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| 258904963 | ion-dipole force | intermolecular force existing between an ion and the partial charge on the end of a polar molecule | |
| 258904964 | ion-dipole forces occur between an ______ and the partial charge on the end of a _________. | ion, polar molecule | |
| 258904965 | The magnitude of attraction increases as either the ___________ or the __________ increases. | charge of the ion, magnitude of the dipole moment | |
| 258904966 | All intermolecular forces tend to be less than ___________ percent as strong as covalent or ionic bonds. | 15 | |
| 258904967 | dipole-dipole forces | intermolecular force existing when a neutral polar molecules attracts each other when the positive end of one molecule is near the negative end of another | |
| 258904968 | Dipole-dipole forces are effective only when __________ are very close together. | polar molecules | |
| 258904969 | Dipole-dipole forces are generally __________ than ion-dipole forces. | weaker | |
| 258904970 | For molecules of approximately equal mass and size, the strengths of intermolecular attractions _____ with increasing _________. | increase, polarity | |
| 258904971 | Boiling point __________ as the dipole moment _______. | increases, increases | |
| 258904972 | London dispersion force | intermolecular force when the temporary dipole on one non polar atom can induce a similar temporary dipole on an adjacent non-polar atom, causing the atoms to be attracted to each other | |
| 258904973 | polarizability | the ease with which the electron distribution in a molecule is distorted | |
| 258904974 | More polarizable molecules have _______ dispersion forces. | stronger | |
| 258904975 | Dispersion forces tend to _____ in strength with _________ molecular weight. | increase, increasing | |
| 258904976 | When the molecules of two substances differ widely in molecular weights, __________ __________ tend to be decisive in determining which substance has the stronger intermolecular attractions. | dispersion forces | |
| 258904977 | hydrogen bonding | a special type of intermolecular attraction between the hydrogen atom in a polar bond (particularly an H-F, H-O, or H-N bond) and an unshared electron pair on a nearby small electronegative ion or atom (usually an F, O, or N atom in another molecule) | |
| 258904978 | Because the electron-poor hydrogen is so small, it can approach an ________ atom very closely and thus interact _____ with it. | electronegative, strongly | |
| 258904979 | viscosity | the resistance of a liquid to flow | |
| 258904980 | Viscosity depends on the _________ __________ between molecules and on whether ______ ______ exist that can cause the molecules to become entangled. | attractive forces, structural features | |
| 258904981 | surface tension | the energy required to increase the surface area of a lquid by a unit amount | |
| 258904982 | As temperature _________, viscosity ________ and surface tension __________. | increases, decreases, decreases | |
| 258904983 | As intermolecular forces of attraction become ______, viscosity ________ and surface tension __________. | stronger, increase, increase | |
| 258904984 | cohesive forces | intermolecular forces that bind similar molecules to one another, such as the hydrogen bonding in water | |
| 258904985 | adhesive forces | intermolecular forces that bind a substance to a surface | |
| 258904986 | meniscus | u-shaped curved upper surface of water that results from the adhesive forces between the water and the glass that are greater than the cohesive forces between water molecules | |
| 258904987 | capillary action | the rise of liquids up very narrow tubes | |
| 258904988 | The adhesive forces between the liquid and the walls of the tube tend to ________ the surface area of the liquid. | increase | |
| 258904989 | The surface tension of the liquid tends to ______ the area, thereby pulling the liquid _____ the tube. | reduce, up | |
| 258904990 | Do the viscosity and surface tension of a substance reflect adhesive forces or cohesive forces of attraction? | cohesive | |
| 258904991 | phase changes | transformations from one state of matter to another | |
| 258904992 | heat of fusion (enthalpy of fusion) | energy required to cause molecules of solid to move into the liquid state | |
