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Chem 2 EXAM 1
| Term | Definition |
|---|---|
| Molarity (M) | Amount of solute (mol)/ volume solution (L) |
| Molality (m) | amount of solute (mol)/ mass solvent (kg) |
| Mole Fraction (x) | amount solute (mol)/ total amount of solute and solvent (mol) |
| Mol Percent (mol %) | amount of solute (mol)/ total amount of solute and solvent (mol) x100 |
| Parts by mass | mass solute / mass solution x (multiplication factor) |
| Multiplication factor: Percent by mass | x100 |
| Multiplication factor: Parts per million by mass (ppm) | x10^6 |
| Multiplication factor: Parts per billion by mass (ppb) | x10^9 |
| Parts by Volume | volume solute / volume solution x multiplication factor |
| VSEPR theory | explains and predicts molecular geometry around a central atom |
| linear | 2 bonding and 0 lone pairs or 2 bonding 3 lone pairs |
| bent | 2 bonding 1 lone pair or 2 bonding and 2 lone pairs |
| trigonal planar | 3 bonding and 0 lone pairs |
| trigonal pyramidal | 3 bonding and 1 lone pair |
| tetrahedral | 4 bonding 0 lone pairs |
| trigonal bipyramidal | 5 bonding and 0 lone pairs |
| seesaw | 4 bonding and 1 lone pair |
| t shaped | 3 bonding 2 lone pairs |
| octahedral | 6 bonding and 0 lone pairs |
| square pyramidal | 5 bonding 1 lone pair |
| square planar | 4 bonding 2 lone pairs |
| If a molecule has one polar bond... | it has net dipole moment; is a polar molecule |
| What are the most electronegative atoms | F O N/Cl |
| When the F,O,N,CL are paired together they are... | polar |
| Non polar | no lone pairs and identical bonds |
| what molecular geometries are ALWAYS nonpolar? | linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral |
| what molecular geometries are polar? | bent, trigonal pyramidal, seesaw, t shaped, and square pyramidal |
| What geometries CAN cancel out and tend to be nonpolar | square planar and linear |
| Properties of gas | low density indefinite shape indefinite volume weak IMF |
| Properties of liquids | high density indefinite shape definite volume moderate IMF |
| Properties of solids | high density definite shape definite volume strong IMF |
| Crystalline solids | regular ordered structure |
| Amorphous Solids | no long range order |
| How do you move from solid > liquid > gas | increase temp |
| How do you move from gas > liquid > solid | decrease temp |
| Increasing pressure | favors more dense (solids) |
| Decreasing pressure | favors less dense (gas) |
| Intermolecular forces are.. | BETWEEN molecules |
| Bonds are... | WITHIN Molecules |
| What is stronger, bonds or IMF? | bonds |
| LDF (dispersion) | between ALL neutral particles only IMF between non-polar molecules Increases w surface area and size |
| Dipole-Dipole | between polar molecules |
| hydrogen bonding | between N-H, O-H, F-H strongest IMF in pure substance |
| Ion-Dipole | between polar molecules and Ions |
| polar solvents for... | polar or ionic solutes |
| non-polar solvents for... | non-polar solutes |
| as molar mass increases so does | boiling point, melting point, and viscosity |
| as IMF increase so does | boiling point, melting point, viscosity, and surface tension |
| Vaporization | process by which thermal energy can overcome IMF and produce a state change from liquid to gas |
| The rate of vaporization increases with | increasing temp and surface area |
| volatile | liquids that vaporize easily (weak IMF) |
| nonvolatile | don't vaporize easily (strong IMF) |
| Vaporization is endo/exo? | endothermic |
| the heat required to vaporize on mole of liquid to gas is | heat (enthalpy) of vaporization. increases with increasing IMF |
| dynamic equilibrium | rate of condensation and rate of vaporization are equal |
| Vapor pressure | pressure of gas when in dynamic equilibrium depends on temp and IMF |
| boiling point of a liquid | temp at which the liquids vapor pressure equals external pressure |
| normal boiling point of a liquid | temp at which the vapor pressure equals 1 atm |
| supercritical fluid | neither liquid nor gas, the temp at which the transition to a supercritical fluid occurs is the critical temperature, the pressure at which the transition occurs is the critical pressure |
| sublimation | the transition from solid directly to gas |
| deposition | transition gas directly to solid |
| melting or fusion is... | the transition from solid to liquid |
| freezing is... | transition from liquid to solid |
| 0 degrees Celsius | melt and freeze |
| 100 degrees Celsius | vaporization and condensation |
| heat of fusion | heat required to melt 1 mole of a solid |
| fusion is... | POSITIVE |
| melting is... | endothermic |
| triple point | the set of conditions at which three states are equally stable and in equilibrium |
| critical point | the temp and pressure above which a supercritical fluid exists |
| if the fusion curve has a positive slope, | the solid state is more dense |
| if the fusion curve has negative slope, | the liquid state is more dense |
| entropy | a measure of energy randomization or energy dispersal in a system |
| entropy increases when | the gases mix |
| What happens when you remove the barrier between gases? | they will mix naturally and increase disorder or entropy |
| how do IMF effect solutions | may contribute or oppose the formation of a solution |
| intermolecular forces exist between: | a) solvent-solute b) solvent-solvent c) solute-solute |
| miscible | when two liquids form a homogeneous solution in all proportions |
| 3 steps of forming solution: | 1. separating the solute into constituent particles 2. separating the solvent particles from each other to make the solute particles 3. mixing the solute and solvent particles |
| enthalpy of solution | is the overall enthalpy change of solution formation |
Created by:
gkarabinas
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