Ap Chemistry--Predicting Reactions

Front 1

NONMETAL OXIDE + H2O

Back 1

ACID

Front 2

METAL OXIDE + H20

Back 2

BASE

Front 3

METAL OXIDE + NONMETAL OXIDE

Back 3

SALT (OF AN OXYANION)

Front 4

ACID + BASE

Back 4

SALT + H2O

Front 5

SALT (WITH OXYANION) heat------>

Back 5

METAL OXIDE + NONMETAL OXIDE

Front 6

METAL CARBONATE + ACID

Back 6

SALT + H2O + CO2

Front 7

METAL SULFATE + ACID

Back 7

SALT + H2O + SO2

Front 8

POSITIVE ION + NEGATIVE ION

Back 8

INSOLUBLE SALT

Front 9

METAL + NONMETAL

Back 9

BINARY COMPOUND

Front 10

ACTIVE METAL + ACID

Back 10

SALT + H2

Front 11

HYDROGEN + COMPOUND OF LESS ACTIVE METAL

Back 11

METAL + HYDROGEN COMPOUND

Front 12

ACTIVE METAL (NONMETAL) + COMPOUND OF LESS ACTIVE METAL (NONMETAL)

Back 12

LESS ACTIVE METAL (NONMETAL) + COMPOUND OF ACTIVE METAL (NONMETAL)

Front 13

HYDROCARBON + EXCESS OXYGEN

Back 13

H2O + CO2

THIS IS A COMBUSTION REACTION

Front 14

HYDROCARBON + LIMITED OXYGEN

Back 14

H2O + CO

COMBUSTION WITH NOT ENOUGH OXYGEN TO PRODUCE CO2

Front 15

GROUP I & II NITRIDES + H2O

Back 15

METALLIC HYDROXIDE + NH3

Front 16

SPECIAL CASE: COMPLEX ION FORMATION:

ALUMINUM PELLETS ARE ADDED TO AN EXCESS OF CONCENTRATED POTASSIUM HYDROXIDE

Back 16

Al + OH- ---> [Al(OH)4] 1- OR Al + OH- ---> [Al(OH)6]3-

HOWEVER, WHEN YOU GO TO BALANCE THESE RACTIONS, YOU WILL NOTICE THAT YOU CANNOT GET THEM TO BALANCE. WHAT ELSE IS HAPPENING IS THAT A REDOX REAX IS ALSO OCCURRING AT THE SAME TIME, THE WATER FROM THE AQUEOUS SOLUTION IS BEING REDUCED FROM H2O TO H2; THE ALUMINUM IS BEING OXIDIZED FROM Al TO Al+3. THE REAL EQUATIONS ARE:

2 Al + 2 OH- + 6H2O ---> 2[Al(OH)4]1- + 3 H2
2 Al + 6 OH- + 6 H2O --> 2[Al(OH)6]3- + 3 H2

Front 17

4 RULES FOR WRITING EQUATIONS:

Back 17

1. YOU DONT HAVE TO WRITE THE PHASES
2. YOU HAVE TO WRITE BALANCED EQUATIONS WITH THE LOWEST WHOLE NUMBER COEFFICIENTS
3. SUBSTANCES THAT DISSOCIATE EXTENSIVELY SHOULD BE WRITTEN AS IONS
EX: NANO3 IONIZES, SO IT SHOULD BE WRITTEN AS Na+ AND NO3-

AgCl DOES NOT IONIZE, SO IT SHOULD BE WRITTEN AS AgCl

Ca(OH)2 IONIZES TO SOME EXTENT, SO EITHER Ca(OH)2 OR Ca2+ AND 2 OH- ARE ACCEPTABLE

4. LEAVE OUT ANY MOLECULES OR IONS THAT ARE NOT CHANGED IN THE REACTION (SPECTATOR IONS)
EX: Mg2+ + 2Cl- + 2Ag+ + 2NO3- ----> Mg2+ 2 NO3- +2 AgCl

LEAVING OUT SPECTATOR IONS LEAVES:
Ag+ + Cl- ----> AgCl
NOTICE THAT THE FINAL REACTION USES THE LOWEST WHOLE NUMBER COEFFICIENTS

Front 18

LOOOK FOR 2 UNCOMBINED ELEMENTS AND COMBINE THEM:

