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370 Cards in this Set

  • Front
  • Back
1.
2.
Decomposition: Breaks substance down into two or more substances (ABA+B)
3.
Single Replacement: Active element takes the place of a less active element in a compound (A + BZ  B+ AZ)
4.
Double Replacement: Two compounds switch partners with each other
a)
Elements only switch with other elements in single and double replacements if the metal by itself is more reactive than the element combined to another element
- The number of moles of a compound on one side to the number of moles of a
- Add the mass of each individual element in the compound
•
•
Write the equation out
•
Count the number ions of the elements on both sides of the equation
•
Adjust the coefficients to make the same number on both sides
•
NO + O2  NO2 will become 2NO + O2  2 NO2
CHEM ch8:5 Be able to go from grams to moles and moles to grams
•
•
Given Moles x Gram Formula Mass
•
•
Ex. Pb(NO3)2(aq) + K2CrO4(aq)  PbCrO4 (s) + 2 KNO3 will become: Pb2+(aq) + 2NO3-(aq) + 2K+(aq) + CrO42-(aq)  PbCrO4(s) + 2K+ + 2NO3-(aq)
•
Spectator ions: elements that do not change from the reactant to the product
o
2K+ and 2NO3-
•
Net Ionic Equation: Shows the ions in the equation excluding spectator ions
o
Pb2+ (aq) + CrO42-(aq)  PbCrO4(s)
Know how to do the problems on page 2 of the Chapter 8 test
•
•
one mole of gas at STP (number of moles x 22.4L/1 Mole)
CHEM ch 9: 4 Gas Laws and Concepts
•
•
Boyle’s Law: P1V1 = P2V2
•
Gay-Lussac’s Law: P1 = P2
•
Combined Gas Law: P1V1 = P2V2
CHEM ch9:5 Molar Volume:
The volume occupied by Avogadro’s number of molecules of gas at STP
CHEM ch9:6 Law of Combining Volumes:
The volumes of reacting gases and their gaseous products are expressed in small whole numbers
CHEM ch9:7 Barometer:
Instrument used to measure atmospheric pressure
CHEM ch9:8 Dalton’s Law of Partial Pressures:
total pressure of a mixture equals sum of partial pressures
CHEM ch9:9 Permeability:
gases easily mingle with other substances
CHEM ch9:10 Elasticity:
Collisions of gas molecules conserve energy
CHEM ch9:11 Diffusion:
Gas molecules move constantly to uniform fill their container
CHEM ch9:12 Compressibility:
High pressures squeeze gases into smaller volumes
CHEM ch9:13 Expansibility:
gas quickly expands to fill low pressure regions
•
•
o
Bonds between polar molecule
•
o
Hydrogen is very positive and small so it can connect to other molecules
•
o
Atoms are more negative on one side for a split second
o
Bigger molecules have greater dispersion forces
•
•
Latent: Form of heat that causes a phase change
CHEM ch10:3 Heat of Vaporization:
amount of energy needed to heat one gram of a substance from a liquid to a gas (no temperature change)
•
540 cal/g in water (Heat of Vaporization x Mass)
CHEM ch10:4 Specific Heat:
Amount of heat required to raise one gram of a substance 1 degree Celsius
CHEM ch10:5 Critical Temperature:
Highest temperature at which a gas can be liquefied based on the pressure in it
CHEM ch10:6 Normal Boiling Point:
Point at which the vapor pressure equals 760 torr
CHEM ch10:7 Distillation:
Process o f using vaporization and condensation to separate mixtures
CHEM ch10:8 Determining the Amount of Heat produced : Going from Ice to Gas:
Add together the Heat of Fusion the Sensible heat and the Heat of vaporization
CHEM ch10:8 Determining the Amount of Heat produced : Heat of Vaporization
Number of Grams x 80 cal/g
CHEM ch10:8 Determining the Amount of Heat produced : Sensible Heat
Number of grams x 1 cal/g x Temperature Change
CHEM ch10:8 Determining the Amount of Heat produced : Heat of Fusion
Number of Grams x 540 cal/g
CHEM ch10:9 Specific Heat:
Number of grams x Specific Heat x Change in Temperature
CHEM ch10:10 Evaporation:
Above average particles of a liquid escape as a gas
CHEM ch10:11 Surfactant:
surface-active substance that will decrease the surface tension of a liquid
CHEM ch10:12 Unit Cell:
Smallest shape like structure of a crystalline solid
CHEM ch10:13 Allotrope:
Elements that exhibit more than one crystalline lattice
CHEM ch10:14 Heat of Fusion:
Amount of energy needed to heat one gram of a substance from a solid to a liquid
1.
