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General Chemistry 2+ L > Exam One Vocabulary > Flashcards

Exam One Vocabulary Flashcards

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1
Q

solution

A

homogeneous mixture of two or more pure substances, can be in any phase, clear as fluids (gas or liquid), can have color

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2
Q

solvent

A

solute dissolves in, most abundant solution component, usually determines solution phase

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3
Q

solute

A

substance that dissolves, less abundant solution component

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4
Q

not solutions

A

suspensions, colloidal dispersions

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5
Q

suspension

A

solid particles in a fluid (gas or liquid), appear cloudy, eventually separates upon standing or with centrifuge

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6
Q

e.s.d

A

equivalent spherical diameter

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7
Q

e.s.d of suspensions

A

> 0.2 µm

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8
Q

colloidal dispersion

A

appears cloudy, does not separate upon standing

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9
Q

colloid e.s.d

A

solid with e.s.d between 0.001 µm and 0.20 µm

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10
Q

enthalpy

A

systems ability to change heat, can be positive or negative

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11
Q

positive enthalpy

A

endothermic

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12
Q

negative enthalpy

A

exothermic

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13
Q

endothermic

A

contributes to increase in E, DOES NOT favor spontaneity

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14
Q

exothermic

A

contributes to decrease in E, favors spontaneity

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15
Q

entropy

A

indication of systems disorder

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16
Q

positive entropy

A

means decrease in system E, favors spontaneity

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17
Q

negative entropy

A

means increase in system E, DOES NOT favor spontaneity

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18
Q

electrolytes

A

a substance that forms an aqueous solution that conducts current, type of solute, creates mobile charge carriers in water, ionic compounds

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19
Q

charge carriers

A

dissolved ions

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20
Q

strong electrolytes

A

complete dissociation

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21
Q

weak electrolytes

A

partial dissociation, covalent solutes

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22
Q

non electrolyte

A

solute that forms a nonconducting solution in water, dissolve but do not dissociate into ions, molecular solute

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23
Q

solubility

A

describes the amount of solute that will dissolve, specific to a solute/solvent combination and condition, max. amount of solute that will dissolve in a given amount of solution

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24
Q

saturated solution

A

contains max. amount of solute, contains the dissolved solute in equilibrium with the undissolved, pure solute

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25
Q

undersaturated solution

A

less than max. solute dissolved

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26
Q

supersaturated solution

A

contains more than max. dissolved solute, disequilibrium, unstable state, formed from saturated solutions following a change of conditions (pressure and temperature)

27
Q

solute-solvent interactions

A

substances with similar intermolecular forces form solutions

28
Q

miscible

A

two liquids that form a solution when mixed

29
Q

immiscible

A

two liquids that DONT form a solution, separate into layers when mixed

30
Q

pressure

A

important for the solubility of gases in liquids, all gases in contact will dissolve

31
Q

Henry’s Law

A

Cg = kPg

32
Q

C (Henry’s Law)

A

concentration of the dissolved gas in the liquid solution

33
Q

k (Henry’s Law)

A

Henry’s Law constant, specific to solute-solvent combination (usually H2O), temperature dependent

34
Q

P (Henry’s Law)

A

partial pressure of the gas in the gas phase O2

35
Q

Pg = XgPtot (what is X)

A

mol formation of gas

36
Q

temperature effects on solids in liquid solutions

A

increase in T = increase in S

37
Q

temperature effects on gases in liquids

A

increase in T = decrease in S

38
Q

colligative properties

A

properties of solutions that depend only on the amount of solute present

39
Q

units of concentration

A

mole fraction (X) and molality (m)

40
Q

Xsolute

A

mols solute/total mols of solution

41
Q

Xsolvent

A

mols solvent/mols solution

42
Q

molality

A

mols/kg

43
Q

vapor pressure

A

pressure exerted by the vapor phase of a substance in equilibrium with the liquid phase of that substance

44
Q

lowering of vapor pressure

A

lowered by the presence of a non volatile solute

45
Q

non volatile

A

doesn’t exert vapor pressure

46
Q

Raoults Law

A

Pa=XaPa

47
Q

Pa (Raoults Law)

A

vapor pressure of A from solution

48
Q

Xa (Raoults Law)

A

mol fraction of substance A
(solvent)

49
Q

Pa (at end of Raoults Law)

A

vapor pressure of pure A

50
Q

boiling point

A

temperature at which vapor pressure of the liquid equals external pressure

51
Q

boiling point elevation (equation)

A

ΔTb = kb x m

52
Q

ΔTb (boiling point elevation)

A

change in boiling point

53
Q

kb (boiling point elevation)

A

boiling point elevation constant, tabulated, specific to solvent

54
Q

m (boiling point elevation)

A

molality

55
Q

osmosis

A

movement of solvent molecules through a semi-permeable membrane in response to a concentration gradient

56
Q

osmosis pressure (Π)

A

the pressure required to prevent osmosis into a solution relative to the pure solvent (physical force overrides the spontaneity)

57
Q

osmosis pressure equation

A

Π = MRT

58
Q

M (osmosis pressure)

A

molarity (mols/L)

59
Q

R (osmosis pressure)

A

constant (0.0821 L x atm/mol x k)

60
Q

T (osmosis pressure)

A

temperature

61
Q

Van’t Hoff factor (i)

A

accounts for association of electrolytes

62
Q

reaction rates

A

change in reactant or product amount over time

63
Q

kinetics

A

study of reaction rates

64
Q

characteristics of reaction rates

A

defined as positive numbers
change over time
depend on:
amount (or concentration) of reactant
temperature
catalyst
surface area (of reactants & catalyst)

General Chemistry 2+ L (4 decks)

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