1. HYDROGEN GAS IS BURNED IN AIR

2. DESCRIBE THE ENTHALPY CHANGE IN THIS REACTION

Back 18

2 H2 + O2 ---> 2 H2O

2. THE REACTION IS EXOTHERMIC. ENERGY IS BEING RELEASED.

Front 19

A. SOLID SULFUR IS BURNED IN OXYGEN
B. WHAT IS THE OXIDATION STATE OF SOLID SULFUR BEFORE AND AFTER THE REACTION?

Back 19

S + O2 ----> SO2

B. THE OXIDATION STATE OF AN UNCOMBINED ELEMENT IS ALWAYS 0, SO SULFUR HAS AN OX STATE OF 0 BEFORE THE REACTION. AFTER IT COMBINES WITH OXYGEN, SULFUR HAS AN OXIDATION STATE OF +4

Front 20

A. SOLID MAGNESIUM IS HEATED TO NITROGEN GAS.

B. IS THIS AN OXIDATION REDUCTION (REDOX) REACTION? EXPLAIN.

Back 20

3 Mg + N2 ---> Mg3N2

B. YES. MAGNESIUM GIVES UP ELECTRONS AND IS OXIDIZED, WHILE NITROGEN GAINS ELECTRONS AND IS REDUCED.

Front 21

A PIECE OF SOLID ZINC IS HEATED IN CHLORINE GAS.

B. DESCRIBE THE BONDING PRESENT IN THE
PRODUCT(S) OF THIS REACTION.

Back 21

Zn + Cl2 ----> ZnCl2


B. ZINC CHLORIDE CONTAINS A METAL AND A NON-METAL, SO IT IS HELD TOGETHER BY IONIC BONDS.

Front 22

A PIECE OF SOLID BARIUM IS PLACED IN OXYGEN GAS.

B. IS THE ENTROPY CHANGE FOR THIS REACTION POSITIVE OR NEGATIVE?

Back 22

2 Ba + O2 ------> 2 BaO

B. NEGATIVE. THE NUMBER OF MOLES DECREASES FROM REACTANTS TO PRODUCTS AND A GAS PHASE REACTANT IS INCORPORATED INTO A SOLID.

Front 23

A PIECE OF SOLID SODIUM IS PLACED IN HYDROGEN GAS.

B. DESCRIBE THE BONDING PRESENT IN SOLID SODIUM.

Back 23

2 Na + H2 --------> 2 NaH


B. SOLID SODIUM IS HELD TOGETHER BY METALLIC BONDING.

Front 24

LOOK FOR A SINGLE REACTANT: IF THERE IS ONLY ONE REACTANT, ALL IT CAN DO IS BREAK UP IN A DECOMPOSITION REACTION, SO YOU'RE GUARANTEED THE REACTANT PARTIAL CREDIT POINT. DECOMPOSITION REACTIONS USUALLY PRODUCE SIMPLE SALTS AND OXIDE GASES:

A SOLUTION OF HYDROGEN PEROXIDE IS PLACED UNDER A BRIGHT LIGHT.

B. WHAT ARE THE OXIDATION STATES OF HYDROGEN AND OXYGEN IN HYDROGEN PEROXIDE?

Back 24

2 H2O2 ----> 2 H2O + O2

B. HYDROGEN IS +1 AND OXYGEN IS -1.

Front 25

SOLID CALCIUM CARBONATE IS HEATED.

B. CALCIUM CARBONATE CONTAINS BOTH IONIC AND COVALENT BONDS. EXPLAIN.

Back 25

CaCO3 ----> CaO + CO2

B. THE CARBON AND OXYGEN ATOMS IN THE CARBONATE ION (CO3-) ARE HELD TOGETHER BY COVALENT BONDS. THE CALCIUM ION AND THE CARBONATE ION ARE HELD TOGETHER BY AN IONIC BOND.

Front 26

SOLID POTASSIUM CHLORATE IS HEATED IN THE PRESENCE OF A CATALYST.

B. HOW DOES THE CATALYST AFFECT THE ACTIVATION ENERGY OF THE REACTION?

Back 26

2 KClO3 ----> 2 KCl + 3 O2


B. THE CATALYST SPEEDS THE REACTION BY LOWERING THE ACTIVATION ENERGY

Front 27

A SAMPLE OF SOLID AMMONIUM CARBONATE IS HEATED.

