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Ch.11,13,14.
Chapter test
24
Chemistry
Undergraduate 1
01/30/2012

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Term
Saturated
Definition
Crystallization and solution occuring at equal rates is saturated.
Term
Unsaturated
Definition
Less solute present then what is needed to saturate the solution
Term
Supersaturated
Definition
When concentrations are higher then equilibrium concentrations
Term
Critical Pressure
Definition
the pressure required to bring about the liquification at critical temperature
Term
Critical temperature
Definition
Is the highest temperature at which a distinct liquid phase can form.
Term
Surface Tension
Definition
Is the energy required to increase the surface area by a unit amount.
Term
Viscosity
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
Hydrogen Bonding
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
Polarizability
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
London Dispersion Force
Definition
Temporary Dipole on one atom can induce similar temporary dipole on another; causes atoms to attract. They have to be close together.
Term
Dipole-Dipole Force
Definition
Neutral polar molecules attracted via negative to positive end and vice versa. Need to be close together, weaker then ion dipole
Term
Ion-Dipole Force
Definition
Exists between and ion and a partial charge at the end of a polar molecule. Solutions of ionic substances in polar liquids.
Term
Solvation
Definition
Interaction of solute and solvent
Term
Hydration
Definition
When the solvent is water
Term
Entropy
Definition
The degree of randomness or disorder
Term
Solubility
Definition
The amount of solute needed to form a saturated solution at any particular temperature
Term
Miscible
Definition
"like dissolves like"; liquids that mix in all proportions
Term
Immiscible
Definition
Those solute that do not dissolve significantly in one another
Term
Henry's Law
Definition
Solubility of gas=K(pressure of gas)
Term
Colligative Property
Definition
A physcial property of a solution that depends on the concentration of solute particules present, regardless of the nature of the solute.
Term
Colloids
Definition
particles that are large enough on a molecular scale but still small enough to remain suspended in a solvent system
Term
Tyndall Effect
Definition
scattering of light by colliods
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