Reaction PredictionsReaction Predictions

Most Commonly Used Most Commonly Used Cations and AnionsCations and Anions

Hydrogen HHydrogen H++

Sodium NaSodium Na++

Potassium KPotassium K++

Calcium CaCalcium Ca++²²Magnesium MgMagnesium Mg++²² Iron (Ferrous) FeIron (Ferrous) Fe++²² Iron (Ferric) FeIron (Ferric) Fe++³³

•Hydroxide OHˉ•Chloride Clˉ•Sulfide Sˉ²•Bicarbonate HCOзˉ•Carbonate COзˉ²•Sulfate SO4ˉ²

•Phosphate PO4ˉ³

Cations/ Anions, contd.Cations/ Anions, contd.

You can figure out the charge of an ion by You can figure out the charge of an ion by using the periodic table. For Example:using the periodic table. For Example:

Alkali metals such as Lithium can easily Alkali metals such as Lithium can easily lose an electron to become stable (just like lose an electron to become stable (just like a Noble gas) so taking away an electron a Noble gas) so taking away an electron give Lithium a +1 charge. give Lithium a +1 charge.

On the other hand Halogens can easily On the other hand Halogens can easily accept an electron to become stable. accept an electron to become stable. Accepting an electron gives halogens a -1 Accepting an electron gives halogens a -1 charge. charge.

PracticePractice

What is the oxidation state of Oxide?What is the oxidation state of Oxide?

What is the oxidation state of Iodide?What is the oxidation state of Iodide?

What is the oxidation state of a Calcium ion?What is the oxidation state of a Calcium ion?

What is the oxidation state of a Lithium ion?What is the oxidation state of a Lithium ion?

AnswersAnswers

-2-2

-1-1

+2+2

+1+1

Net Ionic EquationNet Ionic Equation

To create a net ionic equation, you break To create a net ionic equation, you break apart all ionic molecules in a balanced apart all ionic molecules in a balanced molecular equation into their ions if they molecular equation into their ions if they are soluble.are soluble.

If there are spectator ions, ions that If there are spectator ions, ions that appear on both sides of the equation, they appear on both sides of the equation, they cancel each other.cancel each other.

Net Ionic ExampleNet Ionic Example

Silver nitrate is mixed with potassium Silver nitrate is mixed with potassium chromatechromate2AgNO2AgNO33 + K + K22CrOCrO44 →→ Ag Ag22CrOCrO44 + 2KNO + 2KNO33

Molecular EquationMolecular Equation2Ag2Ag++ + 2NO + 2NO33ˉ̄ + 2K + 2K++ + CrO + CrO44-2-2 → → AgAg22CrOCrO44 + 2K + 2K++

+ 2NO+ 2NO33-2-2

Complete ionic equationComplete ionic equation2Ag2Ag++ + CrO + CrO44-2-2 →→ AgAg22CrOCrO44

Net Ionic EquationNet Ionic Equation

Solubility RulesSolubility Rules NONO33

-- all nitrates are solubleall nitrates are soluble

CH3COOCH3COO-- or C or C22HH33OO22--

all acetates are soluble except AgCHall acetates are soluble except AgCH33COOCOO

ClOClO33-- all chlorates are soluble all chlorates are soluble

ClCl-- all chlorides are soluble except AgCl, Hg all chlorides are soluble except AgCl, Hg22ClCl22, , PbClPbCl2 2

BrBr-- all bromides are soluble except AgBr, PbBr all bromides are soluble except AgBr, PbBr22, , HgHg22BrBr22, and HgBr, and HgBr2 2

II-- all iodides are soluble except AgI, Hg all iodides are soluble except AgI, Hg22II22, HgI, and , HgI, and PbIPbI22

Solubility Rules, contd.Solubility Rules, contd.

SO4¯²SO4¯² all sulfates are soluble except all sulfates are soluble except BaSO4, PbSO4, Hg2SO4, CaSO4, BaSO4, PbSO4, Hg2SO4, CaSO4, AgSO4 and SrSO4 AgSO4 and SrSO4

Alkali metal, cations, and NHAlkali metal, cations, and NH44 – all are – all are solublesoluble

HH++ all common inorganic acids and all common inorganic acids and low molecular mass organic acids are low molecular mass organic acids are solublesoluble

(In)Soubility Rules, contd.(In)Soubility Rules, contd.

