Term
|
Definition
| Crystallization and solution occuring at equal rates is saturated. |
|
|
Term
|
Definition
| Less solute present then what is needed to saturate the solution |
|
|
Term
|
Definition
| When concentrations are higher then equilibrium concentrations |
|
|
Term
|
Definition
| the pressure required to bring about the liquification at critical temperature |
|
|
Term
|
Definition
| Is the highest temperature at which a distinct liquid phase can form. |
|
|
Term
|
Definition
| Is the energy required to increase the surface area by a unit amount. |
|
|
Term
|
Definition
| The resistance of liquid to flow |
|
|
Term
| Order of strength of Molecular Forces. |
|
Definition
1. Hydrogen Bonding
2. Ordinary Ionic or covalent Bonds
3. Ion-Dipole
4. Dipole-Dipole
5. London Dispersion |
|
|
Term
|
Definition
| Attraction between a hydrogen atom in a polar bond and electron pair on another ion. Usually Flourine, oxygen, and Nitrogen. Strongest Bond, effects boiling and freezing |
|
|
Term
|
Definition
| The ease with which the electron distribution in a molecule is distorted. The greater the polarizability, more easily distorted to have temporary dipole. Larger molecules; larger polarizability b/c more electrons |
|
|
Term
|
Definition
| Temporary Dipole on one atom can induce similar temporary dipole on another; causes atoms to attract. They have to be close together. |
|
|
Term
|
Definition
| Neutral polar molecules attracted via negative to positive end and vice versa. Need to be close together, weaker then ion dipole |
|
|
Term
|
Definition
| Exists between and ion and a partial charge at the end of a polar molecule. Solutions of ionic substances in polar liquids. |
|
|
Term
|
Definition
| Interaction of solute and solvent |
|
|
Term
|
Definition
| When the solvent is water |
|
|
Term
|
Definition
| The degree of randomness or disorder |
|
|
Term
|
Definition
| The amount of solute needed to form a saturated solution at any particular temperature |
|
|
Term
|
Definition
| "like dissolves like"; liquids that mix in all proportions |
|
|
Term
|
Definition
| Those solute that do not dissolve significantly in one another |
|
|
Term
|
Definition
| Solubility of gas=K(pressure of gas) |
|
|
Term
|
Definition
| A physcial property of a solution that depends on the concentration of solute particules present, regardless of the nature of the solute. |
|
|
Term
|
Definition
| particles that are large enough on a molecular scale but still small enough to remain suspended in a solvent system |
|
|
Term
|
Definition
| scattering of light by colliods |
|
|
