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Chapter 10
General Chemistry 2 Spring Semester 2026
| Question | Answer |
|---|---|
| Why is an electrostatic potential map (EMP) used? | To represent electron distribution |
| What does red represent on an EPM? What does blue represent? | Red= electron rich Blue= electron poor |
| Properties of a solid (density, motion, and strength of intermolecular forces) | High, very limited freedom of motion, and strong IMFs |
| Properties of a liquid (density, motion, and strength of intermolecular forces) | High, some freedom of motion, and moderate IMFs |
| Properties of a gas (density, motion, and strength of intermolecular forces) | Low, complete freedom of motion, and weak IMFs |
| What does △H crystalization equal? | - △H fusion |
| What does △H vaporization equal? | - △H condensation |
| What does △H sublimation equal? | △H fusion + △H vaporization |
| What is another word for fusion? | Melting |
| Intermolecular forces definition | Attractive forces that exist between all molecules and atoms |
| What are the four types of intermolecular forces (weakest to strongest)? | Dispersion forces Dipole-dipole forces Hydrogen bonding Ion-dipole forces |
| Dispersion Forces | An intermolecular force exhibited by all atoms and molecules that results from fluctuations in the electron distribution |
| Induced dipole | The temporary dipole establish in one molecule, induces a temporary dipole on its neighboring atoms, which then attract one another |
| What does a larger molar mass mean? | More electrons= a larger electron cloud= increased polarizability= stronger attractions |
| What does more surface-to-surface contact mean? | Larger induced dipole= stronger attraction |
| How does molecular shape affect dispersion forces? | the straighter the shape, the stronger dispersion force= a higher melting/boiling point |
| A polar molecule has a ____ dipole | permanent |
| What do all polar molecules display? | A dipole-dipole intermolecular forces |
| What are dipole-dipole forces? | An intermolecular force exhibited by polar molecules that results from an uneven charge distribution |
| Compare the melting and boiling points of polar vs nonpolar molecules | Polar molecules have a higher melting and boiling point than nonpolar molecules |
| What is hydrogen bonding? | Polar molecules containing H atoms bonded directly to smalle and highly electronegative F, O, or N atoms |
| Order dipole-dipole, hydrogen bonding, and LDF forces from weakest to strongest | LDF then dipole-dipole then hydrogen bonding |
| When do ion-dipole forces form? | Occurs when an ionic compound is mixed with a polar compound |
| What is the strongest type of IMF? | Ion dipole |
| When does ion-dipole forces occur? | When an ionic compound is mixed with a polar compound |
| What are the three intermolecular manifestations that we can observe in liquids? | Suface tension Viscosity Capillary action |
| What are factors that affect surface tension? What happens to the surface tension? | Stronger intermolecular attractive forces, the higher the surface tension Raising the temperature of a liquid reduces its surface tension |
| Surface tension definition | The energy required to increase the surface are of a liquid by a unit amount The tendency of liquids to minimize their surface area |
| What is viscosity (definition)? | The resistance of a liquid to flow |
| What are factors that affect viscosity? How is viscosity affected? | Stronger intermolecular forces --> higher viscosity Higher temperature --> lower viscosity |
| What state of matter transformation is happening in vaporization? | liquid to gas |
| What state of matter transformation is happening in condensation? | gas to liquid |
| What kind of process is vaporization? Why? | Endothermic, energy is needed to overcome IMFs |
| What kind of a process of condensation? | Exothermic |
| What is the Heat of vaporization? | the amount of heat required to vaporize one mole of a liquid to a gas |
| Describe sublimation (phase change, endo/exothermic) | solid to gas Endothermic |
| Describe vaporization (phase change, endo/exothermic) | liquid to gas endothermic |
| Describe fusion (phase change, endo/exothermic) | solid to liquid endothermic |
| Describe freezing (phase change, endo/exothermic) | liquid to solid exothermic |
| Describe condensation (phase change, endo/exothermic) | gas to liquid exothermic |
| Describe deposition (phase change, endo/exothermic)Describe (phase change, endo/exothermic) | liquid to solid exothermic |
| what does rate of vaporization increase with? | Increasing temperature, increasing surface area, decreasing strength of intermolecular forces |
| Vapor pressure definition | The pressure of a gas is in a dynamic equilibrium with its liquid |
| dynamic equilibrium definition | rate of condensation equals rate of evaporation |
| what are factors that affect vapor pressure | IMFs (weak IMFs, high vapor pressure) Temperature (higher temperature, higher vapor pressure) |
| What is the boiling point of a liquid? | The temperature at which the liquid's vapor pressure = the external pressure |
| What is the normal boiling point of a liquid | The temperature at which tis vapor pressure equals 1 atm |
| What is the normal boiling point of water? | 100 degrees Celcius |
| As IMFs increase, surface tension... | increases |
| As IMFs increase, rate of vaporization... | decreases |
| As IMFs increase, vapor pressure... | decreases |
| As IMFs increase, heat of vaporization... | increases |
| As IMFs increase, boiling point... | increases |
| As IMFs increase, melting point... | increases |
| As IMFs increase, viscosity... | increases |
| Phase diagram purpose | Map of the states of a substance as a function of pressure (y-axis) and temperature (x-axis) |
| What are the regions of a phase diagram? What do they represent? | The three main regions are solid, liquid and gas Represent conditions where that particular state is stable |
| What are the lines on a phase diagram? | The substance is in equilibrium between the two states on either side of the line Both states coexist and are equally stable |
| What is the triple point | the three states are equally stable (coexist) and in equilibrium |
| What is miscibility | the ability to mix without separating into two liquids |
| What is the rule of thumb when it comes to miscibility? What does it mean? | like dissolves like Poloar substances dissolve in polar solvents Nonpolar molecules dissolve in non-polar solvents |
| What happens when two liquids do not mix? | They are immiscible |
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