B. DESCRIBE THE POLARITY OF THE PRODUCTS OF THIS REACTION.

Back 27

(NH4)2CO3 ---> 2 NH3 + CO3 + H20

B. AMMONIA (NH3) AND WATER (H20) ARE POLAR MOLECULES. CARBON DIOXIDE (CO2) IS NONPOLAR.

Front 28

A PIECE OF SOLID POTASSIUM NITRATE IS HEATED.

B. WHAT IS THE OXIDATION NUMBER OF NITROGEN BEFORE AND AFTER THE REACTION?

Back 28

2 KNO3 ---> 2 KNO2 + O2

B. NITROGEN HAS AN OX NUMBER OF +5 IN KNO3 AND AN O NUMBER OF +3 IN KNO2.

Front 29

LOOK FOR WATER AS A REACTANT: WHEN METALS AND NONMETALS REACT WITH WATER, THEY TEND TO REACT IN PREDICTABLE WAYS. IN GENERAL, METALS REACT WITH WATER TO FORM BASES AND NONMETALS REACT WITH WATER TO FORM ACIDS.

A PURE METAL OR A METAL HYDRIDE IN WATER WILL PRODUCE A BASE AND HYDROGEN GAS.

SODIUM METAL IS ADDED TO DISTILLED WATER.

B. SPARKS ARE OBSERVED AS THE REACTION PROGRESSES. IDENTIFY THE PRODUCT OF THE REACTION THAT UNDERGOES COMBUSTION TO PRODUCE SPARKS.

Back 29

2 Na + 2 H2O ---> 2 Na+ + 2 OH- + H2


B. HYDROGEN GAS (H2) IS EXTREMELY FLAMMABLE AND CAN BURN IN THIS REACTION.

Front 30

CALCIUM METAL IS ADDED TO DISTILLED WATER.

B. THE REACTION TAKES PLACE IN A FLASK AND THE pH IS MONITORED. DOES THE pH INCREASE OR DECREASE AS THE REACTION PROCEEDS? EXPLAIN.

Back 30

Ca + 2 H2O ---> Ca(OH)2 + H2

B. THE pH INCREASES BECAUSE CALCIUM HYDROXIDE, A BASE, IS PRODUCED IN THE REACTION.

Front 31

SOLID CALCIUM HYDRIDE IS ADDED TO WATER.

B. WHAT IS THE OXIDATION STATE OF CALCIUM BEFORE THE REACTION TAKES PLACE? IS CALCIUM OXIDIZED OR REDUCED DURING THE REACTION?

Back 31

CaH2 + H2O -----> Ca(OH)2 + 2 H2

B. THE OX STATE OF Ca IS +2 BEFORE THE REACTION, AND +2 AFTER THE REACTION, SO THE CALCIUM IS NEITHER OXIDIZED NOR REDUCED.

Front 32

SOLID LITHIUM HYDRIDE IS ADDED TO DISTILLED WATER.

B. ELECTRODES ATTTACHED TO A BATTERY AND A LIGHT BULB ARE PLACED IN THE SOLUTION. WILL THE LIGHT BULB SHINE BRIGHTER OR DIMMER AS THE REACTION PROGRESSES?

Back 32

LiH + H2O ---> Li+ + OH- + H2


B. THE BULB WILL GROW BRIGHTER BECAUSE THE REACTION IS PRODUCING CHARGED PARTICLES WHICH WILL CONDUCT ELECTRICITY THROUGH THE SOLUTION.

Front 33

A METAL OXIDE IN WATER WILL PRODUCE A BASE.

METAL OXIDES ARE CALLED BASIC ANHYDRIDES BECAUSE THEY PRODUCE BASES WHEN ADDED TO WATER.

SOLID POTASSIUM OXIDE IS ADDED TO WATER.

B. WILL THE FREEZING POINT OF THE AQUEOUS SOLUTION THAT RESULTS FROM THIS REACTION BE HIGHER OR LOWER THAN THAT OF PURE WATER?