| 258904993 | Heat of vaporization values tend to be ______ than heat of fusion values because in the transition from the _____ to the _____ state, the molecules must essentially sever all their intermolecular attractive interactions; whereas in melting, many of these attractive interactions remain. | larger, liquid, vapor | |
| 258904994 | heat of vaporization (enthalpy of vaporization) | energy required to cause the molecules of the liquid to move into the gaseous state | |
| 258904995 | Heat of freezing is _____________. | exothermic | |
| 258904996 | Heat of deposition is ___________. | exothermic | |
| 258904997 | heat of sublimation | enthalpy change required for molecules of a solid to be transformed directly into the gaseous state | |
| 258904998 | supercooling | removing heat from a liquid so we can temporarily cool it below its freezing point without forming a solid; occurs when heat is removed from a liquid so rapidly that the molecules literally have no time to assume the ordered structure of a solid; unstable | |
| 258904999 | critical pressure | pressure required to bring about liquefaction at critical temperature | |
| 258905000 | critical temperature | the highest temperature at which a distinct liquid phase can form | |
| 258905001 | Nonpolar, low molecular weight substance tend to have ______ intermolecular attractions and ____ critical temperatures and pressures than those that are polar or of higher molecular weight. | weak, lower | |
| 258905002 | vapor pressure | the pressure of the vapor of the substance | |
| 258905003 | dynamic equilibrium | condition in which two opposing forces are occurring simultaneously at equal rates | |
| 258905004 | The ______ of a liquid is the pressure exerted by its vapor when the liquid and vapor states are in ______ _______. | vapor pressure, dynamic equilibrium | |
| 258905005 | volatile | liquids that evaporate readily | |
| 258905006 | Substances with ______ vapor pressure evaporate ______ _______ than substances with ____ vapor pressure. | high, more quickly, low | |
| 258905007 | Hot water evaporates ____ ______ than cold water because _____ ______ increases with increasing temperature. | more quickly, vapor pressure | |
| 258905008 | normal boiling point | boiling point of a liquid at 1 atm | |
| 258905009 | Higher ________ causes water to boil at a _______ temperature, thereby allowing the food to get hotter and to cook more rapidly. | pressure, higher | |
| 258905010 | The atmospheric pressure is _____ at higher altitudes, so water boils at a _____ temperature. | lower, lower | |
| 258905011 | phase diagram | a graphical way to summarize the conditions under which equilibria exist between the different states of matter | |
| 258905012 | The line from A to B is the | vapor-pressure curve of the liquid. | |
| 258905013 | critical point (B) | the critical temperature and pressure of the substance; beyond it, the liquid and gas phases become indistinguishable from each other | |
| 258905014 | line AC represents the | variation in the vapor pressure of the solid as it sublimes at different temperatures | |
| 258905015 | line AD represents the | change in melting point of the solid with increasing pressure | |
| 258905016 | Line AD usually slopes to the ______ because for most substances the _____ form is denser than the _____ form. | right, solid, liquid | |
| 258905017 | the melting point of a substance is identical to the | freezing point | |
| 258905018 | normal melting point | melting point at 1 atm | |
| 258905019 | triple point (A) | where all three curves intersect; all three phases are in equilibrium at this temperature and pressure | |
| 258905020 | crystalline solids | atoms, ions, or molecules are ordered in well-defined arrangements with flat aces in definite angles | |
| 258905021 | amorphous solids | a solid whose particles have no orderly structure, well-defined faces, or shapes and whose mixture of molecules do not stack well together | |
| 258905022 | Quartz is a(n) | crystalline solid. | |
| 258905023 | Diamond is a(n) | crystalline solid. | |
| 258905024 | Rubber is a(n) | amorphous solid. | |
| 258905025 | Glass is a(n) | amorphous solid. | |
| 258905026 | unit cell | repeating unit of a solid, the crystalline "brick | |
| 258905027 | crystal lattice | three-dimensional array of points | |
| 258905028 | lattice point | each point in the lattice which represents an identical environment within the solid | |
