2 BALANCING EQ & STOICH & AQU. SOL.

(1)

OXIDATION-REDUCTION OXIDATION-REDUCTION

BALANCING CHEMICAL EQUATIONS BALANCING CHEMICAL EQUATIONS

STOICHIOMETRY STOICHIOMETRY

(2)

REDOX

 REDOX_REDOX: SHORT FOR OXIDATION _{: SHORT FOR OXIDATION}

REDUCTION. DEFINED AS A REACTION IN REDUCTION. DEFINED AS A REACTION IN WHICH ELECTRONS ARE TRANSFERRED WHICH ELECTRONS ARE TRANSFERRED

FROM ONE ATOM TO ANOTHER. FROM ONE ATOM TO ANOTHER.

 _OXIDATION_OXIDATION_{IS DEFINED AS THE}_{IS DEFINED AS THE}_LOSS_LOSS_OF_OF ELECTRONS FROM ATOMS OF A

ELECTRONS FROM ATOMS OF A SUBSTANCE.

SUBSTANCE.

(3)

REDOX

CATIONSCATIONS:: POSITIVE IONS THAT POSITIVE IONS THAT COMES FROM METALS THAT

COMES FROM METALS THAT LOSELOSE

ELECTRONS

ELECTRONS (OXIDATION)(OXIDATION) IN ORDER IN ORDER TO BECOME

TO BECOME ISOELECTRONICISOELECTRONIC WITH A WITH A NOBLE GAS.

(4)

REDOX

 ANIONS_ANIONS: NEGATIVE IONS THAT COME _{: NEGATIVE IONS THAT COME}

FROM NONMETALS THAT

FROM NONMETALS THAT GAINGAIN

ELECTRONS (REDUCTION) TO

BECOME

BECOME ISOELECTRONICISOELECTRONIC WITH A WITH A NOBLE GAS.

(5)

REDOX

 ISOELECTRONIC_{ISOELECTRONIC}: WHEN TWO _{: WHEN TWO}

ELEMENTS OR IONS HAVE THE SAME

ELECTRON CONFIGURATION.

 _{WHEN ELEMENTS ARE}_{WHEN ELEMENTS ARE}

ISOELECTRONIC THEY TEND TO HAVE

(6)

REDOX

 RULES TO DETERMINE OXIDATION _{RULES TO DETERMINE OXIDATION} NUMBERS.

NUMBERS.

 1) THE OXIDATION NUMBER OF ANY _{1) THE OXIDATION NUMBER OF ANY} ELEMENT IN ITS FREE STATE IS ZERO. ELEMENT IN ITS FREE STATE IS ZERO.  EXAMPLES: Fe, Mg, OEXAMPLES: Fe, Mg, O₂₂, N, N₂₂..

 _{WHEN AN ELEMENT HAS EQUAL NUMBER}_{WHEN AN ELEMENT HAS EQUAL NUMBER} OF PROTONS AND ELECTRONS, ITS

(7)

REDOX

 2) THE OXIDATION NUMBER OF ALKALI _{2) THE OXIDATION NUMBER OF ALKALI}

METALS IN A COMPOUND IS 1

METALS IN A COMPOUND IS 1++

 3) THE OXIDATION NUMBER OF _{3) THE OXIDATION NUMBER OF}

ALKALINE METALS IS 2

(8)

REDOX

 THE OXIDATION NUMBER OF _{THE OXIDATION NUMBER OF}

HYDROGEN IN MOST COMPOUNDS IS

1

1++

 _{OXYGEN HAS A OXIDATION NUMBER}_{OXYGEN HAS A OXIDATION NUMBER}

OF 2

(9)

-REDOX

REDOX

 OXYGEN (AS OOXYGEN (AS O₂₂) HAS A OXIDATION NUMBER ) HAS A OXIDATION NUMBER OF 1

OF 1- - WHEN BONDED TO HYDROGEN IN _{WHEN BONDED TO HYDROGEN IN}

HYDROGEN PEROXIDE H

HYDROGEN PEROXIDE H₂₂OO₂₂. .

 OXYGEN (AS O) HAS A OXIDATION NUMBER _{OXYGEN (AS O) HAS A OXIDATION NUMBER} OF 2

OF 2++ WHEN BONDED TO FLOURINE(F_{WHEN BONDED TO FLOURINE(F} 2

2), THE ), THE

(10)

REDOX

 IN METALLIC HALIDES THE HALOGENS _{IN METALLIC HALIDES THE HALOGENS}

(F, Cl, Br, I, At) ALWAYS HAVE AN

OXIDATION NUMBER OF 1

OXIDATION NUMBER OF 1-

- _{TRANSITIONAL METALS GROUP 3-12}_{TRANSITIONAL METALS GROUP 3-12}

HAVE VARIABLE OXIDATION

NUMBERS.

(11)

REDOX

 THE OXIDATION NUMBER OF A _{THE OXIDATION NUMBER OF A}

MONATOMIC ION IS EQUAL TO THE

CHARGE ON THE ION.

 _{EXAMPLE: Ca}_{EXAMPLE: Ca}2+2+ THE CHARGE IS 2+_{THE CHARGE IS 2+}

(12)

1-REDOX

REDOX

 WHAT ARE THE OXIDATION NUMBERS _{WHAT ARE THE OXIDATION NUMBERS}

OF O

OF O₂₂, Cl, Cl₂₂, AND S, AND S₈₈ ? ?

 ANY ELEMENT IN ITS FREE STATE _{ANY ELEMENT IN ITS FREE STATE}

HAS AN OXIDATION NUMBER OF

ZERO.

 THESE ELEMENTS HAVE THE SAME _{THESE ELEMENTS HAVE THE SAME}

NUMBER OF PROTONS AND

(13)

REDOX

 WHAT IS THE OXIDATION NUMBER OF _{WHAT IS THE OXIDATION NUMBER OF}

Ca

Ca2+2+?_?

 2₂++

 _{THE OXIDATION NUMBER OF A}_{THE OXIDATION NUMBER OF A}

MONATOMIC ION IS EQUAL TO THE

(14)

REDOX

 WHAT ARE THE OXIDATION NUMBERS _{WHAT ARE THE OXIDATION NUMBERS}

FOR NH

FOR NH₃₃? THIS IS AMMONIA. IT IS NOT ? THIS IS AMMONIA. IT IS NOT AN ION.

AN ION.

 NITROGEN 3_{NITROGEN 3}-- HYDROGEN 1_{HYDROGEN 1}++

 THE SUM OF THE OXIDATION _{THE SUM OF THE OXIDATION}

NUMBERS MUST EQUAL ZERO.

(15)

REDOX

 CClCCl₄₄WHAT ARE THE OXIDATION WHAT ARE THE OXIDATION

NUMBERS OF EACH ELEMENT?

 C 4_{C 4}++ Cl 1_{Cl 1}-

(16)

REDOX

 THE TERM POLYATOMIC IS USED TO _{THE TERM POLYATOMIC IS USED TO}

DESCRIBE

DESCRIBE A GROUP OF ATOMS THAT A GROUP OF ATOMS THAT BEHAVE AS A SINGLE ION.

BEHAVE AS A SINGLE ION.