Back 33

K2O + H2O ---> 2 K+ + 2 OH-

B. THE FREEZING POINT WILL BE LOWER BECAUSE PARTICLES OF ANY KIND ADDED TO PURE WATER WILL CAUSE FREEZING POINT DEPRESSION.

Front 34

SOLID BARIUM OXIDE IS ADDED TO WATER

B. A SPLINT DIPPED IN THE SOLUTION RESULTING FROM THIS REACTION WILL PRODUCE A GREEN FLAME. IDENTIFY THE PRODUCT OF THE REACTION THAT BURNS TO PRODUCE THE FLAME.

Back 34

BaO + H2O ---> Ba2+ + 2 OH-

B. BARIUM ION (Ba2+) PRODUCES A GREEN FLAME IN A FLAME TEST.

Front 35

SOLID CALCIUM OXIDE IS ADDED TO WATER.

B. DESCRIBE THE CHANGE THAT TAKES PLACE IN THE CONCENTRATION OF HYDROGEN IONS IN THE SOLUTION AS THE REACTION PROGRESSES? EXPLAIN.

Back 35

CaO + H2O -----> Ca(OH)2

B. THE HYDROGEN ION CONCENTRATION DECREASES BECAUSE THE PRODUCT OF THE REACTION IS A BASE.

Front 36

FLAME TEST COLORS:

BARIUM--
SODIUM--
COPPER--
POTASSIUM--
STRONTIUM--
LITHIUM--
CALCIUM--

Back 36

BARIUM--GREEN
SODIUM--YELLOW
COPPER--BLUE (W/ GREEN)
POTASSIUM--LAVENDER
STRONTIUM--RED
LITHIUM--RED
CALCIUM--ORANGE

Front 37

A NONMETAL OXIDE IN WATER WILL PRODUCE AN ACID.--- NONMETAL OXIDES ARE CALLED ACID ANHYDRIDES BECAUSE THEY PRODUCE ACIDS IN WATER.

SOLID DINITROGEN PENTOXIDE IS ADDED TO WATER

B. DESCRIBE THE CHANGE IN THE pH OF THE SOLUTION AS THE REACTION PROGRESSES. EXPLAIN.

Back 37

N2O5 + H2O ---> 2H+ + 2NO3-

THE pH OF THE SOLUTION WILL DECREASE BECAUSE THE PRODUCT OF THE REACTION IS AN ACID.

Front 38

CARBON DIOXIDE GAS IS BUBBLED THROUGH WATER.

B. BRIEFLY EXPLAIN HOW NON-METAL OXIDES CAUSE ACID RAIN

Back 38

CO2 + H2O ---> H2CO3

B. NON-METAL OXIDES ARE ACID ANHYDRIDES. THEY REACT WITH WATER IN THE ATMOSPHERE TO MAKE RAIN WATER ACIDIC.

Front 39

SOLID PHOSPHORUS PENTOXIDE IS ADDED TO DISTILLED WATER.

B. HOW MANY MOLES OF PRODUCTS ARE PRODUCED WHEN 4 MOLES OF PHOSPHORUS PENTOXIDE REACT WITH EXCESS WATER?

Back 39

P2O5 + 3 H2O --> 2 H3PO4

B. FROM THE BALANCED EQUATION, 4 MOLES OF P2O5 PRODUCE 8 MOLES OF H3PO4.

Front 40

SULFUR DIOXIDE GAS IS BUBBLED THROUGH WATER.

B. WHAT IS THE OXIDATION STATE OF SULFUR BEFORE THE REACTION? WHAT IS THE OXIDATION STATE OF SULFUR AFTER THE REACTION? IS SULFUR OXIDIZED DURING THE REACTION?

Back 40

SO2 + H2O ----> H2SO3

B. THE OXIDATION STATE OF SULFUR IS +4 BEFORE AND AFTER THE REACTION, SO SULFUR IS NEITHER OXIDIZED NOR REDUCED.

Front 41

SULFUR TRIOXIDE GAS IS BUBBLED THROUGH WATER.

