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370 Cards in this Set
- Front
- Back
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1.
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2.
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Decomposition: Breaks substance down into two or more substances (ABA+B)
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3.
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Single Replacement: Active element takes the place of a less active element in a compound (A + BZ B+ AZ)
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4.
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Double Replacement: Two compounds switch partners with each other
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a)
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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
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- The number of moles of a compound on one side to the number of moles of a
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- Add the mass of each individual element in the compound
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•
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•
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Write the equation out
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•
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Count the number ions of the elements on both sides of the equation
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•
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Adjust the coefficients to make the same number on both sides
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•
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NO + O2 NO2 will become 2NO + O2 2 NO2
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CHEM ch8:5 Be able to go from grams to moles and moles to grams
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•
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•
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Given Moles x Gram Formula Mass
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•
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•
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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)
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•
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Spectator ions: elements that do not change from the reactant to the product
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o
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2K+ and 2NO3-
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•
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Net Ionic Equation: Shows the ions in the equation excluding spectator ions
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o
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Pb2+ (aq) + CrO42-(aq) PbCrO4(s)
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Know how to do the problems on page 2 of the Chapter 8 test
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•
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•
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one mole of gas at STP (number of moles x 22.4L/1 Mole)
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CHEM ch 9: 4 Gas Laws and Concepts
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•
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•
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Boyle’s Law: P1V1 = P2V2
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•
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Gay-Lussac’s Law: P1 = P2
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Combined Gas Law: P1V1 = P2V2
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CHEM ch9:5 Molar Volume:
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The volume occupied by Avogadro’s number of molecules of gas at STP
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CHEM ch9:6 Law of Combining Volumes:
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The volumes of reacting gases and their gaseous products are expressed in small whole numbers
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CHEM ch9:7 Barometer:
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Instrument used to measure atmospheric pressure
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CHEM ch9:8 Dalton’s Law of Partial Pressures:
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total pressure of a mixture equals sum of partial pressures
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CHEM ch9:9 Permeability:
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gases easily mingle with other substances
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CHEM ch9:10 Elasticity:
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Collisions of gas molecules conserve energy
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CHEM ch9:11 Diffusion:
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Gas molecules move constantly to uniform fill their container
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CHEM ch9:12 Compressibility:
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High pressures squeeze gases into smaller volumes
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CHEM ch9:13 Expansibility:
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gas quickly expands to fill low pressure regions
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•
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•
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o
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Bonds between polar molecule
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•
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o
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Hydrogen is very positive and small so it can connect to other molecules
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•
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o
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Atoms are more negative on one side for a split second
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o
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Bigger molecules have greater dispersion forces
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•
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•
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Latent: Form of heat that causes a phase change
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CHEM ch10:3 Heat of Vaporization:
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amount of energy needed to heat one gram of a substance from a liquid to a gas (no temperature change)
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•
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540 cal/g in water (Heat of Vaporization x Mass)
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CHEM ch10:4 Specific Heat:
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Amount of heat required to raise one gram of a substance 1 degree Celsius
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CHEM ch10:5 Critical Temperature:
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Highest temperature at which a gas can be liquefied based on the pressure in it
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CHEM ch10:6 Normal Boiling Point:
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Point at which the vapor pressure equals 760 torr
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CHEM ch10:7 Distillation:
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Process o f using vaporization and condensation to separate mixtures
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CHEM ch10:8 Determining the Amount of Heat produced : Going from Ice to Gas:
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Add together the Heat of Fusion the Sensible heat and the Heat of vaporization
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CHEM ch10:8 Determining the Amount of Heat produced : Heat of Vaporization
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Number of Grams x 80 cal/g
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CHEM ch10:8 Determining the Amount of Heat produced : Sensible Heat
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Number of grams x 1 cal/g x Temperature Change
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CHEM ch10:8 Determining the Amount of Heat produced : Heat of Fusion
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Number of Grams x 540 cal/g
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CHEM ch10:9 Specific Heat:
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Number of grams x Specific Heat x Change in Temperature
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CHEM ch10:10 Evaporation:
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Above average particles of a liquid escape as a gas
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CHEM ch10:11 Surfactant:
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surface-active substance that will decrease the surface tension of a liquid
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CHEM ch10:12 Unit Cell:
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Smallest shape like structure of a crystalline solid
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CHEM ch10:13 Allotrope:
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Elements that exhibit more than one crystalline lattice
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CHEM ch10:14 Heat of Fusion:
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Amount of energy needed to heat one gram of a substance from a solid to a liquid
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1.