 _{A MOLECULE WITH A}_{A MOLECULE WITH A}_CHARGE_CHARGE_IS_IS

ANOTHER WAY OF SAYING IT.

(17)

REDOX

 COMMON POLYATOMIC IONS:_{COMMON POLYATOMIC IONS:}

 NHNH₄₄+ + AMMONIUM_AMMONIUM

 POPO₄₄3- 3- PHOSPHATE_PHOSPHATE

 COCO₃₃2- 2- CARBONATE_CARBONATE

(18)

REDOX

 SOSO₃₃-2 -2 IS A POLYATOMIC ION. WHAT _{IS A POLYATOMIC ION. WHAT}

ARE THE OXIDATION NUMBERS?

 S 4+ O 2-_{S 4+ O}

2- THE SUM OF THE OXIDATION _{THE SUM OF THE OXIDATION}

NUMBERS MUST EQUAL THE CHARGE

(19)

REDOX

 NHNH₄₄+ + IS A POLYATOMIC ION. WHAT _{IS A POLYATOMIC ION. WHAT}

ARE THE OXIDATION NUMBERS?

 N 3_{N 3}-- H 1_{H 1}++

(20)

REDOX

 NaClONaClO₄₄WHAT ARE THE OXIDATION WHAT ARE THE OXIDATION

NUMBERS?

 Na 1_{Na 1}++ Cl 7_{Cl 7}++ O 2_{O 2}-

- THE SUM MUST EQUAL ZERO. RARE _{THE SUM MUST EQUAL ZERO. RARE}

TIME WHEN Cl HAS A POSITIVE

(21)

REDOX

 CrOCrO₄₄2- 2- WHAT ARE THE OXIDATION _{WHAT ARE THE OXIDATION}

NUMBERS?

 Cr 6_{Cr 6}++ O 2_{O 2}-

(22)

CHEMICAL REACTIONS

 CHEMICAL REACTION: A PROCESS _{CHEMICAL REACTION: A PROCESS}

WHERE CHEMICAL/PHYSICAL

PROPERTIES OF A SUBSTANCE

CHANGE INTO A SUBSTANCE WITH

NEW CHEMICAL/PHYSICAL

PROPERITES. A NEW SUBSTANCE IS

FORMED.

(23)

REACTIONS

 REACTANT: THE SUBSTANCE THAT _{REACTANT: THE SUBSTANCE THAT}

ENTERS INTO A CHEMICAL REACTION.

 PRODUCT: THE SUBSTANCE _{PRODUCT: THE SUBSTANCE}

PRODUCED.

 _{SOMETHING ALWAYS HAPPENS:}_{SOMETHING ALWAYS HAPPENS:}

ENERGY IS ABSORBED OR

(24)

REACTIONS

 OLD TIMEY FLASHBULB ON A _{OLD TIMEY FLASHBULB ON A}

CAMERA:

 Mg MAGNESIUM COMBINES WITH OMg MAGNESIUM COMBINES WITH O₂₂

OXYGEN TO FORM MAGNESIUM

OXIDE AND GIVES OFF ENERGY IN

THE FORM OF LIGHT.

(25)

REACTIONS

 Mg + 0Mg + 0₂₂ YIELDS MgO + ENERGY. YIELDS MgO + ENERGY.

 _{IMPORTANT TO REALIZE THAT IN ANY}_{IMPORTANT TO REALIZE THAT IN ANY}

CHEMICAL REACTION THERE IS A

RE-ARRANGEMENT

RE-ARRANGEMENT OF ATOMS; OF ATOMS;

ATOMS ARE

ATOMS ARE NOT PRODUCED OR _{NOT PRODUCED OR}

DESTROYED.

(26)

REACTIONS

 YOU CAN’T CHANGE THE _{YOU CAN’T CHANGE THE}SUBSCRIPT_SUBSCRIPT

(# OF ATOMS OF EACH ELEMENT) IF

YOU CHANGED THE SUBSCRIPT THIS

WOULD CHANGE THE SUBSTANCE.

 _{YOU SHOW THE NUMBER OF ATOMS}_{YOU SHOW THE NUMBER OF ATOMS}

OR MOLECULES INVOLVED BY A

NUMBER CALLED THE

(27)

REACTIONS

 Mg + 0Mg + 0₂₂ YIELDS MgO + ENERGY IS NOT YIELDS MgO + ENERGY IS NOT

A BALANCED CHEMICAL EQUATION.

 TO BALANCE: 2Mg + OTO BALANCE: 2Mg + O₂₂YIELDS 2MgO + YIELDS 2MgO +

ENERGY.

(28)

REACTIONS

 TYPES OF CHEMICAL REACTIONS:_{TYPES OF CHEMICAL REACTIONS:}  1) SYNTHESIS REACTION: TWO OR _{1) SYNTHESIS REACTION: TWO OR}

MORE SIMPLE SUBSTANCES

COMBINE TO FORM A NEW MORE

COMPLEX SUBSTANCE.

 A + B YIELDS C_{A + B YIELDS C}  _{2Na + Cl}_{2Na + Cl}

2

2 YIELDS 2NaCl YIELDS 2NaCl

(29)

REACTIONS

 2) DECOMPOSITION REACTION: A _{2) DECOMPOSITION REACTION: A}

COMPLEX SUBSTANCE BREAKS

DOWN INTO TWO OR MORE SIMPLER

SUBSTANCES.

 _{C YIELDS A + B}_{C YIELDS A + B}

(30)

REACTIONS

 3) SINGLE REPLACEMENT REACTION._{3) SINGLE REPLACEMENT REACTION.}  A SINGLE UNCOMBINED ELEMENT _{A SINGLE UNCOMBINED ELEMENT}

REPLACES AN ELEMENT THAT IS

PART OF A COMPOUND.

(31)

REACTIONS

 4) DOUBLE REPLACEMENT REACTION._{4) DOUBLE REPLACEMENT REACTION.}  TWO ATOMS OF DIFFERENT _{TWO ATOMS OF DIFFERENT}

COMPOUNDS REPLACE EACH OTHER.

(32)

REACTIONS

 DURING A CHEMICAL REACTION _{DURING A CHEMICAL REACTION}

ENERGY IS ALWAYS PRESENT.LIKE

THE ATOM, ENERGY IS NOT CREATED

OR DESTROYED IT JUST CHANGES

FORM.

(33)

REACTIONS

 DURING A CHEMICAL REACTION, _{DURING A CHEMICAL REACTION,}

ENERGY IS

ENERGY IS RELEASED OR RELEASED OR

ABSORBED.IT WILL USUALLY TAKE

ONE OF TWO FORMS:

(34)

REACTIONS

 WHEN THE ENERGY REQUIRED TO _{WHEN THE ENERGY REQUIRED TO}

BREAK BONDS IS LESS THAN THE

ENERGY RELEASED, IT IS AN

EXOTHERMIC REACTION

EXOTHERMIC REACTION..

 _{WHEN THE ENERGY REQUIRED TO}_{WHEN THE ENERGY REQUIRED TO}

BREAK BONDS IS GREATER THAN THE

ENERGY RELEASED IT IS AN

ENDOTHERMIC REACTION

(35)

EQUATIONS

 COMPOUNDS CONSISTING OF TWO _{COMPOUNDS CONSISTING OF TWO}

DIFFERENT TYPE ELEMENTS ARE

CONSIDERED TO BE BINARY

COMPOUNDS.

