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Chemistry 2- 11
chapter 11 vocab
| Question | Answer |
|---|---|
| What are Liquids and Solids collectively known as? | condensed state |
| Why are liquid and solids called the condensed state? | they are alike to each other then they are to the gas phase |
| What are some characteristics of solids? | definite volume and shape |
| What are some characteristics of liquids? | indefinite shape and definite volume |
| What are some characteristics of gas'? | indefinite shape and volume |
| what is the fundamental difference between the states of matter? | the distance between particles and the freedom of movement |
| What are all the phase changes? | melting, vaporization, freezing, condensation, sublimation, and deposition |
| What is vaporization? | at a temperature, the molecules of a liquid phase have enough thermal energy to escape the liquid phase and go on to the gaseous phase |
| What is vapor pressure? | the partial pressure of a vapor over a liquid is measured at equilibrium (happens at a particular temperature |
| What is a dynamic equilibrium? | as molecules escape the liquid phase they pressure they exert increases until a dynamic equilibrium is reached |
| What is one factor of vapor pressure? | temperature- as temperature increases so does vapor pressure |
| what does volatile mean? | evaporates quickly |
| what is a boiling point of a liquid? | the temperature in which vapor pressure equals 1 atm |
| what is the relationship between boiling point and pressure? | high vapor pressure= low boiling point low vapor pressure= high boiling point |
| how do you increase boiling point? | increase pressure |
| how do you decrease boiling point? | decrease pressure |
| how do states of matter change? | increase there energy |
| What is heat of fusion? | the energy required to melt a solid |
| what is heat of vaporization? | energy required to change a liquid to a gas |
| Why does the temperature stay constant during phase transitions? | because the heat added is used as energy is used to pull the molecules apart |
| what is a phase diagram? | visualizes the states of matter at particular temperature and pressure as well as where equilibrium exists between the phases |
| what are the two most important points on a phase diagram? | critical point and triple point |
| what is a critical point? | a temperature and pressure in which liquids and gases become indistinguishable after that point- the phase is called a superfluid |
| what is a triple point? | a temperature and pressure in which solids, liquids, and gases are at a equilibrium (all occur) |
| why is water's phase diagram atypical? | high vapor pressure favors solid (this is because the density of the liquid is greater than that of the solid) |
| what is INTRAmolecular force? | the force within molecules (strong) |
| what is INTERmolecular force? | the force between 2 or molecules (weak) |
| what are the three intermolecular forces? (IMF) | 1. london dispersion 2.dipole-dipole 3. hydrogen bonding |
| what is london dispersion force (LDF)? | requires electrons (all molecules have them so all molecules have LDF)- when electrons of one atom are attracted to the nucleus of another atom an instantaneous but temporary dipole occurs |
| what are some characteristics of LDF) | 1. all molecules have them 2. they are the weakest IMF 3. LDF increases as molecular mass increases |
| is boiling point a good measure of IMF? | yes, because a strong IMF means that it takes more energy to pull them apart which means a higher boiling point high BP means high IMF |
| what factors affect LDF? | molecular shape - if there are two molecules that weigh around the same look at molecular shape - the one with bigger surface area is the one the higher LDF |
| what is dipole-dipole force (DD)? | force of attraction between polar molecules |
| what are some characteristics of DD? | 1. second strongest force 2.permanent dipole low energy |
| which one has a greater effect: DD or LDF? | - If there are two molecules that weigh around the same and have the same molecular shape, DD interactions will dominate -If one molecule is much larger than another LDF will determine physical properties |
| what is hydrogen bonding? | when hydrogen is covalently bonded to flourine, oxygen, or nitrogen |
| what are some characteristics of hydrogen bonding? | 1. the strongest IMF 2. highest melting and boiling point |
| what physical properties affect IMF? | surface tension and viscosity |
| what is surface tension | tendency of molecules of a liquid to be attracted more towards one another at the surface of a liquid than to the air above it. |
| how can some insects "walk on water" | the gravity of the insects is not sufficient enough to overcome the surface tension in the liquid. |
| How is surface tension and IMF related? | High IMF= high surface tension |
| what is viscosity? | resistance to flow |
| How is viscosity related to IMF? | Strong IMF= high viscosity HOWEVER= it decreases with higher temperature |
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GelilaB
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