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Chemistry 101/Chem Lab > Chapter 11 Notes > Flashcards

Chapter 11 Notes Flashcards

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1
Q

What is matter?

A

anything that occupies spaces and has mass

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2
Q

What are the 4 phases of matter? What’s another name for them

A

Solids, Liquids, Gasses, and Plasma

Common Phase States

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3
Q

What are the molecular properties of solids?

A
  • hard, rigid
  • molecules touch each other
  • vibrate in fixed positions
  • do not move around each other
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4
Q

What are the molecular properties of liquids?

A
  • in constant motion
  • moves freely about each other(they slide past each other)
  • more tightly packed than gasses
  • compressible
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5
Q

What are the molecular properties of gasses?

A
  • very spaced out from each other
  • don’t often touch each other
  • very random motion
  • compressible
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6
Q

What is Fluidity?

A

the ability of something to flow

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7
Q

Name the Phase Changes

A 
Solid -> Liquid: melting(fusion)
Solid-> Gas: sublimation
Liquid -> Solid: freezing 
Liquid-> Gas: evaporation(vaporization)
Gas-> Solid: deposition
Gas-> Liquid: condensation
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8
Q

What are Intermolecular Forces (IMFs)?

A

forces of attraction between molecules that hold them together in condensed states

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9
Q

What are the 4 types of IMFs?

A

Dispersion
Dipole-Dipole
Ion-Dipole
Hydrogen Bonds

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10
Q

What are Dispersion Forces?

A
  • weak attractive force between 2 molecules due to a temporary shift in electron density
  • it is the weakest type of IMF and occurs in all matter
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11
Q

What are Dipole-Dipole Forces?

A
  • forces between 2 polar molecules; caused by the tendency of dipoles to line up with the positive end of 1 molecule near the negative end of another
  • stronger force than Dispersion with permanent dipoles in the molecules
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12
Q

What are Ion-Dipole Forces?

A
  • forces of attraction between a dipole and anion

- 2nd Strongest type of IMF

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13
Q

What are Hydrogen bonds?

A
  • forces that exist between a hydrogen atom attracted to a more electronegative atom (F,O,N) inside a molecule
  • STRONGEST type of IMFs
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14
Q

What are Factors that affect Dispersion Forces

A
  1. Molar Mass- with similar compounds; the greater the molar mass, the greater the depression force and the boiling point will be higher
  2. Molecular shape- with the same molecular formula, a linear structure has a higher boiling point than those that are branched or round in structure
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15
Q

What is surface tension?

A
  • the tendency of liquids to minimize their surface area

- it is also the energy required to increase the surface area by a unit amount

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16
Q

What is water’s surface tension at room temperature?

A

72.8 mJ/m^2

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17
Q

How does surface tension relate to IMF?

A

surface tension decreases as IMFs decreases

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18
Q

What is Viscosity?

A

the resistance of a liquid to flow

ex: honey, molasses, motor oil

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19
Q

How is viscosity measured?

A

it’s measured in poise (P) or (cP)

1 poise= 1g/ cm*s

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20
Q

How is viscosity related to IMFs?

A

viscosity increases as IMFs increases and also depend on the molecular shape

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21
Q

How does viscosity relate to temperature?

A

As temp increase, viscosity decreases (in vice versa)

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22
Q

What is Capillary Action?

A

the ability of a liquid to flow against gravity up a narrow tube

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23
Q

How does Capillary Action work?

A

The liquid is more attracted to the glass of a tube than it is to itself. This is because the adhesive forces, the force between 2 different types of molecules, are greater than cohesive, force between like molecules, of the liquid in question

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24
Q

What is Vapor Pressure?

A

partial pressure of a vapor over its liquid at equilibrium

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25
Q

How does Vapor Pressure occur?

A

Vapor pressure is due to the evaporation of molecules from the surface of the liquid

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26
Q

What are Volatile and Nonvolatile liquids?

A

Volatile Liquids: liquids that are easily vaporized

Nonvolatile Liquids: liquids that aren’t easily vaporized

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27
Q

What is Dynamic Equilibrium?

A

a state of balance in which 2 opposing processes are occurring at equal rates

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28
Q

How are gasses volatile?

A

Gasses can be liquefied by decreasing temp and increasing pressure

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29
Q

What is Vaporization/Boiling?

A

going from a liquid phase to a gaseous phase

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30
Q

Boiling point

A

temp at which vapor pressure and atmospheric pressure are equal

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31
Q

Normal Boiling point

A

boiling point at 1 atm of pressure

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32
Q

Melting point

A

temp at which a crystalline solid melts

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33
Q

Freezing point

A

temp at which liquid changes to a crystalline solid

34
Q

What is Heat of Vaporization (∆Hvap)?

A

the amount of heat required to vaporize 1 mol or 1 gram of a liquid at its boiling point
p.s. it will always be a positive value

35
Q

What’s another name for ∆Hvap?

A

Enthalpy

36
Q

what is the ∆Hvap of vaporizing water? Condensing water?

A 
Vaporizing water (L -> G): 40.7 kJ/mol
Condensation (G -> L): -40.7 kJ/mol
37
Q

When is pressure endothermic?

A

When ∆Hvap is positive, because heat is absorbed from the surroundings

38
Q

When is pressure exothermic?

A

When ∆Hvap is negative, heat is released into the surroundings

39
Q

What is the Clausius-Clapeyron equation (that is needed for the test)?

