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Gen Chem. (MCAT) > Ch.5 Phases and phase changes > Flashcards

Ch.5 Phases and phase changes Flashcards

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1
Q

Which phase is said to have a fixed shape and volume, and particles do not flow past each other?

A

Solid

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2
Q

What are the two types of solids?

A

Amorphous - not ordered, strong material

Crystalline - Ordered structure, contains a repeating pattern. (there are 4 types of crystalline solids)

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3
Q

What are the crystalline solids?

A

Ionic solids
Molecular - molecules that are not ionic
Covalent network - molecules that contain covalent bonds
Metallic - contains delocalized electrons

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4
Q

Which phase is said to have no fixed shape but does have a fixed volume?

A

Liquids

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5
Q

The resistance of a liquid to flow is known as

A

Viscosity

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6
Q

What is surface tension?

A

amount of energy needed to increase the surface area of a liquid

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7
Q

The attraction of molecules between 2 different substances is known as?

A

Adhesive force

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8
Q

What is capillary action?

A

Movement of a liquid up the side of a narrow tube, against gravity

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9
Q

Which phase is said to have no fixed shape or any volume?

A

Gas

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10
Q

The generic formula of pressure is?

A

force/area

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11
Q

A standard unit of gas is?

A

Paschal (N/meter squared)

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12
Q

Which phase transition is fusion?

A

A solid goes to a liquid form (melting)

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13
Q

Which phase transition is Freezing?

A

liquid to a solid

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14
Q

Which phase transition is VAporization?

A

liquid to a gas

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15
Q

Which phase transition is condensation?

A

gas to a liquid

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16
Q

Which phase transition is sublimation

A

Solid to a gas

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17
Q

Which phase transition is Deposition

A

gas to a solid

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18
Q

Which form of energy determines if phases change?

A

Thermodynamics (ΔG)

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19
Q

To go from a solid to a liquid, how would this affect ΔG

A

Heat is required to melt something, this would mean the ΔH would be positive (Endothermic) and ΔS would be positive as this is a favorable reaction.
The overall ΔG would be positive and form a spontaneous reaction.

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20
Q

What is the Enthalpy of fusion (ΔHf)?

A

how much heat is needed to melt 1 mol of substance.
The unit is given in kJ/mol (Q=mΔHf)
Where is the mass of water/substance

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21
Q

What is Heat of vaporization (ΔHvap)?

A

The heat required to vaporize 1 mol of substance.

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22
Q

The phase of a substance depends on what two factors?

A

Temp and pressure

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23
Q

What is the difference between triple point and critical point?

A

The triple point is where all 3 passes are at equilibrium

critical point is the terminal point of liquid gas

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24
Q

What is supercritical fluid?

A

A substance that has qualities of both gas (low viscosity) and liquid (higher density)

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25
Q

The average kinetic energy of a gas is proportional to?

A

temperature of the gas

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26
Q

What is the ideal gas behavior?

A

High temp make substances more gas-like

Lots of volume and little pressure make favorable behavior

27
Q

When dealing with gas, what should the unit for temp be?

A

Kelivin

C + 273

28
Q

What is boyle’s law?

A

Pressure and volume are inversely related.

p1 V1 = p2 V2

29
Q

What is Charles’s law?

A

Volume and temp of a gas are directly related

V1/T1 = V2/T2) & (V1/T1 = K

30
Q

What is Avagadro’s LAw?

A

Volume of gas is directly related to the number of mol of gas particle
(V1/n1 = V2/n2) & (V/n = K)

31
Q

What are the standard molar volume units for gas?

A

STP = 1 atm and 0°C (273K)

1 mole = 22.4L

32
Q

What is the formula for the IDeal gas law?

A 
PV = nRT
R = Ideal gas constant 
R = 0.08L atm/mol K
R = 8.31 J/mol K
33
Q

How do real gases compare to ideal?

A 
Real gas particles do have size
may exhibit molecular forces (Interforces)
Real gas equations use the Vander Waals equation
(P + a/Vm squared) (Vm - b) = RT
V-b = volume taken up by gas
P + a/Vm - Vm - molar volume
a - attractive intermolecular forces
b - size of particles
34
Q

In regard to the Vander Waals equation, a polar molecule will exhibit a

A

larger “A” term, and behave less ideal-like (compared to non-polar)

35
Q

What is Dalton’s law?

A

The total pressure of the mixture of gasses equas the sum of the partial pressures of individual gasses.

The pressure from a gas is independent of other gasses but depends solely on the total pressure and mole fraction of said gas.

36
Q

How do you calculate mole fraction?

A

Xgas = ngas/ntotal

xgas = Pgas/Ptotal

37
Q

What is Graham’s Law?

A

Smaller lighter particles diffuse faster than larger ones

38
Q

Movement of particles can be described as what type of energy?

A

Kinetic

39
Q

What is the KE equation?

A

KE = 1/2mV squared

40
Q

What is a solution?

A

homogeneous mixture

41
Q

(T/F) solutions can exist in any phase.

A

True

42
Q

(T/F) Solutions can only be formed from one phase.

A

False.

Can be formed from components of different phases

43
Q

What is Dissolution?

A

When a solute interacts with a solvent (disolve).

44
Q

What is the difference between a solute and a solvent?

A

A solute is the minority part. It is typically solid.

A solvent is the majority component and breaks particles into ions.

45
Q

With respect to solutions, what does the term like dissolves like mean?

A

Polar solutes dissolve in polar solvents

non-polar in non-polar

46
Q

When does precipitation occur in a solution?

A

After saturation has reached the maximum

47
Q

What are the units to describe saturation?

A

g/L

48
Q

What two factors affect solubility?

A

Temp and pressure

49
Q

Gas is more soluble in liquids at which temp? Why?

A

lower temp.

Due to the kinetic energy, high temp = high KE for gas

50
Q

Which molecules are always soluble?

A

alkali earth metals

and Nitrate, Chlorate, Acetate

51
Q

Which molecules are sometimes soluble?

A

Halides unless within Ag, Pb, Hg

Sulfate unless with Ca, Sr, Ba, Pb

52
Q

Which molecules are always insoluble?

A

CO3^2-
PO4^3-
S^-2
SO3^2-

53
Q

Which molecules are sometimes insoluble?

A

Hydroxides and metal oxides - unless present with Ca, Sr, Ba

54
Q

Concentration is measured in what 3 ways?

A

Molarity
Molality
Normality

55
Q

What is Molarity?

A

Molarity (M) - equals moles of solute/liter of solution (mol/L)

56
Q

What is molality?

A

molality (m) - moles of solute/kilogram of solvent (mol/kg)

- In low concentrations of solute volume isn’t effected much so 1kg = 1L

57
Q

What is Normality (N)?

A

equivalents/liter of solution

-used in acid/base reactions

58
Q

How do you calculate normality?

A

N(acid) = molarity of acid x acidic protons per molecule

N(base) = Mbase (mol/L) x hydroxide ions per molecule

59
Q

What is the solubility equilibrium?

A

Ksp = Products/reactants

solids and liquids not included

60
Q

What would a high Ksp value mean?

A

high solubility

61
Q

What would a low Ksp value mean?

A

Insoluble

62
Q

How do you calculate molar solubility?

A

Ksp = [cation][Anion]

63
Q

What is the common Ion effect?

A

The solubility of an ionic species decreases when one of its component ions is already present in a solution

Gen Chem. (MCAT) (10 decks)

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