what is the difference between a chemical reaction and physical change?
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What is the difference between a chemical reaction and physical change? When you watch a reaction occur, what are some hints that it is a chemical reaction?. Ch. 11 Chemical Equations Reactions. Describing Chemical Reactions. Objectives. - PowerPoint PPT PresentationTRANSCRIPT
What is the difference between a What is the difference between a chemical reaction and physical chemical reaction and physical change?change?
When you watch a reaction When you watch a reaction occur, what are some hints that occur, what are some hints that it is a chemical reaction?it is a chemical reaction?
Ch. 11 Chemical Ch. 11 Chemical Equations ReactionsEquations Reactions
Describing Chemical Describing Chemical ReactionsReactions
ObjectivesObjectives
List three observations that suggest List three observations that suggest that a chemical reaction has taken that a chemical reaction has taken place.place.
List three requirements for a List three requirements for a correctly written chemical equation.correctly written chemical equation.
Write a word equation and a formula Write a word equation and a formula equation for a given reaction.equation for a given reaction.
Balance a formula equation by Balance a formula equation by inspection.inspection.
Chemical ReactionsChemical Reactions
when a substance when a substance changes identitychanges identity reactants- originalreactants- original products- resultingproducts- resulting
law of conservation law of conservation of massof mass total mass of reactants total mass of reactants
= total mass of products= total mass of products
Chemical ReactionsChemical Reactions
chemical equationchemical equation represents identities and relative represents identities and relative
amounts of reactants and products in amounts of reactants and products in the chemical reactionthe chemical reaction
uses symbols and formulasuses symbols and formulas
Hints of Chemical RxnHints of Chemical Rxn
heat or lightheat or light can also happen with can also happen with
physical changesphysical changes gas bubblesgas bubbles
means a gas is being means a gas is being created as productcreated as product
precipitateprecipitate solid is being createdsolid is being created
color changecolor change
Writing Chemical EquationsWriting Chemical Equations
most pure elementsmost pure elements written as elemental symbolwritten as elemental symbol
diatomic moleculesdiatomic molecules molecule containing only 2 molecule containing only 2
atomsatoms some elements normally exist some elements normally exist
this waythis way HH22, O, O22, N, N22, F, F22, Cl, Cl22, Br, Br22, I, I22
other exceptionsother exceptions
• sulfur: Ssulfur: S88
• phosphorus: Pphosphorus: P44
Word EquationsWord Equations
uses names instead of formulasuses names instead of formulas helps you to write formula equationhelps you to write formula equation
ExampleExample
Description:Description:
Solid sodium oxide is added to water Solid sodium oxide is added to water at room temperature and forms at room temperature and forms sodium hydroxide.sodium hydroxide.
Word Equation:Word Equation:sodium oxide + water sodium oxide + water sodium hydroxide sodium hydroxide
Formula Equation:Formula Equation:
NaNa22O + HO + H22O O NaOH NaOH
Symbols Used in EquationsSymbols Used in Equations
yieldsyields
reversible reversible
above arrow:above arrow:
oror heat heat heatedheated
MnOMnO22 or or PtPt catalystcatalyst
25°C25°C specific T specific T requirementrequirement
2 atm2 atm specific P specific P requirementrequirement
after a after a formula:formula:
(s)(s) solidsolid
(l)(l)liquidliquid
(aq)(aq) aqueous: aqueous: dissolved dissolved
in in waterwater
(g)(g) gasgas
Text Pg. 323 Chart of Text Pg. 323 Chart of symbols used in symbols used in chemical equationschemical equations
List three observations that suggest List three observations that suggest that a chemical reaction has taken that a chemical reaction has taken place.place.
Acids you have to know!Acids you have to know!
HCl hydrochloric acidHCl hydrochloric acidHH22SOSO44 sulfuric acid sulfuric acid
HNOHNO33 nitric acid nitric acid
HH33POPO44 phosphoric acid phosphoric acid
HCHC22HH33OO22 acetic acid acetic acid
Write the chemical equation Write the chemical equation from the following description:from the following description:Zinc metal is added to hydrochloric Zinc metal is added to hydrochloric acid to create zinc chloride and acid to create zinc chloride and hydrogen gas. hydrogen gas.