COCO33--² all carbonates are insoluble except those of alkali ² all carbonates are insoluble except those of alkali

metals and NHmetals and NH44

CrOCrO44--² all chromates are insoluble except those of alkali ² all chromates are insoluble except those of alkali

metals, NHmetals, NH44, CaCrO, CaCrO44, and SrCO, and SrCO44

OHOH-- all hydroxides are insoluble except those of the all hydroxides are insoluble except those of the alkali metals, NHalkali metals, NH44, Ba(OH), Ba(OH)22, Sr(OH), Sr(OH)22, and Ca(OH), and Ca(OH)2 2

POPO44--³ all phosphates are insoluble except those of ³ all phosphates are insoluble except those of

alkali metals and NHalkali metals and NH44

SOSO33--² all sulfites are insoluble except those of alkali ² all sulfites are insoluble except those of alkali

metals and NHmetals and NH44

SS--² all sulfides are insoluble except those of alkali ² all sulfides are insoluble except those of alkali metals and NHmetals and NH44

SynthesisSynthesis Synthesis occurs when two or more reactants combine to form Synthesis occurs when two or more reactants combine to form

a single product. There are several common types of synthesis a single product. There are several common types of synthesis reaction.reaction.

   You know it happens when you have:You know it happens when you have:

-A -A metal combines with a nonmetalmetal combines with a nonmetal to form a bianary salt. to form a bianary salt.   -A piece of lithium metal is dropped into a container of -A piece of lithium metal is dropped into a container of

nitrogen gas.nitrogen gas.6Li+ N6Li+ N22 2Li 2Li33NN

-Metal oxide and water-Metal oxide and water forms a base (metallic hydroxide) forms a base (metallic hydroxide)   -Solid sodium oxide is added to water.-Solid sodium oxide is added to water.

NaNa22O + HO + H22OO 2NaOH 2NaOH

Synthesis, contd.Synthesis, contd.

Nonmetal oxide and waterNonmetal oxide and water forms acids. forms acids. Nonmetal retains its oxidation number.Nonmetal retains its oxidation number.

   -Carbon dioxide is burned in water.-Carbon dioxide is burned in water.

COCO22 + H + H22O O   H  H22COCO33

Metallic oxides and nonmetallic oxidesMetallic oxides and nonmetallic oxides form salts. form salts.

   -Solid sodium oxide is added to -Solid sodium oxide is added to carbon dioxide.carbon dioxide.

NaNa22O + COO + CO22 Na Na22COCO22

DecompositionDecomposition

Occurs when a single reactant is broken Occurs when a single reactant is broken down into two or more products.down into two or more products.

The reactions react to form basic The reactions react to form basic compounds or elements.compounds or elements.

When a compound is heated or When a compound is heated or electrolyzed, it means that it is broken up electrolyzed, it means that it is broken up into its ions.into its ions.

AB AB A+BA+B

Examples of DecompositionExamples of Decomposition

A sample of magnesium carbonate is A sample of magnesium carbonate is heated.heated.

MgCOMgCO33 MgO + CO MgO + CO22

Molten sodium chloride is electrolyzed.Molten sodium chloride is electrolyzed.2NaCl 2NaCl 2Na + Cl 2Na + Cl22

A sample of ammonium carbonate is A sample of ammonium carbonate is heated.heated.

(NH(NH44))22COCO33 2NH 2NH33 + H + H22O + COO + CO22

Single ReplacementSingle Replacement

Reactions that involve an element Reactions that involve an element replacing one part of a compound. The replacing one part of a compound. The products include the displace element and products include the displace element and a new compound. An element can only a new compound. An element can only replace another element that is less active replace another element that is less active than itself. (Look a activity series/ AP than itself. (Look a activity series/ AP packet)packet)

A +BX A +BX B+AXB+AX

Single Replacement RulesSingle Replacement Rules

1.1. Active metals replace less active metals Active metals replace less active metals from the less active metals’ compounds from the less active metals’ compounds in aqueous solutionsin aqueous solutionsex. 3Mg+ 2FeClex. 3Mg+ 2FeCl33—> —> 2Fe + 3MgCl2Fe + 3MgCl2 2

2.2. Active metals replace hydrogen in waterActive metals replace hydrogen in waterex. 2Na + 2Hex. 2Na + 2H22OO—>—> H H22 + 2NaOH + 2NaOH

3.3. Active metals replace hydrogen in acids Active metals replace hydrogen in acids ex. 2Li + 2HCl ex. 2Li + 2HCl —>—> H H22 + 2LiCl + 2LiCl

Single Replacement Rules, Single Replacement Rules, contd.contd.

