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68 Cards in this Set
- Front
- Back
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Thermal Energy |
E=RT |
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Ideal Gas Law |
PV=nRT |
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R in Pascals |
8.314 |
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R in Atmospheres |
.08206 |
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Molarity (M) |
n/V or mol/L |
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Intermolecular |
between molecules |
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Intramolecular |
within molecules |
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Heat of Fusion |
heat needed to melt a substance |
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Heat of Vaporization |
heat required to evaporate a substance |
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Vapor Pressure |
gas pressure when vapor and liquid are at equilibrium |
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Higher pressure = ________ Boiling Point |
higher |
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Heat of Sublimation |
heat required to sublime a substance |
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List in order of INCREASING strength: -Dipole-Dipole -Dispersion Forces -Hydrogen Bonding |
1. Dispersion Forces 2. Dipole-Dipole 3. Hydrogen Bonding |
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Dispersion Forces |
more electrons = stronger force |
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Dipole-Dipole |
Think dipole vectors, which also determine polarity depending on if they cancel out or not |
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Hydrogen Bonding |
occurs only with H, N, O, and F |
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Solids are held together by _____________ forces. |
intermolecular |
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3 types of unit cells |
simple cubic, body-centered cubic, face-centered cubic |
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Coordination Number (CN) |
# of atoms surrounding an atom in a crystal lattice |
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Packing Efficiency (PE) |
fraction of volume of unit cell occupied by particles |
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__________ valence electrons hold cationic metallic atoms together |
Delocalized |
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Valence band |
highest energy filled band |
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Conduction band |
lowest energy empty band |
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Fermi level |
highest energy occupied crystal orbital (HOMO) |
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Ionic solids have _______ melting points |
high |
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To predict melting points of ionic solids... |
remember coulombs law |
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Network Covalent solids contain... |
nonmetals and metalloids |
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Molecular solids have ____________ forces |
weak intermolecular (this makes them have the lowest melting point) |
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1st Law of Thermodynamics |
energy is neither created nor destroyed |
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Energy of a system = |
heat (q) + work (w) |
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Thermal energy = |
RT |
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Volume Work = |
-PdeltaV P is pressure, V is volume |
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Enthalpy When it's positive? When it's negative? |
heat transferred in a reaction endothermic exothermic |
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Standard state (explanation of plimsols) |
25 degrees C and 1 atm |
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Activity |
Concentration (c / c standard) or pressure (p / p standard) In pure solids/liquids, a = 1 |
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Bond Energies (D) |
energy needed to break 1 mol of a type of bond in the gaseous state |
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Change in Enthalpy = |
Sum of D(broken) - Sum of D(formed) **"Just do it in order" |
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Entropy |
disorder of a system |
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Entropy = Just in case this calculation's needed |
..........R * ln(w) ____________ (#avogadro) |
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If Entropy goes up... |
more disordered and favorable |
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If Entropy goes down... |
less disordered, less favorable |
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Keep track of Entropy through # of |
moles of gas |
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Free Energy general equation |
G=H-TS |
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When deltaG is less than 0... |
favorable reaction (spontaneous) |
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when deltaG is greater than 0... |
not favorable |
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Equilibrium constant is with a _______ K. |
CAPITAL |
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Rate Constant is with a ___________ K. |
lowercase |
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xX + yY <--> zZ Equilibrium constant= |
a^z(Z) _____________ a^x(X)a^y(Y) or just products over reagents |
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Activation Energy |
required energy to initiate reaction |
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Reaction Rates are dependent upon... |
Collision frequency, fraction of successful collisions, and temperature |
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Catalysts |
speed reactions up by decreasing activation energy deltaG doesn't change |
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If... 1. K>1 2. K=1 3. K<1 |
1. deltaG <0 , forward reaction favorable 2. deltaG=0, equilibrium 3. deltaG>0, reverse reaction favorable |
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Heterogeneous solution |
not uniform throughout |
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Homogeneous solution |
uniform throughout |
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(Solute/solvent) dissolves in the (solute/solvent) |
Solute; solvent |
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3 kinds of concentration |
Molarity, % by mass, % by volume |
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Density |
mass / volume |
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"solvated" |
solvent surrounds solute molecules |
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"hydrated" |
solvated with water as solvent |
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Solubility |
max amount of solute that can be dissolved in a volume of solvent at a given temperature |
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When it comes to dissolving... |
"like dissolves like" |
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Organic compounds |
molecules containing carbon |
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Electrolytes |
substances that form ions in solution |
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Trends with electrolytes |
more ions that dissolve, stronger electrolyte |
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Precipitation |
formation of insoluble substance from two different soluble substances |
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Solubility Rules: |
1. Group 1A metals and NH4 are soluble 2. NO3's, ClO4's, ClO3's, and C2H3O2's are soluble 3. Cl's, Br's, and I's are soluble EXCEPT Ag, Cu, Tl, Hg2 and Pb 4. SO4's are soluble EXCEPT Ca, Sr, Ba, and Pb 5. Most other ionic compounds are insoluble. |
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Net ionic equation |
balanced equation for formation of precipitate only |
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K(sp) |
solubility product constant |
