Chapter 6 & 10-11

Question 1

Solution

Answer 1

Homogeneous mixture of 2+ substances

Question 2

Solute

Answer 2

Substance dissolved into a solvent

Question 3

Solvent

Answer 3

Substance with the greatest quantity of moles (solution has the most of this)

Question 4

Homogeneous

Answer 4

Uniform / Same composition throughout

Question 5

Heterogeneous

Answer 5

Nonuniform composition throughout

Question 6

Molarity: Units & formula

Answer 6

moles/liters | (moles of solute)/(liters of solution)

Question 7

Molality: Units & formula

Answer 7

moles/kilograms | (moles of solute)/(kilograms of SOLVENT)

Question 8

Mass %: Units & formula

Answer 8

mass/mass | (mass of solute)/(mass of SOLUTION) x 100%

Question 9

Mole Fraction: Units & formula

Answer 9

moles/total moles | (moles of A)/(total moles of solution)

Question 10

IMFs

Answer 10

Intermolecular Forces. Interactions between separate molecules. Stronger the IMF = closer together the molecules are. Determines substance solubility.

Question 11

London Dispersion Forces

Answer 11

Weakest IMF. Found in every molecule. Occurs when the electrons are on the same side. Is short lived and doesn’t occur constantly.
Atoms that contain move electrons and have a greater size are more likely to have more LDFs

Question 12

Instantaneous dipole

Answer 12

When at some point in time the electrons on a molecule are on the same side. Briefly creates a negative and positive side of a molecule.

Question 13

Induced dipole

Answer 13

Occurs on another molecule after an instantaneous dipole emerges. Attracted to each other.

Question 14

Dipole-Dipole Interactions

Answer 14

Medium IMF strength. Present in all polar molecules. Permanent areas of partial negative and positive charges which makes them stronger than LDFs.

Question 15

Hydrogen Bonding

Answer 15

Strongest IMF. Dipole-Dipole bonds between H and either N, O, or F. Is a special dipole-dipole interaction.
*If you have a hydrogen bond you will have all 3 IMFs.

Question 16

[] meaning

Answer 16

Concentration. [x] = concentration of x

Question 17

Colligative properties

Answer 17

Properties of a solution that depend on the amount of solute particles dissolved

Question 18

Freezing Point: Define & its Colligative Properties

Answer 18

Temperature at which a liquid freezes into a solid.
When adding a solute into a solution, the solute occupies the spaces between solvent particles, disrupting IMFs. As solute increases, FP decreases.

Question 19

Freezing Point Depression

Answer 19

The more solutes in our water solution, the lower the FP can become up until a certain point.

Question 20

Freezing Point formula & what the terms are

Answer 20

ΔTf = i * Kf * molal
ΔTf = Change in freezing temperatures
i = Van’t Hoff factor (solute)
Kf = Freezing point depression constant (of solvent)
molal = molality of solution

Question 21

Van Hoff Factor

Answer 21

Number of solute particles per unit of solute. *How many molecules are in the product of an ionic compound splitting.
Remember - Ionic compounds split apart and must contain a metal.

Question 22

Vapor Pressure

Answer 22

The pressure exerted by its gaseous phase when vaporization and condensation are both occurring. Adding solutes will displace the liquid particles at the surface, preventing/hampering the solvent’s ability to turn into a gas.
[solute] increases, evaporation decreases, vapor pressure decreases

Question 23

Vapor Pressure Equation

Answer 23

Psoln = P°solv * Xsolv
Psoln = Pvap of solution
= Pvap of pure solvent
= Mole fraction of solvent

Question 24

Boiling Point Equation

Answer 24

ΔTb = i * Kb * molal
ΔTf = Change in BP temperatures
i = Van’t Hoff factor (solute)
Kf = Boiling point elevation constant (of solvent)
molal = molality of solution

Question 25

Rault’s Law Equation (for Vapor Pressure)

Answer 25

Psoln = (P°A * XA) + (P°B * XB)

X = Mole fraction