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2.
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It is a surface phenomenon
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3.
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It is a cooling process
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CHEM ch10:16 Three factors that determine the shape of crystals
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1.
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2.
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Relative Sizes
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3.
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Number and Kinds or Particles
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CHEM ch10:17 Lattice Energy:
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Energy released when a crystal is formed
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CHEM ch10:18 Vapor Pressure:
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Pressure exerted by the evaporated molecule
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CHEM ch10:19 Factors that Affect Boiling Points:
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Temperature and Pressure
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•
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o
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Ethane: 2C2H6 + 7O2 6H2O + 4CO2
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o
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Propane: C3H8 + 5O2 4H2O + 3CO2
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o
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Octane: 2C8H18 + 25O2 18H2O +16CO2
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o
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Hydrocarbon + Oxygen = CO2 + Water
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•
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Combustion of hydrogen
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o
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2H2 + O2 2H2O
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•
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Acid + Bass form a salt (Metal + Nonmetal) and water
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CHEM ch11:2 Triple Point:
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Point where water can exist in any of its three states
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CHEM ch11:3 Crystalline Structure of Water
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Bent Molecule
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•
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Crystalline Structure of ice is Open Hexagonal Lattice
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•
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Hybridized orbitals of oxygen in the water molecule are in a tetrahedron shape
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CHEM ch11:4 Surface Tension:
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Very high surface tension
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CHEM ch11:5 Hydrates:
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Compounds that have water incorporated into their molecular structure
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CHEM ch11:6 Deliquescence:
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Compound that absorbs so much water from the air that it dissolves
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CHEM ch11:7 Efflorescence:
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Compounds that lose water when exposed to air
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CHEM ch11:8 Hygroscopic:
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Substances that have a strong tendency to attract water from the air
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CHEM ch11:9 Dessicator:
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Prevents compounds that absorb water from absorbing water
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Anhydrides: Compounds that react with water in a composition reaction
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•
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Metal Oxide + Water Basic Anhydride
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o
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Na2O + H2O 2NaOH
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o
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CaO + H2O Ca(OH)2
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•
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Nonmetal Oxide + Water Acidic Anhydride
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o
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CO2 + H2O H2CO3
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o
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SO3 + H2O H2SO4
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o
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P4O10 + 6H2O 4H3PO4
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1.
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a.
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C3H8 + 3H2O –Ni 3CO + 7H2
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2.
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From Coal and Steam
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a.
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C(s) + H2O(g) CO + H2
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3.
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Blue-green Algae- Converts water and sunlight into H2 and O2
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a.
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Sunlight + Water H2 + O2
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4.
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Electrolysis- Method of producing pure Oxygen and Hydrogen by electricity
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a.
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Cathode (-): 4H20 + 4e- 2H2 + 4OH- (Forms Hydrogen)
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b.
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Anode (+): 2H2O O2 + 4H+ + 4e- (Forms Oxygen)
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c.
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Total Reaction: 2H2O O2 + 2H2
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CHEM ch11:12 Extremely reactive F is the only Halogen that displaces O from a water molecule
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•
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CHEM ch11:13 Active Metals (Na, K, Ca) can react with water and form a Hydroxide and Hydrogen
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1.
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2.
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2K + H2O 2KOH + H2(g)
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3.
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Ca + 2H2O CaOH + H2(g)
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CHEM ch11:14 Moderately Reactive Metals (Fe, Zn, Al) need steam to react
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1.