A

The two-point method: ln (P1 / P2) = (-ΔH / R) (1/T2 - 1/T1)

40
Q

What is R (the constant) in the Clausius-Clapeyron equation?

A

R= 8.314 J/molK

41
Q

What is the Critical Point?

A

the point at which a liquid is not distinguishable from a gas

42
Q

What is sublimation?

A

the transition from solid to gas

43
Q

What is deposition?

A

the transition from gas to solid

44
Q

What’s fusion?

A

the transition from solid to liquid

45
Q

What’s freezing?

A

the transition from liquid to solid

46
Q

What is the heat of fusion (ΔHfus)?

A

the amount of heat required to melt 1 gram or 1 mole of a solid

47
Q

ΔHfus of water

A

6.02 kJ/mol; it’s endothermic

48
Q

ΔHfreezing of water

A

-6.02 kJ/mol: it’s exothermic

49
Q

What’s a Phase Diagram?

A

A map of the state of a substance depending on the temp. and pressure
y-axis: displays pressure (Torr)
x-axis: displays temperature (Celcius)

50
Q

What’s a Crystalline Lattice?

A

the regular arrangement of atoms in a crystalline solid (frozen solid)

51
Q

What’s a Unit Cell?

A

the smallest divisible unit of a crystal that, when repeated in 3D, reproduces the entire crystal lattice

52
Q

What’s a Simple Cubic Unit Cell?

A

a unit cell that consists of a cube with one atom at each corner

53
Q

What’s a body-centered cubic unit cell?

A

A unit cell that consists of a cube with 1 atom at each corner and 1 atom (of the same kind) in the very center of the cube

54
Q

What’s a face-centered cubic unit cell?

A

a cube with one atom at each corner and one atom (of the same kind) in the center of each cube face

55
Q

What are the types of molecules?

A

Molecular solids: solids whose composite units are molecules. Ex: H20

Ionic solids: solids whose composite units are ionic Ex: CaF2

Atomic: solids whose composite units are atoms Ex: Xe, Fe, SiO2

56
Q

What are the different types of atomic solids?

A

Nonbonding atomic solids: held together by relatively weak dispersion forces

Metallic atomic solids: held together by metallic bonds which are represented by the interactions of metal cations

Network covalent atomic solids: held together by covalent bonds, the crystal structures of theses solids are more restricted by the geometrical constraints of the covalent bonds

57
Q

What’s a solution?

A

homogenous mixture of two or more substances or components

58
Q

What are the two main parts of a solution?

A

solutes: minor components; usually what is being dissolved
solvent: major components; usually what does the dissolving

59
Q

What is Miscibility?

A

ability to mix

60
Q

What is Solubility?

A

measure of how soluble a substance is

61
Q

What is Entropy?

A

the tendency of a solution to mix; measure of energy randomization or energy dispersal in a system

62
Q

IMFs exists between…

A
  1. solvent- solute particles
  2. solvent particles
  3. solute particles
63
Q

What is the rule of thumb for distinguishing between polar and nonpolar molecules?

A

Like mixes with like:
Polar mixes with polar
Nonpolar mixes with polar

64
Q

Saturated Solution

A

a dissolved solute is in dynamic equilibrium with the undissolved solute; any additional solute will not dissolve

65
Q

Unsaturated solution

A

solution that contains less that the dynamic equilibrium amount of solute; any additional solute will dissolve

66
Q

Supersaturated solution

A

solution that contains more than the equilibrium amount of a solute

67
Q

What are the Factors that Affect Solubility

A

Temperature: solubility of most solids in water increases with increasing temp

Pressure: solubility of gasses in liquids decreases with increasing temp

68
Q

What is pressure?

A

solubility of gasses in liquids increases with increasing pressure

69
Q

What are the ways to measure solution concentration?

A 
Molarity (M) 
Molality (m)
Parts by Mass (% Mass) 
Parts by Volume (ppm/ppb)
Mole Fraction 
Mole Percentage
70
Q

What is Molarity (M)?

A
  • moles of solute/liter of solution
  • this depends on volume
  • varies with temperature
71
Q

What is Molality (m)?

A

mol of solute/ kg of solvent

72
Q

What is Parts by Mass?

A

ratio of the mass of solute to the mass of solution times 100; mass of solute/mass of solution time 100

73
Q

What are the two variants of Parts by Volume?

A

parts by million(ppm): mass of solute/ mass of solution times 10^6

parts by billion (ppb): mass of solute/mass of solution time 10^9

74
Q

What is a Mole Fraction?

A

Xsolute= nsolute/nsolute + nsolvent

75
Q

What is Mole Percentage?

A

Xsolute times 100

76
Q

What is Colligative Properties?

A

properties that depends on the number of dissolved particles in a solution

77
Q

What are the 4 types of Colligative Properties

A

Vapor Pressure Lowering
Freezing Point Depression
Boiling Point Elevation
Osmotic Pressure

78
Q

Raoult’s Law (used to find vapor pressure)

A

the vapor pressure of an ideal solution is dependent on the vapor pressure of each component and the mole fraction of the component in the solution

79
Q

Ideal solution

A

both the solvent and solute contribute to the overall vapor pressre of the solution

80
Q

The Interactions between the solvent-solute particles…

A

are in equal magnitude that distinguishing between solute-solvent is not needed

81
Q

What’s the Freezing Point Depression?

A

Freezing Point of a pure solvent has been reduced by the addition of a solute

82
Q

What is the Van’t Hoff Constant?

A

number of moles of particles/ moles of formula units dissoved

Chemistry 101/Chem Lab (5 decks)

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