(36)

EQUATIONS

 THERE ARE TWO TYPES OF BINARY _{THERE ARE TWO TYPES OF BINARY}

COMPOUNDS:

(37)

EQUATIONS

 BINARY MOLECULES_{BINARY MOLECULES} CONSIST OF _{CONSIST OF}

TWO NONMETALS BONDED VIA

COVALENT BONDING.

 _{BINARY SALTS}_{BINARY SALTS}_{CONSIST OF A METAL}_{CONSIST OF A METAL}

AND A NONMETAL EXHIBITING IONIC

(38)

EQUATIONS

 BINARY MOLECULES: NONMETAL _{BINARY MOLECULES: NONMETAL}

PLUS NONMETAL COMPOUNDS.

EXAMPLES: CO

EXAMPLES: CO₂₂ AND N AND N₂₂OO₃₃..

 PREFIXES_PREFIXES MUST BE USED TO _{MUST BE USED TO}

DESIGNATE THE NUMBER OF ATOMS

OF EACH ELEMENT PRESENT IN ONE

MOLECULE.

(39)

EQUATIONS

 MONO (1) IS NEVER USED IN FRONT _{MONO (1) IS NEVER USED IN FRONT}

OF THE FIRST ELEMENT. IF THERE IS

ONLY ONE ATOM, THE MONO IS

ASSUMED.

(40)

EQUATIONS

 BINARY SALTS: METAL PLUS _{BINARY SALTS: METAL PLUS}

NONMETAL COMPOUNDS.

 PREFIXES GIVING THE NUMBER OF _{PREFIXES GIVING THE NUMBER OF}

ATOMS OF EACH ELEMENT PRESENT

ARE

(41)

EQUATIONS

 SALTS EXHIBIT IONIC BONDING _{SALTS EXHIBIT IONIC BONDING}

BETWEEN A METAL AND A

NONMETAL.

 _{THE METAL IS WRITTEN}_{THE METAL IS WRITTEN}_BEFORE_BEFORE_THE_THE

NONMETAL.

(42)

REDOX

 CATIONS WITH VARIABLE OXIDATION _{CATIONS WITH VARIABLE OXIDATION}

NUMBERS USE ROMAN NUMERALS

ENCLOSED IN PARENTHESIS

ENCLOSED IN PARENTHESIS TO TO

DESIGNATE THE CHARGE ON THE

CATION (METALLIC ION).

 EXAMPLE: FeClEXAMPLE: FeCl₂₂ AND FeCl AND FeCl₃₃; YOU CAN’T ; YOU CAN’T

CALL BOTH OF THESE IRON

CHLORIDE.

(43)

REDOX

 IRON(II) CHLORIDE AND IRON(III) _{IRON(II) CHLORIDE AND IRON(III)}

CHLORIDE.

 AGAIN, THE ROMAN NUMERALS _{AGAIN, THE ROMAN NUMERALS}

REPRESENT

REPRESENT THE CHARGE ON THE THE CHARGE ON THE CATION (METAL) AND DOES NOT

CATION (METAL) AND DOES NOT

REPRESENT THE NUMBER OF ATOMS

(44)

 WHEN WRITING _{WHEN WRITING}EMPIRICAL _EMPIRICAL

FORMULAS:

 1) WRITE THE SYMBOL OF THE _{1) WRITE THE SYMBOL OF THE}

ELEMENT WITH THE POSITIVE

OXIDATION NUMBER FIRST.

HYDROGEN AND ALL OF THE METALS.

 2) WRITE THE SYMBOL OF THE _{2) WRITE THE SYMBOL OF THE}

ELEMENT WITH THE NEGATIVE

(45)

 3) ADD THE SUBSCRIPTS SO THAT _{3) ADD THE SUBSCRIPTS SO THAT}

THE SUM OF THE OXIDATION

NUMBERS OF ALL THE ATOMS IN THE

FORMULA IS EQUAL TO ZERO.

(46)

COMPOUNDS

 A COMPOUND THAT CONTAINS THE _{A COMPOUND THAT CONTAINS THE}

ELEMENTS ALUMINUM AND SULFUR.

 1) WHAT ARE THE OXIDATION _{1) WHAT ARE THE OXIDATION}

NUMBERS?

 _{Al IS A GROUP 13 UNDER THE BORON}_{Al IS A GROUP 13 UNDER THE BORON}

GROUP. USUALLY A +3

(47)

COMPOUNDS

 2) HOW MANY ATOMS OF EACH _{2) HOW MANY ATOMS OF EACH}

ELEMENT DO YOU NEED SO THAT THE

SUM OF THE OXIDATION NUMBERS

EQUALS ZERO?

 _{WHAT IS THE LEAST COMMON}_{WHAT IS THE LEAST COMMON}

MULTIPLE OF 3 AND 2? THE +3 Al AND

(48)

COMPOUNDS

 (+3)2 PLUS 3(-2) EQUALS A PLUS 6 _{(+3)2 PLUS 3(-2) EQUALS A PLUS 6}

AND A MINUS 6 WHICH EQUALS ZERO.

 WRITE ALUMINUM FIRST (IT IS A _{WRITE ALUMINUM FIRST (IT IS A}

METAL AND HAS A POSITIVE OX #)

 AlAl₂₂SS₃₃

(49)

BALANCING MOLECULAR

EQUATIONS

 TIPS:_TIPS:

 1) MENTALLY COUNT OR ACTUALLY _{1) MENTALLY COUNT OR ACTUALLY}

TALLY HOW MANY OF EACH TYPE OF

ATOM IS PRESENT ON EACH SIDE OF

THE EQUATION.

(50)

BALANCING MOLECULAR

EQUATIONS

 3) BALANCE OXYGEN AND HYDROGEN _{3) BALANCE OXYGEN AND HYDROGEN}

LAST.

 4) IF THERE IS AN ODD NUMBER OF _{4) IF THERE IS AN ODD NUMBER OF}

AN ELEMENT ON ONE SIDE AND AN

EVEN NUMBER ON THE OTHER SIDE,

THE ODD NUMBER WILL NEED TO BE

EVENED OUT. USE A COEFFICIENT OF

2 FOR THAT SUBSTANCE.

(51)

BALANCING MOLECULAR

EQUATIONS

 5) IF THERE ARE POLYATOMIC IONS _{5) IF THERE ARE POLYATOMIC IONS}

THAT REMAIN TOGETHER AS A UNIT

DURING THE REACTION, COUNT THE

POLYATOMIC ION AS A UNIT.