2.
It is a surface phenomenon
3.
It is a cooling process
CHEM ch10:16 Three factors that determine the shape of crystals
1.
2.
Relative Sizes
3.
Number and Kinds or Particles
CHEM ch10:17 Lattice Energy:
Energy released when a crystal is formed
CHEM ch10:18 Vapor Pressure:
Pressure exerted by the evaporated molecule
CHEM ch10:19 Factors that Affect Boiling Points:
Temperature and Pressure
•
o
Ethane: 2C2H6 + 7O2  6H2O + 4CO2
o
Propane: C3H8 + 5O2  4H2O + 3CO2
o
Octane: 2C8H18 + 25O2  18H2O +16CO2
o
Hydrocarbon + Oxygen = CO2 + Water
•
Combustion of hydrogen
o
2H2 + O2  2H2O
•
Acid + Bass form a salt (Metal + Nonmetal) and water
CHEM ch11:2 Triple Point:
Point where water can exist in any of its three states
CHEM ch11:3 Crystalline Structure of Water
Bent Molecule
•
Crystalline Structure of ice is Open Hexagonal Lattice
•
Hybridized orbitals of oxygen in the water molecule are in a tetrahedron shape
CHEM ch11:4 Surface Tension:
Very high surface tension
CHEM ch11:5 Hydrates:
Compounds that have water incorporated into their molecular structure
CHEM ch11:6 Deliquescence:
Compound that absorbs so much water from the air that it dissolves
CHEM ch11:7 Efflorescence:
Compounds that lose water when exposed to air
CHEM ch11:8 Hygroscopic:
Substances that have a strong tendency to attract water from the air
CHEM ch11:9 Dessicator:
Prevents compounds that absorb water from absorbing water
Anhydrides: Compounds that react with water in a composition reaction
•
Metal Oxide + Water  Basic Anhydride
o
Na2O + H2O  2NaOH
o
CaO + H2O  Ca(OH)2
•
Nonmetal Oxide + Water  Acidic Anhydride
o
CO2 + H2O  H2CO3
o
SO3 + H2O  H2SO4
o
P4O10 + 6H2O  4H3PO4
1.
a.
C3H8 + 3H2O –Ni 3CO + 7H2
2.
From Coal and Steam
a.
C(s) + H2O(g)  CO + H2
3.
Blue-green Algae- Converts water and sunlight into H2 and O2
a.
Sunlight + Water  H2 + O2
4.
Electrolysis- Method of producing pure Oxygen and Hydrogen by electricity
a.
Cathode (-): 4H20 + 4e-  2H2 + 4OH- (Forms Hydrogen)
b.
Anode (+): 2H2O  O2 + 4H+ + 4e- (Forms Oxygen)
c.
Total Reaction: 2H2O  O2 + 2H2
CHEM ch11:12 Extremely reactive F is the only Halogen that displaces O from a water molecule
•
CHEM ch11:13 Active Metals (Na, K, Ca) can react with water and form a Hydroxide and Hydrogen
1.
2.
2K + H2O  2KOH + H2(g)
3.
Ca + 2H2O  CaOH + H2(g)
CHEM ch11:14 Moderately Reactive Metals (Fe, Zn, Al) need steam to react
1.
2.
Zn + 2H2O(g)  Zn(OH)2 + H2
3.
2Al + 6H2O(g)  2Al(OH)3 + 3H2
4.
Metal + Water = Hydroxide + Hydrogen
CHEM ch11:15 The most significant water-nonmetals involve halogens (I, Br, Cl) react to form acids
•
CHEM ch11:16 Halogen + Water =
Halogen splits between the hydrogen and the hydroxide
1.
