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. |
| |
|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 |
| |
|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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