Aluminum reacts with Aluminum reacts with oxygen to produce oxygen to produce
aluminum oxidealuminum oxide
A.A. Al + O Al + O Al Al22OO33
B.B. Al + OAl + O22 Al Al22OO33
C.C. AlAl33 + O + O Al Al22OO33
Aluminum reacts with Aluminum reacts with oxygen to produce oxygen to produce
aluminum oxidealuminum oxide
A.A. Al + O Al + O Al Al22OO33
B.B. Al + OAl + O22 Al Al22OO33
C.C. AlAl33 + O + O Al Al22OO33
Phosphoric acid is produced Phosphoric acid is produced through the reaction through the reaction
between tetraphosphorus between tetraphosphorus decoxide and waterdecoxide and water
A.A. HH33POPO44 P P44 + H + H22OOB.B. HH33POPO4 4 + H+ H22O O P P44
C.C. PP44OO10 10 + H+ H22O O H H33POPO44
Phosphoric acid is produced Phosphoric acid is produced through the reaction through the reaction
between tetraphosphorus between tetraphosphorus decoxide and waterdecoxide and water
A.A. HH33POPO44 P P44 + H + H22OOB.B. HH33POPO4 4 + H+ H22O O P P44
C.C. PP44OO10 10 + H+ H22O O H H33POPO44
Iron(III)oxide reacts with Iron(III)oxide reacts with carbon monoxide to carbon monoxide to
produce iron and carbon produce iron and carbon dioxidedioxide
A.A. FeO + CO FeO + CO Fe + CO Fe + CO22
B.B. FeFe22OO33 + CO + CO Fe + CO Fe + CO22
C.C. Fe + COFe + CO Fe Fe22OO33 + CO + CO22
Iron(III)oxide reacts with Iron(III)oxide reacts with carbon monoxide to carbon monoxide to
produce iron and carbon produce iron and carbon dioxidedioxide
A.A. FeO + CO FeO + CO Fe + CO Fe + CO22
B.B. FeFe22OO33 + CO + CO Fe + CO Fe + CO22
C.C. Fe + COFe + CO Fe Fe22OO33 + CO + CO22
CoefficientsCoefficients
whole numbers in front of formulawhole numbers in front of formula distributes to numbers of atoms in distributes to numbers of atoms in
formulaformula specifies the relative number of moles specifies the relative number of moles
and molecules involved in the reactionand molecules involved in the reaction used to balance the equationused to balance the equation
Balancing EquationsBalancing Equations ONLY add/change coefficients- ONLY add/change coefficients-
NEVER subscripts!!!NEVER subscripts!!!
1.1. balance one type of atom at a timebalance one type of atom at a time
2.2. balance polyatomic ions firstbalance polyatomic ions first
3.3. balance atoms that appear only balance atoms that appear only once secondonce second
4.4. balance H and O lastbalance H and O last
5.5. simplify if you cansimplify if you can
6.6. Check at end!Check at end!
Rules for writing and Rules for writing and balancing equations – balancing equations – Pg. 327 in text.Pg. 327 in text.
Writing EquationsWriting Equations Write Word equations to help you Write Word equations to help you
organize reactants and productsorganize reactants and products Be sure to include symbols showing Be sure to include symbols showing
states of each reactant and productstates of each reactant and product Be sure to write the correct formula Be sure to write the correct formula
for each (crossing over for ionic for each (crossing over for ionic compounds!)compounds!)
Check your balancing of the Check your balancing of the equation when you are finishedequation when you are finished
Example 1Example 1
Description:Description: Aqueous iron III oxide reacts with Aqueous iron III oxide reacts with
hydrogen gas to produce iron metal hydrogen gas to produce iron metal and liquid waterand liquid water
Word Equation:Word Equation:
Iron III oxide + hydrogen gas Iron III oxide + hydrogen gas
iron + wateriron + water
Example 1Example 1
Formula Equation:Formula Equation:
FeFe22OO3 3 (aq) (aq) + H+ H22 (g)(g) Fe Fe (s)(s) + H + H22O O
(l)(l)
Balanced Formula EquationBalanced Formula Equation
FeFe22OO33 (aq) (aq) + 3H+ 3H22 (g)(g) 2Fe 2Fe (s)(s) + 3H + 3H22O O (l)(l)
Example 2Example 2
Solid calcium metal reacts with water Solid calcium metal reacts with water to form aqueous calcium hydroxide to form aqueous calcium hydroxide and hydrogen gas.and hydrogen gas.