2.
Decomposition: Breaks substance down into two or more substances (ABA+B)
3.
Single Replacement: Active element takes the place of a less active element in a compound (A + BZ  B+ AZ)
4.
Double Replacement: Two compounds switch partners with each other
a)
Elements only switch with other elements in single and double replacements if the metal by itself is more reactive than the element combined to another element
- The number of moles of a compound on one side to the number of moles of a
- Add the mass of each individual element in the compound
•
•
Write the equation out
•
Count the number ions of the elements on both sides of the equation
•
Adjust the coefficients to make the same number on both sides
•
NO + O2  NO2 will become 2NO + O2  2 NO2
CHEM ch8:5 Be able to go from grams to moles and moles to grams
•
•
Given Moles x Gram Formula Mass
•
•
Ex. Pb(NO3)2(aq) + K2CrO4(aq)  PbCrO4 (s) + 2 KNO3 will become: Pb2+(aq) + 2NO3-(aq) + 2K+(aq) + CrO42-(aq)  PbCrO4(s) + 2K+ + 2NO3-(aq)
•
Spectator ions: elements that do not change from the reactant to the product
o
2K+ and 2NO3-
•
Net Ionic Equation: Shows the ions in the equation excluding spectator ions
o
Pb2+ (aq) + CrO42-(aq)  PbCrO4(s)
Know how to do the problems on page 2 of the Chapter 8 test
•
•
one mole of gas at STP (number of moles x 22.4L/1 Mole)
CHEM ch 9: 4 Gas Laws and Concepts
•
•
Boyle’s Law: P1V1 = P2V2
•
Gay-Lussac’s Law: P1 = P2
•
Combined Gas Law: P1V1 = P2V2
CHEM ch9:5 Molar Volume:
The volume occupied by Avogadro’s number of molecules of gas at STP
CHEM ch9:6 Law of Combining Volumes:
The volumes of reacting gases and their gaseous products are expressed in small whole numbers
CHEM ch9:7 Barometer:
Instrument used to measure atmospheric pressure
CHEM ch9:8 Dalton’s Law of Partial Pressures:
total pressure of a mixture equals sum of partial pressures
CHEM ch9:9 Permeability:
gases easily mingle with other substances
CHEM ch9:10 Elasticity:
Collisions of gas molecules conserve energy
CHEM ch9:11 Diffusion:
Gas molecules move constantly to uniform fill their container
CHEM ch9:12 Compressibility:
High pressures squeeze gases into smaller volumes
CHEM ch9:13 Expansibility:
gas quickly expands to fill low pressure regions
•
•
o
Bonds between polar molecule
•
o
Hydrogen is very positive and small so it can connect to other molecules
•
o
Atoms are more negative on one side for a split second
o
Bigger molecules have greater dispersion forces
•
•
Latent: Form of heat that causes a phase change
CHEM ch10:3 Heat of Vaporization:
amount of energy needed to heat one gram of a substance from a liquid to a gas (no temperature change)
•
540 cal/g in water (Heat of Vaporization x Mass)
CHEM ch10:4 Specific Heat:
Amount of heat required to raise one gram of a substance 1 degree Celsius
CHEM ch10:5 Critical Temperature:
Highest temperature at which a gas can be liquefied based on the pressure in it
CHEM ch10:6 Normal Boiling Point:
Point at which the vapor pressure equals 760 torr
CHEM ch10:7 Distillation:
Process o f using vaporization and condensation to separate mixtures
CHEM ch10:8 Determining the Amount of Heat produced : Going from Ice to Gas:
Add together the Heat of Fusion the Sensible heat and the Heat of vaporization
CHEM ch10:8 Determining the Amount of Heat produced : Heat of Vaporization
Number of Grams x 80 cal/g
CHEM ch10:8 Determining the Amount of Heat produced : Sensible Heat
Number of grams x 1 cal/g x Temperature Change
CHEM ch10:8 Determining the Amount of Heat produced : Heat of Fusion
Number of Grams x 540 cal/g
CHEM ch10:9 Specific Heat:
Number of grams x Specific Heat x Change in Temperature
CHEM ch10:10 Evaporation:
Above average particles of a liquid escape as a gas
CHEM ch10:11 Surfactant:
surface-active substance that will decrease the surface tension of a liquid
CHEM ch10:12 Unit Cell:
Smallest shape like structure of a crystalline solid
CHEM ch10:13 Allotrope:
Elements that exhibit more than one crystalline lattice
CHEM ch10:14 Heat of Fusion:
Amount of energy needed to heat one gram of a substance from a solid to a liquid
1.