B. HOW MANY MOLES OF WATER ARE REQUIRED TO REACT WITH 3 MOLES OF SULFUR TRIOXIDE GAS?

Back 41

SO3 + H2O ---> H+ + HSO4-
H+ + OH- ---> H2O
-----------------------------------
SO3 + OH- --------> HSO4-

FROM THE BALANCED EQUATION, 3 MOLES OF H2O WILL REACT WITH 3 MOLES OF SO3

Front 42

LIST THE 8 TYPES OF REACTIONS YOU MAY ENCOUNTER ON THE TEST:

Back 42

1. TWO UNCOMBINED ELEMENTS----> COMBINE THEM
2. A SINGLE REACTANT-----> DECOMPOSITION
3. WATER AS A REACTANT:
TYPE A. PURE METAL OR A METAL HYDRIDE IN WATER-----> BASE + HYDROGEN GAS (H2)
TYPE B: A METAL OXIDE (AKA BASIC ANHYDRIDE)IN WATER-----> BASE
TYPE C: A NONMETAL OXIDE IN WATER-------> ACID
4. ACID-BASE NEUTRALIZATION
TYPE A: EQUAL MOLAR AMOUNT OF AN ACID AND BASE---> STRONG ACID AND STRONG BASE (COMPLETE NEUTRALIZATION = pH 7)
TYPE B: WEAK ACID AND STRONG BASE----->pH GREATER THAN 7 BECAUSE EQUIMOLAR SOLUTIONS OF A STRONG BASE AND WEAK ACID WILL REACT TO FORM A BASIC SOLUTION.
TYPE C: STRONG ACID AND WEAK BASE----> pH LESS THAN 7
TYPE D: WEAK ACID AND WEAK BASE----->CONJ ACID BASE PAIRS
TYPE E: AN ACID AND A BASIC SALT
TYPE F: A BASE AND AN ACID SALT
TYPE G: AN ACID ANHYDRIDE AND A BASE-----> JUST LIKE OTHER ACID-BASE NEUTRALIZATIONS
5. MIXTURE OF 2 SALT SOLUTIONS-----> WHO PRECIPITATES?
6. COMBUSTION OF CARBON COMPOUND
7. SOLID TRANSITION METAL PLACED IN SOLUTION:
REDOX REACTION AND THE SOLID METAL WILL ALWAYS BE OXIDIZED. 2 VARIATIONS:
TYPE A: SOLUTION IS A NEUTRAL TRANSITION METAL SALT SOLUTION------>METAL ION IN SOLUTION WILL BE REDUCED
TYPE B: THE SOLUTION IS A STRONG OXOACID SOLUTION---->THE ANION OF THE OXOACID WILL BE REDUCED TO AN OXIDE GAS AND WATER WILL FORM.

8. TRANSITION METAL IONS IN SOLUTION WITH AMMONIA, HYDROXIDE, CYANIDE OR THIOCYANATE----->COMPLEX IONS

Front 43

carbon dioxide gas and ammonia gas are bubbled into distilled water.

B. describe the polarity of carbon dioxide, ammonia, and water

Back 43

CO2 + H2O ----> H2CO3
H2CO3 + NH3 -----> HCO3- + NH4+
______________________________________
CO2 + H2O + NH3 ------> HCO3- + NH4+

carbon dioxide is nonpolar. Ammonia and water are polar.

Front 44

Look for a mixture of 2 salt solutions: For these questions, you have to predict which salt precipitates. YOU MUST KNOW YOUR SOLUBILITY RULES!:

SOLUTIONS OF CALCIUM NITRATE AND SODIUM SULFATE ARE MIXED

B. IS THE ENTROPY CHANGE FOR THIS REACTION POSITIVE OR NEGATIVE? EXPLAIN.

Back 44

Ca2+ + SO4 2- ----> CaSO4

the enthalpy change is negative BECAUSE AQUEOUS PARTICLES ARE COMBINING AND PRECIPITATING AS A SOLID

Front 45

A SOLUTION OF SILVER NITRATE IS ADDED TO A SOLUTION OF POTASSIUM IODIDE.

IDENTIFY THE SPECTATOR IONS IN THIS REACTION.

Back 45

Ag+ + I- ----> AgI

SPECTATOR IONS: K+ AND NO3-

Front 46

SOLUTIONS OF LEAD (II) NITRATE AND TRI-POTASSIUM PHOSPHATE ARE MIXED.

