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DAT GenChem > GenChem8(Phases and Phase Changes) > Flashcards

GenChem8(Phases and Phase Changes) Flashcards

1
Q

The degree to which two liquids can mix

A

Miscibility

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2
Q

Oil and water can’t mix because of repulsion due to polarity difference, they are

A

immiscible

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3
Q

Under extreme conditions two immiscible liquids can form a fairly homogeneous mixture called an

A

Emulsion

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4
Q

A solid, like NaCl that possesses an ordered structure. Its atoms exist in a specific three-dimensional geometric arrangement with repeating patters of atoms, ions, or molecules

A

Crystalline Solid

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5
Q

A solid that has no ordered three-dimensional arrangement, although the molecules are also fixed in space.

A

Amorphous Solid

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6
Q

Most solids are amorphous or crystalline?

A

Crystalline

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7
Q

What are the two most common forms of crystal solids?

A

Metal and ionic

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8
Q

Aggregates of positively and negatively charged ions; there are no discrete molecules.

A

Ionic Solids

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9
Q

What are the physical properties of ionic solids?

What accounts for these properties?

A

High MP and BP, low electrical conductivity in the solid phase

Strong electrostatic interactions.

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10
Q

These solids consist of metal atoms packed together as closely as possible.

A

Metallic Solids

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11
Q

What are the physical properties of metallic solids?

A

High melting and boiling point

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12
Q

The repeating units of crystals are represented by

A

Unit cells

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13
Q

This occurs when molecules near the surface of a liquid have enough kinetic energy to leave the liquid phase and escape into the gaseous phase.

What happens to the liquid each time it loses a high energy particle this way?

A

Evaporation (or vaporization)

The temperature decreases

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14
Q

The process where gas moves back into the liquid phase

A

Condensation

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15
Q

The pressure that the gas from a liquid exerts over the liquid is called the

A

Vapor Pressure

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16
Q

As temperature increases, vapor pressure….

The temperature at which the vapor pressure of the liquid equals the external pressure is called the

A

Increases

Boiling point

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17
Q

The transition from solid to liquid is…

A

Fusion or melting

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18
Q

The transition from liquid to solid is

A

Solidification, Crystallization, Freezing

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19
Q

The temperature at which fusion and crystallization occur can be called

A

Melting point OR freezing point, depending upon direction

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20
Q

These type of solids have a very sharp melting point

These type of solids have a broad range of melting temperatures

What accounts for this?

A

Crystal solids

Amorphous solids

How ordered their molecular distribution is

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21
Q

Physical properties derived solely from the number of particles present, not the nature of those particles. They are usually associated with dilute solutions.

A

Colligative properties

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22
Q

For every mole of solute particles dissolved in water, how much does the freezing point of water decrease?

A

1.86 °C

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23
Q

What is the freezing point of water?

The boiling point?

A

Freezing point = 0°C

Boiling point = 100°C

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24
Q

What is Chad’s formula for freezing point depression?

A

ΔT= -iKfm

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25
Q

A liquid boils when…

A

Vapor Pressure equals atmospheric pressure

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26
Q

What is Chad’s formula for boiling point elevation

A

ΔT= iKbm

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27
Q

If a 3m solution of something is added to water, how does that affect the ΔT=ikm equation?

A

You multiply K by three

28
Q

What is the formula for osmotic pressure?

A

Π =MRT

M=molarity of the solutoin, R= ideal gas constant, T = temperature in Kelvins

29
Q

Does osmotic pressure depend upon the identity of the solute?

A

No, just the amount of the solute. What it is is IRRELEVANT!

30
Q

Mixtures of substances that combine to form a single phase, generally liquid.

A

Homogenous Solutions

31
Q

Are NaCl, NH3, C12H22O11 solvents or solutes?

Are H20 and benzene solvents or solutes?

A

Solutes

Solvents

32
Q

The interaction between solute and solvent molecules is known as…

A

Solvation or dissolution

33
Q

When water is the solvent in dissolution (aka solvation) what is this process called?

What is the resulting solution called

A

Hydration

Aqueous Solution

34
Q

Defined as the maximum amount of a substance that can be dissolved in a particular solvent at a particular temperature

A

Solubility

35
Q

When the maximum amount of solute has been added to solvent that can be dissolved, the solution is said to be

A solution in which the proportion of solute to solvent is small is said to be…

A solution in which the proportion is large is

A

Saturated

Dilute

Concentrated

36
Q

What are the two solubility rules that Chad mentioned in the videos?

A
  1. All group metals and NO3, NH3, CLO4, C2H3O2 salts are soluble
  2. Most Ag(+), Pb(2+), Hg2 (2+) are in insoluble in water. Exception: not when paired with group 1 metals
37
Q

What is the exception to the second solubility rule?

