Busy. Please wait.

show password
Forgot Password?

Don't have an account?  Sign up 

Username is available taken
show password


Make sure to remember your password. If you forget it there is no way for StudyStack to send you a reset link. You would need to create a new account.
We do not share your email address with others. It is only used to allow you to reset your password. For details read our Privacy Policy and Terms of Service.

Already a StudyStack user? Log In

Reset Password
Enter the associated with your account, and we'll email you a link to reset your password.
Didn't know it?
click below
Knew it?
click below
Don't know
Remaining cards (0)
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.

  Normal Size     Small Size show me how

CHEM 126 Chapter 12

CHEM 126 Final

Ion-Dipole force - strength depends on charge density & size of ion (stronger as charge of ion or magnitude of dipole increases) - most commonly found in solutions - positive (cation) attracts partially negative & anion (anion) attracts partially negative - EX: h20 + N
Dipole - Dipole force attractive forces between positive end of 1 polar molecule & negative end of another polar molecule - weaker than ionic & covalent bonds (only significant when touching) - EX: I + Cl
Ion Induced Dipole force - ion induces a dipole of an atom/in a nonpolar molecule (disrupt e- arrangement in nonpolar specieis --> form a dipole) - EX: Fe+2 induces 02
Dipole Induced Dipole force - polar molecules induce a dipole in an atom/in a nonpolar molecule (disrupt e- arrangement in nonpolar species) - EX: ethanol (polar) induces I2 (nonpolar)
Hydrogen Bond - strongest bond - H + (N, O, or F) - H has high + charge density & high - charge density
Dispersion Forces - NON POLAR molecules induce dipolse on each other - ex: oils, gas, unfamiliar forms of substance - polarizable e-clouds
range of attraction strength 1. ionic 2. covalent 3. ion-dipole 4. hydrogen bonding 5. dispersion forces 6. dipole-dipole 7. ion-induced dipole 8. dipole-induced dipole
properties of a solid high intermolecular forces, low KE, high PE
properties of a liquid medium intermolecular forces, equal KE and PE
properties of a gas low intermolecular forces, high KE and low PE
melt/fusion solid to liquid (increase temp) q = n(∆H°fus)
freeze liquid to solid (decrease temp) q = n(-∆H°fus)
vaporize/boil liquid to gas (increase temp) q = n(∆H°vap)
condensation gas to liquid (decrease temp) q = n(-∆H°vap)
sublimation solid to gas (increase temp)
deposition gas to solid (decrease temp)
vapor pressure - liquid gas equilibium - high vapor pressure --> evaporate more quickly - system will adjust rates of vapor/condensation to return to same vapor pressure
boiling point vapor pressure = external, varies with altitude due to pressure change
melting/freezing point - solid liquid equilibrium, pressure has no effect
PHASE DIAGRAM - line between two phases = where at equilibrium - triple point = all at equilibrium - critical point = when equilibrium between liquid and gas becomes non-existent and turns into state in between both
surface tension -energy required to increase the surface area (J/m2) - increase SA -> molecules move up to exterior by breaking attractions in the interior - stronger intermolecular forces -> more energy to increase SA -> more surface tension
capillarity - rising of a liquid against the pull/gravity through a narrow space - competition between IMAFs within a liquid & those between the liquid & tube walls
concave up vs. concave down meniscus - UP: IMAFs are stronger within substance vs between the substance & glass - DOWN: IMAFs from substance and glass form adhesive bonds with glass, cohesion forces between glass & substance
polar & nonpolar surface interaction - adhesive forces between nonpolar (dipole induced dipole) are weaker than polar (H-bonds)-> pull away - EX: h20 & non polar surface
Viscosity - resistance of a fluid to flow - results from IMAFs that impeded movement of molecules around and past each other - liquid > gas(more places for IM forces to act)
external effects on viscosity - TEMP: v decreases with increased temp - MOLECULAR SHAPE: small/sphere - little contact, pour easily VS. long/large - more contact & pour slower
bond length & covalent radius - bond length: between two bonded atoms in the SAME MOLECULE - 1/2 bond length = covalent raidus
van der waals distance & radius - raidus: distance between nuclei of identical nonbonded atom, always larger than covalent radius - radii decreases across a period and increases down a group
Created by: ccottrel



Use these flashcards to help memorize information. Look at the large card and try to recall what is on the other side. Then click the card to flip it. If you knew the answer, click the green Know box. Otherwise, click the red Don't know box.

When you've placed seven or more cards in the Don't know box, click "retry" to try those cards again.

If you've accidentally put the card in the wrong box, just click on the card to take it out of the box.

You can also use your keyboard to move the cards as follows:

If you are logged in to your account, this website will remember which cards you know and don't know so that they are in the same box the next time you log in.

When you need a break, try one of the other activities listed below the flashcards like Matching, Snowman, or Hungry Bug. Although it may feel like you're playing a game, your brain is still making more connections with the information to help you out.

To see how well you know the information, try the Quiz or Test activity.

Pass complete!

"Know" box contains:
Time elapsed:
restart all cards