2.
It is a surface phenomenon
3.
It is a cooling process
CHEM ch10:16 Three factors that determine the shape of crystals
1.
2.
Relative Sizes
3.
Number and Kinds or Particles
CHEM ch10:17 Lattice Energy:
Energy released when a crystal is formed
CHEM ch10:18 Vapor Pressure:
Pressure exerted by the evaporated molecule
CHEM ch10:19 Factors that Affect Boiling Points:
Temperature and Pressure
•
o
Ethane: 2C2H6 + 7O2  6H2O + 4CO2
o
Propane: C3H8 + 5O2  4H2O + 3CO2
o
Octane: 2C8H18 + 25O2  18H2O +16CO2
o
Hydrocarbon + Oxygen = CO2 + Water
•
Combustion of hydrogen
o
2H2 + O2  2H2O
•
Acid + Bass form a salt (Metal + Nonmetal) and water
CHEM ch11:2 Triple Point:
Point where water can exist in any of its three states
CHEM ch11:3 Crystalline Structure of Water
Bent Molecule
•
Crystalline Structure of ice is Open Hexagonal Lattice
•
Hybridized orbitals of oxygen in the water molecule are in a tetrahedron shape
CHEM ch11:4 Surface Tension:
Very high surface tension
CHEM ch11:5 Hydrates:
Compounds that have water incorporated into their molecular structure
CHEM ch11:6 Deliquescence:
Compound that absorbs so much water from the air that it dissolves
CHEM ch11:7 Efflorescence:
Compounds that lose water when exposed to air
CHEM ch11:8 Hygroscopic:
Substances that have a strong tendency to attract water from the air
CHEM ch11:9 Dessicator:
Prevents compounds that absorb water from absorbing water
Anhydrides: Compounds that react with water in a composition reaction
•
Metal Oxide + Water  Basic Anhydride
o
Na2O + H2O  2NaOH
o
CaO + H2O  Ca(OH)2
•
Nonmetal Oxide + Water  Acidic Anhydride
o
CO2 + H2O  H2CO3
o
SO3 + H2O  H2SO4
o
P4O10 + 6H2O  4H3PO4
1.
a.
C3H8 + 3H2O –Ni 3CO + 7H2
2.
From Coal and Steam
a.
C(s) + H2O(g)  CO + H2
3.
Blue-green Algae- Converts water and sunlight into H2 and O2
a.
Sunlight + Water  H2 + O2
4.
Electrolysis- Method of producing pure Oxygen and Hydrogen by electricity
a.
Cathode (-): 4H20 + 4e-  2H2 + 4OH- (Forms Hydrogen)
b.
Anode (+): 2H2O  O2 + 4H+ + 4e- (Forms Oxygen)
c.
Total Reaction: 2H2O  O2 + 2H2
CHEM ch11:12 Extremely reactive F is the only Halogen that displaces O from a water molecule
•
CHEM ch11:13 Active Metals (Na, K, Ca) can react with water and form a Hydroxide and Hydrogen
1.
2.
2K + H2O  2KOH + H2(g)
3.
Ca + 2H2O  CaOH + H2(g)
CHEM ch11:14 Moderately Reactive Metals (Fe, Zn, Al) need steam to react
1.
2.
Zn + 2H2O(g)  Zn(OH)2 + H2
3.
2Al + 6H2O(g)  2Al(OH)3 + 3H2
4.
Metal + Water = Hydroxide + Hydrogen
CHEM ch11:15 The most significant water-nonmetals involve halogens (I, Br, Cl) react to form acids
•
CHEM ch11:16 Halogen + Water =
Halogen splits between the hydrogen and the hydroxide
1.