4. Active nonmetals replace less active 4. Active nonmetals replace less active nonmetals from their compounds in nonmetals from their compounds in aqueous solutionsaqueous solutionsex. Clex. Cl22 + 2KI + 2KI —> —> II22 + + 2KCl2KCl

5. If a less reactive element is combined with 5. If a less reactive element is combined with a more reactive element in compound form, a more reactive element in compound form, there will be no reactionthere will be no reactionex. Clex. Cl22 + KF + KF —> —> no reaction*no reaction*

* On the AP test reactions will * On the AP test reactions will ALWAYSALWAYS have have products; it will never be “no reaction.”products; it will never be “no reaction.”

Activity Series (Single Replacement)Activity Series (Single Replacement)

MetalsMetalsLi, Ca, Na, Mg, Al, Zn, Fe, Pb, [HLi, Ca, Na, Mg, Al, Zn, Fe, Pb, [H22], Cu, Ag, Pt ], Cu, Ag, Pt 

NonmetalsNonmetalsFF2,2, Cl Cl2,2, Br Br2,2, I I2,2,

More active More active Less Active Less Active

Double ReplacementDouble Replacement Two compounds react to form two new compounds. No Two compounds react to form two new compounds. No

changes in oxidation numbers occur.changes in oxidation numbers occur. Each cation pairs up with the anion in the other Each cation pairs up with the anion in the other

compound.compound. The “driving force” in these reactions is the removal of at The “driving force” in these reactions is the removal of at

least one pair of ions from solution.least one pair of ions from solution. This removal of ions happens with the formation of a This removal of ions happens with the formation of a

precipitate, gas, or molecular species.precipitate, gas, or molecular species. When a double replacement reaction doesn’t go to When a double replacement reaction doesn’t go to

completion, it is a reversible reaction (no ions have been completion, it is a reversible reaction (no ions have been removed).removed).

AX+ BY AX+ BY AY+ BX AY+ BX

How do you know a double How do you know a double replacement reaction occurs?replacement reaction occurs?

The reactants will contain a(n):The reactants will contain a(n):

-gas-gas

-insoluble precipitate -insoluble precipitate

-molecular species-molecular species

*Remember– on the AP test the reaction will *Remember– on the AP test the reaction will always occuralways occur

Common Gases Released (Dbl. Repl.)Common Gases Released (Dbl. Repl.)

HH22S Any sulfide plus any acid forms S Any sulfide plus any acid forms H2S and a salt. H2S and a salt.

COCO22 Any carbonate plus any acid form Any carbonate plus any acid form COCO33, water, and a salt., water, and a salt.

SOSO22 Any sulfite plus any acid form SO Any sulfite plus any acid form SO22, , water, and a salt.water, and a salt.

NHNH33 Any ammonium plus a soluble Any ammonium plus a soluble hydroxide form NH hydroxide form NH33, water, and a , water, and a

salt. salt.

Acid/ Base Reactions (Dbl. Acid/ Base Reactions (Dbl. Repl.)Repl.)

An acid and a base will react and form An acid and a base will react and form water and a salt.water and a salt.

Hydrochloric acid is added to sodium Hydrochloric acid is added to sodium hydroxide.hydroxide.

HCl + NaOH HCl + NaOH NaCl + H NaCl + H22OO

Hydrolysis (Dbl. Repl.)Hydrolysis (Dbl. Repl.) It is the reverse of neutralization and results when a salt plus a water molecule yields It is the reverse of neutralization and results when a salt plus a water molecule yields

an acid plus a base.an acid plus a base. Salt + water  Salt + water  acid + base  acid + base 

Key things to know about hydrolysis reactions: Key things to know about hydrolysis reactions: Salts of a strong acid plus a weak base will hydrolyze into an acidic solution. Salts of a strong acid plus a weak base will hydrolyze into an acidic solution.

NHNH44+   +Cl+   +Cl--   +H   +H22O   O   →→    H    H++   +Cl   +Cl--   +  (NH)   +  (NH)44OH OH 

Salts of a weak acid and a strong base will always hydrolyze to give a basic Salts of a weak acid and a strong base will always hydrolyze to give a basic solution. solution.

KK+ +   +F  +F--  +H  +H22O O →→  K  K+ +  +OH +OH--   +HF    +HF 

Salts of a strong acid and a strong base will never undergo hydrolysis and Salts of a strong acid and a strong base will never undergo hydrolysis and therefore make a neutral solution. therefore make a neutral solution.

