![Page 1: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/1.jpg)
Reactions in Aqueous Solutions
Chapter 7Chapter 7
![Page 2: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/2.jpg)
Aqueous Solutions
Water is the dissolving Water is the dissolving medium, or medium, or solventsolvent..
![Page 3: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/3.jpg)
Driving Forces for Chemical Reactions
1. Formation of a precipitate (solid). 2. Formation of molecular substance (water). 3. Formation of a gas. 4. Transfer of electrons (Redox).
![Page 4: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/4.jpg)
Types of Solution Reactions
- Precipitation reactionsPrecipitation reactionsAgNOAgNO33((aqaq) + NaCl() + NaCl(aqaq) ) AgCl( AgCl(ss) + NaNO) + NaNO33((aqaq))
- Acid-base reactionsAcid-base reactionsNaOH(NaOH(aqaq) + HCl() + HCl(aqaq) ) NaCl( NaCl(aqaq) + H) + H22O(O(ll))
![Page 5: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/5.jpg)
ElectrolytesStrongStrong - conduct current efficiently - many ions in solution. - conduct current efficiently - many ions in solution.
NaCl, KNONaCl, KNO33, HNO, HNO33, NaOH, NaOH
Weak Weak - conduct only a small current - few ions in solution,- conduct only a small current - few ions in solution,
HCHC22HH33OO22, aq. NH, aq. NH33, tap H, tap H22OO
NonNon - no current flows - no ions in solution. - no current flows - no ions in solution.
pure Hpure H22O, sugar solution, glycerolO, sugar solution, glycerol
![Page 6: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/6.jpg)
In what two ways can a solid ionic compound be made to conduct electricity?
•Dissolve it in water.
•Melt or fuse it.
Ions must be free to move
(mobile) in order to conduct electricity!
![Page 7: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/7.jpg)
Dissociationionic compoundsionic compounds
metal + nonmetal (Type I & II)metal + nonmetal (Type I & II)metal + polyatomic anionmetal + polyatomic anionAmmonium compoundsAmmonium compoundsAcidsAcids
When ionic compounds dissolve in water the anions and When ionic compounds dissolve in water the anions and cations are separated from each other; this is called cations are separated from each other; this is called dissociationdissociation
We know that ionic compounds dissociate when they We know that ionic compounds dissociate when they dissolve in water because the solution conducts electricitydissolve in water because the solution conducts electricity
![Page 8: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/8.jpg)
Dissociationpotassium chloride dissociates in water into potassium chloride dissociates in water into
potassium cations and chloride anionspotassium cations and chloride anions
KCl(aq) = KKCl(aq) = K+ + (aq) + Cl(aq) + Cl- - (aq)(aq)
copper(II) sulfate dissociates in water into copper(II) copper(II) sulfate dissociates in water into copper(II) cations and sulfate anionscations and sulfate anions
CuSOCuSO44(aq) = Cu(aq) = Cu+2+2(aq) + SO(aq) + SO442-2-(aq)(aq)
K+ Cl-K Cl
Cu+2 SO42-Cu SO4
![Page 9: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/9.jpg)
Dissociation
potassium sulfate dissociates in water into potassium sulfate dissociates in water into potassium cations and sulfate anionspotassium cations and sulfate anions
KK22SOSO44(aq) = 2 K(aq) = 2 K+ + (aq) + SO(aq) + SO442-2-(aq)(aq)
K+
SO42-
K+
KK SO4
![Page 10: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/10.jpg)
Ionic Compounds in Solution
In aqueous solution, soluble ionic compoundsexist in the form of ions.
K2CrO4(aq) + Ba(NO3)2(aq) ----> BaCrO4(s) + 2KNO3(aq)
![Page 11: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/11.jpg)
Figure 7.1: The precipitation reaction that occurs when yellow potassium chormate, K2CrO4 (aq), is mixed with a colorless barium nitrate solution, Ba(NO3)2 (aq)
![Page 12: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/12.jpg)
Solubility
1. A soluble solid readily dissolves in water-- 1. A soluble solid readily dissolves in water-- designated with (aq).designated with (aq).
2. A slightly soluble solid only dissolves to a tiny 2. A slightly soluble solid only dissolves to a tiny extent in water--designated with (s).extent in water--designated with (s).
