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37 Cards in this Set
- Front
- Back
Properties of Liquids
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1. High density compared to gases
2. Indefinite shape and assume shape of container 3. Definite volume; not easily compressed |
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Properties of solids
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1. High density in comparison to gases
2. Definite shape 3. Definite volume 4. Crystalline (ordered) or amorphous (disordered) |
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Properties of gas
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1. Low density
2. Indefinite shape 3. Indefinite volume |
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Which has strong molecular forces? weak?
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1. Strong - solids
2. Weak - gases |
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Crystalline solid versus amorphous solid?
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1. Crystalline - atoms/molecules arranged in an order
2. Amorphous - disordered |
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Intermolecular forces are _____________ than bonding forces.
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1. much weaker
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Dispersion force (London force)
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1. Intermolecular force exhibited by all atoms/molecules that results from fluctuations in the electron distribution.
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An instantaneous dipole on any one helium atom induces _____________________________, which then attract one another.
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1. Instantaneous dipoles on neighboring atoms
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Dispersion force increases with __________ molar mass because _________________________________.
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1. Increasing
2. higher molar mass = more electrons dispersed over greater volume. |
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Boiling points ________ with increasing _______________.
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1. Rise
2. Molar Mass |
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Miscibility - of liquids
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1. Ability to mix without separating into two phases
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Dipole-Dipole force exists______________________.
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1. In all molecules that are polar
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Dipole-Dipole force
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1. Intermolecular force exhibited by polar molecules that results in an uneven charge distribution.
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Permanent Dipole
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1. Permanent separation of charge
2. Molecule always has one end slightly negative and the other slightly positive. |
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Boiling points ______________ with decreasing dipole moment.
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1. Decreases
2. It increases with increasing dipole moment. |
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Hydrogen bond
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1. Strong dipole-dipole attraction force between a hydrogen bonded to O, N or F and one of these electronegative atoms on a neighboring molecule.
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Ion-Dipole forces are present in mixtures between ______________________ and are ___________.
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1. Ionic Compounds and Polar Compounds
2. VERY STRONG 3. Important in aqueous solutions. |
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Four types of Intermolecular forces going from weakest to strongest...
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1. Dispersion
2. Dipole-Dipole 3. Hydrogen Bonding 4. Ion-Dipole |
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Surface Tension
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1. Tendency of liquids to minimize their surface area.
2. Energy required to increase the surface area by a unit amount. 3. Decreases with decreasing intermolecular forces. |
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Viscosity
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1. Resistance of a liquid to flow
2. Greater in substances with strong intermolecular forces because molecules strongly attracted to eachother and don't flow around eachother as easily. |
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Capillary Action
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1. Ability of a liquid to flow against gravity up a narrow tube.
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Vaporization
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1. Phase transition from liquid to gas
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Condensation
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1. Phase transition from gas to liquid
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Volatile vs Non-volatile
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1. Volatile - vaporize easily
2. Nonvolatile - do not vaporize easily |
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Rate of vaporization in comparison to temp, surface, strength of intermolecular forces
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1. RofVap increases with increasing TEMP
2. RofVap increases with increasing SURFACE AREA 3. RofVap increases with decreasing strength of intermolecular forces. |
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Heat of Vaporization
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1. Amount of heat required to vaporize one mole of a liquid to gas
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Dynamic Equilibrium...
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1. Rate of evaporation = Rate of Condensation
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Strong Intermolecular Forces result in _______________ substances and ___________ vapor pressures.
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1. Nonvolatile
2. Low |
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Boiling point of a liquid
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1. Temperature at which vapor pressure equals external pressure.
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Critical Pressure/Temperature
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1. Point at which liquid cannot exist
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Sublimation vs deposition
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1. Phase transition from solid to gas - Sublimation
2. Phase transition from gas to solid - deposition |
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Melting/Fusion vs freezing
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1. Phase transition from solid to liquid - melting/fusion
2. Phase transition from liquid to solid - freezing |
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How large is the band gap in a conductor, semiconductor and insulator?
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1. Conductor - no energy gap
2. Semiconductor - small energy gap 3. Insulator - large energy gap |
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n-type semiconductor vs p-type semiconductor?
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1. N-type: charge carries are negatively charged
2. P-type: hole acts as a positive charge |
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Diodes
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1. Elements that allow the flow of electrical current in one direction.
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Solute vs Solvent
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1. Solvent - majority
2. Solute - minority |
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Entropy
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1. Energy randomization or energy dispersal in a system.
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