NaNa+  +   +Cl +Cl--  +H  +H22O   O   →→   Na   Na++   +OH   +OH--   +H   +H++   Cl   Cl--  

Salts of a weak acid plus salts of a weak base may hydrolyze as an acid, base, Salts of a weak acid plus salts of a weak base may hydrolyze as an acid, base, or a neutral solution; the final result depends on the Ka’s and Kb’s of the acids or a neutral solution; the final result depends on the Ka’s and Kb’s of the acids and bases formed during the hydrolysis process.and bases formed during the hydrolysis process.

Disclaimer!! The spectator ions were not removed Disclaimer!! The spectator ions were not removed

Examples of Dbl. ReplacementExamples of Dbl. Replacement

Solutions of potassium bromide and silver Solutions of potassium bromide and silver nitrate are mixed.nitrate are mixed.

KBr + AgNOKBr + AgNO33 AgBr + KNO AgBr + KNO33

A solution of sodium sulfate is added to a A solution of sodium sulfate is added to a solution of hydrochloric acid.solution of hydrochloric acid.

NaNa22SOSO33 + 2HCl + 2HCl 2NaCl + H 2NaCl + H22SOSO33

Hydrolysis Sample ProblemsHydrolysis Sample Problems

Try these: Try these: An aqueous solution of manganese (II) sulfate An aqueous solution of manganese (II) sulfate

undergoes hydrolysis. undergoes hydrolysis. Ammonium fluoride and water are mixed Ammonium fluoride and water are mixed

together. together.

Hydrolysis answersHydrolysis answers

MnSOMnSO44 + 2H + 2H22O O →→  H  H22SOSO44 + Mn(OH) + Mn(OH)22

NHNH44F + HF + H22O O →→ HF + NH HF + NH44OHOH

Combustion (Organic Reacs.)Combustion (Organic Reacs.)

An organic compound reacts with OAn organic compound reacts with O2 2 to to form water and carbon dioxide.form water and carbon dioxide.

If something is burned there is a If something is burned there is a combustion reaction.combustion reaction.

Methanol is burned in oxygen gas.Methanol is burned in oxygen gas.2CH2CH33OH + 3OOH + 3O22 4H 4H22O + 2COO + 2CO22

Addition (Organic Reacs.)Addition (Organic Reacs.)

A halogen or hydrogen is added to an A halogen or hydrogen is added to an alkene or alkyne, breaking apart the alkene or alkyne, breaking apart the double or triple bonds and forming single double or triple bonds and forming single bonds.bonds.

Fluorine is added to etheneFluorine is added to etheneFF22 + CH + CH22=CH=CH22 CH CH22F-CHF-CH22FF

Substitution (Organic Reacs.)Substitution (Organic Reacs.)

An atom attached to a carbon is removed An atom attached to a carbon is removed and something else takes its place.and something else takes its place.

Bromine is added to methaneBromine is added to methaneBrBr22 + CH + CH44 CH CH33Br + HBrBr + HBr

Oxidizing Agents (Redox Oxidizing Agents (Redox Reacs.)Reacs.)

Common Oxidizing AgentsCommon Oxidizing Agents

MnOMnO44¯̄ in acidic solution in acidic solution

MnOMnO22 in acidic solution in acidic solution MnOMnO44

¯̄ in neutral or basic solution in neutral or basic solution CrCr22OO77ˉ² in acidic solutionˉ² in acidic solution HNOHNO33, concentrated, concentrated HNOHNO33, dilute, dilute HH22SOSO44, hot, concentrated, hot, concentrated Metallic ions (higher oxidation #)Metallic ions (higher oxidation #) Free halogensFree halogens NaNa22OO22 HClOHClO44 CC22OO44ˉ² ˉ² H H 22OO22

Products FormedMn+²Mn+²MnO2(s)Cr+³NO2

NOSO2

Metallous ions (lower oxidation #)Halide ionsNaOHClˉCO2

O2

Reduction Agents (Redo Reduction Agents (Redo Reacs.)Reacs.)

Common Reducing AgentsCommon Reducing Agents Halide ionsHalide ions Free metalsFree metals Sulfite ions or SOSulfite ions or SO22

Nitrite ionsNitrite ions Free halogens, dilute Free halogens, dilute

basic solutionbasic solution Free halogens, Free halogens,

concentrated basic concentrated basic solutionsolution

Metallous ions (lower Metallous ions (lower oxidation #)oxidation #)

Products FormedFree halogenMetal ionsSulfate ionsNitrate ionsHypohalite ionsHalite ionsMetallic ions (higher oxidation #)

Electrolysis (Redox Reacs.)Electrolysis (Redox Reacs.) An electrolysis reaction is a reaction in which a non-An electrolysis reaction is a reaction in which a non-

spontaneous redox reaction is brought about by the spontaneous redox reaction is brought about by the passage of current under sufficient external electrical passage of current under sufficient external electrical potential. The devices in which electrolysis reactions potential. The devices in which electrolysis reactions occur are called electrolytic cells.occur are called electrolytic cells.