3. An insoluble solid does not dissolve to any 3. An insoluble solid does not dissolve to any appreciable extent in water--designated with (s).appreciable extent in water--designated with (s).
![Page 13: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/13.jpg)
Simple Rules for Solubility1.1. Most nitrate (NOMost nitrate (NO33
), acetate (C), acetate (C22HH33OO22-)-), & chlorate (ClO, & chlorate (ClO33
--) )
salts salts are solubleare soluble..
2.2. Most alkali (group 1A) salts and NHMost alkali (group 1A) salts and NH44++ are solubleare soluble..
3.3. Most ClMost Cl, Br, Br, and I, and I salts salts are soluble are soluble ((NOTNOT AgAg++, Pb, Pb2+2+, , HgHg22
2+2+))
4.4. Most sulfate salts Most sulfate salts are soluble are soluble ((NOTNOT BaSOBaSO44, PbSO, PbSO44, ,
HgSOHgSO44, CaSO, CaSO44))
5.5. Most OHMost OH salts salts are only slightly soluble are only slightly soluble (NaOH, KOH are (NaOH, KOH are soluble, Ba(OH)soluble, Ba(OH)22, Ca(OH), Ca(OH)22 are marginally soluble) are marginally soluble)
6.6. Most SMost S22, CO, CO3322, CrO, CrO44
22, PO, PO4433 salts salts are only slightly are only slightly
solublesoluble. .
![Page 14: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/14.jpg)
![Page 15: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/15.jpg)
Precipitation ReactionsIn all precipitation reactions, the ions of one substance In all precipitation reactions, the ions of one substance
are exchanged with the ions of another substance when are exchanged with the ions of another substance when their aqueous solutions are mixedtheir aqueous solutions are mixed
At least one of the products formed is insoluble in waterAt least one of the products formed is insoluble in water
KI(aq) + AgNOKI(aq) + AgNO33(aq) (aq) KNOKNO33(aq) + AgI(aq) + AgIss
K+
I-
Ag+
NO3-
K+
NO3-
Ag I
![Page 16: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/16.jpg)
Describing Reactions in Solution
1.1. Molecular equation Molecular equation (reactants and products as (reactants and products as compoundscompounds))
AgNOAgNO33((aqaq) + NaCl() + NaCl(aqaq) ) AgCl( AgCl(ss) + NaNO) + NaNO33((aqaq))
2.2. Complete ionic equation Complete ionic equation (all strong (all strong electrolytes shown as electrolytes shown as ionsions))
AgAg++((aqaq) + NO) + NO33((aqaq) + Na) + Na++((aqaq) + Cl) + Cl((aqaq) )
AgCl(AgCl(ss) + Na) + Na++((aqaq) + NO) + NO33((aqaq))
![Page 17: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/17.jpg)
Describing Reactions in Solution (continued)
3.3. Net ionic equation Net ionic equation (show only (show only components that actually react)components that actually react)
AgAg++((aqaq) + Cl) + Cl((aqaq) ) AgCl( AgCl(ss))
NaNa++ and NO and NO33 are spectator ions. are spectator ions.
![Page 18: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/18.jpg)
Solutions of:
AgNO3
Na2SO4
![Page 19: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/19.jpg)
If AgNO3 is mixed with Na2SO4 what ions are most abundant in the solution?
AgNO3
Na2SO4
With what ions is the solution saturated?
![Page 20: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/20.jpg)
2AgNO3(aq) + Na2SO4(aq) 2 NaNO3 (aq) + Ag2SO4(s)
Silver Sulfate
Precipitate
2Ag+(aq)
+ 2 NO3-(aq) + 2Na+
(aq) + SO42-
(aq) 2Na+(aq) + 2 NO3
- (aq) + Ag2SO4(s)
2Ag+(aq)
+ SO42-
(aq) Ag2SO4(s)
Molecular Equation
Overall Ionic Equation
Net Ionic Equation
![Page 21: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/21.jpg)
Acids
The nature of acids was discovered by Svante The nature of acids was discovered by Svante Arrhenius. Arrhenius.
Acids are characterized by:Acids are characterized by:
• a sour taste (lemons -- citric acid).a sour taste (lemons -- citric acid).
• producing Hproducing H+ + ions (protons) in aqueous ions (protons) in aqueous solution.solution.
• turn blue litmus red.turn blue litmus red.