 _{6) WHEN TALLYING, BE SURE TO}_{6) WHEN TALLYING, BE SURE TO}

ADJUST THE COUNT FOR EACH AND

(52)

Balancing equations

 NaOH + HNaOH + H₂₂SOSO₄₄ YIELDS Na YIELDS Na₂₂SOSO₄₄ + H + H₂₂OO

 ELEMENT BEFORE AFTER_{ELEMENT BEFORE AFTER}  Na 1 2_{Na 1 2}

 O 5 5_{O 5 5}  H 3 2_{H 3 2}

(53)

BALANCING EQUATIONS

 2NaOH + H2NaOH + H₂₂SOSO₄₄ YIELDS Na YIELDS Na₂₂SOSO₄₄ + H + H₂₂00  _{ELEMENT BEFORE AFTER}_{ELEMENT BEFORE AFTER}  Na 2 2_{Na 2 2}

(54)

BALANCING EQUATIONS

 2NaOH + H2NaOH + H₂₂SOSO₄₄ YIELDS Na YIELDS Na₂₂SOSO₄₄ + 2H + 2H₂₂00  _{ELEMENT BEFORE AFTER}_{ELEMENT BEFORE AFTER}  Na 2 2_{Na 2 2}

(55)

BALANCING EQUATIONS

 BALANCE THE FOLLOWING:_{BALANCE THE FOLLOWING:}  NaCl + BeFNaCl + BeF₂₂ -- -- NaF + BeCl NaF + BeCl₂₂  AgNOAgNO₃₃ + LiOH + LiOH  AgOH +LiNO AgOH +LiNO₃₃  CHCH₄₄ + O + O₂₂  CO CO₂₂ + H + H₂₂00

(56)

BALANCING MOLECULAR

EQUATIONS

 AMMONIUM NITRATE REACTS WITH _{AMMONIUM NITRATE REACTS WITH} CALCIUM PHOSPHATE TO FORM

CALCIUM PHOSPHATE TO FORM

AMMONIUM PHOSPHATE AND CALCIUM AMMONIUM PHOSPHATE AND CALCIUM

NITRATE. NITRATE.

 NHNH₄₄NONO₃₃ + Ca + Ca₃₃(PO(PO₄₄))₂₂ YIELDS (NH YIELDS (NH₄₄))₃₃POPO₄₄ + + Ca(NO

Ca(NO₃₃))₂₂

 _{FIRST, NOTICE THAT EACH OF THE}_{FIRST, NOTICE THAT EACH OF THE}

(57)

BALANCING MOLECULAR

EQUATIONS

 NHNH₄₄NONO₃₃ + Ca + Ca₃₃(PO(PO₄₄))₂₂ YIELDS (NH YIELDS (NH₄₄))₃₃POPO₄₄ + Ca(NO + Ca(NO₃₃))₂₂

(58)

BALANCING MOLECULAR

EQUATIONS

 1) BEGIN WITH CALCIUM, ADD A _{1) BEGIN WITH CALCIUM, ADD A}

COEFFICIENT OF 3 ON THE

COEFFICIENT OF 3 ON THE RIGHT RIGHT TO TO

BALANCE THE CALCIUM.

 2) DOING THIS CHANGES THE _{2) DOING THIS CHANGES THE}

NITRATE COUNT TO 6 ON THE RIGHT,

SO ADD A COEFFICIENT OF 6 ON THE

LEFT SIDE.

(59)

BALANCING MOLECULAR

EQUATIONS

 6NH₄NO₃ + Ca₃(PO₄)₂ YIELDS (NH₄)₃PO₄ + 3Ca(NO₃)₂

 NH₄ 6 NH₄ 3

 NO₃ 6 NO₃ 6

 Ca 3 Ca 3

(60)

BALANCING MOLECULAR

EQUATIONS

 FINALLY ADD A COEFFICIENT OF 2 IN FRONT OF _{FINALLY ADD A COEFFICIENT OF 2 IN FRONT OF}

AMMONIUM PHOSPHATE TO COMPLETE THE AMMONIUM PHOSPHATE TO COMPLETE THE

BALANCING. BALANCING.

 _6NH

4NO3 + Ca3(PO4)2 YIELDS 2(NH4)3PO4 +

3Ca(NO₃)₂

 _NH

4 6 NH4 6

 _NO

3 6 NO3 6

(61)

REACTIONS

 FOUR FACTORS AFFECT THE RATE _{FOUR FACTORS AFFECT THE RATE}

OF CHEMICAL REACTIONS.

 1) ₁₎CONCENTRATION_{CONCENTRATION}: A HIGH _{: A HIGH}

CONCENTRATION OF A REACTANT

MEANS MORE PARTICLES PER UNIT

VOLUME. THIS MEANS MORE

(62)

REACTIONS

 EXAMPLE: BURNING CHARCOAL. IF _{EXAMPLE: BURNING CHARCOAL. IF}

YOU BLOW ON IT, YOU ARE ADDING

OXYGEN OR INCREASING THE

REACTANT CAUSING MORE

COLLISIONS, SO THE CHARCOAL

BURNS FASTER.

(63)

REACTIONS

 2) ₂₎SURFACE AREA_{SURFACE AREA}: IF A SOLID _{: IF A SOLID}

BREAKS INTO SMALLER PIECES THE

SURFACE AREA IS INCREASED. A

INCREASED SURFACE AREA

INCREASES COLLISIONS.

(64)

REACTIONS

 EXAMPLE: A PIECE OF WOOD VS. A _{EXAMPLE: A PIECE OF WOOD VS. A}

PILE OF SAWDUST. SAWDUST HAS

GREATER SURFACE AREA.

(65)

REACTIONS

 3) ₃₎TEMPERATURE:_TEMPERATURE: PARTICLES AT _{PARTICLES AT}

INCREASED TEMPERATURES HAVE

MORE MOTION/MOVE FASTER, SO

THEY COLLIDE MORE OFTEN AND

WITH GREATER ENERGY. AT A

DECREASED TEMPERATURE,

PARTICLES HAVE LESS MOTION.

(66)

REACTIONS

 EXAMPLE: IF YOU DECREASE THE _{EXAMPLE: IF YOU DECREASE THE}

TEMPERATURE, (REFRIGERATION)

YOU SLOW CHEMICAL

REACTIONS(SPOILING).

(67)

REACTIONS

 4) ₄₎CATALYSTS_CATALYSTS: A SUBSTANCE WHICH _{: A SUBSTANCE WHICH}

INCREASES THE RATE OF REACTION

BUT IS NOT CHANGED BY THE

REACTION.

(68)

REACTIONS

 EXAMPLE: CATALYTIC CONVERTERS _{EXAMPLE: CATALYTIC CONVERTERS}

IN CARS INCREASE REACTIONS

CHANGING HARMFUL GASES INTO

LESS HARMFUL GAS.

(69)

REACTIONS

 CATALYSTS IN THE BODY ARE _{CATALYSTS IN THE BODY ARE}

CALLED ENZYMES.

(70)

STOICHIOMETRY

 STOICHEION MEANS ELEMENT_{STOICHEION MEANS ELEMENT}  METRON MEANING MEASURE_{METRON MEANING MEASURE}  REACTION STOICHIOMETRY: _{REACTION STOICHIOMETRY:}

INVOLVES THE MASS RELATIONSHIPS

BETWEEN REACTANTS AND

PRODUCTS IN A CHEMICAL

REACTION.

(71)

STOICHIOMETRY

 IN REACTION STOICHIOMETRY _{IN REACTION STOICHIOMETRY}

PROBLEMS, YOU WILL HAVE:

 1) INFORMATION THAT IS GIVEN_{1) INFORMATION THAT IS GIVEN}

 2) INFO YOU ARE EXPECTED TO FIND _{2) INFO YOU ARE EXPECTED TO FIND}

(UNKNOWN)

(72)

STOICHIOMETRY

 CHEMICAL EQUATIONS HELP US TO _{CHEMICAL EQUATIONS HELP US TO}

MAKE PREDICTIONS ABOUT

CHEMICAL REACTIONS WITHOUT

HAVING TO ACTUALLY RUN THE

REACTIONS IN THE LAB.