2.
Decomposition: Breaks substance down into two or more substances (ABA+B)
3.
Single Replacement: Active element takes the place of a less active element in a compound (A + BZ  B+ AZ)
4.
Double Replacement: Two compounds switch partners with each other
a)
Elements only switch with other elements in single and double replacements if the metal by itself is more reactive than the element combined to another element
- The number of moles of a compound on one side to the number of moles of a
- Add the mass of each individual element in the compound
•
•
Write the equation out
•
Count the number ions of the elements on both sides of the equation
•
Adjust the coefficients to make the same number on both sides
•
NO + O2  NO2 will become 2NO + O2  2 NO2
CHEM ch8:5 Be able to go from grams to moles and moles to grams
•
•
Given Moles x Gram Formula Mass
•
•
Ex. Pb(NO3)2(aq) + K2CrO4(aq)  PbCrO4 (s) + 2 KNO3 will become: Pb2+(aq) + 2NO3-(aq) + 2K+(aq) + CrO42-(aq)  PbCrO4(s) + 2K+ + 2NO3-(aq)
•
Spectator ions: elements that do not change from the reactant to the product
o
2K+ and 2NO3-
•
Net Ionic Equation: Shows the ions in the equation excluding spectator ions
o
Pb2+ (aq) + CrO42-(aq)  PbCrO4(s)
Know how to do the problems on page 2 of the Chapter 8 test
•
•
one mole of gas at STP (number of moles x 22.4L/1 Mole)
CHEM ch 9: 4 Gas Laws and Concepts
•
•
Boyle’s Law: P1V1 = P2V2
•
Gay-Lussac’s Law: P1 = P2
•
Combined Gas Law: P1V1 = P2V2
CHEM ch9:5 Molar Volume:
The volume occupied by Avogadro’s number of molecules of gas at STP
CHEM ch9:6 Law of Combining Volumes:
The volumes of reacting gases and their gaseous products are expressed in small whole numbers
CHEM ch9:7 Barometer:
Instrument used to measure atmospheric pressure
CHEM ch9:8 Dalton’s Law of Partial Pressures:
total pressure of a mixture equals sum of partial pressures
CHEM ch9:9 Permeability:
gases easily mingle with other substances
CHEM ch9:10 Elasticity:
Collisions of gas molecules conserve energy
CHEM ch9:11 Diffusion:
Gas molecules move constantly to uniform fill their container
CHEM ch9:12 Compressibility:
High pressures squeeze gases into smaller volumes
CHEM ch9:13 Expansibility:
gas quickly expands to fill low pressure regions
•
•
o
Bonds between polar molecule
•
o
Hydrogen is very positive and small so it can connect to other molecules
•
o
Atoms are more negative on one side for a split second
o
Bigger molecules have greater dispersion forces
•
•
Latent: Form of heat that causes a phase change
CHEM ch10:3 Heat of Vaporization:
amount of energy needed to heat one gram of a substance from a liquid to a gas (no temperature change)
•
540 cal/g in water (Heat of Vaporization x Mass)
CHEM ch10:4 Specific Heat:
Amount of heat required to raise one gram of a substance 1 degree Celsius
CHEM ch10:5 Critical Temperature:
Highest temperature at which a gas can be liquefied based on the pressure in it
CHEM ch10:6 Normal Boiling Point:
Point at which the vapor pressure equals 760 torr
CHEM ch10:7 Distillation:
Process o f using vaporization and condensation to separate mixtures
CHEM ch10:8 Determining the Amount of Heat produced : Going from Ice to Gas:
Add together the Heat of Fusion the Sensible heat and the Heat of vaporization
CHEM ch10:8 Determining the Amount of Heat produced : Heat of Vaporization
Number of Grams x 80 cal/g
CHEM ch10:8 Determining the Amount of Heat produced : Sensible Heat
Number of grams x 1 cal/g x Temperature Change
CHEM ch10:8 Determining the Amount of Heat produced : Heat of Fusion
Number of Grams x 540 cal/g
CHEM ch10:9 Specific Heat:
Number of grams x Specific Heat x Change in Temperature
CHEM ch10:10 Evaporation:
Above average particles of a liquid escape as a gas
CHEM ch10:11 Surfactant:
surface-active substance that will decrease the surface tension of a liquid
CHEM ch10:12 Unit Cell:
Smallest shape like structure of a crystalline solid
CHEM ch10:13 Allotrope:
Elements that exhibit more than one crystalline lattice
CHEM ch10:14 Heat of Fusion:
Amount of energy needed to heat one gram of a substance from a solid to a liquid
1.
