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33 Cards in this Set
- Front
- Back
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Rules of Solubility |
Li+, Na+, K+ and NH4+: all soluble NO3- and C2H3O2-: all soluble Cl-, Br- and I-: soluble, not w/ Ag+, HG22+, Ca2+ SO42-: soluble, not w/ Sr2+, Ba2+, Pb2+, Ag2+, Ca2+ |
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Rules of Insolubility |
OH-, S2-, CO32- and PO43- insoluble - except w/ Li+, Na+, K+, NH4+ S2-: soluble w/ Ca2+, Sr2+, Ba2+ OH-: slightly soluble w/ Ca2+, Sr2+, Ba2+ |
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VSEPR Theory |
Valence Shell Electron Pair Repulsion Theory - shape of molecule corresponds to arrangement of central valence e- in lowest repulsion/nrg |
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Electron Geometry
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Distribution of e- pairs
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Molecular Geometry
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Arrangement of atoms in molecule
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Linear Geometry
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2 e- pairs 2 bonding pairs 180 degrees |
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Trigonal Geometry
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3 e- pairs 3 boding pairs 120 degrees |
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Bent
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3 e- pairs 2 boding pairs <120 deg |
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Tetrahedral
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4 e- pairs 4 bonding pairs 109.5 deg |
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Pyramidal
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4 e- pairs 3 bonding pairs <109.5 deg |
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Bent
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4 e- pairs 2 bonding pairs <109.5 deg |
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Trigonal Bipyramidal
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5 e- pairs 5 bonding pairs 180, 120, 90deg |
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See Saw
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5 e- pairs 4 bonding pairs 180, <120, 90 deg |
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T Shape
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5 e- pairs 3 bonding pairs 180, 90 deg |
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Linear
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5 e- pairs 2 bonding pairs 180 deg |
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Octahedral
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6 e- pairs 6 bonding pairs 90 deg |
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Square pyramidal
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6 e- pairs 5 bonding pairs 90, <90 deg |
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Square Planar
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6 e- pairs 4 bonding pairs 90 deg |
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Chemical Equations
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reactants -> products
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Mole
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1 mole = 6.022E23 particles
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Molar Mass
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grams/mole
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Combustion Reaction
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Hydrocarbon(CxHy) + O2 -> CO2 + H2O
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Double Displacement Reaction
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AB + CD -> AD + CB Does not always have rxn - only if precipitate, weak acid or gas forms |
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Single Replacement Reaction
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AB + C -> A + CB ion being replaced is less reactive than ion coming into the compound |
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Neutralization Reaction
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Special type of Double Displacement HA + BOH -> H2O + BA(salt) |
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Combination Reactions
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A + B -> AB 2 elements or 2 compounds combine to form one compound. |
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Decomposition Reactions
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AB (heat)-> A + B
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Ionic Solutions
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Ionic compounds introduced to water break up into constituent ions. Ions become hydrated (surrounded by polar water molecules)
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Ion Pair Formation
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Cations and Anions are partially hydrated and closely associate with each other. Decreases total number of ions in solution decreasing conductivity. Factors increasing formation: - greater concentrations - greater charge magnitude - smaller ion size |
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Ionic Strength
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Quantifies amount of ions in solution. I=1/2 sum(ci*zi^2) c: concentration z: ion charge |
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Molar Ionic Conductivity
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v+: coeff of cation v-: coeff of anion A+: molar ionic conductivity of cation A-: molar ionic conductivity of anion (S/M*cm) |
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Molarity
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Moles, solute / Liters, solution
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molality
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moles, solute / kg, solvent
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