chem ch. 10
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Created by:
katieshaughnessy013 on February 14, 2011
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43 terms
Terms | Definitions |
|---|---|
 liquids | have a definite volume but take the shape of the container |
| liquid particles | in constant random motion; close together due to strong attractive forces |
| attractive forces of liquid particles | dipole-dipole, london dispersion, hydrogen bonding |
| fluid | a substance that flows and takes the shape of its container |
| properties of liquids | high density, incompressible, ability to diffuse, surface tension, capillary action, vaporization and evaporation, ability to freeze |
| high densities of liquids? | molecules are very close together |
| liquids incompressible? | not much space to allow a liquid to allow a liquid to be compressed (molecules close together) |
| liquids can diffuse? | molecules move randomly. slower than in gases; particles much closer together |
| liquids surface tension? | decreases surface area to the smallest possible size because of favorable liquid |
| capillary action | a favorable interaction between a liquid and the surface of a solid (plants move water from roots to other parts of the plant) |
| liquids evaporate and boil? | undergo vaporization and evaporation |
| vaporization | phase change from liquid to gas |
| evaporation | phase change from liquid to gas occurs under nonboiling conditions (i.e, rain puddles drying up, clothes drying when hung up) |
| why does evaporation occur? | some molecules posses high enough KE to enter the gas phase |
| liquids can freeze? | phase change from liquid to highly ordered and dense solid state -- particles do not posses enough KE to move around a lot |
| solids have strong... | IMFs: dipole-dipole, london dispersion, hydrogen bonding |
| crystalline solid | particles in highly ordered patterns |
| amorphus solid | particles randomly arranged |
| solids have definite volume because... | particles are close together |
| solids have definite shape because... | strong IMFs do not allow particles to flow |
| melting point | defined temp at which solids change into liquids; unique to each pure substance and related to strength of IMFs |
| amorphus solids-definite melting point? | none, melting range of temperatures instead |
| solids are incompressible because... | all space is occupied by closely packed particles |
| solids have a slow rate of _____ | diffusion |
| types of crystalline solids | ionic, covalent network, metallic, and covalent molecular |
| ionic crystals | consist of cations and anions arranges in a regular pattern |
| covalent network crystals | consist of covalently bonded atoms; the whole crystal is one "molecule." (diamond, C) |
| metallic crystals | consist of metal nuclei surrounded by a sea of electrons - each metal atom's valence electrons contribute to/are shared with the "electron sea" |
| covalent molecular crystals | consist of regularly arranged crystals of molecules held together by intermolecular forces; ice crystals are an example of them - soft, easily vaporized, low melting points |
| glasses and plastics are... | amorphus solids |
| properties of gas | weakest IMF, expand to fill containers, fluids, low density, are compressible, high rates of diffusion and effusion |
| high pressure and low temperature make gases... | deviate from ideal behavior |
| polar gases have greater forces of _______ that _____ | attraction; deviate from ideality |
| types of phase equilibria | solid-liquid, solid-vapor, vapor-liquid |
| equilibrium vapor pressure | pressure that a vapor exerts when a liquid and its vapor are in equilibrium at a constant temperature |
| why does temperature remain constant in freezing and melting? | energy is related to phase change |
| sublimation and deposition | a phase change that occurs between solids and gases |
| sublimation | the phase change from a solid directly to gas |
| deposition | the phase change from a gas/vapor to solid |
| triple point | the temperature and pressure at which all three phases of solid, liquid, and gas coexist in equilibrium |
| critical point | intersection of critical temp and crit. pressure |
| critical temperature | the substance cannot exist as a gas above this temperature regardless of pressure |
| critical pressure | the lowest pressure at which the substance can exist as a liquid |
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