 STOICHIOMETRY WILL TELL US THE _{STOICHIOMETRY WILL TELL US THE}

AMOUNT OF REACTANTS AND

PRODUCTS FOR A CHEMICAL

REACTION.

(73)

STOICHIOMETRY

 EXAMPLE: 2AlEXAMPLE: 2Al₂₂OO₃₃ YIELDS 4Al + 3O YIELDS 4Al + 3O₂₂

 THIS EQUATION SAYS THAT _{THIS EQUATION SAYS THAT}

ALUMINUM OXIDE DECOMPOSES INTO

ALUMINUM AND OXYGEN.

(74)

STOICHIOMETRY

 ONE QUESTION MIGHT BE: _{ONE QUESTION MIGHT BE:}

DETERMINE THE AMOUNT OF MOLES

OF ALUMINUM THAT CAN BE

PRODUCED FROM 13.0 MOLES OF

ALUMINUM OXIDE?

 IS THE EQUATION BALANCED? WHAT _{IS THE EQUATION BALANCED? WHAT}

IS THE PROPER RATIO NEEDED TO

(75)

STOICHIOMETRY

 THE PROPER RATIO IS 4 MOL Al/ 2 _{THE PROPER RATIO IS 4 MOL Al/ 2}

MOL AL

MOL AL₂₂OO_3._3.

 SET UP THE EQUATION:_{SET UP THE EQUATION:}  13.0 MOL AL13.0 MOL AL₂₂OO₃₃ X 4MOL Al X 4MOL Al

(76)

STOICHIOMETRY

 A REAL PROBLEM: IN A SPACECRAFT, _{A REAL PROBLEM: IN A SPACECRAFT,}

THE CARBON DIOXIDE EXHALED BY

ASTRONAUTS CAN BE REMOVED BY

ITS REACTION WITH LITHIUM

HYDROXIDE ACCORDING TO THE

FOLLOWING CHEMICAL EQUATION:

(77)

STOICHIOMETRY

 COCO₂₂ + 2 LiOH YIELDS Li + 2 LiOH YIELDS Li₂₂COCO₃₃ + H + H₂₂OO

 QUESTION: HOW MANY MOLES OF _{QUESTION: HOW MANY MOLES OF}

LITHIUM HYDROXIDE ARE REQUIRED

TO REACT WITH 20 MOL CO

TO REACT WITH 20 MOL CO₂₂, THE _{, THE}

AVERAGE AMOUNT EXHALED BY A

(78)

STOICHIOMETRY

 STEP 1: WHAT IS GIVEN? WHAT IS _{STEP 1: WHAT IS GIVEN? WHAT IS}

UNKNOWN? GIVEN: CO

UNKNOWN? GIVEN: CO₂₂=20 MOL UNKNOWN: =20 MOL UNKNOWN: AMOUNT OF LiOH IN MOL

AMOUNT OF LiOH IN MOL

 STEP 2: CONVERSION RATIO_{STEP 2: CONVERSION RATIO}

 MOL LiOH_{MOL LiOH}

(79)

STOICHIOMETRY

 STEP 3: FILL IN THE NUMBERS_{STEP 3: FILL IN THE NUMBERS} 

 2 MOL LiOH_{2 MOL LiOH}

 20 MOL CO20 MOL CO₂₂ X _________ = 40 MOL X _________ = 40 MOL

LiOH

(80)

STOICHIOMETRY

 IN PHOTOSYNTHESIS, PLANTS USE _{IN PHOTOSYNTHESIS, PLANTS USE}

ENERGY FROM THE SUN TO

PRODUCE GLUCOSE AND OXYGEN

FROM THE REACTION OF CARBON

DIOXIDE AND WATER.

 QUESTION: WHAT MASS, IN GRAMS, _{QUESTION: WHAT MASS, IN GRAMS,}

OF GLUCOSE IS PRODUCED WHEN 3.0

MOL OF WATER REACT WITH CARBON

DIOXIDE.

(81)

STOICHIOMETRY

 WHEN SODIUM AZIDE IS ACTIVATED _{WHEN SODIUM AZIDE IS ACTIVATED}

IN A CARS AIRBAG, NITROGEN GAS

AND SODIUM ARE PRODUCED.

 CHEMICAL EQUATION:_{CHEMICAL EQUATION:}  _2NaN_2NaN

3

(82)

CHEMICAL EQUILIBRIUM

 WHEN NITROGLYCERIN EXPLODES, _{WHEN NITROGLYCERIN EXPLODES,}

NOT MUCH NITROGLYCERIN IS LEFT.

WHEN AN IRON NAIL RUSTS GOING

FROM IRON TO IRON OXIDE, GIVEN

TIME, ONLY THE RUST REMAINS.

 ALTHOUGH ONE REACTION OCCURS _{ALTHOUGH ONE REACTION OCCURS}

FAST AND THE OTHER SLOWLY, BOTH

REACTIONS GO TO

(83)

CHEMICAL EQUILIBRIUM

 ANOTHER WAY OF SAYING THIS IS _{ANOTHER WAY OF SAYING THIS IS}

THAT MOST OF THE REACTANTS ARE

CONVERTED TO PRODUCTS.

 NOT ALL REACTIONS GO TO _{NOT ALL REACTIONS GO TO}

COMPLETION, SOME ARE

REVERSIBLE

(84)

CHEMICAL EQUILIBRIUM

 CHEMICAL EQUILIBRIUM:_{CHEMICAL EQUILIBRIUM:} A STATE OF _{A STATE OF}

BALANCE IN WHICH THE RATE OF A

FORWARD REACTION EQUALS THE

RATE OF THE REVERSE REACTION

AND THE CONCENTRATION OF THE

REACTANTS AND PRODUCTS REMAIN

UNCHANGED.

 (INDICATED BY TWO YIELD ARROWS _{(INDICATED BY TWO YIELD ARROWS}

GOING IN BOTH DIRECTIONS)

(85)

CHEMICAL EQUILIBRIUM

 EXAMPLE. A CARBONATED DRINK _{EXAMPLE. A CARBONATED DRINK}

 (CO(CO₂₂ DISSOLVED IN WATER UNDER DISSOLVED IN WATER UNDER PRESSURE)

PRESSURE)

 _{WHEN THE CAP IS ON AND THE CONTENTS}_{WHEN THE CAP IS ON AND THE CONTENTS} REMAIN UNDER PRESSURE, CO

REMAIN UNDER PRESSURE, CO₂₂

MOLECULES ARE COMING OUT OF MOLECULES ARE COMING OUT OF

(86)

CHEMICAL EQUILIBRIUM

 EXAMPLE: CaCOEXAMPLE: CaCO₃₃ (LIMESTONE) WHEN (LIMESTONE) WHEN EXPOSED TO HEAT, IT PRODUCES CaO EXPOSED TO HEAT, IT PRODUCES CaO

(LIME) AND CO

(LIME) AND CO₂₂. THIS PROCESS WAS USED . THIS PROCESS WAS USED TO MAKE CEMENT IN BUILDINGS.