A

Ag, Pb, and Hg are soluble when paired with group 1 metals

38
Q

What does a roman numeral in front of an element indicate? Ex: Iron (II)

A

The positive charge of an ion of that element

Fe(2+)

39
Q

When ous and ic, like ferrous and ferric, and cuprous and cupric, are added to the endings of the Latin name of an element, that indicates…

A

Lesser and greater charged ions of that element, respectively, of positively charged ions

(Iron II and III and Copper I and II)

40
Q

-ide at the end of an element represent

A

Monoatomic anions

ex: Hydride, H-
Fluoride F-

41
Q

Polyatomic anions that contain oxygen are called

When an element forms two oxyanions, the element with more oxygen ends in

The one with less oxygen end in

A

oxyanions

- ate
- ite
ex: nitrate - NO3-, nitrite NO2(-), Sulfate-SO4(2-), sulfite - SO3 (2-)

42
Q

When a series of oxyanions contains four oxyanions, prefixes are also used. Which are used to inicate less and more oxygen, respectively?

A

Hypo and per

Ex: 
Hypochlorite: CLO(-)
Chlorite: CLO2(-) 
Chlorate: CLO3 (-)
Perchlorate: CLO4(-)
43
Q

Polyatomic ions often gain one or more H+ ions to form anions of lower charge. The resulting ions are named by adding the words _____ and _____ to the front of the anions name.

An older method uses the prefix ___ to indicate the addition of a single hydrogen ion

A

Hydrogen and dihydrogen

bi

ex:
HCO3- —>Hydrogen carbonate or bicarbonate
HSO4 —-> Hydrogen sulfate or Bisulfate
H2PO4 —> Dihydrogen phosphate

44
Q

Do metals generally form positive or negative ions?

What about nonmetals?

A

Metals generally form positive ions

Note: ions may contain metallic elements: chromate, CrO4 (2-) and permanganate, MnO4(-)

Nonmetals generally form negative ions

45
Q

These two groups tend to form cations and and anions

A

Group IIA and VIIA, respectively, with +2 and -1 charges, respectively

46
Q

The electrical conductivity of aqueous solutions is governed by the presence and concentration of ____ in solution

A

Ions

Pure water is a poor conductor.

47
Q

A solute that dissolves completely into its constituent ions is called a…

A

Strong electrolyte

ex: NaCl, KI, HCl, in water

48
Q

A solute that dissolves incompletely in aqueous solution and only some of the solute is present in ionic form is called

A

Weak electrolyte

Ex: weak acids like acetic acid, weak bases like ammonia, and HgCl2

49
Q

Compounds that do not ionize at all in aqueous solution are called

A

Nonelectrolytes

Ex: Nonpolar gases, organic compounds, like oxygen and sugar

50
Q

The number of moles per liter of solution is the

A

Molarity

51
Q

The number of moles per kilogram of solvent is the

A

Molality

52
Q

For dilute solutions at 25 degrees Celsius, the molarity of a solution is approximately _____ to the molality of a solution

A

Equal

The density of water at 25 degrees Celsius is 1kg per liter

53
Q

The number of gram equivalent weights of solute per liter of solution is the…

A

Normality

54
Q

The reactive capacity of a molecule is referred to as the

A

Gram equivalent weight, or equivalent

55
Q

A 1 molar solution of sulfuric acid is how many normal in acid base reactions? Why?

A

2 because one mole of sulfuric acid donates 2 moles of H+

56
Q

What is the equation solving for the concentration of a solution after dilution?

A

MiVi=MfVf

M= molarity, V = volume

57
Q

What is the equation for ion product of a compound, Qsp?

A

[An+]m[Bn-]n

initial concentrations, not necessarily equilibrium

58
Q

What is the expression for the solubility product constant for a saturated solution at equilibrium, Ksp?

A

The same as ion product

[An+]m[Bn-]n

59
Q

What can be said about a solution who’s I.P. is equal its Ksp?

A

The solution is saturated

60
Q

What can be said about a solution who’s I.P. exceeds it’s Ksp?

A

The solution is supersaturated and unstable

61
Q

What can be said about a solution who’s I.P. is less than Ksp?

A

The solution is unsaturated and no precipitate will form

62
Q

The solubility of Fe(OH)3 in an aqueous solution is determined to be 4.5*10^-10 mol/L. What is the Ksp for Fe(OH)3?

A 
[Fe] = 4.5 *10^-10 M
[OH] = 3*[Fe]

Ksp= [OH]^3*[Fe] = (3[Fe])^3 * [Fe]

= 27(4.510^-10)^4

63
Q

What are the concentrations of each of the ions in a saturated solution of PbBr2 given that the Ksp of PbBr2 is 2.1*10^-6

A

Pb=x
Br=2x

Ksp=(x)(2x)^2
Ksp=4x^3=2.1*10^-6

x=8.0710^-3 M
2x=1.6110^-2 M

64
Q

The Ksp of AgI in aqueous solution is 110^-16 mol/L. If a 110^-5 M soution of AgNO3 is saturated with AgI what will be the final concentration of the iodide ion?

A 
1*10^-16 = [Ag] [I]
(1*10^-16)/(1*10^-5) = [I]

[I] = 1*10^-11 mol/L

65
Q

What is Chad’s calorimetric equation to solve for the heat required to raise a substance to a certain temperature with the specific heat?

A

q=mcΔT

DAT GenChem (11 decks)

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