CHEM 126 Final
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
|
|
||||
|---|---|---|---|---|---|
| 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
🗑
|
Review the information in the table. When you are ready to quiz yourself you can hide individual columns or the entire table. Then you can click on the empty cells to reveal the answer. Try to recall what will be displayed before clicking the empty cell.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
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
Normal Size Small Size show me how
Created by:
ccottrel
Popular Chemistry sets