calcium + water calcium + water
calcium hydroxide + calcium hydroxide + hydrogenhydrogen
CaCa(s)(s) + H + H22OO(l)(l) Ca(OH) Ca(OH)2(aq)2(aq) + H + H2(g)2(g)
CaCa(s)(s) + 2H + 2H22OO(l)(l) Ca(OH) Ca(OH)2(aq) 2(aq) + H+ H2(g)2(g)
Example 3Example 3
solid zinc metal reacts with aqueous solid zinc metal reacts with aqueous copper (II) sulfate to produce solid copper (II) sulfate to produce solid copper metal and aqueous zinc sulfatecopper metal and aqueous zinc sulfate
zinc + copper (II) sulfate zinc + copper (II) sulfate
copper + zinc sulfatecopper + zinc sulfate ZnZn(s)(s) + CuSO + CuSO4 4 (aq) (aq) Cu Cu (s)(s) + ZnSO + ZnSO4 4 (aq)(aq)
ZnZn(s)(s) + CuSO + CuSO4 4 (aq) (aq) Cu Cu(s)(s) + ZnSO + ZnSO4 4 (aq)(aq)
Example 4Example 4
Hydrogen peroxide in an Hydrogen peroxide in an aqueous solution aqueous solution decomposes to produce decomposes to produce oxygen and wateroxygen and water
hydrogen peroxide hydrogen peroxide oxygen + wateroxygen + water
HH22OO2 (aq) 2 (aq) O O2 (g)2 (g) + H + H22O O (l)(l)
2H2H22OO2 (aq) 2 (aq) O O2 (g)2 (g) + 2H + 2H22O O (l)(l)
Example 5Example 5
Solid copper metal reacts with Solid copper metal reacts with aqueous silver nitrate to produce aqueous silver nitrate to produce solid silver metal and aqueous solid silver metal and aqueous copper (II) nitratecopper (II) nitrate
copper + silver nitrate copper + silver nitrate silver + copper (II) silver + copper (II)
nitratenitrate Cu Cu (s)(s) + AgNO + AgNO3 (aq) 3 (aq) Ag Ag (s)(s) + Cu(NO + Cu(NO33))2 (aq)2 (aq)
Cu Cu (s)(s) + 2AgNO + 2AgNO3 (aq) 3 (aq) 2Ag 2Ag (s)(s) + Cu(NO + Cu(NO33))2 (aq)2 (aq)
Example 6Example 6
Carbon dioxide gas is bubbled through Carbon dioxide gas is bubbled through water containing solid barium carbonate, water containing solid barium carbonate, creating aqueous barium bicarbonatecreating aqueous barium bicarbonate
carbon dioxide + water + barium carbon dioxide + water + barium carbonate carbonate barium bicarbonate barium bicarbonate
COCO2 (g)2 (g) + H + H22O O (l)(l) + BaCO + BaCO3 (s)3 (s) Ba(HCO Ba(HCO33))2 2 (aq)(aq)
COCO2 (g)2 (g) + H + H22O O (l)(l) + BaCO + BaCO3 (s)3 (s) Ba(HCO Ba(HCO33))2 2 (aq)(aq)
Example 7Example 7 Acetic acid solution is added to a solution of Acetic acid solution is added to a solution of
magnesium bicarbonate to create water, magnesium bicarbonate to create water, carbon dioxide gas, and aqueous carbon dioxide gas, and aqueous magnesium acetate.magnesium acetate.
acetic acid + magnesium bicarbonate acetic acid + magnesium bicarbonate water + carbon dioxide + magnesium acetatewater + carbon dioxide + magnesium acetate HCHHCH33COO COO (aq) (aq) + Mg(HCO+ Mg(HCO33))2 2 (aq) (aq)
HH22OO(l)(l) + CO + CO2 (g)2 (g) + Mg(CH + Mg(CH33COO)COO)2 2 (aq)(aq)
2HCH2HCH33COO COO (aq) (aq) + Mg(HCO+ Mg(HCO33))2 (aq) 2 (aq)
2H2H22OO(l)(l) + 2CO + 2CO2 2 (g)(g) + Mg(CH + Mg(CH33COO)COO)2 2 (aq)(aq)
Write the Write the balancedbalanced formula equation formula equation for:for:
Lithium metal is added to a solution Lithium metal is added to a solution of aluminum sulfate to make of aluminum sulfate to make aqueous lithium sulfate and aqueous lithium sulfate and aluminum metal.aluminum metal.