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2.
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Zn + 2H2O(g) Zn(OH)2 + H2
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3.
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2Al + 6H2O(g) 2Al(OH)3 + 3H2
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4.
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Metal + Water = Hydroxide + Hydrogen
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CHEM ch11:15 The most significant water-nonmetals involve halogens (I, Br, Cl) react to form acids
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•
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CHEM ch11:16 Halogen + Water =
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Halogen splits between the hydrogen and the hydroxide
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1.
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2.
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Decomposition: Breaks substance down into two or more substances (ABA+B)
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|
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)
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|
•
|
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 (ABA+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
|
|
|
•
|
|
•
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Latent: Form of heat that causes a phase change
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CHEM ch10:3 Heat of Vaporization:
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amount of energy needed to heat one gram of a substance from a liquid to a gas (no temperature change)
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•
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540 cal/g in water (Heat of Vaporization x Mass)
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CHEM ch10:4 Specific Heat:
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Amount of heat required to raise one gram of a substance 1 degree Celsius
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CHEM ch10:5 Critical Temperature:
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Highest temperature at which a gas can be liquefied based on the pressure in it
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CHEM ch10:6 Normal Boiling Point:
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Point at which the vapor pressure equals 760 torr
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CHEM ch10:7 Distillation:
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Process o f using vaporization and condensation to separate mixtures
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CHEM ch10:8 Determining the Amount of Heat produced : Going from Ice to Gas:
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Add together the Heat of Fusion the Sensible heat and the Heat of vaporization
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CHEM ch10:8 Determining the Amount of Heat produced : Heat of Vaporization
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Number of Grams x 80 cal/g
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CHEM ch10:8 Determining the Amount of Heat produced : Sensible Heat
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Number of grams x 1 cal/g x Temperature Change
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CHEM ch10:8 Determining the Amount of Heat produced : Heat of Fusion
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Number of Grams x 540 cal/g
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CHEM ch10:9 Specific Heat:
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Number of grams x Specific Heat x Change in Temperature
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CHEM ch10:10 Evaporation:
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Above average particles of a liquid escape as a gas
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CHEM ch10:11 Surfactant:
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surface-active substance that will decrease the surface tension of a liquid
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CHEM ch10:12 Unit Cell:
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Smallest shape like structure of a crystalline solid
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CHEM ch10:13 Allotrope:
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Elements that exhibit more than one crystalline lattice
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CHEM ch10:14 Heat of Fusion:
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Amount of energy needed to heat one gram of a substance from a solid to a liquid
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1.
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2.
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It is a surface phenomenon
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3.
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It is a cooling process
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CHEM ch10:16 Three factors that determine the shape of crystals
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1.
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2.
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Relative Sizes
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3.
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Number and Kinds or Particles
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CHEM ch10:17 Lattice Energy:
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Energy released when a crystal is formed
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CHEM ch10:18 Vapor Pressure:
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Pressure exerted by the evaporated molecule
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CHEM ch10:19 Factors that Affect Boiling Points:
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Temperature and Pressure
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•
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o
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Ethane: 2C2H6 + 7O2 6H2O + 4CO2
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o
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Propane: C3H8 + 5O2 4H2O + 3CO2
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o
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Octane: 2C8H18 + 25O2 18H2O +16CO2
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o
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Hydrocarbon + Oxygen = CO2 + Water
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•
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Combustion of hydrogen
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o
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2H2 + O2 2H2O
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•
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Acid + Bass form a salt (Metal + Nonmetal) and water
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CHEM ch11:2 Triple Point:
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Point where water can exist in any of its three states
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CHEM ch11:3 Crystalline Structure of Water
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Bent Molecule
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•
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Crystalline Structure of ice is Open Hexagonal Lattice
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•
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Hybridized orbitals of oxygen in the water molecule are in a tetrahedron shape
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CHEM ch11:4 Surface Tension:
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Very high surface tension
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CHEM ch11:5 Hydrates:
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Compounds that have water incorporated into their molecular structure
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CHEM ch11:6 Deliquescence:
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Compound that absorbs so much water from the air that it dissolves
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CHEM ch11:7 Efflorescence:
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Compounds that lose water when exposed to air
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CHEM ch11:8 Hygroscopic:
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Substances that have a strong tendency to attract water from the air
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CHEM ch11:9 Dessicator:
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Prevents compounds that absorb water from absorbing water
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Anhydrides: Compounds that react with water in a composition reaction
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•
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Metal Oxide + Water Basic Anhydride
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o
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Na2O + H2O 2NaOH
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o
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CaO + H2O Ca(OH)2
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•
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Nonmetal Oxide + Water Acidic Anhydride
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o
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CO2 + H2O H2CO3
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o
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SO3 + H2O H2SO4
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o
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P4O10 + 6H2O 4H3PO4
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1.
