NOTES: CHEMICAL REACTIONS - Livingston



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|UNIT 4: Chemical Reactions – Stoichiometry and Thermodynamics |

|Part A: Chemical Reactions |

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|Big Picture Ideas: |

|The identity of the reactants helps scientists to predict the products in a chemical reaction. |

|Quantitative relationships exist with all chemical reactions that allow scientists to predict amounts of products formed, reactants consumed, |

|and percent yield based on theoretical maximum. |

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|Big Picture Question: How can you predict the products in a chemical reaction? |

|Suggested Resources… |

|Homework Assignments |

|Classwork Assignments |

|Laboratory Activities |

|Formative Assessments |

|Textbook pages: Chapter 9 |

|Websites: |

|Key Terms: |

|chemical reaction |

|chemical equation |

|reactants |

|yields |

|products |

|coefficient/mole |

|subscript |

|diatomic molecules |

|synthesis/direct combination |

|decomposition |

|single replacement/displacement |

|double replacement/displacement |

|combustion |

|activity series |

|aqueous |

|kinetics |

|catalyst |

|surface area |

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|Directions: Use this information as a general reference tool to guide you through this unit. Don’t hesitate to ask your teacher for help! |

|By the conclusion of this unit, you should know the following: |By the conclusion of this unit, you should be able to do the following: |

|There are five basic types of chemical reactions (S, D, SR, DR, Comb.)|Balance chemical reactions. |

|that exhibit distinct patterns for the prediction of products. |Identify type of chemical reaction. |

|Experimental evidence can be used to identify products in a reaction. |Identify if a reaction will occur using an activity series. |

|All reactions follow the Law of Conservation of Matter (balancing |Predict products for a reaction. |

|equations). |Write balance formula equation given chemical equation (words). |

|Symbols are used to identify different aspects of a chemical reaction |Using the collision theory, explain how altering the temperature, surface |

|(states of matter, catalysts, heat, etc.). |area, concentration and the addition of a catalyst affects the rate of a |

|Collision theory describes characteristics for a successful reaction. |reaction. |

|Factors can be altered to affect the rate of a reaction (temperature, |Draw an energy diagram for both endothermic and exothermic reactions. |

|surface area, catalyst, concentration). | |

1. What type of reaction is it?

a. element + element (

b. ionic compound + ionic compound (

c. element + ionic compound (

d. compound (

e. compound + oxygen (

2. How can you tell if a chemical change has taken place? List examples.

3. Define a chemical reaction. Why must we balance chemical equations? (if it is a “must” there must be a “law” governing the concept).

4. Balance each reaction below. Identify each type the following reactions are:

a)  NaOH(aq) + Pb(NO3)2(aq) --> NaNO3(aq) + Pb(OH)2(s)

b)  CH4(g) + O2(g) --> CO2(g) + H2O(l)

c)  Fe(s) + NaBr(aq) --> FeBr3(aq) + Na(s)

d)  Pb(s) + O2(g) --> PbO (g)

e)  Na2CO3(s) --> Na2O(s) + CO2(g)

5. Complete and balance each reaction below:

a) Mg + HCl ( _________ + ____________

b) C2H6 + O2 ( _________ + ____________

c) CaF2 + Na2SO4 ( _________ + ____________

d) Sr + N2 ( __________

6. List three factors effecting the rate of a chemical reaction. Know why they effect the reaction rate (collision theory!)

7. Describe the standard test for hydrogen, oxygen and carbon dioxide

NOTES: CHEMICAL REACTIONS

VOCABULARY:

Products result after reaction occurs

Reactants starting substances in a reaction

(”yields”

+ and

(s) solid

(l) liquid

(g) gas

(aq) aqueous – substance dissolved in water

Catalyst speads up a reaction by lowering activation energy

Activation Energy (Ea) starting amount of energy

ENERGY OF CHEMICAL REACTIONS:

Exothermic Reaction: ΔH is – Endothermic Reaction: ΔH = +

(heat is a “product”) (heat is a “reactant”)

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KINETICS: RATE OF CHEMICAL REACTIONS

Collision Theory: reactants must collide with (1) at least the activation energy and with (2) the correct orientation

Factors Effecting Reaction Rate:

Temperature quicker particles collide with energy and they collide more often (due to the high temperature)

Particle size (surface area) more surface area = more collisions = faster rate

Mixing/Stirring creates more surface area = more collisions = faster rate

Nature of Reaction how reactive the particles are

Adding a Catalyst or Inhibitor catalyst – speeds up the reaction by lowering the activation energy; inhibitor – slows down reactions by preventing correct collisions