Types of Chemical Types of Chemical ReactionsReactions
Types of Chemical Types of Chemical ReactionsReactions
5 basic types discussed here5 basic types discussed here not all reactions fall in these not all reactions fall in these
categoriescategories you should be able to:you should be able to:
categorize a reaction categorize a reaction predict the product(s)predict the product(s)
1. Synthesis1. Synthesis
also called combination reactionalso called combination reaction reactants:reactants:
more than onemore than one can be elements or compoundscan be elements or compounds
products: only one compoundproducts: only one compound
A + X A + X AX AX
where A is the cation and X is anionwhere A is the cation and X is anion
1. Synthesis1. Synthesis
Rubidium and sulfurRubidium and sulfur
Rb Rb (s)(s) + S + S8 (s)8 (s) Rb Rb22S S (s)(s)
Magnesium and oxygenMagnesium and oxygen
Mg Mg (s)(s) + O + O2 (g)2 (g) MgO MgO (s)(s)
Sodium and chlorineSodium and chlorine
Na Na (s)(s) + Cl + Cl2 (g)2 (g) NaCl NaCl (s)(s)
Magnesium and fluorineMagnesium and fluorine
Mg Mg (s)(s) + F + F2 (g)2 (g) MgF MgF2 (s)2 (s)
1. Synthesis1. Synthesis
calcium oxide and watercalcium oxide and water
CaOCaO(s)(s) + H + H22OO(l)(l) Ca(OH) Ca(OH)2 (aq)2 (aq)
sulfur dioxide and watersulfur dioxide and water
SOSO2 (g)2 (g) + H + H22O O (l)(l) H H22SOSO3 (aq)3 (aq)
calcium oxide and sulfur dioxidecalcium oxide and sulfur dioxide
CaO CaO (s)(s) + SO + SO2 (g)2 (g) CaSO CaSO3 (s)3 (s)
2. Decomposition2. Decomposition
opposite of synthesisopposite of synthesis usually require energyusually require energy reactants: only one compoundreactants: only one compound products: more than oneproducts: more than one
usually elements but can be compoundsusually elements but can be compounds
AX AX A + X A + X
2. Decomposition2. Decomposition waterwater
HH22O O (l)(l) H H2 (g)2 (g) + O + O2 (g)2 (g)
calcium carbonatecalcium carbonate
CaCOCaCO3 (s)3 (s) CaO CaO (s)(s) + CO + CO2 (g)2 (g)
calcium hydroxidecalcium hydroxide
Ca(OH)Ca(OH)2 (s)2 (s) CaO CaO (s)(s) + H + H22O O (l)(l)
carbonic acidcarbonic acid
HH22COCO3 (aq) 3 (aq) CO CO2 (g)2 (g) + H + H22O O (l)(l)
3. Single Replacement3. Single Replacement
an element replaces a similar an element replaces a similar element in a compoundelement in a compound
reactants: 1 element & 1 compoundreactants: 1 element & 1 compound products: 1 element & 1 compoundproducts: 1 element & 1 compound
A + BX A + BX B + AX B + AX
Y + AX Y + AX X + AY X + AY
3. Single Replacement3. Single Replacement zinc and hydrochloric acidzinc and hydrochloric acid
Zn Zn (s)(s) + HCl + HCl (aq) (aq) ZnCl ZnCl2 (aq) 2 (aq) + H+ H2 (g)2 (g)
iron and wateriron and water
Fe Fe (s)(s) + H + H22O O (l)(l) FeO FeO (aq) (aq) + H+ H2 (g)2 (g)
magnesium and lead (II) nitratemagnesium and lead (II) nitrate
Mg Mg (s)(s) + Pb(NO + Pb(NO33))2 (aq) 2 (aq) Mg(NO Mg(NO33))3 (aq) 3 (aq) + Pb + Pb (s)(s)
chlorine and potassium bromidechlorine and potassium bromide
ClCl2 (g)2 (g) + KBr + KBr (s)(s) KCl KCl (s)(s) + Br + Br2 (g)2 (g)
4. Double Replacement4. Double Replacement
two similar elements switch placestwo similar elements switch places reactants: 2 compoundsreactants: 2 compounds products: 2 compounds products: 2 compounds
AX + BY AX + BY BX + AY BX + AY
4. Double Replacement4. Double Replacement barium chloride and sodium sulfatebarium chloride and sodium sulfate
BaClBaCl2 (aq) 2 (aq) + Na+ Na22SOSO4 (aq) 4 (aq) NaCl NaCl (aq) (aq) + BaSO+ BaSO4 (s)4 (s)
iron sulfide and hydrochloric acidiron sulfide and hydrochloric acid
FeS FeS (aq) (aq) + HCl + HCl (aq) (aq) FeCl FeCl2 (aq) 2 (aq) + H+ H22S S (g)(g)