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a.
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C3H8 + 3H2O –Ni 3CO + 7H2
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2.
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From Coal and Steam
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a.
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C(s) + H2O(g) CO + H2
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3.
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Blue-green Algae- Converts water and sunlight into H2 and O2
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a.
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Sunlight + Water H2 + O2
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4.
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Electrolysis- Method of producing pure Oxygen and Hydrogen by electricity
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a.
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Cathode (-): 4H20 + 4e- 2H2 + 4OH- (Forms Hydrogen)
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b.
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Anode (+): 2H2O O2 + 4H+ + 4e- (Forms Oxygen)
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c.
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Total Reaction: 2H2O O2 + 2H2
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CHEM ch11:12 Extremely reactive F is the only Halogen that displaces O from a water molecule
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•
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CHEM ch11:13 Active Metals (Na, K, Ca) can react with water and form a Hydroxide and Hydrogen
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1.
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2.
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2K + H2O 2KOH + H2(g)
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3.
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Ca + 2H2O CaOH + H2(g)
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CHEM ch11:14 Moderately Reactive Metals (Fe, Zn, Al) need steam to react
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1.
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2.
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Zn + 2H2O(g) Zn(OH)2 + H2
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3.
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2Al + 6H2O(g) 2Al(OH)3 + 3H2
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4.
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Metal + Water = Hydroxide + Hydrogen
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CHEM ch11:15 The most significant water-nonmetals involve halogens (I, Br, Cl) react to form acids
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•
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CHEM ch11:16 Halogen + Water =
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Halogen splits between the hydrogen and the hydroxide
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Entropy: a measurement of randomness
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• ΔS° = ΣS°products - ΣS°reactants (negative change = less entropy)
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Enthalpy:
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Thermodynamic quantity that describes the energy of a substance at constant pressure
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• Endothermic: has a positive enthalpy (more heat than before the reaction)
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Gibbs Free Energy (G)- relates enthalpy to entropy
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• + ΔG reaction is unfavorable and will not occur
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CHEM ch8:1 Types of Reactions:
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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 |
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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 (ABA+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 |
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CHEM ch8:3 Gram Molecular Mass/Gram Formula Mass
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- 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 |
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CHEM ch8:4 Be able to Balance reactions
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• 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 |
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CHEM ch8:5 Be able to go from grams to moles and moles to grams
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• Given Mass x 1 mole of the given Compound (over) Gram Formula Mass
• Given Moles x Gram Formula Mass (Over) 1 Mole |
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CHEM ch8:6 Ionic Equation: represents all the particles present before and after the reaction
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• 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) |
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Know how to do the problems on page 2 of the Chapter 8 test
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...
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CHEM ch9: 1 PV=nRT (Ideal Gas law)
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• n = number of moles, P = Pressure, V = Volume, T = temperature, R = constant
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CHEM ch 9: 2 STP: Standard temperature and pressure
|
273k and 760 torr/1 atm/ 101.3 kpa
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CHEM ch 9: 3 There are 22.4 L in ___?
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/ 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 |