2.
It is a surface phenomenon
3.
It is a cooling process
CHEM ch10:16 Three factors that determine the shape of crystals
1.
2.
Relative Sizes
3.
Number and Kinds or Particles
CHEM ch10:17 Lattice Energy:
Energy released when a crystal is formed
CHEM ch10:18 Vapor Pressure:
Pressure exerted by the evaporated molecule
CHEM ch10:19 Factors that Affect Boiling Points:
Temperature and Pressure
•
o
Ethane: 2C2H6 + 7O2  6H2O + 4CO2
o
Propane: C3H8 + 5O2  4H2O + 3CO2
o
Octane: 2C8H18 + 25O2  18H2O +16CO2
o
Hydrocarbon + Oxygen = CO2 + Water
•
Combustion of hydrogen
o
2H2 + O2  2H2O
•
Acid + Bass form a salt (Metal + Nonmetal) and water
CHEM ch11:2 Triple Point:
Point where water can exist in any of its three states
CHEM ch11:3 Crystalline Structure of Water
Bent Molecule
•
Crystalline Structure of ice is Open Hexagonal Lattice
•
Hybridized orbitals of oxygen in the water molecule are in a tetrahedron shape
CHEM ch11:4 Surface Tension:
Very high surface tension
CHEM ch11:5 Hydrates:
Compounds that have water incorporated into their molecular structure
CHEM ch11:6 Deliquescence:
Compound that absorbs so much water from the air that it dissolves
CHEM ch11:7 Efflorescence:
Compounds that lose water when exposed to air
CHEM ch11:8 Hygroscopic:
Substances that have a strong tendency to attract water from the air
CHEM ch11:9 Dessicator:
Prevents compounds that absorb water from absorbing water
Anhydrides: Compounds that react with water in a composition reaction
•
Metal Oxide + Water  Basic Anhydride
o
Na2O + H2O  2NaOH
o
CaO + H2O  Ca(OH)2
•
Nonmetal Oxide + Water  Acidic Anhydride
o
CO2 + H2O  H2CO3
o
SO3 + H2O  H2SO4
o
P4O10 + 6H2O  4H3PO4
1.
a.
C3H8 + 3H2O –Ni 3CO + 7H2
2.
From Coal and Steam
a.
C(s) + H2O(g)  CO + H2
3.
Blue-green Algae- Converts water and sunlight into H2 and O2
a.
Sunlight + Water  H2 + O2
4.
Electrolysis- Method of producing pure Oxygen and Hydrogen by electricity
a.
Cathode (-): 4H20 + 4e-  2H2 + 4OH- (Forms Hydrogen)
b.
Anode (+): 2H2O  O2 + 4H+ + 4e- (Forms Oxygen)
c.
Total Reaction: 2H2O  O2 + 2H2
CHEM ch11:12 Extremely reactive F is the only Halogen that displaces O from a water molecule
•
CHEM ch11:13 Active Metals (Na, K, Ca) can react with water and form a Hydroxide and Hydrogen
1.
2.
2K + H2O  2KOH + H2(g)
3.
Ca + 2H2O  CaOH + H2(g)
CHEM ch11:14 Moderately Reactive Metals (Fe, Zn, Al) need steam to react
1.
2.
Zn + 2H2O(g)  Zn(OH)2 + H2
3.
2Al + 6H2O(g)  2Al(OH)3 + 3H2
4.