In theory, EIn theory, E° values (Standard Reduction Potentials) can ° values (Standard Reduction Potentials) can be used to predict which element will plate out at a be used to predict which element will plate out at a particular electrode when various solutions are particular electrode when various solutions are combined.combined.

(B&L text)(B&L text)

Rules for Predicting Cathode Rules for Predicting Cathode Reactions (Reduction)Reactions (Reduction)

When a direct electric current is passed When a direct electric current is passed through a water solution of an electrolyte, through a water solution of an electrolyte, two possible reduction processes may two possible reduction processes may occur at the cathode.occur at the cathode.

The cation may be reduced to the The cation may be reduced to the corresponding metal.corresponding metal.

MMn+ n+ + ne+ ne- - M(s) (reaction 1) M(s) (reaction 1) n = (charge of cation)n = (charge of cation)

Water molecule may be reduced to Water molecule may be reduced to elementary hydrogenelementary hydrogen

2H2H22O + 2eˉ O + 2eˉ H2 + 2OHˉ H2 + 2OHˉ (reaction 2) (reaction 2)

Rules for Predicting Cathode Rules for Predicting Cathode Reactions, contd.Reactions, contd.

For salts containing transition metal cations, For salts containing transition metal cations, which are relatively easy to reduced compared which are relatively easy to reduced compared to water, reaction #1 will occur at the cathode to water, reaction #1 will occur at the cathode (and the transition metal will plate out).(and the transition metal will plate out).

MMn+ n+ + ne+ ne- - M(s) M(s) If the cation is representative metal, the water If the cation is representative metal, the water

molecules will be easier to reduce compared to molecules will be easier to reduce compared to the cation, and reaction #2 will occur at the the cation, and reaction #2 will occur at the cathode, producing hydrogen gas and hydrogen cathode, producing hydrogen gas and hydrogen ions.ions.

2H2H22O + 2eˉ O + 2eˉ H2 + 2OHˉ H2 + 2OHˉ

Rules for Predicting Anode Rules for Predicting Anode Reaction (oxidation)Reaction (oxidation)

The oxidation process that occurs at the anode of an The oxidation process that occurs at the anode of an electrolytic cell operating in aqueous solution may be electrolytic cell operating in aqueous solution may be one of two oxidation processes.one of two oxidation processes.

The anion may be oxidized to the corresponding The anion may be oxidized to the corresponding nonmetal.nonmetal.

- 2X- 2Xˉ ˉ X X2 2 + 2eˉ (reaction 1)+ 2eˉ (reaction 1) Water molecules may be oxidized to elementary oxygen.Water molecules may be oxidized to elementary oxygen.

- HOH - HOH ½ O ½ O2 2 + 2H+ 2H++ + 2eˉ (reaction 2) + 2eˉ (reaction 2)

Rules for Predicting Anode Rules for Predicting Anode Reactions, contd.Reactions, contd.

For salts containing iodide, bromide, or chloride For salts containing iodide, bromide, or chloride ions, it is usually easier to oxidize these ions, it is usually easier to oxidize these nonmetals rather than water. It will be found that nonmetals rather than water. It will be found that the nonmetal is formed at the anode.the nonmetal is formed at the anode.

When the anion present is any other ion that is When the anion present is any other ion that is more difficult to oxidize than water, Reaction #2 more difficult to oxidize than water, Reaction #2 will occur at the anode producing elementary will occur at the anode producing elementary oxygen and aqueous hydrogen ions.oxygen and aqueous hydrogen ions.

Example Electrolysis ReactionsExample Electrolysis Reactions

1.1. Copper (II) chloride in waterCopper (II) chloride in waterCuCu+2 +2 + 2Cl+ 2Clˉ ˉ Cu + Cl Cu + Cl22

2. Copper (II) sulfate in water 2. Copper (II) sulfate in water CuCu+2+2 + HOH + HOH Cu + ½ O Cu + ½ O22 + 2H + 2H+ +

3. Sodium chloride in water 3. Sodium chloride in water 2Clˉ + 2HOH 2Clˉ + 2HOH H H2 2 + Cl+ Cl2 2 + 2OHˉ+ 2OHˉ

4. Sodium sulfate in water 4. Sodium sulfate in water 2HOH 2HOH 2H 2H2 2 + O+ O22

Metals w/ Multiple Oxidation Levels Metals w/ Multiple Oxidation Levels (Redox Reacs.)(Redox Reacs.)