B. IF 0.6 MOLES OF LEAD (II) NITRATE ARE CONSUMED IN THIS REACTION, HOW MANY MOLES OF PRODUCTS ARE PRODUCED?

Back 46

3 Pb2+ + 2 PO4 3- ----> Pb3(PO4)2


FROM THE BALANCED EQUATION, IF 3 MOLES OF
Pb(NO3)2 ARE CONSUMED, THEN 1 MOLE OF
Pb3(PO4)2 IS PRODUCED. SO, IF 0.6 MOLES ARE CONSUMED, THEN 0.2 MOLES ARE PRODUCED.

Front 47

A SOLUTION OF AMMONIUM SULFIDE IS ADDED TO A SOLUTION OF MAGNESIUM IODIDE.

IDENTIFY THE BONDING IN THE PRODUCTS OF THIS REACTION

Back 47

Mg2+ + S2- ------> MgS

MgS IS HELD TOGETHER BY IONIC BONDS

Front 48

LOOK FOR THE COMBUSTION OF A CARBON COMPOUND: carbon cmpds always burn to form oxide gases. even if you cant get the reactant formula from the name of a hydrocarbon cmpd, you can probably get the 2 product points by knowing that it produces carbon dioxide and water when it burns.

ethane is burned in oxygen

if equal molar quantities of ethane and oxygen are combined, which will be the limiting reactant?

Back 48

2 C2H6 + 7 O2 ----> 4 CO2 + 6 H2O

oxygen; 3.5 moles of oxygen are required for each mole of ethane, so oxygen will run out first.

Front 49

methanol is burned in air.

is the enthalpy change of the reaction positive or negative? Explain.

Back 49

2CH3OH + 3O2 -----> 2CO2 + 4H2O


the enthalpy change is negative. combustion releases energy, so it is exothermic.

Front 50

carbon disulfide is burned in excess oxygen

describe the molecular geometry of the products of this reaction.

Back 50

CS2 + 3 O2 ----> CO2 + 2 SO2

CO2 is linear and SO2 is bent

the word "excess" is there to indicate that there is enough oxygen to form CO2, rather than CO.

Front 51

Look for a solid transition metal placed in solution: this will be a REDOX REACTION and the solid metal will always be oxidized. There are 2 variations of this reaction:

1. the solution is a neutral transition metal salt solution: the metal ion will be reduced.

solid manganese flakes are placed in a solution of copper (II) sulfate.

identify the oxidizing and reducing agents in the reaction.

2. the solution is a strong oxoacid solution: the anion of the oxoacid will be reduced to an oxide gas and water will form:

a piece of copper is immersed in concentrated warm sulfuric acid.

what is the oxidation state of sulfur before the reaction? what is the oxidation state of sulfur after the reaction?

Back 51

type 1:

Mn + Cu2+ -----> Mn 2+ + Cu

Mn is ox, so it is the red agent. Cu2+ is reduced, so it is the ox agent.

Type 2: Cu + 3 H+ + HSO4- ----> Cu2+ + SO2 + 2H2O

the ox state of sulfur before the reaction is +6. The oxidation state after the reaction is +4.

Front 52

a piece of solid nickel is placed in a solution of silver nitrate.

if the solid nickel was placed in 0.50 L of a 0.40 M silver nitrate solution and the reaction went to completion, how many grams of nickel were consumed?

Back 52

(this is a solid transition metal in solution type 1--redox)

Ni + 2 Ag+ ----> Ni 2+ + 2 Ag

there are 0.5 L x 0.4 M = 0.2 mole of silver, so from the balanced equation, 0.1 mole of nickel was consumed. (0.1 mole)(59 g/mol) = 5.9 grams of nickel.

Front 53

a bar of zinc is immersed in a solution of silver nitrate

describe the oxidation state of zinc before and after the reaction

Back 53

Type 1 redox.

Zn + 2 Ag+ ----> Zn 2+ + 2 Ag

before the reaction, Zn has an ox state of 0. after the reaction, the oxidation state is +2.

Front 54

a piece of silver is placed in dilute nitric acid

if the reaction above took place in a battery and one mole of silver was consumed, how much charge was generated?