BALANCED CHEMICAL REACTIONS

Law of Conservation of Matter: matter cannot be created or destroyed (number of atoms of each element need to be the same on each side of the equation)

Try balancing these chemical reactions:**subscripts are used to write formulas**coefficients are used to balance**

a. 2 Na + H2SO4 ( Na2SO4 + H2

b. 2 K + Cl2 ( 2 KCl

c. S8 + 8 O2 ( 8 SO2

d. 3F2 + 2 FeBr3 ( 2 FeF3 + 3Br2

e. 3H2SO4 + 2 Al ( Al2(SO4)3 + 3H2

f. 2 C2H6 + 7 O2 ( 4CO2 + 6H2O

g. 2 NaNO3 + Ca(MnO4)2 ( 2 NaMnO4 + Ca(NO3)2

h. 3 P4 + 10 KClO3 ( 10 KCl + 6 P2O5

WORD ( FORMULA ( BALANCED EQUATIONS

word equation: Hydrogen gas reacts with oxygen gas to form water

formula equation: ______ H2 + O2 ( H2O _________________________________________

diagram:

balanced reaction ________2 H2 + O2 ( 2 H2O _______________________________________

word equation: Magnesium reacts with hydrochloric acid solution (HCl in water) to form

magnesium chloride and hydrogen.

Formula equation: _______ Mg + HCl ( MgCl2 + H2 __________________________

diagram:

balanced reaction _______ Mg + 2 HCl ( MgCl2 + H2 ________________________

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SYNTHESIS, DECOMPOSITION AND COMBUSTION REACTIONS

Types of Reactions: Synthesis, Decomposition and Combustion

Synthesis – A + B ( AB (1 product only)

Combination reaction (2 or more substances combine to form 1 product)

1 substance to the right of the (

Decomposition – AB ( A + B (1 reactant only)

Breaking 1 substance down

Combustion of a hydrocarbon – CxHy + O2 ( CO2 + H2O

Hydrocarbon reacting with oxygen

Exothermic (burning releases heat)

Practice:

Balance each reaction below. Then identify the reaction type.

a. H2 + Br2 ( 2 HBr ____synthesis_____________

b. C4H8 + 6 O2 ( 4 CO2 + 4 H2O ___combustion____________

c. 2 NaOH ( Na2O + H2O _____decomposition_________

d. Ba(ClO3)2 ( BaCl2 + 3 O2 ____decomposition_________

HOMEWORK: BALANCING CHEMICAL REACTIONS NAME:

DATE:

1. ___P4 + _5__O2 ( _2__P2O5

2. _2__Al + _6__HCl ( _2__AlCl3 + _3__H2

3. ___Al2(SO4)3 + _3__Ca(OH)2 ( _2__Al(OH)3 + _3__CaSO4

4. _8__H2S + _8__Cl2 ( ___S8 + _16__HCl

5. _3___Mg + ____N2 ( ____Mg3N2

6. _3___Fe + _4___H2O ( ____Fe3O4 + _4___H2

7. _2___NaOH + ____Cl2 ( ____NaCl + ____NaClO + ____H2O

8. _2___C4H10 + _13___O2 ( _8___CO2 + _10___H2O

9. __2___CH3OH + __3___O2 ( _2___CO2 + __4___ H2O

HOMEWORK: SYNTHESIS, DECOMPOSITION AND COMBUSTION REACTIONS

1. Classify each equation below as synthesis, decomposition or combustion. Then balance each equation.

__decomposition______________________ 1. 2 NaClO3 ( 2 NaCl + 3 O2

___synthesis_____________________ 2. 2 Cu + S ( Cu2S

___synthesis_____________________ 3. 2 S + 3 O2 ( 2 SO3

___combustion____________________ 4. 2 C3H6 + 9 O2 ( 6 CO2 + 6 H2O

2. Classify each equation below as synthesis, decomposition or combustion. Write and balance the equation for the reaction.

___decomposition_________ 1. potassium hydroxide ( potassium oxide + hydrogen water

2 KOH ( K2O + H2O

___combustion___________ 2. dicarbon tetrahydride + oxygen ( carbon dioxide + water

C2H4 + 3 O2 ( 2 CO2 + 2 H2O

___decomposition________ 3. lithium chlorate ( lithium chloride + oxygen

2 LiClO3 ( 2 LiCl + 3 O2

____synthesis_____________ 4. magnesium + nitrogen ( magnesium nitride

3 Mg + N2 ( Mg3N2

___synthesis______________ 5. aluminum burns in pure oxygen to form aluminum oxide

4 Al + 3 O2 ( 2 Al2O3

____decomposition________ 6. sodium carbonate is heated to form sodium oxide and carbon dioxide

Na2CO3 ( Na2O + CO2

___synthesis_______________ 7. water and dinitrogen pentoxide combine to form nitric acid

H2O + N2O5 ( 2 HNO3

First write and then balance the equation. Then identify the reaction type.