Metal + Water = Hydroxide + Hydrogen
CHEM ch11:15 The most significant water-nonmetals involve halogens (I, Br, Cl) react to form acids
•
CHEM ch11:16 Halogen + Water =
Halogen splits between the hydrogen and the hydroxide
Entropy: a measurement of randomness
• ΔS° = ΣS°products - ΣS°reactants (negative change = less entropy)
Enthalpy:
Thermodynamic quantity that describes the energy of a substance at constant pressure
• Endothermic: has a positive enthalpy (more heat than before the reaction)
Gibbs Free Energy (G)- relates enthalpy to entropy
• + ΔG  reaction is unfavorable and will not occur
CHEM ch8:1 Types of Reactions:
1. Combination: combines two or more substances into a single product (A+B> AB)
2. Decomposition: Breaks substance down into two or more substances (AB>A+B)
3. Single Replacement: Active element takes the place of a less active element in a compound (A + BZ > B+ AZ)
4. Double Replacement: Two compounds switch partners with each other
(AX + BZ >AZ +BX)
a) Elements only switch with other elements in single and double replacements if the metal by itself is more reactive than the element combined to another element
CHEM ch8:1 Types of Reactions:
1. Combination: combines two or more substances into a single product (A+B AB)
2. Decomposition: Breaks substance down into two or more substances (ABA+B)
3. Single Replacement: Active element takes the place of a less active element in a compound (A + BZ  B+ AZ)
4. Double Replacement: Two compounds switch partners with each other
(AX + BZ AZ +BX)
a) Elements only switch with other elements in single and double replacements if the metal by itself is more reactive than the element combined to another element

CHEM ch8:2 Know Molar Relationships in Reactions
- The number of moles of a compound on one side to the number of moles of a
compound on the other side
- Ex. The molar relationship between Fe2O3 and CO2 in
Fe2O3 + 3CO  2Fe + 3CO2 is 1:3
- The number of moles of a compound on one side to the number of moles of a
compound on the other side
- Ex. The molar relationship between Fe2O3 and CO2 in
Fe2O3 + 3CO > 2Fe + 3CO2 is 1:3
CHEM ch8:3 Gram Molecular Mass/Gram Formula Mass
- Add the mass of each individual element in the compound
- Multiply the element by the number of moles in the compound if there are more than one
- Ex. NaCl = Na + Cl = 23 + 35.45 = 58.45g
- H2O = 2 H + O = 2(1) + 16 = 18g
CHEM ch8:4 Be able to Balance reactions
• Must have the same number of ions of all elements on both sides of the equation
• Write the equation out
• Count the number ions of the elements on both sides of the equation
• Adjust the coefficients to make the same number on both sides
• NO + O2 > NO2 will become 2NO + O2 > 2 NO2
CHEM ch8:5 Be able to go from grams to moles and moles to grams
• Given Mass x 1 mole of the given Compound (over) Gram Formula Mass
• Given Moles x Gram Formula Mass (Over) 1 Mole
CHEM ch8:6 Ionic Equation: represents all the particles present before and after the reaction
• Write each element separately in the equation only in aqueous solutions
• Ex. Pb(NO3)2(aq) + K2CrO4(aq)  PbCrO4 (s) + 2 KNO3 will become: Pb2+(aq) + 2NO3-(aq) + 2K+(aq) + CrO42-(aq)  PbCrO4(s) + 2K+ + 2NO3-(aq)
• Spectator ions: elements that do not change from the reactant to the product
o 2K+ and 2NO3-
• Net Ionic Equation: Shows the ions in the equation excluding spectator ions
o Pb2+ (aq) + CrO42-(aq)  PbCrO4(s)
Know how to do the problems on page 2 of the Chapter 8 test
...
CHEM ch9: 1 PV=nRT (Ideal Gas law)
• n = number of moles, P = Pressure, V = Volume, T = temperature, R = constant
CHEM ch 9: 2 STP: Standard temperature and pressure
273k and 760 torr/1 atm/ 101.3 kpa
CHEM ch 9: 3 There are 22.4 L in ___?
/ means (over)
• Charles’ Law: V1/T1 = V2/T2 (indirect relationship)
• Boyle’s Law: P1V1 = P2V2
• Gay-Lussac’s Law: P1/T1 = P2/T2
• Combined Gas Law: P1V1/T1 = P2V2/T2