Back 54

type 2 redox: the solution is a strong oxoacid solution: the anion of the oxoacid will be reduced to an oxide gas and water will form:

3 Ag + 4 H+ + NO3- ---> 3 Ag+ + NO + 2 H2O

if one mole of silver was consumed, then one mole of electrons was transferred. the charge on one mole of electrons is one Faraday, or 96,500 C.

Front 55

Look for transition metal ions in solution with ammonia, hydroxide, cyanide, or thiocyanate: transition metal ions form complex ions with those species. it doesnt matter how many of them you place on the transition metal, as long as you get the charge on the complex ion right:

excess ammonia is added to solution of silver nitrate

identify the Lewis base in the reaction. Explain.

Back 55

Ag+ + 2 NH3 -----> Ag(NH3)2+

ammonia acts as the Lewis base because it donates an electron pair to the silver ion.

Front 56

a solution of sodium cyanide is added to a solution of iron (II) chloride.

identify the spectator ions in the reaction.

Back 56

complex ion reaction

Fe 2+ + 6 CN- -------> Fe(CN)6 4-

sodium ion (Na+) and chloride ion (Cl-) are the spectator ions

Front 57

a solution of potassium thiocyanate is added to a solution of copper (II) chloride.

briefly explain why solutions containing transition metal ions tend to be brightly colored.

Back 57

complex ion reaction

Cu 2+ + SCN- -------> Cu(SCN)+

the intervals between energy levels of the d-subshell electrons correspond to the energy levels of visible light. so when these electrons make energy transitions, electromagenetic radiation in the visible spectrum is released.

Front 58

How different values of enthalpy and entropy affect spontaneity:

^H ^S T ^G
- + low -
high -

+ - low +
high +

+ + low +
high -

- - low -
high +

Back 58

1st set (-, -) : always spontaeous

2nd set (++): never spontaeous

3rd set (+, -): not spontaneous at low temp, spontaneous at high temp

4th set (-, +): spontaneous at low temp, not spontaneous at high temp

Front 59

8 reaction types

Back 59

1. TWO UNCOMBINED ELEMENTS----> COMBINE THEM
2. A SINGLE REACTANT-----> DECOMPOSITION
3. WATER AS A REACTANT:
TYPE A. PURE METAL OR A METAL HYDRIDE IN WATER-----> BASE + HYDROGEN GAS (H2)
TYPE B: A METAL OXIDE (AKA BASIC ANHYDRIDE)IN WATER-----> BASE
TYPE C: A NONMETAL OXIDE IN WATER-------> ACID
4. ACID-BASE NEUTRALIZATION
TYPE A: EQUAL MOLAR AMOUNT OF AN ACID AND BASE---> STRONG ACID AND STRONG BASE (COMPLETE NEUTRALIZATION = pH 7)
TYPE B: WEAK ACID AND STRONG BASE----->pH GREATER THAN 7 BECAUSE EQUIMOLAR SOLUTIONS OF A STRONG BASE AND WEAK ACID WILL REACT TO FORM A BASIC SOLUTION.
TYPE C: STRONG ACID AND WEAK BASE----> pH LESS THAN 7
TYPE D: WEAK ACID AND WEAK BASE----->CONJ ACID BASE PAIRS
TYPE E: AN ACID AND A BASIC SALT
TYPE F: A BASE AND AN ACID SALT
TYPE G: AN ACID ANHYDRIDE AND A BASE-----> JUST LIKE OTHER ACID-BASE NEUTRALIZATIONS
5. MIXTURE OF 2 SALT SOLUTIONS-----> WHO PRECIPITATES?
6. COMBUSTION OF CARBON COMPOUND
7. SOLID TRANSITION METAL PLACED IN SOLUTION:
REDOX REACTION AND THE SOLID METAL WILL ALWAYS BE OXIDIZED. 2 VARIATIONS:
TYPE A: SOLUTION IS A NEUTRAL TRANSITION METAL SALT SOLUTION------>METAL ION IN SOLUTION WILL BE REDUCED
TYPE B: THE SOLUTION IS A STRONG OXOACID SOLUTION---->THE ANION OF THE OXOACID WILL BE REDUCED TO AN OXIDE GAS AND WATER WILL FORM.
8. TRANSITION METAL IONS IN SOLUTION WITH AMMONIA, HYDROXIDE, CYANIDE OR THIOCYANATE----->COMPLEX IONS