| 258905029 | primitive cubic (or simple cubic) | unit cell in which the lattice points are at the corners only | |
| 258905030 | body-centered cubic | unit cell in which a lattice point occurs at the corners and at the center of the unit cell | |
| 258905031 | face-centered cubic | unit cell in which there are lattice points at the center of each face as well as at each corner | |
| 258905032 | parallelepipeds | six-sided figures whose faces are parallelograms | |
| 258905033 | hexagonal close packing | if the spheres of the third layer are place in line with those of the first layer | |
| 258905034 | cubic close packing | if the spheres of the third layer can be placed so they do not sit above the spheres in the first layer | |
| 258905035 | coordination number | the number of particles immediately surrounding a particle in the crystal structure | |
| 258905036 | In both ______ close packing and ______ close packing, _____ percent of the total volume of the structure is occupied by ______ and ______ percent is empty space between the spheres. | hexagonal, cubic, 74, 26 | |
| 258905037 | In primitive cubic structure, the coordination number is ______ and only _____ percent of the space is occupied | 6, 52 | |
| 258905038 | When unequal-sized spheres are packed in a lattice, the larger particles sometimes assume one of the _________ arrangements, with the smaller particles occupying the _____ between the larger spheres. | close-packed, holes | |
| 258905039 | The higher the _________, the _______ the packing efficiency. | coordination number, greater | |
| 258905040 | molecular solids | solids consisting of atoms or molecules held together by (weak) intermolecular forces; soft, low melting pints, mostly gases/liquids at room temperature | |
| 258905041 | Ar is a | molecular solid. | |
| 258905042 | H20 is a | molecular solid. | |
| 258905043 | CO2 is a | molecular solid. | |
| 258905044 | The properties of molecular solids depend not only on the __________ of the forces that exist between the molecules, but also on the abilities of the molecules to ________ efficiently in three dimensions. | strengths, pack | |
| 258905045 | diffraction | when light waves pass through a narrow slit, they are scattered in such a way that the wave seems to spread out | |
| 258905046 | array detector | device analogous to that used in digital cameras to capture and measure the intensities of diffracted rays | |
| 258905047 | covalent-network solids | solids consisting of atoms held together in large networks or chains by covalent bonds; hard, high melting points | |
| 258905048 | Diamond is a | covalent-network solid. | |
| 258905049 | Graphite is a | covalent-network solid. | |
| 258905050 | Two allotropes of carbon are | covalent-network solids. | |
| 258905051 | Quartz is a | covalent-network solid. | |
| 258905052 | The interconnected three-dimensional array of strong ______-_______ bonds contributes to diamonds's unusual hardness. | carbon-carbon | |
| 258905053 | In graphite, the carbon atoms are arranged in layers of interconnected _____ _____. | hexagonal rings | |
| 258905054 | Electrons move freely through the ______ orbitals, making graphite a good ______ of _____ along the layers | delocalized, conductor, electricity | |
| 258905055 | ionic solids | solids consisting of ions held together by bonds | |
| 258905056 | The strength of an ionic bond depends greatly on the ______ of the ______. | charges, ions | |
| 258905057 | The structure adopted by an ionic solid depends largely on the ____ and the relative _____ of the ions. | charges, sizes | |
| 258905058 | metallic solids | solids consisting entirely of metal atoms | |
| 258905059 | Metallic solids usually have a _________ close-pakced, _____ close-pakced, or ________ cubic structures. | hexagonal, cubic, body-centered | |
| 258905060 | Bonding in metals is too strong to be due to ______ forces, and yet there are not enough valence electrons for ordinary ____ bonds between atoms; the bonding is due to valence electrons that are ______ throughout the entire solid. | London-dispersion, covalent, delocalized | |
| 258905061 | The strength of the bonding _______ as the number of electrons available for bonding ______. | increases, increases | |
| 258905062 | In both cubic close packing and hexagonal close packing, each sphere has a coordination number of ______. | 12 |
