Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
25 Cards in this Set
- Front
- Back
|
Define solvent |
The major component of a solution |
|
|
Define solute |
The minor component |
|
|
Solutions form in part because of IF. Why? |
The particles of the solute interact with the particles of the solvent through IF |
|
|
When one substance (solute) dissolves in another (solvent) it is said to be ___________. |
Soluble |
|
|
When one substance does not dissolve in another it is said to be ___________. |
insoluble |
|
|
___________ solute dissolves in polar solvents. |
Polar |
|
|
Nonpolar solute dissolves in _____________ solvents. |
non-polar |
|
|
Concentration = |
amount of solute in a given amount of solution - occasionally amount of solvent |
|
|
What is the equation for molarity (M)? |
Amount solute (in mol) ________________________ Volume of solution (in L) |
|
|
What is the equation for Molality (m)? |
amount solute (in mol) _______________________ mass solvent (in kg) |
|
|
What is the equation for mole fraction (x)? |
amount solute (in mol) _______________________ total amount of solute and solvent (in mol) |
|
|
Define Colligative properties |
properties whose value depends only on the number of solute particles, and not on what they are - value of the property depends on the concentration of the solution |
|
|
The freezing point of a ___________ is lower than a freezing point of the pure __________. |
solution; solvent |
|
|
The difference between the freezing point of the solution and freezing point of the pure solvent is directly proportional to the _________ concentration of solute particles. What is this the same as? |
molal boiling point |
|
|
What is the proportionality constant K sub f? |
The freezing point depression constant, K sub f - the value of K sub f depends on the solvent - The units of K sub f are degrees celsius/m |
|
|
The boiling point of a __________ is higher than the boiling point of the pure ____________. |
solution; solvent - for a nonvolatile solute |
|
|
What is the proportionality constant, K sub b? |
Boiling point elevation constant, K sub b - The value of K sub b depends on the solvent - The units of K sub b are degrees Celsius/m |
|
|
Define Dispersion Force |
An instantaneous dipole on any one helium atom induces instantaneous dipoles on neighboring atoms, which then attract one another |
|
|
Define Dipole Dipole interaction |
The positive end of a polar molecule is attracted to the negative end of its neighbor |
|
|
Define H-bonding |
When H bonds directly to F, O, or N the bonding atoms acquire relatively large partial charges, giving rise to strong dipole-dipole attractions between neighboring molecules |
|
|
Define Ion-Dipole Forces |
The positively charged end of a polar molecule such as H2O is attracted to negative ions and the negatively charged end of the molecule is attracted to positive ions |
|
|
Electronegativity increases ..... |
up and to the right |
|
|
How is a nonpolar bond classified? Why? |
If the Electronegativity difference is between 0 and 0.4 Constitutes for an even sharing of electrons |
|
|
How is a polar bond classified? Why? |
The electronegativity difference is between 0.4 and 2.0 Constitutes uneven sharing of electrons |
|
|
How are ions created and how are they classifed? |
Ions are created by the transfer of electrons Electronegativity difference is greater than 2 (leads to nonmetals with metals) |