![Page 22: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/22.jpg)
Acids
Strong acids Strong acids -- dissociate completely dissociate completely (nearly (nearly 100 %)100 %) to produce H to produce H++ in solution in solution
HCl, HHCl, H22SOSO44, HNO, HNO33, HBr, HI, & HClO, HBr, HI, & HClO44
Weak acids Weak acids - dissociate to a slight extent - dissociate to a slight extent (approximately 1 %)(approximately 1 %) to give H to give H++ in solution in solution
HCHC22HH33OO22, HCOOH, HNO, HCOOH, HNO22, & H, & H22SOSO33
![Page 23: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/23.jpg)
Figure 7.5: When gaseous HCl is dissolved in water, each molecule dissociates to produce H+
and Cl- ions
![Page 24: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/24.jpg)
Bases
Bases are characterized by:Bases are characterized by:
• bitter taste (soap).bitter taste (soap).
• feel slippery.feel slippery.
• produce hydroxide (OHproduce hydroxide (OH--) ions in aqueous ) ions in aqueous solution.solution.
• turn red litmus blue.turn red litmus blue.
A basic solution is said to be A basic solution is said to be alkalinealkaline since they often since they often contain one of the contain one of the alkalialkali metals --Na, K, Li, etc. metals --Na, K, Li, etc.
![Page 25: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/25.jpg)
Bases
Strong bases Strong bases - react completely with water to - react completely with water to give OHgive OH ions. ions.
sodium hydroxidesodium hydroxide
Weak bases Weak bases - react only slightly with water to - react only slightly with water to give OHgive OH ions. ions.
ammoniaammonia
![Page 26: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/26.jpg)
Acid-Base Reactions
Acid + Base ----> Salt + water
Molecular EquationHCl(aq) + NaOH(aq) ----> NaCl(aq) + HOH(l)
Complete Ionic EquationH+
(aq) + Cl-(aq) + Na+
(aq) + OH-(aq) -----> Na+
(aq) + Cl-(aq)
+ HOH(l)Net Ionic EquationH+
(aq) + OH-(aq) -----> HOH(l)
![Page 27: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/27.jpg)
Acid-Base Neutralization
The net ionic equation for the neutralization of any strong acid and base will always be:
HH++(aq) (aq) + OH+ OH--
(aq)(aq) -----> HOH -----> HOH(l)(l)
![Page 28: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/28.jpg)
Salts
Salts are Salts are ionic compoundsionic compounds consisting of: consisting of:
a. metal & nonmetal -- a. metal & nonmetal -- KClKCl
b. metal & polyatomic ion -- b. metal & polyatomic ion -- CuSOCuSO44
c. polyatomic ion & nonmetal -- c. polyatomic ion & nonmetal -- NHNH44ClCl
d. two polyatomic ions -- d. two polyatomic ions -- (NH(NH44))22SOSO44
![Page 29: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/29.jpg)
Oxidation-Reduction Reactions(Redox Reactions)
Redox reaction -- Redox reaction -- involves the transfer of involves the transfer of electronselectrons
• loss and gain of electrons must be loss and gain of electrons must be exactlyexactly equal. equal.
• loss and gain of electrons must be loss and gain of electrons must be simultaneous.simultaneous.
![Page 30: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/30.jpg)
Oxidation
• loss of electrons loss of electrons
• metal atoms -- Na, Ca, & Kmetal atoms -- Na, Ca, & K
• NaNaoo ---> Na ---> Na1+ 1+ + 1e+ 1e--
• CaCao o ---> Ca---> Ca2+ 2+ + 2e+ 2e--
• nonmetal ions -- Clnonmetal ions -- Cl--, S, S2-2-, & O, & O2-2-
• ClCl1-1- ---> Cl ---> Clo o ++ 1e-1e-
• SS2-2- ---> S ---> So o + 2+ 2 e-e-
![Page 31: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/31.jpg)
Reduction
• gain of electrons.gain of electrons.
• nonmetal atoms.nonmetal atoms.
• OOoo + 2e + 2e-- ---> O ---> O2-2-
• FFoo + 1e + 1e-- ---> F ---> F1-1-
• metal ions.metal ions.