TO MAKE CEMENT IN BUILDINGS.

 _{LIKE THE CARBONATED DRINK, IF THE}_{LIKE THE CARBONATED DRINK, IF THE} CONTAINER IS CLOSED, CO

CONTAINER IS CLOSED, CO₂₂ BUILDS UP BUILDS UP SHOWN AS:

SHOWN AS:

(87)

CHEMICAL EQUILIBRIUM

 Le CHATELIERS PRINCIPLE:_{Le CHATELIERS PRINCIPLE:} IF A _{IF A}

CHANGE IS MADE TO A SYSTEM IN

CHEMICAL EQUILIBRIUM, THE

EQUILIBRIUM SHIFTS TO OPPOSE THE

CHANGE UNTIL A NEW EQUILIBRIUM

IS REACHED.

(88)

CHEMICAL EQUILIBRIUM

 THREE PRIMARY CONDITIONS THAT _{THREE PRIMARY CONDITIONS THAT}

CAN CHANGE EQUILIBRIUM:

 TEMPERATURE, PRESSURE, AND _{TEMPERATURE, PRESSURE, AND}

CONCENTRATION

(89)

CHEMICAL EQUILIBRIUM

 A REAL LIFE EXAMPLE OF CHEMICAL _{A REAL LIFE EXAMPLE OF CHEMICAL} EQUILIBRIUM AND Le CHATELIERS

EQUILIBRIUM AND Le CHATELIERS

PRINCIPLE INVOLVES THE PRODUCTION OF PRINCIPLE INVOLVES THE PRODUCTION OF

AMMONIA.

AMMONIA. (THE HABER PROCESS)(THE HABER PROCESS)

(90)

CHEMICAL EQUILIBRIUM

 THE CHALLENGE IS TO CREATE _{THE CHALLENGE IS TO CREATE}

CONDITIONS THAT FAVOR THE

HIGHEST YIELD

HIGHEST YIELD OF AMMONIA (NH OF AMMONIA (NH₃₃))

 IN OTHER WORDS, THE EQUILIBRIUM _{IN OTHER WORDS, THE EQUILIBRIUM}

SHOULD FAVOR AMMONIA

PRODUCTION BY MANIPULATING

TEMPERATURE, PRESSURE, AND

(91)

CHEMICAL EQUILIBRIUM

 TEMPERATURE: INCREASING _{TEMPERATURE: INCREASING}

TEMPERATURE FAVORS THE

REACTION THAT ABSORBS ENERGY.

(NH

(NH₃₃ PRODUCTION IS EXOTHERMIC) PRODUCTION IS EXOTHERMIC)

(92)

CHEMICAL EQUILIBRIUM

 PRESSURE: INCREASING PRESSURE _{PRESSURE: INCREASING PRESSURE}

FAVORS THE REACTION THAT

PRODUCES FEWER GAS MOLECULES.

 (NH(NH₃₃ PRODUCTION IS A GAS ON THE PRODUCTION IS A GAS ON THE

REACTANT SIDE BUT THE WANTED

LIQUID ON THE PRODUCT SIDE)

(93)

CHEMICAL EQUILIBRIUM

 SO THE HABER PROCESS FOR _{SO THE HABER PROCESS FOR}

AMMONIA PRODUCTION USES

AMMONIA PRODUCTION USES HIGHHIGH

PRESSURE AND

PRESSURE AND LOWLOW TEMPERATURE TEMPERATURE

TO HAVE

(94)

REACTIONS IN

AQUEOUS SOLUTION

AQUEOUS SOLUTIONS

(95)

AQUEOUS SOLUTION

 A SOLUTION IN WHICH WATER IS THE _{A SOLUTION IN WHICH WATER IS THE}

DISSOLVING MEDIUM IS CALLED AN

AQUEOUS SOLUTION

(96)

AQUEOUS SOLUTION

 THE _THESOLVENT_SOLVENT DOES THE DISSOLVING _{DOES THE DISSOLVING}

AND THE

AND THE SOLUTESSOLUTES ARE DISSOLVED ARE DISSOLVED IN THE SOLVENT.

(97)

AQUEOUS SOLUTION

 A SUBSTANCE (SUCH AS NaCl) WHOSE _{A SUBSTANCE (SUCH AS NaCl) WHOSE} AQUEOUS SOLUTIONS CONTAIN IONS

AQUEOUS SOLUTIONS CONTAIN IONS

IS CALLED AN

IS CALLED AN ELECTROLYTEELECTROLYTE..

 A SUBSTANCE (SUCH AS CA SUBSTANCE (SUCH AS C₁₂₁₂HH₂₂₂₂OO₁₁₁₁) ) THAT DOES NOT FORM IONS IN

(98)

AQUEOUS SOLUTIONS

 SOLID NaCl CONSISTS OF AN _{SOLID NaCl CONSISTS OF AN}

ORDERLY ARRANGEMENT OF Na

ORDERLY ARRANGEMENT OF Na++ AND _AND

Cl

Cl-- IONS. WHEN NaCl DISSOLVES IN _{IONS. WHEN NaCl DISSOLVES IN}

WATER, EACH ION SEPARATES FROM

THE SOLID STRUCTURE AND

DISPERSES THROUGHOUT THE

SOLUTION.

(99)

AQUEOUS SOLUTIONS

 THE IONIC SOLID (NaCl) _{THE IONIC SOLID (NaCl)}DISSOCIATES_DISSOCIATES

INTO ITS COMPONENT IONS AS IT

DISSOLVES.

 _{WATER IS A VERY EFFECTIVE}_{WATER IS A VERY EFFECTIVE}

SOLVENT FOR IONIC COMPOUNDS.

(100)

AQUEOUS SOLUTIONS

 ALTHOUGH WATER IS AN _{ALTHOUGH WATER IS AN}

ELECTRICALLY NEUTRAL MOLECULE,

THE O ATOM IS RICH IN ELECTRONS

AND HAS A PARTIAL NEGATIVE

CHARGE. DENOTED q-.

 EACH HYDROGEN ATOM HAS A _{EACH HYDROGEN ATOM HAS A}

PARTIAL POSITIVE CHARGE,

DENOTED q+.

(101)

AQUEOUS SOLUTIONS

 CATIONS ARE ATTRACTED BY THE _{CATIONS ARE ATTRACTED BY THE}

NEGATIVE END OF H

NEGATIVE END OF H₂₂O, AND ANIONS O, AND ANIONS ARE ATTRACTED BY THE POSITIVE

ARE ATTRACTED BY THE POSITIVE

END.

(102)

AQUEOUS SOLUTIONS

 THE IONS ARE SAID TO BE _{THE IONS ARE SAID TO BE}

SOLVATED

SOLVATED. IN CHEMICAL EQUATIONS, . IN CHEMICAL EQUATIONS, WE DENOTE SOLVATED IONS BY

WE DENOTE SOLVATED IONS BY

WRITING THEM AS Na

WRITING THEM AS Na++ (aq) AND Cl_{(aq) AND Cl}-

-(aq).

