Flashcards and Answers – Chapter 10
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| kinetic-molecular theory |
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| based on the idea that particles of matter are always in motion |
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| ideal gas |
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| a hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory (don't actually exist) |
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| elastic collision |
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| one in which there is no net loss of total kinetic energy |
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| gas expansion |
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| gasses do not have definite shape or a definite volume |
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| gas fluidity |
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| gas particles glide easily past one another. this flow causes gases to behave as liquids do. Both referred to as FLUIDS. |
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| gas Low Density |
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| the density of a gaseous substance at atmospheric pressure is about 1/1000 the density of the same substance in the liquid or solid state. |
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| gas compressibiliy |
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| When they are are full, such cylinders may contain more than 100 times as many particles of gas as nonpressurized containers of the same size could contain. |
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| diffusion |
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| spontaneous mixing of the paricles of two substances caused by their random motion. |
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| effusion |
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| a process by which gas particles pass through a tiny opening |
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| real gas |
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| does not behave completely according to the assumptions of the kinetic-molecular theory |
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| gas forces of attraction |
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| there are no forces of attraction between gas particles |
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| gas temperature |
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| the temperature of a gas depends on the average kinetic energy of the particles of the gas. KE=1/2mv^2. All gases of the same temp have the same kinetic energy. |
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| liquid |
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| a form of matter that has a definite volume and takes the shape of its container. |
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| liquid attraction |
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| cause by the IMF's such as dipoles and London Dispersion forces and hydrogen bonding |
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| fluid |
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| a substance that can flow and therefore take the shape of its container. |
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| liquid density |
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| less dense than a solid, but more than a gas. WATER IS LESS DENSE WHEN IT SOLIDIFIES. |
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| liquid incompressibility |
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| much less compressible than gases. can't be compressed very easily. LOW COMPRESSIBILITY |
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| liquid diffusion |
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| much slower in liquids than in gases, but can go faster as the temp increases. liquid particles diffuse to combine with other liquid particles. |
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| surface tension |
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| a force that tends to pull adjacent parts of a liquid's surface together, thereby decreasing surface area to the smallest possible size. SPHERICAL SHAPE. |
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| Capillary action |
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| the attraction of the surface of a liquid to the surface of a solid. i.e. MENISCUS. |
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| vaporization |
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| the process by which a liquid or solid changes to a gas |
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| Evaporation |
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| the process by which particles escape from the surface of a non boiling liquid and enter the gas state. occurs because the particles of a liquid have different kinetic energies |
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| boiling |
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| the change of a liquid to bubbles of vapor that appear throughout the liquid |
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| Formation of solids - Freezing/solidification |
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| The physical change of a liquid to a solid by removal of energy as heat |
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| crystalline solids |
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| consist of crystals |
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| crystal |
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| a substance in which the particles are arranged in an orderly, geometric, repeating pattern. |
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| amorphous solid |
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| one in which the particles are arranged randomly in a solid |
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| Melting |
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| the physical change of a solid to a liquid by the addition of energy as heat |
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| melting point |
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| The temperature at which a solid becomes a liquid |
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| supercooled liquids |
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| substances that retain certain liquid properties even at temperatures at which they appear to be solid |
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| solid high density/incompressibility |
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| solids have the highest density and incompressibility of all the states of matter. |
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| solid rate of diffusion |
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| they do sometimes diffuse, however, it takes a solid millions of times longer than a liquid or a gas |
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| crystal structure |
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| the total 3-D arrangement of particles of a crystal |
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| unit cell |
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| the smallest portion of a crystal lattice that shows the 3-D pattern of the entire lattice. each crystal lattice contains many of these. |
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| ionic crystals |
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| consists of positive and negative ions arranged in a regular pattern. can be monatomic or polyatomic |
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| covalent network crystals |
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| each atom is covalently bonded to its nearest neighboring atoms |
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| metallic crystals |
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| consists of metal cations surrounded by a sea of delocalized valence electrons |
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| covalent molecular crystals |
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| consists of covalently bonded molecules held together by IMF's |
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| amorphous |
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| without shape |
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| phase |
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| any part of a system that has uniform composition and properties |
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| condensation |
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| the process by which a gas changes to a liquid |
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| equilibrium |
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| a dynamic condition in which two opposing changes occur at equal rates in a closed system. |
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| equilibrium vapor pressure |
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| the pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature |
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| volaile liquids |
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| liquids that evaporate readily (have relatively weak forces of attraction between their particles |
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| boiling |
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| the conversion of a liquid to a vapor within the liquid as well as at its surface |
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| boiling point |
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| the temperature at which the equilibrium vapor pressure of the liquid equals the atmospheric pressure (lower the atmospheric pressure, the lower the boiling point) |
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| vacuum evaporator |
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| causes boiling at lower than normal temperatures |
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| molar enthalpy of vaporization |
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| the amount of energy as heat that is needed to vaporize one mole of liquid at the liquid's boiling point at constant pressure |
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| freezing |
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| the physical change of a liquid to a solid |
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| freezing point |
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| the temperature at which the solid and liquid are in equilibrium at 1 atm |
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| molar enthalpy of fusion |
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| the amount of energy as heat required to melt one mole of solid at the solid's melting point |
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| sublimation |
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| he change of state from a solid directly to a gas |
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| deposition |
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| the change of state from a gas directly to a solid |
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| phase diagram |
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| a graph of pressure versus temperature that shows the conditions under which the phases of a substance exist |
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| triple point |
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| indicates the temperature and pressure conditions at which the solid, liquid, and vapor of the substance can coexist at equilibrium |
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| critical point |
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| indicates the critical temperature and critical pressure |
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| critical temperature |
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| the temperature above which the substance cannot exist in the liquid state |
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| critical pressure |
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| the lowest pressure at which the substance can exist as a liquid at the critical temperature |
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| specific heat |
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| C=mAT/Q |