• KK1+ 1+ + 1e+ 1e- - ---> K---> Koo
• BaBa2+2+ + 2e + 2e-- ---> Ba ---> Baoo
![Page 32: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/32.jpg)
Figure 7.7: When powdered aluminum and iodine (shown in the foreground) are mixed (and a little water added), they react
vigorously
![Page 33: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/33.jpg)
Oxidation & Reduction Half-Reactions
• Always add electrons (negative) to the Always add electrons (negative) to the more positive side of the equation.more positive side of the equation.
• The charge on both sides of an equation The charge on both sides of an equation must be equal.must be equal.
• Oxidation -- NaOxidation -- Naoo ----> Na ----> Na1+ 1+ + 1 e-+ 1 e-
• Reduction -- ClReduction -- Cl2 2 + 2 e+ 2 e- - ----> 2 Cl----> 2 Cl- -
![Page 34: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/34.jpg)
OIL RIG
Oxidation Is Loss.
Reduction Is Gain.
![Page 35: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/35.jpg)
Redox Reactions
• Metal-nonmetal reactions are Metal-nonmetal reactions are alwaysalways redox reactions.redox reactions.
• Any reaction that has a free element (such Any reaction that has a free element (such as Oas O22) as a reactant or product are redox.) as a reactant or product are redox.
• All single replacement reactions are redox.All single replacement reactions are redox.
• All combustion reactions are redox.All combustion reactions are redox.
![Page 36: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/36.jpg)
Synthesis I (Composition)
A + X ----> AX A + X ----> AX ALWAYS REDOXALWAYS REDOX
Element + Element -----> Binary CompoundElement + Element -----> Binary Compound
FeFe(s)(s) + S + S(s)(s) ----> FeS ----> FeS(s)(s)
4 Al4 Al(s)(s) + 3 O + 3 O2(g)2(g) ----> 2 Al ----> 2 Al22OO3(s)3(s)
![Page 37: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/37.jpg)
Synthesis II (Composition)
A + X ----> AX A + X ----> AX NOT REDOXNOT REDOX
Compound + Compound ----> Compound (3 Compound + Compound ----> Compound (3 or more or more elements)elements)
Ammonia + Acid ----> Ammonium SaltAmmonia + Acid ----> Ammonium Salt
NHNH3(g)3(g) + HCl + HCl(g)(g) ----> NH ----> NH44ClCl(s)(s)
2 NH2 NH3(aq)3(aq) + H + H22SOSO4(aq)4(aq) ----> (NH ----> (NH44))22SOSO4(aq)4(aq)
![Page 38: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/38.jpg)
Synthesis II (Composition)ContinuedWater + An OxideWater + An Oxide
Rule # 1 --Rule # 1 --Water + Water + Metal OxideMetal Oxide ----> Metal ----> Metal Hydroxide (Base)Hydroxide (Base)
HOHHOH(l)(l) + CaO + CaO(s)(s) ----> Ca(OH) ----> Ca(OH)2(s)2(s)
HOHHOH(l)(l) + Na + Na22OO(s)(s) ----> 2 NaOH ----> 2 NaOH(aq)(aq)
Rule # 2 --Water + Nonmetal Oxide ----> Acid
HOH(l) + SO3(g) ----> H2SO4(aq)
HOH(l) + N2O5(g) ----> 2 HNO3(aq)
![Page 39: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/39.jpg)
Single Replacement I
A + BX ----> AX + B ALWAYS REDOX
Element + Compound ----> Different Element + Different
Compound
Metal Reactivities:
K > Na > Ca > Mg > Al > Zn > Cr > Fe > Cd > Co > Ni > Sn > Pb > H > Sb > Cu > Hg > Ag > Pt > Au
![Page 40: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/40.jpg)
Single Replacement I(Continued)A is a metal.
A is more reactive than B A + BX ----> AX + B
Cu(s) + 2 AgNO3(aq) ---->Cu(NO3)2(aq) + 2 Ag(s)
Zn(s) + 2 HCl(aq) ----> ZnCl2(aq) + H2(g)
Rule # 3 -- Active Metal + Water ----> Metal Hydroxide + Hydrogen
Ca(s) + 2 HOH(l) ----> Ca(OH)2(s) + H2(g)
![Page 41: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/41.jpg)
Single Replacement I(Continued)
A is a metal.