hydrochloric acid and sodium hydroxidehydrochloric acid and sodium hydroxide
HCl HCl (aq) (aq) + NaOH+ NaOH (aq) (aq) NaCl NaCl (aq) (aq) + H+ H22O O (l)(l)
potassium iodide and lead (II) nitratepotassium iodide and lead (II) nitrate
KI KI (aq) (aq) + Pb(NO+ Pb(NO33))2 (aq)2 (aq) KNO KNO3 (aq) 3 (aq) + PbI+ PbI2 (s)2 (s)
5. Combustion5. Combustion
Only responsible for one typeOnly responsible for one type releases energy in form of heat/lightreleases energy in form of heat/light reactants: hydrocarbon + Oreactants: hydrocarbon + O22
HH22O and COO and CO2 2 as the only productsas the only products
Ex: CHEx: CH44 + O + O22 CO CO22 + H + H22OO
CombustionCombustion
propane and oxygenpropane and oxygen
CC33HH88(g) + O(g) + O22(g) (g) CO CO22(g) + H(g) + H22O(g)O(g)
PracticePractice
Classify each of the following reactions Classify each of the following reactions one of the five basic types:one of the five basic types:
NaNa22O + HO + H22O O NaOH NaOH synthesissynthesis
Zn Zn (s)(s) + 2HCl + 2HCl (aq) (aq) ZnCl ZnCl2 (aq) 2 (aq) + H+ H2 (g)2 (g)
single replacementsingle replacement
Ca Ca (s)(s) + 2H + 2H22O O (l)(l) Ca(OH) Ca(OH)2 (aq) 2 (aq) + H+ H2 (g)2 (g)
single replacementsingle replacement
PracticePractice
2H2H22OO2 (aq) 2 (aq) O O2 (g)2 (g) + 2H + 2H22O O (l)(l) decompositiondecomposition
Cu Cu (s)(s) + 2AgNO + 2AgNO3 (aq) 3 (aq) 2Ag 2Ag (s)(s) +Cu(NO +Cu(NO33))2 (aq)2 (aq) single replacementsingle replacement
CC22HH4 (g)4 (g) + O + O2 (g)2 (g) CO CO2 (g)2 (g) + H + H22O O (g)(g) combustioncombustion
ZnO ZnO (s)(s) + C + C (s)(s) 2Zn 2Zn (s)(s) + CO + CO2 (g)2 (g) single replacementsingle replacement
PracticePractice
NaNa22O O (s)(s) + 2CO + 2CO2 (g)2 (g) + H + H22O O (l)(l) NaHCO NaHCO3 (s)3 (s)
synthesissynthesis
CaCa(s)(s) + H + H22OO(l)(l) Ca(OH) Ca(OH)22 (aq) (aq) + H+ H2 (g)2 (g)
single replacementsingle replacement
KClOKClO3 (s)3 (s) KCl KCl (s)(s) + O + O2 (g)2 (g)
decompositiondecomposition
HH22SOSO4 (aq) 4 (aq) + BaCl+ BaCl2 (aq) 2 (aq) HCl HCl (aq) (aq) + BaSO+ BaSO4 (s)4 (s)
double replacementdouble replacement
Activity SeriesActivity Series
Activity Series Pg. 333Activity Series Pg. 333
ActivityActivity ability of an element to reactability of an element to react
easier it reacts, higher the activityeasier it reacts, higher the activity
activity seriesactivity series list of elements organized according to list of elements organized according to
activitiesactivities from highest to lowestfrom highest to lowest
Activity SeriesActivity Series
metalsmetals greater activity, easier to lose electronsgreater activity, easier to lose electrons easier to become a cationeasier to become a cation
nonmetalsnonmetals greater activity, easier to gain electronsgreater activity, easier to gain electrons easier to become an anioneasier to become an anion
Activity SeriesActivity Series
used to predict whether single used to predict whether single replacement reactions will occurreplacement reactions will occur
most active is on topmost active is on top
an element can replace anything below it an element can replace anything below it but not any above itbut not any above it
PracticePractice
zinc and hydrofluoric acidzinc and hydrofluoric acid Zn Zn (s)(s) + HCl + HCl (aq) (aq) ZnCl ZnCl2 (aq)2 (aq) + H + H2 (g)2 (g)
calcium and lead (II) nitratecalcium and lead (II) nitrate CaCa (s) (s) + Pb(NO + Pb(NO33))2 (aq)2 (aq) Ca(NO Ca(NO33))2 (aq) 2 (aq) + Pb+ Pb (s) (s)
copper and lithium sulfatecopper and lithium sulfate CuCu (s) (s) + Li + Li22SOSO4 (aq)4 (aq) no reaction no reaction
bromine and iron (II) chloridebromine and iron (II) chloride BrBr2 (l)2 (l) + FeCl + FeCl2 (aq)2 (aq) no reaction no reaction