These metals can change their oxidation state in a redox reactionThese metals can change their oxidation state in a redox reaction Antimony (III) or (V)Antimony (III) or (V) Bismuth (III) or (IV)Bismuth (III) or (IV) Cerium (III) or (IV)Cerium (III) or (IV) Chromium (II) or (III)Chromium (II) or (III) Cobalt (II) or (III)Cobalt (II) or (III) Copper (I) or (II)Copper (I) or (II) Gallium (I) or (II) or (III)Gallium (I) or (II) or (III) Germanium (II) or (IV)Germanium (II) or (IV) Gold (I) or (III)Gold (I) or (III) Iron (II) or (III)Iron (II) or (III) Lead (II) or (IV)Lead (II) or (IV) Mercury (I) or (II)Mercury (I) or (II) Nickel (II) or (III)Nickel (II) or (III) Thallium (I) or (III)Thallium (I) or (III) Thorium (II) or (IV)Thorium (II) or (IV) Tin (II) or (IV)Tin (II) or (IV)

Tin (II) sulfate is added to iron (III) sulfateTin (II) sulfate is added to iron (III) sulfate SnSO4 + Fe2(SO4)3 SnSO4 + Fe2(SO4)3 Sn(SO4)2 + 2FeSO4Sn(SO4)2 + 2FeSO4

Complex Ion ReactionsComplex Ion Reactions Nomenclature is on pages 23-27 of The Ultimate Nomenclature is on pages 23-27 of The Ultimate

Chemical Equations HandbookChemical Equations Handbook There are a lot of very complicated types of these There are a lot of very complicated types of these

reactions, but, for all intensive purposes and for the AP reactions, but, for all intensive purposes and for the AP test, you only need to be familiar with those reactions test, you only need to be familiar with those reactions pertaining to ammonia and water.pertaining to ammonia and water.

In a complex ion reaction, ligands will attach to a In a complex ion reaction, ligands will attach to a transition metal ion.transition metal ion.

There will usually be twice as many ligands as the There will usually be twice as many ligands as the metals oxidation numbermetals oxidation number

Complex Ion Reactions, contd.Complex Ion Reactions, contd.

These reactions usually occur in a These reactions usually occur in a concentrated solution of the ligand.concentrated solution of the ligand.

Copper chloride (II) is added to a Copper chloride (II) is added to a concentrated solution of ammoniaconcentrated solution of ammoniaCuCu2+2+ +NH +NH33 [Cu(NH [Cu(NH33))44]]2+2+

Common Reaction TermsCommon Reaction Terms Electrolysis: Electricity is run through a compound, Electrolysis: Electricity is run through a compound,

resulting in a change of oxidation states.resulting in a change of oxidation states. Hydrolysis: The reaction of a salt with water to form Hydrolysis: The reaction of a salt with water to form

molecular species. Salts of a strong acid + a weak base molecular species. Salts of a strong acid + a weak base will always hydrolyze to give an acidic solution.will always hydrolyze to give an acidic solution.

Neutralization: Acid and base react to form a salt and Neutralization: Acid and base react to form a salt and water.water.

Catalyst: A molecule that speeds that speeds a reaction Catalyst: A molecule that speeds that speeds a reaction but that does not appear in the reaction.but that does not appear in the reaction.

Oxidation number: the charge that it would have if all the Oxidation number: the charge that it would have if all the ligands (atoms that donate electrons) were removed ligands (atoms that donate electrons) were removed along with the electron pairs that were shared with the along with the electron pairs that were shared with the central atom central atom

Common Reaction Terms, Common Reaction Terms, contd.contd.

Precipitate: an insoluble substance formed Precipitate: an insoluble substance formed by the reaction of two aqueous by the reaction of two aqueous substances.substances.

Anode: the electrode where oxidation Anode: the electrode where oxidation occursoccurs an oxan ox

Cathode: the electrode where reduction Cathode: the electrode where reduction occursoccurs red catred cat

By: Will Lambert, Adam Robinson, By: Will Lambert, Adam Robinson, Michelle Klassen, and Tori Waldron Michelle Klassen, and Tori Waldron

(APChem ‘06-’07) (APChem ‘06-’07)