A is less reactive than B
A + BX ----> No Reaction (NR)
Cu(s) + HCl(aq) ----> NR
![Page 42: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/42.jpg)
Single Replacement II
Y + BX ----> BY + X ALWAYS REDOX
Element + Compound ----> Different Element + Different
Compound
Nonmetal Reactivities:
F > O > Cl > Br > I
![Page 43: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/43.jpg)
Single Replacement II(Continued)
Y is a nonmetal.Y is more reactive than X Y + BX ----> BY + X
Cl2(g) + 2 KBr(aq) ----> 2 KCl(aq) + Br2(aq)
Y is less reactive than X Y + BX ----> No Reaction
Cl2(g) + KF(aq) ----> NR
![Page 44: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/44.jpg)
Single Replacement(Continued)
Remember!!Remember!!Metals replace metals.Metals replace metals.
MgMg(s) (s) + 2 Ag(NO+ 2 Ag(NO33))2(aq) 2(aq) ----> 2 Ag----> 2 Ag(s)(s) + Mg(NO + Mg(NO33))2(aq) 2(aq)
Nonmetals replace nonmetals.Nonmetals replace nonmetals.
ClCl2(g)2(g) + 2 KBr + 2 KBr(aq) (aq) ----> Br----> Br2(aq) 2(aq) + 2 KCl+ 2 KCl(aq)(aq)
![Page 45: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/45.jpg)
Figure 7.6: The thermite reaction
gives off so much heat that the iron formed
is molten
![Page 46: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/46.jpg)
Decomposition I
AX ----> A + X ALWAYS REDOX
AX is a binary compound.
Binary Compound ----> Element + Element
elect
2 NaCl(l) ----> 2 Na(l) + Cl2(g)
elect
2 HOH(l) ----> 2 H2(g) + O2(g)
![Page 47: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/47.jpg)
Decomposition II
AX -----> A + X MAY OR MAY NOT BE REDOX
AX is a ternary compound.
Rule # 4 -- Metal Chlorates ----> Metal Chlorides + Oxygen
2 KClO3(s) ----> 2 KCl (s) + 3 O2(g) REDOX
![Page 48: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/48.jpg)
Decomposition II(Continued)
Rule # 5 -- Metal Carbonates ----> Metal Oxides + Carbon
Dioxide
CuCO3(s) ----> CuO (s) + CO2(g) NOT REDOX
![Page 49: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/49.jpg)
Decomposition II(Continued)
Rule # 6 -- Metal Hydroxides ----> Metal Oxides + Water
Ca(OH)2(s) ----> CaO (s) + HOH(g) NOT REDOX
![Page 50: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/50.jpg)
Decomposition II(Continued)
Rule # 7 -- Acid ----> Nonmetal Oxide + Water
H2SO4(aq) ----> SO3(g) + HOH(g) NOT REDOX
![Page 51: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/51.jpg)
Double Displacement (Double Replacement)
AX + BY ----> AY + BX NEVER REDOX
Compound + Compound ----> 2 New Compounds
Acid-Base & Precipitation Reactions (Chapter 7)
HH22SOSO4(aq)4(aq) + 2 NaOH + 2 NaOH(aq) (aq) ----> Na----> Na22SOSO4(aq) 4(aq) + 2 HOH+ 2 HOH(l)(l)
NaClNaCl(aq) (aq) + AgNO+ AgNO3(aq)3(aq) ----> NaNO ----> NaNO3(aq)3(aq) + AgCl + AgCl(s)(s)
![Page 52: Reactions in Aqueous Solutions Chapter 7 Chapter 7](https://reader033.vdocuments.us/reader033/viewer/2022061305/55143647550346d8488b6214/html5/thumbnails/52.jpg)
Combustion
AX + OAX + O2 2 ALWAYS REDOXALWAYS REDOX
AX is a hydrocarbon.AX is a hydrocarbon.
CCxxHHyy + O + O2(g)2(g) ----> CO ----> CO2(g)2(g) + HOH + HOH(g)(g)
CHCH4(g)4(g) + 2 O + 2 O2(g)2(g) ----> CO ----> CO2(g)2(g) + 2 HOH + 2 HOH(g)(g)
2 C2 C66HH6(l) 6(l) + 15 O+ 15 O2(g) 2(g) ----> 12 CO----> 12 CO2(g) 2(g) + 6 HOH+ 6 HOH(g)(g)