(103)

AQUEOUS SOLUTIONS

 WHEN A _{WHEN A}MOLECULAR COMPOUND_{MOLECULAR COMPOUND}

DISSOLVES IN WATER, THE SOLUTION

USUALLY CONSISTS OF INTACT

MOLECULES DISPERESED

THROUGHOUT THE SOLUTION.

(104)

AQUEOUS SOLUTIONS

 ACETIC ACID (CHACETIC ACID (CH₃₃COOH), MOST OF COOH), MOST OF

THE SOLUTE IS PRESENT AS

CH

CH₃₃COOH (aq) MOLECULES. ONLY A COOH (aq) MOLECULES. ONLY A SMALL FRACTION DISSOCIATES INTO

SMALL FRACTION DISSOCIATES INTO

H+ (aq) AND CH

(105)

AQUEOUS SOLUTIONS

 WHEN A WEAK ELECTROLYTE SUCH AS _{WHEN A WEAK ELECTROLYTE SUCH AS} ACETIC ACID (CH

ACETIC ACID (CH₃₃COOH) IONIZES IN COOH) IONIZES IN SOLUTION, WE WRITE THE REACTION

SOLUTION, WE WRITE THE REACTION

WITH TWO YIELDS SIGN HALF-ARROWS

POINTING IN OPPOSITE DIRECTIONS.

(106)

AQUEOUS SOLUTIONS

 THE HALF-ARROWS POINTING IN _{THE HALF-ARROWS POINTING IN}

OPPOSITE DIRECTIONS MEAN THAT

THE REACTION IS SIGNIFICANT IN

BOTH DIRECTIONS.

(107)

AQUEOUS SOLUTIONS

 AT ANY GIVEN MOMENT CHAT ANY GIVEN MOMENT CH₃₃COOH COOH

MOLECULES ARE IONIZING TO FORM

H

H++ AND CH_{AND CH} 3

3COOCOO-- IONS BUT H IONS BUT H++ AND AND

CH

CH₃₃COOCOO- - IONS ARE RECOMBINING TO _{IONS ARE RECOMBINING TO}

FORM CH

(108)

AQUEOUS SOLUTIONS

 THIS BALANCE PRODUCES A STATE _{THIS BALANCE PRODUCES A STATE}

OF

OF CHEMICAL EQUILIBRIUMCHEMICAL EQUILIBRIUM IN WHICH IN WHICH THE RELATIVE NUMBER OF EACH

THE RELATIVE NUMBER OF EACH

TYPE OF ION OR MOLECULE IN THE

REACTION ARE CONSTANT OVER

TIME.

(109)

AQUEOUS SOLUTIONS

 REACTIONS THAT RESULT IN THE _{REACTIONS THAT RESULT IN THE}

FORMATION OF AN INSOLUBLE

PRODUCT ARE CALLED

PRECIPITATION REACTIONS.

(110)

AQUEOUS SOLUTIONS

 PRECIPITATION REACTIONS OCCUR _{PRECIPITATION REACTIONS OCCUR}

WHEN PAIRS OF OPPOSITELY

CHARGED IONS ATTRACT EACH

OTHER SO STRONGLY THAT THEY

FORM AN INSOLUBLE IONIC SOLID.

(111)

AQUEOUS SOLUTIONS

 EXAMPLE:_EXAMPLE:

 Pb(NOPb(NO₃₃))₂₂(aq) + 2KI(aq) YIELDS PbI(aq) + 2KI(aq) YIELDS PbI₂₂(s) + (s) +

2KNO

2KNO₃₃(aq) (aq)

 THE LEAD IODIDE PbITHE LEAD IODIDE PbI₂₂ BECOMES THE BECOMES THE

PRECIPITATE, WHILE THE POTASSIUM

(112)

AQUEOUS SOLUTIONS

 REACTIONS IN WHICH CATIONS AND _{REACTIONS IN WHICH CATIONS AND}

ANIONS APPEAR TO EXCHANGE

PARTNERS ARE CALLED

PARTNERS ARE CALLED METATHESIS METATHESIS

REACTIONS

REACTIONS OR OR EXCHANGE EXCHANGE REACTIONS

(113)

AQUEOUS SOLUTIONS

 PRECIPITATION REACTIONS AND _{PRECIPITATION REACTIONS AND}

MANY NEUTRALIZATION REACTIONS

BETWEEN ACIDS AND BASES ARE

METATHESIS REACTIONS.

(114)

AQUEOUS SOLUTIONS

 GENERICALLY IT CAN BE WRITTEN:_{GENERICALLY IT CAN BE WRITTEN:}  AX + BY YIELDS AY + BX_{AX + BY YIELDS AY + BX}

 REAL EXAMPLE:_{REAL EXAMPLE:}

 AgNOAgNO₃₃(aq) + KCl(aq) YIELDS AgCl(s) + (aq) + KCl(aq) YIELDS AgCl(s) +

KNO

(115)

AQUEOUS SOLUTIONS

 PREDICT THE IDENTITY OF THE _{PREDICT THE IDENTITY OF THE}

PRECIPITATE THAT FORMS WHEN

AQUEOUS SOLUTIONS OF BaCl

AQUEOUS SOLUTIONS OF BaCl₂₂ AND AND

K

K₂₂SOSO₄₄ ARE MIXED. WRITE THE ARE MIXED. WRITE THE BALANCED EQUATION FOR THE

BALANCED EQUATION FOR THE

REACTION.

(116)

AQUEOUS SOLUTIONS

 THE REACTANTS CONTAIN Ba_{THE REACTANTS CONTAIN Ba}2+2+, Cl_{, Cl}--, K_{, K}++, _,

AND SO

AND SO₄₄2-2- IONS._IONS.

 EXCHANGING THE ANIONS GIVES US _{EXCHANGING THE ANIONS GIVES US}

BaSO

(117)

AQUEOUS SOLUTIONS

 THE BALANCED EQUATION:_{THE BALANCED EQUATION:}

 BaClBaCl₂₂(aq) + K(aq) + K₂₂SOSO₄₄(aq) YIELDS BaSO(aq) YIELDS BaSO₄₄(s) (s)

+ 2KCl.

 ACCORDING TO MY EQUATION BaSOACCORDING TO MY EQUATION BaSO₄₄

BECAME THE PRECIPITATE.

(118)

AQUEOUS SOLUTIONS

 IONIC EQUATIONS:_{IONIC EQUATIONS:}

 LETS LOOK AT THE PRECIPITATION _{LETS LOOK AT THE PRECIPITATION}

REACTION WE USED EARLIER:

2KNO

(119)

AQUEOUS SOLUTIONS

2KNO

2KNO₃₃(aq).(aq).

 _{AN EQUATION WRITTEN IN THIS}_{AN EQUATION WRITTEN IN THIS}

FASHION IS CALLED A MOLECULAR

EQUATION.

(120)

AQUEOUS SOLUTIONS

2KNO

2KNO₃₃(aq).(aq).

 _{BASED ON OUR SOLUBILITY CHART,}_{BASED ON OUR SOLUBILITY CHART,}

Pb(NO

Pb(NO₃₃))₂₂, KI, AND KNO, KI, AND KNO₃₃ ARE ALL ARE ALL

WATER SOLUBLE IONIC COMPOUNDS

AND STRONG ELECTROLYTES.

