4)3 à ____ CaSO4 + ____ Al(OH)3

Type of reaction: ____________________

3) ____ Mg + ____ Fe2O3 à ____ Fe + ____ MgO

Type of reaction: ____________________

4) ____ C2H4 + ____ O2 à ____ CO2 + ____ H2O

Type of reaction: ____________________

5) ____ PbSO4 à ____ PbSO3 + ____ O2

Type of reaction: ____________________

6) ____ NH3 + ____ I2 à ____ N2I6 + ____ H2

Type of reaction: ____________________

7) ____ H2O + ____ SO3 à ____ H2SO4

Type of reaction: ____________________

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Practice Problems: Balance Equations (add or ∆ coefficients only) 1. ___C ___O2 ___CO2

Type of reaction is ___________________________________ 2. ___NaCl ___F2 ___NaF ___Cl2

Type of reaction is ___________________________________ 3. ___H2 ___F2 ___HF

Type of reaction is ___________________________________ 4. ___C6H12O6 ___C ___H2O

Type of reaction is ___________________________________ 5. ___AgNO3 ___NaCl ___AgCl ___NaNO3

Type of reaction is ___________________________________

8) ____ H2SO4 + ____ NH4OH à ____ H2O + ____ (NH4)2SO4

Type of reaction: ____________________

Reaction Types + Balancing Equations

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Types of Reactions Worksheet Indicate the type of reaction taking place: 1) NaBr + H3PO4 Na3PO4 + HBr Reaction type:____________________________________ 2) Ca(OH)2 + Al2(SO4)3 CaSO4 + Al(OH)3 Reaction type:____________________________________ 3) Mg + Fe2O3 Fe + MgO Reaction type:____________________________________ 4) C2H4 + O2 CO2 + H2O Reaction type:____________________________________ 5) PbSO4 PbSO3 + O2 Reaction type:____________________________________ 6) NH3 + I2 N2I6 + H2 Reaction type:____________________________________ 7) H2O + SO3 H2SO4 Reaction type:____________________________________ 8) O2 + C3H8 H2O + CO2 Reaction type:____________________________________

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9) NaOH + KNO3 --> NaNO3 + KOH

Reaction type:____________________________________

10) CH4 + O2 --> CO2 + H2O Reaction type:____________________________________

11) Fe + NaBr --> FeBr3 + Na Reaction type:____________________________________

12) CaSO4 + Mg(OH)2 --> Ca(OH)2 + MgSO4 Reaction type:____________________________________

13) Na2CO3 --> Na2O + CO2 Reaction type:____________________________________

14) Pb + O2 --> PbO2 Reaction type:____________________________________

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Chemistry I Worksheet 6-2 Name Chemical Reaction Types Period Glencoe pp. 277-279, 284-291 Identify each chemical reaction as a synthesis (combination), decomposition, single-replacement, double-replacement, or combustion reaction. 1. 2SO2 + O2 2SO3

2. Al2(SO4)3 + 3Ca(OH)2 2Al(OH)3 + 3CaSO4

3. 2C2H2 + 5O2 4CO2 + 2H2O

4. Mg + 2AgNO3 Mg(NO3)2 + 2Ag

5. 3Ba(NO3)2 + 2H3PO4 Ba3(PO4)2 + 6HNO3

6. Mg(ClO3)2 MgCl2 + 3O2

7. 2Be + O2 2BeO

8. 2Al + 3CuSO4 Al2(SO4)3 + 3Cu

9. 2PbO2 2PbO + O2

10. 2C2H6 + 7O2 4CO2 + 6H2O

Complete the chemical equations for the following SYNTHESIS (COMBINATION) reactions. 11. Mg + O2

12. Ca + S

13. Na + O2

14. Na + Cl2

15. Al + O2

Use the activity series of metals to complete the following SINGLE-REPLACEMENT reactions. Write “NR” if there is no reaction. 16. Zn(s) + AgNO3

17. Au(s) + KNO3

18. Al(s) + H2SO4

19. Cu(s) + H2O

20. Al(s) + CuSO4

Write the chemical equation for the complete COMBUSTION of the following compounds. 21. octane (C8H18) C8H18 + +

22. glucose (C6H12O6) C6H12O6 + +

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Chemistry I Complete the chemical equations for the following DOUBLE-REPLACEMENT reactions. 23. Ag2SO4 + AlCl3

24. CdBr2 + Na2S

25. Pb(NO3)2 + NaI

26. NaOH + Fe(NO3)3

27. NaNO3 + BaCl2

Write the type of reaction on the line. Then, predict the products of each reaction to complete the chemical equation. Write the correct formulas of the products after the arrow. Write “NR” if there is no reaction. 28. Ag2O

29. C4H8 + O2

30. Al + N2

31. Zn + CuSO4

32. Pb(NO3)2 + K2CrO4

33. Li + O2

34. Al2(SO4)3 + Ba(OH)2

35. Cu + CaCO3

36. C3H6 + O2

37. Na3PO4 + Pb(NO3)2

Write the chemical equation for the following reactions. Remember the diatomics. Use appropriate state symbols . 38. Solid silver carbonate decomposes into solid silver oxide and gaseous carbon dioxide when

heated. 39. Adding chlorine gas to a solution of potassium iodide gives solid iodine and a solution of

potassium chloride. 40. Iodine crystals react with chlorine gas to form solid iodine trichloride.

