Term
| dipole-dipole interaction in regards to: dependance of the interaction energy on the 1. dipole moment 2.the distance seperating the ion and polar molecule |
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Definition
-exists between 2 polar molecules
-^ mu, ^ int energy
-v mu, v int energy
molecules dont have to be identical
-^ distance seperating polar molecules, v mag of inter energy |
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Term
| ion-dipole interaction including the dependance of the interaction energy on the 1. magnitude of the ion charge 2. dipole moment 3.the distance seperating the ion and polar molecule |
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Definition
-exists between an ion and polar molecule
1. ^mag of ion charge/^mag. of inter. energy-also vice versa
2.^dipole moment, ^ mag of inter. energy and vice versa
3.distance sep. ion and polar molecules^, mag of inter energy v and vice versa |
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Term
hydrogen bond interaction
1.relationship to dipole dipole interaction
2.requirements of the molecules involved |
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Definition
1.unusually strong dipole dipole interaction
2.Molecule 1=contains H atom to a small electronegative element and Molecule 2=contains small electronegative element |
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Term
| ion-induced dipole interaction |
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Definition
| -interaction of a nonpolar molecule with an ion or polar(dipole>0) species |
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Term
| what of a nonpolar species is thought to be symmetrical? |
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Definition
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Term
| an induced dipole moment is resulted from |
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Definition
| an ion or a polar molecule approaching the electron could of the nonpolar species is distorted |
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Term
in the london interaction:
list size of electron compared to mag of int. energy
list number of interacting atoms compared to mag of int. energy
-and the distance of seperating species compared to mag of inter. energy
and mm compared w/ london forces |
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Definition
-^size of electron cloud ^mag of int. energy and vice versa
-^number of int. atoms ^mag of inter. energy and vice versa
-^distance of seperating species v mag of inter. energy
^ mm ^ london interaction energy |
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Term
| order of interactions in terms of relative interaction energy from strong, to moderate, weak and weak, to very weak |
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Definition
| ion-dipole;H-bond;ion-induced dipole;dipole induced dipole;london |
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Term
| partial spacing and order of intermolecular interaction energy |
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Definition
spacing: gas-liquid-solid
order: solid-gas-liquid |
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Term
| ion ion is a dominant interaction between... |
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Definition
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Term
| ion-dipole interaction dominant interaction between.... |
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Definition
| all ionic species and a polar molecule |
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Term
| hydrogen bond and dipole dipole interactions have dominant interactions between.... |
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Definition
two polar molecules
[h-bond>dipole dipole] |
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Term
| london interactions dominant interactions between... |
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Definition
| nonpolar molecules(all molecules) |
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Term
| seven basica crystal systems: |
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Definition
| cubic simple; tetragonal simple; orthorhombic simple; monoclinic simple; rhombohedral; hexagonal; triclinic |
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Term
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Definition
| mixture of two or more substances |
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Term
| a solution is aqueous when |
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Definition
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Term
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Definition
| produced in greater amount, what solute is dissolved in |
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Term
| mass percent is written as: |
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Definition
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Term
| mass percent is written as: |
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Definition
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Term
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Definition
| mass of substance/mass of sample * 100 |
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Term
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Definition
| volume of substance/volume of sample * 100 |
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Term
| volume percent written as; |
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Definition
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Term
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Definition
| mass of substance/mass of sample *10^6, 10^9, 10^12 |
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Term
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Definition
| max amount of solute that can be dissolved in a specified quantity of solvent as a constant temp and pressure and remain stable |
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Term
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Definition
| the max amount of solute to solvent ratio where under specific temp and pressure it is stable |
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Term
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Definition
| unstable solution in which contains more dissolved solute than a saturated solution at a given temp and pressure |
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Term
as temp increases so does solubility in:
as temp increases, solubility decreases in: |
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Definition
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Term
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Definition
| relates the partial pressure of a gas aboce a solution to the concentration of a gas in a solution |
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Term
| henry's law is strictly true when- |
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Definition
the gas solute dissolves in the liquid solvent, but does not react with the solvent
and at low partial pressures and concentrations |
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Term
| henry's law equation and explanations |
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Definition
C(gas)=kP(gas)
Cgas=concentration of dissolved gas in solution(mol frac. molarity)
Pgas=partial pressure of gas above solution
k=henry's law constant |
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Term
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Definition
if one liquid dissolves in the other in all proportions without seperation
ex. alcohol and water |
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Term
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Definition
if two liquids cannot be mixed with all proportions without seperation
ex. oil/water |
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Term
| 3 steps describing dissolution |
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Definition
expand the solute:endothermic
expand the solvent:endothermic
intermolecular attractions develop:exothermic |
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Term
| explain how "like dissolves like" |
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Definition
| the more similar the intermolecular forces, the more likely the solute is going to dissolve into the solvent |
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Term
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Definition
| energy absorbed when a mole of formula units of a solid is sperated into its constituent ions in the gas phase |
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Term
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Definition
| a physical property of a solution which depends on a # of solute particles in a given amount of solvent, but not on the identity of the solute particles |
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Term
| 4 colligative properties: |
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Definition
| vapor pressure, boiling pressure, freezing point depression,osmotic pressure |
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Term
| difference in dissociation and ionization: |
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Definition
dissociation:process of a solid IONIC COMPOUND seperating into ions with dissolved into h2o
-ionization the process of a COVALENT COMPOUND seperating into ions when dissolved in h20 |
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Term
| difference in electrolyte and nonelectrolyte |
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Definition
electrolyte:dissolves in water 2 OR MORE particles result, produces ions when dissolved in water
non electrolyte:dissolves in water ONLY ONE partice results DOES NOT PRODUCE IONS WHEN DISSOLVED IN WATER |
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Term
| vapor pressure lowering in colligative properties |
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Definition
| a solution with a nonvolatile solute will have a lower VP than the pure solvent |
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Term
| in Raoults law what is correlated in the plot graph? |
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Definition
| vapor pressure of solvent will increase with the mole fraction of the solvent but the solute will go the opposite direction |
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Term
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Definition
| the vapor pressure of the solvent is directly proportional to the mol fraction of solvent in the solution |
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Term
| boiling point elevation equation |
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Definition
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Term
| boiling point is a ____ number always |
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Definition
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Term
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Definition
| pressure which must be exerted on the more concentrated solution in order to preent the movement of solvent across the semi-permeable membrane |
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Term
| osmotic pressure equation |
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Definition
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