(121)

AQUEOUS SOLUTIONS

 WE CAN WRITE THE EQUATION IN A _{WE CAN WRITE THE EQUATION IN A}

FORM THAT INDICATES WHICH

SPECIES EXISTS AS IONS IN THE

SOLUTION.

 PbPb2+2+(aq) + 2NO_{(aq) + 2NO} 3

(122)

AQUEOUS SOLUTIONS

 _Pb_Pb2+2+(aq) + 2NO_{(aq) + 2NO} 3

3--(aq) + 2K(aq) + 2K++(aq) + 2I(aq) + 2I--(aq)(aq)

 YIELDS_YIELDS  _PbI_PbI

2

2(s) + 2K(s) + 2K++(aq) + 2NO(aq) + 2NO33--(aq)(aq)

 AN EQUATION WRITTEN IN THIS FORM, _{AN EQUATION WRITTEN IN THIS FORM,}

WITH ALL SOLUBLE STRONG

ELECTROLYTES SHOWN AS IONS, IS

CALLED A

(123)

AQUEOUS SOLUTIONS

 PbPb2+2+(aq) + 2NO_{(aq) + 2NO} 3

3--(aq) + 2K(aq) + 2K++(aq) + 2I(aq) + 2I--(aq)(aq)

 _YIELDS_YIELDS

 PbIPbI₂₂(s) + 2K(s) + 2K++(aq) + 2NO_{(aq) + 2NO} 3

3--(aq)(aq)

 NOTICE THAT KNOTICE THAT K++(aq) AND NO_{(aq) AND NO} 3

(124)

AQUEOUS SOLUTIONS

 IONS THAT APPEAR IN IDENTICAL _{IONS THAT APPEAR IN IDENTICAL}

FORMS ON BOTH SIDES OF A

COMPLETE IONIC EQUATION ARE

CALLED

CALLED SPECTATOR IONSSPECTATOR IONS, THEY , THEY PLAY NO DIRECT ROLE IN THE

PLAY NO DIRECT ROLE IN THE

REACTION.

(125)

AQUEOUS SOLUTIONS

 WHEN SPECTATOR IONS ARE _{WHEN SPECTATOR IONS ARE}

OMITTED FROM THE EQUATION (THEY

CANCEL OUT LIKE ALGEBRAIC

EQUATIONS), WE ARE LEFT WITH THE

NET IONIC EQUATION

NET IONIC EQUATION, WHICH ONLY , WHICH ONLY

INCLUDES IONS AND MOLECULES

DIRECTLY INVOLVED IN THE

(126)

AQUEOUS SOLUTIONS

 THE NET IONIC REACTION:_{THE NET IONIC REACTION:}  PbPb2+2+(aq) + 2I_{(aq) + 2I}--(aq) YIELDS PbI_{(aq) YIELDS PbI}

2

2(s)(s)

 IF EVERY ION IN A COMPLETE IONIC _{IF EVERY ION IN A COMPLETE IONIC}

EQUATION IS A SPECTATOR, NO

REACTION OCCURS.

(127)

AQUEOUS SOLUTIONS

 PROCEDURE FOR WRITING _{PROCEDURE FOR WRITING}NET IONIC_{NET IONIC}

EQUATIONS:

 1) WRITE A BALANCED MOLECULAR _{1) WRITE A BALANCED MOLECULAR}

EQUATION FOR THE REACTION.

(128)

AQUEOUS SOLUTIONS

 2) REWRITE THE EQUATION TO SHOW _{2) REWRITE THE EQUATION TO SHOW}

THE IONS THAT FORM IN SOLUTION

WHEN EACH SOLUBLE STRONG

ELECTROLYTE DISSOCIATES INTO ITS

IONS.

 3) IDENTIFY AND CANCEL SPECTATOR _{3) IDENTIFY AND CANCEL SPECTATOR}

IONS.

(129)

AQUEOUS SOLUTIONS

 WRITE THE NET IONIC EQUATION FOR _{WRITE THE NET IONIC EQUATION FOR}

THE PRECIPITATION REACTION THAT

OCCURS WHEN AQUEOUS

SOLUTIONS OF CALCIUM CHLORIDE

AND SODIUM CARBONATE ARE

(130)

AQUEOUS SOLUTIONS

 WHAT IS THE BALANCED MOLECULAR _{WHAT IS THE BALANCED MOLECULAR}

EQUATION FOR THIS WORD

REACTION?

 CaClCaCl₂₂(aq) + Na(aq) + Na₂₂COCO₃₃(aq) YIELDS CaCO(aq) YIELDS CaCO₃₃(s) (s)

+ 2NaCl(aq).

(131)

AQUEOUS SOLUTIONS

 CALCIUM ION Ca_{CALCIUM ION Ca}2+2+ AND CHLORIDE ION _{AND CHLORIDE ION}

Cl

Cl--, SO WE NEED CaCl_{, SO WE NEED CaCl} 2

2..

 SODIUM IS Na_{SODIUM IS Na}++ AND CARBONATE IS _{AND CARBONATE IS}

CO

CO₃₃2-2- SO WE NEED Na_{SO WE NEED Na} 2

2COCO33..

 WHEN WE WRITE A BALANCED _{WHEN WE WRITE A BALANCED}

MOLECULAR EQUATION, WE KNOW

(132)

AQUEOUS SOLUTIONS

 NOW WE NEED TO WRITE A COMPLETE _{NOW WE NEED TO WRITE A COMPLETE} IONIC EQUATION BASED ON THE

IONIC EQUATION BASED ON THE

BALANCED MOLECULAR EQUATION.

 YOU ALSO NEED TO RECOGNIZE THAT _{YOU ALSO NEED TO RECOGNIZE THAT} THE CO

THE CO₃₃2-2- IN CaCO_{IN CaCO} 3

3 IS INSOLUBLE. IS INSOLUBLE.

 WHEN WRITING THE COMPLETE IONIC _{WHEN WRITING THE COMPLETE IONIC} EQUATION, WE DON’T WRITE THE

EQUATION, WE DON’T WRITE THE

FORMULA OF ANY INSOLUBLE

COMPOUND AS ITS COMPONENT IONS.

(133)

AQUEOUS SOLUTIONS

 COMPLETE IONIC EQUATION:_{COMPLETE IONIC EQUATION:}

 CaCa2+2+(aq) + 2Cl_{(aq) + 2Cl}--(aq) + 2Na_{(aq) + 2Na}++(aq) + CO_{(aq) + CO} 3

32-2-(aq) (aq)

 YIELDS_YIELDS

(134)

AQUEOUS SOLUTIONS

 NOW WE NEED TO IDENTIFY AND _{NOW WE NEED TO IDENTIFY AND}

CANCEL THE SPECTATOR IONS AND

WRITE THE NET IONIC EQUATION.

 SPECTATOR IONS, THOSE THAT _{SPECTATOR IONS, THOSE THAT}

APPEAR IN IDENTICAL FORMS ON

BOTH SIDES OF THE IONIC EQUATION.

(135)

AQUEOUS SOLUTIONS

 NET IONIC EQUATION:_{NET IONIC EQUATION:}

 CaCa2+2+(aq) + CO_{(aq) + CO} 3