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Chemistry: Chapter 6
Intermolecular Forces: Boiling Point, Freezing/Melting Point, Density, etc.
| Term | Definition |
|---|---|
| equilibrium | can be met in closed systems (bottles), and is established liquid and vapor |
| vapor pressure | the partial pressure of the vapor over a liquid measured at equilibrium at a given temperature |
| dynamic equilibrium | when the transfer rate between liquid and gas are equal; pressure is equal to molecules; normal pressure will equal the vapor pressure of the liquid; as pressure increases, temperature increases |
| statistic equilibrium | when molecules get into the gas phase, they stay there as the temperature increases, the kinetic energy of the gas changes; more molecules will enter the gas phase |
| more molecules in the vapor phase translates to | vapor pressure |
| volatile liquids and solids | liquids and solids which have relatively high vapor pressures at normal temperatures |
| boiling point | where vapor pressure equals ambient pressure |
| tabulated | recorded numerically; how ambient pressure is recorded |
| normal boiling point | the temperature where vapor pressure equals 1 atm |
| where does evaporation occur when a liquid is below boiling point? | the surface |
| at boiling point what is the liquid equal to? | ambient pressure |
| freezing/melting point | temperature at which a liquid and solid are in dynamic equilibrium; relatively insensitive to small changes in pressure |
| what do changes in phase require? | energy |
| heat of phase transition | amount of heat absorbed or evolved during phase change |
| heat of fusion | energy it takes to perform the phase change; ice must absorb 6.01 kJ/mol & water freezes at -6.01 kJ/mol |
| heat of vaporization | 40.7 kJ/mol absorbed or released to form new states; why steam burns worse then water |
| Clausius-Clapeyron equation | relates vapor pressure of vaporization |
| intermolecular forces | relatively weak forces of interaction between molecules; weaker than iconic and covalent bonds; explain the physical properties of liquids and solids; can keep molecules in liquid phase; effect the ability of molecules to reach the vapor phase |
| London Dispersion Forces | football shape; distribution of electrons may be imperfect, forming an instantaneous dipole |
| polarizability | the ease at which the electron cloud in a molecule, ion, or atom can be distorted |
| dispersion | momentary shift in electron density |
| dipole-induced dipole is caused by | proximity of polar molecules |
| factors effecting strength of dispersion | size: the larger, the more polarizable; dispersion increases with polarizability shape: increase in area equals increase in molecule interaction boiling point increases with mass increase in noble gases and halogens |
| constitutional isomers | same formulas, different constitutions between atoms in molecules; higher surface area causes stronger interactions and vise versa; strength affects physical and chemical properties |
| dipole-dipole forces | attractive forces between the positive end and a negative end of another molecule; align into a plus minus fashion |
| ion-dipole forces | result from electrostatic attraction between an ion and a neutral, polar molecule; commonly found in solutions; cation attracts negative polar molecule end; anion attracts positive polar molecule end; magnitude of the polar dipole increases |
| hydrogen bond | a weak to moderately strong attractive force between an H atom covalently bonded to a highly electronegative atom (F,O, and N); stringer than van Der Walls forces; can be mixed and matched |
| characteristics of hydrogen bonds | vary in strength, responsible for some properties of liquid and solid water and the 2nd structure of proteins; generally weak |
| solution | a homologous mixture of 1 or more substances (solutes) that are dispersed in a medium |
| solute | present in smallest number of moles (component) |
| solvent | component that is present in largest number of moles |
| solubility | maximum dissolvable quantity in a given volume of solution |
| miscible | liquids that are mutually soluble in any proportion |
| solubility | depends on relative strength of solute, compared to solute-solute or solvent-solvent; ionic/polar solutes will be soluble in polar solvents; non polar solutes soluble in non polar solvent |
| ion-dipole | attractive force between an ion and a molecule that has a permanent dipole |
| sphere of hydration | cluster of water molecules surrounding an ion in aqueous medium |
| sphere of solvation | not water; but some other solvent; like forces = a solution; dissimilar forces = no solution |
| solubility decreases | energy of hydration bonding decreases and dispersion increases |
| inter molecular forces characteristics | attractive forces compared to kinetic energy |
| temperature characteristics | affects kinetic energy of atoms and molecules |
| pressure characteristics | affects distance between atoms |
| phase diagram | a graphical way to summarize conditions under which different phases of substances are stable; stability of gas, liquids, and solids are represented as a function of pressure and temperature |
| curve AB | shows equilibrium of solids and liquids under pressure and temperature; gives the freezing/melting point of water as a function of pressure |
| Curve AC | represents the vapor pressure of the liquid as a function of temperature, or boiling point as a function of pressure |
| curve AD | vapor pressure of the solid as a function of temperature, or boiling point as a function of pressure |
| point A | the triple point and where all three phases are at temperature and pressure equilibrium |
| point C | the critical point where the liquid-vapor curve ends (374 degrees and 218 atm) |
| viscosity | the resistance to flow of a liquid; the stronger the IMFs, the more viscous the liquid is; temperature increases, and viscosity decreases |
| surface tension | energy needed to separate the molecules at the surface of a liquid; attractive forces increase and surface tension increases; expands liquid surface area |
| adhesive forces | interactions between unlike particles |
| cohesive forces | interactions between like particles |
| concave | adhesive is greater than or equal to cohesive forces |
| convex | cohesive greater than adhesive forces |
| capillary action | ability of a liquid to spontaneously flow against gravity; adhesive forces are in the tube, and cohesive forces are in the liquid |
| what does water's density do as it freezes? | it decreases |
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livabirch4
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