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49 Cards in this Set
- Front
- Back
What are liquids and solids often referred to as?
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The condensed phases
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How are atoms or molecules held in liquid?
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They are held close together with little space between them
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What does this result in?
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It makes liquids have definite volumes that cannot easily be expanded or compressed
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Can liquid diffuse and evaporate?
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Yes
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What do liquids form when they mix, both with each other and with other phases?
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They form solutions
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What is the degree to which two liquids can mix?
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It is called their miscibility
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What are oil and water?
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They are almost completely immiscible
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What can two immiscible liquids form?
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A fairly homogenous mixture called an emulsion
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What may a solid be?
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It may be crystalline or amorphous
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What is the structure of a crystalline solid?
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It possess an ordered structure
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How do is atoms exist?
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They exist in a specific three-dimensional geometric arrangement with repeating patterns of atoms, ions, or molecules
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What is the structure of an amorphous solid?
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It has no ordered three-dimensional arrangement, although the molecules are also fixed in place
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What are most solids?
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Most are crystalline in structure
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What are ionic solids?
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They are aggregates of positively and negatively charged ions
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Are there any discrete molecules?
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No
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What are the physical properties of ionic solids?
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They include high melting points, high boiling points, and poor electrical conductivity in the solid phase
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What are these properties due to?
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They are due to the compounds’ strong electrostatic interactions, which also cause the ions to be relatively immobile
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What are metallic solids?
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They consist of metal atoms packed together as closely as possible
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What are characteristics of metallic solids?
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They have high melting and boiling points as a result of their strong covalent attractions
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What are pure metallic structures?
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They are usually described as layers of spheres of roughly similar radii
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What are repeating units of crystals?
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They are represented by unit cells
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What are the types of unit cells?
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Simple cubic, body-centered cubic, and face-centered cubic
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What are atoms represented by?
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They are represented by points
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In an isolated system, are phase changes reversible?
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Yes
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Does an equilibrium exist between phases?
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Yes
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What is the temperature of a liquid related to?
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It is related to the average kinetic energy of the liquid molecules
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What is evaporation or vaporization
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It is when some molecules near the surface of a liquid have enough energy to leave the liquid phase and escape into the gaseous phase
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What happens each time the liquid loses a high-energy particle?
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The temperature of the remaining liquid decreases
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What does this imply about evaporation?
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It is a cooling process
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What is condensation?
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It is when some gas molecules go back into the liquid phase
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What is vapor pressure?
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It is the pressure that the gas exerts over the liquid
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How does vapor pressure relate to temperature?
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It increases with temperatures
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Why?
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Because more molecules have sufficient kinetic energy to escape into the gas phase
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What is the term for the temperature at which the vapor pressure of the liquid equals the external pressure?
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The boiling point
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What is the transition from solid to liquid?
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It is called fusion or melting
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What is the process from liquid to solid?
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It is called solidification, crystallization, or freezing
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What is it called when a solid goes directly into the gas phase?
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It is called sublimation
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What is gaseous to the solid phase?
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It is called deposition
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What does a phase diagram depict?
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It shows the phases and phase equilibria of a substance at defined temperatures and pressures
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Where is the gas typically found?
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It is typically found at high temperature and low pressure
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Where is the solid phase found?
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Low temperature and high pressure
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Where is the liquid phase found?
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It is found at high temperature and high pressure
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What is the triple point?
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It is the point on a phase diagram where the three lines meet
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What is the critical point?
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It is the temperature and pressure above which no distinction between liquid and gas is possible
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What does Raoult’s Law do?
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It enables one to determine the relationship between the vapor pressure of A and the concentration of liquid A in the solution
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What are colligative properties?
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They are physical properties derived solely from the number of particles present, not the nature of those particles
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What is the formula for calculating freezing-point depression?
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Tf = Kfm. Tf is the freezing-point depression, Kf is a proportionality constant, and m is the molality of the solution
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When does a liquid boil?
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It boils when its vapor pressure equals the atmospheric pressure
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What if the vapor pressure of a solution is lower than that of the pure solvent?
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More energy and a higher temperature will be required before its vapor pressure equals atmospheric pressure
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