e. phosphorus + oxygen ( tetraphosphorus decoxide

4 P + 5 O2 ( P4O10 synthesis

f. pentane (C5H12) + oxygen ( carbon dioxide + water

C5H12 + 8 O2 ( 5 CO2 + 6 H2O combustion

g. magnesium chlorate ( magnesium chloride + oxygen

Mg(ClO3)2 ( MgCl2 + 3 O2 decomposition

h. when solid calcium carbonate is heated calcium oxide and carbon dioxide are formed

CaCO3 ( CaO + CO2 decomposition

i. the formation of calcium nitride from calcium and nitrogen

3 Ca + N2 ( Ca3N2 synthesis

j. sulfur trioxide mixes with water in the atmosphere to form sulfuric acid

SO3 + H2O ( H2SO4 synthesis

NOTES: SINGLE DISPLACEMENT REACTIONS & DOUBLE DISPLACEMENT REACTIONS

1. Single Displacement Reactions (aqueous ONLY) element + compound

metals:

standard: A + BC ( B + AC

example: Cu + 2 AgNO3 ( Ag + Cu(NO3)2

metal + acid:

standard: A + HC ( H2 + AC

example: Zn + H2SO4 ( H2 + ZnSO4

metal + water: **replace metal with only 1 hydrogen in water!

standard: A + HOH ( H2 + AOH

example: 2 Na + 2 HOH ( H2 + 2 NaOH

halogens:

standard: A + BC ( C + BA

example: F2 + 2 NaCl ( Cl2 + 2 NaF

2. Double Displacement (aqueous only) ion exchange reaction : compound + compound

standard : AB + CD ( AD + CB

example : NaCl + AgNO3 ( NaNO3 + AgCl

3. Identify the reaction type for each reaction below. Then complete and balance the reaction.

_single displacement_ a. Ba + 2 AgNO3 ( Ba(NO3)2 + 2Ag

__single displacement________b. F2 + 2KI ( 2 KF + I2

double displacement c. NaOH + CaCl2 ( _2 NaCl + Ca(OH)2

___single displacement d. Zn + H2SO4 ( ZnSO4 + H2

WRITING WORD EQUATIONS

__decomposition_______________1. aluminum chlorate ( aluminum chloride + oxygen

2 Al(ClO3)3 ( 9 O2 + 2 AlCl3

__SR_______________ 2. lithium + iron (III) nitrate ( lithium nitrate + iron

3 Li + Fe(NO3)3 ( 3 LiNO3 + Fe

__decomposition_______________ 3. magnesium carbonate ( magnesium oxide + carbon dioxide

MgCO3 ( MgO + CO2

__synthesis____________ 4. tin + nitrogen ( tin (IV) nitride

3 Sn + 2 N2 ( Sn3N4

__SR____________ 5. Zinc reacts with nitric acid to form zinc nitrate and hydrogen

Zn + 2 HNO3 ( Zn(NO3)2 + H2

__decomposition__________6. calcium hydroxide breaks down to form calcium oxide and water

Ca(OH)2 ( CaO + H2O

WRITING WORD EQUATIONS WITH PREDICTING PRODUCTS

__synthesis_______________ 1. aluminum + oxygen (

4 Al + 3 O2 ( 2 Al2O3

__SR____________ 2. sodium + silver nitrate (

Na + AgNO3 ( NaNO3 + Ag

__SR_______________ 3. magnesium + hydrochloric acid (

2 Mg + 2 HCl ( 2 MgCl + H2

___DR______________ 4. solutions of iron (III) nitrate + potassium sulfate are mixed (

2 Fe(NO3)3 + 3 K2(SO4)3 ( Fe2(SO4)3 + 6 KNO3

____SR_____________ 5. Chlorine gas is bubbled through a solution of lithium iodide (

Cl2 + 2 LiI ( 2 LiCl + I2

Fun With Predicting Reaction Products

Predict the products of each of the following chemical reactions. If a reaction will not occur, explain why not:

1) ____ Ag2SO4 + __2__ NaNO3 ( 2 AgNO3 + Na2SO4

2) __2__ NaI + ____ CaSO4 ( CaI2 + Na2SO4

3) __2__ HNO3 + ____ Ca(OH)2 ( 2 H2O + Ca(NO3)2

4) ____ Zn + ___2__ HNO3 ( Zn(NO3)2 + H2

5) ____ AlCl3 + ____ (NH4)3PO4 ( AlPO4 + 3 NH4Cl

6) ___3_ Pb + ___2_ Fe(NO3)3 ( 3 Pb(NO3)2 + 2 Fe

7) ___2_ C3H6 + __9__ O2 ( 6 CO2 + 6 H2O

8) __2__ Na + ____ CaSO4 ( Na2SO4 + Ca

CLASSIFICATION OF CHEMICAL REACTIONS

Classify the reactions below as sythesis, decomposition, single replacement or double replacement:

1. 2H2 + O2 ( 2H2O ____synthesis______________________

2. 2H2O ( 2H2 + O2 ____decomposition________________

3. Zn + H2SO4 ( ZnSO4 + H2 ____SR______________________

4. 2CO + O2 ( 2CO2 _____synthesis_____________________

5. 2HgO ( 2Hg + O2 ____decomposition__________________

6. 2 KBr + Cl2 ( 2 KCl + Br2 ____SR______________________

7. CaO + H2O ( Ca(OH)2 ____synthesis______________________

8. AgNO3 + NaCl ( AgCl + NaNO3 ____DR______________________

9. 2 H2O2 ( 2H2O + O2 ____decomposition________________

10. Ca(OH)2 + H2SO4 ( CaSO4 + 2H2O _____DR_____________________

11. Copper metal is put into a solution of silver nitrate. Solid silver precipitates, and copper (II) nitrate solution is formed.

___SR________________________

12. Methane gas burns in pure oxygen to give carbon dioxide and water

___combustion_________

13. When sodium carbonate is heated, it breaks down to form sodium oxide and carbon dioxide. ___decomposition________

WRITING WORD EQUATIONS

a. lithium + nitrogen ( lithium nitride

6 Li + N2 ( 2 Li3N

b. aluminum + oxygen ( aluminum oxide

4 Al + 3 O2 ( 2 Al2O3

c. sodium carbonate ( sodium oxide + carbon dioxide

Na2CO3 ( Na2O + CO2

d. zinc + phosphoric acid ( zinc phosphate + hydrogen gas

3 Zn + 2 H3PO4 ( Zn3(PO4)2 + 3 H2

e. chlorine gas + lithium iodide ( lithium chloride + iodine

Cl2 + 2 LiI ( 2 LiCl + I2

f. sodium hydroxide ( sodium oxide + water

2 NaOH ( Na2O + H2O

g. magnesium reacts with hydrochloric acid to form magnesium chloride and hydrogen gas

Mg + 2 HCl ( MgCl2 + H2

h. solutions of iron (III) chloride and sodium hydroxide react to form iron (III) hydroxide and sodium chloride

FeCl3 + 3 NaOH ( Fe(OH)3 + 3 NaCl

i. when sodium is added to water, sodium hydroxide and hydrogen gas are produced\

2 Na + 2 H2O ( 2NaOH + H2

j. when zinc is placed in a solution of lead (II) nitrate, zinc nitrate and solid lead metal are formed

Zn + Pb(NO3)2 ( Zn(NO3)2 + Pb

HOMEWORK – PRACTICE REACTION WRITING

Identify the reaction type for each reaction written below. Then write the balanced equation for each reaction.

____single displacement___ 1. Magnesium is placed in a solution of aluminum nitrate

3 Mg + 2 Al(NO3)3 (3 Mg(NO3)2 + 2 Al

_______synthesis________________ 2. Calcium burns in pure oxygen.

2 Ca + O2 ( 2CaO

____combustion hydrocarbon_____ 3. The combustion of propane (C3H8)

__________C3H8 + 5 O2 ( 3 CO2 + 4 H2O_________________

____single displacement_____ 4. Fluorine is bubble through a solution of sodium bromide

__________F2 + 2 NaBr ( 2 NaF + Br2 _______________________________________

___double displacement______ 5. Solutions of potassium chloride and barium hydroxide are mixed.

_____2 KCl + Ba(OH)2 ( 2 KOH + BaCl2 ______________________________

REACTION WRITING PRACTICE NAME:

1. Ammonium Dichromate Volcano:



Observations:

Reaction:

Type:

2. Zinc and Sulfur:



Observations:

Reaction:

Type:

3. Aluminum and copper(II) chloride (demonstration)

Observations:

Reaction:

Type:

4. Lead (II) Nitrate and Potassium Iodide: (demonstration)

Observations:

Reaction:

Type:

5. Sodium and chlorine:



Observations:

Reaction:

Type:

6. Hindenburgh Explosion:



Observations:

Reaction:

Type:

7. Thermite



Observations:

Reaction:

Type:

8. Magnesium and carbon dioxide



Observations:

Reaction:

Type:

9. Burning magnesium and water



Observations:

Reaction:

Type:

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