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WebQuest!!

http://questgarden.com/06/98/4/051031220120/index.htm -Get into your pre-assigned groups for this project. -Go to the link listed above. -First: read the introduction -Second: read the task -Third: read the process etc…. -Your lesson should be at least 20 minutes, but no more than 30 minutes!

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Chemical Formula Writing Worksheet Two Write chemical formulas for the compounds in each box. The names are found by finding the intersection between the cations and anions. Example: The first box is the intersection between the “zinc” cation and the “chloride” anion, so you should write “ZnCl2”, as shown. Cations Anions zinc iron (II) iron (III) gallium silver lead (IV) chloride ZnCl2 acetate nitrate oxide nitride sulfate

Write the formulas for the following compounds: 1) copper (II) chloride ____________________________________ 2) lithium acetate ____________________________________ 3) vanadium (III) selenide ____________________________________ 4) manganese (IV) nitride ____________________________________ 5) beryllium oxide ____________________________________ 6) sodium sulfate ____________________________________ 7) aluminum arsenide ____________________________________ 8) potassium permanganate ____________________________________ 9) chromium (VI) cyanide ____________________________________ 10) tin (II) sulfite ____________________________________ 11) vanadium (V) fluoride ____________________________________ 12) ammonium nitrate ____________________________________

Formula Writing Refresher

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reacts

formed

Writing Word Equations

1. You will combine formula writing, reaction type, and balancing equation to create an appropriate chemical reaction from each of the word equations provided.

Diatomic Molecules- molecules that naturally occur in pairs, and they are:

H2, N2, O2, F2, Cl2, Br2, I2 EX: When sodium reacts with iron (II) chloride, iron and sodium chloride are formed. 1. Break the sentence down: When sodium with iron (II) chloride, iron and sodium chloride are

2. Write out the reactant and product formulas. Reactants, reacts: Sodium (Na), Iron (II) Chloride (FeCl2) Products, formed: Iron (Fe), Sodium Chloride (NaCl) 3. Put it all together: Na + FeCl2 à Fe + NaCl 4. Make sure everything is balanced!! Na + FeCl2 à Fe + NaCl Na: 1 Na: 1 Fe: 1 Fe: 1 Cl: 2 Cl: 1 SO…… our final reaction: 2 Na + FeCl2 à Fe + 2 NaCl

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Writing the Complete Equation HomeworkWrite the complete chemical equation for each of the following chemicalreactions:

1) When iron solid is placed in liquid lithium sulfate and electricity is added toit, iron (II) sulfate crystals and solid lithium metal are formed.

2) When the ethanol (C2H6O) in some gasoline burns with oxygen gas in anautomobile engine, it forms carbon dioxide gas and water vapor.

3) When the pressure on an aqueous solution of carbonic acid is decreasedto 0.1 atmospheres, it decomposes to form carbon dioxide gas and water.

4) When iodine gas reacts with methane gas at very high temperatures, CH3Igas and hydrogen iodide gas are formed.

5) When dinitrogen hexaiodide crystals are hit with a hammer, theyspontaneously and explosively decompose to form nitrogen gas andiodine powder.

6) When hydrochloric acid gas reacts with gaseous ammonia, water vaporand solid ammonium chloride are formed.

36 WKS001x020 © 2000 Cavalcade Publishing (http://www.cavalcadepublishing.com) All Rights Reserved

Word EquationsWrite the word equations below as chemical equations and balance:

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

_______________________________________________________________2) Aluminum bromide and chlorine gas react to form aluminum chloride and

bromine gas.

_______________________________________________________________3) Sodium phosphate and calcium chloride react to form calcium phosphate

and sodium chloride.

_______________________________________________________________4) Potassium metal and chlorine gas combine to form potassium chloride.

_______________________________________________________________5) Aluminum and hydrochloric acid react to form aluminum chloride and

hydrogen gas.

_______________________________________________________________6) Calcium hydroxide and phosphoric acid react to form calcium phosphate

and water.

_______________________________________________________________7) Copper and sulfuric acid react to form copper (II) sulfate and water and

sulfur dioxide.

_______________________________________________________________8) Hydrogen gas and nitrogen monoxide react to form water and nitrogen

gas.

37

Word Equations Problems Write out the following chemical equations, be sure to balance the equations.

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

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

3. Sodium phosphate and calcium chloride react to form calcium phosphate and sodium chloride.

4. Potassium metal and chlorine gas combine to form potassium chloride.

38

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

6. Calcium hydroxide and phosphoric acid (HPO4) react to form calcium phosphate and water.

7. Copper and sulfuric acid (H2SO4) react to form copper (II) sulfate and water and sulfur dioxide.

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

39

Activity Series Chart

Metals Non-Metals

Name Symbol Name Symbol

Lithium Li Fluorine F Potassium K Chlorine Cl Barium Ba Bromine Br Strontium Sr Iodine I Calcium Ca

Sodium Na Magnesium Mg Aluminum Al Manganese Mn Zinc ZnIron Fe Cadmium CdCobalt Co Nickel Ni Tin Sn Lead Pb Hydrogen HCopper Cu Silver Ag Mercury HgGold Au

***Elements CANNOT replace anything ABOVE them. The reaction DOES

NOT OCCUR in this situation.***

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